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CHM 142 +145 > CHM 142 Exam 1 > Flashcards

CHM 142 Exam 1 Flashcards

1
Q

weakest of the intermolecular forces, present in all molecules

A

london-dispersion forces

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2
Q

the attraction of the - and + charges of ions

A

dipole-dipole interactions

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3
Q

when H is bonded to O N or F

A

hydrogen bonding

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4
Q

attraction between an ion and a polar molecule, strongest of the forces

A

ion-dipole interaction

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5
Q

when a dissolved solutes particles re-attatch in a solution to form a solid

A

crystallization

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6
Q

a solution that has the amount of solute added that is measured by solubility

any more solute added will not dissolve

A

saturated

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7
Q

the amount of solute needed to saturate a solution

max amt of solute that can be added

A

solubility

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8
Q

the—the attraction between a solute and solvent the — the solubility of the solute in that solvent

A

stronger, greater

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9
Q

does hydrogen bonding increase or decrease solubility?

A

Increases solubility

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10
Q

liquids that mix in all proportions no matter the amount

A

miscible

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11
Q

liquids that do not and can not mix

A

immiscible

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12
Q

is the solublity of liquids and solids affected by pressure?

A

no, but gases are

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13
Q

the solubility of a gas is — to its partial pressure

A

proportional

will increase if P increases, will decrease if P decreases

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14
Q

solublity of a gas in a solvent=

A

K Pg

K= constant
P= partial pressure of gas

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15
Q

how does temperature affect the solubility of gases?

A

as temperature increases the solublity of the gas decreases

gas escapes through bubbles when soln boils

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16
Q

mass percentage =

A

mass of solute/ total mass of soln * 100

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17
Q

ppm=

A

mass of solute/total mass of soln * 10^6

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18
Q

ppb=

A

mass of solute/total mass of soln *10^9

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19
Q

molality

A

moles of solute/ mass (Kg) of solvent

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20
Q

molarity

A

moles of solute/ volume (L) of soln

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21
Q

what do you need to convert to molarity if you’re using ppms or ppb

A

density

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22
Q

is molality affected by increasing temp?

A

no, increasing temp does not change moles

it does affect molarity (V)

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23
Q

properties that depend on the quantity (aka concentration) of molecules and not the identity of the molecule

vapor pressure, boiling point, freezing point, osmotic pressure

A

Colligative properties

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24
Q

the pressre exerted by a gas over a liquid while in equilibrium

A

vapor pressure

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25
Q

how do you calculate partial pressure?

A

total pressure * the mole fraction of the the moleucle

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26
Q

when a solute is added to a pure solvent what happens to the vapor pressure?

A

the vapor pressure is lowered

less molecules can escape as gas so VP is lower

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27
Q

vapor pressure of a soln=

A

pressure of solvent * mole fraction of solvent

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28
Q

moles of component/ total moles

A

mole fraction

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29
Q

is the boiling point of a solution lower or higher than that of a pure solvent?

A

it is (typically) higher than that of a pure solvent because the vapor pressure is lower so it takes a higher temp to boil the solution

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30
Q

change in BP of a soln=

A

iKbm or boiling point of soln. - boiling point of the solvent

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31
Q

the number of ions a molecule dissociates into when placed in a solvent

A

van hoff factor

it is 1 for nonelectrolytes

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32
Q

is the freezing point of a solution higher or lower than the FP of a pure solvent?

A

it is lower than the pure solvent

think about icing roads and what the ice does to the water on the road

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33
Q

Osmotic Pressure

equation

A

IMRT

i(n/v)RT

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34
Q

Osmotic Pressure

defenition

A

the pressure needed to stop osmosis

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35
Q

the movement of solvent molecules from a solution of low concentration (high solvent) to high concentration (low solvent)

A

osmosis

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36
Q

what happens if two solutions are isotonic?

aka osmotic pressure is equal

A

No osmosis occurs

37
Q

what does it mean if a solution is hypertonic?

A

high osmotic pressure

38
Q

what does it mean if a solution is hypotonic?

A

low osmotic pressure

39
Q

dispersion of a soltue where the particles do not evenly/completely dissolve

intermediate kind of dispersion

A

colloids

40
Q

what allows colloids to be able to scatter light while solutions cannot?

A

the tyndall effect (and their larger molecules)

41
Q

all of the reactants exist in the same state of matter

A

Homogenous reactions

42
Q

the reactants exist in different states of matter

A

heterogenous reactions

43
Q

do heterogenous or homogenous reactions proceed at faster rates?

