Chem II

Hydroxide

OH-

Sulfate

SO4 2-

Nitrate

NO3-

Phosphate

PO4 3-

Sulfite

So3 2-

Acetate

CH3CO2-

Nitrite

NO2-

Thiosulfate

S2O3-

Ammonium

NH4+

Ammonia

NH3

Carbonate

CO3 2-

Perchlorate

ClO4-

Chlorate

ClO3-

Chlorite

ClO2-

Hypochlorite

ClO-

VESPR

valence shell electron repulsion theory

2e-

linear

3e-

trigonal planar

4e-

tetrahedral

5e-

trigonal bipyramidal

Ion dipole

Important to solutions of ions (Ion must be present and salt needs to be soluble in water)

dipole-dipole force

-When molecules are close to each other

-must be polar

Hydrogen bonding

when H is covalently bonded to N, O, F

London Dispersion

occur in all molecules (depending on the size can be stronger than hydrogen bonding)

Heat of fusion (delta Hfus)

energy required to change a solid, at melting point, to liquid

Heat of vaporization (delta Hvap)

energy required to change liquid, at boiling point, to gas

Sublimation

Solid to gas

Deposition

gas to solid

Melt

solid to liquid

Freeze

liquid to solid

Condensation

gas to liquid

vaporization

liquid to gas

Vapor Pressure

ln(P vap) = - (delta Hvap/R) + (1/T) +C

Solvation

The acting of dissolving solutes in solution

Dissolution

physical change that occurs when solute dissolves in solvent

Saturated Solution

holds as much solute as possible at that temperature; dynamic equilibrium

Unsaturated solution

holds less solute than possible at that temperature

Supersaturated solution

solvent holds more solute than is normally possible at that temp

Miscible

dissolves completely into each other

Immiscible

when two things will not dissolve into each other; i.e oil and water

Factors that Affect Solubility

1. Structure of molecule

2. Pressure

3. temperature

Molarity

moles of solute/L of solution

Mass percentage

(mass of A in solution/total mass of solution)

Molality

moles of solute/ kg of solvent

Mole fraction

moles of A/ total number of moles in solution

Colligative Properties

1. vapor pressure lowering

2. boiling point elevation

3. melting point depression

4. osmotic pressure

Raoult’s Law

Pa= Xa (mole fraction) Pnot a

Boiling Point Elevation

delta Tb = i * Kb * molality

Freezing point depression

delta Tf = i *Kf * molality

Osmotic Pressure

pie = (n/v) RT = MRT

Colloids

A suspension of particles larger than individual ions or molecules, but too small to be settled out by gravity; i.e fog, smoke, whipped cream, milk, or marshmallow

Tyndall Effect

colloidal suspensions can scatter rays of light