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CHM 1220 > Exam 1 > Flashcards

Exam 1 Flashcards

1
Q

commonly used prefixes in metric system

A

prefix symbol meaning power of 10
giga G 10^9
mega M 1,000,000 10^6
kilo k 1000 10^3
deci d 0.1 10^-1
centi c 0.01 10^-2
milli m 0.001 10^-3
micro μ 0.000001 10^-6
nano n 0.000000001 10^-9
pico p 10^-12

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2
Q

rules for sig figs

A

1) all nonzero integers ALWAYS count for significance ex: 3456 has 4 sig figs
2) zeros (3 classes of zeros)
a) leading zeros:NEVER count as sig figs
ex: 0.048 has 2 sig figs
b) captive zeros: ALWAYS count as sig figs ex: 16.07 has 4 sig figs
c) trailing zeros: only significant when # HAS A DECIMAL POINT
ex: 9.300 has 4 sig figs; 0.004020 has 4 sig figs; 150 has 2 sig figs

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3
Q

given: CH2O

calculate the mass percent of C, H2, and O

A 
CH2O = 30.026 (12.01 + 2(1.008) + 16.00)
C = 12.01 / 30.026 x 100 = 39.9%
H2 = 6.71%
O = 53.3%
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4
Q

Fe2O3 (s) + 3 CO (g) -> 2 Fe (s) + 3 CO2 (g)
1.00 kg Fe2O3
find g of Fe

A

699g Fe

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5
Q

2 CH3CHO (l) + O2 (g) -> 2 HC2H3O2 (l)

  • 20.0g CH3CHO
  • 10.0g O2
  • find g of HC2H3O2
  • find amnt of excess left
A
  1. 3 g HC2H3O2

2. 73 g excess left

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6
Q

which has a higher frequency, blue or red light?

A

blue

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7
Q

units of frequency

A

Hz, s^-1, 1/s

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8
Q

units of h (planck’s constant)

A

J x s

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9
Q

units of wavelength

A

m

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10
Q

given a wavelength of 671 nm. find the E of 1 photon of light

A

2.96 x 10^-19

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11
Q

wave

A

a continuously repeating change in matter or in a physical field

  • light is an electromagnetic wave
  • can be characterized by its wavelength and frequency
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12
Q

wavelength

A

λ (lambda); the distance between any 2 identical points on adjacent waves

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13
Q

frequency

A

ν (nu); the # of wavelengths that pass a fixed pt in one unit of time (s).
- unit: Hertz (Hz); 1/s; s^-1

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14
Q

wavelength and frequency are related by the __

A

wave speed (c)

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15
Q

equation of speed of light

A 
c = νλ
c = speed (m/s)
λ = wavelength (m)
ν = frequency (1/s)
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16
Q

the speed of light equation is

A

inversely proportional

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17
Q

given 742 nm. find ν

A 
c = νλ
*742 nm = 742 x 10^-9 m 
c = ν (742 x 10^-9 m ) 
(2.998 x 10^8 m/s) = ν (742 x 10^-9 m ) 
 ν = (2.998 x 10^8 m/s) / (742 x 10^-9 m ) 
 ν = 4.04 x 10^14 s
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18
Q

what is the speed of light?

A

2.998 x 10^8 m/s

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19
Q

the energy of each photon is __ to its frequency

A

proportional

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20
Q

what is the electromagnetic spectrum?

A

gamma, x-rays, far UV, near UV, visible, near infrared, far infrared, microwaves, radar, radio waves (TV, FM, AM)

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21
Q

what is the visible spectrum?

A

ROYGBV flipped

- blue has higher frequency than red

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22
Q

waves can be __

A

diffracted

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23
Q

Thomas Young

A
  • British physicist
  • showed light could be diffracted
  • by 1900s, wave theory of light was established
  • wave theory couldn’t explain the photoelectric effect
  • diagram of current
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24
Q

the photoelectric effect

A
  • shouldn’t be a current cuz there’s an open circuit but there is
  • e- attracted to (+) wire
  • Einstein figured this out
  • particle-wave duality
  • ammeter measures current
  • higher frequency = more energy
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25
Q

ammeter

A

measures current

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26
Q

Einstein proposed..

