1. MO diagram for homonuclear diatomic molecules Li 2 through N 2 MO diagram for homonuclear diatomic molecules O 2 and F 2

2. N 2 Lewis diagram :N  N: each atom supplies 5 electrons; a total of 10 electrons must be assigned N 2 :  2s 2  * 2s 2  2p 4  2p 2 Bond order for N 2 = 0.5 (8 - 2) = 3

3. O 2 Molecular Orbital Theory O 2 :  2s 2  * 2s 2  2p 2  2p 4  * 2p 1  * 2p 1 Unpaired electrons - paramagnetic Bond order = 2 Agrees with Lewis diagram Lewis model

5. Heteronuclear diatomics - electrons are unequally shared by the two atoms due to electronegativity differences.  = c A  A + c B  B Where c A and c B are coefficients which indicate the contribution of each AO in the MO In a homonuclear molecule: c A = c B = 1

6. MO energy-level diagram for a AB type molecule. A is more electronegative than B Energy levels of the more electronegative element is lower than the less electronegative element  : higher contribution from A2s   : higher contribution from B2s

7. CO - ten valence electrons CO:  2s 2  * 2s 2  2p 4  2p 2 Bond order = 0.5 (8 - 2) = 3 Highest occupied MO (HOMO) Lowest unoccupied MO (LUMO)

8. Polyatomics - same principles as diatomics except that the MOs spread all over the atoms in the molecule An electron pair helps to bind the whole molecule, not just a pair of atoms. H 2 O: six atomic orbitals (one O2s, three O2p, and two H1s) These six orbitals are used to build six molecular orbitals in which the degree of net bonding characters is related to the number of internuclear nodes.

9. Molecular Orbitals of H 2 O

11. http://www.shef.ac.uk/chemistry/orbitron/ http://www.whfreeman.com/chemicalprinciples/con_index.ht m?03

12. Spectroscopy Spectroscopy: interaction of light with matter Average Bond energies (kJ/mol) C-H: 413C=C: 610H-F: 565 H-H: 436C  C: 835