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Chapter 9: Bonding Theories

Multiple Choice
Identify the choice that best completes the statement or answers the question.
 

 1. 
For a molecule with the formula AB2 the molecular shape is __________.
a.
linear or bent
b.
linear or trigonal planar
c.
linear or T-shaped
d.
T-shaped
e.
trigonal planar
 

 2. 
According to VSEPR theory, if there are five electron domains in the valence shell of an atom, they will be arranged in a(n) __________ geometry.
a.
octahedral
b.
linear
c.
tetrahedral
d.
trigonal planar
e.
trigonal bipyramidal
 

 3. 
The molecular geometry of the SF2 molecule is __________.
a.
linear
b.
bent
c.
trigonal planar
d.
tetrahedral
e.
octahedral
 

 4. 
The F-B-F bond angle in the BF3 molecule is __________.
a.
90°
b.
109.5°
c.
120°
d.
180°
e.
60°
 

 5. 
According to valence bond theory, which orbitals on bromine atoms overlap in the formation of the bond in Br2?
a.
3s
b.
3p
c.
4s
d.
4p
e.
3d
 

 6. 
The electron-domain geometry of a sulfur-centered compound is trigonal bipyramidal.  The hybridization of the central nitrogen atom is __________.
a.
sp
b.
sp2
c.
sp3
d.
sp3d
e.
sp3d2
 

 7. 
The hybridization of orbitals on the central atom in a molecule is sp. The electron-domain geometry around this central atom is __________.
a.
octahedral
b.
linear
c.
trigonal planar
d.
trigonal bipyramidal
e.
tetrahedral
 

 8. 
The hybridization of orbitals on the central atom in a molecule is sp2. The electron-domain geometry about this central atom is __________.
a.
octahedral
b.
linear
c.
trigonal planar
d.
trigonal bipyramidal
e.
tetrahedral
 

 9. 
In order to produce sp3 hybrid orbitals, __________ s atomic orbital(s) and __________ p atomic orbital(s) must be mixed.
a.
one, two
b.
one, three
c.
one, one
d.
two, two
e.
two, three
 

 10. 
The angles between sp2 orbitals are __________.
a.
45°
b.
180°
c.
90°
d.
109.5°
e.
120°
 

 11. 
There are __________ s and __________ p bonds in the H–CºC–H molecule.
a.
3 and 2
b.
3 and 4
c.
4 and 3
d.
2 and 3
e.
5 and 0
 

 12. 
The basis of the VSEPR model of molecular bonding is __________.
a.
regions of electron density on an atom will organize themselves so as to maximize s-character
b.
regions of electron density in the valence shell of an atom will arrange themselves so as to maximize overlap
c.
atomic orbitals of the bonding atoms must overlap for a bond to form
d.
electron domains in the valence shell of an atom will arrange themselves so as to minimize repulsions
e.
hybrid orbitals will form as necessary to, as closely as possible, achieve spherical symmetry
 

 13. 
According to VSEPR theory, if there are three electron domains in the valence shell of an atom, they will be arranged in a(n) __________ geometry.
a.
octahedral
b.
linear
c.
tetrahedral
d.
trigonal planar
e.
trigonal bipyramidal
 

 14. 
ClF3 has "T-shaped" geometry. There are __________ non-bonding domains in this molecule.
a.
0
b.
1
c.
2
d.
3
e.
4
 

 15. 
In counting the electron domains around the central atom in VSEPR theory, a __________ is not included.
a.
nonbonding pair of electrons
b.
single covalent bond
c.
core level electron pair
d.
double covalent bond
e.
triple covalent bond
 

 16. 
Of the molecules below, only __________ is nonpolar.
a.
CO2
b.
H2O
c.
NH3
d.
HCl
e.
TeCl2
 

 17. 
Of the molecules below, only __________ is nonpolar.
a.
BF3
b.
NF3
c.
IF3
d.
PBr3
e.
BrCl3
 

 18. 
The molecular geometry of the BeCl2 molecule is __________, and this molecule is __________.
a.
linear, nonpolar
b.
linear, polar
c.
bent, nonpolar
d.
bent, polar
e.
trigonal planar, polar
 

 19. 
A typical double bond __________.
a.
is stronger and shorter than a single bond
b.
consists of one s bond and one p bond
c.
imparts rigidity to a molecule
d.
consists of two shared electron pairs
e.
All of the above answers are correct.
 

 20. 
In order to exhibit delocalized p bonding, a molecule must have __________.
a.
at least two p bonds
b.
at least two resonance structures
c.
at least three s bonds
d.
at least four atoms
e.
trigonal planar electron domain geometry
 

 21. 
Electrons in __________ bonds remain localized between two atoms.  Electrons in __________ bonds can become delocalized between more than two atoms.
a.
pi, sigma
b.
sigma, pi
c.
pi, pi
d.
sigma, sigma
e.
ionic, sigma
 

 22. 
The bond order of any molecule containing equal numbers of bonding and antibonding electrons is __________.
a.
0
b.
1
c.
2
d.
3
e.
1/2
 

 23. 
In comparing the same two atoms bonded together, the __________ the bond order, the __________ the bond length, and the __________ the bond energy.
a.
greater, shorter, greater
b.
greater, greater, greater
c.
greater, longer, greater
d.
greater, greater, smaller
e.
smaller, greater, greater
 

 24. 
In molecular orbital theory, the s1s orbital is __________ and the s1s* orbital is __________ in the H2 molecule.
a.
filled, filled
b.
filled, empty
c.
filled, half-filled
d.
half-filled, filled
e.
empty, filled
 

 25. 
Based on molecular orbital theory, the bond order of the H–H bond in the H2+ ion is __________.
a.
0
b.
1/2
c.
1
d.
3/2
e.
2
 

 26. 
According to MO theory, overlap of two s atomic orbitals produces __________.
a.
one bonding molecular orbital and one hybrid orbital
b.
two bonding molecular orbitals
c.
two bonding molecular orbitals and two antibonding molecular orbitals
d.
two bonding molecular orbitals and one antibonding molecular orbital
e.
one bonding molecular orbital and one antibonding molecular orbital
 

 27. 
A molecular orbital can accommodate a maximum of __________ electron(s).
a.
one
b.
two
c.
four
d.
six
e.
twelve
 

 28. 
Molecular Orbital theory correctly predicts paramagnetism of oxygen gas, O2. This is because __________.
a.
the bond order in O2 can be shown to be equal to 2.
b.
there are more electrons in the bonding orbitals than in the antibonding orbitals.
c.
the energy of the p2p MOs is higher than that of the s2p MO
d.
there are two unpaired electrons in the MO electron configuration of  O2
e.
the O–O bond distance is relatively short
 

 29. 
Molecular Orbital theory correctly predicts diamagnetism of fluorine gas, F2. This is because __________.
a.
the bond order in F2 can be shown to be equal to 1.
b.
there are more electrons in the bonding orbitals than in the antibonding orbitals.
c.
all electrons in the MO electron configuration of F2 are paired.
d.
the energy of the p2p MOs is higher than that of the s2p MO
e.
the F–F bond enthalpy is very low
 

 30. 
Based on molecular orbital theory, the bond order of the Be–Be bond in the Be2 molecule is __________.
a.
0
b.
1
c.
2
d.
3
e.
4
 

 31. 
An antibonding MO __________ the corresponding bonding MO.
a.
is always lower in energy than
b.
can accommodate more electrons than
c.
can accommodate fewer electrons than
d.
is always higher in energy than
e.
is always degenerate with
 



 
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