Intermolecular Forces

-H atom is covalently bonded to a small, highly electronegative element: -F, O, or N -Strongest IMFs because it has the most polar bonds

attraction between + and -end of neighboring molecules IMF’s=dipole-dipole attraction greater electronegativity diffrence than the stronger attraction

• polarization causes dipole to form then chain reaction All molecules are LDF but more significant in larger molecules with lots of e- and larger NP molecules are only LDF

Intramolecular force, within a molecule, - or Bonds Stronger forces than Inter

Intermolcular force, between molecules, |||| or IMFs Weaker than Intra

Temporary random shift of e- could towards any inside of a molecule

the measure the resistance of a liquid to flow

inward pull of particle, the energy required to increase the surface area of a liquid by a given amount Stronger surface tension, stronger IMFs

amount of heat required to raise temp: 1 gram, 1 degree C

the flow of energy

average kinetic energy (moment)

energy in a system

change in enthalpy

units of energy

feels cool absorbs energy/to break bonds + H energy in products

feels hot releases energy/to form bonds -H energy in reactants

molecules settle out in a solution Phase transition: gas into solid

Phase transition: solid into a gas

only temp/pressure that 3 states of matter can be in equilibrum

liquid and gas phases of a substance are identical

overall enthalpy change in a reaction is equal to the sum of the enthalpy changes for the individual steps