1. Which property increases down group 1?

A. First ionization energy

B. Melting point

C. Reactivity

D. Electronegativity(Total 1 mark)

2. (i) Define the term first ionization energy.

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

(ii) Explain why the first ionization energy of magnesium is higher than that of sodium.

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

(Total 4 marks)

3. Samples of sodium oxide and sulfur trioxide are added to separate beakers of water.Deduce the equation for each reaction and identify each oxide as acidic, basic or neutral.

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

4. Carbon and silicon belong to the same group of the periodic table.

(a) Distinguish between the terms group and period in terms of electron arrangement.

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

(b) State the period numbers of both carbon and silicon.

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

(Total 3 marks)

5. Which statement about the elements in group 7 is correct?

A. Br2 will oxidize Cl–.

B. F2 has the least tendency to be reduced.

C. Cl2 will oxidize I–.

D. I2 is a stronger oxidizing agent than F2.(Total 1 mark)

6. Which electron transitions are responsible for the colours of transition metal compounds?

A. Between d orbitals and s orbitals

B. Among the attached ligands

C. From the metal ion to the attached ligands

D. Between d orbitals(Total 1 mark)

7. Which change explains why the boiling points of the halogens increase as their molecular masses increase?

A. The intermolecular attraction due to temporarily induced dipoles increases.

B. The gravitational attraction between molecules increases.

C. The polarity of the bond within the molecule increases.

D. The strength of the bond within the molecule increases.(Total 1 mark)

8. Which pair of elements has the greatest difference in electronegativity?

A. Cs and F

B. Cs and Cl

C. Cs and Br

D. Cs and I(Total 1 mark)

9. Ligands can form dative covalent bonds with metal ions to form complex ions. Which of the following can act as a ligand?

I. Cl–

II. NH3

III. H2O

A. I and II only

B. I and III only

C. II and III only

D. I, II and III(Total 1 mark)

10. Which metal nitrate solution is coloured?

A. Zn (NO3)2(aq)

B. Ni (NO3)2(aq)

C. Mg (NO3)2(aq)

D. Sc (NO3)3(aq)(Total 1 mark)

11. When concentrated hydrochloric acid is added to a solution containing hydrated copper(II) ions, the colour of the solution changes from light blue to green. The equation for the reaction is:

[Cu(H2O)6]2+(aq) + 4Cl–(aq) → [CuCl4]2–(aq) + 6H2O(l)

(i) Explain what the square brackets around the copper containing species represent.

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

(ii) Explain why the [Cu(H2O)6]2+ ion is coloured and why the [CuCl4]2– ion has a different colour.

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

(Total 3 marks)

12. State the equations for the reactions of sodium oxide, Na2O, and phosphorus(V) oxide, P4O10, with water.

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

13. Which statements about the periodic table are correct?

I. Elements in period 3 have similar chemical properties.

II. Elements in group 7 show a gradual change in physical properties.

III. The position of an element in period 3 is related to the number of electrons in the highest occupied energy level.

A. I and II only

B. I and III only

C. II and III only

D. I, II and III(Total 1 mark)

14. Which statements about period 3 are correct?

I. The electronegativity of the elements increases across period 3.

II. The atomic radii of the elements decreases across period 3.

III. The oxides of the elements change from acidic to basic across period 3.

A. I and II only

B. I and III only

C. II and III only

D. I, II and III(Total 1 mark)

15. (a) State a balanced equation for the reaction of sodium with water. Include state symbols.(2)

(b) With reference to electronic arrangements, suggest why the reaction between rubidium and water is more vigorous than that between sodium and water.

(2)(Total 4 marks)

16. Describe and explain what you will see if chlorine gas is bubbled through a solution of

(i) potassium iodide.(2)

(ii) potassium fluoride.(1)

(Total 3 marks)

17. Explain why the melting points of the elements decrease down group 1 and increase down group 7.(Total 4 marks)

18. Which statements are correct for the complex ion [CuCl4]2–?

I. The oxidation number of Cu in the complex ion is +2.

II. The coordination number of the copper ion is 4.

III. Chloride ions are behaving as ligands.

A. I and II only

B. I and III only

C. II and III only

D. I, II and III(Total 1 mark)

19. Explain why copper is considered a transition metal while scandium is not.(Total 3 marks)

20. (i) Compare the structure and bonding in AlCl3 and Al2O3.(2)

(ii) Describe the acid-base behaviour of AlCl3, Na2O and P4O10. Include suitable equations in your answer.

