The molecular orbital model can be used to predict molecular structure, bonding properties, and magnetism. Molecular orbitals are formed from the constructive and destructive interference of overlapping atomic orbitals. Bonding molecular orbitals lower energy and contain bonding electrons, while antibonding orbitals have higher energy. Bond order is calculated from the difference between bonding and antibonding electrons. Homonuclear diatomic molecules like H2, Li2, and B2 as well as heteronuclear diatomics like NO can be analyzed using molecular orbital theory to determine properties like bond strength.

1. Covalent Bonding Orbitals

2. Hybridization and the Localized Electron Model

5. Hybridization

6. Hybridization

7. sp 3 example: Methane

8. sp 3 example: Ammonia

9. sp 2 Hybridization

10. sp 2 Hybridization

12. sp 2 Hybridization

13. sp 2 Hybridization: Ethylene

15. sp 2 Hybridization: Ethylene

17. sp Hybridization

18. sp Hybridization: CO 2

19. sp Hybridization: CO 2

20. sp Hybridization: CO 2

21. sp Hybridization: N 2

27. Effective Pairs and Their Spatial Arrangement

28. The Molecular Orbital Model

36. Bonding and Antibonding

42. Bonding in Homonuclear Diatomic Molecules

52. Paramagnetism

58. Bonding in Heteronuclear Diatomic Molecules

63. Combining the Localized Electron and MO models

69. The End

70. MO Worksheet B 2 C 2 N 2 O 2 F 2 σ 2p * σ 2p * π 2p * π 2p * σ 2p π 2p π 2p σ 2p σ 2s * σ 2s * σ 2s σ 2s σ 1s * σ 1s * σ 1s σ 1s