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Chemistry 1 > Chapter 8 The Quantum Mechanical Model of the Atom > Flashcards

Chapter 8 The Quantum Mechanical Model of the Atom Flashcards

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1
Q

Until the beginning of the twentieth century it was
believed that all physical phenomena were what?

A

deterministic

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2
Q

Final state could be determined from the initial state

A

deterministic

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3
Q

the present condition does not determine the future condition

A

indeterministic

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4
Q

describes the behavior of subatomic
particles.

A

Quantum mechanics

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5
Q

key point of quantum mechanics

A

Explaining the periodic table
– The behavior of the elements in chemical
bonding
– Provides the practical basis for lasers,
computers, and countless other applications

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6
Q

are incredibly small particles.

A

electrons

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7
Q

what determines the properties of atoms.

A

Electron behavior

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8
Q

a form of electromagnetic radiation

A

Light

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9
Q

Composed of perpendicular oscillating waves, one for the
electric field and one for the magnetic field

A

Light

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10
Q

is a region where an electrically
charged particle experiences a force.

A

electric field

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11
Q

is a region where a magnetized
particle experiences a force.

A

magnetic field

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12
Q

is the height of the wave.

A

amplitude

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13
Q

The distance from node to crest or node to trough (or valley)

A

amplitude

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14
Q

The amplitude is a measure of what?

A

light intensity

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15
Q

is a measure of the distance covered by the wave.

A

wavelength

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16
Q

The distance from one crest to the next

A

wavelength

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17
Q

what determines the color of light

A

the wavelength

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18
Q

is the number of waves that
pass a point in a given period of time.

A

frequency

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19
Q

how do you find out how long a cycle is?

A

number of waves

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20
Q

what is the units of frequency?

A

hertz

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21
Q

is proportional to the amplitude of
the waves and the frequency.

A

total energy

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22
Q

the larger the what the more force/energy in the wave

A

amplitude
or
frequently the waves strike a particular point

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23
Q

The color of light is determined by its

A

wavelength (or frequency).

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24
Q

is composed of light of
several wavelengths:

A

white light

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25
Q

All the wavelengths of light comprise the

A

electromagnetic spectrum

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26
Q

have the lowest energy

A

Radio waves

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27
Q

have the highest energy.

A

– Gamma rays

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28
Q

what kind of wavelengths of light have higher energy
(higher frequency).

A

shoter

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29
Q

The interaction between waves is called

A

interference

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30
Q

what kind of interference is this?
when waves interact so that they add to make a larger wave

A

Constructive interference

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31
Q

when waves interact so that they add to make a larger wave

A

in phase

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32
Q

what kind of interference is this?
when waves interact
so they cancel each other it is called

A

out of phase

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33
Q

When traveling waves encounter an obstacle or
opening in a barrier that is about the same size as
the wavelength, the waves bend around the
obstacle;

A

diffraction

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34
Q

The diffraction of light through two slits separated by a distance comparable to the wavelength results in an

A

interference
pattern

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35
Q

what is the photoelectric effect

A

was observed that many metals emit electrons
when a light shines on their surface.

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36
Q

light energy being transferred to the electron.

A

Classic wave theory

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37
Q

According to this theory, only the amplitudeof
the light (i.e. intensity) determines emission of the
electron.

A

Classic wave theory

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38
Q

was needed for electrons to be
emitted regardless of the light
intensity

A

minimum frequency

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39
Q

light intensity

A

threshold
frequency

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40
Q

light from a dim source caused
electron emission without any
lag time.

A

High-frequency low-intensity

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41
Q

packets that deliver atoms

A

quanta or photons

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42
Q

what is Planck’s constant?

A

6.626 ×10−34 J ∙ s.

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43
Q

One photon at the threshold frequency gives
the electron just enough energy for it to what?

A

escape the atom.

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44
Q

When irradiated with a what? the electron
absorbs more energy than is necessary to
escape.

A

shorter wavelength
photon (higher frequency),

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45
Q

the energy needed for a electron to escape the atom

A

binding energy

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46
Q

This excess energy becomes

A

kinetic energy of the ejected electron.

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47
Q

When atoms or molecules absorb energy, that
energy is often released as what?

A

light energy

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48
Q

When that emitted light is passed through a
prism, a pattern of particular wavelengths of
light is seen that is unique to that type of atom
or molecule – the pattern is called an

A

emission spectrum.

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49
Q

analyzed the spectrum of
hydrogen and found that it could be
described using the following mathematical
equation:

A

Johannes Rydberg

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50
Q

how the structure of atoms change when it undergoes energy transitions.

A

The Bohr Model of the Atom

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51
Q

explains absorption and emission spectra.

A

Bohr model of the atom

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52
Q

Bohr’s major idea was what?

A

that the energy of the atom
was quantized, and that the amount of energy in
the atom was related to the electron’s position
in the atom

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53
Q

means that the atom could only have very
specific amounts of energy.

A

Quantized

54
Q

the electrons travel in orbits that are at a

A

fixed
distance from the nucleus.

55
Q

when do electrons emit radiation?

A

hen they “jump”from
an orbit with higher energy down to an orbit with
lower energy.

56
Q

what determines the energy of a photon?

A

distance between the orbits

57
Q

are manifestations of the wave nature of electrons

A

stationary states

58
Q

Electrons are never observed between what?

A

stationary states

59
Q

proposed that particles have wave-
like properties.

A

Louis de Broglie

60
Q

predicted that the wavelength of a
particle was inversely proportional to its
momentum.

A

Louis de Broglie

61
Q

predicted that energy is proportional to the radius of orbit

A

bohr

62
Q

proof that electrons had wave nature came from what?

