Covalent Bonding Review
Name________________________________
Period_________Date___________________
Part I: True & False – If the statement is true, write “true.” If it is false, change the underlined word or
words to make it true.
1. ______________________ A group of atoms united by ionic bonds is called a molecule.
2. ______________________ A covalent bond is formed by a shared pair of electrons.
3. ______________________ A double covalent bond consists of two shared electrons.
4. ______________________ A molecular formula tells you how many atoms are in a single
molecule of the compound.
5. ______________________ The empirical formula for a molecule specifies which atoms are
bonded to each other in the molecule.
6. ______________________ A pair of electrons not involved in bonding is called a shared electron
pair.
7. ______________________ In nonpolar covalent bonds, the electrons are shared unequally
between two atoms.
8. ______________________ Lewis structures use a triple dash to represent a double bond.
Part II: Using your table of electronegativities, calculate the electronegativity difference
between each pair of elements and predict whether the bond formed between them would be
ionic, polar covalent, or nonpolar covalent.
Electronegativity
Difference
9.
H-O
10.
C-H
11.
K-F
12.
N-H
13.
Na-F
14.
O-Cl
Type of Bond
Part III: Write the Lewis Structures for each of the following molecules. Indicate each bond (shared pair
of electrons) with a dash, and each unshared pair of electrons with two dots as directed in class.
15. NH3
18. PCl3
16. H2
19. CCl4
17. C2H4
20. C2H6
Part IV: Short answer
21. Explain the relationship between electronegativity and polarity: ______________________________
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22. Compare and contrast single, double and triple covalent bonds: ______________________________
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