(4)

(iii) Explain whether AlCl3 and Al2O3 will conduct in the solid or molten state.(3)

(Total 9 marks)

21. Which property decreases down group 7 in the periodic table?

A. Melting point

B. Electronegativity

C. Atomic radius

D. Ionic radius(Total 1 mark)

22. Which oxides produce an acidic solution when added to water?

I. P4O10

II. MgO

III. SO3

A. I and II only

B. I and III only

C. II and III only

D. I, II and III(Total 1 mark)

23. Consider the bonding and structure of the period 3 elements.

(a) Explain the increase in the melting point from sodium to aluminium.

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

(b) Explain why sulfur, S8, has a higher melting point than phosphorus, P4.

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

(c) Explain why silicon has the highest melting point and argon has the lowest melting point.

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

(Total 6 marks)

24. The periodic table shows the relationship between electron arrangement and the properties of elements and is a valuable tool for making predictions in chemistry.

(i) Identify the property used to arrange the elements in the periodic table.(1)

(ii) Outline two reasons why electronegativity increases across period 3 in the periodic table and one reason why noble gases are not assigned electronegativity values.

(3)(Total 4 marks)

25. (i) Define the term first ionization energy of an atom.(2)

(ii) Explain the general increasing trend in the first ionization energies of the period 3 elements, Na to Ar.

(2)

(iii) Explain why sodium conducts electricity but phosphorus does not.(2)

(Total 6 marks)

26. Which ion has the largest radius?

A. Cl–

B. K+

C. Br–

D. F–

(Total 1 mark)

27. What is the ligand in the complex K3[Fe(CN)6]?

A. CN–

B. Fe3+

C. K+

D. [Fe(CN)6]3–

(Total 1 mark)

28. (i) Outline two reasons why a sodium ion has a smaller radius than a sodium atom.(2)

(ii) Explain why the ionic radius of P3– is greater than the ionic radius of Si4+.(2)

(Total 4 marks)

29. (i) Explain why the first ionization energy of aluminium is lower than the first ionization energy of magnesium.

(2)

(ii) Explain why the first ionization energy of sulfur is lower than the first ionization energy of phosphorus.

(2)(Total 4 marks)

30. The ten elements in the first-row d-block have characteristic properties and many uses.

(i) State and explain the type of reaction that takes place between Fe3+ and H2O to form [Fe(H2O)6]3+ in terms of acid-base theories.

(2)

(ii) Explain why [Fe(H2O)6]3+ is coloured.(3)

(Total 5 marks)

31. Which properties of the alkali metals decrease going down group 1?

A. First ionization energy and reactivity

B. Melting point and atomic radius

C. Reactivity and electronegativity

D. First ionization energy and melting point(Total 1 mark)

32. Which statements about the periodic table are correct?

I. The elements Mg, Ca and Sr have similar chemical properties.

II. Elements in the same period have the same number of main energy levels.

III. The oxides of Na, Mg and P are basic.

A. I and II only

B. I and III only

C. II and III only

D. I, II and III(Total 1 mark)

33. The x-axis of the graph below represents the atomic number of the elements in period 3.

Which variable could represent the y-axis?

A. Melting point

B. Electronegativity

C. Ionic radius

D. Atomic radius(Total 1 mark)

34. In which complexes does iron have an oxidation number of +3?

I. [Fe(H2O)6]3+

II. [Fe(H2O)5(CN)]2+

III. [Fe(CN)6]3–

A. I and II only

B. I and III only

C. II and III only

D. I, II and III(Total 1 mark)

35. Explain the origin of colour in transition metal complexes and use your explanation to suggest why copper(II) sulfate, CuSO4(aq), is blue, but zinc sulfate, ZnSO4(aq), is colourless.

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

36. Cu2+(aq) reacts with ammonia to form the complex ion [Cu(NH3)4]2+. Explain this reaction in terms of an acid-base theory, and outline how the bond is formed between Cu2+ and NH3.

