2. Which of the following salts form coloured solutions when dissolved in water? I. Atomic radius II. Melting point III.

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1 1. Which pair of elements reacts most readily? A. Li + Br 2 B. Li + Cl 2 C. K + Br 2 D. K + Cl 2 2. Which of the following salts form coloured solutions when dissolved in water? I. ScCl 3 II. FeCl 3 III. NiCl 2 IV. ZnCl 2 A. I and II only B. II and III only C. III and IV only D. I, II, III and IV 3. The compounds Na 2 O, Al 2 O 3 and SO 2 respectively are A. acidic, amphoteric and basic. B. amphoteric, basic and acidic. C. basic, acidic and amphoteric. D. basic, amphoteric and acidic. 4. Which of the following properties of the halogens increase from F to I? I. Atomic radius II. Melting point III. Electronegativity A. I only B. I and II only C. I and III only D. I, II and III 5. Which pair would react together most vigorously? A. Li and Cl 2 B. Li and Br 2 C. K and Cl 2 D. K and Br 2 6. Which properties of period 3 elements increase from sodium to argon? I. Nuclear charge II. Atomic radius III. Electronegativity 7. Which general trends are correct for the oxides of the period 3 elements (Na 2 O to Cl 2 O)? I. Acid character decreases. II. III. Electrical conductivity (in the molten state) decreases. Bonding changes from ionic to covalent. 8. For which element are the group number and the period number the same? A. Li B. Be C. B D. Mg 9. Which of the physical properties below decrease with increasing atomic number for both the alkali metals and the halogens? I. Atomic radius II. Ionization energy III. Melting point A. I only B. II only C. III only D. I and III only 10. Which of the reactions below occur as written? I. Br 2 + 2I 2Br + I 2 II. Br 2 + 2Cl 2Br + Cl 2 A. I only B. II only C. Both I and II D. Neither I nor II 11. Rubidium is an element in the same group of the periodic table as lithium and sodium. It is likely to be a metal which has a A. high melting point and reacts slowly with water. B. high melting point and reacts vigorously with water. C. low melting point and reacts vigorously with water. D. low melting point and reacts slowly with water. 12. When the following species are arranged in order of increasing radius, what is the correct order? 1

2 A. Cl, Ar, K + B. K +, Ar, Cl C. Cl, K +, Ar D. Ar, Cl, K What increases in equal steps of one from left to right in the periodic table for the elements lithium to neon? A. the number of occupied electron energy levels B. the number of neutrons in the most common isotope C. the number of electrons in the atom D. the atomic mass 14. Which property decreases down group 7 in the periodic table? A. atomic radius B. electronegativity C. ionic radius D. melting point 15. Which two elements react most vigorously with each other? A. chlorine and lithium B. chlorine and potassium C. iodine and lithium D.iodine and potassium 16. Which is an essential feature of a ligand? A. a negative charge ` B. an odd number of electrons C. the presence of two or more atoms D. the presence of a non-bonding pair of electrons 17. Which properties are typical of most non-metals in period 3 (Na to Ar)? I. They form ions by gaining one or more electrons. II. III. They are poor conductors of heat and electricity. They have high melting points. 18. A potassium atom has a larger atomic radius than a sodium atom. Which statement about potassium correctly explains this difference? A. It has a larger nuclear charge. B. It has a lower electronegativity. C. It has more energy levels occupied by electrons. D. It has a lower ionization energy. 19. Which equation represents the third ionization energy of an element M? A. M + (g) M 4+ (g) + 3e B. M 2+ (g) M 3+ (g) + e C. M(g) M 3+ (g) + 3e D. M 3+ (g) M 4+ (g) + e 20. Which factors lead to an element having a low value of first ionization energy? I. large atomic radius II. III. high number of occupied energy levels high nuclear charge 21. Which statement about electronegativity is correct? A. Electronegativity decreases across a period. B. Electronegativity increases down a group. C. Metals generally have lower electronegativity values than non-metals. D. Noble gases have the highest electronegativity values. 22. Which statement is correct for a periodic trend? A. Ionization energy increases from Li to Cs. B. Melting point increases from Li to Cs. C. Ionization energy increases from F to I. D. Melting point increases from F to I. 2

