AP Chem Ch 8,9,10 Practice Quiz

1. The type of compound that is most likely to contain a covalent bond isa) one that is composed of a metal from the far left of the periodic table and a nonmetal from the far right of the periodic tableb) a solid metalc) one that is composed of only nonmetalsd) held together by the electrostatic forces between oppositely charged ions

2. Lattice energy _______ as ionic radium increases and ______ as ionic charge increases.a) decreases, increasesb) increases, decreasesc) increases, increasesd) decreases, decreases

3. Which one of the following ionic compounds would have the highest melting point?a) K2Ob) KClc) CaCl2

d) MgO

4. The halide ion with the smallest diameter isa) Br-

b) Cl-

c) I-

d) F-

5. Which ion has the largest radius?a) Al3+

b) Na+

c) O2-

d) F-

e) N3-

6. Which one of the following species is isoelectronic with argon?a) Krb) O2-

c) Cl-

d) Mg2+

7. In general, the distance between bonded atoms __________ as the number of shared electron pairs increases.a) increasesb) decreasesc) remains the same

8. Which atom below has the highest electronegativity?a) Sib) Clc) Rbd) Cae) S

9. Of the molecules below, which is the most polar?a) HBrb) HIc) HCld) HF

10. How many pairs of electrons not involved in bonds are located on the central atom of arsine, AsH3?a) 0b) 1c) 2d) 3

11. The Lewis structure of N2H2

a) shows a nitrogen-nitrogen triple bondb) shows a nitrogen-nitrogen single bondc) gives each nitrogen 1 nonbonding paird) gives each nitrogen 2 nonbonding pairse) gives each hydrogen 1 nonbonding pair

12. When the Lewis structure for SF4 is drawn, how many lone pairs of electrons are on the sulfur atom?a) 0b) 1c) 2d) 3

13. How many resonance structures must be drawn for the ion CO3-2?

a) 0b) 2c) 3d) 4

14. The species below which violates the octet rule isa) NF3

b) IF3

c) PF3

d) SbF3

e) AsF3

15. Which species below does not have more than an octet on the central atom?a) SF4

b) KrF2

c) CF4

d) XeF4

e) IF4-

16. Given that the average bond energies for C-H and C-Br bonds are 413 kJ/mole and 276 kJ/mole, respectively, calculate the heat required to turn bromoform, CHBr3, into individual atoms.a) 1241 kJ/moleb) 689 kJ/molec) -689 kJ/moled) 1378 kJ/molee) -1378 kJ/mole

17. Of the bonds CN (single bond), CN (double bond), CN(triple bond), the CN(single bond) isa) strongest/shortestb) strongest/longestc) weakest/shortestd) weakest/longeste) intermediate in both strength and length

18. What is the shape of the hydronium ion, H3O+?

a) linearb) tetrahedralc) bentd) trigonal pyramide) triangle

19. What is the shape of the CS2 molecule?a) linearb) bentc) tetrahedrald) trigonal pyramide) triangle

20. What is the shape of a PF4+ ion?

a) octahedralb) tetrahedralc) trigonal pyramidd) trianglee) square planar

21. The approximate F-B-F bond angle in BF3 isa) 90 degreesb) 109 degreesc) 120 degreesd) 180 degrees

22. Which of the following molecules below is polar?a) CCl4

b) XeF4

c) SeF4

d) SiCl4

e) SiF4

23. Which of the following molecules below is polar?a) SbF5

b) AsH3

c) I2

d) SF6

24. Which of the following is nonpolar?a) BF3

b) NF3

c) IF3

d) PBr3

e) BrCl3

25. What is the predominant intermolecular force in AsH3?a) London dispersion forcesb) ionicc) dipole-dipoled) hydrogen bonding

26. The principle difference in respective normal boiling points of ICl (97 degrees C) and Br2 (59 degrees C) is due toa) London dispersion forcesb) dipole - dipole forcesc) hydrogen bondingd) ionic bonding

27. Which noble gas has the highest boiling point?a) Neb) Arc) Krd) Xee) Rn

28. What is the predominant intermolecular force in CBr4?a) London dispersion forcesb) dipole-dipole forcesc) ionic bondingd) hydrogen bonding

29. Which of the following compounds will have hydrogen bonds as one of its intermolecular forces?a) H2Sb) SiH4

c) HCld) NH3

e) BH3

30. Which one of the following should have the lowest boiling point?a) PH3

b) H2Sc) HCld) SiH4

31. Which of the following substances would have the highest boiling point?a) N2

b) Br2

c) H2

d) Cl2

e) O2

32. The direct conversion of a solid to a gas is calleda) fusionb) vaporizationc) condensationd) boilinge) sublimation

33. Which of the following is an exothermic process?a) meltingb) sublimingc) freezingd) boiling

34. As vapor pressure increases, boiling point _____ and volatility ______________.a) decreases, increasesb) increases, decreasesc) increases, increasesd) decreases, decreasese) decreases, remains constant

