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Chem 0330 > Exam 1: Atoms and Molecules > Flashcards

Exam 1: Atoms and Molecules Flashcards

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1
Q

Development of Atomic Theory

Who discovered the electron?

A

JJ Tompson

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2
Q

Development of Atomic Theory

How was the electron discovered?

What expirement?

A

Cathode Ray Expirement

Particles deflected based on charge

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3
Q

Development of Atomic Theory

JJ Thompsons model of the atom

A

Plum Pudding Model

Negative electrons, surrounded by positivity

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4
Q

Development of Atomic Theory

Who discovered the nucleus? With what expirement?

A

Ernest Rutherford, Gold Foil Expirement

Alpha Particles pass through gold foil and bounce of nucleus

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5
Q

Development of Atomic Theory

What atomic model came of the Gold Foil Expirement?

A

Rutherford Model

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6
Q

Quantum Mechanics

Quantum Mechanics explains…

A

behaviour of microscopic matter

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7
Q

Classical Mechanics

According to Classical Mechanics is light a particle or a wave?

CLASSICAL MECHANICS

A

Wave

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8
Q

Classical Mechanics

F= (Q1)(Q2)/(4)(π)(ε)(r²)

Coulomb’s Force Law is used for…

A

Q= charge of particles
ε = permivitity constant
r = distances between pa

Force between 2 charged particles

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9
Q

Classical Mechanics

F=(m)(a)

Newton’s Second Law states…

A

F= force applied to particle
m= mass of particle
a= acceleration of particle

how fast particles are moving

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10
Q

Classical Mechanics

Classical Mechanics fails because…

A

it does not explain microscopic particle behaviour.

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11
Q

Quantum Mechanics

What two assumptions are made in Quantum Mechanics

A
  1. Radiation and matter display wave-like and particle-like properties (wave-particle duality)
  2. Energy is quanticed into discrete packets (photons)
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12
Q

Quantum Mechanics - Wave-Particle Duality

λ

Lambda

A

Wavelength: Distance between two successive maxima (or minima)

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13
Q

Quantum Mechanics - Wave-Particle Duality

μ

Mu

A

Frequency: Number of cycles per unit time

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14
Q

Unit Conversions

m to nm

A

m x 10^-9

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15
Q

Unit Conversions

nm to m

A

nm/10^-9

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16
Q

Light as a Wave

Causes periodic variation of ____ and ____ field

A

Electric and Magnetic

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17
Q

Light as a Wave

Emits ____ radiation

A

Electromagnetic

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18
Q

Light as a Wave

c = λμ

c = constant for electromagnetic waves

A

c = speed of wave (light) (m/s)
λ = wavelength (m)
μ = frequency (s^-1)

c = 2.9979 x 10^8 m/s

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19
Q

Colour of Light

Red has a ____ wavelength?

A

High

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20
Q

Colour of Light

Purple has a ____ wavelength?

A

Low

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21
Q

Colour of Light

Red has a ____ frequency

A

Low

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22
Q

Colour of Light

Purple has a ____ frequency

A

High

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23
Q

Wave Interaction

Define superposition

A

The result when two or more waves interact

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24
Q

Wave Interaction

Constructive interference is____

A

When two waves meet and there absolute amplitudes increase

Max + Max or Min + Min

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25
Q

Wave Interactiopn

Destructive Interference is ____

A

When two waves meet and their amplitudes cancel out

Max + Min

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26
Q

Wave Interference

At superposition wavelength and frequency of the waves change

True or False

A

False

Wavelength and frequency of the wave(s) does not change

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27
Q

Wave Interaction

Thomas ____’s ____ expirement proved ____

Name, Expirement Name, Expirement Purpose

A

Young, Double Slit Expirement, Light has wave properties

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28
Q

Photoelectric Effect

Electrons ejected if:
1. Frequency of light is less than the metal’s threshold frequency
2. Metal’s threshold frequency is less than the frequency of light

Choose 1 or 2

A

2

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29
Q

Photoelectric Effect

Number of electrons ejected increases as frequncy increase after the threshold frequency

True or False

A

False

After the threshold frequency the number of electrons is constant

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30
Q

Photoelectric Effect

Kinetic Energy (KE) of ejected electrons stays constant as frequency increase after the threshold frequency.

True or False

A

False

KE increases as frequency increases

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31
Q

Photoelectric Effect

Light intensity (photons/second) has no affect on Kinetic Energy

True or False

A

True

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32
Q

Photoelectric Effect

Number of electrons ejected increases as light intensity increases

True or False

A

True

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33
Q

Kinetic Energy Equation

KE = Ei - Φ

A

KE = Kinetic Energy
Ei = hµ = hc/λ = Energy of incident light
Φ = hµ (threshold frequency) = workfunction

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34
Q

New Photoelectric Effect

If KE is _ than zero there are no electrons ejected

Fill in the Blank

A

≤
Less than

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35
Q

New Photoelectric Effect

Number of electrons ejected is always less than the number of photons applied.

