Molecule Shapes

Molecule Shapes

1. 2 e- pairs gives you a linear shape with a bond angle of 180 degrees.

2. 3e- pairs give you a trigonal planar shape with a bond angle of 120 degrees.

3. 4e- pairs give you a tetrahedral shape with a bond angle of 109.5 degrees.

4. 5e- pairs give you a trigonal bipyramid with two bond angles of 90/120 degrees

5. 6e- pairs give you a octahedral shape with a bond angle of 90 degrees.

6. Lone pair of electrons account for approximately 2.5 degrees, so subtract 2.5 degrees from the normal bond angle of that shape for every lone pairs of electrons present

7. Don't forget to account for the charge on a compound. + charge = subtract electrons, - charge = add electrons