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Spring 24 > Chemistry Final > Flashcards

Chemistry Final Flashcards

1
Q

molarity

A

mols solute/vol (L)

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2
Q

Dilution equation

A

M1V1=M2V2

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3
Q

Mass Percent

A

Mass A in Sol/total mass solution x 100%

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4
Q

Mole Fraction

A

moles A/total mols

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5
Q

molality

A

mols of solute/kg of solvent

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6
Q

Raoults Law

A

Pa=XaPoa

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7
Q

Freezing point depression

A

deltaTf=Kfxmxi

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8
Q

boiling point elevation

A

deltaTb=Kbxmxi

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9
Q

osmotic pressure

A

pie=IMRT

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10
Q

Rate law

A

k[A]^m[B]^n

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11
Q

1st order rate law

A

lnAt=-kt+lnAo, s^-1

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12
Q

2nd order rate law

A

1/At=kt+1/Ao, M^-1s^-1

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13
Q

3rd order rate law

A

M^-2s^-1

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14
Q

1st order half life

A

0.693/k=t1/2

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15
Q

2nd order half life

A

1/kxAo=t1/2

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16
Q

Arrhenius Equation

A

lnk=(-Ea/R)(1/T)+lnA

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17
Q

equilibrium

A

Rate forward=Rate reverse

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18
Q

pH

A

-log(H+)

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19
Q

pOH

A

-log(OH-)

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20
Q

H+=

A

10^-pH

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21
Q

OH-=

A

10^-pOH

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22
Q

Kw

A

KaxKb
1.0x10^-14

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23
Q

Buffer equation

A

pH=pKa+log(base/acid)

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24
Q

enthalpy equation

A

deltaH=q

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25
Q

entropy equation

A

deltaH/T

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26
Q

Gibbs Free Energy

A

deltaG=deltaH-TdeltaS
deltaG=-nFE

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27
Q

Ecell

A

E cathode- E anode

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28
Q

nernst equation

A

E-0.0592/n logQ

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29
Q

oxidized

A

loss of electrons, anode(-)

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30
Q

reduction

A

gain of electrons,cathode(+)

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31
Q

element being reduced

A

oxidizing agent

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32
Q

element being oxidized

A

reducing agent

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33
Q

in electrolysis

A

anode(+) cathode(-)

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34
Q

alpha decay

A

loss of alpha particles

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35
Q

beta decay

A

loss of bata particles

36
Q

gamma emission

A

loss of y rays

37
Q

radioactive decay is which order

A

first order
lnNt/No=-kt

38
Q

radioactive half life

A

0.693/k=t1/2

39
Q

enthalpy

A

the internal energy plus the product of pressure and volume

40
Q

+delta H

A

endothermic(heat in system)

41
Q

-delatH

A

exothermic(heat out of system)

42
Q

spontaneous process

A

process that can proceed without any ouside intervention

43
Q

entropy

A

measure of randomness or disorder of a system

44
Q

entropy increases when

A

gases formed from liquids/ soilds
liquids or solutions are formed from solids
# of gas mol increases
# moles increases
solid is dissolved into solvent

45
Q

when delta S is positive

A

delta G is negative

46
Q

if delta G is negative

A

spontaneous reaction

47
Q

if delta G is positive

A

nonsponatneous reaction

48
Q

buffers

A

weak acid and it conjugate base, resistant to ph changes

49
Q

ksp

A

solubility product constant, the higher the ksp the greater the solubility of compound

50
Q

arrhenius acid

A

increased concentration of H+ ions

51
Q

arrhenius base

A

increased concentration of OH- ions

52
Q

bronsted lowry acid

A

proton donor

53
Q

bronsted lowry base

A

proton acceptor

54
Q

acid goes to

A

conjgate base removing H+

55
Q

base goes to

A

conjugate acid adding H+

56
Q

strong acids

A

HI,HBr,HCl,H2SO4,HNO3,HClO3,HClO4

57
Q

strong bases

A

alkali metals, alkaline earth metals, group 1/2

58
Q

the greater the Ka value

A

the stronger the acid

59
Q

the greater the Kb value

A

the stronger the base

60
Q

lewis acid

A

electron pair acceptor

61
Q

lewis base

A

electron pair donor

62
Q

if k>1

A

reaction is product favored

63
Q

if k<1

A

reaction is reactant favored

64
Q

Q>k

A

too much products, shifts left

65
Q

q<k

A

too much reactants, shifts right

66
Q

if concentration of reactants is increased

A

shifts left to right

67
Q

if concentration of reactants is decreased

A

shifts right to left

68
Q

if concentration of products is decreased

A

shifts left to right

69
Q

if concentration of product is increased

A

shifts right to left

70
Q

increase pressure, decrease volume

A

favor fewer moles

71
Q

decrease pressure, increase volume

A

favor more moles

72
Q

increase temp

A

favor endothermic reaction

73
Q

decrease temp

A

favor exothermic reaction

74
Q

factors affecting reaction rates

A

physical state of reactants, concentration of reactants, temp, presence of a catalyst

75
Q

activation energy

A

minimum amount of energy required for reaction

76
Q

catalysts

A

increase rate of reaction by decreasing activation energy

77
Q

colligative properties

A

depend on # of solute particles
vapor pressure lowering
boiling point elevation
melting point depression
osmotic pressure

78
Q

micelles

A

water hydroprobic ends cluster together with hydrophilic ends pointing outwards

79
Q

cubic

A

8 corners, 1/8

80
Q

body

A

1/4 8 corners, 1 center

81
Q

face

A

1/2 8 corner, 6 faces

82
Q

intermolecular forces

A

van der waal forces
dipole dipole
HB
london dispersion
ion dipole

83
Q

london dispersion

A

present in all molecules, larger surface area, strength increases with molecular weight

84
Q

dipole dipole

A

center atom is surrounded by same atom, the more polar the strong the dipole interaction, more CH bonds= lower dipole movement

85
Q

HB

A

strongest, H bonded to N,O,F

Spring 24 (6 decks)

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