True or False

A

False

Number of electrons out = Number of photons in

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36
Q

Unit Conversion

eV to J

How to convert?

A

x (1.6022 x 10^-19)

Number on Equation Package

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37
Q

Unit Conversion

J to eV

A

J / (1.6022 x 10^-19)

Number on Equation Package

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38
Q

Photon Momentum

DeBroglie Wavelength Equation

Can be determined by equations on Equation Package

A

λ = h/mv

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39
Q

Schrodinger Equation

GP Thomson discovered light’s ….

He is also the son of …

A

Wave-like properties

JJ Thomson

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40
Q

Schrodinger Equation (Hydrogen)

The gorund state is the ____ energy level and it is the ____ stable state

Fill in the blanks

A

Lowest, most

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41
Q

Schrodinger Equation

En = -RH/n^2
This is the equation for binding energy of all atoms

Define variables and answer True or False

A

En = binding energy
RH = Rydberg’s Constant (on Equation Package)
n = Principle Quantum Number

False

This is the equation for Hydrogen ONLY with one elecetron

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42
Q

Binding Energy

For any one electron systems binding energy is equal to
En = -(Z^2)(RH)/n^2

True or False then define Z

A

True
Z = atomic number

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43
Q

Binding Energy

Binding energy is always….

+ or -

A

Negative

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44
Q

Binding Energy

A free electron has a binding energy > zero

True or False

A

False

Free electrons have 0 binding energy

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45
Q

Binding Energy

Consider the binding energy equation…
1. As n increases binding energy gets more negative and therefore electron is strongy bound
2. As Z increases binding energy gets more negative and therefore electron is weakly bound

True or False for each

A
  1. False, as n increases binding energy gets less negative causing weakly bound electrons
  2. False, as Z increase binding energy gets more negative causing strongly bound electrons
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46
Q

Ionization Energy and Binding Energy

En = -IE

Define and explain both sides of the equation

A

En = Binding energy and is always negative
IE = Ionization energy and is always positive

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47
Q

Ionization Energy

Ionization energy is the ____ energy needed to ____ electron

Fill in the blanks

A

minimum, remove

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48
Q

Ionization Energy

Ionization energy is always > zero

True or False

A

True

IE is always positive

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49
Q

Photon Emission

Electron goes from ____ n state to ____ low n state

Fill in the blanks

A

high, low

High to Low

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50
Q

Photon Emission

Electromagnetic Radiation is…

A

Photon Emission

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51
Q

Photon Emission

∆E = Ei - Ef

Define Variables

A

∆E = Change in energy = energy of photon emitted
Ei = energy at initial n state
Ef = energy at final n state

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52
Q

Balmer Series

____ Balmer discovered that H atoms emit visable light in the year ____

Fill in the blanks

A

JJ, 1885

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53
Q

Photon Emission

Large ∆E means ____ µ and ____ λ

Fill in the blanks

A

high, low

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54
Q

Photon Emission

Low µ and high λ results from a ____ ∆E

Fill in the blank

A

Small

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55
Q

Photon Emission

µ = [(Z^2)(RH)/h] [(1/nf^2)-(1/ni^2)]

Define Variables

A

Z = atomic number
RH = Rydberg’s constant
h = Planck’s constant
nf = final n state
ni = initial n state

56
Q

Photon Absorbtion

Photon absorbtion is the ____ of photon emission. It occurs when photon goes from ____ n state to ____ n state.

Fill in the blanks

A

opposite/reverse, low, high

Low to High

57
Q

Photon Absorbtion

µ = [(Z^2)(RH)/h] [(1/ni^2)-(1/nf^2)]

Define Variables

A

Z = atomic number
RH = Rydberg’s constant
h = Planck’s constant
ni = initial n state
nf = final n state

58
Q

Wavefunctions

Wavefunction Symbol

A

𝚿

59
Q

Wavefunctions

Wavefunctions depend on which 3 quantum numbers?

A

n, l, ml

60
Q

Wavefunction Shapes

Degenerate wavefunctions (orbitals) have the same ____ and therefore same ____

Fill in the blanks

A

n value, energy

61
Q

Wavefunction Shapes

Number of degenerate orbitals (wavefunctions) equal…

A

n^2

62
Q

Wavefunction Composition

𝚿 = radial wavefunction x angular wavefunction

Define terms

A

Radial Wavefunction: dependent on n and l

Angular Wavefunction: dependent on l and ml

63
Q

Wavefunction Composition

s orbitals are ____ symetric so all s orbitals share the same value for ____ wavefunction

Fill in the blanks

A

spherically, angular

64
Q

Wavefunction Composition

Wavefunctions of s orbitals are dependent on radial or angular wavefunction?

