D. K and Br 2 (Total 1 mark)
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1 IB Chemistry SL Topic 3 Questions 1. 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 2. Which of the physical properties below decrease with increasing atomic number for both the alkali metals and the halogens? I. Atomic radius II. III. Ionization energy Melting point A. I only B. II only C. III only D. I and III only 3. When the following species are arranged in order of increasing radius, what is the correct order? A. Cl, Ar, K + B. K +, Ar, Cl C. Cl, K +, Ar D. Ar, Cl, K + 4. 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 Page 1 of 10
2 5. Which property decreases down group 7 in the periodic table? A. atomic radius B. electronegativity C. ionic radius D. melting point 6. 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. A. I and II only B. I and III only C. II and III only D. I, II and III 7. 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 A. I and II only B. I and III only C. II and III only D. I, II and III 8. 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. 9. Which statement is correct for a periodic trend? A. Ionization energy increases from Li to Cs. Page 2 of 10
3 B. Melting point increases from Li to Cs. C. Ionization energy increases from F to I. D. Melting point increases from F to I. 10. 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. 11. 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. A. I and II only B. I and III only C. II and III only D. I, II and III 12. Which element is a transition metal? A. Ca B. Cr C. Ge D. Se 13. 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 14. Which oxides produce an acidic solution when added to water? I. SiO 2 Page 3 of 10
4 II. P 4 O 6 III. SO 2 A. I and II only B. I and III only C. II and III only D. I, II and III 15. 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 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. 17. State and explain the trends in the atomic radius and the ionization energy (Total 8 marks) for the alkali metals Li to Cs. for the period 3 elements Na to Cl. (4) (4) (Total 8 marks) 18. (a) Classify each of the following oxides as acidic, basic or amphoteric. (iii) aluminium oxide sodium oxide sulfur dioxide Write an equation for each reaction between water and sodium oxide sulfur dioxide. Page 4 of 10
5 (Total 5 marks) 19. Explain why the first ionization energy of magnesium is lower than that of fluorine. magnesium has a higher melting point than sodium. (3) (Total 5 marks) 20. 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. (Total 5 marks) 21. 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. (3) (Total 5 marks) 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. (7) (Total 13 marks) ) 22. Explain why sulfur has a lower first ionization energy than oxygen, and also a lower first ionization energy than phosphorus. (Total 4 marks) 23. With reference to the types of bonding present in period 3 elements: (iii) 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) 24. 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) 25. Explain the following statements. (a) The first ionization energy of sodium is less than that of magnesium. Page 5 of 10
6 greater than that of potassium. The electronegativity of chlorine is higher than that of sulfur. (Total 5 marks) 26. (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. (3) IB Chemistry SL Topic 3 Answers 1. C 2. B 3. B 4. C 5. B 6. A 7. A 8. C 9. D 10. D 11. A Page 6 of 10
7 12. B 13. D 14. C 15. C 16. alkali metals: metallic bonding/a bed of cations in a sea of electrons; as radius increases down the group, valence electrons are further away from nucleus (and strength of metallic bonding decreases); halogens: non-polar/van der Waals forces between molecules; as size increases van der Waals forces increase (and melting point increases); period 3 elements: increase in melting points of metals (Na, Mg, Al) due to increase in number of valence electrons and decrease in size/the way atoms are packed as solids; Award mark just for increased number of delocalized or valence electrons. silicon: network covalent solid (with very high melting point); Award mark also for many or strong covalent bonds. P Ar: simple molecular (atomic in case of Ar) substances with weak van der Waals forces (and lower melting points); trend in P 4, S 8, Cl 2, Ar due to size/mass of particles; 8 Award mark for