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CHEM1045 > Chapter 7 Quantum Mechanical Model Of Atom > Flashcards

Chapter 7 Quantum Mechanical Model Of Atom Flashcards

1
Q

Forms the foundation of chemistry

A

Quantum Mechanics

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2
Q

Electron behavior determines much of the

A

Behavior of Atoms

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3
Q

Why is directly observing electrons in the atoms impossible?

A

The electron is so small that observing it changes its behavior

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4
Q

The ___ explains the manner in which electrons exist and behave in atoms

A

Quantum - Mechanical Model

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5
Q

What does the Quantum - Mechanical Model explain?

A
  • Why some elements are metals and some are Nonmetals
  • Why some elements gain one electron when forming an anion, while others gain two
  • Why some elements are very reactive while others are practically inert
  • Periodic patterns we see in the properties of elements
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6
Q

Light is a form of

A

Electromagnetic Radiation

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7
Q

Why is light composed of ?

A

Perpendicular oscillating waves, one for the electric field and one for the magnetic field

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8
Q

An ___ field is a region where an electrically charged particle experiences a force

A

Electric

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9
Q

A ___ field is a region where a magnetized particle experiences a force

A

Magnetic

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10
Q

What is the speed of light?

A

3.00 x 10^8 m/s in a vacuum

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11
Q

Wha is the speed of sound?

A

340 m/s

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12
Q
  • The ___ is the height of the wave

* The distance from node to crest

A

Amplitude

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13
Q

The larger the amplitude, the ___ the light

A

Brighter

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14
Q
  • The ___ is a measure of the distance covered by the wave

* The distance from one crest to the next

A

Wavelength (l)

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15
Q
  • The ___ is the number of waves that pass a point in a given period of time
  • The number of waves = of cycles
A

Frequency (n)

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16
Q

What are the units for frequency ?

A

Hertz (Hz) or cycles = s-1

1 Hz = 1 s-1

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17
Q

The ___ is proportional to the amplitude of the waves and the frequency

A

Total Energy

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18
Q

The larger the amplitude, the ___ force it has

A

More

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19
Q

The more frequency the waves strikes, the ___ total force there is

A

More

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20
Q

For waves traveling at the same speed, the shorter the wave length, the ___ frequently they pass

A

More

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21
Q

Wavelength and frequency of electromagnetic waves are

A

Inversely proportional

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22
Q

Because the speed of light is constant, if we know the wavelength we can find

A

The Frequency and vice versa

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23
Q

What is the formula for frequency ?

A

v(s-1) = c(m/s) / ?(m)

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24
Q

The color is determined by

A

It’s wavelength (or frequency)

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25
Q

White light is a mixture of

A

All colors of visible light (a spectrum)

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26
Q

When an object absorbs some of the wavelengths of white light and reflects others

A

It appears colored

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27
Q

The observed color is predominately

A

The colors reflected

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28
Q

Different wavelength, different

A

Color

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29
Q

Different amplitude, different

A

Brightness

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30
Q

Visible light compromises only a small fraction of all wavelengths of light - called

A

The Electromagnetic Spectrum

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31
Q

Shorter wavelength (higher frequency) light has ___ energy

A

Higher

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32
Q

Radio wave light has the ___ energy

A

Lowest

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33
Q

Gamma ray light has the ___

A

Energy

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34
Q

High-Energy electromagnetic radiation can potentially damage biological molecules

A

Ionizing radiation

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35
Q

What is the order of electromagnetic waves from low frequency and energy to high frequency and energy ?

A
  • Radiowaves
  • Microwaves
  • Infrared
  • Visible
  • Ultraviolet (UV)
  • Xray
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36
Q

High-Energy radiation can also be used to kill

A

Cancer Cells

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37
Q

The interaction between waves is called

A

Interference

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38
Q

When waves interact so that they add to make a larger wave it is called

A

Constructive Interference

• Waves are in-phase

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39
Q

When waves interact so they cancel each other it is called

A

Destructive Interference

• Waves are out-of-phase

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40
Q

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

A

Diffraction

• traveling particles do not diffract

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41
Q

The diffraction of light through 2 slits separated by a distance comparable to the wavelength results in an ___ ___ of the diffracted waves

A

Interference Pattern

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42
Q

An interference pattern is a characteristic of

A

All light waves

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43
Q

Destructive interference

A

Path lengths differ by ?/2

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44
Q

Constructive Interference

A

Equal path lengths

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45
Q

Waves out-of-phases make ___ spots

A

Dark

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46
Q

Waves in-phase make ___ spots

A

Bright

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47
Q

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

A

Photoelectric Effect

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48
Q

Classic wave theory attributed this effect to the ___ ___ being transferred to the ___

