Chem Ch 5 & 6: Electron Geometry, Molecular Geometry, Formal Charge, Lone Pairs

molecular geometry of 3 electron groups

triagonal planar, bond angle 120

molecular geometry of 4 electron groups

tetrahedral, bond angle 109.5

molecular geometry of 5 electron groups

trigonal bipyramidal, bond angle 90 between axial and equatorial, 120 between equaltorial and equatorial

molecular geometry of 6 electron groups

octahedral, bond angle 90

molecular geometry of 2 electron groups

linear, bond angle 180

lone pairs of electrons

valence electrons that are not shared between atoms in a molecule, take up more space than bonding pairs

bent molecular geometry

bond angle is LESS than ideal because of LONE PAIRS

electron geometry when there is 5 electron groups

lone pairs love the equatorial position, 1 lone pair = see saw, 2 lone pairs= t shape, and 3 lone pairs=linear

electron geometry vs molecular geometry

molecular geometry only takes into account BONDING PAIRS, while electron geometry takes into account LONE AND BONDING PAIRS

electron geometry when there is 6 electron groups

1 LP= square pyramidal, 2 LP = square planar