decreasing mass or size. Molecular formulae not necessary. [8] 17. Li to Cs atomic radius increases; because more full energy levels are used or occupied/outer electrons further from nucleus/outer electrons in a higher shell; ionization energy decreases; because the electron removed is further from the nucleus/increased repulsion by inner-shell electrons; 4 Accept increased shielding effect. Na to Cl atomic radius decreases; because nuclear charge increases and electrons are added to same main (outer) energy level; ionization energy increases; because nuclear charge increases and the electron removed is closer to the nucleus/is in the same energy level; 4 Accept core charge for nuclear charge. In and explanation mark dependent on correct trend. [8] 18. (a) aluminium oxide Page 7 of 10
8 amphoteric; (iii) sodium oxide basic; sulfur dioxide acidic; 3 Na 2 O + H 2 O 2Na + + 2OH ; SO 2 + H 2 O H 2 SO 3 ; 2 Accept NaOH and H + + HSO 3 /2H + + SO 3 2. [5] 19. electron removed from higher energy level/further from nucleus/ greater atomic radius; increased repulsion by extra inner shell electrons/increased shielding effect; 2 Mg has twice as many/more delocalized electrons (compared to Na); the ionic charge is twice as big/greater in Mg (than Na); (electrostatic) attraction between ions and electrons is much greater; 3 [5] 20. oxides of Na, Mg are basic Al is amphoteric Si, P, S and Cl are acidic Award 7 correct [3], 6/5 correct [2] and 4/3 correct. SO 2 + H 2 O H 2 SO 3 /SO 3 + H 2 O H 2 SO 4 / P 4 O H 2 O 4H 3 PO 4 /P 4 O 6 + 6H 2 O 4H 3 PO 3 ; Na 2 O + H 2 O 2NaOH/MgO + H 2 O Mg(OH) 2 ; 5 Accept equation using P 2 O 3 or P 2 O 5. [5] 21. (chlorine has) an extra proton/more protons/greater nuclear charge/ 17+ compared to 16+; outer electrons attracted more strongly; 2 ability of atom to attract bonding pair of electrons/electrons in a covalent bond; chlorine has a smaller radius/(electrons) closer to nucleus/in lower energy level; repelled by fewer inner electrons/decreased shielding effect; 3 [5] 22. IE S < IE O : valence electron in S in n = 3, in O in n = 2/e further away/s has another electron shell/atomic radius of S greater than that of O; less attracted to nucleus/experiences greater screening from inner electrons; IE S < IE P : electron removed from S is paired; Page 8 of 10
9 greater repulsion due to two electrons in the same (p) orbital/paired electrons in S; 4 [4] 23. Mg has greater nuclear charge/greater charge on cation/more valence e /greater number of delocalized electrons/na has lesser nuclear charge/lesser charge on cation/less valence e /lesser number of delocalized electrons; stronger attraction between cation and delocalized/ free/valence electrons; 2 If neither mark scored, accept stronger metallic bonding in Mg for [1 max]. (iii) giant/network/lattice/macromolecular structure; many/strong covalent bonds (need to be broken); 2 (simple) molecular substances; weak van der Waals /dispersion/london forces between molecules; 2 Weak intermolecular forces not sufficient for second mark [6] 24. Oxides of: Na and Mg are basic; Al is amphoteric; Si to Cl are acidic; Ar has no oxide; All four correct award [2], two or three correct award. Na 2 O + H 2 O 2NaOH and SO 3 + H 2 O H 2 SO 4 ; 3 Must be balanced for mark. Award marks for alternative correct equations such as SO 3 with NaOH. [3] 25. (a) Na has lower nuclear charge/number of protons; electrons being removed are from same energy level/shell; or Na has larger radius/electron further from nucleus; 2 max Award this mark if both electron arrangements are given. Na electron closer to nucleus/in lower energy level/na has less 1 shielding effect; Allow counter arguments for Mg in and K in. chlorine has a higher nuclear charge; attracts the electron pair/electrons in bond more strongly; 2 [5] 26. (a) the (minimum) energy required/needed for the removal of one electron; from a gaseous/isolated atom; 2 Al(g) Al + (g) + e; 1 Do not penalize the answer if (g) is after e. greater nuclear charge/greater number of protons/atom radius g is smaller; stronger attraction (for electron); 2 (c) 2Li + 2H 2 O 2LiOH + H 2 ; Ignore state symbols. Page 9 of 10
10 effervescence/fizzing/bubbles/owtte; lithium moves around/decrease in size of piece; Accept dissolves or disappears. heat produced; 3 Award each for any two of last three observations. [8] Page 10 of 10
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