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CHEM 180 > Exam 2 > Flashcards

Exam 2 Flashcards

(99 cards)

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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
Predominant Species: HgCl2
HgCl2 and water
26
Predominant Species: SnCl2
SnCl2 and water
27
28
Nitric acid
HNO3
29
Phosphoric acid
H3PO4
30
Perchloric acid
HClO4
31
Nitratoauric acid
Au(NO3) 3
32
Bisulfide
HS-
33
Chromate
CrO4 2-
34
Dichromate
Cr2O7 2-
35
Gas property: expansion
Increase in volume of gas due to increase in temperature or decrease in pressure
36
Pressure
Force/Area
37
Ideal gas equation
PV = nRT
38
Root-mean-square velocity
V(rms) = square root of (3RT/mm)
39
Combined gas law
P1V1/n1T1 = P2V2/n2T2
40
Isobaric
constant pressure
41
Gas property: compression
Increase of gas pressure because of lowering of volume
42
Gas property: diffusion
How the molecules disperse in a closed container
43
Gas property: effusion
how fast they escape through a pinhole
44
45
M
mRT/PV = dRT/P
46
A balloon won't rise when
Its density is greater than air
47
A barometer
Measures atmospheric pressure
48
Manometer
Measures the pressure of a sample of gas relative to atmospheric pressure
49
Ideal gas
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
Real gases
Take into account fluctuating temps and pressures
51
d
MP/RT
52
Boyle's law
As pressure decreases, volume increases, P1V1 = P2V2
53
Charles' law
V1/T1 = V2/T2
54
Dalton's law of partial pressures
In a mixture of two or more gases, the total pressure is the sum of the partial pressures of all the components
55
Volume of gas in liquid displacement
Is equal to volume of liquid
56
Conditions for assuming ideal gas behavior
Negligible volume, no intermolecular forces, perfect elastic collisions, low pressure, low temperature
57
Kinetic energy
ME = 1/2 mv^2
58
System
Is what's being studied
59
Surroundings
Everything outside of what's being studied
60
Heat
Due to a temperature difference
61
Work
Movement of an object over a distance or gas expansion
62
Specific heat
S, the amount of heat energy required to increase the temperature of 1 gram of a substance by 1 °C
63
Heat capacity
C, is for any specified amount of mass that requires an amount of heat to raise the temperature by 1°C
64
Open system
Has external interactions, which can tak the form of information, energy, or material transfers
65
Closed system
Matter goes in, doesn't go out, freely exchanges energy
66
Isolated system
Doesn't exchange either energy or matter
67
Heat calculation for temp changes of matter
q = ms🔺T
68
Endothermic
Heat is absorbed by system from surroundings
69
Exothermic
Heat is released by the system to the surroundings
70
Constant volume process
q(rxn) = qv = 🔺U, where the heat of reaction is the change in internal energy (ie. Bomb calorimeter)
71
Constant pressure process
q(rxn) = qp = 🔺H, where the heat of reaction is change in enthalpy (ie. Coffee cup calorimeter)
72
Oxidizer
Gains electrons
73
Reduction
Loses electrons
74
1 J
1 kg m2/s2
75
🔺E
q + w
76
Electromagnetic spectrum from lowest to highest energy
Radio, microwave, infrared, visible, ultraviolet, x-ray, gamma ray
77
Causes electronic excitation
Visible
78
Causes rotational excitation
Microwave
79
Is absorbed by ozone
Ultraviolet
80
Is "heat" radiation
Infrared
81
Photoelectric effect
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
Atomic line spectra
When atoms absorb energy, they emit light made up of a discrete number of wavelengths. Neils Bohr in 1913
83
Energy
hv/e^hv/kt - 1
84
Black body radiation
8pi kTv^2/c^3
85
Max planck
In 1901 suggested that energy cna not be continuous, rather it comtes in packets called quanta
86
Work function
E = KE + o
87
E
hc/wave
88
If the speed is negative
No ejection of electrons
89
1 J
1 kg m^2/s^2
90
Particle in a box
Matter waves seem particle like when not confined, but wave like when confined
91
wave length
= h/P
92
P
mv
93
Permitted energies of particle in box, E
n^2h^2/8 mL^2
94
Approximate radius of atom
10^-11 m
95
DE for decay of electron
-Rh (1/nf2 - 1/ni2)
96
l
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
l
S = 0, p = 1, d = 2, f = 3
98
Ml
S = 0, p = - 1, 0, +1, etc
99
Ms
When all shells are filled, it's - 1/2, +1/2

CHEM 180 (7 decks)

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