Molecular Shapes

1
Molecular Shapes
2
Review from yesterday

• Determine the Lewis structure for
• CO
• N2O
• OCl2
• SiO2
• AlBr3

3
VSEPR

• Valence Shell Electron Pair Repulsion model
• The like charges of the electrons repel one
  another.
• Therefore, each electron
• pair gets the most amount
• of room as possible.

4
Linear

• Can occur with 2 pairs total, both bonding
• OR if there are two double bonds
• Contains NO lone pairs
• Bond angle 180
• CO2
• BeH2
• BeCl2

5
Tetrahedral

• Occurs with 4 total pairs for the central atom
  and all in bonds.
• Contains NO lone pairs
• Bond angle 109.5
• CH4
• CCl4

6
Trigonal Pyramidal

• Contains 4 total pairs 3 bonding pairs and ONE
  LONE PAIR
• Bond angle 107.3
• PH3
• Ammonia

7
Bent

• Occurs with 4 pairs total 2 bonded and 2 lone
  pairs
• Bond angle 104.5
• H2Se
• H2O

8
Now, lets go back to theum, nevermind.

• Return to todays warm-up assignment and note the
  molecular geometry and bond angle for each of the
  molecules.