1. Which of the following statements is incorrect? [A] Dipole moments result from the unequal distribution of electrons in a molecule.
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1 1. Which of the following statements is incorrect? [A] Dipole moments result from the unequal distribution of electrons in a molecule. 2. Atoms having greatly differing electronegativities are expected to form: [A] nonpolar covalent bonds [B] no bonds [C] covalent bonds [D] ionic bonds [E] polar covalent bonds 3. Which of the following bonds is least polar? [A] Br Br [B] S Cl [C] They are all nonpolar. [D] H C [E] C O 4. Choose the compound with the most ionic bond. [A] KF [B] LiF [C] LiCl [D] KCl [E] NaCl 5. For the elements Rb, F, and O, the order of increasing electronegativity is: [A] Rb < O < F [B] F < Rb < O [C] O < F < Rb [D] Rb < F < O [E] None of these 6. For the elements Cs, F, and Cl, the order of increasing electronegativity is: [A] Cs < Cl < F [B] Cl < Cs < F [C] F < Cs < Cl [D] F < Cl < Cs [E] None of these 7. In the gaseous phase, which of the following diatomic molecules would be the most polar? [A] CsCl [B] CsF [C] NaCl [D] LiF [E] NaF 8. Based on electronegativities, which of the following would you expect to be most ionic? [A] CF 4 [B] CH 4 [C] N 2 [D] CO 2 [E] CaF 2 9. In which case is the bond polarity incorrect? [A] δ+ Mg H δ [B] δ+ Cl I δ [C] δ+ Si S δ [D] δ+ K O δ [E] δ+ H F δ 10. Which of the following groups contains no ionic compounds? [A] PCl 5, LiBr, Zn(OH) 2 [B] NaH, CaF 2, NaNH 2 [C] CH 2 O, H 2 S, NH 3 [D] HCN, NO 2, Ca(NO 3 ) 2 [E] KOH, CCl 4, SF 4
2 11. In which pair do both compounds exhibit predominantly ionic bonding? [A] Na 2 SO 3 and BH 3 [B] NaF and H 2 O [C] KI and O 3 [D] PCl 5 and HF [E] RbCl and CaO 12. Metals typically have electronegativity values. [A] high [B] low [C] negative [D] no [E] two of these 13. The electron pair in a C-F bond could be considered [A] an inadequate model since the bond is ionic. [B] closer to C because carbon has a larger radius and thus exerts greater control over the shared electron pair. [C] closer to C because carbon has a lower electronegativity than fluorine. [D] centrally located directly between the C and F. [E] closer to F because fluorine has a higher electronegativity than carbon. 14. Based on electronegativity differences, which of the following is most likely to be ionic? [A] CH 4 [B] BaF 2 [C] NO 3 [D] NH 3 [E] Cl What is the correct order of the following bonds in terms of decreasing polarity? [A] As-Cl, P-Cl, N-Cl [B] As-Cl, N-Cl, P-Cl [C] P-Cl, N-Cl, As-Cl [D] P-Cl, As-Cl, N-Cl [E] N-Cl, P-Cl, As-Cl 16. Which of the following bonds would be the most polar without being considered ionic? [A] C-O [B] N-O [C] Mg-O [D] O-O [E] Si-O 17. Which of the following bonds would be the least polar yet still be considered polar covalent? [A] Si-O [B] N-O [C] O-O [D] Mg-O [E] C-O 18. How many of the following molecules possess dipole moments? BH 3, CH 4, PCl 5, H 2 O, HF, H 2 [A] 4 [B] 2 [C] 3 [D] 5 [E] Which of the following molecules has a dipole moment? [A] CH 4 [B] CCl 4 [C] CO 2 [D] SO 3 [E] none of these
