An orbital by any other name...

Types of bonds

1.   Ionic
2.   Covalent
   1. One bond uses 2 AOs; two electrons

      

      1. Nonpolar
      2. Polar

Molecular orbital theory

1. Pure AOs
   1. MOs = 1s ± 1s ; get 1 new MO for every AO used:

      

       

      

2. Hybrid AOs

   Observed bond angles in carbon compounds:

   

                                                

   1. Tetrahedral carbon

      2s + 2p_x + 2p_y + 2p_z = four sp³

                     

      four 1s + four sp³ = 4 s + 4 s *

      

       

   2. Trigonal (planar) carbon

      2s + 2p_x + 2p_y + 2p_z = three sp² + 2p_z

                     

      six sp² + four 1s + two 2p_z = five s and one p + five s* + one p*

           

       

   3. Linear carbon

      2s + 2p_x + 2p_y + 2p_z = two sp + 2p_y + 2p_z

                     

      four sp + two 1s + four 2p = three s + two p bonding + three s * + two p *