Questions

Q1.

Bonding and separation techniques

(a) The diagram shows the structure of diamond.

(i) Describe what each represents.

(2)

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(ii) State the type of bonding in the diamond structure.

(1)

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(b) Give the name of the process used to obtain oxygen from liquid air.

(2)

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(c) A colouring in some sweets was analysed using paper chromatography.

One of the dyes in the colouring moved 2 cm up the paper while the solvent moved 8 cm.

What is the Rf value of this dye?

Put a cross ( ) in the box next to your answer.

(1)

A 0.25

B 2

C 4

D 6

*(d) Here is some information about magnesium, oxygen and magnesium oxide.

The electronic configuration of magnesium atoms is 2.8.2The electronic configuration of oxygen atoms is 2.6Magnesium oxide is an ionic compound.

When magnesium ribbon is heated, it reacts with oxygen from the air to form magnesium oxide,MgO.

Describe how the reaction can be carried out, including an explanation of what happens to themagnesium and oxygen atoms when they form magnesium oxide.

(6)

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(Total for question = 12 marks)

Q2.

(a) Calcium oxide is manufactured by heating calcium carbonate.

The waste product of this process is carbon dioxide.

(i) Calculate the relative formula mass of carbon dioxide, CO2. (Relative atomic masses: C = 12, O = 16)

(1)

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relative formula mass = . . . . . . . . . . . . . . . . . . . . .

(ii) The equation for the reaction is

CaCO3(s) → CaO(s) + CO2(g)

Calculate the maximum mass of calcium oxide that can be obtained by heating 25tonnes of calcium carbonate. (Relative atomic masses: C = 12, O = 16, Ca = 40)

(3)

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mass calcium oxide = . . . . . . . . . . . . . . . . . . . . . . tonnes

(b) (i) State what is meant by theoretical yield.

(1)

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(ii) Explain why the actual yield for a reaction is usually less than the theoretical yield forthe reaction.

(2)

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(c) Many industrial processes produce waste products.

Suggest reasons why manufacturers try to find uses for these waste products.

(2)

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(Total for Question is 9 marks)

Q3.

Compounds

(a) (i) Balance the equation for the reaction between sodium and chlorine to produce sodiumchloride by putting numbers in the spaces provided.

(2)

.................. Na + Cl2 → .................. NaCl

(ii) In an experiment to make sodium chloride, the yield is 2.5 g.The theoretical yield of sodium chloride for this experiment is 4.0 g.

Calculate the percentage yield of sodium chloride in this experiment.

(2)

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percentage yield = ........................................................... %

(iii) Sodium chloride has a high melting point.Sodium chloride does not conduct electricity when solid but does conduct electricity whenmolten.

Complete the sentence by putting a cross ( ) in the box next to your answer.

These properties show that the structure of sodium chloride is

(1)

A ionic

B giant molecular, covalent

C simple molecular, covalent

D metallic

(iv) Calculate the relative formula mass of sodium chloride, NaCl. (relative atomic masses: Na =23, Cl = 35.5)

(1)

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relative formula mass = ...........................................................

(b) Calculate the percentage by mass of magnesium in magnesium sulfate, MgSO4.

(relative atomic masses: O = 16, Mg = 24, S = 32

relative formula mass: MgSO4 = 120)

(2)

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percentage of magnesium = ........................................................... %

(c) The formula of a molecule of ethane is C2H6.

(i) Give the empirical formula of ethane.

(1)

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(ii) Ethane is a simple molecular, covalent compound.

Ethane has a low boiling point.

Explain, in terms of particles it contains, why ethane has a low boiling point.

(2)

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(Total for question = 11 marks)

Q4. Copper and its compounds

(a) Copper is a transition metal.

Which of these is a property of copper?

Put a cross ( ) in the box next to your answer.

(1)

A it is a poor conductor of electricity

B it is brittle

C it has a low melting point

D it forms coloured compounds

(b) Jasmine reacted an oxide of copper with carbon.

copper oxide + carbon → copper + carbon dioxide

She reacted 5.0 g of copper oxide.

In her reaction, 2.8 g of copper was formed.

The theoretical yield for this reaction is 4.0 g.

(i) State what is meant by the term theoretical yield.

(1)

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(ii) The percentage yield of Jasmine’s experiment was 70%.

Explain how this value was calculated.

(2)

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(iii) State two reasons why the yield of Jasmine’s experiment was not 100%.

(2)

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(c) Calculate the relative formula mass of copper chloride, CuCl2.

(Relative atomic masses: Cu = 63.5, Cl = 35.5)

(1)

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answer = ................................................................

(d) 14.3 g of an oxide of copper contained 12.7 g of copper.

Calculate the empirical formula of this oxide.

Show your working.

(Relative atomic masses: Cu = 63.5, O = 16)

(3)

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answer = .........................................................................

Q5.