3 20. Select the molecule among the following that has a dipole moment. [A] BeCl 2 [B] XeF 4 [C] SeO 3 [D] SF 4 [E] CO Which of the following molecules has no dipole moment? [A] NH 3 [B] CO 2 [C] H 2 O [D] all [E] none 22. Which of the following has the smallest radius? [A] Ca 2+ [B] Kr [C] S 2 [D] Br [E] Xe 23. Which of these is an isoelectronic series? [A] Na +, Mg 2+, S 2, Cl [B] Li, Be, B, C [C] K +, Ca 2+, Ar, S 2 [D] Na +, K +, Rb +, Cs + [E] none of these (a-d) 24. Which of the following has the smallest radius? [A] S 2 [B] Cl [C] Ar [D] K + [E] Rb Which of the following ionic compounds has the smallest lattice energy, i.e., the lattice energy least favorable to a stable lattice? [A] LiF [B] BaO [C] NaCl [D] MgO [E] CsI 26. Calculate the lattice energy for LiF(s) given the following: sublimation energy for Li(s) +166 kj / mol ΔH f for F(g) + 77 kj / mol first ionization energy of Li(g) kj / mol electron affinity of F(g) 328 kj / mol enthalpy of formation of LiF(s) 617 kj / mol [A] 650. kj/mol [B] 285 kj/mol [C] 800. kj/mol [D] 1047 kj/mol [E] None of these 27. When electrons in a molecule are not found between a pair of atoms but move throughout the molecule, this is called [A] a dipole moment. [B] delocalization of the electrons. [C] covalent bonding. [D] ionic bonding. [E] polar covalent bonding.
4 28. Which of the following statements concerning lattice energy is false? [A] The lattice energy for a solid with 2+ and 2 ions should be two times that for a solid with 1+ and 1 ions. [B] It is often defined as the energy released when an ionic solid forms from its ions. [C] MgO has a larger lattice energy than NaF. [D] MgO has a larger lattice energy than LiF. [E] All of these are true. 29. Which of the following pairs is isoelectronic? [A] Al 3+ and B 3+ [B] Li + and K + [C] I and Cl [D] Na + and Ne [E] S 2 and Ne 30. Which of the following arrangements is in order of increasing size? [A] Ga 3+ > Ca 2+ > S 2 > Cl > K + [B] Ga 3+ > Ca 2+ > K + > Cl > S 2 [C] Ga 3+ > S 2 > Ca 2+ > Cl > K + [D] S 2 > Cl > K + > Ca 2+ > Ga 3+ [E] Ga 3+ > Ca 2+ > S 2 > K + > Cl 31. Given the following information: Li(s) Li(g) heat of sublimation of Li(s) = 166 kj / mol HCl(g) H(g) + Cl(g) bond energy of HCl = 427 kj / mol Li(g) + Li (g) + e ionization energy of Li(g) = 520. kj / mol Cl(g) + e Cl (g) electron affinity of Cl(g) = 349 kj / mol + Li (g) + Cl ( g ) LiCl(s) lattice energy of LiCl(s) = 829 kj / mol H (g) 2H(g) bond energy of H = 432 kj / mol 2 2 calculate the net change in energy for the reaction 2Li(s) + 2HCl(g) 2LiCl(s) + H 2 (g) [A] 179 kj [B] 363 kj [C] 73 kj [D] 562 kj [E] None of these 32. Choose the molecule with the strongest bond. [A] I 2 [B] Cl 2 [C] F 2 [D] Br 2 [E] All are equal. 33. Choose the molecule with the strongest bond. [A] HF [B] HCl [C] HBr [D] HI [E] All are equal.
