Chem 2 Exam 1

Solid

High Pressure Low Temp

Gas

High Temp Low pressure

triple point

in between all 3 phases

critical point

between liquid and gas

high intermolecular forces = __ vapor pressure

Low

High Temp = ___vapor pressure

high

T2

Boiling Point

Within a phase

q = nCT

between phases

q=nH

London Dispersion

weakest, e temp distributed unevenly

Dipole-Diople

depends on size and electronegativity, polar

Ion-Dipole

attractive forces between ion and dipole

ex: ionic compound dissolves in a polar solvent

H bonding

strongest, N O F

Metallic Solids

positive cores of atoms held together metallic bonding

covalent network

atoms held together in large chains by covalent bonding

molality

moles solute/kg solvent l

molarity

moles solute/L solution

wt%

mass of solute/mass total x 100

Henry’s Law

at constant temp amount of gas that dissolves in a liquid is directly proportional to partial pressure of gas, Does work for gases at high pressure, at equilibrium

Vapor Pressure Lowering

VP solvent lower than VP pure solvent

Raoults Law:

change P= Xsolute x Psolvent

Freezing Point Depression

freezing Points of solutions are lower than pure solvent

change in Tf= Kf x m

Osmotic pressure

difference needed to stop flow of solvent across semipermeable membrane

TT= MRT

Boiling Point Elevation

boiling points higher than that of pure solvent

0 order rate

K[A]^0=1

1st order rate

K[A]

2nd order rate

K[A]²