Chemistry 2 Test 2

• Ion-dipole
• Dipole-dipole
• London dispersion
• Hydrogen bonding

Exist between an ion and the partial charge on the end of a polar molecule.

Attractions occur when the partial positive end of one polar molecule is near the partial negative end of another polar molecule. Between neutral, polar molecules.

A type of dipole dipole attraction. Are very strong and can only occur between an electropositive H and O, N, or F.

Exist among all molecules, caused by electrons shifting and briefly making a dipole dipole connection.

• Dispersion→dipole-dipole→hydrogen bonding→
• ion-dipole

sublimation

deposition

Volatile. The larger the intermolecular forces in the liquid, the lower its vapor pressure and the less volatile it will be.

1 atm

The temperature at which solid and liquid coexist at 1 atm

The temperature and pressure at which three phases of a substance coexist.

Point beyond which liquid and gaseous phases cannot be distinguished.

• The solubility of a gas in any solvent increases as the pressure over the solvent increases.
• S_g = kP_g

(Mass of solute A / mass of solution) x 100

(mass of solute A / mass of solution) x 10⁶

(mass of solute A / mass of solution) x 10⁹

X_a= mol of A / total mol

M = mol solute / volume of solution (L)

m = mol solute / mass of solvent (kg)

• Properties of solutions that depend soley on the number of particles of solute and NOT of their chemical identity.
• Vapor pressure
• Boiling point
• freezing point
• osmotic pressure

One that has no measurable vapor pressure

P_{solvent over solution} = X_solventP°_solvent

P°_solvent = vapor pressure of the pure solvent at the solution temperature

X_solvent= mol_solvent / mol_solvent + mol_{solute particles}

• ΔT_b = K_bm
• ΔT_b = T_bp(solution) - T_bp(pure solvent) 

ΔT_b is never negative

ΔT_f = K_fm

• ΔT_f = Tfp(pure solvent) - T_fp(solution)

ΔT_f is never negative!

• ℵ = MRT
• M= molarity of solute particles
• R= gas constant
• T= temperature in K

One that has an excessively high salt concentration and can cause blood cells to shrink

One that has a low concentration of salt and can cause blood cells to expand and burst

Al³⁺

Br^-

BrO^-

BrO₃^-

C₂H₃O₂^-

CO₃^2-

HCO₃^-

ClO-

ClO₂^-

ClO₃^-

ClO₄^-

CrO₄^2-

Cr₂O₇^2-

IO₃^-

IO₄^-

MnO₄^-

N^3-

NO₂^-

NO₃^-

P^3-

PO₃^3-

PO₄^3-

HPO₄^2-

H₂PO₄^-

SO₃^2-

SO₄^2-

HSO₄^-

• 1: Ionic + H₂O soluble
• Any ionic compound containing alkali metal ion
• vvvvvvvvvvvvvvvvv containing NH₄⁺
• vvvvvvvvvvvvvvvvv containing NO₃^-
• vvvvvvvvvvvvvvvvv containing C₂H₃O₂^-
• 8 strong bases

2: Covalent compound 7 strong acids

• Solute: minor
• Solvent: major