5 34. Choose the molecule with the strongest bond. [A] HF [B] NH 3 [C] CH 4 [D] H 2 O [E] All are equal 35. Which of the following molecules exhibits the greatest bond energy? [A] Br 2 [B] I 2 [C] F 2 [D] Cl 2 [E] all the same 36. Using the following bond energies estimate the heat of combustion for one mole of acetylene: C 2 H 2 (g) + (5/2)O 2 (g) 2CO 2 (g) + H 2 O(g) [A] 447 kj [B] 1228 kj [C] +447 kj [D] 1228 kj [E] +365 kj 37. Which of the following species would be expected to have the lowest ionization energy? [A] Mg 2+ [B] F [C] Na + [D] O 2 [E] Ne 38. In which of the following compounds does the bond between the central atom and bromine have the greatest ionic character? [A] AsBr 2 [B] KBr [C] CaBr 2 [D] LiBr [E] SeBr Which of the following species is best described by drawing resonance structures? [A] HCN [B] O 3 [C] SO 3 [D] NH 4 + [E] PH Using the following data reactions ΔH (kj) H (g) + Cl (g) 2 2 2HCl(g) H 2(g) 2H(g) Cl 2(g) 2Cla(g) calculate the energy of an H Cl bond [A] 856 kj [B] 326 kj [C] 770 kj [D] 518 kj [E] 428 kj
6 41. Given the following bond energies C C 347 kj / mol C=C 614 kj / mol C=O 358 kj / mol C=O 799 kj / mol C H 413 kj / mol O H 463 kj / mol O O 146 kj / mol estimate ΔH for the reaction H 2 O 2 + CH 3 OH H 2 CO + 2H 2 O. [A] 345 kj [B] +345 kj [C] +199 kj [D] 105 kj [E] 199 kj Using the following electronegativity values C 25. Cl 3.2 H 22. N 3.0 O 3.4 select from the following group the molecule that fits the given statement: a) CH 3 CHO b) CO 2 c) CH 3 Cl d) C 2 H 6 e) none 42. This molecule is the most polar. 43. This molecule shows the smallest number of lone pairs in its Lewis structure. 44. As indicated by Lewis structures, which of the following would probably not exist as a stable molecule? [A] CH 2 O [B] CH 3 O [C] C 3 H 4 [D] C 2 H 2 [E] CH 3 OH 45. Which of the following molecules is non-polar overall? [A] SF 4 [B] H 2 S [C] OCl 2 [D] SF 2 [E] CCl 4
7 46. Select the best Lewis structure for acetone, CH 3 COCH 3. [A] [B] [C] [D] [E] 47. Which of the following is the correct order for molecules from most to least polar? [A] CH 4 > CF 2 H 2 > CF 2 Cl 2 > CCl 4 > CCl 2 H 2 [B] CH 4 > CF 2 Cl 2 > CF 2 H 2 > CCl 4 > CCl 2 H 2 [C] CF 2 H 2 > CCl 2 H 2 > CF 2 Cl 2 > CH 4 = CCl 4 [D] CF 2 Cl > CF 2 H 2 > CCl 4 > CCl 2 H 2 > CH 4 [E] CF 2 Cl 2 > CF 2 H 2 > CCl 2 H 2 > CH 4 = CCl Of the following, which molecule has the largest bond angle? [A] HCN [B] O 3 [C] OF 2 [D] H 2 O [E] More than one of these have equally large bond angles. 49. The Cl Kr Cl bond angle in KrCl 4 is closest to [A] 150 [B] 360 [C] 90 [D] 109 [E] How many of the following molecules SF 2, SF 4, SF 6, SiO 2 are polar? [A] 2 [B] 3 [C] 1 [D] 4 [E] Which of the following exhibits resonance? [A] PCl 5 [B] CH 4 [C] H 2 O [D] NO 2 [E] At least two of the molecules (a-d) exhibit resonance.
