VSEPR & Determining the Polarity of Molecules
(Valence Shell Electron Pair Repulsion Theory)
Lewis structures look at molecules in a two dimensional way; however molecules are NOT two dimensional. Many
of the properties of molecular compounds depend on the three dimensional shape of the molecule. The shape of a
molecule is predicted by using the VSEPR theory:
____________________________ the electrostatic repulsion between the valence level electron pairs surrounding
an atom causes these pairs to be oriented as far apart as possible.
To use VSEPR theory:
1. Draw the Lewis Dot Structure for the molecule.
2. Determine the number of links on the central atom (single, double and triple bonds all count as one link.)
3. Determine the number of lone pairs on the central atom.
Number of Links on
Central Atom
2
3
2
2
4
3
Number of Lone Pairs
on Central Atom
0
0
1
2
0
1
Shape of Molecule
Linear
Trigonal Planar
Bent
Bent
Tetrahedral
Trigonal Pyramidal
Polar Molecule vs Nonpolar Molecules
______- If the electrons in a molecule are not evenly distributed, the molecule can have a negative and positive side
______________ – All the electrons are evenly distributed
________________________ states polar substances dissolve polar substances and nonpolar substances dissolve
nonpolar substances.
We can determine if a molecule is polar or nonpolar by looking at the Lewis Dot Structure and following the rules
below:
To determine if a molecule is a polar or nonpolar, look at the central atom.
1. If the central atom has no lone pairs and has all the same types of atoms attached to it, then the molecule is
nonpolar.
2. If the central atom has no lone pairs but different atoms attached to it, the molecule is polar.
3. If the central atom has lone pairs, the molecule is polar,
Draw the Lewis Dot structure, determine the shape and if the molecule is polar/nonpolar for each of the following…
1.
N
A
S
L
NH3
2.
N
A
S
L
CCl4
bonds
Lone Pairs
bonds
Lone Pairs
Lewis Structures, VSEPR, and Molecule Polarity Homework
Draw the Lewis Structure for each compound or ion listed below, give its shape, and determine if it’s polar or not:
1.
HOCl
6. HOF
Shape:
Shape:
Polar or nonpolar:
Polar or nonpolar:
2.
7. CS2
Cl2CO
Shape:
Shape:
Polar or nonpolar:
Polar or nonpolar:
3. CHClF2
8. HBF2
Shape:
Shape:
Polar or nonpolar:
Polar or nonpolar:
4. NH2Cl
9. SiH4
Shape:
Shape:
Polar or nonpolar:
Polar or nonpolar:
5. Cl2O
10. SO2
Shape:
Shape:
Polar or nonpolar:
Polar or nonpolar:
VSEPR Homework 1-10
Draw the Lewis Structure for each compound or ion listed below, give its shape, and determine if it’s polar or not:
1. FCl2+
6. SO3
Shape:
Shape:
Polar or nonpolar:
Polar or nonpolar:
2. CS2
7. FO3-
Shape:
Shape:
Polar or nonpolar:
Polar or nonpolar:
3. AsO3-3
8. N2O (put 1 N in the middle)
Shape:
Polar or nonpolar:
4. IO4-
Shape:
Polar or nonpolar:
Shape:
Polar or nonpolar:
9. H2CO
Shape:
Polar or nonpolar:
5. SeO2
10. NO2-
Shape:
Shape:
Polar or nonpolar:
Polar or nonpolar:
VSEPR Homework 11-20
Draw the Lewis Structure for each compound or ion listed below, give its shape, and determine if it’s polar or not:
11. SbH3
16. PCl4+
Shape:
Shape:
Polar or nonpolar:
Polar or nonpolar:
12. NF3
17. CO3-2
Shape:
Shape:
Polar or nonpolar:
Polar or nonpolar:
13. IO2-
18. SiO4-4
Shape:
Polar or nonpolar:
14. NO3-
Shape:
Polar or nonpolar:
Shape:
Polar or nonpolar:
19. BF3
Shape:
Polar or nonpolar:
15. CNBr
20. CBr4
Shape:
Shape:
Polar or nonpolar:
Polar or nonpolar: