Name: _______________________________ Date: _____________________
Period: _________
Covalent Bonding and Mixed Nomenclature Review
Bonding:
1. What type of elements (metal, nonmetal, or metalloid) are found in each of the following compounds or
bonds
a. Molecular compounds
c. Ionic compound
e. Polar compound
b. Covalent compounds
d. Acids
f. Nonpolar compounds
2. What type of bond (single, double, or triple) holds each of the following diatomic molecules together?
a. Oxygen O2
c. Fluorine F2
e. Chlorine Cl2
g. water
b. Nitrogen N2
d. Hydrogen H2
f. SO
h. NH3
3. How many lone pairs surround each element in the following diatomic molecules?
a. Oxygen O2
c. Fluorine F2
e. Chlorine Cl2
g. oxygen in water
b. Nitrogen N2
d. Hydrogen H2
f. SO
h. nitrogen in NH3
4. Classify each of the following compound as Ionic, Covalent or an Acid
a. CS2
d. CaSO4
g. N2O4
b. BaI2
e. PCl3
h. VO3
c. HP
f. H3PO3
i. PCl5
5. Classify each of the following as polar or nonpolar covalent bonds
a. O2
c. H2O
e. FCl
b. HCl
d. SO
g. SCl2
Naming
6. What covalent prefix corresponds to each of the following numbers
a. One
d. Four
g. Seven
j. Ten
b. Two
e. Five
h. Eight
c. Three
f. Six
i. Nine
7. When naming a transition metal ion that can have more than one common ionic charge, the numerical value
of the charge is indicated by a __________________________.
8. When the name of the polyatomic ion that is part of an acid ends in -ite, the acid name includes the suffix
________________________________________.
9. When the name of the polyatomic ion that is part of an acid ends in -ate, the acid name includes the suffix
________________________________________.
10. In naming a binary covalent compound, the number of atoms of each element present in the molecule is
indicated by ___________________________________.
11. For the following items if given the name write the chemical formula and if given the formula write the
name
1. Phosphorous acid
9. S2F6
2. Phosphorous pentachloride
10. Vanadium (IV) sulfide
3. Aluminum oxide
11. HBr
4. Fe2(SO4)3
12. Calcium sulfate
5. Iron (III) chloride
13. Hydrosulfuric acid
6. SO3
14. Sulfuric acid
7. AlPO4
15. KCl
8. H2SO3
16. CoO2
Properties
12. Ionic bonds form by _________________________________ electrons, covalent bonds form by
_____________electrons.
13. Ionic compound have _______________ melting and boiling points while covalent compounds have
__________________.
Lewis Structures
14. Draw the Lewis Structure for CF2S, and complete the table below showing number and types of
bonds or lone pairs that each element has.
C
F
S
Single Bond
Double Bond
Triple Bond
Lone Pair Electrons
15. Draw the Lewis Structure for CH3I, and complete the table below showing number and types of
bonds or lone pairs that each element has.
C
H
I
Single Bond
Double Bond
Triple Bond
Lone Pair Electrons
16. Draw the Lewis Structure for HCN, and complete the table below showing number and types of
bonds or lone pairs that each element has.
H
Single Bond
Double Bond
Triple Bond
Lone Pair Electrons
C
N