AP Chem Ch 8,9,10 Practice Quiz
1. The type of compound that is most likely to contain a covalent bond is
a) 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 table
b) a solid metal
c) one that is composed of only nonmetals
d) held together by the electrostatic forces between oppositely charged ions
2. Lattice energy _______ as ionic radium increases and ______ as ionic charge increases.
a) decreases, increases
b) increases, decreases
c) increases, increases
d) decreases, decreases
3. Which one of the following ionic compounds would have the highest melting point?
a) K2O
b) KCl
c) CaCl2
d) MgO
4. The halide ion with the smallest diameter is
a) Brb) Clc) Id) F5. Which ion has the largest radius?
a) Al3+
b) Na+
c) O2d) Fe) N36. Which one of the following species is isoelectronic with argon?
a) Kr
b) O2c) Cld) Mg2+
7. In general, the distance between bonded atoms __________ as the number of shared electron pairs
increases.
a) increases
b) decreases
c) remains the same
8. Which atom below has the highest electronegativity?
a) Si
b) Cl
c) Rb
d) Ca
e) S
9. Of the molecules below, which is the most polar?
a) HBr
b) HI
c) HCl
d) HF
10. How many pairs of electrons not involved in bonds are located on the central atom of arsine, AsH 3?
a) 0
b) 1
c) 2
d) 3
11. The Lewis structure of N2H2
a) shows a nitrogen-nitrogen triple bond
b) shows a nitrogen-nitrogen single bond
c) gives each nitrogen 1 nonbonding pair
d) gives each nitrogen 2 nonbonding pairs
e) 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) 0
b) 1
c) 2
d) 3
13. How many resonance structures must be drawn for the ion CO3-2?
a) 0
b) 2
c) 3
d) 4
14. The species below which violates the octet rule is
a) 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) IF416. 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, CHBr 3, into individual atoms.
a) 1241 kJ/mole
b) 689 kJ/mole
c) -689 kJ/mole
d) 1378 kJ/mole
e) -1378 kJ/mole
17. Of the bonds CN (single bond), CN (double bond), CN(triple bond), the CN(single bond) is
a) strongest/shortest
b) strongest/longest
c) weakest/shortest
d) weakest/longest
e) intermediate in both strength and length
18. What is the shape of the hydronium ion, H3O+?
a) linear
b) tetrahedral
c) bent
d) trigonal pyramid
e) triangle
19. What is the shape of the CS2 molecule?
a) linear
b) bent
c) tetrahedral
d) trigonal pyramid
e) triangle
20. What is the shape of a PF4+ ion?
a) octahedral
b) tetrahedral
c) trigonal pyramid
d) triangle
e) square planar
21. The approximate F-B-F bond angle in BF3 is
a) 90 degrees
b) 109 degrees
c) 120 degrees
d) 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 forces
b) ionic
c) dipole-dipole
d) hydrogen bonding
26. The principle difference in respective normal boiling points of ICl (97 degrees C) and Br 2 (59 degrees
C) is due to
a) London dispersion forces
b) dipole - dipole forces
c) hydrogen bonding
d) ionic bonding
27. Which noble gas has the highest boiling point?
a) Ne
b) Ar
c) Kr
d) Xe
e) Rn
28. What is the predominant intermolecular force in CBr 4?
a) London dispersion forces
b) dipole-dipole forces
c) ionic bonding
d) hydrogen bonding
29. Which of the following compounds will have hydrogen bonds as one of its intermolecular forces?
a) H2S
b) SiH4
c) HCl
d) NH3
e) BH3
30. Which one of the following should have the lowest boiling point?
a) PH3
b) H2S
c) HCl
d) 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 called
a) fusion
b) vaporization
c) condensation
d) boiling
e) sublimation
33. Which of the following is an exothermic process?
a) melting
b) subliming
c) freezing
d) boiling
34. As vapor pressure increases, boiling point _____ and volatility ______________.
a) decreases, increases
b) increases, decreases
c) increases, increases
d) decreases, decreases
e) decreases, remains constant
35. Increasing the total pressure above a liquid will cause the boiling point of the liquid to
a) increase
b) decrease
c) remain the same
d) depends on the liquid
36. On a phase diagram (Pressure vs. Temperature), the
a) critical point is that beyond which gas and solid are indistinguishable
b) triple point is that at which solid, liquid, and gas are in equilibrium
c) solid is generally found at high temperature and low pressure
d) liquid is generally found at high temperature and low pressure
e) 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) A
b) B
c) C
d) D
e) E
f) F
38. On the diagram above, the coordinates of point ____ correspond to the critical temperature and
pressure.
a) A
b) B
c) C
d) D
e) E
f) F
39. Which portion of below diagram corresponds to the gas phase?
a) w
b) x
c) y
d) z
40. What is the normal boiling point of this substance?
a) -3
b) 10
c) 25
d) 38
41. Of the following, which molecule has the largest bond angle?
a) O3
b) OF2
c) HCN
d) H2O
e) More than one of the above have equally large bond angles.
42. The Cl – Kr – Cl bond angle in KrCl4 is closest to
a) 90°
b) 109°
c) 120°
d) 150°
e) 360°
43. How many of the following molecules – SF2, SF4, SF6, SiO2, are polar?
a) 0
b) 1
c) 2
d) 3
e) 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 CS 2. (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 is
a) trigonal bipyramidal
b) square pyramidal
c) distorted tetrahedral
d) octahedral
e) none of the above
48-55. Select the correct molecular structure for the given species from the choices below:
a) trigonal pyramid
b) tetrahedral
c) square planar
d) octahedral
e) other
48. PF649. PCl4+
50. XeF6
51. NI3
52. SiH4
53. ClO2
54. IF455. SO3256. Which ion is planar?
a) NH4+
b) CO32c) SO32d) ClO3e) all are planar
57. In the molecule XeF2, how many pairs of electrons surround Xe and what is the molecular geometry?
a) 4, bent
b) 4, trigonal planar
c) 5, linear
d) 5, bent
e) 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 be
a) not hybridized
b) sp hybridized
c) sp2 hybridized
d) sp3 hybridized
e) dsp hybridized
60-64 Use the following responses
a) sp
b) 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) H2CO
b) PF2c) C2H6
d) HClO
e) CCl4
66. What is the formal charge on the Se atom in the SeF4 molecule?
a) 0
b) -1
c) -2
d) +1
e) +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)