35. Increasing the total pressure above a liquid will cause the boiling point of the liquid toa) increaseb) decreasec) remain the samed) depends on the liquid

36. On a phase diagram (Pressure vs. Temperature), thea) critical point is that beyond which gas and solid are indistinguishableb) triple point is that at which solid, liquid, and gas are in equilibriumc) solid is generally found at high temperature and low pressured) liquid is generally found at high temperature and low pressuree) both A and B

37. On the diagram below, which curve corresponds to the conditions of temperature and pressure under which the solid and the gas of the substance are in equilibrium?a) Ab) Bc) Cd) De) Ef) F

38. On the diagram above, the coordinates of point ____ correspond to the critical temperature and pressure.a) Ab) Bc) Cd) De) Ef) F

39. Which portion of below diagram corresponds to the gas phase?a) wb) xc) yd) z

40. What is the normal boiling point of this substance?a) -3b) 10c) 25d) 38

41. Of the following, which molecule has the largest bond angle? a) O3

b) OF2

c) HCNd) H2Oe) More than one of the above have equally large bond angles.

42. The Cl – Kr – Cl bond angle in KrCl4 is closest toa) 90°b) 109°c) 120°d) 150°e) 360°

43. How many of the following molecules – SF2, SF4, SF6, SiO2, are polar?a) 0b) 1c) 2d) 3e) 4

44. As indicated by Lewis Structures, which of the following species could probably not exist as a stable molecule?a) NH3

b) N2H2

c) N2H4

d) N2H6

e) N2O4

45. Choose the electron dot formula that most accurately describes the bonding in CS2. (Hint: Consider formal charges.)a) ::S=C=S::b) ::C=S=S::c) :::S – C – S:::d) :::S – :C = S::e) :::S – C≡S:

46. Which of the following molecules has a nonlinear structure?a) XeF2

b) BeCl2

c) O3

d) CO2

e) N2O (central atom is N)

47. The geometry of AsCl5 isa) trigonal bipyramidalb) square pyramidalc) distorted tetrahedrald) octahedrale) none of the above

48-55. Select the correct molecular structure for the given species from the choices below:a) trigonal pyramidb) tetrahedral c) square planard) octahedrale) other

48. PF6-

49. PCl4+

50. XeF6

51. NI3

52. SiH4

53. ClO2

54. IF4-

55. SO32-

56. Which ion is planar? a) NH4

+

b) CO32-

c) SO32-

d) ClO3-

e) all are planar

57. In the molecule XeF2, how many pairs of electrons surround Xe and what is the molecular geometry?a) 4, bentb) 4, trigonal planarc) 5, lineard) 5, bente) 6, linear

58. According to VSEPR theory, which of the following species has a square planar molecular structure?a) TeBr4

b) BrF3

c) IF5

d) XeF4

e) SCl2

59. In the molecule C2H4, the valence orbitals of the carbon atoms are assumed to bea) not hybridizedb) sp hybridizedc) sp2 hybridizedd) sp3 hybridizede) dsp hybridized

60-64 Use the following responsesa) spb) sp2

c) sp3

d) dsp3

e) d2sp3

60. The hybridization of the central atom in SF3+ is

61. The hybridization of the central atom in XeCl3+ is

62. The hybridization of the central atom in SeF4 is

63. The hybridization of the central atom in KrF4O is

64. The hybridization of the central atom in IF4- is

65. Which of the following contains a pi bond?a) H2COb) PF2

-

c) C2H6

d) HClOe) CCl4

66. What is the formal charge on the Se atom in the SeF4 molecule?a) 0b) -1c) -2d) +1e) +2

----------Key----------

1. (c) 2. (a) 3. (d) 4. (d) 5. (e) 6. (c) 7. (b) 8. (b) 9. (d) 10. (b) 11. (c) 12. (b) 13. (c) 14. (b) 15. (c) 16. (a) 17. (d) 18. (d) 19. (a) 20. (b) 21. (c) 22. (c) 23. (b) 24. (a) 25. (c) 26. (b)27. (e) 28. (a) 29. (d) 30. (d) 31. (b) 32. (e) 33. (c) 34. (a) 35. (a) 36. (b) 37. (a) 38. (f) 39. (c) 40. (c)41. (c)42. (a)43. (c)44. (d) 45. (a)46. (c)47. (a)48. (d)49. (b)50. (e)51. (a)52. (b)

53. (e)54. (c)55. (a)56. (b) 57. (c) 58. (d) 59. (c) 60. (c) 61. (d) 62. (d) 63. (e) 64. (e) 65. (a)66. (a)