Explain why

A

Radial because it is independent of θ and Φ therefore angular wavefunction is consistant across all s orbitals (spherical symetry)

65
Q

Wavefunction Composition

All p orbitals have l = ____, so their ____ wavefunctions are all the same

Fill in the blanks

A

1, radial

66
Q

Wavefunction Composition

p orbitals’ wavefunctions depend on their angular or radial wavefunctions?

Explain why

A

Angular because all p orbitals share a radial wavefunction, and angular wavefunctions differ due to differing ml values

67
Q

Nodes

Radial nodes occur when a radius causes 𝚿 = ?

A

0

68
Q

Nodes

Angular nodes occur when ____ cause 𝚿 = 0

Fill in the blank

A

θ and Φ/ angles

69
Q

Nodes

Number of radial nodes =

A

n - 1 - l

70
Q

Nodes

Number of angular nodes =

A

l

71
Q

Nodes

Total number of nodes =

A

n-1

72
Q

Radial Probability Distribution (RPD)

RPD graphs plot…

A

Probability of finding an electron at a certain radius

73
Q

Radial Probability Distribution

The highest point on a RPD (rpm) is …

A

The value of r (the radius) where there is most likely to be an electron

74
Q

Radial Probability Distribution

Radial nodes occur when RPD function …

A

touches x-axis/ equals zero

75
Q

Radial Probability Distribution

As n increases, rpm…

A

increases

76
Q

Radial Probability Distribution

As l increaes, rpm…

A

decreases

77
Q

Multi Electron Systems

When describing an orbital ____ quantum number(s) should be used

Fill in the blank with a number

A

3

78
Q

Multi Electron Systems

When describing an electron ____ quantum number(s) should be used

Fill in the blank with a number

A

4

79
Q

Multi Electron Systems

Aufbau’s Principle says:

A

Electrons fill orbitals in order of lowest energy state to highest energy state

80
Q

Multi Electron Systems

Hund’s Rule states:

A

A single electron occupies each orbital in each energy state before doubling up, and all single electrons are spin up.

81
Q

Multi Electron Systems

Pauli’s Exclusion Principle states:

A

No two electrons can have the same exact quantum numbers, so when electrons share an orbital one will be spin up and the other spin down (ms = +1/2 vs. ms = -1/2)

82
Q

Multi Electron Systems

Binding energy depends on ____ and ____ quantum numbers

Fill in the blanks

A

n, l

83
Q

Multi Electron Systems

Enl = -IEnl = -(Zeff^2)(RH)/n^2

Define variables

A

Enl = Binding energy of multi electron system
IEnl = Ionization energy of multi electron system
Zeff = Effective charge (from sheilding effect)
RH = Rynberg’s constant
n = Principle quantum number

84
Q

Sheilding Effect

Zeff should always be between Z is there was ____ sheilding and Z is there was ____ sheilding

Fill in the blanks

A

no, complete

Reminder: Z = atomic number, sheilding effect changes charge

85
Q

Electron Configurations

Which 2 elements have exceptions to Aufbau’s principle? Why?

A

Cr and Cu because half filled and fully filled d orbitals are favoured over s orbitals.

d orbital steals electron from s orbital

86
Q

Electron Configurations

s orbitals contain ____ electrons, p orbitals contain ____ electrons, d orbitals contain ____ electrons, f orbitals contain ____ electrons

Fill in the blanks with numbers

A

2, 6, 10, 14

87
Q

Periodic Trends

On the periodic table, n quantum number is represented by….

Details!!!!!

A

Period

Groups 3 - 12 see that n = period number -1

88
Q

Periodic Trends

On the periodic table, groups ____ and ____ will have their valence electrons in s orbitals

Fill in the blanks with numbers

A

1 and 2

89
Q

Periodic Trends

On the periodic table, groups ____ to ____ will have their valence electrons in p orbitals

Fill in the blanks with numbers

A

13 to 18

90
Q

Periodic Trends

On the periodic table, groups ____ to ____ will have their valence electrons in d orbitals

Fill in the blanks with numbers

A

3 to 12

91
Q

Periodic Trends

On the periodic table, which elements have their valance electrons in f orbitals?

