1. Which sample of the following compounds contains both ionic and covalent bonds?
[A] H2O2
[B] CH3Cl
[C] NH2OH
[D] C2H3OH
[E] NaNO3
2. Which of the compounds listed below would require the greatest energy to separate it into ions in the gaseous state?	
[A] MgCl2
[B] NaCl
[C] MgO
[D] Na2O
[E] NaI
3. Metals typically have _______ electronegativity values.
[A] negative
[B] high
[C] no
[D] low
[E] two of these
4. The geometry of AsCl5 is
[A] trigonal bipyramidal.
[B] square pyramidal.
[C] distorted tetrahedral.
[D] octahedral.
[E] none of these

5. The CCH bond angles in ethylene, C2H4, are 120°. What is the hybridization of the carbon orbitals?

6. Which form of orbital hybridization can form molecules with shapes that are either trigonal pyramidal or tetrahedral?
[A] sp3
[B] sp3d
[C] sp
[D] sp2
[E] spd2
7. Atoms having greatly differing electronegativities are expected to form:
[A] covalent bonds
[B] polar covalent bonds
[C] ionic bonds
[D] no bonds
[E] nonpolar covalent bonds
8. The shape of an ammonia molecule is tetrahedral.
[A] True
[B] False
9. Complete the Lewis structure for the following molecule:
	
This molecule has __________ sigma and __________ pi bonds.
[A] 13, 2
[B] 6, 3
[C] 11, 5
[D] 4, 5
[E] 13, 3

10. A molecule whose central atom has d2sp3 hybridization can have which of the following shapes?
I. Tetrahedral
II. Square pyramidal
III. Square planar

[A] III only
[B] I, II, and III
[C] I only
[D] II and III only
[E] I and II only
11. The Lewis structure for H3BO3 is

[A] 

[B] 

[C] 

[D] 

[E] 

12. Which of the following types of molecules has a dipole moment (when polar bonds are present)?
[A] tetrahedral molecules (four identical bonds equally spaced)
[B] linear molecules with two identical bonds
[C] trigonal pyramid molecules (three identical bonds)
[D] trigonal planar molecules (three identical bonds equally spaced)
[E] None has a dipole moment.
13. The six carbon atoms in a benzene molecule are shown in different resonance forms as three single bonds and three double bonds. If the length of a single carbon-carbon bond is 154 pm and the length of a double carbon-carbon bond is 133 pm, what length would be expected for the carbon-carbon bonds in benzene?
[A] 169 pm
[B] 140 pm
[C] 133 pm
[D] 126 pm
[E] 154 pm

14. Which of the following pairs is isoelectronic?
[A] Al3+ and B3+
[B] S2- and Ne
[C] Na+ and Ne
[D] I- and Cl-
[E] Li+ and K+
15. In the molecule XeF2, how many pairs of electrons surround Xe and what is the molecular geometry?
[A] 4, bent
[B] 4, pyramidal
[C] 5, linear
[D] 5, bent
[E] 6, linear
16. 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
 
PF6-

17. Given the following information:
	
calculate the net change in energy for the reaction 2Li(s) + 2HCl(g) ® 2LiCl(s) + H2(g)
[A] 363 kJ
[B] -73 kJ
[C] -179 kJ
[D] -562 kJ
[E] None of these
18. Solid NaCl melts at a temperature of 800 degrees Celsius, while solid NaBr melts at 750 degrees Celsius. Which of the following is an explanation for the higher melting point of NaCl?
[A] A chlorine ion has a greater negative charge than a bromine ion.
[B] A chlorine ion has less mass than a bromine ion.
[C] A chlorine ion is smaller than a bromine ion.
[D] A chlorine ion has a lesser negative charge than a bromine ion.
[E] A chlorine ion is larger than a bromine ion.
19. The hybridization of the B in BH3 is sp3.
[A] True
[B] False

20. Which of the following has the greatest bond strength?
[A] B2
[B] O2+
[C] O2-
[D] CN-
[E] NO-
21. Consider the following Lewis structure:
	
What is the hybridization of the oxygen atom and carbon atoms 1, 2, and 4, respectively?

[A] Option E
[B] Option B
[C] Option D
[D] Option C
[E] Option A
22. For the elements Rb, F, and O, the order of increasing electronegativity is:
[A] O < F < Rb
[B] F < Rb < O
[C] Rb < F < O
[D] Rb < O < F
[E] None of these
23. For the following compound:
a) draw the Lewis structure
b) give the shape of the molecule
c) indicate the polarity of the molecule
 
CBrI3

24. Which of the following has an incomplete octet in its Lewis structure?
[A] F2
[B] ICl
[C] NO
[D] SO2
[E] CO2

Reference: 9.1
[1] [E]

Reference: 8.10
[2] [C]

Reference: 8.2
[3] [D]

Reference: 8.13
[4] [A]

Reference: 9.1
[5] sp2

Reference: 8.2
[6] [A]

Reference: 8:1,2
[7] [C]

Reference: 8.13
[8] [B]

Reference: 9.1
[9] [E]

Reference: 8.10, 12
[10] [D]

Reference: 8.11
[11] [A]

Reference: 8.3
[12] [C]

Reference: 8.1-3,13
[13] [B]

Reference: 8.4
[14] [C]

Reference: 8.13
[15] [C]

Reference: 8.13
[16] d) octahedral

Reference: 8.5
[17] [D]

Reference: 6.3,8.8
[18] [C]

Reference: 9.1
[19] [B]

Reference: 9.3
[20] [D]

Reference: 9.1
[21] [E]

Reference: 8.2
[22] [D]

Reference: 8.3,10,13
[23] a) 
b) tetrahedral
c) polar

Reference: 8.11
[24] [C]