A

Light Energy, Electron

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49
Q

According to the Classic Wave Theory, if the wavelength of light is made ___, or the light waves intensity was made ___, more electrons should be ejected

A

Shorter, Brighter

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50
Q

If a dim light were used they would be a ___ before the electrons were emitted

A

Lag in time

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51
Q

In experiments it was observed that there was a minimum frequency needed before electrons would be emitted (regardless of intensity)

A

Threshold Frequency

52
Q

High-Frequency light from a dim source caused electron emission

A

Without any lag time

53
Q

Einstein propose that the light energy was delivers to atoms in packets, called ___ or ___

A

Quanta, Photons

54
Q

The energy of a photon of light is ___ to its frequency

A

Directly proportional

55
Q

The proportional constant between a photon of light and its frequency is called

A

Planck’s Constant (h)

56
Q

What is the value of Planck’s Constant ?

A

6.626 x 10^-34 J•s

57
Q

What is the equation for total energy?

A

E = hv = (h•c) / ?

58
Q

Order wavelength (short to long)

A
  • Gamma
  • UV
  • Green
  • Red
  • Microwaves
59
Q

Order by energy (least to most)

A
  • Microwaves
  • Red
  • Green
  • UV
  • Gamma
60
Q

Order by frequency (low to high)

A
  • Microwaves
  • Red
  • Green
  • UV
  • Gamma
61
Q

One photon at the threshold frequency gives the electron just enough energy for it to escape the atom

A

Binding Energy (f)

62
Q

When irradiated with a ___ wavelength photon, the electron absorbs more energy than is necessary to escape

A

Shorter

63
Q

The excess energy becomes ___ energy of the ejected electron

A

Kinetic

64
Q

Equation for Kinetic Energy

A

Kinetic Energy = E photon - E binding

KE = hn - f

65
Q

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

A

Light Energy

Ex: fireworks, neon lights

66
Q

When 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

A

Emission Spectrum
• Non-continuous
• Can be used to identify the material

67
Q

Prism separates component

A

Wavelengths

68
Q

Rydberg analyzed the spectrum of hydrogen and found that it could be described with an equation that involved an inverse square of integers

A

1/? = 1.097 x 10^7 m^-1 (1/n1^2 - 1/n2^2)

69
Q

The atom contains a tiny dense center called the

A

Nucleus

• 1/10 trillionth the volume of the atom

70
Q

The nucleus is essentially the ___ of the atom

A

Entire mass

71
Q

The nucleus is ___ charged

A

Positively

72
Q

Electorons are ___ and ___ particles

A

Moving and Charged

73
Q

According to classical physics, moving charges give off ___

A

Energy

74
Q

Based on classical physics, electrons should constantly be

A

Giving off energy, make the atom flow, and lose energy when it crashes into the nucleus and cause the atom to collapse
• but it doesn’t (problem with Rutherfords Nuclear Model of the Atom)

75
Q

Bohr developed a model of the atom to explain how

A

The structure of the atom changes when it undergoes energy transitions

76
Q

Bohr’s major idea was that the energy of the atom was ___, and that the amount of energy in the atom was related to the electron’s position in the atom

A

Quantized

77
Q

Quantized means that

A

The atom could only have very specific amounts of energy

78
Q

The electrons travel in orbits that are at a fixed distance from the nucleus

A

Stationary states

79
Q

The energy of the electron was ____ the distance the orbit was from the nucleus

A

Proportional

80
Q

Electrons emit radiation when they “jump” from an orbit with ___ energy to an orbit with ___ energy

A

Higher, lower

81
Q

The distance between the orbits determined the energy of the ___ produced

A

Photon of light

82
Q

De Broglie predicted that the wavelength of a particle was ___ to its momentum

A

Inversely Proportional

83
Q

Formula for the wave character of electrons

A

?(m) = h(kg•m^2/s^2 •s) / mass(kg) • velocity(m•s^-1)

84
Q

What was proof that electrons had wave nature

A

The demonstration that a beam of electrons would produce an interference pattern as waves do

85
Q

Wave nature =

A

Interference Pattern

86
Q

Particle nature =

A

Position, which slit it is passing through

87
Q

When you try to observe the wave nature of the electron, you ___ observe its particle nature (and vice versa)

A

Cannot

88
Q

The wave and particle nature of the electron are

A

Complementary properties

• The more you about one the less you know about the other

89
Q

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

A

Inversely Proportional

• the more accurately you know the positions of a small particle, the less you know about its speed