A

light consists of quanta/particles of EM energy called photons
E = hν

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27
Q

photon

A

package of light

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28
Q

what is Planck’s constant?

A

6.626 x 10^-34 J x s

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29
Q

when photon has enough E, the e- will be __ from atom

A

ejected

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30
Q

given a wavelength of 742 nm, find the E.

A

2.68 x 10^-19 J

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31
Q

given a wavelength of 486 nm, find the E

A

4.09 x 10^-19 J

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32
Q

E = hν

A 
E = energy (J)
h = planck's constant (6.626 x 10^-34 J x s)
ν = frequency (1/s)
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33
Q

light has properties of both __ and __

A

wave; matter

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34
Q

when a photon is absorbed, the e- is

A

ejected out

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35
Q

continuous spectrum

A

contains all wavelengths of light

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36
Q

line spectrum

A

shows only certain colors or specific wavelengths of light

  • heated atoms emit light
  • lines
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37
Q

atoms are

A

stable

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38
Q

energy-level postulate

A
  • an e- can have only specific energy values called energy levels
  • e levels are quantized
    E = Rh / n^2
    n= 1, 2, 3, …∞
    n = energy level/ principal quantum #
    Rh = 2.179 x 10^-18 J (Rydberg constant)
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39
Q

going from n = 1 to n = 2, energy is

A

absorbed

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40
Q

going from n = 2 to n = 1, energy is

A

released

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41
Q

energy decreases as n __

A

increases

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42
Q

when n is 0, E is

A

∞

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43
Q

transitions between energy levels

A
  • an e- can change e levels by absorbing e to move to a higher e level or by emitting e in the form of a photon to move to a lower e level
  • for a H e-, the energy lost is given by:
    ∆E = Ef - Ei
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44
Q

light is __ by an atom when the e- transition is from lower n to a higher n ( nf > ni)

A

absorbed

∆E (+)

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45
Q

light is __ by an atom when the e- transition is from higher n to a lower n ( nf ≤ ni)

A

emitted

∆E (-)

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46
Q

Louis de Broglie

A
  • French physicist
  • reasoned that particles (matter) might have wave properties similar to light particles
  • wavelength of a particle of mass (e-, p+, neutron), m (kg), and velocity, v (m/s), is given by the de Broglie rxn
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47
Q

de Broglie rxn

A 
λ = h / mv
λ = wavelength (m)
h = planck's constant (J x s)
v = velocity (m/s)
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48
Q

calculate the wavelength of light emitted when e- in an H atom goes from n = 6 to n = 3

A

1.094 x 10^-6 m

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49
Q

Erwin Schrodinger

A
  • invented quantum mechanics
  • based off Broglie’s work
  • devised theory that could be used to explain the wave properties of e- in atoms and molecules
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50
Q

quantum mechanics

A
  • mathematically describes the wave properties of submicroscopic particles
  • uncertainty principle
  • (∆x) (∆px) ≥ h / 4π
  • ∆x: uncertainty of the x coordinate of the particle
  • ∆px: uncertainty in the coordinate in the x direction
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51
Q

uncertainty principle

A

the product of the uncertainty in position and the uncertainty in momentum of a particle can be no smaller than Planck’s constant divided by 4π

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52
Q

∆x

A

uncertainty of the x coordinate of the particle

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53
Q

∆px

A

uncertainty in the coordinate in the x direction

54
Q

quantum mechanisms allows us to make..