Group 7 elements

(a) A compound of iron and chlorine was formed by reacting 2.80 g of iron with 3.55 g ofchlorine.

Calculate the empirical formula of the compound.(relative atomic masses: Cl = 35.5, Fe = 56.0)

(3)

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empirical formula ...........................................................

(b) Sodium reacts with chlorine to form sodium chloride.

2Na + Cl2 → 2NaCl

Calculate the maximum mass of sodium chloride that could be formed by reacting 9.20 g ofsodium with excess chlorine.(relative atomic masses: Na = 23.0, Cl = 35.5)

(3)

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mass of sodium chloride ........................................................... g

*(c) Chlorine, bromine and iodine are in group 7 of the periodic table.

The order of reactivity of these three elements can be shown by carrying out displacementexperiments.

You are provided with

potassium bromide solutionpotassium chloride solutionpotassium iodide solutionbromine solutionchlorine solutioniodine solution

Describe how these solutions could be used to carry out experiments to show the order ofreactivity of bromine, chlorine and iodine, explaining how the results would show the order ofreactivity.You may use equations if you wish.

(6)

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(Total for question = 12 marks)

Q6.

The diagram shows a piece of magnesium ribbon being heated.

During the heating, the magnesium reacts with oxygen from the air.The lid of the crucible was raised slightly from time to time.Magnesium oxide was formed as a white powder.The experiment was repeated with different masses of magnesium.

The table shows the mass of magnesium used and the mass of the magnesium oxide formed ineach experiment.

experiment mass ofmagnesium

used /g

mass ofmagnesium

oxide formed

mass ofoxygen in

magnesium

/g oxide /g1 0.10 0.16 0.062 0.15 0.24 0.093 0.25 0.40 0.154 0.30 0.48 0.185 0.35 0.49 0.146 0.50 0.80 0.30

(a) Suggest why the lid had to be raised from time to time during the experiment.

(1)

(b) (i) On the grid provided, draw a graph of the mass of oxygen in magnesium oxide against themass of magnesium used.

(3)

(ii) The result of experiment 5 is anomalous. The masses were all measured accurately.

Suggest what might have caused this anomalous result.

(1)

(c) Write the balanced equation for the reaction of magnesium with oxygen to form magnesiumoxide.

(3)

(d) An oxide of lead was analysed. 0.414 g of lead was combined with 0.064 g of oxygen in this oxide.

Calculate the empirical formula of this lead oxide.

(relative atomic masses: O = 16, Pb = 207)

(3)

empirical formula . . . . . . . . . . . . . . . . . . . .

(Total for Question is 11 marks)

Q7.

(a) Calcium chloride solution reacts with silver nitrate solution. Solid silver chloride and calcium nitrate solution are formed.

(i) Complete the sentence by putting a cross ( ) in the box next to your answer.

The formula of a salt is Ca(NO3)2.

The name of this salt is

(1)

A calcium nitride

B calcium nitrate

C calcium chloride

D silver nitrate

(ii) The mixture produced in the reaction is filtered to obtain the silver chloride. The solid silver chloride is washed with water and left to dry. The yield of dry silver chloride was 3.0 g.

The theoretical yield of dry silver chloride in this experiment was 4.0 g.

1. Suggest why the yield was less than 4.0 g.

(2)

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2. Calculate the percentage yield of this experiment.

(2)

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(b) (i) Calculate the relative formula mass of silver chloride, AgCl.

(relative atomic masses: Cl = 35.5, Ag = 108)

(1)

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relative formula mass = . . . . . . . . . . . . . . . . . . . .

(ii) Calculate the percentage by mass of silver, Ag, in silver chloride, AgCl.

(relative atomic masses: Cl = 35.5, Ag = 108)

(2)

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(Total for Question is 8 marks)

Q8.

(a) A separating funnel is shown.

The separating funnel can be used to separate two immiscible liquids, such as oil and water.

Describe how you would use a separating funnel to separate two immiscible liquids.

(2)

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(b) Paper chromatography can be used to separate coloured substances.

A student carried out a chromatography experiment on four food colourings.The four food colourings were brown, green, yellow and red.

The diagram shows the results.

Use the results of the chromatography experiment to describe the colours present in the brownfood colouring.

(2)

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(c) An experiment is carried out on two solutions to see if they conduct electricity.

The apparatus used is shown.

The two solutions used are sodium chloride solution and sucrose solution.Sodium chloride is an ionic compound.Sucrose is a simple molecular, covalent compound.

Explain what happens when each solution is tested in the circuit shown.

(3)

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(d) Calculate the relative formula mass of water, H2O.

(Relative atomic masses: H = 1.0, O = 16)

(1)

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relative formula mass = ...........................................................

(Total for Question = 8 marks)

Mark Scheme

Q1.

Q2.

