Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry 1 > Lectures 1-8 > Flashcards

Lectures 1-8 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

gases at room temperature

A

HEFONC & noble gases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

1 L

A

1 dm^3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

1 Pa

A

1 N/m^2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

1 bar

A

1 x 10^5 Pa

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

1 kPa

A

1000 Pa

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

equal volumes of gas at constant T and p contain

A

equal number of particles

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

volumes of all gases extrapolate to zero at

A

0 K

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

R

A

8.314 J K^-1 mol^-1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

V is proportional to

A

1/p

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

V is proportional to

A

T

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

V is proportional to

A

n

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

density

A

pM/RT

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

to find partial pressure

A

n(a) x (RT/V)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

to find total pressure

A

(n(a) + n(b) + n(c)) x (RT/V)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

to find mole fraction

A

n(a)/n(total)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

to find mole fraction

A

p(a)/p(total)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

to find partial pressure

A

x(a)/p(total)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

kinetic molecular theory assumptions

A

negligible particle size, elastic collisions, no interaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

average kinetic energy of particles

A

3/2kT where k is R/N(A)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

RMS speeds related to

A

temperature and molar mass

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

all gases at same temperature have same

A

kinetic energy, but not same average speed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

effusion

A

gas escapes through a hole

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

diffusion

A

different gases mix

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

diffusion occurs from regions of

A

high to low concentration

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

rate of effusion is inversely proportional to

A

square root of molar mass

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

rate of effusion

A

number of molecules passing through a hole per second

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

particles attract each other

A

p decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

particles repel each other

A

p increases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

wavelength

A

distance from maximum to maximum

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

frequency

A

how many cycles a second

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

wavelength and frequency are

A

anti-proportional

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

wave number

A

inverse of wavelength; number of wavelengths per unit distance

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

light intensity is related to

A

amplitude

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

light colour is related to

A

wavelength

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

constructive interference

A

when two waves in phase interfere

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

destructive interference

A

when two waves out of phase interfere (amplitude = 0)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

wavelength and energy content are

A

anti-proportional

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

same temperature

A

same kinetic energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

to calculate RMS, molar mass must be in

A

kg/mol

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

RMS

A

(3RT/M)^1/2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

rate of effusion of gas 1/rate of effusion of gas 2

A

SQUARE ROOT OF: molar mass gas 2/molar mass gas 1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

p1V1/T1 =

A

p2V2/T2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
43
Q

frequency =

A

c/wavelength

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
44
Q

photons

A

energy packets of light

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
45
Q

energy of a single photon (E)

A

hv

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
46
Q

absorption spectroscopy

A

input light, analyse what was absorbed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
47
Q

in absorption spectroscopy, the sample transitions from a

A

lower to higher energy state

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
48
Q

emission spectroscopy

A

input heat, analyse what was emitted

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
49
Q

in emission spectroscopy, sample transitions from

A

higher to lower energy state

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
50
Q

deltaE

A

E2-E1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
51
Q

predicting positions of lines in emission spectra

A

RH(1/n^2final - 1/n^2initial)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
52
Q

energy of emitted light

A

-hv or -hRydberg equation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
53
Q

quantum numbers

A

n(initial) and n(final)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
54
Q

emission quantum numbers

A

n(final) < n(initial) and deltaE is negative

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
55
Q

absorption quantum numbers

A

n(final) > n(initial) and deltaE is positive

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
56
Q

the Bohr model does not work because

A

emission spectra of many-electron atoms cannot be described, does not explain intensity of spectral lines, does not take into account particles as waves

