1. Which of the following pairs is isoelectronic?
[A] Na+ and Ne
[B] Al3+ and B3+
[C] Li+ and K+
[D] S2- and Ne
[E] I- and Cl-
2. The CCH bond angles in ethylene, C2H4, are 120°. What is the hybridization of the carbon orbitals?

3. For the elements Rb, F, and O, the order of increasing electronegativity is:
[A] F < Rb < O
[B] O < F < Rb
[C] Rb < O < F
[D] Rb < F < O
[E] None of these
4. 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 is smaller than a bromine ion.
[B] A chlorine ion has less mass than a bromine ion.
[C] A chlorine ion is larger than a bromine ion.
[D] A c hlorine ion has a greater negative charge than a bromine ion.
[E] A chlorine ion has a lesser negative charge than a bromine ion.
5. Which of the following has an incomplete octet in its Lewis structure?
[A] SO2
[B] F2
[C] CO2
[D] NO
[E] ICl
6. For the following compound:
a) draw the Lewis structure
b) give the shape of the molecule
c) indicate the polarity of the molecule
 
CBrI3

7. The Lewis structure for H3BO3 is

[A] 

[B] 

[C] 

[D] 

[E] 

8. Which form of orbital hybridization can form molecules with shapes that are either trigonal pyramidal or tetrahedral?
[A] sp3d
[B] spd2
[C] sp2
[D] sp3
[E] sp
9. 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-

10. Which of the compounds listed below would require the greatest energy to separate it into ions in the gaseous state?	
 [A] NaI
[B] MgO
[C] NaCl
[D] MgCl2
[E] Na2O
11. Given the following information:
	
calculate the net change in energy for the reaction 2Li(s) + 2HCl(g) ® 2LiCl(s) + H2(g)
[A] -562 kJ
[B] -73 kJ
[C] -179 kJ
[D] 363 kJ
[E] None of these

12. Consider the following Lewis structure:
	
What is the hybridization of the oxygen atom and carbon atoms 1, 2, and 4, respectively?

[A] Option A
[B] Option C
[C] Option D
[D] Option E
[E] Option B
13. Which of the following has the greatest bond strength?
[A] CN-
[B] NO-
[C] O2+
[D] O2-
[E] B2
14. The shape of an ammonia molecule is tetrahedral.
[A] True
[B] False
15. The geometry of AsCl5 is
[A] distorted tetrahedral.
[B] trigonal bipyramidal.
[C] octahedral.
[D] square pyramidal.
[E] none of these
16. A molecule whose central atom has d2sp3 hybridization can have which of the following shapes?
I. Tetrahedral
II. Square pyramidal
III. Square planar

[A] I and II only
[B] I only
[C] I, II, and III
[D] III only
[E] II and III only

17. Complete the Lewis structure for the following molecule:
	
This molecule has __________ sigma and __________ pi bonds.
[A] 4, 5
[B] 13, 2
[C] 6, 3
[D] 11, 5
[E] 13, 3

18. Which of the following types of molecules has a dipole moment (when polar bonds are present)?
[A] trigonal pyramid molecules (three identical bonds)
[B] linear molecules with two identical bonds
[C] trigonal planar molecules (three identical bonds equally spaced)
[D] tetrahedral molecules (four identical bonds equally spaced)
[E] None has a dipole moment.
19. The hybridization of the B in BH3 is sp3.
[A] True
[B] False
20. In the molecule XeF2, how many pairs of electrons surround Xe and what is the molecular geometry?
[A] 5, linear
[B] 4, pyramidal
[C] 6, linear
[D] 4, bent
[E] 5, bent
21. Atoms having greatly differing electronegativities are expected to form:
[A] no bonds
[B] nonpolar covalent bonds
[C] ionic bonds
[D] polar covalent bonds
[E] covalent bonds
22. Which sample of the following compounds contains both ionic and covalent bonds?
[A] CH3Cl
[B] C2H3OH
[C] NaNO3
[D] H2O2
[E] NH2OH
23. Metals typically have _______ electronegativity values.
[A] high
[B] negative
[C] low
[D] no
[E] two of these
24. 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] 126 pm
[B] 169 pm
[C] 133 pm
[D] 154 pm
[E] 140 pm

Reference: 8.4
[1] [A]

Reference: 9.1
[2] sp2

Reference: 8.2
[3] [C]

Reference: 6.3,8.8
[4] [A]

Reference: 8.11
[5] [D]

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

Reference: 8.11
[7] [E]

Reference: 8.2
[8] [D]

Reference: 8.13
[9] d) octahedral

Reference: 8.10
[10] [B]

Reference: 8.5
[11] [A]

Reference: 9.1
[12] [A]

Reference: 9.3
[13] [A]

Reference: 8.13
[14] [B]

Reference: 8.13
[15] [B]

Reference: 8.10, 12
[16] [E]

Reference: 9.1
[17] [E]

Reference: 8.3
[18] [A]

Reference: 9.1
[19] [B]

Reference: 8.13
[20] [A]

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

Reference: 9.1
[22] [C]

Reference: 8.2
[23] [C]

Reference: 8.1-3,13
[24] [E]