A

statistical statements abt the regions in which we are most likely to find the e-

55
Q

4 quantum #s

A

1) principal quantum number (n): energy level
2) angular momentum quantum number (l): shape of orbital
3) magnetic quantum number (ml): orientations
4) spin quantum number (ms): observing nature
- 1-3 define wave function of e-
- 4 defines magnetic property of e-

56
Q

wave function for an e- in an atom is called an

A

atomic orbital

57
Q

finding the angular momentum quantum number (l) for s, p, d, and f orbitals

A

s: l = 0
p: l = 1
d: l = 2
f: l = 3

58
Q

angular momentum quantum number (l); L =

A

(n-1)

* can have any integer value from 0 to n-1

59
Q

the smaller the value of n, the __ the energy and sometimes the __ the orbital

A

lower; smaller

60
Q

principal quantum # can have any

A

(+) value

61
Q

orbitals w same value for n are said to be in the same __

A

shell

62
Q

magnetic quantum number (ml)

A
  • distinguishes orbitals of a given n and l
  • for l = 0, ml = 0
  • for l = 1, ml = -1, +1
  • orbitals have same shape but diff orientations in space
63
Q

spin quantum number (ms)

A
  • 2 possible orientations of the spin axis of an e-

- may have a value of either + 1/2 or - 1/2

64
Q

shape of an s orbital

A

spherical

65
Q

shape of a p orbital

A

2 lobes along straight line thru nucleus w one lobe on either side (kinda like a propeller)

66
Q

shape of a d orbital

A

has a more complicated shape than an s or a p orbital

67
Q

n

A

principal quantum number (energy level)

1,2,3,4,…

68
Q

l

A

0, 1, 2,3, …., (n-1)

69
Q

ml

A

(-L, … -1, 0, 1, …+L)

70
Q

ms

A

(+1/2, -1/2)

71
Q

n = 1

A

l = 0, 1s

72
Q

n = 2

A 
l = 0, 2s
l = 1, 2p
73
Q

n = 3

A 
l = 0, 3s
l = 1, 3p
l = 2, 3d
74
Q

s-subshell, ml =

A

0 (1 orbital)

75
Q

p-subshell, ml =

A

-1, 0, +1 (3 orbitals)

76
Q

d-subshell, ml =

A

-2, -1, 0, +1, +2 (5 orbitals)

77
Q

e- configuration tree

A 
1s
2s 2p 
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f 
6s 6p 6d 6f 
7s 7p 7d 7f
78
Q

e- configuration periodic table

A 
period 1A: 1s
period 2A: 2s 2p 
period 3A: 3s 3p
period 4A: 4s 3d 4p
period 5A: 5s 4d 5p 
period 6A: 6s 5d 6p
period 7A: 7s 6d 7p
4f 
5f
79
Q

valence e-

A

outer e- involved in bonding rxns

80
Q

valence configuration

A

just valence e-

81
Q

s & p block

A

main group elements; valence is highest n subshell only

*forget d-subshell

82
Q

d block

A

transition metals; valence is ns & (n-1) d sub shells only
*include d-subshell

83
Q

what is the valence configuration of B

A

2s2 2p1

84
Q

what is the valence configuration of Al

A

3s2 3p1

85
Q

what is the valence configuration of Ga

A

4s2 4p1

86
Q

what is the valence configuration of Zn

A

4s2 3d10

87
Q

what is the valence configuration of Mn

A

4s2 3d5

88
Q

what is the valence configuration of K

A

4s1

89
Q

what is the valence configuration of As

A

4s2 4p3

90
Q

what is the valence configuration of Te

A

5s2 5p4

91
Q

magnetic properties

A
  • paramagnetic substance: weakly attracted; unpaired e-

- diamagnetic substance: only paired e-

92
Q

is group 1A paramagnetic or diamagnetic

A

paramagnetic

93
Q

is group 2A paramagnetic or diamagnetic

A

diamagnetic

94
Q

atomic radius

A

maximum in radial distribution function of outer shell

  • down a group, atomic radius INCREASES
  • across a period, atomic radius DECREASES
  • e levels are concentric
  • across a period, effective nuclear charge increases
95
Q

effective nuclear charge

A

the (+) charge that e- experiences from nucleus

  • equal to nuclear charge
  • increases across period
  • shell # is same across period
  • size of outermost orbital and radius of atom decreases w/ increase of atomic #
  • 1A is largest
  • 8A is smallest
96
Q

put the following elements in order of increasing atomic radius: Se, Ar, S

A

Ar, S, Se

97
Q

1st Ionization Energy

A

minimum e needed to remove the highest/outermost e- from a neutral atom in the gaseous state