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
57
Q

photoelectric effect

A

electromagnetic radiation hits a metal surface and electrons are emitted

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
58
Q

electrons are only ejected if light reaches

A

critical/threshold frequency

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
59
Q

intensity increase causes

A

higher number of electrons to be ejected

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
60
Q

photons must overcome both

A

binding energy and threshold frequency

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
61
Q

kinetic energy of electron

A

hv(photon) - Ebind

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
62
Q

kinetic energy of electron

A

hv(photon) - h x threshold frequency

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
63
Q

Hz

A

1/s

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
64
Q

de Broglie wavelength of matter

A

wavelength = h/p = h/mv

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
65
Q

wavelength and mass are

A

anti-proportional

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
66
Q

fast-moving particles have

A

shorter wavelengths

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
67
Q

slow-moving particles have

A

longer wavelengths

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
68
Q

Heisenberg’s Uncertainty Principle

A

it is not possible to accurately detect the exact position of a particle and its momentum at the same time

69
Q

Heisenberg’s Uncertainty Principle

A

deltaxdeltap >/ h/4pi

70
Q

wavefunction

A

used to describe the standing wave for an electron

71
Q

for each energy state of an electron/particle, we assign a different

A

wavefunction

72
Q

regions with positive and negative signs for each wavefunction

A

phases (there is a negative phase and a positive phase)

73
Q

regions where wavefunction is zero

A

nodes

74
Q

wavefunction^2

A

related to probability of finding a particle at a particular point in space

75
Q

when wavefunctions are squared, nodes are

A

unchanged

76
Q

point with maximum probability of finding a particle

A

maximum of wavefunction^2

77
Q

point where probability of finding particle is zero

A

node

78
Q

electron density

A

calculated through wavefunction^2, gives us probability of finding an electron in area around nucleus

79
Q

orbital

A

a one-electron wavefunction in three-dimensional space

80
Q

energy levels are always

A

negative

81
Q

orbitals with the same energy are called

A

energetically degenerate

82
Q

angular momentum quantum number; l

A

determines type & shape of orbital; tells us subshell/letter

83
Q

limit for angular momentum quantum number (l)

A

n-1

84
Q

magnetic momentum quantum number; ml

A

determines orientation of orbital; allows us to distinguish between each individual p, d orbital

85
Q

limit to magnetic momentum quantum number (ml)

A

-l and l

86
Q

principle quantum number; n

A

determines energy for that shell

87
Q

s orbitals are

A

spherical

88
Q

p orbitals are

A

dumbbell-shaped

89
Q

two lobes of p orbitals have different

A

signs

90
Q

two lobes of p orbitals separated by

A

angular node/nodal plane (zero)

91
Q

keep radius fixed and

A

plot angles to explore shape

92
Q

keep angles fixed and

A

play around with radius (can be graphed)

93
Q

higher n,

A

higher number of nodes (for example, 1s orbital has no nodes, 2s orbital has one node, 3s orbital has two nodes)

94
Q

the first time an orbital appears there are

A

no nodes

95
Q

shell volume increases with

A

radius

96
Q

wavefunction and probability decrease with

A

r

97
Q

for larger shells, you’re more likely to find an electron

A

further away from the nucleus

98
Q

to find wavelength when given mass

A

wavelength = h/mv

99
Q

in many electron atoms, orbital degeneracy

A

disappears

100
Q

electron spin is

A

quantised; two different angular momenta

101
Q

spin magnetic quantum number ms for spin up/clockwise

A

+1/2

102
Q

spin magnetic quantum number ms for spin down/anti-clockwise

A

-1/2

103
Q

in an atom, no two electrons can have the same

A

four quantum numbers

104
Q

the same orbital can only hold two electrons if they have

A

opposite spins

105
Q

orbitals cannot hold more than

A

two electrons

106
Q

fill up lower-lying orbitals

A

first

107
Q

only fill next orbital once orbital below is

A

occupied

108
Q

principal quantum number determines

A

row

109
Q

superscripted number

A

number of electrons in that orbital

110
Q

two degenerate orbitals want to be

A

singly occupied first

111
Q

number of p orbitals in a shell

A

3 (6 electrons)

112
Q

number of d orbitals in a shell

A

5 (10 electrons)

113
Q

same group, same

A

electronic configuration in outer shell

114
Q

core electrons

A

electrons in shells that are energetically lower than outer shell

115
Q

nucleus has

A

positive charge Z

116
Q

shielding is a

A

consequence of electron repulsion, which reduces net interaction between the positive nucleus and valence electrons

117
Q

valence electrons do not experience full Z, only

A

effective charge Zeff

118
Q

why do p orbitals have higher energies than s orbitals for many-electron atoms?

