chemistry chm1 unit 1 atomic structure, bonding and … · 3 leave margin blank (e) using arrows...

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General Certificate of EducationJanuary 2001Advanced Subsidiary Examination

CHEMISTRY CHM1Unit 1 Atomic Structure, Bonding and Periodicity

Friday 12 January 2001 Morning Session

In addition to this paper you will require:

a Periodic Table;

a calculator.

Time allowed: 1 hour 30 minutes

Instructions• Use blue or black ink or ball-point pen.• Fill in the boxes at the top of this page.• Answer all questions in Section A and Section B in the spaces provided.

All working must be shown.• Do all rough work in this book. Cross through any work you do not

want marked.

Information• The maximum mark for this paper is 90.• Mark allocations are shown in brackets.• This paper carries 30 per cent of the total marks for AS. For Advanced

Level this paper carries 15 per cent of the total marks.• You are expected to use a calculator where appropriate.• The following data may be required.

Gas constant R = 8.31 J mol–1 K–1

• Your answers to questions in Section B should be written in continuousprose, where appropriate. You will be assessed on your ability to use anappropriate form and style of writing, to organise relevant informationclearly and coherently, and to use specialist vocabulary, whereappropriate.

Advice• You are advised to spend about 1 hour on Section A and about

30 minutes on Section B.

For ExaminerÕs Use

Number

1

2

3

4

5

6

Mark Number Mark

ExaminerÕs Initials

TOTAL

Total(Column 2)

Total(Column 1)

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1 (a) Give the relative mass and relative charge of a neutron.

Relative mass ...............................................................................................................................

Relative charge ............................................................................................................................(2 marks)

(b) In terms of the number of their fundamental particles, what do two isotopes of anelement have in common and how do they differ?

In common ..................................................................................................................................

Difference ....................................................................................................................................(2 marks)

(c) Give the complete atomic symbol, including mass number and atomic number, for anatom of the isotope with 22 neutrons and 19 electrons.

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(d) In a mass spectrometer the isotopes of an element are separated and two measurementsare made for each isotope.

(i) Which two measurements are made for each isotope?

Measurement 1 ..................................................................................................................

Measurement 2 ..................................................................................................................

(ii) State how the detector in a mass spectrometer works.

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(iii) Why is a mass spectrometer incapable of distinguishing between the ions 14N+ and14N2

2+ ?

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SECTION A

Answer all questions in the spaces provided.

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(e) Using arrows ↑ and ↓ to represent electrons, complete the energy-level diagram belowto show the electronic arrangement in an atom of carbon.

(2 marks)

(f) In terms of sub-levels, give the electronic configuration of the carbon ion C2+

.......................................................................................................................................................(1 mark)

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— — —— 2p2s

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2 (a) The mass of one atom of 12C is 1.99 × 10–23g. Use this information to calculate a valuefor the Avogadro constant. Show your working.

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(b) Give the meaning of the term empirical formula.

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(c) Define the term relative molecular mass.

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(d) The empirical formula of a compound is CHO and its relative molecular mass has thevalue 174. Determine the molecular formula of this compound and show your working.

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(e) A compound with molecular formula CH4O burns in air to form carbon dioxide andwater. Write a balanced equation for this reaction.

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3 Ammonium nitrate can be prepared by the reaction between ammonia and nitric acid:

NH3 + HNO3 → NH4NO3

(a) The concentration of a nitric acid solution is 2.00 mol dm–3. Calculate the volume of thissolution which would be required to react with exactly 20.0 g of ammonia.

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(b) A sample of ammonium nitrate decomposed on heating as shown in the equation below.

NH4NO3 → 2H2O + N2 + 12O2

On cooling the resulting gases to 298 K, the volume of nitrogen and oxygen together wasfound to be 0.0500 m3 at a pressure of 95.0 kPa.

(i) State the ideal gas equation and use it to calculate the total number of moles ofnitrogen and oxygen formed. (The gas constant R = 8.31 J mol–1 K–1)

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(ii) Using your answer to part (b)(i), deduce the number of moles of ammoniumnitrate decomposed and hence calculate the mass of ammonium nitrate in thesample.

Moles of ammonium nitrate ............................................................................................

Mass of ammonium nitrate ..............................................................................................

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4 The diagram below shows the trend in the first ionisation energies of the elements from neonto aluminium.

(a) Draw crosses on the graph to show the first ionisation energies of silicon, phosphorusand sulphur.

(3 marks)

(b) Write an equation to illustrate the process which occurs during the first ionisation ofneon.

.......................................................................................................................................................(1 mark)

(c) Explain why the first ionisation energy of neon and that of magnesium are both higherthan that of sodium.

Explanation for neon .................................................................................................................

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Explanation for magnesium ......................................................................................................

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Ne Na Mg Al Si P S

First ionisationenergy

Element

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(d) Explain why the first ionisation energy of aluminium is lower than that of magnesium.

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(e) State which one of the elements neon, sodium, magnesium, aluminium and silicon hasthe lowest melting point and explain your answer in terms of the structure and bondingpresent in that element.

Element with lowest melting point ............................................................................................

Explanation .................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(3 marks)

(f) State which one of the elements neon, sodium, magnesium, aluminium and silicon hasthe highest melting point and explain your answer in terms of the structure and bondingpresent in that element.

Element with highest melting point ...........................................................................................

Explanation .................................................................................................................................

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.......................................................................................................................................................(3 marks)


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5 (a) Define the term electronegativity.

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.......................................................................................................................................................(2 marks)

(b) State and explain the trend in electronegativity down Group II.

Trend ............................................................................................................................................

Explanation .................................................................................................................................

.......................................................................................................................................................(3 marks)

(c) Write an equation for the reaction of strontium with water, and suggest an approximatevalue for the pH of the resulting solution.

Equation ......................................................................................................................................

pH .................................................................................................................................................(2 marks)

(d) Describe what is seen when an aqueous solution of barium chloride is added to dilutesulphuric acid. Write an equation for the reaction which occurs.

Observation .................................................................................................................................

Equation ......................................................................................................................................(2 marks)

(e) Give two examples which illustrate the atypical properties of beryllium compounds inGroup II.

Example 1 ....................................................................................................................................

Example 2 ....................................................................................................................................(2 marks)

(f) Give one feature of the beryllium ion which causes the atypical properties of berylliumcompounds.

.......................................................................................................................................................(1 mark)

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6 (a) With the aid of diagrams, describe the structure of, and bonding in, crystals of sodiumchloride, graphite and magnesium. In each case, explain how the melting point and theability to conduct electricity of these substances can be understood by a consideration ofthe structure and bonding involved. (23 marks)

(b) Explain how the electron-pair repulsion theory can be used to predict the shapes of themolecules H2O and PF5. Illustrate your answer with diagrams of the molecules on whichthe bond angles are shown. (7 marks)

END OF QUESTIONS

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SECTION B

Answer the question below in the space provided on pages 9 to 12 of this booklet.

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Surname

Centre Number

Candidate Signature

Candidate Number


General Certificate of EducationJune 2001Advanced Subsidiary Examination


Monday 4 June 2001 Afternoon Session


a Periodic Table;

a calculator.




want marked.







For ExaminerÕs Use

Number

1

2

3

4

5

Mark Number Mark

ExaminerÕs Initials

TOTAL

Total(Column 2)

Total(Column 1)

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CHM1 June pgs 1-16 14/3/2001 9:25 am Page 1

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1 (a) Define the terms mass number and atomic number of an atom.

Mass number ...............................................................................................................................

Atomic number ...........................................................................................................................(2 marks)

(b) Give the symbol, including the mass number and the atomic number, for the atom whichhas 3 fewer neutrons and 2 fewer protons than 14

7N.

.......................................................................................................................................................(2 marks)

(c) In terms of sub-levels, give the complete electronic configuration of the nitrogenatom, N, and of the nitride ion, N3–.

N ...................................................................................................................................................

N3– .................................................................................................................................................(2 marks)

(d) Define the term relative atomic mass of an element.

.......................................................................................................................................................

.......................................................................................................................................................(2 marks)

SECTION A



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(e) When a pure, gaseous sample of element X is introduced into a mass spectrometer, fourmononuclear, singly-charged ions are detected, as shown in the spectrum below.

(i) Describe the process by which the gaseous sample of X is converted into ions in amass spectrometer.

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(ii) What adjustment is made to the operating conditions in order to direct thedifferent ions, in turn, onto the detector of a mass spectrometer?

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(iii) Use data from the spectrum above to calculate the relative atomic mass of X.

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(iv) Identify the element X.

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Relativeabundance

m/z82 83 84 85 86


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2 (a) What is the name given to the number of molecules in one mole of carbon dioxide?

.......................................................................................................................................................(1 mark)

(b) (i) State the ideal gas equation.

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(ii) Calculate the volume of 1.00 mol of carbon dioxide gas at 298K and 100kPa.(The gas constant R = 8.31 J mol–1 K–1)

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(iii) Calculate the mass of carbon dioxide gas at 273 K and 500 kPa contained in acylinder of volume 0.00500 m3.

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(c) Hydrogen can be made by the reaction of hydrochloric acid with magnesium accordingto the equation

2HCl + Mg → MgCl2 + H2

What mass of hydrogen is formed when 100 cm3 of hydrochloric acid of concentration5.0moldm–3 reacts with an excess of magnesium?

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(d) A compound of iron contains 38.9% by mass of iron and 16.7% by mass of carbon, theremainder being oxygen.

(i) Determine the empirical formula of the iron compound.

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(ii) When one mole of this iron compound is heated, it decomposes to give one moleof iron(II) oxide, FeO, one mole of carbon dioxide and one mole of another gas.Identify this other gas. (The molecular formula of the iron compound is the sameas its empirical formula.)

.............................................................................................................................................(4 marks)

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3 (a) Name the type of force that holds the particles together in an ionic crystal.

.......................................................................................................................................................(1 mark)

(b) What is a covalent bond?

.......................................................................................................................................................(1 mark)

(c) State how a co-ordinate bond is formed.

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.......................................................................................................................................................(2 marks)

(d) Describe the bonding in a metal.

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.......................................................................................................................................................(2 marks)

(e) A molecule of hydrogen chloride has a dipole and molecules of hydrogen chlorideattract each other by permanent dipole–dipole forces. Molecules of chlorine arenon-polar.

(i) What is a permanent dipole?

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(ii) Explain why a molecule of hydrogen chloride is polar.

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(iii) Name the type of force which exists between molecules of chlorine.

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(f) Show, by means of a diagram, how two molecules of hydrogen fluoride are attracted toeach other by hydrogen bonding; include all lone-pair electrons and partial charges inyour diagram.

(3 marks)

(g) Why is there no hydrogen bonding between molecules of hydrogen bromide?

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4 (a) Describe the motion of the particles in solid iodine and in iodine vapour.

Motion in solid iodine ................................................................................................................

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Motion in iodine vapour ............................................................................................................

.......................................................................................................................................................(3 marks)

(b) Explain why solid iodine vaporises when warmed gently.

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.......................................................................................................................................................(2 marks)

(c) Silver and sodium chloride melt at similar temperatures. Give two physical propertiesof silver which are different from those of sodium chloride and, in each case, give onereason why the property of silver is different from that of sodium chloride.

First property of silver ................................................................................................................

Reason for difference .................................................................................................................

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Second property of silver ...........................................................................................................

Reason for difference .................................................................................................................

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(d) Draw the shapes of BeCl2, NCl3 and BeCl24–. In each case, show any lone-pair electrons

on the central atom and state the value of the bond angle.

BeCl2 NCl3 BeCl 24–

(6 marks)

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5 (a) In terms of structure and bonding, describe and explain fully the difference between themelting points of the Period 3 elements aluminium, silicon and phosphorus.

(12 marks)

(b) Describe and explain the difference between the electrical conductivities of the elementsaluminium, silicon and phosphorus. (4 marks)

(c) State appropriate conditions under which magnesium and calcium react with water.Give equations for the reactions and describe what you would observe. (7 marks)

(d) “Beryllium is an atypical element in Group II.” Justify this statement by comparing thereactions of beryllium hydroxide and magnesium hydroxide with hydrochloric acid andalso with sodium hydroxide. Write equations to illustrate your answer. (7 marks)

END OF QUESTIONS

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Surname

Centre Number

Candidate Signature

Candidate Number




Friday 11 January 2002 Afternoon Session

In addition to this paper you will require:a Periodic Table;

a calculator.




want marked.







For Examiner’s Use

Number

1

2

3

4

5

6

7

Mark Number Mark

Examiner’s Initials

TOTAL

Total(Column 2)

Total(Column 1)

APW/0102/CHM1

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1 (a) Define the term atomic number of an element.

.......................................................................................................................................................(1 mark)

(b) Give the symbol, including mass number and atomic number, for an atom of an elementwhich contains 12 neutrons and 11 electrons.

.......................................................................................................................................................(2 marks)

(c) In terms of s and p sub-levels, give the electronic configuration of an aluminium atom.

.......................................................................................................................................................(1 mark)

(d) How many neutrons are there in one 27Al atom?

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(e) Define the term relative atomic mass of an element.

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(f) Parts (i) to (iv) below refer to the operation of a mass spectrometer.

(i) Name the device used to ionise atoms in a mass spectrometer.

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(ii) Why is it necessary to ionise atoms before acceleration?

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(iii) What deflects the ions?

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(iv) What is adjusted in order to direct ions of different mass to charge ratio onto thedetector?

.............................................................................................................................................(4 marks)

(g) A meteorite was found to contain three isotopes of element X. A mass spectrometergave the following information about these isotopes.

(i) Calculate the relative atomic mass of X.

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(ii) Using the Periodic Table, suggest the most likely identity of element X.

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(iii) Suggest one reason why the relative atomic mass of X, given in the Periodic Table,differs from your answer to part (g)(i).

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m/z 24.0 25.0 26.0

Relative abundance 64.2 20.3 15.5

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2 (a) The diagram below represents a part of the structure of sodium chloride. The ioniccharge is shown on the centre of only one of the ions.

