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Chapter 8 Bonding General Concepts

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

 1. 
There are __________ paired and __________ unpaired electrons in the Lewis symbol for a phosphorus atom.
a.
4, 2
b.
2, 4
c.
2, 3
d.
4, 3
e.
0, 3
 

 2. 
Based on the octet rule, magnesium most likely forms a __________ ion.
a.
Mg2+
b.
Mg2-
c.
Mg6-
d.
Mg6+
e.
Mg-
 

 3. 
How many unpaired electrons are there in the Lewis structures of a N3- ion?
a.
0
b.
1
c.
2
d.
3
e.
This cannot be predicted.
 

 4. 
For a given arrangement of ions, the lattice energy increases as ionic radius __________ and as ionic charge __________.
a.
decreases, increases
b.
increases, decreases
c.
increases, increases
d.
decreases, decreases
e.
This cannot be predicted.
 

 5. 
Elements from opposite sides of the periodic table tend to form __________.
a.
covalent compounds
b.
ionic compounds
c.
compounds that are gaseous at room temperature
d.
homonuclear diatomic compounds
e.
covalent compounds that are gaseous at room temperature
 

 6. 
Determining lattice energy from Born-Haber cycle data requires the use of __________.
a.
the octet rule
b.
Coulomb's law
c.
Periodic law
d.
Hess's law
e.
Avogadro's number
 

 7. 
A double bond consists of __________ pairs of electrons shared between two atoms.
a.
1
b.
2
c.
3
d.
4
e.
6
 

 8. 
What is the maximum number of double bonds that a hydrogen atom can form?
a.
0
b.
1
c.
2
d.
3
e.
4
 

 9. 
In the molecule below, which atom has the largest partial negative charge __________?

mc009-1.jpg
a.
Cl
b.
F
c.
Br
d.
I
e.
C
 

 10. 
The ability of an atom in a molecule to attract electrons is best quantified by the __________.
a.
paramagnetism
b.
diamagnetism
c.
electronegativity
d.
electron change-to-mass ratio
e.
first ionization potential
 

 11. 
Given the electronegativities below, which covalent single bond is most polar?

Element:
H
C
N
O
Electronegativity:
2.1
2.5
3.0
3.5
a.
C-H
b.
N-H
c.
O-H
d.
O-C
e.
O-N
 

 12. 
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a.
decreases, increases
b.
increases, increases
c.
increases, decreases
d.
stays the same, increases
e.
increases, stays the same
 

 13. 
A nonpolar bond will form between two __________ atoms of __________ electronegativity.
a.
different, opposite
b.
identical, different
c.
different, different
d.
similar, different
e.
identical, equal
 

 14. 
The formal charge on carbon in the molecule below is __________.

mc014-1.jpg
a.
0
b.
+1
c.
+2
d.
+3
e.
-1
 

 15. 
The formal charge on nitrogen in NO3- is __________.
mc015-1.jpg
a.
-1
b.
0
c.
+1
d.
+2
e.
-2
 

 16. 
Using the table of average bond energies below, the DH for the reaction is __________ kJ.

mc016-1.jpg

Bond:
CºC
C=C
H-I
C-I
C-H
D (kJ/mol):
839
348
299
240
413
a.
+160
b.
-160
c.
-217
d.
-63
e.
+63
 

 17. 
Using the table of average bond energies below, the DH for the reaction is __________ kJ.

H – CºC–H (g)  +  H–I (g) ® H2C=CHI (g)

Bond:
CºC
C=C
H-I
C-I
C-H
D (kJ/mol):
839
614
299
240
413
a.
+506
b.
-931
c.
-506
d.
-129
e.
+129
 

 18. 
Lattice energy is __________.
a.
the energy required to convert a mole of ionic solid into its constituent ions in the gas phase
b.
the energy given off when gaseous ions combine to form one mole of an ionic solid
c.
the energy required to produce one mole of an ionic compound from its constituent elements in their standard states
d.
the sum of ionization energies of the components in an ionic solid
e.
the sum of electron affinities of the components in an ionic solid
 

 19. 
The diagram below is the Born-Huber cycle for the formation of crystalline potassium fluoride. 

mc019-1.jpg

Which energy change corresponds to the electron affinity of fluorine?
a.
2
b.
5
c.
4
d.
1
e.
6
 

 20. 
The diagram below is the Born-Huber cycle for the formation of crystalline potassium fluoride. 

mc020-1.jpg

Which energy change corresponds to the first ionization energy of potassium?
a.
2
b.
5
c.
4
d.
3
e.
6
 

 21. 
In which of the molecules below is the carbon-carbon distance the shortest?
a.
H2Cmc021-1.jpgCH2
b.
H-CºC-H
c.
H3C-CH3
d.
H2Cmc021-2.jpgCmc021-3.jpgCH2
e.
H3C-CH2-CH3
 

 22. 
The Lewis structure of the CO32- ion is __________.
a.

mc022-1.jpg
b.

mc022-2.jpg
c.

mc022-3.jpg
d.

mc022-4.jpg
e.

mc022-5.jpg
 

 23. 
Resonance structures differ by __________.
a.
number and placement of electrons
b.
number of electrons only
c.
placement of atoms only
d.
number of atoms only
e.
placement of electrons only
 

 24. 
For resonance forms of a molecule or ion, __________.
a.
one always corresponds to the observed structure
b.
all the resonance structures are observed in various proportions
c.
the observed structure is an average of the resonance forms
d.
the same atoms need not be bonded to each other in all resonance forms
e.
there cannot be more than two resonance structures for a given species
 

 25. 
The central atom in __________ violates the octet rule.
a.
NH3
b.
SeF2
c.
BF3
d.
AsF3
e.
CF4
 

 26. 
A valid Lewis structure of __________ cannot be drawn without violating the octet rule.
a.
ClF3
b.
PCl3
c.
SO3
d.
CCl4
e.
CO2
 

 27. 
Which atom can accommodate an octet of electrons, but doesn't necessarily have to accommodate an octet?
a.
N
b.
C
c.
H
d.
O
e.
B
 

 28. 
Of the bonds C-N, Cmc028-1.jpgN, and CºN, the C-N bond is __________.
a.
strongest/shortest
b.
strongest/longest
c.
weakest/shortest
d.
weakest/longest
e.
intermediate in both strength and length
 



 
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