A

shielding

119
Q

because 3d orbitals are shielded by 3s and 3p orbitals, they are

A

less stable and have higher energies than 4s orbitals

120
Q

3d is filled after

A

4s

121
Q

4d is filled after

A

5s

122
Q

4f is filled after

A

6s

123
Q

5d is filled after

A

4f

124
Q

number of f orbitals in shell

A

7; 14 electrons

125
Q

first transition metals

A

3d metals (fourth period)

126
Q

4d transition metals appear after

A

5s orbital has been filled (fifth period)

127
Q

chromium electronic configuration

A

[Ar]4s^13d^5

128
Q

additional stabilisation in chromium is due to

A

half-filled 3d subshell with all 5 electrons having parallel spin

129
Q

copper electronic configuration

A

[Ar]4s^13d^10

130
Q

stabilisation in copper due to

A

fully-filled 3d subshell

131
Q

after lanthanum, we fill

A

4f orbitals before remaining 5d orbitals

132
Q

after actinium, we fill

A

5f orbitals before remaining 5d orbitals

133
Q

after actinium, we fill

A

5f orbitals before remaining 5d orbitals

134
Q

ionisation energy for a single H atom

A

13.6 eV

135
Q

covalent radius

A

atomic radius estimated by halving distance between two chemically bound nuclei of the same type

136
Q

size increases

A

down a group

137
Q

as we go down a group,

A

principal quantum number (n) increases

138
Q

size decreases

A

across a period

139
Q

across a period, electrons from outer shell are drawn closer to nucleus due to

A

increasing positive charge

140
Q

across a period, electron-electron repulsion

A

increases as we increase the number of electrons

141
Q

cations are always

A

smaller than the parent atom

142
Q

anions are always

A

larger than the parent atom

143
Q

isoelectric

A

two species that contain the same number of electrons

144
Q

for an isoelectric series, size decreases as

A

number of protons increases/nuclear charge increases

145
Q

ionisation energy (IE)

A

energy required to remove the highest energy (most loosely held) electron from an atom/ion

146
Q

removing an electron is

A

endothermic

147
Q

first ionisation energy < second < third because

A

consecutively removed electrons cause a reduction in electron-electron repulsion and experience a greater attraction to Z

148
Q

IE decreases

A

down a group

149
Q

IE increases

A

across a period

150
Q

across a period, nuclear charge

A

increases but the number of core electrons remains the same

151
Q

high ionisation energy

A

small size

152
Q

low ionisation energy

A

large size

153
Q

electron affinity (EA)

A

the energy change associated with the addition of an electron to a gaseous atom

154
Q

electron affinity is

A

exothermic, generally

155
Q

the closer the vacant orbital is to the nucleus, the more favourable the addition of an electron and the

A

more negative EA; more energy released

156
Q

EA decreases/is less negative

A

down a group

157
Q

EA increases/is more negative

A

across a period

158
Q

EA is not always exothermic due to

A

electron-electron repulsion

159
Q

electronegativity

A

the ability of an atom to attract shared electrons to itself

160
Q

electronegativity numerically

A

IE + EA

161
Q

electronegativity increases

A

across a period

162
Q

electronegativity decreases

A

down a group

163
Q

metallic character increases

A

down a group

164
Q

metallic character decreases

A

across a period

165
Q

metals have relatively low

A

IEs

166
Q

total number of orbitals in a shell

A

n^2

167
Q

substance that has one or more unpaired electrons

A

paramagnetic

168
Q

substance that has no unpaired electrons

A

diamagnetic

169
Q

substance that has unpaired electrons that are aligned in a particular direction

A

ferromagnetic

Chemistry 1 (4 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions