CHM136H1 Lecture Notes - Lecture 3: Orbital Hybridisation, Sigma Bond, Pi Bond

• School: UTSG
• Department: Chemistry
• Course: CHM136H1
• Professor: Clive Scott Browning, Kristine Quinlan

Document Summary

Sp3 hybrid orbitals : structure of ethane. Two c atoms bond by head-on overlap of sp3 orbital. Remaining 3 sp3 orbitals overlap with h1s orbitals. 2s orbital combined with two 2p orbitals. Head on bond = sigma, side to side = pi, sigma is stronger than pi bonds. Electrons in sigma bond are centered between nuclei. Electrons in pi bond are located away from nuclei. C=c double bond (shorter and stronger than single bond) H 1s form sigma bond with four sp2 orbitals sp hybrid orbitals. 2s orbital combined with a p orbital giving two sp hybrids. An sp hybrid orbital from each of two c atoms overlap head-on to form an sp-sp sigma bond. Pz orbitals from each c form a pz-pz pi bond. Sharing of six electrons forms c=c triple bond (very short and strong) H 1s orbitals form sigma bonds with two c sp orbitals. In methylamine, n"s orbitals combine to form four sp3 orbitals.