3 23. Which compound of an element in period 3 reacts with water to form a solution with a ph greater than 7? A. SiO 2 B. SiCl 4 C. NaCl D. Na 2 O 24. Which electrons are lost by an atom of iron when it forms the Fe 3+ ion? A. One s orbital electron and two d orbital electrons B. Two s orbital electrons and one d orbital electron C. Three s orbital electrons D. Three d orbital electrons 25. Which equation represents the first ionization energy of fluorine? A. F(g) + e F (g) B. F (g) F(g) + e C. F + (g) F(g) + e D. F(g) F + (g) + e 26. Which properties are typical of d-block elements? I. complex ion formation II. catalytic behaviour III. colourless compounds 27. Which statement is correct for the halogen group? A. Halide ions are all reducing agents, with iodide ions being the weakest. B. Halogens are all oxidizing agents, with chlorine being the strongest. C. Chloride ions can be oxidized to chlorine by bromine. D. Iodide ions can be oxidized to iodine by chlorine. 28. Which of the following statements are correct? I. The melting points decrease from Li Cs for the alkali metals. II. The melting points increase from F I for the halogens. III. The melting points decrease from Na Ar for the period 3 elements. 29. Which element is a transition metal? A. Ca B. Cr C. Ge D. Se 30. When Na, K, and Mg are arranged in increasing order of atomic radius (smallest first), which order is correct? A. Na, K, Mg B. Na, Mg, K C. K, Mg, Na D. Mg, Na, K 31. Which oxides produce an acidic solution when added to water? I. SiO 2 II. P 4 O 6 III. SO Which combination of ion charge and ion size produces the greatest lattice enthalpy? A. High charge, large size B. High charge, small size C. Low charge, small size D. Low charge, large size 33. Which series is arranged in order of increasing radius? A. Ca 2+ < Cl < K + B. K + < Ca 2+ < Cl C. Ca 2+ < K + < Cl D. Cl < K + < Ca Which salts form coloured solutions when dissolved in water? I. FeCl 3 II. NiCl 2 III. ZnCl 2 3

4 35. Which combination is correct for the complex ion in [Co(NH 3 ) 4 (H 2 O)Cl]Br? Oxidation state of cobalt Shape of the complex ion Overall charge of the complex ion A. +2 Octahedral +2 B. +3 Octahedral 1 C. +2 Octahedral +1 D. +2 Tetrahedral 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 Table 6 of the Data Booklet lists melting points of the elements. Explain the trend in the melting points of the alkali metals, halogens and period 3 elements Explain how the first ionization energy of K compares with that of Na and Ar. Explain the difference between the first ionization energies of Na and Mg. Suggest why much more energy is needed to remove an electron from Na + than from Mg Define the term ligand. Cu 2+ (aq) reacts with ammonia to form the complex ion (Total 8 marks) 4

5 [Cu(NH 3 ) 4 ] 2+. Explain this reaction in terms of an acid-base theory, and outline the bonding in the complex ion formed between Cu 2+ and NH (Total 4 marks) 40. Nitrogen is found in period 2 and group 5 of the periodic table. Distinguish between the terms period and group. State the electron arrangement of nitrogen and explain why it is found in period 2 and group 5 of the periodic table. (Total 4 marks) 41. Table 8 of the Data Booklet gives the atomic and ionic radii of elements. State and explain the difference between the atomic radius of nitrogen and oxygen. the atomic radius of nitrogen and phosphorus. the atomic and ionic radius of nitrogen. 42. State and explain the trends in the atomic radius and the ionization energy for the alkali metals Li to Cs. 5

6 for the period 3 elements Na to Cl. (Total 8 marks) 43. Describe three similarities and one difference in the reactions of lithium and potassium with water. Give an equation for one of these reactions. Suggest a ph value for the resulting solution, and give a reason for your answer. (Total 7 marks) 44. (a) Classify each of the following oxides as acidic, basic or amphoteric. aluminium oxide sodium oxide sulfur dioxide Write an equation for each reaction between water and sodium oxide sulfur dioxide. 45. By reference to the structure and bonding in the compounds NaCl and SiCl 4 6

7 state and explain the differences in conductivity in the liquid state. predict an approximate ph value for a solution formed by adding each compound separately to water. (Total 7 marks) 46. Two characteristics of the d-block (transition) elements are that they exhibit variable oxidation states and form coloured compounds. State two possible oxidation states for iron and explain these in terms of electron arrangements. Explain why many compounds of d-block (transition) elements are coloured. 47. This question is about Period 3 elements and their compounds. (a) Explain, in terms of their structure and bonding, why the element sulfur is a non-conductor of electricity and aluminium is a good conductor of electricity. Explain, in terms of its structure and bonding, why silicon dioxide, SiO 2, has a high melting point. (Total 6 marks) 48. Silicon tetrachloride, SiCl 4, reacts with water to form an acidic solution. Explain why silicon tetrachloride has a low melting point. 7

