Necessary Molecules, Shape, Polarity, etc.

H2O

• 2 bonds, 2 lp

• sp3

• bent

• 104.5

• 2 sigma bonds, no pi bonds

• asymmetric, polar (bond dipoles do not cancel)

CO2

• two double bonds

• sp

• linear

• 180

• 2 sigma, 2 pi

• symmetry, nonpolar

N2

• one triple bond

• sp

• linear

• 180

• 1 sigma, 2 pi

• nonpolar bond, nonpolar

F2

• one single bond

• sp3

• linear

• 180

• 1 sigma, no pi

• nonpolar bond, nonpolar

NH3

• 3 single bonds

• sp3

• trigonal pyramidal

• 107

• 3 sigma, no pi

• asymmetry, polar

HF

• 1 single bond

• F is sp3

• linear

• 180

• 1 sigma, no pi

• asymmetry, polar (f is more electronegative)

CH4

• 4 single bonds

• sp3

• tetrahedral

• 109.5

• 4 sigma, no pi

• symmetrical, all nonpolar bonds, nonpolar

SiBr4

• 4 single bonds

• sp3

• tetrahedral

• 109.5

• 4 sigma, no pi

• polar bonds but dipoles cancel due to symmetry, nonpolar

• Despite being similar in shape, SiBr4 will have larger boiling point than CH4 due to larger electron cloud (think of H v. Br), which means stronger IMFs