90
Q

Definite, predictable future

A

Determinacy

91
Q

Indefinite future, can only predict probability

A

Indeterminacy

92
Q

According to classical physics, particles move in a path ___ by the particles velocity

A

Determined

93
Q

Because we cannot know both the position and velocity of an electron, we cannot predict the path it will follow

A

Indeterminacy

94
Q

For an electron with a given energy, the best we can do is

A

Describe a region in the atom of high probability of finding it

95
Q

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

A

Schrödinger’s Equation

96
Q

A plot of distance vs. Y2 represents an ___, a probability distribution map of a region where the electron is likely to be found

A

Orbital

97
Q

Calculations show that the size, shape, and orientation in space of an orbital are determined to be three integer terms in the wave function called

A

Quantum Numbers

98
Q
  • Characterizes the energy of the electron in a particular orbital
  • n (can be any untether => 1)
  • The larger the n value, the more energy and the larger the orbital
A

Principal Quantum Number, n

99
Q

Principal Quantum Number Equation, n

A

E n = -2.18 x 10^-18 J (1 / n^2)

100
Q

• Determines the shape of the orbital
• I can have an integer values from 0 to (n-1)
• Each value of ___ is called by a particular letter that designated the shape of the orbital
- s orbitals are spherical
- p orbitals are like two Ballons tied at the knot
- d orbitals are like four Ballons tied at the knot
- f orbitals are mainly like eight balloons tied at the knot

A

Angular Momentum Quantum Number, l

101
Q 
Each value of l is called by a particular letter that designates the shape of the orbital 
• s =
• p =
• d =
• f =
A
  • s = orbitals are spherical
  • p = orbitals are like two Ballons tied at the knots
  • d = orbitals are mainly like four Ballons tied at the knot
  • f = orbitals are mainly like eight Ballons tied at knot
102
Q

The ___ number is an integer that specifies the orientation of the orbital
• The direction in space the orbital is aligned relative to the other orbitals

A

Magnetic Quantum

103
Q

Each set of n, l, and ml describes

A

One Orbital

104
Q

Orbitals with the same value of n are in the same

A

Principal Energy Level

• Aka Principal Shell

105
Q

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

A

Sublevel

• Aka Subshell

106
Q

When an electron is ___, it transitions from an orbital in a lower energy level to an orbital in a higher energy level

A

Excited

107
Q

When an electron ___, it transitions from an orbital in a higher energy level to an orbital in a lower energy level

A

Relaxes

108
Q

When an electron ___, a photon of light is released whose energy equals the energy difference between the orbitals

A

Relaxes

109
Q

To transitions to a higher energy state,

A

The electron must gain the correct amount of energy corresponding to the difference in energy between the final and initial states

110
Q

Electrons in high energy states are unstable and tend to

A

Lose energy and transition to lower energy states

111
Q

Each line in the emission spectrum corresponds to the difference in

A

Energy between two energy states

112
Q

The wavelength of lines in the emission spectrum of hydrogen can be predicted by

A

Calculating the difference in energy between two states

113
Q

Both the ___ and the ___ models can predict these lines very accurately for a 1-electron system

A

Bohr and Quantum Mechanical

114
Q

The energy of a photon released is equal to the difference in

A

Energy between the two levels the electron is jumping between

115
Q

It can be calculated by

A

Subtracting the energy of the initial state from the energy of the final state

116
Q

The probability of finding an electron at a particular point in space

A

Y2 is the probability density

• decreases as you move away from the nucleus

117
Q

The ___ function represents the total probability at a certain distance from the nucleus

A

Radial Distribution

• Maximum at most probable radius

118
Q

___ in the functions are where the probability drops to 0

A

Nodes

119
Q

The ___ function represents the total probability of finding an electron at a particularly point in space

A

Probability Density

120
Q

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

A

Radial Distribution

121
Q

The probability at a point ___ with increasing distance from nucleus, but the volume of the spherical shell ___

A

Decreases, increases

122
Q

The quantum l primarily determines

A

The shape of orbital

123
Q

Orbitals are determined from

A

Mathematical wave functions

124
Q

A wave function can have a __ or __ value

A

Positive and negative (as well as nodes where the wave function = 0)

125
Q

The sign of the wave function is called its

A

Phase

126
Q

When orbitals interact, their wave functions may be ___ (same sign) or ___ (opposite sign)

A

In-phase, out-of-phase

CHEM1045 (7 decks)

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