8 Write an equation for the reaction of silicon tetrachloride with water. (Total 3 marks) 49. Explain why the first ionization energy of magnesium is lower than that of fluorine. magnesium has a higher melting point than sodium. 50. Discuss the acid-base nature of the period 3 oxides. Write an equation to illustrate the reaction of one of these oxides to produce an acid, and another equation of another of these oxides to produce a hydroxide. 51. Information about the halogens appears in the Data Booklet. Explain why the ionic radius of chlorine is less than that of sulfur. Explain what is meant by the term electronegativity and explain why the electronegativity of chlorine is greater than that of bromine. 52. Magnesium chloride and silicon(iv) chloride have very different properties. Give the formula and physical state at room temperature of each chloride. State the conditions under which, if at all, each chloride conducts electricity. Each chloride is added to water in separate experiments. Suggest an approximate ph value for the solution formed, and write an equation for any reaction that occurs. (Total 7 marks) 53. The elements in the d-block in the periodic table have several characteristics in common. Give the electronic configuration of Ni 2+. Explain what is meant by a ligand, and describe the type of bond formed between a ligand and a d-block element. Determine the oxidation numbers of copper in the species [Cu(NH 3 ) 4 ] 2+ and [CuCl 4 ] 2 (iv) Explain why the species in are coloured. (v) Identify the d-block element used as a catalyst in the Haber process and write an equation for the reaction occurring. (Total 10 marks) 54. (a) State the meaning of the term electronegativity and explain why the noble gases are not assigned electronegativity values. State and explain the trend in electronegativity across period 3 from Na to Cl. Explain why Cl 2 rather than Br 2 would react more vigorously with a solution of I. 8

9 State the acid-base properties of the following period 3 oxides. MgO Al 2 O 3 P 4 O 6 Write equations to demonstrate the acid-base properties of each compound. 55. Define the term ionization energy. (7) (Total 13 marks) (iv) Write an equation for the reaction of lithium with water. State and explain the trend in the ionization energy of alkali metals down the group. Explain why the electronegativity of phosphorus is greater than that of aluminium. (v) Table 8 in the Data Booklet contains two values for the ionic radius of silicon. Explain, by reference to atomic structure and electron arrangements, why the two values are very different. (Total 11 marks) 56. Explain why sulfur has a lower first ionization energy than oxygen, and also a lower first ionization energy than phosphorus. (Total 4 marks) 57. With reference to the types of bonding present in period 3 elements: explain why Mg has a higher melting point than Na. explain why Si has a very high melting point. explain why the other non-metal elements of period 3 have low melting points. (Total 6 marks) 58. Explain why complexes of Zn 2+ are colourless whereas complexes containing Cu 2+ are coloured. Give the formula and describe the shape of the complex ion formed between Fe 3+ and the ligand CN. 59. 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) 60. Consider the transition metal complex, K 3 [Fe(CN) 6 ]. Define the term ligand, and identify the ligand in this complex. 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. Explain why many transition metal d-block complexes are coloured. (Total 7 marks) 61. By reference to the structure and bonding in NaCl and SiCl 4 : State and explain the differences in electrical conductivity in the liquid state. Predict an approximate ph value for the solutions formed by adding each compound separately to water. Explain your answer. 9

10 (Total 7 marks) 62. Explain the following statements. (a) The first ionization energy of sodium is less than that of magnesium. greater than that of potassium. The electronegativity of chlorine is higher than that of sulfur. 63. The following table shows values that appear in the Data Booklet. Table 1 Covalent (atomic) radii /10 12 m N 0 F Na Mg Al Si P S Cl Table 2 Ionic radii/10 12 m N 3 O 2 F Na + Mg 2+ Al 3+ Si 4+ P 3 S 2 Cl Explain why the magnesium ion is much smaller than the magnesium atom. there is a large increase in ionic radius from silicon to phosphorus. the ionic radius of Na + is less than that of F. 64. Elements with atomic number 21 to 30 are d-block elements. (a) (c) Identify which of these elements are not considered to be typical transition elements. Complex ions consist of a central metal ion surrounded by ligands. Define the term ligand. Complete the table below to show the oxidation state of the transition element. ion 2 Cr 2 O 7 [CuCl 4 ] 2 [Fe(H 2 O) 6 ] 3+ oxidation state (d) (e) Identify two transition elements used as catalysts in industrial processes, stating the process in each case. Apart from the formation of complex ions and apart from their use as catalysts, state two other properties of transition elements. 65. (a) Define the term ionization energy. Write an equation, including state symbols, for the process occurring when measuring the first ionization energy of aluminium. (c) The first ionization energies of the elements are shown in Table 7 of the Data Booklet. Explain why the first ionization energy of magnesium is greater than that of sodium. Lithium reacts with water. Write an equation for the reaction and state two observations that could be made during the reaction. 10

11 66. (a) State the meaning of the term electronegativity. State and explain the trend in electronegativity across period 3 from Na to Cl. (c) Explain why Cl 2 rather than Br 2 would react more vigorously with a solution of I. 11