1. Chapter 9 Covalent Bonding: Orbitals Hybridization The mixing of atomic orbitals to form special orbitals for bonding. The atoms are responding as needed to give the minimum energy for the molecule.

2. The Valence Orbitals on a Free Carbon Atom: 2s, 2p x, 2p y, and 2p z

3. The Formation of sp 3 Hybrid Orbitals

4. An Energy-Level Diagram Showing the Formation of Four sp 3 Orbitals

5. Tetrahedral Set of Four sp 3 Orbitals

6. The Nitrogen Atom in Ammonia is sp 3 Hybridized

7. sp 3 Hybridization The experimentally known structure of CH 4 molecule can be explained if we assume that the carbon atom adopts a special set of atomic orbitals. These new orbital are obtained by combining the 2s and the three 2p orbitals of the carbon atom to produce four identically shaped orbital that are oriented toward the corners of a tetrahedron and are used to bond to the hydrogen atoms. Whenever a set of equivalent tetrahedral atomic orbitals is required by an atom, this model assumes that the atom adopts a set of sp 3 orbitals; the atom becomes sp 3 hybridized.

8. The Hybridization of the s, p x, and p y Atomic Orbitals

9. An Orbital Energy-Level Diagram for sp 2 Hybridization

10. A sigma (  ) bond centers along the internuclear axis. A pi (  ) bond occupies the space above and below the internuclear axis.

11. An sp 2 Hybridized C Atom

12. The  Bonds in Ethylene

13. Sigma and Pi Bonding

14. The Orbitals for C 2 H 4

15. When One s Orbital and One p Orbital are Hybridized, a Set of Two sp Orbitals Oriented at 180 Degrees Results

16. The Hybrid Orbitals in the CO 2 Molecule

17. The Orbital Energy-Level Diagram for the Formation of sp Hybrid Orbitals on Carbon

18. The Orbitals of an sp Hybridized Carbon Atom

19. The Orbital Arrangement for an sp 2 Hybridized Oxygen Atom

20. The Orbitals for CO 2

21. The Orbitals for N 2

22. A Set of dsp 3 Hybrid Orbitals on a Phosphorus Atom

23. An Octahedral Set of d 2 sp 3 Orbitals on a Sulfur Atom

24. The Relationship of the Number of Effective Pairs, Their Spatial Arrangement, and the Hybrid Orbital Set Required

25. The Localized Electron Model Three Steps:  Draw the Lewis structure(s)  Determine the arrangement of electron pairs (VSEPR model).  Specify the necessary hybrid orbitals.

26. Molecular Orbitals (MO) Analagous to atomic orbitals for atoms, MOs are the quantum mechanical solutions to the organization of valence electrons in molecules. Molecular orbitals have many of the same characteristics as atomic orbitals, such as they can hold two electrons with opposite spins and the square of the molecular orbital wave function indicates electron probability.

27. The Combination of Hydrogen 1s Atomic Orbitals to Form Molecular Orbitals

28. The Molecular Orbitals for H 2

29. Types of MOs bonding: lower in energy than the atomic orbitals from which it is composed. Electrons in this type of orbital will favor the molecule. antibonding: higher in energy than the atomic orbitals from which it is composed. Electrons in this type of orbital will favor the separated atoms.

30. Bonding and Antibonding Molecular Orbitals (MOs)

31. The Molecular Orbital Energy-Level Diagram for the H 2 Molecule

32. The Molecular Orbital Energy-Level Diagram for the H 2 - Ion

33. Bond Order (BO) Difference between the number of bonding electrons and number of antibonding electrons divided by two. Bonds order is an indication of bond strength. Large bond order means greater bond strength.

34. The Molecular Orbital Energy-Level Diagram for the He 2 Molecule

35. Bonding in Homonuclear Diatomic Molecules In order to participate in MOs, atomic orbitals must overlap in space. (Therefore, only valence orbitals of atoms contribute significantly to MOs.)

36. The Relative Sizes of the Lithium 1s and 2s Atomic Orbitals

37. The Molecular Orbital Energy-Level Diagram for the Li 2 Molecule

38. The Molecular Orbitals from p Atomic Orbitals

39. The Expected Molecular Orbital Energy-Level Diagram Resulting from the Combination of the 2p Orbitals on Two Boron Atoms

40. The Expected Molecular Orbital Energy-Level Diagram for the B 2 Molecule

41. Paramagnetism  unpaired electrons  attracted to induced magnetic field  much stronger than diamagnetism

42. Diamagnetism  paired electrons  repelled from induced magnetic field  much weaker than paramagnetism

43. Diagram of the Kind of Apparatus Used to Measure the Paramagnetism of a Sample

44. The Correct Molecular Orbital Energy-Level Diagram for the B 2 Molecule

45. Molecular Orbital Summary of Second Row Diatomics

46. Outcomes of MO Model 1.As bond order increases, bond energy increases and bond length decreases. 2.Bond order is not absolutely associated with a particular bond energy. 3.N 2 has a triple bond, and a correspondingly high bond energy. 4.O 2 is paramagnetic. This is predicted by the MO model, not by the LE model, which predicts diamagnetism.

47. Combining LE and MO Models  bonds can be described as being localized.  bonding must be treated as being delocalized.

48. The Resonance Structures for O 3 and NO 3 -

49. A Benzene Ring

50. The Sigma System for Benzene

51. The Pi System for Benzene

52. The NO 3 - Ion