Chapter 3 Orbitals and Valence Bond Theory

Chapter 3 Orbitals and Valence Bond Theory - Chapter 3...

Info iconThis preview shows pages 1–5. Sign up to view the full content.

View Full Document Right Arrow Icon
1 Chapter 3 Orbitals and Valence Bond Theory 3.2 Atomic orbitals (AO) The shapes of AOs s--sphere (positive phase sign) p x , p y , p z --two lobes (one with a positive phase sign, and another with a negative phase sign) The energy of atomic orbitals 1s < 2s < 2p x ,p y ,p z < 3s < 3p x ,p y ,p z (degenerate orbitals, C ) + + _
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
2 How to fill electrons into AOs 3 principles: i. The Aufbau principle ( . u ): Orbitals with lowest energy are filled first. ii. The Pauli exclusion principle ( . u ) A maximum of 2es can be placed into each orbital and the spins of the two es must be paired. iii. Hund’s rule ( C ): For degenerate orbitals, one e should be filled to each orbital with their spins unpaired, until each orbital has one e, then the left es can be filled to each ( )
Background image of page 2
3 e.g. C (6e) O (8e) S (16e) 2p 2s 1s 2p 2s 1s 3p 3s 2p 2s 1s
Background image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
4 3.3 Molecular orbitals The formation of molecular orbitals (MO) bonding MO : 2AOs of the same phase sign overlap with each other.
Background image of page 4
Image of page 5
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 10/16/2010 for the course CHEM 60280 taught by Professor Ryu during the Spring '09 term at TCU.

Page1 / 18

Chapter 3 Orbitals and Valence Bond Theory - Chapter 3...

This preview shows document pages 1 - 5. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online