(i) On the diagram, mark the charges on the four negative ions.

(ii) What change occurs to the motion of the ions in sodium chloride when it is heatedfrom room temperature to a temperature below its melting point?

.............................................................................................................................................(2 marks)

(b) Sodium chloride can be formed by reacting sodium with chlorine.

(i) Write an equation for this reaction.

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(ii) A chloride ion has one more electron than a chlorine atom. In the formation ofsodium chloride, from where does this electron come?

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(c) In some ionic compounds the chloride ions are polarised.

(i) What is a polarised chloride ion?

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(ii) What feature of a cation causes a chloride ion to become polarised?

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(d) (i) What is a covalent bond?

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(ii) What property of the atoms joined by a covalent bond causes the bond to bepolar?

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3 (a) The shape of the molecule BCl3 and that of the unstable molecule CCl2 are shown below.

(i) Why is each bond angle exactly 120° in BCl3?

.............................................................................................................................................

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(ii) Predict the bond angle in CCl2 and explain why this angle is different from that inBCl3

Predicted bond angle .......................................................................................................

Explanation .......................................................................................................................

.............................................................................................................................................(5 marks)

(b) Give the name which describes the shape of molecules having bond angles of 109° 28'.Give an example of one such molecule.

Name of shape ............................................................................................................................

Example .......................................................................................................................................(2 marks)

(c) The shape of the XeF4 molecule is shown below.

(i) State the bond angle in XeF4

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(ii) Suggest why the lone pairs of electrons are opposite each other in this molecule.

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Cl

B

Cl Cl

C

Cl Cl

XeF F

F F

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(iii) Name the shape of this molecule, given that the shape describes the positions ofthe Xe and F atoms only.

.............................................................................................................................................(4 marks)

(d) Draw a sketch of the NF3 molecule. Indicate in your sketch any lone pairs of electronson nitrogen.

(2 marks)


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4 (a) State the meaning of the term electronegativity.

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(b) State and explain the trend in electronegativity values across Period 3 from sodium tochlorine.

Trend ............................................................................................................................................

Explanation .................................................................................................................................

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(c) What is meant by the term first ionisation energy?

.......................................................................................................................................................

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(d) The diagram below shows the variation in first ionisation energy across Period 3.

(i) What is the maximum number of electrons that can be accommodated in an s sub-level?

.............................................................................................................................................

First ionisationenergy

Na Mg Al Si P S Cl ArPeriod 3 element

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(ii) What evidence from the diagram supports your answer to part (d)(i)?

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(iii) What evidence from the diagram supports the fact that the 3p sub-level is higherin energy than the 3s?

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(iv) What evidence from the diagram supports the fact that no more than threeunpaired electrons can be accommodated in the 3p sub-level?

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5 (a) (i) Describe the bonding in a metal.

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(ii) Explain why magnesium has a higher melting point than sodium.

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(b) Why do diamond and graphite both have high melting points?

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(c) Why is graphite a good conductor of electricity?

.......................................................................................................................................................(1 mark)

(d) Why is graphite soft?

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10

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6 (a) A small sample of barium metal was added to water in a flask. When the reaction hadceased, the contents of the flask were treated with a small amount of dilute aqueoussodium sulphate.Describe all that you would observe and write equations, with state symbols, for thereactions that occur. (8 marks)

(b) Dilute sodium hydroxide solution was added dropwise until in excess to separate diluteaqueous solutions of beryllium chloride, magnesium chloride and barium chloride.Describe what you would observe in each case and account for your observations.

(8 marks)

(c) (i) A naturally occurring compound of calcium contains by mass 23.29% of calcium,18.64% of sulphur and 2.32% of hydrogen, the remainder being oxygen.Determine the empirical formula of this compound.

(ii) For any compound, what is the relationship between empirical and molecularformula? What additional information is required to determine a molecularformula from an empirical formula? (5 marks)

7 The chloride of an element Z reacts with water according to the following equation.

ZCl4(l) + 2H2O(l) → ZO2(s) + 4HCl(aq)

A 1.304 g sample of ZCl4 was added to water. The solid ZO2 was removed by filtration andthe resulting solution was made up to 250 cm3 in a volumetric flask. A 25.0 cm3 portion of thissolution was titrated against a 0.112 mol dm–3 solution of sodium hydroxide, of which 21.7 cm3

were required to reach the end point.

Use this information to calculate the number of moles of HCl produced and hence the numberof moles of ZCl4 present in the sample. Calculate the relative molecular mass, Mr, of ZCl4.From your answer deduce the relative atomic mass, Ar, of element Z and hence its identity.

(9 marks)

END OF QUESTIONS

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SECTION B

Answer both questions in the spaces provided on pages 12 to 16 of this booklet.

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Surname

Centre Number

Candidate Signature

Candidate Number




Wednesday 29 May 2002 Morning Session


the AQA Periodic Table (Reference CHEM/PT/EX);

a calculator.




want marked.








Number

1

2

3

4

5

6

Mark Number Mark


TOTAL

Total(Column 2)

Total(Column 1)

APW/0202/CHM1

→

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APW/0202/CHM1

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1 (a) The mass of one mole of 1H atoms is 1.0078g and that of one 1H atom is 1.6734 × 10–24g.Use these data to calculate a value for the Avogadro constant accurate to five significantfigures. Show your working.

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(2 marks)

(b) How does the number of atoms in one mole of argon compare with the number ofmolecules in one mole of ammonia?

.......................................................................................................................................................(1 mark)

(c) A sample of ammonia gas occupied a volume of 0.0352 m3 at 298 K and 98.0 kPa.Calculate the number of moles of ammonia in the sample.(The gas constant R = 8.31JK–1 mol–1)

.......................................................................................................................................................

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.......................................................................................................................................................(3 marks)

SECTION A


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16

(d) A solution containing 0.732 mol of ammonia was made up to 250 cm3 in a volumetricflask by adding water. Calculate the concentration of ammonia in this final solution andstate the appropriate units.

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(2 marks)

(e) A different solution of ammonia was reacted with sulphuric acid as shown in theequation below.

2NH3(aq) + H2SO4(aq) → (NH4)2SO4(aq)

In a titration, 25.0 cm3 of a 1.24 mol dm–3 solution of sulphuric acid required 30.8 cm3 ofthis ammonia solution for complete reaction.

(i) Calculate the concentration of ammonia in this solution.

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(ii) Calculate the mass of ammonium sulphate in the solution at the end of thistitration.

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(f) The reaction of magnesium nitride, Mg3N2, with water produces ammonia andmagnesium hydroxide. Write an equation for this reaction.

.......................................................................................................................................................(2 marks)

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2 (a) An ammonium ion, made by the reaction between an ammonia molecule and ahydrogen ion, can be represented as shown in the diagram below.

(i) Name the type of bond represented in the diagram by N—H

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(ii) Name the type of bond represented in the diagram by N→H

.............................................................................................................................................

(iii) In terms of electrons, explain why an arrow is used to represent this N→H bond.

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(iv) In terms of electron pairs, explain why the bond angles in the NH4+ ion are all

109° 289

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(b) Define the term electronegativity.

.......................................................................................................................................................

.......................................................................................................................................................(2 marks)

HH

H

N H

+

→

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δ– δ+(c) A bond between nitrogen and hydrogen can be represented as N—H

(i) In this representation, what is the meaning of the symbol δ+ ?

.............................................................................................................................................

(ii) From this bond representation, what can be deduced about the electronegativityof hydrogen relative to that of nitrogen?

.............................................................................................................................................

.............................................................................................................................................(2 marks)


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3 The table below shows some values of melting points and some heat energies needed formelting.

(a) Name three types of intermolecular force.

Force 1 ..........................................................................................................................................

Force 2 ..........................................................................................................................................

Force 3 ..........................................................................................................................................(3 marks)

(b) (i) Describe the bonding in a crystal of iodine.

.............................................................................................................................................

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(ii) Name the crystal type which describes an iodine crystal.

.............................................................................................................................................

(iii) Explain why heat energy is required to melt an iodine crystal.

.............................................................................................................................................

.............................................................................................................................................(4 marks)

Substance I2 NaCl HF HCl HI

Melting point/K 387 1074 190 158 222

Heat energy for melting /kJmol–1 7.9 28.9 3.9 2.0 2.9

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(c) In terms of the intermolecular forces involved, suggest why

(i) hydrogen fluoride requires more heat energy for melting than does hydrogenchloride,

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(ii) hydrogen iodide requires more heat energy for melting than does hydrogenchloride.

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(d) (i) Explain why the heat energy required to melt sodium chloride is large.

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(ii) The heat energy needed to vaporise one mole of sodium chloride (171kJmol–1) ismuch greater than the heat energy required to melt one mole of sodium chloride.Explain why this is so.

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(e) In terms of its structure and bonding, suggest why graphite has a very high melting point.

.......................................................................................................................................................

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4 (a) State the trend in atomic radius down Group II from Be to Ba and give a reason for thistrend.

Trend ............................................................................................................................................

Reason ..........................................................................................................................................

.......................................................................................................................................................(2 marks)

(b) State and explain the trend in melting points of the elements down Group II from Be toBa.

Trend ............................................................................................................................................

Explanation .................................................................................................................................

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(c) State the trend in reactivity with water of the elements down Group II from Be to Ba.Write an equation for the reaction of magnesium with steam and an equation for thereaction of strontium with water.

Trend ............................................................................................................................................

Equation for magnesium ............................................................................................................

Equation for strontium................................................................................................................(3 marks)

(d) Sulphates of the Group II elements from Be to Ba have different solubilities. Give theformula of the least soluble of these sulphates and state one use that depends upon theinsolubility of this sulphate.

Formula ........................................................................................................................................

Use ................................................................................................................................................(2 marks)

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(e) A solution contains ions of a Group II element, M. When aqueous sodium hydroxide isadded a white precipitate forms. This precipitate dissolves in an excess of aqueoussodium hydroxide. Identify M and write ionic equations for the two reactions.

Identity of M ................................................................................................................................

Equation 1 ...................................................................................................................................

Equation 2 ...................................................................................................................................(3 marks)

(f) With the exception of beryllium chloride, Group II chlorides are classed as ionic.Explain why beryllium chloride is different by considering how a beryllium ion wouldinteract with a chloride ion.

.......................................................................................................................................................

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5 (a) State the relative charge and relative mass of a proton, of a neutron and of an electron.In terms of particles, explain the relationship between two isotopes of the same element.Explain why these isotopes have identical chemical properties. (7 marks)

(b) Define the term relative atomic mass. An element exists as a mixture of three isotopes.Explain, in detail, how the relative atomic mass of this element can be calculated fromdata obtained from the mass spectrum of the element. (7 marks)

6 (a) Explain why certain elements in the Periodic Table are classified as p-block elements.Illustrate your answer with an example of a p-block element and give its electronicconfiguration. (3 marks)

(b) Explain the meaning of the term periodicity as applied to the properties of rows ofelements in the Periodic Table. Describe and explain the trends in atomic radius, inelectronegativity and in conductivity for the elements sodium to argon. (13 marks)

END OF QUESTIONS

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SECTION B

Answer both the questions below in the space provided on pages 10 to 16 of this booklet.

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Number

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2

3

4

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6

7

Mark Number Mark


TOTAL

Total(Column 2)

Total(Column 1)

APW/0103/CHM1

→

→

In addition to this paper you will require:a calculator.




want marked.• The Periodic Table/Data Sheet is provided on pages 3 and 4. Detach this

perforated sheet at the start of the examination.



Gas constant R = 8.31 J K–1 mol–1




CHM1 pgs 1-16 10/10/02 10:18 am Page 1

TClappison

Copyright © 2003 AQA and its licensors. All rights reserved.

APW/0103/CHM1

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SECTION A


1 (a) Complete the following table.

(3 marks)

(b) An atom of element Z has two more protons and two more neutrons than an atom of3416S. Give the symbol, including mass number and atomic number, for this atom of Z.

.......................................................................................................................................................(2 marks)

(c) Complete the electronic configurations for the sulphur atom, S, and the sulphide ion, S2–.

S l s2 ..................................................................................................................................

S2– l s2 ..................................................................................................................................(2 marks)

(d) State the block in the Periodic Table in which sulphur is placed and explain your answer.

Block .............................................................................................................................................

Explanation ..................................................................................................................................(2 marks)

Particle Relative charge Relative mass

Proton

Neutron

Electron

CHM1 pgs 1-16 10/10/02 10:18 am Page 2

1.0

HH

ydro

gen

1

4.0H

eH

eliu

m2

10.8B

Bor

on5

12.0C

Car

bon

6

14.0N

Nitr

ogen

7

16.0O

Oxy

gen

8

19.0

FF

luor

ine

9

20.2 N

eN

eon

10

27.0 A

lA

lum

iniu

m13

28.1 S

iS

ilico

n14

31.0

PP

hosp

horu

s15

32.1

SS

ulph

ur16

35.5 C

lC

hlor

ine

17

39.9 A

rA

rgon

18

6.9

Li

Lith

ium

3

6.9

Li

Lith

ium

3

9.0B

eB

eryl

lium

4

III

IIIIV

VV

IV

II0

*58

– 7

1La

ntha

nide

s

†90

– 1

03A

ctin

ides

Key

rela

tive

atom

ic m

ass

atom

ic n

umbe

r

Th

e P

erio

dic

Tab

le o

f th

e E

lem

ents

�T

he a

tom

ic n

umbe

rs a

nd a

ppro

xim

ate

rela

tive

ato

mic

mas

ses

show

n in

the

tab

le a

re f

or u

se in

the

exa

min

atio

n un

less

sta

ted

othe

rwis

e in

an

indi

vidu

al q

uest

ion.

