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Chem 111- Unit 4

molecular polarity a net imbalance of charge over an entire molecule
polarity depends on bonds, shape, orientation
6 intermolecular forces (strongest -> weakest) 1) ion-dipole 2) H-bonds 3) Dipole-dipole 4) Ion-induced dipole 5) Dipole-induced dipole 6) Dispersion
Polarity and boiling point As polarity increases, so does boiling (& melting) point
particle motion assumption (2) (kinetic molecular theory) -constant, random, straight-line motion (until collision) -distribution of speeds
particle collisions assumption (3) (kinetic molecular theory) -collisions exchange kinetic energy -total kinetic energy is constant (Ek) -between collisions, molecules don't influence each other
particle volume assumption (3) (kinetic molecular theory) -large collection of molecules -particles have mass but no volume -volume of gas=volume of container
at the temperature b/w substances... Ek is constant
___mm Hg (or torr) = 1 atm 760
P is prop. to (n)(T)/(V)
Dalton's law of partial pressures in a mixture, the total pressure = sum of pressures of gases
exception to ideal gas law at high pressure, IM forces lower the pressure
Molarity Moles of solute/L solution
polarizability (pattern) the more dispersion, the more susceptible an atom is to induced polarization (larger atoms)
does NOT change during reactions (3) mass, #atoms, types of atoms,
DOES change during reactions (4) types of molecules, # of bonds, total moles, pressure
electrolyte charged particles that can move (& conduct electricity)
molecular speeds of heavier particles steep graphs
during H-bonding, NOF need ____ lone pairs!
polarizability (definition) how easily an electron cloud can be distorted
dispersion force (definition) the intermolecular force responsible for the condensed states of nonpolar substances
molecular speeds of lighter particles long graphs
Created by: melaniebeale



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