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finals Flashcards

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1
Q

gases tend to have ___

A

low molecular weight

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2
Q

pressure is the same no matter the ____

A

element

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3
Q

1 atm = ___ mm Hg = ___ torr = ___ Pa = ___psi

A

760 mm Hg, 760 torr, 1.01325 x 10^5 Pa, 14.70 Psi

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4
Q

manometer measure the pressure of _____

A

gas

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5
Q

open ended manometer = ___ , closed ended =___

A

compare to 1 atm (760 mm Hg), compare to 0 mm Hg

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6
Q

boyles law

A

volume is inversely proportional to pressure V= 1/p

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7
Q

boyles law math

A

P1V1=P2V2

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8
Q

Charles law

A

temp is proportional to volume

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9
Q

Charles law math

A

V1/T1 = V2/T2

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10
Q

Combined gas law

A

(P1V1)/T1 = (P2T2)/T2

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11
Q

Gay-Lussac’s law

A

temp goes down, pressure goes down

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12
Q

Gay-Lussac’s math

A

P1/T1 = P2/T1

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13
Q

avogandros law

A

volume is proportional to moles at STP

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14
Q

ideal gas law

A

Volume is proportional to (moles*temp)/pressure

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15
Q

ideal gas law math

A

PV=nRT

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16
Q

R in ideal gas law

A

0.08206 (Latm)/(molK)

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17
Q

density version of PV=nRT

A

m/V=MP/RT (M=molarity)

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18
Q

Daltons law of partial pressures

A

IT DOESNT MATTER THE WEIGHT PRESSURE WILL ALWAYS BE THE SAME FOR EACH PARTICLE Ptotal = P1 + p2 + p3 + p4 +……

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19
Q

mole fraction for gases

A

P1/Pt = (N1RT/V)/(ntRT/V) = N1/Nt

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20
Q

mole fraction

A

mole of particular gas/total moles of all gas

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21
Q

pressure ratio = _______

A

= mole ratio

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22
Q

kinetic molecular theory (5)

A
  1. gases are in continuous motion
  2. The volume of the molecules is negligible relative to the total volume in which the gas is contained (FALSE)
  3. there are no attractive and repulsive forces (FALSE)
  4. energy can be transferred between molecules during collisions, but average energy does not change.
  5. the average kinetic energy is proportional to the absolute temperature
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23
Q

average kinetic energy equation

A

KE=1/2mv^2

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24
Q

lighter gases move ____ and have greater _____ of speed and heavier move ____ and haver less ____ of speed

A

faster, distribution, slower, distribution

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25
Q

learn about most probable speed, root speed and the other one

A

on it

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26
Q

u(rms) equation (average kinetic energy of gas)

A

square root of 3RT/M

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27
Q

R in average kinetic energy of gas

A

= 8.314 J/molK = (kgm^2/S^2)/mole*K

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28
Q

effusion

A

escape of gas molecules through a tiny hole into an evactauted space (leaky air tank)

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29
Q

diffusion

A

gas spreads throughout a space (like febreeze)

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30
Q

mean free path

A

average distance a gas travels before a collision (pressure increases, distance decreases)

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31
Q

rate of effusion is related to ____

A

collision rate

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32
Q

Grahams law

A

R1/R2= square root of Mass2/Mass1 (compares the rate that gases effuse)

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33
Q

deviations from ideal gas happens when _____ and ____

A

theres high and low pressure

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34
Q

at low temp, you move ____ and have to deal with _____ forces

A

slower, attractive

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35
Q

van der Waal’s equation for real gases

A

(P + (n^2a)/V^2)*(V - nb) = nRT

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36
Q

Kinetic molecular theory (KMT) breaks down at ____

A

high and low pressures

37
Q

large a in van der Waals=

A

strong intermolecular forces

38
Q

large b in van der waals =

A

larger particle size

39
Q

b term breaks down _____ in KMT

A

the second postulate (gas got no volume)

40
Q

a term breaks down ____ in KMT

A

the third postulate (intermolular forces dont exist nerd)

41
Q

what determines matter’s state?