23.0 N

aS

odiu

m11 39

.1K

Pot

assi

um19

40.1 C

aC

alci

um20

45.0 S

cS

cand

ium

21

47.9 T

iT

itani

um22

50.9

VV

anad

ium

23

52.0 C

rC

hrom

ium

24

54.9 M

nM

anga

nese

25

55.8 F

eIr

on26

58.9 C

oC

obal

t27

58.7 N

iN

icke

l28

63.5 C

uC

oppe

r29

65.4 Z

nZ

inc

30

69.7 G

aG

alliu

m31

72.6 G

eG

erm

aniu

m32

74.9 A

sA

rsen

ic33

79.0 S

eS

elen

ium

34

79.9 B

rB

rom

ine

35

83.8 K

rK

rypt

on36

85.5 R

bR

ubid

ium

37

87.6 S

rS

tron

tium

38

88.9

YY

ttriu

m39

91.2 Z

rZ

ircon

ium

40

92.9 N

bN

iobi

um41

95.9 M

oM

olyb

denu

m42

98.9 T

cTe

chne

tium

43

101.

1 Ru

Rut

heni

um44

102.

9 Rh

Rho

dium

45

106.

4 Pd

Pal

ladi

um46

107.

9 Ag

Silv

er47

112.

4 Cd

Cad

miu

m48

114.

8 InIn

dium

49

118.

7 Sn

Tin

50

121.

8 Sb

Ant

imon

y51

127.

6 TeTe

lluriu

m52

126.

9 IIo

dine

53

131.

3 Xe

Xen

on54

132.

9 Cs

Cae

sium

55

137.

3 Ba

Bar

ium

56

138.

9 La

Lant

hanu

m57

*

178.

5 Hf

Haf

nium

72

180.

9 TaTa

ntal

um73

183.

9 WTu

ngst

en74

186.

2 Re

Rhe

nium

75

190.

2 Os

Osm

ium

76

192.

2 IrIr

idiu

m77

195.

1 Pt

Pla

tinum

78

197.

0 Au

Gol

d79

200.

6 Hg

Mer

cury

80

204.

4 Tl

Tha

llium

81

207.

2 Pb

Lead

82

209.

0 Bi

Bis

mut

h83

210.

0 Po

Pol

oniu

m84

210.

0 At

Ast

atin

e85

222.

0 Rn

Rad

on86

223.

0 Fr

Fran

cium

87

226.

0 Ra

Rad

ium

88

227 A

cA

ctin

ium

89

†

140.

1 Ce

Cer

ium

58

140.

9 Pr

Pras

eody

miu

m59

144.

2 Nd

Neo

dym

ium

60

144.

9 Pm

Pro

met

hium

61

150.

4 Sm

Sam

ariu

m62

152.

0 Eu

Eur

opiu

m63

157.

3 Gd

Gad

olin

ium

64

158.

9 Tb

Terb

ium

65

162.

5 Dy

Dys

pros

ium

66

164.

9 Ho

Hol

miu

m67

167.

3 Er

Erb

ium

68

168.

9 Tm

Thu

lium

69

173.

0 Yb

Ytte

rbiu

m70

175.

0 Lu

Lute

tium

71

232.

0 Th

Tho

rium

90

231.

0 Pa

Pro

tact

iniu

m91

238.

0 UU

rani

um92

237.

0 Np

Nep

tuni

um93

239.

1 Pu

Plu

toni

um94

243.

1 Am

Am

eric

ium

95

247.

1 Cm

Cur

ium

96

247.

1 Bk

Ber

keliu

m97

252.

1 Cf

Cal

iforn

ium

98

(252

) Es

Ein

stei

nium

99

(257

) Fm

Fer

miu

m10

0

(258

) Md

Men

dele

vium

101

(259

) No

Nob

eliu

m10

2

(260

) Lr

Law

renc

ium

103

24.3 M

gM

agne

sium

12

APW/0103/CHM1

3

CHM1 pgs 1-16 10/10/02 10:18 am Page 3

Table 1Proton n.m.r chemical shift data

Type of proton δ/ppm

RCH3 0.7–1.2

R2CH2 1.2–1.4

R3CH 1.4–1.6

RCOCH3 2.1–2.6

ROCH3 3.1–3.9

RCOOCH3 3.7–4.1

ROH 0.5–5.0

Table 2Infra-red absorption data

Bond Wavenumber/cm–1

C—H 2850–3300

C—C 750–1100

C C 1620–1680

C O 1680–1750

C—O 1000–1300

O—H (alcohols) 3230–3550

O—H (acids) 2500–3000

APW/0103/CHM1

4

CHM1 pgs 1-16 10/10/02 10:18 am Page 4

5LEAVE

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Turn over �

APW/0103/CHM1

(e) Sodium sulphide, Na2S, is a high melting point solid which conducts electricity whenmolten. Carbon disulphide, CS2, is a liquid which does not conduct electricity.

(i) Deduce the type of bonding present in Na2S and that present in CS2

Bonding in Na2S ................................................................................................................

Bonding in CS2 ..................................................................................................................

(ii) By reference to all the atoms involved explain, in terms of electrons, how Na2S isformed from its atoms.

.............................................................................................................................................

.............................................................................................................................................

(iii) Draw a diagram, including all the outer electrons, to represent the bonding presentin CS2

(iv) When heated with steam, CS2 reacts to form hydrogen sulphide, H2S, and carbon dioxide.Write an equation for this reaction.

.............................................................................................................................................(7 marks)


16

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2 (a) Calculate the concentration, in mol dm–3, of the solution formed when 19.6 g ofhydrogen chloride, HCl, are dissolved in water and the volume made up to 250 cm3.

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(3 marks)

(b) The carbonate of metal M has the formula M2CO3. The equation for the reaction of thiscarbonate with hydrochloric acid is given below.

M2CO3 + 2HCl → 2MCl + CO2 + H2O

A sample of M2CO3, of mass 0.394 g, required the addition of 21.7 cm3 of a 0.263 mol dm–3 solution of hydrochloric acid for complete reaction.

(i) Calculate the number of moles of hydrochloric acid used.

.............................................................................................................................................

.............................................................................................................................................

(ii) Calculate the number of moles of M2CO3 in 0.394 g.

.............................................................................................................................................

.............................................................................................................................................

(iii) Calculate the relative molecular mass of M2CO3

.............................................................................................................................................

.............................................................................................................................................

(iv) Deduce the relative atomic mass of M and hence suggest its identity.

Relative atomic mass of M ..............................................................................................

.............................................................................................................................................

Identity of M .....................................................................................................................(6 marks)

9

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3 When a sample of liquid, X, of mass 0.406 g was vaporised, the vapour was found to occupy avolume of 2.34 × 10–4 m3 at a pressure of 110 kPa and a temperature of 473 K.

(a) Give the name of the equation pV = nRT.

.......................................................................................................................................................(1 mark)

(b) Use the equation pV = nRT to calculate the number of moles of X in the sample andhence deduce the relative molecular mass of X.(The gas constant R = 8.31 J K–1 mol–1)

Moles of X ....................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................

Relative molecular mass of X .....................................................................................................

.......................................................................................................................................................(4 marks)

(c) Compound X, which contains carbon, hydrogen and oxygen only, has 38.7% carbon and9.68% hydrogen by mass. Calculate the empirical formula of X.

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(3 marks)

(d) Using your answers to parts (b) and (c) above, deduce the molecular formula of X.

.......................................................................................................................................................

.......................................................................................................................................................(1 mark)

Turn over �

APW/0103/CHM1

9

CHM1 pgs 1-16 10/10/02 10:18 am Page 7

4 (a) The boiling point of H2O is 373 K and that of H2S is 212 K.

(i) Name the strongest type of intermolecular attraction present in water.

.............................................................................................................................................

(ii) Name the strongest type of intermolecular attraction present in hydrogensulphide.

.............................................................................................................................................

(iii) Explain why the boiling point of water is so much higher than that of hydrogensulphide.

.............................................................................................................................................

.............................................................................................................................................(4 marks)

(b) Define the term electronegativity.

.......................................................................................................................................................

.......................................................................................................................................................(2 marks)

(c) State and explain the trend in electronegativity down Group II from Be to Ba.

Trend ............................................................................................................................................

Explanation .................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(3 marks)

(d) (i) Give the type of bonding present in BeCl2

.............................................................................................................................................

(ii) Give the type of bonding present in BaCl2

.............................................................................................................................................

(iii) Explain why the type of bonding is different in these two compounds.

.............................................................................................................................................

.............................................................................................................................................(3 marks)

APW/0103/CHM1

8LEAVE

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CHM1 pgs 1-16 10/10/02 10:18 am Page 8

9LEAVE

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(e) (i) Explain what is meant by the term amphoteric. Write two equations involvingBe(OH)2 to illustrate your answer.

Explanation .......................................................................................................................

.............................................................................................................................................

Equation 1 .........................................................................................................................

Equation 2 .........................................................................................................................

(ii) In what way is this behaviour of Be(OH)2 atypical of the behaviour of Group IImetal hydroxides?

.............................................................................................................................................

.............................................................................................................................................(4 marks)


Turn over �

APW/0103/CHM1

16

CHM1 pgs 1-16 10/10/02 10:18 am Page 9

APW/0103/CHM1

10LEAVE

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5 There is a general trend in the values of the first ionisation energies of the elements Na to Ar.The first ionisation energies of the elements Al and S deviate from this trend.

(a) Write an equation, including state symbols, to represent the process for which the energychange is the first ionisation energy of Na.

.......................................................................................................................................................(2 marks)

(b) State and explain the general trend in the values of the first ionisation energies of theelements Na to Ar.

Trend ............................................................................................................................................

Explanation .................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(3 marks)

(c) State how, and explain why, the values of the first ionisation energies of the elements Al and S deviate from the general trend.

How the values deviate from the trend .....................................................................................

Explanation for Al ......................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................

Explanation for S ........................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(5 marks)

10

CHM1 pgs 1-16 10/10/02 10:18 am Page 10

11LEAVE

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6 (a) Ionisation is the first of the four main stages involved in obtaining the mass spectrum ofa sample of gaseous titanium atoms. Explain how ionisation is achieved. Name theremaining three stages and, in each case, state how each stage is achieved. Explain whyit would be difficult to distinguish between 48Ti2+ and 24Mg+ ions using a massspectrometer. (10 marks)

(b) State any differences and similarities in the atomic structure of the isotopes of anelement. State the difference, if any, in the chemistry of these isotopes. Explain youranswer. (4 marks)

(c) The table below gives the percentage abundance of each isotope in the mass spectrumof a sample of titanium.

Define the term relative atomic mass of an element. Use the above data to calculate thevalue of the relative atomic mass of titanium in this sample. Give your answer to twodecimal places. (4 marks)

7 (a) Predict the shapes of the SF6 molecule and the AlCl4– ion. Draw diagrams of these

species to show their three-dimensional shapes. Name the shapes and suggest values forthe bond angles. Explain your reasoning. (8 marks)

(b) Perfume is a mixture of fragrant compounds dissolved in a volatile solvent.

When applied to the skin the solvent evaporates, causing the skin to cool for a short time.After a while, the fragrance may be detected some distance away. Explain theseobservations. (4 marks)

END OF QUESTIONS

Turn over �

APW/0103/CHM1

SECTION B

Answer both questions below in the space provided on pages 12 to 16 of this booklet.

m/z 46 47 48 49 50

% abundance 8.02 7.31 73.81 5.54 5.32

CHM1 pgs 1-16 10/10/02 10:18 am Page 11

Surname

Centre Number

Candidate Signature

Candidate Number




Wednesday 4 June 2003 Morning Session


a calculator.

Time allowed: 1 hour







Gas constant R = 8.31JK–1 mol–1

• Your answers to the question in Section B should be written incontinuous prose, where appropriate. You will be assessed on your abilityto use an appropriate form and style of writing, to organise relevantinformation clearly and coherently, and to use specialist vocabulary,where appropriate.

Advice• You are advised to spend about 45 minutes on Section A and about



Number

1

2

3

4

5

Mark Number Mark


TOTAL

Total(Column 2)

Total(Column 1)

APW/0203/CHM1

→

→

CHM1 pgs 1-16 6/2/03 9:08 am Page 1

TClappison


1.0

HH

ydro

gen

1

4.0H

eH

eliu

m2

10.8B

Bor

on5

12.0C

Car

bon

6

14.0N

Nitr

ogen

7

16.0O

Oxy

gen

8

19.0

FF

luor

ine

9

20.2 N

eN

eon

10

27.0 A

lA

lum

iniu

m13

28.1 S

iS

ilico

n14

31.0

PP

hosp

horu

s15

32.1

SS

ulph

ur16

35.5 C

lC

hlor

ine

17

39.9 A

rA

rgon

18

6.9

Li

Lith

ium

3

6.9

Li

Lith

ium

3

9.0B

eB

eryl

lium

4

III

IIIIV

VV

IV

II0

*58

– 7

1La

ntha

nide

s

†90

– 1

03A

ctin

ides

Key

rela

tive

atom

ic m

ass

atom

ic n

umbe

r

Th

e P

erio

dic

Tab

le o

f th

e E

lem

ents

�T

he a

tom

ic n

umbe

rs a

nd a

ppro

xim

ate

rela

tive

ato

mic

mas

ses

show

n in

the

tab

le a

re f

or u

se in

the

exa

min

atio

n un

less

sta

ted

othe

rwis

e in

an

indi

vidu

al q

uest

ion.

23.0 N

aS

odiu

m11 39

.1K

Pot

assi

um19

40.1 C

aC

alci

um20

45.0 S

cS

cand

ium

21

47.9 T

iT

itani

um22

50.9

VV

anad

ium

23

52.0 C

rC

hrom

ium

24

54.9 M

nM

anga

nese

25

55.8 F

eIr

on26

58.9 C

oC

obal

t27

58.7 N

iN

icke

l28

63.5 C

uC

oppe

r29

65.4 Z

nZ

inc

30

69.7 G

aG

alliu

m31

72.6 G

eG

erm

aniu

m32

74.9 A

sA

rsen

ic33

79.0 S

eS

elen

ium

34

79.9 B

rB

rom

ine

35

83.8 K

rK

rypt

on36

85.5 R

bR

ubid

ium

37

87.6 S

rS

tron

tium

38

88.9

YY

ttriu

m39

91.2 Z

rZ

ircon

ium

40

92.9 N

bN

iobi

um41

95.9 M

oM

olyb

denu

m42

98.9 T

cTe

chne

tium

43

101.

