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Chem & Physics > Week 2 > Flashcards

Week 2 Flashcards

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1
Q

Solid—> gas

A

Sublimation

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2
Q

Gas—> solid

A

Deposition

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3
Q

Solid—> liquid

A

Melting

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4
Q

Liquid—> solid

A

Freezing

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5
Q

Liquid —> gas

A

Evaporation

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6
Q

Gas—> liquid

A

Condensation

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7
Q

EN

A

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

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8
Q

Intermolecular forces in order strong-weakest

A

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)

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9
Q

Solvent

A

Thing doing dissolving

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10
Q

Solute

A

What is being dissolved

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11
Q

Ampphipathic

A

Attraction to both polar and non polar

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12
Q

Bent shape

A

AX2E

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13
Q

Trigonal planar

A

AX3

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14
Q

Tetrahedral

A

AX4

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15
Q

Linear

A

AX2

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16
Q

PYRAMIDAL

A

AX3E

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17
Q

Vapor pressure

A

Pressure of vapor in contact with the matters liquid

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18
Q

Relative humidity =

A

Pp H2O/vapor pressure h2o

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19
Q

Heat of vaporization

A

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

20
Q

Heat of fusion

A

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

21
Q

Q-

A

Exothermic- feels hot

22
Q

Q+

A

Endothermic- feels cold

23
Q

Higher intermolecule force does what to vapor pressure?

A

Decreases

24
Q

Boiling point

A

Vapor pressure equal to pressure it is exposed to

25
Q

Which one is greater, heat of fusion of vaporization?

A

Heat of vaporization

26
Q

Specific heat

A

Amt energy necessary to heat 1g 1degree C

27
Q

Which concentration is not temp dependent?

A

Molality

28
Q

Osmolarity is

A

Sum of all molarities. 1 M Nacl is 2 osm

29
Q

Increased pressure does what to solubility

A

Increases

30
Q

Increased temperature does what to solubility liquid solid and gas?

A

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

31
Q

Colligative properties

A

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

32
Q

Raoult’s law

A

Vapor pressure of solute depends on concentration

33
Q

Boyle’s law

A

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

34
Q

Charle’s law

A

Volume/temp. Directly, volume up, temp up

35
Q

Gay-Lussac’s law

A

Pressure/temperature, temp up, pressure up direct.

36
Q

Avogadro’s law

A

Volume/mole. Direct. Mole up, volume up

37
Q

Dalton’s Law

A

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

38
Q

Xi

A

Mole freaction mi/mtotal

39
Q

Dew point

A

Point at which air cannot hold any more water

40
Q

Assumptions of kinetic molecular theory of gas

A

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

41
Q

Boltzmann’s constant

A

R/avogradro’s number.

42
Q

KE of particle

A

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

43
Q

Graham’s law of effusion

A

Smaller particles move faster and heating them up moves them faster

44
Q

Real gas rules

A

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

45
Q

Van der Waals

A

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

Chem & Physics (4 decks)

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