Chapter 2:
Chemical Bonds
1. The ionic model of binding is best utilized to describe what type of atoms joining
together?
a. Two metallic elements.
b. Two non-metallic elements.
c. A metallic and a non-metallic element, especially a metallic p-block element.
d. A non-metallic and a metallic element, especially a metallic s-block element.
Answer:
D
2. Why are ionic structures typically brittle, and why do they have high melting points?
a. Because they are stacked in irregular, non-crystalline structures displaying large,
coulombic interactions.
b. Because they are stacked in regular, crystalline structures displaying large, coulombic
interactions.
c. Because they are stacked in regular, crystalline structures displaying small, ionic
interactions
d. None of the above.
Answer:
B
3. What atom has the electron configuration [Ar]3d104s24p2?
a. Si
b. Ga
c. Ge
d. Sn
Answer:
C
4. Which elements, when forming molecules, do not reach an octet in their Lewis
structures?
a. He, Li, and F.
b. H, Li, and Mg.
c. He, Li, and Be.
d. H, Li, and Be.
Answer:
D
5. What property do all covalent bonds have in common?
a. The sharing of pairs of electrons.
b. The loss of one or more outer shell electrons.
c. The gain of one or more outer shell electrons.
d. The loss or gain of one or more outer shell electrons.
Answer:
A
6.
a.
b.
c.
How is a multiple bond defined?
By the presence of two or more electrons in at least one bond in the Lewis structure.
By the presence of four or more electrons in at least one bond in the Lewis structure.
By the presence of one or more bonds in the Lewis structure.
d. By the presence of four or more electrons shared between two or more atoms in the
Lewis structure.
Answer:
B
7. What does a resonance structure represent?
a. A blending of two or more representations of a molecule’s atomic placement.
b. A blending of two or more representations of an atom’s atomic placement.
c. A hybrid between two or more representations of a molecule’s Lewis structure.
d. A hybrid between two or more representations of an atom’s Lewis structure.
Answer:
C
8.
a.
b.
c.
Why is formal charge used in determining Lewis structures of certain molecules?
It is not; rather, it is used only to determine the charges on atoms in a molecule.
It can predict the polarizability of the molecule.
It can predict the most chemically stable placement of inner electrons in bonds within
the structure.
d. It can predict the most favorable arrangement of atoms within the structure.
Answer:
D
9. What electron arrangement must a compound have to be considered a radical?
a. One or more unshared electrons pairs within the compound.
b. One or more metallic elements with an unpaired electron in the molecule.
c. At least one unpaired electron somewhere in the molecule.
d. At least one atom in a molecule with more than eight electrons.
Answer:
C
10. How are most actual bonds defined in terms of the ionic and covalent models?
a. As mostly ionic.
b. As mostly covalent.
c. As somewhere between purely covalent and purely ionic bonds.
d. As none of the above.
Answer:
C
11. How is ionic character in a bond determined using electronegativities?
a. The greater the electronegativity difference between the atoms in a bond, the more
ionic character the bond exhibits.
b. The greater the electronegativity difference between the atoms in a bond, the less
ionic character the bond exhibits.
c. The less the electronegativity difference between the atoms in a bond, the more ionic
character the bond exhibits.
d. There is no direct correlation between electronegativity and ionic bond character.
Answer:
A
12. For a cation to have a high polarizing power, what requirements must be met?
a. It must be either large or highly charged.
b. It must be either small or of low charge.
c. It must be both large and highly charged.
d. It must be both small and highly charged.
Answer:
D
13. Dissociation energy is a measure of what?
a. The energy added to a bond to force its electrons to separate.
b. The energy required to separate bonded atoms.
c. The energy required to cause new bonds to form in a molecule.
d. None of the above.
Answer:
B
14. How does bond strength change as multiplicity in a bond decreases?
a. It decreases.
b. It increases.
c. It decreases only when the bond is between polarizable atoms.
d. It increases only when the bond is between polarizable atoms.
Answer:
A
15. Why are multiple bonds longer than single bonds?
a. Because of additional bonding electrons.
b. Because more electrons in the multiple bond require more physical space.
c. Because more electrons in the bond push the bonding nuclei farther apart.
d. They are not longer; rather, they are shorter because of additional bonding electrons.
Answer:
D