1 Ru

Rut

heni

um44

102.

9 Rh

Rho

dium

45

106.

4 Pd

Pal

ladi

um46

107.

9 Ag

Silv

er47

112.

4 Cd

Cad

miu

m48

114.

8 InIn

dium

49

118.

7 Sn

Tin

50

121.

8 Sb

Ant

imon

y51

127.

6 TeTe

lluriu

m52

126.

9 IIo

dine

53

131.

3 Xe

Xen

on54

132.

9 Cs

Cae

sium

55

137.

3 Ba

Bar

ium

56

138.

9 La

Lant

hanu

m57

*

178.

5 Hf

Haf

nium

72

180.

9 TaTa

ntal

um73

183.

9 WTu

ngst

en74

186.

2 Re

Rhe

nium

75

190.

2 Os

Osm

ium

76

192.

2 IrIr

idiu

m77

195.

1 Pt

Pla

tinum

78

197.

0 Au

Gol

d79

200.

6 Hg

Mer

cury

80

204.

4 Tl

Tha

llium

81

207.

2 Pb

Lead

82

209.

0 Bi

Bis

mut

h83

210.

0 Po

Pol

oniu

m84

210.

0 At

Ast

atin

e85

222.

0 Rn

Rad

on86

223.

0 Fr

Fran

cium

87

226.

0 Ra

Rad

ium

88

227 A

cA

ctin

ium

89

†

140.

1 Ce

Cer

ium

58

140.

9 Pr

Pras

eody

miu

m59

144.

2 Nd

Neo

dym

ium

60

144.

9 Pm

Pro

met

hium

61

150.

4 Sm

Sam

ariu

m62

152.

0 Eu

Eur

opiu

m63

157.

3 Gd

Gad

olin

ium

64

158.

9 Tb

Terb

ium

65

162.

5 Dy

Dys

pros

ium

66

164.

9 Ho

Hol

miu

m67

167.

3 Er

Erb

ium

68

168.

9 Tm

Thu

lium

69

173.

0 Yb

Ytte

rbiu

m70

175.

0 Lu

Lute

tium

71

232.

0 Th

Tho

rium

90

231.

0 Pa

Pro

tact

iniu

m91

238.

0 UU

rani

um92

237.

0 Np

Nep

tuni

um93

239.

1 Pu

Plu

toni

um94

243.

1 Am

Am

eric

ium

95

247.

1 Cm

Cur

ium

96

247.

1 Bk

Ber

keliu

m97

252.

1 Cf

Cal

iforn

ium

98

(252

) Es

Ein

stei

nium

99

(257

) Fm

Fer

miu

m10

0

(258

) Md

Men

dele

vium

101

(259

) No

Nob

eliu

m10

2

(260

) Lr

Law

renc

ium

103

24.3 M

gM

agne

sium

12

3

APW/0203/CHM1

CHM1 pgs 1-16 6/2/03 9:08 am Page 3

APW/0203/CHM1



RCH3 0.7–1.2

R2CH2 1.2–1.4

R3CH 1.4–1.6

RCOCH3 2.1–2.6

ROCH3 3.1–3.9

RCOOCH3 3.7–4.1

ROH 0.5–5.0



C—H 2850–3300

C—C 750–1100

C C 1620–1680

C O 1680–1750

C—O 1000–1300


O—H (acids) 2500–3000

4

CHM1 pgs 1-16 6/2/03 9:08 am Page 4

5LEAVE

MARGINBLANK

Turn over �

APW/0203/CHM1

1 (a) (i) Complete the electronic configuration of aluminium.

1s2 .......................................................................................................................................

(ii) State the block in the Periodic Table to which aluminium belongs.

.............................................................................................................................................(2 marks)

(b) Describe the bonding in metals.

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(2 marks)

(c) Explain why the melting point of magnesium is higher than that of sodium.

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(3 marks)

(d) Explain how metals conduct electricity.

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(2 marks)

9

SECTION A


CHM1 pgs 1-16 6/2/03 9:08 am Page 5

APW/0203/CHM1

6LEAVE

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2 (a) Give the relative charge and relative mass of an electron.

Relative charge ............................................................................................................................

Relative mass ...............................................................................................................................(2 marks)

(b) Isotopes of chromium include 54Cr and 52Cr

(i) Give the number of protons present in an atom of 54Cr

.............................................................................................................................................

(ii) Deduce the number of neutrons present in an atom of 52Cr

.............................................................................................................................................

(iii) Apart from the relative mass of each isotope, what else would need to be knownfor the relative atomic mass of chromium to be calculated?

.............................................................................................................................................(3 marks)

(c) In order to obtain a mass spectrum of a gaseous sample of chromium, the sample mustfirst be ionised.

(i) Give two reasons why it is necessary to ionise the chromium atoms in the sample.

Reason 1 ............................................................................................................................

Reason 2 ............................................................................................................................

(ii) State what is adjusted so that each of the isotopes of chromium can be detected inturn.

.............................................................................................................................................

(iii) Explain how the adjustment given in part (c)(ii) enables the isotopes of chromiumto be separated.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................(4 marks)

CHM1 pgs 1-16 6/2/03 9:08 am Page 6

7LEAVE

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(d) (i) State what is meant by the term empirical formula.

.............................................................................................................................................

.............................................................................................................................................

(ii) A chromium compound contains 28.4% of sodium and 32.1% of chromium bymass, the remainder being oxygen.Calculate the empirical formula of this compound.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................(4 marks)


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APW/0203/CHM1

13

CHM1 pgs 1-16 6/2/03 9:08 am Page 7

3 (a) A sample of ethanol vapour, C2H5OH (Mr = 46.0), was maintained at a pressure of100kPa and at a temperature of 366K.

(i) State the ideal gas equation.

.............................................................................................................................................

(ii) Use the ideal gas equation to calculate the volume, in cm3, that 1.36 g of ethanolvapour would occupy under these conditions.(The gas constant R = 8.31JK–1 mol–1)

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................(5 marks)

(b) Magnesium nitride reacts with water to form magnesium hydroxide and ammonia.

(i) Balance the equation, given below, for the reaction between magnesium nitrideand water.

Mg3N2 + H2O → Mg(OH)2 + NH3

(ii) Calculate the number of moles, and hence the number of molecules, of NH3 in0.263g of ammonia gas.(The Avogadro constant L = 6.02 × 1023 mol–1)

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................(4 marks)

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CHM1 pgs 1-16 6/2/03 9:08 am Page 8

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(c) Sodium carbonate is manufactured in a two-stage process as shown by the equationsbelow.

NaCl + NH3 + CO2 + H2O → NaHCO3 + NH4Cl

2NaHCO3 → Na2CO3 + H2O + CO2

Calculate the maximum mass of sodium carbonate which could be obtained from 800 gof sodium chloride.

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(4 marks)


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APW/0203/CHM1

13

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4 (a) Both HF and HCl are molecules having a polar covalent bond. Their boiling points are293K and 188K respectively.

(i) State which property of the atoms involved causes a bond to be polar.

.............................................................................................................................................

.............................................................................................................................................

(ii) Explain, in terms of the intermolecular forces present in each compound, why HFhas a higher boiling point than HCl.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................(4 marks)

(b) When aluminium chloride reacts with chloride ions, as shown by the equation below, aco-ordinate bond is formed.

AlCl3 + Cl– → AlCl4–

Explain how this co-ordinate bond is formed.

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(2 marks)

CHM1 pgs 1-16 6/2/03 9:08 am Page 10

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(c) Draw the shape of the PCl5 molecule and of the PCl4+ ion. State the value(s) of the bond

angles.

PCl5 PCl4+

Bond angle(s) ................................................ Bond angle(s) ...............................................

(4 marks)


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APW/0203/CHM1

10

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SECTION B


5 (a) The table below gives the melting point for each of the Period 3 elements Na – Ar.

In terms of structure and bonding, explain why silicon has a high melting point, and whythe melting point of sulphur is higher than that of phosphorus. (7 marks)

(b) Draw a diagram to show the structure of sodium chloride. Explain, in terms of bonding,why sodium chloride has a high melting point. (4 marks)

(c) Give the conditions under which, if at all, beryllium and magnesium react with water.For any reaction that occurs, state one observation you would make and write anequation. (4 marks)

END OF QUESTIONS

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

Element Na Mg Al Si P S Cl Ar

Melting point /K 371 923 933 1680 317 392 172 84

CHM1 pgs 1-16 6/2/03 9:08 am Page 12

Surname

Centre Number

Candidate Signature

Candidate Number






Number

1

2

3

4

5

6

Mark Number Mark


TOTAL

Total(Column 2)

Total(Column 1)

APW/0104/CHM1

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→


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CHM1

CHM1 pgs 1-12 13/10/03 10:49 am Page 1

APW/0104/CHM1

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SECTION A


1 (a) One isotope of sodium has a relative mass of 23.

(i) Define, in terms of the fundamental particles present, the meaning of the termisotopes.

.............................................................................................................................................

.............................................................................................................................................

(ii) Explain why isotopes of the same element have the same chemical properties.

.............................................................................................................................................

.............................................................................................................................................

(iii) Calculate the mass, in grams, of a single atom of this isotope of sodium.(The Avogadro constant, L, is 6.023×1023 mol–1)

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................(5 marks)

(b) Give the electronic configuration, showing all sub-levels, for a sodium atom.

.......................................................................................................................................................(1 mark)

(c) Explain why chromium is placed in the d block in the Periodic Table.

.......................................................................................................................................................

.......................................................................................................................................................(1 mark)

(d) An atom has half as many protons as an atom of 28Si and also has six fewer neutrons thanan atom of 28Si. Give the symbol, including the mass number and the atomic number, ofthis atom.

.......................................................................................................................................................(2 marks)

9

CHM1 pgs 1-12 13/10/03 10:49 am Page 2

1.0

HH

ydro

gen

1

4.0H

eH

eliu

m2

10.8B

Bor

on5

12.0C

Car

bon

6

14.0N

Nitr

ogen

7

16.0O

Oxy

gen

8

19.0

FF

luor

ine

9

20.2 N

eN

eon

10

27.0 A

lA

lum

iniu

m13

28.1 S

iS

ilico

n14

31.0

PP

hosp

horu

s15

32.1

SS

ulph

ur16

35.5 C

lC

hlor

ine

17

39.9 A

rA

rgon

18

6.9

Li

Lith

ium

3

6.9

Li

Lith

ium

3

9.0B

eB

eryl

lium

4

III

IIIIV

VV

IV

II0

*58

– 7

1La

ntha

nide

s

†90

– 1

03A

ctin

ides

Key

rela

tive

atom

ic m

ass

atom

ic n

umbe

r

Th

e P

erio

dic

Tab

le o

f th

e E

lem

ents

�T

he a

tom

ic n

umbe

rs a

nd a

ppro

xim

ate

rela

tive

ato

mic

mas

ses

show

n in

the

tab

le a

re f

or u

se in

the

exa

min

atio

n un

less

sta

ted

othe

rwis

e in

an

indi

vidu

al q

uest

ion.

23.0 N

aS

odiu

m11 39

.1K

Pot

assi

um19

40.1 C

aC

alci

um20

45.0 S

cS

cand

ium

21

47.9 T

iT

itani

um22

50.9

VV

anad

ium

23

52.0 C

rC

hrom

ium

24

54.9 M

nM

anga

nese

25

55.8 F

eIr

on26

58.9 C

oC

obal

t27

58.7 N

iN

icke

l28

63.5 C

uC

oppe

r29

65.4 Z

nZ

inc

30

69.7 G

aG

alliu

m31

72.6 G

eG

erm

aniu

m32

74.9 A

sA

rsen

ic33

79.0 S

eS

elen

ium

34

79.9 B

rB

rom

ine

35

83.8 K

rK

rypt

on36

85.5 R

bR

ubid

ium

37

87.6 S

rS

tron

tium

38

88.9

YY

ttriu

m39

91.2 Z

rZ

ircon

ium

40

92.9 N

bN

iobi

um41

95.9 M

oM

olyb

denu

m42

98.9 T

cTe

chne

tium

43

101.

1 Ru

Rut

heni

um44

102.

9 Rh

Rho

dium

45

106.

4 Pd

Pal

ladi

um46

107.

9 Ag

Silv

er47

112.

4 Cd

Cad

miu

m48

114.

8 InIn

dium

49

118.

7 Sn

Tin

50

121.

8 Sb

Ant

imon

y51

127.

6 TeTe

lluriu

m52

126.

9 IIo

dine

53

131.

3 Xe

Xen

on54

132.

9 Cs

Cae

sium

55

137.

3 Ba

Bar

ium

56

138.

9 La

Lant

hanu

m57

*

178.

5 Hf

Haf

nium

72

180.

9 TaTa

ntal

um73

183.

9 WTu

ngst

en74

186.

2 Re

Rhe

nium

75

190.

2 Os

Osm

ium

76

192.

2 IrIr

idiu

m77

195.

1 Pt

Pla

tinum

78

197.

0 Au

Gol

d79

200.

6 Hg

Mer

cury

80

204.

4 Tl

Tha

llium

81

207.

2 Pb

Lead

82

209.

0 Bi

Bis

mut

h83

210.

0 Po

Pol

oniu

m84

210.

0 At

Ast

atin

e85

222.

0 Rn

Rad

on86

223.

0 Fr

Fran

cium

87

226.

0 Ra

Rad

ium

88

227 A

cA

ctin

ium

89

†

140.

1 Ce

Cer

ium

58

140.

9 Pr

Pras

eody

miu

m59

144.

2 Nd

Neo

dym

ium

60

144.

9 Pm

Pro

met

hium

61

150.

