CI2: p-p overlap Constructive overlap along the same axis forms a sigma bond +(+ o bonding mo Chapter 2
Chapter 2 6 Cl2 : p-p overlap => Constructive overlap along the same axis forms a sigma bond
HCI: S-p overlap Question Draw the predicted shape for the bonding molecular orbital and the antibonding molecular orbital of the hcl molecule Answer: See bottom of page 42 in your text Chapter 2
Chapter 2 7 HCl: s-p overlap Question: Draw the predicted shape for the bonding molecular orbital and the antibonding molecular orbital of the HCl molecule. Answer: See bottom of page 42 in your text. =>
Pi Bonding Pi bonds form after sigma bonds Sideways overlap of parallel p orbitals node destructive(antibonding) interaction T antibonding mo ener constructive(bonding) interaction T bonding mo Chapter 2
Chapter 2 8 Pi Bonding • Pi bonds form after sigma bonds. • Sideways overlap of parallel p orbitals. =>
Multiple Bonds a double bond(2 pairs of shared electrons) consists of a sigma bond and a pi bond a triple bond (3 pairs of shared electrons consists of a sigma bond and two pi bonds half of Tr bond H H C o bond C H(sp sp(H H p. half of r bond Chapter 2
Chapter 2 9 Multiple Bonds • A double bond (2 pairs of shared electrons) consists of a sigma bond and a pi bond. • A triple bond (3 pairs of shared electrons) consists of a sigma bond and two pi bonds. =>
Molecular Shapes Bond angles cannot be explained with simple s and p orbitals. Use VsEPr theory. Hybridized orbitals are lower in energy because electron pairs are farther apart Hybridization is lCao within one atom just prior to bonding Chapter 2 10
Chapter 2 10 Molecular Shapes • Bond angles cannot be explained with simple s and p orbitals. Use VSEPR theory. • Hybridized orbitals are lower in energy because electron pairs are farther apart. • Hybridization is LCAO within one atom, just prior to bonding. =>