A

electrons would produce an interference
pattern

63
Q

Any experiment designed to observe the electron
results in detection of a single electron particle and no interference pattern.

A

Uncertainty Principle Demonstration

64
Q

interference pattern

A

Wave nature

65
Q

position, which slit it is passing
through (waves do not have defined positions)

A

Particle nature

66
Q

The wave and particle nature of the electron
are

A

complementary properties.

67
Q

stated that the product of the uncertainties in
both the position and speed of a particle was inversely proportional to its mass

A

Heisenberg

68
Q

the more accurately you know the
position of a small particle, such as an electron, what?

A

the less you know about its speed, and vice versa.

69
Q

particles move in a path determined by what?

A

particle’s velocity,
position, and forces acting on it.

70
Q

definite, predictable future

A

Determinacy

71
Q

indefinite future, can only predict
probability

A

indeterminacy

72
Q

Because we cannot know both the what and what we cannot predict the path it will follow.

A

position and
velocity of an electron,

73
Q

what can we find out about electrons with the information given to us?

A

probability an electron will be found in a particular region

74
Q

Electron energy and position are what?

A

complementary

75
Q

slide 67 on The spin quantum number specifies the

A

orientation of the spin of the electron.

76
Q

spin up

A

+1/2

77
Q

spin down

A

-1/2

78
Q

it transitions from an orbital in a lower energy level to an orbital in a higher
energy level.

A

excited

79
Q

it transitions from an orbital in a higher energy level to an orbital in a lower energy level.

A

relaxes

80
Q

When an electron relaxes what happens?

A

a photon of light is released
whose energy equals the energy difference between
the orbitals.

81
Q

allows us to calculate the probability of finding an electron with a particular amount of energy at a
particular location in the atom.

A

Schrödinger’s equation

82
Q

a probability distribution map of a region where the electron is likely to be found.

A

orbital,

83
Q

three integer terms in the wave function.

A

quantum numbers

84
Q

what does n stand for?

A

Principal quantum number,

85
Q

what does l mean

A

Angular momentum quantum number

86
Q

what does ml mean?

A

Magnetic quantum number,

87
Q

what to know ab n

A

on notes

88
Q

determines the shape of the orbital

A

l

89
Q

what kind of orbitals are s?
what is the number of l associated with it?

A

spherical
l = 0

90
Q

what to know ab l

A

look on notes

91
Q

what kind of orbitals are p?
what is the number of l associated with it?

A

two balloons tied at the knots.
l = 1

92
Q

what kind of orbitals are d?
what is the number of l associated with it?

A

like four balloons tied at
the knots.
l = 2

93
Q

what kind of orbitals are f?
what is the number of l associated with it?

A

orbitals are mainly like
eight balloons tied at the knots.
l = 3

94
Q

specifies the orientation of the orbital

A

ml

95
Q

what to know ab ml

A

look at notes

96
Q

Orbitals with the same value of are in the
same what?

A

principle energy level or principle shell

97
Q

Orbitals with the same values of n and l
are said to be in the same what

A

in the same sub level or subshell

98
Q

the number of sublevels within a
level = to what?

A

n

99
Q

the number of orbitals (ml) within a sublevel = to what?

A

2l + l

100
Q

the number of orbitals in a level is equal to what?

A

n squared

101
Q

specifies the orientation of the
spin of the electron. (ms)

A

The spin quantum number

102
Q

The wavelengths of lines in the emission
spectrum of hydrogen can be predicted by what?

A

calculating the difference in energy between any two states.

103
Q

can predict these lines very accurately
for a 1-electron system.

A

Bohr mechanical models
and
quantum mechanical models

104
Q

The energy of a photon released is equal to

A

the difference in energy between the two
levels between which the electron is
transitioning.

105
Q

represents the probability (per unit volume)
of finding an electron at a particular point in space.

A

probability density function

106
Q

what we need to know ab s orbitals

A

look at notes

107
Q
A

s orbital

108
Q

To get a better idea of the orbital radius of the electron, we use the what?

A

radial distribution function.

109
Q

represents the total probability of finding an
electron within a thin spherical shell at a distance r
from the nucleus.

A

The radial distribution function

110
Q

is the net result of the radial distribution function

A

is a plot that
indicates the most probable
distance (r) of the electron

111
Q

the shape of the radial distribution
function is the result of

A

multiplying
two functions with opposite trends:

112
Q

decreases with increasing r.

A

probability density function

113
Q

increases with increasing r

A

volume of the thin shell

114
Q
A

2s orbital

115
Q

volume of the thin shell, which is
what ? at the nucleus

A

zero

116
Q

The Probability Density/unit volume maximum is where for the s orbital.

A

the nucleus

117
Q

represents the total probability of finding
an electron at a certain radius from the nucleus.

A

The radial distribution function

118
Q

where is the radial distribution function at maximum?

A

at the most probable radius

119
Q

in the functions are where the probability drops to 0.

A

nodes

120
Q

how many and where are the nodes in p orbital?

A

one and at the nuclues

121
Q

where does the p orbital stand energy wise?

A

second lowest

122
Q

n levels are d orbitals found

A

3 and greater

123
Q

what n levels are p orbital found

A

2 and up

124
Q

what n values are s orbitals found?

A

1 and up

125
Q

what rank is the s orbital according the amount of energy

A

lowest energy

126
Q

what rank is the d orbital according the amount of energy

A

third lowest energy

127
Q

what rank is the f orbital according the amount of energy

A

4 and greater

128
Q

what rank is the f orbital according the amount of energy

A

the fourth lowest

129
Q

are determined from mathematical wave functions

A

orbitals

130
Q

how are orbitals determined?

A

wave functions

131
Q

The sign of the wave function is called its

A

phase

Chemistry 1 (14 decks)

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