4 Sm

Sam

ariu

m62

152.

0 Eu

Eur

opiu

m63

157.

3 Gd

Gad

olin

ium

64

158.

9 Tb

Terb

ium

65

162.

5 Dy

Dys

pros

ium

66

164.

9 Ho

Hol

miu

m67

167.

3 Er

Erb

ium

68

168.

9 Tm

Thu

lium

69

173.

0 Yb

Ytte

rbiu

m70

175.

0 Lu

Lute

tium

71

232.

0 Th

Tho

rium

90

231.

0 Pa

Pro

tact

iniu

m91

238.

0 UU

rani

um92

237.

0 Np

Nep

tuni

um93

239.

1 Pu

Plu

toni

um94

243.

1 Am

Am

eric

ium

95

247.

1 Cm

Cur

ium

96

247.

1 Bk

Ber

keliu

m97

252.

1 Cf

Cal

iforn

ium

98

(252

) Es

Ein

stei

nium

99

(257

) Fm

Fer

miu

m10

0

(258

) Md

Men

dele

vium

101

(259

) No

Nob

eliu

m10

2

(260

) Lr

Law

renc

ium

103

24.3 M

gM

agne

sium

12

APW/0104/CHM1

3

CHM1 pgs 1-12 13/10/03 10:49 am Page 3



RCH3 0.7–1.2

R2CH2 1.2–1.4

R3CH 1.4–1.6

RCOCH3 2.1–2.6

ROCH3 3.1–3.9

RCOOCH3 3.7–4.1

ROH 0.5–5.0



C—H 2850–3300

C—C 750–1100

C C 1620–1680

C O 1680–1750

C—O 1000–1300


O—H (acids) 2500–3000

APW/0104/CHM1

4

CHM1 pgs 1-12 13/10/03 10:49 am Page 4

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APW/0104/CHM1

2 A gaseous sample of chromium can be analysed in a mass spectrometer. Before deflection, thechromium atoms are ionised and then accelerated.

(a) Describe briefly how positive ions are formed from gaseous chromium atoms in a massspectrometer.

.......................................................................................................................................................

.......................................................................................................................................................(2 marks)

(b) What is used in a mass spectrometer to accelerate the positive ions?

.......................................................................................................................................................(1 mark)

(c) What is used in a mass spectrometer to deflect the positive ions?

.......................................................................................................................................................(1 mark)

(d) The mass spectrum of a sample of chromium shows four peaks. Use the data below tocalculate the relative atomic mass of chromium in the sample. Give your answer to twodecimal places.

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(2 marks)

6

m/z 50 52 53 54

Relative abundance/% 4.3 83.8 9.5 2.4

CHM1 pgs 1-12 13/10/03 10:49 am Page 5

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3 (a) The equation for the reaction between magnesium carbonate and hydrochloric acid isgiven below.

MgCO3 + 2HCl → MgCl2 + H2O + CO2

When 75.0 cm3 of 0.500 mol dm–3 hydrochloric acid were added to 1.25 g of impureMgCO3 some acid was left unreacted. This unreacted acid required 21.6 cm3 of a 0.500 mol dm–3 solution of sodium hydroxide for complete reaction.

(i) Calculate the number of moles of HCl in 75.0 cm3 of 0.500 mol dm–3 hydrochloricacid.

.............................................................................................................................................

(ii) Calculate the number of moles of NaOH used to neutralise the unreacted HCl.

.............................................................................................................................................

.............................................................................................................................................

(iii) Show that the number of moles of HCl which reacted with the MgCO3 in thesample was 0.0267

.............................................................................................................................................

(iv) Calculate the number of moles and the mass of MgCO3 in the sample, and hencededuce the percentage by mass of MgCO3 in the sample.

Moles of MgCO3 ..............................................................................................................

.............................................................................................................................................

Mass of MgCO3 ................................................................................................................

.............................................................................................................................................

Percentage of MgCO3 ......................................................................................................

.............................................................................................................................................(8 marks)

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(b) A compound contains 36.5% of sodium and 25.5% of sulphur by mass, the rest beingoxygen.

(i) Use this information to show that the empirical formula of the compound is Na2SO3

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

(ii) When Na2SO3 is treated with an excess of hydrochloric acid, aqueous sodiumchloride is formed and sulphur dioxide gas is evolved. Write an equation torepresent this reaction.

.............................................................................................................................................

.............................................................................................................................................(4 marks)


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12

CHM1 pgs 1-12 13/10/03 10:49 am Page 7

4 (a) Compound A is an oxide of sulphur. At 415 K, a gaseous sample of A, of mass 0.304 g,occupied a volume of 127cm3 at a pressure of 103kPa.

State the ideal gas equation and use it to calculate the number of moles of A in thesample, and hence calculate the relative molecular mass of A.(The gas constant R = 8.31JK–1 mol–1)

Ideal gas equation .......................................................................................................................

Calculation ..................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(5 marks)

(b) The presence of sulphate ions in an aqueous solution can be shown by means of a simplechemical test.

(i) Identify a reagent you would use in this chemical test.

.............................................................................................................................................

(ii) State what you would observe if the test were positive.

.............................................................................................................................................

(iii) Write an ionic equation for the reaction occurring when the test is positive.

.............................................................................................................................................

.............................................................................................................................................(3 marks)

APW/0104/CHM1

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8

CHM1 pgs 1-12 13/10/03 10:49 am Page 8

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5 The diagram below shows the values of the first ionisation energies of some of the elements inPeriod 3.

(a) On the above diagram, use crosses to mark the approximate positions of the values ofthe first ionisation energies for the elements Na, P and S. Complete the diagram byjoining the crosses. (3 marks)

(b) Explain the general increase in the values of the first ionisation energies of the elementsNa–Ar.

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(3 marks)

(c) In terms of the electron sub-levels involved, explain the position of aluminium and theposition of sulphur in the diagram.

Explanation for aluminium .......................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................

Explanation for sulphur .............................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(4 marks)

Turn over �

APW/0104/CHM1

10

1600

1400

1200

1000

800

600

400

200

0

First ionisationenergy/kJ mol –1

Na Mg Al Si P S Cl Ar

CHM1 pgs 1-12 13/10/03 10:49 am Page 9

6 (a) Iodine and graphite crystals both contain covalent bonds and yet the physical propertiesof their crystals are very different.For iodine and graphite, state and explain the differences in their melting points and intheir electrical conductivities. (9 marks)

(b) Draw the shape of the BeCl2 molecule and explain why it has this shape.State and explain the effect that an isolated Be2+ ion would have on an isolated Cl– ionand explain how this effect would lead to the formation of a covalent bond.Give one chemical property of Be(OH)2 which is atypical of the chemistry of Group IIhydroxides. (6 marks)

END OF QUESTIONS

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

............................................................................................................................................................................

APW/0104/CHM1

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SECTION B


CHM1 pgs 1-12 13/10/03 10:49 am Page 10

Surname

Centre Number

Candidate Signature

Candidate Number




Thursday 10 June 2004 Morning Session


a calculator.













Number

1

2

3

4

5

6

Mark Number Mark


TOTAL

Total(Column 2)

Total(Column 1)

APW/0204/CHM1

→

→

CHM1

CHM1 pgs 1-16 12/12/03 1:45 pm Page 1

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(2 marks)

(b) An atom of element Q contains the same number of neutrons as are found in an atomof 27Al. An atom of Q also contains 14 protons.

(i) Give the number of protons in an atom of 27Al.

.............................................................................................................................................

(ii) Deduce the symbol, including mass number and atomic number, for this atom ofelement Q.

.............................................................................................................................................(3 marks)

(c) Define the term relative atomic mass of an element.

.......................................................................................................................................................

.......................................................................................................................................................(2 marks)

SECTION A


Relative mass Relative charge

Proton

Electron

CHM1 pgs 1-16 12/12/03 1:45 pm Page 2

1.0

HH

ydro

gen

1

4.0H

eH

eliu

m2

10.8B

Bor

on5

12.0C

Car

bon

6

14.0N

Nitr

ogen

7

16.0O

Oxy

gen

8

19.0

FF

luor

ine

9

20.2 N

eN

eon

10

27.0 A

lA

lum

iniu

m13

28.1 S

iS

ilico

n14

31.0

PP

hosp

horu

s15

32.1

SS

ulph

ur16

35.5 C

lC

hlor

ine

17

39.9 A

rA

rgon

18

6.9

Li

Lith

ium

3

6.9

Li

Lith

ium

3

9.0B

eB

eryl

lium

4

III

IIIIV

VV

IV

II0

*58

– 7

1La

ntha

nide

s

†90

– 1

03A

ctin

ides

Key

rela

tive

atom

ic m

ass

atom

ic n

umbe

r

Th

e P

erio

dic

Tab

le o

f th

e E

lem

ents

�T

he a

tom

ic n

umbe

rs a

nd a

ppro

xim

ate

rela

tive

ato

mic

mas

ses

show

n in

the

tab

le a

re f

or u

se in

the

exa

min

atio

n un

less

sta

ted

othe

rwis

e in

an

indi

vidu

al q

uest

ion.

23.0 N

aS

odiu

m11 39

.1K

Pot

assi

um19

40.1 C

aC

alci

um20

45.0 S

cS

cand

ium

21

47.9 T

iT

itani

um22

50.9

VV

anad

ium

23

52.0 C

rC

hrom

ium

24

54.9 M

nM

anga

nese

25

55.8 F

eIr

on26

58.9 C

oC

obal

t27

58.7 N

iN

icke

l28

63.5 C

uC

oppe

r29

65.4 Z

nZ

inc

30

69.7 G

aG

alliu

m31

72.6 G

eG

erm

aniu

m32

74.9 A

sA

rsen

ic33

79.0 S

eS

elen

ium

34

79.9 B

rB

rom

ine

35

83.8 K

rK

rypt

on36

85.5 R

bR

ubid

ium

37

87.6 S

rS

tron

tium

38

88.9

YY

ttriu

m39

91.2 Z

rZ

ircon

ium

40

92.9 N

bN

iobi

um41

95.9 M

oM

olyb

denu

m42

98.9 T

cTe

chne

tium

43

101.

1 Ru

Rut

heni

um44

102.

9 Rh

Rho

dium

45

106.

4 Pd

Pal

ladi

um46

107.

9 Ag

Silv

er47

112.

4 Cd

Cad

miu

m48

114.

8 InIn

dium

49

118.

7 Sn

Tin

50

121.

8 Sb

Ant

imon

y51

127.

6 TeTe

lluriu

m52

126.

9 IIo

dine

53

131.

3 Xe

Xen

on54

132.

9 Cs

Cae

sium

55

137.

3 Ba

Bar

ium

56

138.

9 La

Lant

hanu

m57

*

178.

5 Hf

Haf

nium

72

180.

9 TaTa

ntal

um73

183.

9 WTu

ngst

en74

186.

2 Re

Rhe

nium

75

190.

2 Os

Osm

ium

76

192.

2 IrIr

idiu

m77

195.

1 Pt

Pla

tinum

78

197.

0 Au

Gol

d79

200.

6 Hg

Mer

cury

80

204.

4 Tl

Tha

llium

81

207.

2 Pb

Lead

82

209.

0 Bi

Bis

mut

h83

210.

0 Po

Pol

oniu

m84

210.

0 At

Ast

atin

e85

222.

0 Rn

Rad

on86

223.

0 Fr

Fran

cium

87

226.

0 Ra

Rad

ium

88

227 A

cA

ctin

ium

89

†

140.

1 Ce

Cer

ium

58

140.

9 Pr

Pras

eody

miu

m59

144.

2 Nd

Neo

dym

ium

60

144.

9 Pm

Pro

met

hium

61

150.

4 Sm

Sam

ariu

m62

152.

0 Eu

Eur

opiu

m63

157.

3 Gd

Gad

olin

ium

64

158.

9 Tb

Terb

ium

65

162.

5 Dy

Dys

pros

ium

66

164.

9 Ho

Hol

miu

m67

167.

3 Er

Erb

ium

68

168.

9 Tm

Thu

lium

69

173.

0 Yb

Ytte

rbiu

m70

175.

0 Lu

Lute

tium

71

232.

0 Th

Tho

rium

90

231.

0 Pa

Pro

tact

iniu

m91

238.

0 UU

rani

um92

237.

0 Np

Nep

tuni

um93

239.

1 Pu

Plu

toni

um94

243.

1 Am

Am

eric

ium

95

247.

1 Cm

Cur

ium

96

247.

1 Bk

Ber

keliu

m97

252.

1 Cf

Cal

iforn

ium

98

(252

) Es

Ein

stei

nium

99

(257

) Fm

Fer

miu

m10

0

(258

) Md

Men

dele

vium

101

(259

) No

Nob

eliu

m10

2

(260

) Lr

Law

renc

ium

103

24.3 M

gM

agne

sium

12

3

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APW/0204/CHM1



RCH3 0.7–1.2

R2CH2 1.2–1.4

R3CH 1.4–1.6

RCOCH3 2.1–2.6

ROCH3 3.1–3.9

RCOOCH3 3.7–4.1

ROH 0.5–5.0



C—H 2850–3300

C—C 750–1100

C C 1620–1680

C O 1680–1750

C—O 1000–1300


O—H (acids) 2500–3000

4

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(d) The table below gives the relative abundance of each isotope in a mass spectrum of asample of magnesium.

Use the data above to calculate the relative atomic mass of this sample of magnesium.Give your answer to one decimal place.

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(2 marks)

(e) State how the relative molecular mass of a covalent compound is obtained from its massspectrum.

.......................................................................................................................................................

.......................................................................................................................................................(1 mark)


10

m/z 24 25 26

Relative abundance (%) 73.5 10.1 16.4

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2 (a) Sodium carbonate forms a number of hydrates of general formula Na2CO3.xH2OA 3.01 g sample of one of these hydrates was dissolved in water and the solution madeup to 250cm3.In a titration, a 25.0 cm3 portion of this solution required 24.3 cm3 of 0.200 mol dm–3

hydrochloric acid for complete reaction.The equation for this reaction is shown below.

