solubility rules + vsepr + polarity + acids/bases

solubility rule 1 + exceptions

most nitrate (NO3^-) salts are solubles

no exceptions

solubility rule 2 + exceptions

most Na+, K+, NH4^+ salts are soluble

no exceptions

solubility rule 3 + exceptions

most chloride (Cl-) salts are soluble

exceptions - AgCl, PbCl2, Hg2Cl2

linear (EG)

2 electron groups, 180

EG

trigonal planar (EG)

3 electron groups, 120

EG

tetrahedral (EG)

4 electron groups, 109.5

EG

trigonal bipyramidal (EG)

5 electron groups, 90, 120

EG

octahedral (EG)

6 electron groups, 90

EG

when is a molecule nonpolar?

• symmetrical shape

• AND all bonds identical OR bond dipoles cancel

when is a molecule polar?

• asymmetrical shape OR different surrounding atoms → dipole doesn’t cancel

nonpolar bond def

equal sharing of electrons; EN difference < ~0.4

polar bond def

unequal sharing; EN difference > ~0.4

how to decide overall polarity?

1. draw lewis

2. determine shape

3. identify bond dipoles

4. check if they cancel

lone pairs effect on polarity

lone pairs usually create asymmetry → molecule becomes polar

C—H bonds polarity

considered nonpolar for molecular geometry

strong acids

• start with H

  • HCl - hydrochloric acid

  • HBr - hydrobromic acid

  • HI - hydroiodic acid

  • HNO3 - nitric acid

  • HClO3 - chloric acid

  • HClO4 - perchloric acid

  • H2SO4 - sulfuric acid

weak acids examples

• HF

• CH3COOH

• H2CO3

• H3PO4

• most organic acids

strong bases list

• group 1 hydroxides (group 1 w/ OH)

• group 2 heavy hydroxides (group 2 w/ OH2)

weak bases examples

• NH3

• amines (smth w/ C—H)

• N-containing bases

arrhenius acid + base

acid - produces H+ in water

base - produces OH- in water

bronsted-lowry acid + base

acid - proton donor

base - proton acceptor