CHEM 14C Lecture Notes - Lecture 2: Octet Rule, Electron Density, Lewis Structure
23 Mar 2020
School
Department
Course
Professor
Document Summary
Periodic table of electronegatives in bonding, en a ect electron distribution atoms with higher en steal electron density from partners in a bond electron distribution can be even covalent bonding uneven polar covalent or ionic bonding. Electroneagtivity di ernces lead to molecualr dipoles consequences of polar covalent bonds electrostatic interactions in uences chemical properties, physical properties, biologial properties polar bonds hydrogen bonding dna bonding. Covalent bonds are formed by overlap of orbitals. Atomic orbitals: mathematical equation describe where an electron is likely to be found. Atomic orbitals combine to form molecular orbitals sigma bond = single pi bond = double// overlap so. Test - which are sigma/pi bonds dont have to draw them but identify. Hare spa a overlapping of orbitals along the internuclear axis gives a sigma bond ( ) Fee oppn. to fp overlapping or orbitals perpendicular to internuclear axis gives a pi bond ( ) Shortcut to hybridization atoms attached not bonds t y.