Na2CO3 + 2HCl → 2NaCl + H2O + CO2

(i) Calculate the number of moles of HCl in 24.3 cm3 of 0.200 mol dm–3 hydrochloricacid.

.............................................................................................................................................

(ii) Deduce the number of moles of Na2CO3 in 25.0cm3 of the Na2CO3 solution.

.............................................................................................................................................

(iii) Hence deduce the number of moles of Na2CO3 in the original 250cm3 of solution.

.............................................................................................................................................

(iv) Calculate the Mr of the hydrated sodium carbonate.

.............................................................................................................................................

.............................................................................................................................................(5 marks)

(b) In an experiment, the Mr of a different hydrated sodium carbonate was found to be 250.Use this value to calculate the number of molecules of water of crystallisation, x, in thishydrated sodium carbonate, Na2CO3.xH2O

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(3 marks)

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(c) A gas cylinder, of volume 5.00 × 10–3 m3, contains 325g of argon gas.

(i) Give the ideal gas equation.

.............................................................................................................................................

(ii) Use the ideal gas equation to calculate the pressure of the argon gas in the cylinderat a temperature of 298K.(The gas constant R = 8.31JK–1 mol–1)

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................(4 marks)


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3 The values of the first ionisation energies of neon, sodium and magnesium are 2080, 494 and736 kJmol–1, respectively.

(a) Explain the meaning of the term first ionisation energy of an atom.

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(2 marks)

(b) Write an equation to illustrate the process occurring when the second ionisation energyof magnesium is measured.

.......................................................................................................................................................

.......................................................................................................................................................(2 marks)

(c) Explain why the value of the first ionisation energy of magnesium is higher than that ofsodium.

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(2 marks)

(d) Explain why the value of the first ionisation energy of neon is higher than that ofsodium.

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(2 marks)

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4 Lithium hydride, LiH, is an ionic compound containing the hydride ion, H–

The reaction between LiH and aluminium chloride, AlCl3, produces the ionic compoundLiAlH4

(a) Balance the equation below which represents the reaction between LiH and AlCl3

LiH + AlCl3 → LiAlH4 + LiCl

(1 mark)

(b) Give the electronic configuration of the hydride ion, H–

.......................................................................................................................................................(1 mark)

(c) Predict the shape of the AlH–4 ion. Explain why it has this shape.

Shape ............................................................................................................................................

Explanation .................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(3 marks)

(d) A bond in AlH–4 can be represented by H→Al

Name this type of bond and explain how it is formed.

Type of bond ...............................................................................................................................

Explanation .................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(3 marks)


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5 (a) There is a trend in the reactivity of the Group II metals, Be–Ba, with water. State thistrend and give the conditions under which magnesium reacts rapidly with water. Writean equation to represent this reaction.

Trend Be to Ba ............................................................................................................................

Conditions ...................................................................................................................................

Equation ......................................................................................................................................(3 marks)

(b) Describe what you would observe when a few drops of aqueous sodium hydroxide areadded to aqueous beryllium chloride, followed by a large excess of aqueous sodiumhydroxide. Write equations for the two reactions which occur.

Observation when a few drops are added ................................................................................

.......................................................................................................................................................

Equation ......................................................................................................................................

Observation with excess .............................................................................................................

.......................................................................................................................................................

Equation ......................................................................................................................................(4 marks)

7

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6 (a) Define the term electronegativity and explain why the electronegativity values of theGroup II elements Be–Ba decrease down the group. (4 marks)

(b) Name the strongest type of intermolecular force between hydrogen fluoride moleculesand draw a diagram to illustrate how two molecules of HF are attracted to each other.In your diagram show all lone pairs of electrons and any partial charges. Explain theorigin of these charges.Suggest why this strong intermolecular force is not present between HI molecules.

(7 marks)

(c) Crystals of sodium chloride and of diamond both have giant structures. Their meltingpoints are 1074 K and 3827 K, respectively. State the type of structure present in eachcase and explain why the melting point of diamond is so high. (4 marks)

END OF QUESTIONS

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CHM1 pgs 1-16 12/12/03 1:45 pm Page 16

Surname

Centre Number

Candidate Signature

Candidate Number




Tuesday 11 January 2005 Morning Session


Number

1

2

3

4

5

Mark Number Mark


TOTAL

Total(Column 2)

Total(Column 1)

APW/0105/CHM1

→

→


a calculator.












CHM1

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SECTION A


1 (a) Define the terms

(i) mass number of an atom,

.............................................................................................................................................

(ii) relative molecular mass.

.............................................................................................................................................

.............................................................................................................................................(3 marks)

(b) (i) Complete the electron arrangement for a copper atom.

1s2 .......................................................................................................................................

(ii) Identify the block in the Periodic Table to which copper belongs.

.............................................................................................................................................

(iii) Deduce the number of neutrons in one atom of 65Cu

.............................................................................................................................................(3 marks)

CHM1 pgs 1-12 28/9/04 11:07 am Page 2

1.0

HH

ydro

gen

1

4.0H

eH

eliu

m2

10.8B

Bor

on5

12.0C

Car

bon

6

14.0N

Nitr

ogen

7

16.0O

Oxy

gen

8

19.0

FF

luor

ine

9

20.2 N

eN

eon

10

27.0 A

lA

lum

iniu

m13

28.1 S

iS

ilico

n14

31.0

PP

hosp

horu

s15

32.1

SS

ulph

ur16

35.5 C

lC

hlor

ine

17

39.9 A

rA

rgon

18

6.9

Li

Lith

ium

3

6.9

Li

Lith

ium

3

9.0B

eB

eryl

lium

4

III

IIIIV

VV

IV

II0

*58

– 7

1La

ntha

nide

s

†90

– 1

03A

ctin

ides

Key

rela

tive

atom

ic m

ass

atom

ic n

umbe

r

Th

e P

erio

dic

Tab

le o

f th

e E

lem

ents

�T

he a

tom

ic n

umbe

rs a

nd a

ppro

xim

ate

rela

tive

ato

mic

mas

ses

show

n in

the

tab

le a

re f

or u

se in

the

exa

min

atio

n un

less

sta

ted

othe

rwis

e in

an

indi

vidu

al q

uest

ion.

23.0 N

aS

odiu

m11 39

.1K

Pot

assi

um19

40.1 C

aC

alci

um20

45.0 S

cS

cand

ium

21

47.9 T

iT

itani

um22

50.9

VV

anad

ium

23

52.0 C

rC

hrom

ium

24

54.9 M

nM

anga

nese

25

55.8 F

eIr

on26

58.9 C

oC

obal

t27

58.7 N

iN

icke

l28

63.5 C

uC

oppe

r29

65.4 Z

nZ

inc

30

69.7 G

aG

alliu

m31

72.6 G

eG

erm

aniu

m32

74.9 A

sA

rsen

ic33

79.0 S

eS

elen

ium

34

79.9 B

rB

rom

ine

35

83.8 K

rK

rypt

on36

85.5 R

bR

ubid

ium

37

87.6 S

rS

tron

tium

38

88.9

YY

ttriu

m39

91.2 Z

rZ

ircon

ium

40

92.9 N

bN

iobi

um41

95.9 M

oM

olyb

denu

m42

98.9 T

cTe

chne

tium

43

101.

1 Ru

Rut

heni

um44

102.

9 Rh

Rho

dium

45

106.

4 Pd

Pal

ladi

um46

107.

9 Ag

Silv

er47

112.

4 Cd

Cad

miu

m48

114.

8 InIn

dium

49

118.

7 Sn

Tin

50

121.

8 Sb

Ant

imon

y51

127.

6 TeTe

lluriu

m52

126.

9 IIo

dine

53

131.

3 Xe

Xen

on54

132.

9 Cs

Cae

sium

55

137.

3 Ba

Bar

ium

56

138.

9 La

Lant

hanu

m57

*

178.

5 Hf

Haf

nium

72

180.

9 TaTa

ntal

um73

183.

9 WTu

ngst

en74

186.

2 Re

Rhe

nium

75

190.

2 Os

Osm

ium

76

192.

2 IrIr

idiu

m77

195.

1 Pt

Pla

tinum

78

197.

0 Au

Gol

d79

200.

6 Hg

Mer

cury

80

204.

4 Tl

Tha

llium

81

207.

2 Pb

Lead

82

209.

0 Bi

Bis

mut

h83

210.

0 Po

Pol

oniu

m84

210.

0 At

Ast

atin

e85

222.

0 Rn

Rad

on86

223.

0 Fr

Fran

cium

87

226.

0 Ra

Rad

ium

88

227 A

cA

ctin

ium

89

†

140.

1 Ce

Cer

ium

58

140.

9 Pr

Pras

eody

miu

m59

144.

2 Nd

Neo

dym

ium

60

144.

9 Pm

Pro

met

hium

61

150.

4 Sm

Sam

ariu

m62

152.

0 Eu

Eur

opiu

m63

157.

3 Gd

Gad

olin

ium

64

158.

9 Tb

Terb

ium

65

162.

5 Dy

Dys

pros

ium

66

164.

9 Ho

Hol

miu

m67

167.

3 Er

Erb

ium

68

168.

9 Tm

Thu

lium

69

173.

0 Yb

Ytte

rbiu

m70

175.

0 Lu

Lute

tium

71

232.

0 Th

Tho

rium

90

231.

0 Pa

Pro

tact

iniu

m91

238.

0 UU

rani

um92

237.

0 Np

Nep

tuni

um93

239.

1 Pu

Plu

toni

um94

243.

1 Am

Am

eric

ium

95

247.

1 Cm

Cur

ium

96

247.

1 Bk

Ber

keliu

m97

252.

1 Cf

Cal

iforn

ium

98

(252

) Es

Ein

stei

nium

99

(257

) Fm

Fer

miu

m10

0

(258

) Md

Men

dele

vium

101

(259

) No

Nob

eliu

m10

2

(260

) Lr

Law

renc

ium

103

24.3 M

gM

agne

sium

12

APW/0105/CHM1

3

CHM1 pgs 1-12 28/9/04 11:07 am Page 3



RCH3 0.7–1.2

R2CH2 1.2–1.4

R3CH 1.4–1.6

RCOCH3 2.1–2.6

ROCH3 3.1–3.9

RCOOCH3 3.7–4.1

ROH 0.5–5.0



C—H 2850–3300

C—C 750–1100

C C 1620–1680

C O 1680–1750

C—O 1000–1300


O—H (acids) 2500–3000

APW/0105/CHM1

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(c) A sample of copper contains the two isotopes 63Cu and 65Cu only. It has a relativeatomic mass, Ar, less than 64. The mass spectrum of this sample shows major peaks withm/z values of 63 and 65, respectively.

(i) Explain why the Ar of this sample is less than 64.

.............................................................................................................................................

(ii) Explain how Cu atoms are converted into Cu+ ions in a mass spectrometer.

.............................................................................................................................................

.............................................................................................................................................

(iii) In addition to the major peaks at m/z = 63 and 65, much smaller peaks at m/z = 31.5and 32.5 are also present in the mass spectrum. Identify the ion responsible for thepeak at m/z = 31.5 in the mass spectrum. Explain why your chosen ion has this m/zvalue and suggest one reason why this peak is very small.

Identity of the ion .............................................................................................................

Explanation for m/z value ...............................................................................................

.............................................................................................................................................

Reason why this peak is very small ................................................................................

.............................................................................................................................................(6 marks)


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2 (a) Ammonium sulphate reacts with aqueous sodium hydroxide as shown by the equationbelow.

(NH4)2SO4 + 2NaOH → 2NH3 + Na2SO4 + 2H2O

A sample of ammonium sulphate was heated with 100 cm3 of 0.500 mol dm–3 aqueoussodium hydroxide. To ensure that all the ammonium sulphate reacted, an excess ofsodium hydroxide was used.Heating was continued until all of the ammonia had been driven off as a gas.The unreacted sodium hydroxide remaining in the solution required 27.3 cm3 of0.600moldm–3 hydrochloric acid for neutralisation.

(i) Calculate the original number of moles of NaOH in 100 cm3 of 0.500 mol dm–3

aqueous sodium hydroxide.

.............................................................................................................................................

.............................................................................................................................................

(ii) Calculate the number of moles of HCl in 27.3 cm3 of 0.600 mol dm–3 hydrochloricacid.

.............................................................................................................................................

.............................................................................................................................................

(iii) Deduce the number of moles of the unreacted NaOH neutralised by thehydrochloric acid.

.............................................................................................................................................

(iv) Use your answers from parts (a)(i) and (a)(iii) to calculate the number of moles ofNaOH which reacted with the ammonium sulphate.

.............................................................................................................................................

.............................................................................................................................................

(v) Use your answer in part (a)(iv) to calculate the number of moles and the mass ofammonium sulphate in the sample.(If you have been unable to obtain an answer to part (a)(iv), you may assume thatthe number of moles of NaOH which reacted with ammonium sulphate equals2.78 × 10–2 mol. This is not the correct answer.)

Moles of ammonium sulphate .........................................................................................

.............................................................................................................................................

Mass of ammonium sulphate ..........................................................................................

.............................................................................................................................................(7 marks)

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(b) A 0.143g gaseous sample of ammonia occupied a volume of 2.86 × 10–4 m3 at atemperature T and a pressure of 100kPa.

State the ideal gas equation, calculate the number of moles of ammonia present anddeduce the value of the temperature T.(The gas constant R=8.31JK–1 mol–1)

Ideal gas equation .......................................................................................................................

Moles of ammonia ......................................................................................................................

.......................................................................................................................................................

Value of T ....................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(4 marks)


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3 (a) Magnesium and chlorine react together to form the ionic compound magnesiumchloride, MgCl2.

(i) Explain how each of the ions in this compound is formed.

.............................................................................................................................................

.............................................................................................................................................

(ii) Explain why compounds with ionic bonding tend to have high melting points.