Answer Acceptable answers Mark(a)(i) 12 + 16 +16 (= 44) 44 with no working (1)(a)(ii) 40+12+(3×16)/(CaCO3)100 (1)

gives 40+16 /(CaO) 56 (1)

25 (tonnes) gives 56×25 (tonnes) (1) 100

allow ecf14 (tonnes)correct answer no working (3)

(3)

(b(i) theoretical yield is calculated yield/value calculated from balancedequation/maximum yieldpossible/maximum amount of productwhen reactants have fully reacted.

(1)

(b)(ii) An explanation linking two of the (2)

following

reaction may be incomplete

product/reactant lost

other (side-)reactions mayoccur

impure reactants

unwanted reactions

(c) A suggestion including two of thefollowing

save money/improveprofit/disposal of waste costsmoney (1)

waste product may be harmfulto the environment/causepollution/damage theenvironment (1)

any specific examples

ignore references to landfill

(2)

(Total for question = 9 marks)

Q3.

Q4.

QuestionNumber

Answer Acceptable answers Mark

(a) D (1)

QuestionNumber

Answer Acceptable answers Mark

(b)(i) the mass (of product)is calculated (from thebalanced equation) (1)

(1)

QuestionNumber

Answer Acceptable answers Mark

(b)(ii)

× 100 (1)

allow formuladescribed in words

(2)

QuestionNumber

Answer Acceptable answers Mark

(b)(iii) Any two from thefollowing points

• loss of productduring experiment (1)

• reaction does notcomplete (1)

• not enough carbonin mixture (1)

• other (unwanted)reactions occur (1)

(2)

QuestionNumber

Answer Acceptable answers Mark

(c) 63.5 + (2 × 35.5) /134.5 (1)

(1)

QuestionNumber

Answer Acceptable answers Mark

(d) • mass of oxygen =14.3 � 12.7 (1)

=1.6

copper atoms: oxygenatoms =

12.7/63.5 : 1.6/16 (1)

0.2 : 0.1

• Cu2O (1)

(3)

Answer Acceptable answers Mark(a) to allow air/oxygen in to ensure magnesium

reacts/burns / combusts(1)

(b)(i) all points correctly plotted to halfa small square (2)line of best fit (1)

Allow one mark for four or fivecorrectly plotted pointsecf their points

(3)

(b)(ii) Any one from

not all magnesium {burned /reacted} / some left / incompletereactionnot enough air/oxygensome magnesium oxide / smoke lost

lid not lifted / not enough times lid leftoff too long (so loses MgO)

(1)

(c) 2Mg + O2 → 2MgOleft hand formulae (1)right hand formula (1)balancing correct formulae (1)

correct multiples (3)

(d) 0.414 / 207 or 0.064 / 16 (1)

0.002 : 0.004 or 1 : 2 (1)empirical formula PbO2 (1)

if 207 / 0.414 and 16 / 0.064ratio 500 : 250 or 2 : 1 (1)empirical formula Pb2O (1)

allow 3 marks for0.414 / 207 or 0.064 / 32ratio 1 : 1empirical formula PbO2

allow 2 marks forif 0.414 / 207 and 0.064 / 32ratio 1 : 1empirical formula PbO

(3)

Answer Acceptable answers Mark(a)(i) B calcium nitrate (1)

(a)(ii)1 A suggestion to include two from:

the reaction was incomplete (1)

unwanted reaction(s) / side reactionstook place (1)

some was lost (in transfer) / left in thebeaker (1)

some of the solid remained on thefilter paper (1)

ignore some of reactant solutions lost

spillagewashed away

lost in filtering

(2)

(a)(ii)2 3.0/4.0 (1)(any fraction) &times 100 (1) (= 75 %)

¾75(%) only scores 2 marks

(2)(b)(i) 108 + 35.5 (1) (= 143.5) 143.5 with no working scores the mark(1)(ii) 108/answer to (b)(i) (1)

(any fraction) × 100 (1) (= 75.261 %)× 100 (1)

If no working allow 2 marks for 75or 75.3 or 75.2 or 75.26 or 75.261 (%)

(2)

Answer Acceptable answers Mark(a) A description to include two from

allow layers to {form /

ignore inverted

(2)

separate} / liquids toseparate(1)operate tap / OWTTE(1)run out one layer / OWTTE(1)pour remaining upper layerfrom top / run out secondlayer(1)

oil/water layers

discard interface

(b) A description to include

green (1)(and) red (1)

{combination of /mixture of / two}colours (1)note: if all three coloursmentioned (1)

(2)

(c) An explanation to include three from

{sodium chloride / ioniccompound} – bulb lights /{sucrose / covalentcompound} – bulb does notlight up (1)

sodium chloride (solution){conducts / ions present} (1)

sucrose (solution) {does notconduct / no ions present (1)

ignore references toelectrolytic processes

circuit will work (inplace of bulb lights) /ORA

(3)

(d) 2x1 + 16 (=18) (1)

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