1. Journal Entry: December 13
Determine the molecular geometry of PCl3.
Are the P–Cl bonds in PCl3 polar or nonpolar? Explain the reasoning of your choice.

2. Use the Modeling kits to build all 5 base shapes
The central ball is important
Make sure it has the appropriate number and spacing of holes
Go over the 5 base shapes’ names and angles
Show me your collection when you’re done
Remove one atom at a time and name the shapes and angles as a team

3. Draw the lewis structures, name the shapes, identify the bond angles for:
SOF4
Bromate
SiO2

4. Dipoles and Molecular Polarity
Covalent bonds can be classified as either polar or nonpolar.
Polar bonds are created when there is an unequal sharing of bonded electrons occurring between two atoms (this is due to differences in electronegativity)
Nonpolar bonds are created when there is equal sharing of electrons (same atom, or very small difference in EN like carbon and hydrogen)
Molecules as a whole can also be classified as either polar or nonpolar.
This affects many of the properties of the substance such as boiling point and melting point.

5. Polar Molecules
Polar molecules are created when the center of partial positive charge does not coincide with the center of partial negative charge.
Example: HCl
Polar molecules are often called dipoles.
A dipole is created when the center of partial positive charge and the center of partial negative charge are separated by a short distance.

6. For molecules that contain more than one bond, polar molecules are created when the polar bonds are asymmetrically arranged.
Example: H2O
Molecule has a bent shape.
The molecule has two distinct regions of charge.
Therefore, water is considered a polar molecule.
Polarity of Water Video Clip

7. Nonpolar Molecules
Molecules with polar bonds do not always create polar molecules.
Example: CCl4
Shape is tetrahedral.
This time the centers of positive charge and negative charge coincide.
This has the net effect of cancelling each other.
CCl4 is a nonpolar molecule.

8. Whenever polar bonds are symmetrically arranged, they produce nonpolar molecules.
Another example: CO2

9. Molecular Polarity and Molecular Geometry
The shape of the molecule determines how the bonds are distributed in the molecule.
The following geometries give asymmetrical arrangements and produce polar molecules:
Trigonal pyramidal and bent (Linear if the molecule only contains two atoms)
The following geometries give symmetrical arrangements and produce nonpolar molecules:
Linear, trigonal planar, and tetrahedral.

10. What Do You Think?
CHCl3 is commonly known as chloroform. Would this molecule be considered polar or nonpolar? Explain the reasoning of your choice.

11. Just remember “SNAP”
SNAP Symmetrical Nonpolar Asymmetrical Polar
Molecular polarity is determined by the shape and distribution of charge in the molecule. To make your life easier, just look the atoms.
If the atoms in the molecule are symmetrical, the charges are balanced by each other. The molecules are considered to be nonpolar. 
However, if the molecule is asymmetrical, it is considered to be polar.
So if it is lopsided, it is polar. If it is balanced, it is nonpolar.

12. Intermolecular Forces
The negative region in one polar molecule attracts the positive region in adjacent molecules. So the molecules all attract each other from opposite sides.
The forces of attraction between molecules are known as intermolecular forces.

13. Wrapping It Up
Reflect on what you have learned concerning the day’s topic.
Respond to the following…
What are the three most important things you learned today?
What is one question you would still like answered?
What is the one way what you have learned connects with what you knew before?