8 52. Choose the electron dot formula that most accurately describes the bonding in CS 2. (Hint: Consider formal charges.) [A] [B] [C] [D] [E] Draw the Lewis structures of the molecules below and use them to answer the following questions: I. BH3 II. NO2 III. SF6 IV. O3 V. PCl Which of the molecules obeys the octet rule? [A] IV [B] II [C] III [D] I [E] V 54. How many of the molecules have no dipole moment? [A] 1 [B] 2 [C] 4 [D] 3 [E] they are all polar 55. Which of these molecules show resonance? [A] III, IV [B] II, IV [C] I, II [D] II, V [E] III, V 56. Which of the following molecules contains a double bond? [A] CO 2 [B] H 2 O [C] NH 3 [D] all [E] none 57. In the Lewis structure for SF 6, the central sulfur atom shares electrons. [A] 8 [B] 10 [C] 12 [D] 4 [E] none of these, because SF 6 is an ionic compound
9 58. Which of the following Lewis structures best describes BF 3? [A] [B] [C] [D] [E] 59. Which of the following molecules has a nonlinear structure? [A] XeF 2 [B] BeCl 2 [C] CO 2 [D] N 2 O (central atom is N) [E] O 3 Select the correct molecular structure for the given species from the choices below: a) pyramidal b) none of these c) octahedral d) trigonal planar e) bent 60. OF NCl The geometry of AsCl 5 is [A] square pyramidal. [B] trigonal bipyramidal. [C] distorted tetrahedral. [D] octahedral. [E] none of these 63. The bond angles about the carbon atom in the formaldehyde molecule, H 2 C=O, are about: [A] 180 [B] 90 [C] 120 [D] What type of structure does the XeOF 2 molecule have? [A] T-shaped [B] pyramidal [C] trigonal planar [D] tetrahedral [E] octahedral
10 65. Which of the following species has a trigonal bipyramid structure? [A] I 3 [B] NH 3 [C] IF 5 [D] PCl 5 [E] none of these Select the correct molecular structure for the given species from the choices below: a) pyramidal b) tetrahedral c) square planar d) octahedral e) none of these 66. PF XeF NI SiH IF SO 3 2
11 [1] [2] [3] [4] [5] [6] [7] [8] [9] [10] [11] [12] [13] [14] [15] [16] [17]
12 [18] [19] [20] [21] [22] [23] [24] [25] [26] [27] [28] [29] [30] [31] [32] [33] [34]
13 [35] [36] [37] [38] [39] [40] [41] [42] [43] [44] [45] [46] [47] [48] [49] [50] [51]
14 [52] [53] [54] [55] [56] [57] [58] [59] [60] [61] [62] [63] [64] [65] [66] [67] [68]
15 [69] [70] [71]
16 Reference: 8.1,3 [1] [B] Reference: 8:1,2 [2] [D] [3] [A] [4] [A] [5] [A] [6] [A] [7] [B] [8] [E] [9] [B] [10] [C] [11] [E]
17 [12] [B] [13] [E] [14] [B] [15] [A] [16] [E] [17] [B] Reference: 8.3,13 [18] [B] Reference: 8.3,13 [19] [D] Reference: 8.3,13 [20] [D] Reference: 8.3,13 [21] [B] Reference: 8.4 [22] [A]
18 Reference: 8.4 [23] [C] Reference: 8.4 [24] [D] Reference: 8.5 [25] [E] Reference: 8.5 [26] [D] Reference: 8.1,7 [27] [B] Reference: 8.5 [28] [A] Reference: 8.4 [29] [D] Reference: 8.4 [30] [B] Reference: 8.5 [31] [D] Reference: 8.8 [32] [B] Reference: 8.8 [33] [A]
19 Reference: 8.8 [34] [A] Reference: 8.8 [35] [D] Reference: 8.8 [36] [D] Reference: 8.4 [37] [D] [38] [B] Reference: 8.12 [39] [B] Reference: 6.3,8.8 [40] [E] Reference: 8.8 [41] [A] Reference: 8.3,13 [42] a) CH 3 CHO Reference: 8.10 [43] d) C 2 H 6 Reference: 8.10,11 [44] [B]
20 Reference: 8.3,13 [45] [E] Reference: 8.10,12 [46] [A] Reference: 8.1-3,13 [47] [C] [48] [A] [49] [C] Reference: 8.1-3,13 [50] [A] Reference: 8.12 [51] [D] Reference: 8.10, 12 [52] [B] Reference: 8.10,11 [53] [A] Reference: 8.3,13 [54] [D] Reference: 8.12 [55] [B]
21 Reference: 8.10 [56] [A] Reference: 8.11 [57] [C] Reference: 8.11 [58] [A] [59] [E] [60] e) bent [61] a) pyramidal [62] [B] [63] [C] [64] [A] [65] [D] [66] d) octahedral
22 [67] e) none of these [68] a) pyramidal [69] b) tetrahedral [70] c) square planar [71] a) pyramidal
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