Gen Chem - Bonding/Chemical interactions

Coordinate covalent bonding

If both of the shared e- are contributed by only one of the 2 atoms

Bond length and Bond strength

single: longest, weakest

double: medium, medium

triple: shortest, strongest

Formal Charge

Difference between # of electrons normally found in that atom’s valence shell and the # of electrons assigned to an atom in a Lewis structure.

Formal Charge equation

V - N(nonbonding) - ½ N(bonding)
or valence electrons - dots - sticks

Electronic vs molecular geometry

electronic describes spatial arrangement of all pairs of e-

molecular describes spatial arrangement of only the bonding pairs of electrons

London Dispersion Forces (type of van Der Waals force)

attractive or repulsive interactions of these short-lived and rapidly shifting dipoles. this is due to the unequal distribution of electron density. temporary interactions.

Dipole-dipole interaction

polar molecules tend to orient themselves sot hat positive region is close to negative region. a favorable electrostatic force is formed. present in solid and liquid phases but not in gas phase

Hydrogen bonding

this is an unusually strong dipole-dipole interaction, not an actual bond. H-bonds exist in Fluorine, Oxygen, Nitrogen (FON). Substances with hydrogen bonding typically have unusually high boiling points.