CHM 2045C Module Four Part II Part M
Kotz 5e Chapter 10 Sample Multiple Choice

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1. Which is the best definition of a covalent bond?

a.	Electrons simultaneously attracted by more than one nucleus
b.	Overlapping of two electron-filled orbitals having different energies
c.	Overlapping of unoccupied orbitals of two or more atoms
d.	Positive ion attracting negative ions
e.	Interaction between outer electrons

2. Which formula represents the most probable bromine compound?

a.	CaBr
b.	AlBr
c.	BrCl
d.	HBr2
e.	NBr2

3. The hybridization of the central atom in a molecule is described as sp². The arrangement in space of the hybrid orbitals about that atom is

a.	linear.
b.	trigonal planar.
c.	tetrahedral.
d.	trigonal bipyramidal.
e.	octahedral.

4. When a carbon atom has sp³ hybridization, it has

a.	4 pi bonds.
b.	3 pi bonds and 1 sigma bond.
c.	2 pi bonds and 2 sigma bonds.
d.	1 pi bond and 3 sigma bonds.
e.	4 sigma bonds.

5. The electron pairs on the central nitrogen atom can be considered to be in sp² hybridized orbitals in all the following species EXCEPT

a.	FNO.
b.	NO3^-.
c.	H2NNH2.
d.	HNNH.
e.	HONO.

6. A given mass of gas in a rigid container is heated from 100?C to 500?C. Which of the following responses best describes what will happen to the pressure of the gas? Top of Form

a.	The pressure will remain the same.
b.	The pressure will decrease by a factor of five.
c.	The pressure will increase by a factor of five.
d.	The pressure will increase by a factor less than five.
e.	The pressure will increase by a factor greater than five.

7. When ammonium nitrite undergoes decomposition, only gases are produced according to the equation

NH₄NO₂(s) --> N₂(g) + 2H₂O(g)

What is the total volume of gases produced at 819 K and 1.00 atm pressure when 128 g of ammonium nitrite undergoes the above decomposition reaction?

a.	3 x 22.4 L
b.	6 x 22.4 L
c.	9 x 22.4 L
d.	12 x 22.4 L
e.	18 x 22.4 L

8. At standard conditions, it was found that 1.12 L of a gas weighed 2.78 g. Its molecular weight is

a.	2.78 g/mol.
b.	27.8 g/mol.
c.	55.6 g/mol.
d.	111 g/mol.
e.	Not enough information is given to solve this problem.

9. At 27?C and 1.00 atm, the density of a gaseous hydrocarbon is 1.79 g·L^-1. The hydrocarbon is

a.	CH4.
b.	C2H4.
c.	C2H6.
d.	C3H8.
e.	C4H8.

10. At 27?C and 0.45 atm, an unknown pure gas has a density of 1.30 g/L. Which of the following gases could be the unknown gas?

a.	NF3
b.	Ne
c.	CO2
d.	CH4
e.	N2

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11. What is the hybridization of the oxygen atoms in hydrogen peroxide, H₂O₂, and formaldehyde, H₂CO, respectively?

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a.	sp^3, sp^3
b.	sp^3, sp^2
c.	sp^2, sp^2
d.	sp^2, sp
e.	sp, sp

12. The number of pi bonds in diazine, HNNH, is

a.	0.
b.	1.
c.	2.
d.	3.
e.	4.

13. All of the following species contain two pi bonds EXCEPT

a.	OCN^-.
b.	H2CCCH2.
c.	CS2.
d.	NO^+.
e.	H2CCH2.

14. Which one of the following species has a Lewis structure most like that of N₂O?

a.	SO2
b.	NO2^-
c.	NO2^+
d.	NO2
e.	NO3^-

15. The number of sigma bonds in CN^- is

a.	0.
b.	1.
c.	2.
d.	3.
e.	4.

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16. The oxalate ion, C₂O₄^2-, has a C-C bond and two oxygen atoms attached to each carbon. How many sigma and pi bonds, respectively, does it have?

a.	3, 2
b.	2, 3
c.	4, 2
d.	5, 2
e.	7, 0

17. Which of the following statements is TRUE?

a.	Sigma bonds are formed only by the overlap of s orbitals.
b.	Sigma bonds are formed only by the overlap of p orbitals.
c.	Sigma bonds are formed only by the overlap of hybridized orbitals.
d.	Sigma bonds are present in double bonds.
e.	Sigma bonds are formed by the sideways overlap of p orbitals.

18. The following bonds ordered according to increasing bond length are

a.	N-N < N=N < NN
b.	NN < N=N < N-N
c.	N-N < NN < N=N
d.	N=N < N-N < NN
e.	N=N < NN < N-N

19. Which of the following species would be expected to have unpaired electron(s)?

1. O₂²⁺
2. O₂
3. NO^-

a.	1 only
b.	2 only
c.	3 only
d.	1 and 3 only
e.	2 and 3 only

20. Pi bonds are formed by the

a.	overlap of hybrid orbitals.
b.	overlap of s orbitals.
c.	endwise overlap of p orbitals.
d.	sidewise overlap of p orbitals.
e.	overlap of s orbitals with p orbitals.

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21. Consider the following diatomic species from the second period:
Be₂, BO, NO, C₂
Which response contains the two paramagnetic species?

a.	Be2 and BO
b.	Be2 and C2
c.	BO and C2
d.	BO and NO
e.	NO and C2

22. The following molecular orbital energy level diagram is appropriate for which one of the listed species?

a.	O2^2+
b.	O2^2-
c.	O2
d.	NO^-
e.	NO

23. The molecular orbital configuration for C₂ is

a.	[core electrons] (s2s)^2 (s2s*)^2 (p2p)^4.
b.	[core electrons] (s2s)^2 (s2s*)^2 (p2p)^2 (s2p)^2.
c.	[core electrons] (s2s)^2 (s2s*)^2 (p2p)^2 (p2p*)^2.
d.	[core electrons] (s2s)^2 (s2s*)^2 (p2p)^2 (s2p*)^2.
e.	[core electrons] (s2s)^2 (s2s*)^2 (p2p*)^4.

24. Which of the following best accounts for the bond order, bond energy, and paramagnetism of O₂?

a.	Valence Shell Electron Pair Repulsion
b.	Valence Bond Theory
c.	Lewis Octet
d.	Band Theory
e.	Molecular Orbital Theory

25. Which of the following species has a bond order of 2?
1. NO^-
2. NO⁺
3. O₂²⁺

a.	1 only
b.	2 only
c.	3 only
d.	1 and 2 only
e.	2 and 3 only

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