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

37. (i) State whether aqueous solutions of magnesium oxide and magnesium chloride are acidic, alkaline or neutral.

(1)

(ii) State an equation for the reaction between magnesium oxide and water.(1)

(Total 2 marks)

38. How many protons, neutrons and electrons are present in each atom of 31P?

Protons Neutrons Electrons

A. 16 15 16

B. 15 16 15

C. 15 31 15

D. 16 31 16(Total 1 mark)

39. An element is in group 4 and period 3 of the periodic table. How many electrons are in the highest occupied energy level of an atom of this element?

A. 3

B. 4

C. 12

D. 14(Total 1 mark)

40. Which is the best definition of electronegativity?

A. Electronegativity is the energy required for a gaseous atom to gain an electron.

B. Electronegativity is the attraction of an atom for a bonding pair of electrons.

C. Electronegativity is the attraction between the nucleus and the valence electrons of an atom.

D. Electronegativity is the ability of an atom to attract electrons from another atom.(Total 1 mark)

41. Sodium oxide, Na2O, is a white solid with a high melting point.

(a) Explain why solid sodium oxide is a non-conductor of electricity.

(b) Molten sodium oxide is a good conductor of electricity. State the half-equation for the reaction occurring at the positive electrode during the electrolysis of molten sodium oxide.

(c) (i) State the acid-base nature of sodium oxide.

(ii) State the equation for the reaction of sodium oxide with water.

(Total 4 marks)

42. The graph of the first ionization energy plotted against atomic number for the first twenty elements shows periodicity.

(i) Define the term first ionization energy and state what is meant by the term periodicity.(2)

(ii) State the electron arrangement of argon and explain why the noble gases, helium, neon and argon show the highest first ionization energies for their respective periods.

(3)

(iii) A graph of atomic radius plotted against atomic number shows that the atomic radius decreases across a period. Explain why chlorine has a smaller atomic radius than sodium.

(1)

(iv) Explain why a sulfide ion, S2–, is larger than a chloride ion, Cl–.(1)

(v) Explain why the melting points of the Group 1 metals (Li → Cs) decrease down the group whereas the melting points of the Group 7 elements (F → I) increase down the group.

(3)(Total 10 marks)

43. Which statements are correct for the reactions of Cl2, MgCl2 and SiCl4 with water?

Cl2 MgCl2 SiCl4

A. forms a neutral solution

forms a neutral solution

no reaction

B. forms an acidic solution

forms an acidic solution

forms an acidic solution

C. forms an acidic solution

forms an acidic solution

no reaction

D. forms a neutral solution

forms a neutral solution

forms an acidic solution

(Total 1 mark)

44. Which transition element, or compound of a transition element, is used as a catalyst in the Contact process?

A. Fe

B. MnO2

C. V2O5

D. Ni

(Total 1 mark)

45. Deduce the oxidation number of cobalt in the following species.

(i) [Co(H2O)6]2+

(1)

(ii) Co2(SO4)3(1)

(iii) [CoCl4]2–

(1)(Total 3 marks)

46. (i) State the full electronic configurations of copper, Cu, and the copper(I) ion, Cu+.(2)

(ii) Explain why copper(II) compounds in aqueous solution are coloured whereas scandium(III) compounds in aqueous solution are colourless.

(2)(Total 4 marks)

47. Which statement describes the trends of electronegativity values in the periodic table?

A. Values increase from left to right across a period and increase down a group.

B. Values increase from left to right across a period and decrease down a group.

C. Values decrease from left to right across a period and increase down a group.

D. Values decrease from left to right across a period and decrease down a group.(Total 1 mark)

48. Which statement is correct for all elements in the same period?

A. They have the same number of electrons in the highest occupied energy level.

B. They have the same chemical reactivity.

C. They have the same number of occupied energy levels.

D. They have the same number of neutrons.

(Total 1 mark)

49. Some of the most important processes in chemistry involve acid-base reactions.

(a) Describe the acid-base character of the oxides of each of the period 3 elements, Na to Cl.

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

(b) State one example of an acidic gas, produced by an industrial process or the internal combustion engine, which can cause large-scale pollution to lakes and forests.

