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Polar Covalent Bonds
Electrons shared unevenly between 2 bonded atoms. atoms with higher electronegativity pulls electrons closer. A polar molecule needs polar bonds and asymmetry
Dipole
slightly negative charge side of polar molecules
Van der Waals Forces
Dispersion: caused by motion of electrons, more electrons = greater force Dipole interactions: polar molecules attract positive to negative end
Hydrogen Bonding
attractive forces between hydrogen bonded to 1 atom to very electronegative atom’s lone pairs in another molecule, only with O, N, F
Mole to Volume
1 mol = 22.4 L at STP
Molarity
moles/L
Molality
moles/kg
Dilutions
M1V1 = M2V2
Colligative properties
T = kM. for boiling, add to original. for freezing, subtract from the original.
