CHEM101 Lecture Notes - Lecture 17: Covalent Bond, Orbital Hybridisation, Valence Electron

• School: University of Alberta
• Department: Chemistry
• Course: CHEM101
• Professor: Rylan Lundgren

Document Summary

Summary of the last few lectures (post midterm 1: lewis structures (sec 10. 1 in the text, 10. 1-10. 22 quesions) Resonance structures: vespr (sec 10. 2 in the text, 10. 27-10. 58 quesions) Number of groups/points in space (parent structure) Molecular shape: based on # of bonding groups. Valence bond theory: we know electrons are in orbitals, deined by quantum mechanics. Valence electrons can be shared between atoms to form covalent bonds : the valence bond theory explains molecular shapes/bonding based on the interacion of atomic orbitals, basic principal: Covalent bonds form when orbitals of two atoms overlap. In phase addiion results in a bonding interacion. Out of phase addiion results in an ani bonding interacion: key points. Electrons pair in orbitals will opposing spins (ms or ). There is a max of 2 e- in an orbital. The degree of orbital overlap between atoms determines the bond strength. Orbitals sharing electrons leads to bonding, increased overlap = increased bond strength.