A

KE (avg) vs Intermolecular forces (IMFs)

42
Q

liquid has equal ___ and ____

A

KE and intermolecular forces (almost equal)

43
Q

gas has more _____ than ____

A

KE than IMFS

44
Q

solid has more _____ than ____

A

IMFs than KE

45
Q

vander waals paremeters

A

b = size a =attraction

46
Q

intramolecular forces vs intermolecular forces

A

intra = in the same molecule inter = inbetween many molecules

47
Q

intermolecular forces we care about (4)

A
  1. dispersion forces (london dispersion force)
  2. dipole-dipole interactions
  3. hydrogen bonding
  4. ion-dipole interactions
48
Q

(london) dispersion force (LDFs)

A

(surface area) instantaneous dipoles lead to attractions between atoms because one electrical imbalance leads to another. MORE surface area MORE LDFs

49
Q

Dipole-dipole interactions

A

all molecules have to be polar, positives line up with negatives and higher numbers leads to higher boiling point (bp).

50
Q

hydrogen bonding

A

when hydrogen bonds to N, O, or F, and another N, O, or F bonds to the hydrogen (with a lone pair) since the hydrogen has so much unequal positive charge due to the unequal electronegativity. STRONGEST IMF you gonna get

51
Q

hydrogen bond is ~ _______ of a covalent bond

A

5-15%

52
Q

in order to h bond, _____

A

must have a N,O,F bonded directly to a H

53
Q

as molar mass goes up, _____

A

imf goes up due to LDFs (ignoring hydrogen bonding anomaly)

54
Q

to hydrogen bond, you need a ____

A

lone pair

55
Q

tendency for the electron cloud to distort

A

polarizability

56
Q

factors of polarizability

A
  1. number of electrons
  2. size of atoms
  3. shape of molecules
57
Q

molar mass leads to ____ which leads to ___ which leads to _____ thus ______

A

more electrons, more LDFs, more IMFs, higher boiling point

58
Q

weaking to strongest forces

A

LDFs, Dipole-dipole, hydrogen bonding

59
Q

Ion-dipole interactions

A

basically hydrogen bonding but with ions. requires high polar solvent.

60
Q

low lattice energy leads to _____

A

easier ion-dipole dissolving

61
Q

every molecule expierences ______

A

LDFs (dispersion forces)

62
Q

viscosity =

A

the resistance to flow

63
Q

higher IMF = ______ in fluids

A

Higher viscosity

64
Q

surface tension

A

guys near the surface of water are more densely packed than guys at the bottom due to IMFs pulling the surface downward.

65
Q

Cohesion

A

IMF’s that bond a material to itself (water to water)

66
Q

adhesion

A

IMF’s that bond a material to other materials (water to a towel)

67
Q

capillary action

A

basically using stronger IMF’s to move liquids like water. can be done in reverse like in mercury

68
Q

why do we have a menescus in water?

A

because waters adhesive force to glass is stronger than its cohesive force to itself

69
Q

vapor pressure

A

the pressure vapor exerts at equilibrium

70
Q

boiling point

A

temperature at which the vapor pressure becomes more powerful than the surrounding pressure.

71
Q

in order to escape the liquid phase, you need to overcome _____

A

IMFs

72
Q

normal boiling point

A

the boiling point at 1 atm for a liquid

73
Q

lower vapor pressure for chemicals with _____

A

higher IMFs

74
Q

volatile

A

evaporate easily

75
Q

critical point

A

the point where you go past the normal graph and become supercritical

75
Q

triple point

A

where you are all three phases at once

76
Q

supercritical fluids

A

behaves kinda like a fluid and a gas at the same time

77
Q

memorize and draw phase diagram in slides

A

oki

78
Q

crystalline

A

highly ordered

79
Q

amorphous

A

lack of order

80
Q

metallic solids

A

held together by a “sea” of electrons, not brittle (metals)

81
Q

Ionic Solids

A

salts, cations and anions bonded together, brittle DO NOT CONDUCT ELECTRICITY AS A SOLID

82
Q

covalent-network solids

A

diamond, SUPER strong,

83
Q

molecular solids

A

held together with IMFs, not very strong, WEAKEST

84
Q

memorize the solids slide

A

oki doki

85
Q

polymers

A

long chains of covalent bonds

86
Q

nanomaterials

A

crystalline compounds the sizer of 1-100 nm

87
Q
A

Gen chem (6 decks)

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