Name ______________________________________ Hour______
What will be on Wednesday’s test?





Covalent basics
Covalent nomenclature
Drawing Lewis Structures
Determining whether a bond is polar, nonpolar, or ionic using electronegavities
Determining whether a molecule is poar or nonpolar
Review
1. In your own words, write the rules for naming covalent molecules.
2. Write the prefixes for 1-6
1-2-4--
5--
3. Write formulas for the following molecules
Nitrogen monoxide
3—
6--
Sulfur hexafluoride
Phosphorous pentachloride
Carbon tetrahydride
Nitrogen trihydride
Dicarbon hexahydride
Carbon dioxide
Silicon tetrafluoride
Diphosphorus dioxide
Dinitrogen pentoxide
4. Name the following molecules
CBr4
SO2
N2O4
BF3
PF5
C2H6
SI6
SeO2
CO
SiO3
5. A covalent molecule is made of two _____________________ with high ______________________________
and _________________________________
6. What is happening to electrons in a covalent molecule vs. an ionic compound?
7. Draw Lewis Structures for the following molecules: I2, CH4, NO3-, CO2, SO2, NF3, PF5, SBr6
8. What is a resonance structure? Draw all of the resonance structures for CO32-
9. If the electronegativity difference is _____________________, the molecule is nonpolar. If the difference is
____________________, the molecule is polar, and if it is ___________________________ the molecule is
considered ionic.
10. What does it mean if a bond is polar? What does it mean if a bond is nonpolar?
11. In a polar bond, which atom in the bond is considered “partially positive” and which is considered “partially
negative” and WHY? Use H—Cl as an example.
12. Fill in the table below
Bond
Electronegativity
difference
Polar,
Nonpolar,
Ionic
Bond
H—C
K—S
Na—Cl
C—F
C—Br
H—F
N—O
P—H
P—Cl
S—O
Electronegativity
difference
13. Determine if the following molecules are polar or nonpolar. Draw dipoles to help you.
Polar,
Nonpolar,
Ionic