  • bigger = easier to take e-
  • atoms get smaller
  • down a group, ionization e DECREASES
  • across a period, ionization e INCREASES
98
Q

2nd Ionization Energy is __ than the 1st Ionization Energy

A

larger

99
Q

1/2 filled is more __ and means a __ ionization energy

A

stable; higher

100
Q

when the 3rd ionization energy is dramatically higher, it means there are __ valence e-

A

2

101
Q

electron affinity

A

e required to remove e- from atom’s (-) ion
X + e- -> X-
X- -> X + e-
- 7A is highest, 6A, 4A, 1A, 5A,… lowest: 2A and 8A

102
Q

building up principle

A

scheme used to reproduce the ground-state e- configurations by successfully filling sub shells w/e- in a specific order

  • ground-state configurations determined by the total energies of the atoms
  • ground state of atom obtained by filling orbitals of lowest e first
103
Q

pauli exclusion principle

A

no 2 e- in 1 atom can have the same 4 quantum #s

104
Q

what are the 3 physical properties of an atom?

A

1) atomic radius
2) ionization energy
3) electron affinity

105
Q

metallic character

A
  • elements w/ low ionization energies tend to be metals

- those w/ high ionization energies tend to be non-metals

106
Q

group 1A

A

ns1

107
Q

group 2A

A

ns2

108
Q

group 3A

A

ns2 np1

109
Q

group 4A

A

ns2 np2

110
Q

group 5A

A

ns2 np3

111
Q

group 6A

A

ns2 np4

112
Q

group 7A

A

ns2 np5

113
Q

group 8A

A

ns2 np6

114
Q

fixed charges

A

group 1 & 2; Al 3+, Ga 3+, Zn 2+, Cd 2+, Ag+

115
Q

why is N more stable than O?

A

because half-filled orbitals in nitrogen’s 2p orbital produce a more stable atom and a higher ionization energy
O: 2s2 2p4
N: 2s2 2p3

116
Q

ground state

A

the lowest energy state available

117
Q

excited state

A

higher energy level above ground state

118
Q

pm to m

A

1 pm = 10^-12 m

119
Q

GHz to Hz

A

x 10^9

120
Q

exceptions to the ground state

A

Mo, Cr, Cu, Au, Ag

121
Q

ground state

A

the lowest e configuration of an atom

*5 exceptions

122
Q

excited state

A

any other allowed configuration

  • out of order
  • each sub shell exists and can hold that # of e-
  • not ground state, but is allowed
123
Q

is 1s2 2s2 2p6 4s2 ground state or excited state?

A

excited bc it’s out of order but is allowed and can hold that # of e-

124
Q

not allowed (permitted)

A

sub shell doesn’t exist (2d, 1p, 1d, 3f) and/or sub shell doesn’t have that # of e- (s > 2, p > 6, d > 10)

125
Q

valence configurations

A

1) main group ns np

2) transitions ns (n-1)d

126
Q

l = 0

A

s subshell

ml = 0

127
Q

l = 1

A

p subshell

ml = -1, 0, 1

128
Q

l = 2

A

d subshell

ml = -2, -1, 0, 1, 2

129
Q

l = 3

A

f subshell

ml = -3, -2, -1, 0, 1, 2, 3

130
Q

E photon formula

A

|∆E electron|

131
Q

what is the name of group 6A

A

chalcogens

CHM 1220 (2 decks)

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