.............................................................................................................................................

.............................................................................................................................................(4 marks)

(b) (i) Define the term electronegativity.

.............................................................................................................................................

.............................................................................................................................................

(ii) Explain why electronegativity increases across a period in the Periodic Table.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................(4 marks)

(c) Chloride ions are polarised more by aluminium ions than they are by magnesium ions.

(i) State what is meant by the term polarised.

.............................................................................................................................................

.............................................................................................................................................

(ii) Why is a chloride ion polarised more by an aluminium ion than by a magnesiumion?

.............................................................................................................................................

.............................................................................................................................................

(iii) Predict the type of bonding in aluminium chloride.

.............................................................................................................................................(5 marks)

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4 (a) Ammonia, NH3, reacts with sodium to form sodium amide, NaNH2, and hydrogen.

(i) Write an equation for the reaction between ammonia and sodium.

.............................................................................................................................................

(ii) Draw the shape of an ammonia molecule and that of an amide ion, NH–2

In each case show any lone pairs of electrons.

NH3 NH–2

(iii) State the bond angle found in an ammonia molecule.

.............................................................................................................................................

(iv) Explain why the bond angle in an amide ion is smaller than that in an ammoniamolecule.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................(6 marks)

(b) A salt, X, contains 16.2% by mass of magnesium, 18.9% by mass of nitrogen and 64.9%by mass of oxygen.

(i) State what is meant by the term empirical formula.

.............................................................................................................................................

.............................................................................................................................................

(ii) Determine the empirical formula of X.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................(3 marks)

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9

CHM1 pgs 1-12 28/9/04 11:07 am Page 9

5 (a) Iodine and diamond are both crystalline solids at room temperature. Identify onesimilarity in the bonding, and one difference in the structures, of these two solids.Explain why these two solids have very different melting points.

(6 marks)

(b) (i) For the elements Mg–Ba, state how the solubilities of the hydroxides and thesolubilities of the sulphates change down Group II.

(ii) Describe a test to show the presence of sulphate ions in an aqueous solution. Givethe results of this test when performed on separate aqueous solutions ofmagnesium chloride and magnesium sulphate. Write equations for any reactionsoccurring.

(iii) State the trend in the reactivity of the Group II elements Mg–Ba with water.Write an equation for the reaction of barium with water.

(9 marks)

END OF QUESTIONS

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CHM1 pgs 1-12 28/9/04 11:07 am Page 12

Surname

Centre Number

Candidate Signature

Candidate Number






a calculator.









• Your answers to the questions in Section B should be written incontinuous prose, where appropriate. You will be assessed on your abilityto use an appropriate form and style of writing, to organise relevantinformation clearly and coherently, and to use specialist vocabulary,where appropriate.




Number

1

2

3

4

5

6

7

Mark Number Mark


TOTAL

Total(Column 2)

Total(Column 1)

APW/0205/CHM1

→

→

CHM1

CHM1 pgs 1-16 for 05 27/10/04 3:26 pm Page 1

APW/0205/CHM1

2LEAVE

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1 A sample of iron from a meteorite was found to contain the isotopes 54Fe, 56Fe and 57Fe.

(a) The relative abundances of these isotopes can be determined using a mass spectrometer.In the mass spectrometer, the sample is first vaporised and then ionised.

(i) State what is meant by the term isotopes.

.............................................................................................................................................

.............................................................................................................................................

(ii) Explain how, in a mass spectrometer, ions are detected and how their abundanceis measured.

How ions are detected ......................................................................................................

.............................................................................................................................................

How abundance is measured ..........................................................................................

.............................................................................................................................................(5 marks)

(b) (i) Define the term relative atomic mass of an element.

.............................................................................................................................................

.............................................................................................................................................

(ii) The relative abundances of the isotopes in this sample of iron were found to be asfollows.

Use the data above to calculate the relative atomic mass of iron in this sample.Give your answer to one decimal place.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................(4 marks)

SECTION A


m/z 54 56 57



1.0

HH

ydro

gen

1

4.0H

eH

eliu

m2

10.8B

Bor

on5

12.0C

Car

bon

6

14.0N

Nitr

ogen

7

16.0O

Oxy

gen

8

19.0

FF

luor

ine

9

20.2 N

eN

eon

10

27.0 A

lA

lum

iniu

m13

28.1 S

iS

ilico

n14

31.0

PP

hosp

horu

s15

32.1

SS

ulph

ur16

35.5 C

lC

hlor

ine

17

39.9 A

rA

rgon

18

6.9

Li

Lith

ium

3

6.9

Li

Lith

ium

3

9.0B

eB

eryl

lium

4

III

IIIIV

VV

IV

II0

*58

– 7

1La

ntha

nide

s

†90

– 1

03A

ctin

ides

Key

rela

tive

atom

ic m

ass

atom

ic n

umbe

r

Th

e P

erio

dic

Tab

le o

f th

e E

lem

ents

�T

he a

tom

ic n

umbe

rs a

nd a

ppro

xim

ate

rela

tive

ato

mic

mas

ses

show

n in

the

tab

le a

re f

or u

se in

the

exa

min

atio

n un

less

sta

ted

othe

rwis

e in

an

indi

vidu

al q

uest

ion.

23.0 N

aS

odiu

m11 39

.1K

Pot

assi

um19

40.1 C

aC

alci

um20

45.0 S

cS

cand

ium

21

47.9 T

iT

itani

um22

50.9

VV

anad

ium

23

52.0 C

rC

hrom

ium

24

54.9 M

nM

anga

nese

25

55.8 F

eIr

on26

58.9 C

oC

obal

t27

58.7 N

iN

icke

l28

63.5 C

uC

oppe

r29

65.4 Z

nZ

inc

30

69.7 G

aG

alliu

m31

72.6 G

eG

erm

aniu

m32

74.9 A

sA

rsen

ic33

79.0 S

eS

elen

ium

34

79.9 B

rB

rom

ine

35

83.8 K

rK

rypt

on36

85.5 R

bR

ubid

ium

37

87.6 S

rS

tron

tium

38

88.9

YY

ttriu

m39

91.2 Z

rZ

ircon

ium

40

92.9 N

bN

iobi

um41

95.9 M

oM

olyb

denu

m42

98.9 T

cTe

chne

tium

43

101.

1 Ru

Rut

heni

um44

102.

9 Rh

Rho

dium

45

106.

4 Pd

Pal

ladi

um46

107.

9 Ag

Silv

er47

112.

4 Cd

Cad

miu

m48

114.

8 InIn

dium

49

118.

7 Sn

Tin

50

121.

8 Sb

Ant

imon

y51

127.

6 TeTe

lluriu

m52

126.

9 IIo

dine

53

131.

3 Xe

Xen

on54

132.

9 Cs

Cae

sium

55

137.

3 Ba

Bar

ium

56

138.

9 La

Lant

hanu

m57

*

178.

5 Hf

Haf

nium

72

180.

9 TaTa

ntal

um73

183.

9 WTu

ngst

en74

186.

2 Re

Rhe

nium

75

190.

2 Os

Osm

ium

76

192.

2 IrIr

idiu

m77

195.

1 Pt

Pla

tinum

78

197.

0 Au

Gol

d79

200.

6 Hg

Mer

cury

80

204.

4 Tl

Tha

llium

81

207.

2 Pb

Lead

82

209.

0 Bi

Bis

mut

h83

210.

0 Po

Pol

oniu

m84

210.

0 At

Ast

atin

e85

222.

0 Rn

Rad

on86

223.

0 Fr

Fran

cium

87

226.

0 Ra

Rad

ium

88

227 A

cA

ctin

ium

89

†

140.

1 Ce

Cer

ium

58

140.

9 Pr

Pras

eody

miu

m59

144.

2 Nd

Neo

dym

ium

60

144.

9 Pm

Pro

met

hium

61

150.

4 Sm

Sam

ariu

m62

152.

0 Eu

Eur

opiu

m63

157.

3 Gd

Gad

olin

ium

64

158.

9 Tb

Terb

ium

65

162.

5 Dy

Dys

pros

ium

66

164.

9 Ho

Hol

miu

m67

167.

3 Er

Erb

ium

68

168.

9 Tm

Thu

lium

69

173.

0 Yb

Ytte

rbiu

m70

175.

0 Lu

Lute

tium

71

232.

0 Th

Tho

rium

90

231.

0 Pa

Pro

tact

iniu

m91

238.

0 UU

rani

um92

237.

0 Np

Nep

tuni

um93

239.

1 Pu

Plu

toni

um94

243.

1 Am

Am

eric

ium

95

247.

1 Cm

Cur

ium

96

247.

1 Bk

Ber

keliu

m97

252.

1 Cf

Cal

iforn

ium

98

(252

) Es

Ein

stei

nium

99

(257

) Fm

Fer

miu

m10

0

(258

) Md

Men

dele

vium

101

(259

) No

Nob

eliu

m10

2

(260

) Lr

Law

renc

ium

103

24.3 M

gM

agne

sium

12

3

APW/0205/CHM1


APW/0205/CHM1



RCH3 0.7–1.2

R2CH2 1.2–1.4

R3CH 1.4–1.6

RCOCH3 2.1–2.6

ROCH3 3.1–3.9

RCOOCH3 3.7–4.1

ROH 0.5–5.0



C—H 2850–3300

C—C 750–1100

C C 1620–1680

C O 1680–1750

C—O 1000–1300


O—H (acids) 2500–3000

4


5LEAVE

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APW/0205/CHM1

(c) (i) Give the electron arrangement of an Fe2+ ion.

.............................................................................................................................................

(ii) State why iron is placed in the d block of the Periodic Table.

.............................................................................................................................................

.............................................................................................................................................

(iii) State the difference, if any, in the chemical properties of isotopes of the sameelement. Explain your answer.

Difference ..........................................................................................................................

Explanation .......................................................................................................................

.............................................................................................................................................(4 marks)


13


APW/0205/CHM1

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2 (a) Lead(II) nitrate may be produced by the reaction between nitric acid and lead(II) oxideas shown by the equation below.

PbO + 2HNO3 → Pb(NO3)2 + H2O

An excess of lead(II) oxide was allowed to react with 175cm3 of 1.50moldm–3 nitric acid.Calculate the maximum mass of lead(II) nitrate which could be obtained from thisreaction.

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(4 marks)

(b) An equation representing the thermal decomposition of lead(II) nitrate is shown below.

2Pb(NO3)2(s) → 2PbO(s) + 4NO2(g) + O2(g)

A sample of lead(II) nitrate was heated until the decomposition was complete. At atemperature of 500K and a pressure of 100kPa, the total volume of the gaseous mixtureproduced was found to be 1.50 × 10– 4 m3.

(i) State the ideal gas equation and use it to calculate the total number of moles of gasproduced in this decomposition.(The gas constant R = 8.31JK–1 mol–1)

Ideal gas equation .............................................................................................................

Total number of moles of gas ..........................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................


7LEAVE

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(ii) Deduce the number of moles, and the mass, of NO2 present in this gaseousmixture. (If you have been unable to calculate the total number of moles of gas inpart (b)(i), you should assume this to be 2.23 × 10–3 mol. This is not the correctanswer.)

Number of moles of NO2 ................................................................................................

.............................................................................................................................................

Mass of NO2 .....................................................................................................................

.............................................................................................................................................(7 marks)


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APW/0205/CHM1

11


3 (a) When aluminium is added to an aqueous solution of copper(II) chloride, CuCl2, coppermetal and aluminium chloride, AlCl3, are formed. Write an equation to represent thisreaction.

.......................................................................................................................................................(1 mark)

(b) (i) State the general trend in the first ionisation energy of the Period 3 elements fromNa to Ar.

.............................................................................................................................................

(ii) State how, and explain why, the first ionisation energy of aluminium does notfollow this general trend.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................(4 marks)

(c) Give the equation, including state symbols, for the process which represents the secondionisation energy of aluminium.

.......................................................................................................................................................(1 mark)

(d) State and explain the trend in the melting points of the Period 3 metals Na, Mg and Al.

Trend ............................................................................................................................................

Explanation .................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(3 marks)

APW/0205/CHM1

8LEAVE

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9


9LEAVE

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4 Phosphorus and nitrogen are in Group V of the Periodic Table and both elements formhydrides. Phosphine, PH3, reacts to form phosphonium ions, PH+

4, in a similar way to that bywhich ammonia, NH3, forms ammonium ions, NH+

4

(a) Give the name of the type of bond formed when phosphine reacts with an H+ ion.Explain how this bond is formed.

Type of bond ...............................................................................................................................

Explanation .................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(3 marks)

(b) Draw the shapes, including any lone pairs of electrons, of a phosphine molecule and of aphosphonium ion.Give the name of the shape of the phosphine molecule and state the bond angle foundin the phosphonium ion.

PH3 PH4+

Shape of PH3 ……………………… Bond angle in PH4+ ………………………

(4 marks)

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APW/0205/CHM1

7


APW/0205/CHM1

10LEAVE

MARGINBLANK

5 (a) Methanol has the structure

Explain why the O–H bond in a methanol molecule is polar.

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(2 marks)

(b) The boiling point of methanol is +65 °C; the boiling point of oxygen is –183 °C.Methanol and oxygen each have an Mr value of 32. Explain, in terms of theintermolecular forces present in each case, why the boiling point of methanol is muchhigher than that of oxygen.

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................

.......................................................................................................................................................(3 marks)

5

O HH C

H

H


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6 Diamond and graphite are both forms of carbon.Diamond is able to scratch almost all other substances, whereas graphite may be used as alubricant.Diamond and graphite both have high melting points.

Explain each of these properties of diamond and graphite in terms of structure and bonding.Give one other difference in the properties of diamond and graphite.

(9 marks)

7 This question concerns the chemistry of the Group II metals Mg to Ba.An aqueous solution of a Group II metal chloride, XCl2, forms a white precipitate when diluteaqueous sodium hydroxide is added. A separate sample of the solution of XCl2 does not forma precipitate when dilute aqueous sodium sulphate is added.

