CHEM CH8 - Solids, Liquids & Gasses

Intramolecular bonds

Bonds within the molecules ex: ionic and covalent bonding

Intermolecular Forces of Attraction

Between the molecules (dipole-dipole, hydrogen, and dispersion / london forces of attraction)

types of bond from strongest to weakest

ionic

covalent

dipole-dipole

hydrogen

london FOA

dipole-dipole forces of attraction

when oppositely charged poles of different molecules are attracted to each other

hydrogen bond

exists between the positively charged H+ atom of one molecules & a highly electronegative atom such as O, N, or F atom of another (two molecules needed)

dispersion or london FOA

weakest bond; attraction occurs between the positive charges nucleus of one atom and the negative electrons of another atom of a another molecule

types of solids

crystals (smooth edges / columns)

amorphous solid (does not have sharp edges) ex: glass or plastic

chunky solids (ex: zinc)

powder solids (ex: zinc)

granulated solids (ex: granulated sugar)

wire (ex: Cu, Fe wire)

sheets (ex: Cu, Fe sheets)

Liquids triple point characteristic

at 0°C, H2O can exist as a solid, liquid of gas

gas

• has the largest amount of energy compared to S and L

• moves around randomly, in different direction via gentle collision w/ each other and the container around it

  • creates gaseous pressure

Boyles Law

at constant temperature, volume is inversely proportionate to pressure

P1V1 = P2V2

1 atm = 760 mmHg = 14.7 psi

1 atm = 760 mmHg = 14.7 psi

Charle’s Law

at constant pressure the volume of a gas is directly proportional to its absolute temperature (K)

V1/T1 = V2/T2

Gay - Lussac’s Law

at constant volume, the pressure of a gas is directly proportional to its absolute temperature (K).

P1/T1 = P2/T2

Combined Gas Law

It relates the pressure, volume, and temperature of a gas, combining Charles's and Gay-Lussac's laws.

The formula is P1V1/T1 = P2V2/T2.

Avogadro’s Law

at constant temperature and pressure, the volume of a gas is directly proportional to the number of moles of gas.

V1/n1 = V2/n2

Ideal Gas Law

describes the relationship between pressure, volume, temperature, and number of moles of a gas, combining all the gas laws into one equation.

Pv = nrt (HAS TO BE CONVERTED TO L, ATM, K AND MOLE)

Daltons Gas Law of Partial Pressure

states that the total pressure of a gas mixture is equal to the sum of the partial pressures of each individual gas in the mixture.

Daltons Gas Law of Partial Pressure (scenario 1)

add total pressures up

Daltons Gas Law of Partial Pressure (scenario 2)

add moles, then divide by total and mult. by ptotal given

Daltons Gas Law of Partial Pressure (scenario 3)

1. find the molar mass for the compounds

2. add together

3. divide grams/total mm

4. mult by ptotal