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CHEM 180 > Exam 2 > Flashcards

Exam 2 Flashcards

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1
Q

Strong electrolytes

A

A substance that is essentially completely ionized in aqueous solution

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2
Q

Weak electrolyte

A

Only partially ionized in aqueous solution

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3
Q

Non-electrolyte

A

Do not provide ions in water

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4
Q

Precipitate

A

Insoluble ionic solid

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5
Q

Solubility Rules: Soluble

A

Salts of group 1 cations and the NH4+ cation, nitrates, acetates, perchlorates, chlorides, bromides, iodides, and sulfates (except those of calcium, strontium, and barium)

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6
Q

Solubility Rules: Insoluble

A

Salts of silver, lead, and mercury (I), carbonates, phosphates, sulfides, oxides, hydroxides

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7
Q

Predominant Species: Sodium carbonates

A

Na+ and CO3 2-

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8
Q

Predominant Species: cesium bromates

A

Cs+ and BrO3-

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9
Q

Predominant Species: calcium hydroxides

A

Ca2+ and OH-

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10
Q

Predominant Species: cobalt (II) nitrate

A

Co2+ and NO3-

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11
Q

Predominant Species: zinc sulfates

A

Zn2+ and SO4 2-

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12
Q

Predominant Species: lithium hydroxide

A

Li+ and OH-

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13
Q

Predominant Species: hydrochloric acid

A

H3O+ and Cl-

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14
Q

Predominant Species: hydrobromic acid

A

H3O+ and Br-

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15
Q

Predominant Species: hydroiodic acid

A

H3O+ and I-

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16
Q

Predominant Species: nitric acid

A

H3O+ and NO3-

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17
Q

Predominant Species: sulfuric acid (<17M)

A

H3O+ and HSO4-

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18
Q

Predominant Species: perchloric acid

A

H3O+ and ClO4-

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19
Q

Predominant Species: ammonium chloride

A

NH4+ and Cl-

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20
Q

Predominant Species: ammonium sulfate

A

NH4+ and SO4 2-

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21
Q

Predominant Species: ammonium bromide

A

NH4+ and Br-

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22
Q

Predominant Species: ammonium nitrate

A

NH4+ and NO3-

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23
Q

Predominant Species: methylammonium chloride

A

CH3NH3+ and Cl-

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24
Q

Predominant Species: dimethylammonium sulfate

A

(CH3)2NH+ and SO4 2-

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25
Q

Predominant Species: HgCl2

A

HgCl2 and water

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26
Q

Predominant Species: SnCl2

A

SnCl2 and water

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27
Q
A
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28
Q

Nitric acid

A

HNO3

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29
Q

Phosphoric acid

A

H3PO4

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30
Q

Perchloric acid

A

HClO4

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31
Q

Nitratoauric acid

A

Au(NO3) 3

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32
Q

Bisulfide

A

HS-

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33
Q

Chromate

A

CrO4 2-

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34
Q

Dichromate

A

Cr2O7 2-

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35
Q

Gas property: expansion

A

Increase in volume of gas due to increase in temperature or decrease in pressure

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36
Q

Pressure

A

Force/Area

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37
Q

Ideal gas equation

A

PV = nRT

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38
Q

Root-mean-square velocity

A

V(rms) = square root of (3RT/mm)

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39
Q

Combined gas law

A

P1V1/n1T1 = P2V2/n2T2

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40
Q

Isobaric

A

constant pressure

41
Q

Gas property: compression

A

Increase of gas pressure because of lowering of volume

42
Q

Gas property: diffusion

A

How the molecules disperse in a closed container

43
Q

Gas property: effusion

A

how fast they escape through a pinhole

44
Q
A
45
Q

M

A

mRT/PV = dRT/P

46
Q

A balloon won’t rise when

A

Its density is greater than air

47
Q

A barometer

A

Measures atmospheric pressure

48
Q

Manometer

A

Measures the pressure of a sample of gas relative to atmospheric pressure

49
Q

Ideal gas

A

Assumed to have no forces of attraction or repulsion between gas particles and have no volume for the gas particles without taking into account fluctuating temperatures and pressures

