Week 2

Question 1

Solid—> gas

Answer 1

Sublimation

Question 2

Gas—> solid

Answer 2

Deposition

Question 3

Solid—> liquid

Answer 3

Melting

Question 4

Liquid—> solid

Answer 4

Freezing

Question 5

Liquid —> gas

Answer 5

Evaporation

Question 6

Gas—> liquid

Answer 6

Condensation

Question 7

EN

Answer 7

Atoms with higher electro negativity will get shared electrons more; the result is a polar covalent bond. Partial - on high EN and partial + on lower en

Question 8

Intermolecular forces in order strong-weakest

Answer 8

1) Force between permanent dipole and ion
2) force between permanent dipole (hydrogen bonding is much stronger)
3) force b/w permanent dipole and induced dipole
4) London force (force between induced dipole)

Question 9

Solvent

Answer 9

Thing doing dissolving

Question 10

Solute

Answer 10

What is being dissolved

Question 11

Ampphipathic

Answer 11

Attraction to both polar and non polar

Question 12

Bent shape

Answer 12

AX2E

Question 13

Trigonal planar

Answer 13

AX3

Question 14

Tetrahedral

Answer 14

AX4

Question 15

Linear

Answer 15

AX2

Question 16

PYRAMIDAL

Answer 16

AX3E

Question 17

Vapor pressure

Answer 17

Pressure of vapor in contact with the matters liquid

Question 18

Relative humidity =

Answer 18

Pp H2O/vapor pressure h2o

Question 19

Heat of vaporization

Answer 19

Energy necessary to overcome all intermolecular forces so that molecules can escape into gas phase. Heat needed to boil

Question 20

Heat of fusion

Answer 20

Necessary energy to convert 1 mole of solid into liquid at normal melting point. Heat needed to melt

Question 21

Q-

Answer 21

Exothermic- feels hot

Question 22

Q+

Answer 22

Endothermic- feels cold

Question 23

Higher intermolecule force does what to vapor pressure?

Answer 23

Decreases

Question 24

Boiling point

Answer 24

Vapor pressure equal to pressure it is exposed to

Question 25

Which one is greater, heat of fusion of vaporization?

Answer 25

Heat of vaporization

Question 26

Specific heat

Answer 26

Amt energy necessary to heat 1g 1degree C

Question 27

Which concentration is not temp dependent?

Answer 27

Molality

Question 28

Osmolarity is

Answer 28

Sum of all molarities. 1 M Nacl is 2 osm

Question 29

Increased pressure does what to solubility

Answer 29

Increases

Question 30

Increased temperature does what to solubility liquid solid and gas?

Answer 30

Temp increases solubility of liquid and solid but decreases in solubility of gases

Question 31

Colligative properties

Answer 31

1) Vapor pressure decreases with increasing solute concentration 2) boiling point increases with increasing solute concentration 3) freezing point decreases with increasing solute concentration 4) osmotic pressure increases with increasing solute concentration

Question 32

Raoult’s law

Answer 32

Vapor pressure of solute depends on concentration

Question 33

Boyle’s law

Answer 33

PV with temp constant. Indirect. Press something, it gets smaller

Question 34

Charle’s law

Answer 34

Volume/temp. Directly, volume up, temp up

Question 35

Gay-Lussac’s law

Answer 35

Pressure/temperature, temp up, pressure up direct.

Question 36

Avogadro’s law

Answer 36

Volume/mole. Direct. Mole up, volume up

Question 37

Dalton’s Law

Answer 37

Sum of all pressures of each gas is the total pressure of the system.

Question 38

Xi

Answer 38

Mole freaction mi/mtotal

Question 39

Dew point

Answer 39

Point at which air cannot hold any more water

Question 40

Assumptions of kinetic molecular theory of gas

Answer 40

1) gas molecules are small compared to volume of gas, so we can ignore the size of the molecule 2) gas molecules are in constant, random motion 3) gas molecules show range of kinetic energies, but average kinetic energy depends on temp 4) gas molecules are not attracted or repulsed from each other, so all collisions are elastic

Question 41

Boltzmann’s constant

Answer 41

R/avogradro’s number.

Question 42

KE of particle

Answer 42

1/2 mv2= 3/2 RT. M=molecular weight

Question 43

Graham’s law of effusion

Answer 43

Smaller particles move faster and heating them up moves them faster

Question 44

Real gas rules

Answer 44

Cannot completely ignore size of particles, especially at high pressures. At very low temperature, particles also begin to be more attracted to eachother

Question 45

Van der Waals

Answer 45

Used when high pressure or low temp. Takes into account attraction.