CHEM 110 Lecture Notes - Molecular Geometry, Orbital Hybridisation, Atomic Orbital

• School: McGill University
• Department: Chemistry
• Course: CHEM 110
• Professor: Ariel Fenster

Document Summary

Atom must go from ground state to excited state by absorbing energy and promoting an electron. The number of hybrid orbitals equals the total number of atomic orbitals that are combined. Hybridization occurs only when the bonds are being formed. Energy and the number of orbitals is conserved. Hybridization: process of replacing pure atomic orbitals with reformulated atomic orbitals for bonded atoms. Octahedral: draw lewis dot diagram, fill in s and p orbitals, promote electron into the p orbital. 2basicvalencebondtheoryvalence bond theoryapplication:can be used to explain thebondingof moleculesbasicvalencebondtheoryvalence bond theorylimitation:doesn"t describe thegeometryof moleculesatomic orbital hybridizationgeometry bonding(vsepr)(v. b. Theory)sp hybridizationexample: becl2lewis structureclbeclgeometry (vsepr)1800linear molecule1802basicvalencebondtheoryvalence bond theoryapplication:can be used to explain thebondingof moleculesbasicvalencebondtheoryvalence bond theorylimitation:doesn"t describe thegeometryof moleculesatomic orbital hybridizationgeometry bonding(vsepr)(v. b. Theory)sp hybridizationexample: becl2lewis structureclbeclgeometry (vsepr)1800linear molecule1805clbeclclbeclbe3s3pclsp2p3s3pclbe3s3pclsp2p3s3pclcl be clsp (2)cl be clsp (2)pcl be clpsp (2)p: 3 hybridization. Results in a two sp with p overlaps. Results in a four hybrid sp3 atomic orbital.