50
Q

Real gases

A

Take into account fluctuating temps and pressures

51
Q

d

A

MP/RT

52
Q

Boyle’s law

A

As pressure decreases, volume increases, P1V1 = P2V2

53
Q

Charles’ law

A

V1/T1 = V2/T2

54
Q

Dalton’s law of partial pressures

A

In a mixture of two or more gases, the total pressure is the sum of the partial pressures of all the components

55
Q

Volume of gas in liquid displacement

A

Is equal to volume of liquid

56
Q

Conditions for assuming ideal gas behavior

A

Negligible volume, no intermolecular forces, perfect elastic collisions, low pressure, low temperature

57
Q

Kinetic energy

A

ME = 1/2 mv^2

58
Q

System

A

Is what’s being studied

59
Q

Surroundings

A

Everything outside of what’s being studied

60
Q

Heat

A

Due to a temperature difference

61
Q

Work

A

Movement of an object over a distance or gas expansion

62
Q

Specific heat

A

S, the amount of heat energy required to increase the temperature of 1 gram of a substance by 1 °C

63
Q

Heat capacity

A

C, is for any specified amount of mass that requires an amount of heat to raise the temperature by 1°C

64
Q

Open system

A

Has external interactions, which can tak the form of information, energy, or material transfers

65
Q

Closed system

A

Matter goes in, doesn’t go out, freely exchanges energy

66
Q

Isolated system

A

Doesn’t exchange either energy or matter

67
Q

Heat calculation for temp changes of matter

A

q = ms🔺T

68
Q

Endothermic

A

Heat is absorbed by system from surroundings

69
Q

Exothermic

A

Heat is released by the system to the surroundings

70
Q

Constant volume process

A

q(rxn) = qv = 🔺U, where the heat of reaction is the change in internal energy (ie. Bomb calorimeter)

71
Q

Constant pressure process

A

q(rxn) = qp = 🔺H, where the heat of reaction is change in enthalpy (ie. Coffee cup calorimeter)

72
Q

Oxidizer

A

Gains electrons

73
Q

Reduction

A

Loses electrons

74
Q

1 J

A

1 kg m2/s2

75
Q

🔺E

A

q + w

76
Q

Electromagnetic spectrum from lowest to highest energy

A

Radio, microwave, infrared, visible, ultraviolet, x-ray, gamma ray

77
Q

Causes electronic excitation

A

Visible

78
Q

Causes rotational excitation

A

Microwave

79
Q

Is absorbed by ozone

A

Ultraviolet

80
Q

Is “heat” radiation

A

Infrared

81
Q

Photoelectric effect

A

Light strikes metal, electrons are ejected. More light intensity, more ejected electrons. Classical theory couldn’t explain why. Albert Einstein in 1905 proposed the light particle concept and said that a single photon striking the metal surface will eject a single electron as long as the photon energy is greater than the work function (binding energy of the electron)

82
Q

Atomic line spectra

A

When atoms absorb energy, they emit light made up of a discrete number of wavelengths. Neils Bohr in 1913

83
Q

Energy

A

hv/e^hv/kt - 1

84
Q

Black body radiation

A

8pi kTv^2/c^3

85
Q

Max planck

A

In 1901 suggested that energy cna not be continuous, rather it comtes in packets called quanta

86
Q

Work function

A

E = KE + o

87
Q

E

A

hc/wave

88
Q

If the speed is negative

A

No ejection of electrons

89
Q

1 J

A

1 kg m^2/s^2

90
Q

Particle in a box

A

Matter waves seem particle like when not confined, but wave like when confined

91
Q

wave length

A

= h/P

92
Q

P

A

mv

93
Q

Permitted energies of particle in box, E

A

n^2h^2/8 mL^2

94
Q

Approximate radius of atom

A

10^-11 m

95
Q

DE for decay of electron

A

-Rh (1/nf2 - 1/ni2)

96
Q

l

A

Can not be larger than n-1, when n = 1, l is 0 and cna only be 1 subshell, when n = 2, l is 0, 1 cuz of two possible subshell

97
Q

l

A

S = 0, p = 1, d = 2, f = 3

98
Q

Ml

A

S = 0, p = - 1, 0, +1, etc

99
Q

Ms

A

When all shells are filled, it’s - 1/2, +1/2

CHEM 180 (7 decks)

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