Chemistry: Covalent Bonds Ch 8 Review
1.	What are dispersion forces? How is the strength of dispersion forces related to the number of electrons in a molecule? Give an example of molecules that are attracted to each other by dispersion forces.
2.	Indicate how bonding is explained in terms of molecular orbitals.
3.	Explain a pi bond and a sigma bond. Which of these bond types tends to be the weaker? Why?
4.	Explain what is meant by VSEPR theory. Give an example of how VSEPR theory can be applied to predict the shape of a molecule.
5.	What determines the degree of polarity in a bond? Distinguish between nonpolar covalent, polar covalent, and ionic bonds in terms of relative polarity.
6.	How many electrons are shared in a single covalent bond?
7.	How many electrons does a nitrogen atom need to gain in order to attain a noble-gas electron configuration?
8.	How many unshared pairs of electrons does the nitrogen atom in ammonia possess?
9.	How many electrons does carbon need to gain in order to obtain a noble-gas electron configuration?
10.	How many electrons are shared in a double covalent bond?
11.	What is the bond angle in a water molecule?
12.	What is bond dissociation energy, and how does it affect carbon compounds?
13.	Can some atoms exceed the limits of the octet rule in bonding? If so, give an example.
14.	What element(s) form compounds that exceed the octet rule with 12 electrons?
15.	What element can form diatomic molecules held together by triple covalent bonds?
16.	Which noble gas has the same electron configuration as the oxygen in a water molecule?
17.	What element can form diatomic molecules by a double covalent bond?
18.	What bond type (sigma/pi) is normally the weakest?
19.	Determine which atom acquires the most negative charge in a covalent bond with hydrogen?
20.	What causes hydrogen bonding?
21.	Which is a typical characteristic of an ionic compound?
22.	How do atoms achieve noble-gas electron configurations in single covalent bonds?
23.	Why do atoms share electrons in covalent bonds?
24.	A molecule with a single covalent bond is ____.
25.	Once formed, how are coordinate covalent bonds different from other covalent bonds?
26.	When H forms a bond with HO to form the hydronium ion HO, this bond is called a coordinate covalent bond because ____.
27.	How is a pair of molecular orbitals formed?
28.	The side-by-side overlap of p orbitals produces what kind of bond?
29.	Where are the electrons most probably located in a molecular bonding orbital?
30.	Sigma bonds are formed as a result of the overlapping of which type(s) of atomic orbital(s)?
31.	What causes water molecules to have a bent shape, according to VSEPR theory?
32.	What type of hybrid orbital exists in the methane molecule?
33.	What is the shape of a molecule with a triple bond?
34.	What type of hybridization occurs in the orbitals of a carbon atom participating in a triple bond with another carbon atom?
35.	How many pi bonds are formed when sp hybridization occurs in ethene, CH?
36.	Why is hydrogen bonding only possible with hydrogen?
37.	When one atom contributes both bonding electrons in a single covalent bond, the bond is called a(n) ____.
38.	A bond formed between a silicon atom and an oxygen atom is likely to be ____.
39.	Explain what a polar molecule is. Provide an example.

Vocabulary
coordinate covalent bond
single covalent bond
double covalent bond
polar bond
structural formula
hydrogen bond
network solid
tetrahedral angle
bonding orbital
VSEPR theory
dipole interaction
sigma bond
bond dissociation energy