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

(c) Suggest one method, other than measuring pH, which could be used to distinguish between solutions of a strong acid and a weak acid of the same molar concentration.State the expected results.

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

(Total 6 marks)

50. Which equation best represents the first ionization energy of magnesium?

A. Mg(s) → Mg+(s) + e–

B. Mg(g) → Mg2+(g) + 2e–

C. Mg(g) → Mg+(g) + e–

D. Mg(s) → Mg+(g) + e–

(Total 1 mark)

51. What are the products of the reaction between chlorine and water?

A. O2, H2 and HCl

B. H2 and OCl2

C. HCl and HOCl

D. HOCl, H2 and Cl2(Total 1 mark)

52. (a) (i) Draw the shape of the pz orbital using the coordinates shown.

(1)

(ii) State the electron configuration of Fe3+.

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

(iii) Define the term ligand.

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

(iv) Explain why the complex [Fe(H2O)6]3+ is coloured.

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

(v) The element selenium (Z = 34) has electrons in the 4s, 3d and 4p orbitals. Draw an orbital box diagram (arrow-in-box notation) to represent these electrons.

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

(Total 7 marks)

53. Nitrogen and silicon belong to different groups in the periodic table.

(i) Distinguish in terms of electronic structure, between the terms group and period.(2)

(ii) State the maximum number of orbitals in the n = 2 energy level.(1)

(Total 3 marks)

54. What happens when sodium is added to water?

I. A gas is evolved

II. The temperature of the water increases

III. A clear, colourless solution is formed

A. I and II only

B. I and III only

C. II and III only

D. I, II and III(Total 1 mark)

55. An atom of an element contains 19 electrons. In which group of the periodic table does it occur?

A. 1

B. 2

C. 5

D. 7(Total 1 mark)

56. Which species has the largest radius?

A. Cl–

B. K

C. Na+

D. K+

(Total 1 mark)

57. Which process is responsible for the colour of a transition metal complex?

A. The absorption of light when electrons move between s orbitals and d orbitals

B. The emission of light when electrons move between s orbitals and d orbitals

C. The absorption of light when electrons move between different d orbitals

D. The emission of light when electrons move between different d orbitals(Total 1 mark)

58. Transition elements form complexes such as [Fe(CN)6]4– and [FeCl4]–. Deduce the oxidation number of iron in each of these complex ions.

[Fe(CN)6]4– ............................................................................................................................

[FeCl4]– ..................................................................................................................................(Total 2 marks)

59. Which series is arranged in order of increasing radius?

A. Ca2+ < Cl– < K+

B. K+ < Ca2+ < Cl–

C. Ca2+ < K+ < Cl–

D. Cl– < K+ < Ca2+

(Total 1 mark)

60. Describe the acid-base character of the oxides of the period 3 elements Na to Ar. For sodium oxide and sulfur trioxide, write balanced equations to illustrate their acid-base character.

(Total 3 marks)

61. Which salts form coloured solutions when dissolved in water?

I. FeCl3II. NiCl2III. ZnCl2

A. I and II only

B. I and III only

C. II and III only

D. I, II and III(Total 1 mark)

62. Which combination is correct for the complex ion in [Co(NH3)4(H2O)Cl]Br?

Oxidation state of cobalt

Shape of the complex ion

Overall charge of thecomplex ion

A. +2 Octahedral +2

B. +3 Octahedral –1

C. +2 Octahedral +1

D. +2 Tetrahedral +1(Total 1 mark)

63. Consider the transition metal complex, K3[Fe(CN)6].

(i) Define the term ligand, and identify the ligand in this complex.(1)

(ii) Write the full electron configuration and draw the orbital box diagram of iron in its oxidation state in this complex, and hence, determine the number of unpaired electrons in this state.

(3)

(iii) Explain why many transition metal d-block complexes are coloured.(3)

(Total 7 marks)

64. By reference to the structure and bonding in NaCl and SiCl4:

(i) State and explain the differences in electrical conductivity in the liquid state.(3)

(ii) Predict an approximate pH value for the solutions formed by adding each compound separately to water. Explain your answer.

(4)(Total 7 marks)

65. Which property generally decreases across period 3?

A. Atomic number

B. Electronegativity

C. Atomic radius

D. First ionization energy(Total 1 mark)