An aqueous solution of a different Group II metal chloride, YCl2, does not form a precipitatewhen dilute aqueous sodium hydroxide is added. A separate sample of the solution of YCl2forms a white precipitate when dilute aqueous sodium sulphate is added.

Suggest identities for the Group II metals X and Y. Write equations, including state symbols,for the reactions which occur.

(6 marks)

END OF QUESTIONS

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APW/0205/CHM1

SECTION B

Answer the questions below in the space provided on pages 11 to 16 of this booklet.


APW/0205/CHM1

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Surname

Centre Number

Candidate Signature

Candidate Number




Wednesday 11 January 2006 9.00 am to 10.00 am


Instructions� Use blue or black ink or ball-point pen.� Fill in the boxes at the top of this page.� Answer all questions.� Answer the questions in Section A and Section B in the spaces

provided.� All working must be shown.� Do all rough work in this book. Cross through any work you do not

want marked.� The Periodic Table/Data Sheet is provided on pages 3 and 4. Detach

this perforated sheet at the start of the examination.

Information� The maximum mark for this paper is 60.� The marks for questions are shown in brackets.� You are expected to use a calculator where appropriate.� The following data may be required.


� Your answers to the question in Section B should be written incontinuous prose, where appropriate.

� You will be assessed on your ability to use an appropriate form andstyle of writing, to organise relevant information clearly andcoherently, and to use specialist vocabulary, where appropriate.

Advice� You are advised to spend about 45 minutes on Section A and about


APW/Jan06/CHM1

For this paper you must have� a calculator

CHM1


1

2

3

4

5

6

Number Mark Number Mark


TOTAL

Total (Column 2)

Total (Column 1)→

→

AQA-CHM1-W-QP-Jan06 21/10/05 11:23 am Page 1

APW/Jan06/CHM1

2 LEAVEMARGINBLANK

SECTION A



(2 marks)

(b) An atom has twice as many protons as, and four more neutrons than, an atom of 9Be.Deduce the symbol, including the mass number, of this atom.

.............................................................................................................................................(2 marks)

(c) Draw the shape of a molecule of BeCl2 and the shape of a molecule of Cl2O. Showany lone pairs of electrons on the central atom. Name the shape of each molecule.

BeCl2 Cl2O

Name of shape ......................................... Name of shape .........................................(4 marks)

(d) The equation for the reaction between magnesium hydroxide and hydrochloric acid isshown below.

Mg(OH)2(s) + 2HCl(aq) → MgCl2(aq) + 2H2O(l)

Calculate the volume, in cm3, of 1.00 mol dm–3 hydrochloric acid required to reactcompletely with 1.00 g of magnesium hydroxide.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................(4 marks)

Relative mass Relative charge

Neutron

Electron

12


3

APW/Jan06/CHM1

1.0

HH

ydro

gen

1

4.0H

eH

eliu

m2

10.8B

Bor

on5

12.0C

Car

bon

6

14.0N

Nitr

ogen

7

16.0O

Oxy

gen

8

19.0

FF

luor

ine

9

20.2 N

eN

eon

10

27.0 A

lA

lum

iniu

m13

28.1 S

iS

ilico

n14

31.0

PP

hosp

horu

s15

32.1

SS

ulph

ur16

35.5 C

lC

hlor

ine

17

39.9 A

rA

rgon

18

6.9

Li

Lith

ium

3

6.9

Li

Lith

ium

3

9.0B

eB

eryl

lium

4

III

IIIIV

VV

IV

II0

*58

– 7

1La

ntha

nide

s

†90

– 1

03A

ctin

ides

Key

rela

tive

atom

ic m

ass

atom

ic n

umbe

r

Th

e P

erio

dic

Tab

le o

f th

e E

lem

ents

�T

he a

tom

ic n

umbe

rs a

nd a

ppro

xim

ate

rela

tive

ato

mic

mas

ses

show

n in

the

tab

le a

re f

or u

se in

the

exa

min

atio

n un

less

sta

ted

othe

rwis

e in

an

indi

vidu

al q

uest

ion.

23.0 N

aS

odiu

m11 39

.1K

Pot

assi

um19

40.1 C

aC

alci

um20

45.0 S

cS

cand

ium

21

47.9 T

iT

itani

um22

50.9

VV

anad

ium

23

52.0 C

rC

hrom

ium

24

54.9 M

nM

anga

nese

25

55.8 F

eIr

on26

58.9 C

oC

obal

t27

58.7 N

iN

icke

l28

63.5 C

uC

oppe

r29

65.4 Z

nZ

inc

30

69.7 G

aG

alliu

m31

72.6 G

eG

erm

aniu

m32

74.9 A

sA

rsen

ic33

79.0 S

eS

elen

ium

34

79.9 B

rB

rom

ine

35

83.8 K

rK

rypt

on36

85.5 R

bR

ubid

ium

37

87.6 S

rS

tron

tium

38

88.9

YY

ttriu

m39

91.2 Z

rZ

ircon

ium

40

92.9 N

bN

iobi

um41

95.9 M

oM

olyb

denu

m42

98.9 T

cTe

chne

tium

43

101.

1 Ru

Rut

heni

um44

102.

9 Rh

Rho

dium

45

106.

4 Pd

Pal

ladi

um46

107.

9 Ag

Silv

er47

112.

4 Cd

Cad

miu

m48

114.

8 InIn

dium

49

118.

7 Sn

Tin

50

121.

8 Sb

Ant

imon

y51

127.

6 TeTe

lluriu

m52

126.

9 IIo

dine

53

131.

3 Xe

Xen

on54

132.

9 Cs

Cae

sium

55

137.

3 Ba

Bar

ium

56

138.

9 La

Lant

hanu

m57

*

178.

5 Hf

Haf

nium

72

180.

9 TaTa

ntal

um73

183.

9 WTu

ngst

en74

186.

2 Re

Rhe

nium

75

190.

2 Os

Osm

ium

76

192.

2 IrIr

idiu

m77

195.

1 Pt

Pla

tinum

78

197.

0 Au

Gol

d79

200.

6 Hg

Mer

cury

80

204.

4 Tl

Tha

llium

81

207.

2 Pb

Lead

82

209.

0 Bi

Bis

mut

h83

210.

0 Po

Pol

oniu

m84

210.

0 At

Ast

atin

e85

222.

0 Rn

Rad

on86

223.

0 Fr

Fran

cium

87

226.

0 Ra

Rad

ium

88

227 A

cA

ctin

ium

89

†

140.

1 Ce

Cer

ium

58

140.

9 Pr

Pras

eody

miu

m59

144.

2 Nd

Neo

dym

ium

60

144.

9 Pm

Pro

met

hium

61

150.

4 Sm

Sam

ariu

m62

152.

0 Eu

Eur

opiu

m63

157.

3 Gd

Gad

olin

ium

64

158.

9 Tb

Terb

ium

65

162.

5 Dy

Dys

pros

ium

66

164.

9 Ho

Hol

miu

m67

167.

3 Er

Erb

ium

68

168.

9 Tm

Thu

lium

69

173.

0 Yb

Ytte

rbiu

m70

175.

0 Lu

Lute

tium

71

232.

0 Th

Tho

rium

90

231.

0 Pa

Pro

tact

iniu

m91

238.

0 UU

rani

um92

237.

0 Np

Nep

tuni

um93

239.

1 Pu

Plu

toni

um94

243.

1 Am

Am

eric

ium

95

247.

1 Cm

Cur

ium

96

247.

1 Bk

Ber

keliu

m97

252.

1 Cf

Cal

iforn

ium

98

(252

) Es

Ein

stei

nium

99

(257

) Fm

Fer

miu

m10

0

(258

) Md

Men

dele

vium

101

(259

) No

Nob

eliu

m10

2

(260

) Lr

Law

renc

ium

103

24.3 M

gM

agne

sium

12


APW/Jan06/CHM1

4



RCH3 0.7–1.2

R2CH2 1.2–1.4

R3CH 1.4–1.6

RCOCH3 2.1–2.6

ROCH3 3.1–3.9

RCOOCH3 3.7–4.1

ROH 0.5–5.0



C—H 2850–3300

C—C 750–1100

C C 1620–1680

C O 1680–1750

C—O 1000–1300


O—H (acids) 2500–3000


5 LEAVEMARGINBLANK

Turn over �APW/Jan06/CHM1

10

2 Potassium nitrate, KNO3, decomposes on strong heating, forming oxygen and solid Y as theonly products.

(a) A 1.00 g sample of KNO3 (Mr = 101.1) was heated strongly until fully decomposedinto Y.

(i) Calculate the number of moles of KNO3 in the 1.00 g sample.

...................................................................................................................................

...................................................................................................................................

(ii) At 298 K and 100 kPa, the oxygen gas produced in this decomposition occupied avolume of 1.22 × 10–4 m3.State the ideal gas equation and use it to calculate the number of moles ofoxygen produced in this decomposition.(The gas constant R = 8.31 J K–1 mol–1)

Ideal gas equation ....................................................................................................

Moles of oxygen ........................................................................................................

...................................................................................................................................

...................................................................................................................................

...................................................................................................................................

...................................................................................................................................(5 marks)

(b) Compound Y contains 45.9 % of potassium and 16.5 % of nitrogen by mass, theremainder being oxygen.

(i) State what is meant by the term empirical formula.

...................................................................................................................................

...................................................................................................................................

(ii) Use the data above to calculate the empirical formula of Y.

...................................................................................................................................

...................................................................................................................................

...................................................................................................................................(4 marks)

(c) Deduce an equation for the decomposition of KNO3 into Y and oxygen.

.............................................................................................................................................(1 mark)


APW/Jan06/CHM1

6 LEAVEMARGINBLANK

3 The table below shows the electronegativity values of some elements.

(a) Define the term electronegativity.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................(2 marks)

(b) The table below shows the boiling points of fluorine, fluoromethane (CH3F) andhydrogen fluoride.

(i) Name the strongest type of intermolecular force present in:

Liquid F2 ...................................................................................................................

Liquid CH3F .............................................................................................................

Liquid HF .................................................................................................................

(ii) Explain how the strongest type of intermolecular force in liquid HF arises.

...................................................................................................................................

...................................................................................................................................

...................................................................................................................................

...................................................................................................................................(6 marks)

Fluorine Chlorine Bromine Iodine Carbon Hydrogen

Electronegativity 4.0 3.0 2.8 2.5 2.5 2.1

Boiling point / K 85 194 293

F—F

F

CH H

H

H—F


7 LEAVEMARGINBLANK

(c) The table below shows the boiling points of some other hydrogen halides.

(i) Explain the trend in the boiling points of the hydrogen halides from HCl to HI.

...................................................................................................................................

...................................................................................................................................

...................................................................................................................................

(ii) Give one reason why the boiling point of HF is higher than that of all the otherhydrogen halides.

...................................................................................................................................

...................................................................................................................................(3 marks)

Turn over for the next question


11

HCl HBr HI

Boiling point / K 188 206 238


APW/Jan06/CHM1

8 LEAVEMARGINBLANK

4 (a) State the meaning of the term first ionisation energy of an atom.

.............................................................................................................................................

.............................................................................................................................................

.............................................................................................................................................(2 marks)

(b) Complete the electron arrangement for the Mg2+ ion.

1s2 ......................................................................................................................................(1 mark)

(c) Identify the block in the Periodic Table to which magnesium belongs.

.............................................................................................................................................(1 mark)

(d) Write an equation to illustrate the process occurring when the second ionisation energyof magnesium is measured.

.............................................................................................................................................(1 mark)

(e) The Ne atom and the Mg2+ ion have the same number of electrons. Give two reasonswhy the first ionisation energy of neon is lower than the third ionisation energy ofmagnesium.

Reason 1 .............................................................................................................................

Reason 2 .............................................................................................................................(2 marks)


9 LEAVEMARGINBLANK

(f) There is a general trend in the first ionisation energies of the Period 3 elements, Na – Ar

(i) State and explain this general trend.

Trend .........................................................................................................................

Explanation ..............................................................................................................

...................................................................................................................................

...................................................................................................................................

(ii) Explain why the first ionisation energy of sulphur is lower than would bepredicted from the general trend.

...................................................................................................................................

...................................................................................................................................

...................................................................................................................................(5 marks)

Turn over for the next question


12


APW/Jan06/CHM1

10 LEAVEMARGINBLANK

SECTION B

Answer both questions in the space provided on pages 10–12 of this booklet.

5 A sample of element Q was extracted from a meteorite. The table below shows the relativeabundance of each isotope in a mass spectrum of this sample of Q.

(a) Define the term relative atomic mass of an element. (2 marks)

(b) Use the data above to calculate the relative atomic mass of this sample of Q. Giveyour answer to one decimal place. Suggest the identity of Q. (3 marks)

(c) In order to obtain a mass spectrum of Q, a gaseous sample is first ionised. Describehow ionisation is achieved in a mass spectrometer. Give three reasons why ionisationis necessary. (5 marks)

6 Phosphorus exists in several different forms, two of which are white phosphorus and redphosphorus. White phosphorus consists of P4 molecules, and melts at 44 °C.Red phosphorus is macromolecular, and has a melting point above 550 °C.

Explain what is meant by the term macromolecular. By considering the structure andbonding present in these two forms of phosphorus, explain why their melting points are sodifferent. (5 marks)

END OF QUESTIONS

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m/z 64 66 67 68

Relative abundance (%) 38.9 27.8 14.7 18.6


11 LEAVEMARGINBLANK

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APW/Jan06/CHM1

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Surname

Centre Number

Candidate Signature

Candidate Number






a calculator.









• Your answers to the questions in Section B should be written incontinuous prose, where appropriate. You will be assessed on your abilityto use an appropriate form and style of writing, to organise relevantinformation clearly and coherently, and to use specialist vocabulary,where appropriate.




Number

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2

3

4

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Mark Number Mark


TOTAL

Total(Column 2)

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APW/0205/CHM1

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→

CHM1