A

homogenous reactions

44
Q

how does concentration affect reaction rates?

A

the higher the concentration of reactants the quicker the reaction proceeds

more opportunities for mlecules to collide

45
Q

-change in concentration/ change in time

reactants

A

rate of dissappearnace

46
Q

rate of appearance

product

A

change in concentration/ change in time

47
Q

the rate of of a particlar instant/ point in time of a reaction

A

instantanous rate

48
Q

t=0

A

initial rate

49
Q

how do you calculate the instant rate when the products and reactants dont have a 1:1 ratio?

A

-1/a({A}/change in time)=1/b({B}/change in time)

50
Q

General Rate law

A

rate =k{A}^x*{B}^y

51
Q

the exponents x and y (or m and n) in the rate law equation that determine how the rate is affected by the reactants

A

reaction order

52
Q

when the rate depends on a single reactant to the 1st power

A

first order reaction

53
Q

rate=k{A}

A

rate law for first order reactions

54
Q

ln{A}=-kt+ln{A}0

A

Integrated rate law for first order reactions

55
Q

when the rate depends on one reactant to the second power or two reactants to the first order

A

second order reactions

56
Q

=K{A}^2

A

rate law for second order reactions

57
Q

integrated rate law for second order reactions

A

1/{A}=kt+1/{A}0

58
Q

when the rate of disappearance of a reactant is independent of concentration

A

Zeroth order reactions

59
Q

rate =k

A

rate law for zeroth order reactions

60
Q

=kt+{A}0

A

integrated rate law for zeroth reactions

61
Q

half-life for first order reactions

A

-ln(1/2)/k

62
Q

half-life for second order reactions

A

1/k{A}0

63
Q

rate laws relate — and —

A

rate and concentration

64
Q

integrated rate laws relate— and —

A

time and concentration

65
Q

molecules in a reaction must be aligned in the correct way to create a reaction/ form and break bonds

A

orientation factor

66
Q

the minimum energy required to complete a chemical reaction

A

activation energy

67
Q

the arrangment of molecules at the ‘peak’ of the Ea

not an intermediate

A

activation complex/transition state

68
Q

the — the value of activation energy the — the rate constant

A

lower, greater

or greater and lower

69
Q

fraction of molecules with the energy to reach the activation energy

A

f= e^(-Ea/RT)

70
Q

Arrhenius Equation

A

k=Ae^(-Ea/RT)

71
Q

equation for determining the activation energy when you have 1 rate constant

A

Ln(k)=-Ea/RT+ ln(A)

72
Q

eqaution for determing the activation energy when you have 2 rate constants

A

ln(k1/k2)=-Ea/R(1/T2-1/T1)

73
Q

reactions that occur in a single step/event

A

elementary reactions

74
Q

A—products

one step, one molecule

A

unimolecular

75
Q

A+B—products

or A+A—products

A

bimolecular

76
Q

true or false, the steps of a chemical reaction always add up/cancel out to a new reaction equation?

A

false, they will always result in the original equation

77
Q

not an initial reactant or intial product in the reaction, it is only seen in the reaction steps

and is used up in the steps

A

Intermediate

78
Q

for a mechansism with a slow first step
rate law=

A

the rate of the slow first step

79
Q

a substance that is not affected/ used in a reaction that also increases the reaction rate

lowers activation E or changes orientation of molecules

A

catalyst

80
Q

when catalysts are in the same phase as the reactants

A

homogenous catalysis

81
Q

when the catalysts are in different phases than the reactants

A

heterogenous catalysis

82
Q

when molecules attatch to the bind to a surface

they do not permeate the inside

A

Adsorbtion

83
Q

biological molecules that use the Lock-in Key model and are very specific about what they choose to react with

A

Enzymes

84
Q

when reactants and product concentration is no longer changing but forward and reverse reactions are continuing to happen

A

equilibrium state

85
Q

Kc/Keq=

A

The concentration of products/ concentration of reactants to their coefficients

86
Q

How to calculate Kc/Keq for gases

A

Kp= Kc(RT)^change in moles

you can also use the pressures like you would use concentrations

87
Q

if Kc/Kp»1 what does this indicate?

A

that the reaction favors the products

lies to the right, numerator is larger

88
Q

If Kc/Kp«1 what does this indicate?

A

that the reaction favors the reactants

lies to the left, large denominator

CHM 142 +145 (6 decks)

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