1. Chapter 4 Compounds and Their Bonds
4.7
Shapes and Polarity of Molecules
Copyright © by Pearson Education, Inc.
Publishing as Benjamin Cummings

2. VSEPR In the valence-shell electron-pair repulsion theory
(VSEPR), the electron groups around a central atom
are arranged as far apart from each other as possible.
have the least amount of repulsion of the negatively charged electrons.
have a geometry around the central atom that determines molecular shape.

3. Guide to Predicting Molecular Shape (VSEPR Theory)
1. Write the electron-dot structure.
2. Arrange the electron groups around the
central atom to minimize repulsion.
3. Use the atoms bonded to the central to determine the
shape of the molecule.

4. Four Electron Groups In a molecule of CH4,
there are four electron groups around C.
repulsion is minimized by placing four electron groups at angles of 109°, which is a tetrahedral arrangement.
the shape with four bonded atoms is tetrahedral.
Copyright © by Pearson Education, Inc.
Publishing as Benjamin Cummings

5. Three Bonding Atoms and One Lone Pair
In a molecule of NH3,
three electron groups bond to H atoms and the fourth one is a lone (nonbonding) pair.
repulsion is minimized with 4 electron groups in a tetrahedral arrangement.
with three bonded atoms, the shape is pyramidal.
Copyright © by Pearson Education, Inc.
Publishing as Benjamin Cummings

6. Two Bonding Atoms and Two Lone Pairs
In a molecule of H2O,
two electrons groups are bonded to H atoms and two are lone pairs (4 electron groups).
four electron groups minimize repulsion in a tetrahedral arrangement.
the shape with two bonded atoms is bent(~109).
Copyright © by Pearson Education, Inc.
Publishing as Benjamin Cummings

7. Shapes with 4 Electron Groups
Bonded Atoms
Lone Pairs
Bond Angles
Molecular Shape
Example 4
109
tetrahedral
CH4 3 1
~109
Pyramidal
NH3 2
Bent
H2O
Copyright © by Pearson Education, Inc.
Publishing as Benjamin Cummings

8. Learning Check
State the number of electron groups, lone pairs, and use VSEPR theory to determine the shape of the following molecules or ions.
1) tetrahedral ) pyramidal 3) bent
A. PF3
B. H2S
C. CCl4

9. Solution A. PF3 4 electron groups, 1 lone pair, (2) pyramidal B. H2S
4 electron groups, 2 lone pairs, (3) bent
C. CCl4
4 electron groups, 0 lone pairs, (1) tetrahedral

10. Polar Molecules A polar molecule contains polar bonds.
has a separation of positive and negative charge called a dipole indicated with + and -.
has dipoles that do not cancel.
+  • •
H–Cl H—N—H
dipole H
dipoles do not cancel

11. Nonpolar Molecules A nonpolar molecule contains nonpolar bonds.
Cl–Cl H–H
or has a symmetrical arrangement of polar bonds.
O=C=O Cl
Cl–C–Cl Cl
dipoles cancel

12. Determining Molecular Polarity
STEP 1: Write the electron-dot formula.
STEP 2: Determine the polarity of the bonds.
STEP 3: Determine if dipoles cancel.
Example: H2O
. .
H─O: H2O is polar │ H
dipoles do not cancel

13. Learning Check Identify each of the following molecules as
1) polar or 2) nonpolar. Explain.
A. PBr3
B. HBr
C. Br2
D. SiBr4

14. Solution Identify each of the following molecules as
1) polar or 2) nonpolar. Explain.
A. PBr3 1) pyramidal; dipoles don’t cancel; polar
B. HBr 1) linear; one polar bond (dipole); polar
C. Br2 2) linear; nonpolar bond; nonpolar
D. SiBr4 2) tetrahedral; dipoles cancel; nonpolar