A

Special elements (atomic numbers 57-71 and 89-103)

92
Q

Quantum Numbers

n is the…

A

principle quantum number

93
Q

Quantum Numbers

l =

A

n-1

94
Q

Quantum Numbers

l = 0 results in which orbital

A

s

95
Q

Quantum Numbers

l = 1 results in which orbital

A

p

96
Q

Quantum Numbers

l = 2 results in which orbital

A

d

97
Q

Quantum Numbers

l = 3 results in which orbital

A

f

98
Q

Quantum Numbers

ml =

A

range from -l to +l

99
Q

Quantum Numbers

ms =

A

+1/2 or -1/2

100
Q

Ions Electron Configurations

Once a d orbital is filled
(when an atom becomes ionized) the electrons are removed from previous s orbital

True or False

A

True

101
Q

Electron Configurations

Isoelectronic ions and atoms are…

A

ions and atoms that have the same electron configurations

102
Q

Periodic Trends

Describe the trend of IE in terms of the periodic table

A

IE increase as you move up and right across the periodic table

103
Q

Periodic Trends

Describe the trend of Electron Affinity (EA) in terms of the periodic table

A

EA increase as you move up and right across the periodic table

104
Q

Periodic Trends

Describe the trend of Electronegativity (X) in terms of the periodic table

A

X increase as you move up and right across the periodic table

105
Q

Periodic Trends

Describe the trend of Atomic Radius in terms of the periodic table

Ionic Radius?

A

Atomic Radius increase as you move down and left across the periodic table

Increases as you move down the periodic table

106
Q

Periodic Trends

What are the exceptions to the IE periodic trend?

A

Half full/ full orbitals are more stable and therefore favoured, so they have higher than expected ionization energies

107
Q

Periodic Trends

What are the exceptions to the EA periodic trend?

A

Noble Gases are stable and do not seak stability therefore they have very negative EA

108
Q

Bonding

Chemical bonding is the arrangment of atoms that result in ____ ____ energy than the atoms have seperatley

A

more negative

109
Q

Periodic Trends

What are the exceptions to the X periodic trend?

A

Noble Gases are stable and do not seak electrons therefore they have X = 0

110
Q

Bonding

The complete transfer of electrons is which type of bonding?

Ionic, Covalent, Polar-Covalent

A

Ionic

111
Q

Bonding

Ionic bonding results in a ∆X

A

≥1.7

112
Q

Bonding

Covalent bonding is when an electron pair is ____ shared between two atoms

Fill in the blank

A

equally

113
Q

Bonding

∆X ≤ 0.4 is a result of which type of bonding?

Ionic, Covalent, Polar-Covalent

A

Covalent

114
Q

Bonding

An unqual sharing of an electron pair is what type of bonding?

Ionic, Covalent, Polar-Covalent

A

Polar-Covalent

115
Q

Bonding

Polar-Covalnet bonds have ∆X =

A

0.4-1.7

116
Q

Bonding

Dissociation Energy is…

A

The amount of energy required to break a chemical bond and seperate chemically bonded atoms

117
Q

Lewis Structures

In step 1, when drawing Lewis Structures, which atom goes in the middle?

A

The atom with the lowest IE

118
Q

Lewis Structures

In step 2, when drawing Lewis Structures, one should total the number of…

A

Valence electrons

119
Q

Lewis Structures

In step 3, when drawing Lewis Structures, one should total…

A

The number of electrons in full valence shells

120
Q

Lewis Structures

In step 3, when drawing Lewis Structures, one should total…

A

The number of electrons in full valence shells

121
Q

Lewis Structures

In step 4, when drawing Lewis Structures, one should determine the number of bonding electrons by…

A

Subtracting valence electrons (step 2) from full valence electrons (step 3)

122
Q

Lewis Structures

In step 5, when drawing Lewis Structures, one bond is made up of ____ bonding electrons

Fill in the blank with a number

A

2

123
Q

Lewis Structures

In step 6, when drawing Lewis Structures, if there are bonding electrons remaining one should

A

include double/tripple bonds

124
Q

Lewis Structures

In step 7, when drawing Lewis Structures, one should determine the number of loan pair electrons by…

A

Subtracting bonding electrons (step 4) from total valence electrons (step 3)

125
Q

Formal Charge

Formal charge applies to ____ bonding only

Fill in the blank

A

Covalent

126
Q

Formal Charge

FC =

A

V-L-B

V = valence electrons
L = loan pair electrons
B = number of bonds

127
Q

Formal Charge

Formal Charge is the extent to which an atom has lost/gained an electron

True or False

A

True

128
Q

Formal Charge

How does formal charge relate to the charge of the molecule?

A

Sum of FC of each atom = molecule charge

129
Q

Formal Charge

Lewis structures with highest absolute FC are the most stable and therefore have the lowest energy

True or False

A

False

*lowest absolute FC

130
Q

Formal Charge

Negative FC = most electrnegative = most stable = highest energy

True or False

A

False

*lowest energy

131
Q

Resonance Structures

All molecules have resonance structures

True or False

A

False

132
Q

Resonance Structures

Resonance structures have ____ atom arrangment and ____ bond arrangment

Fill in the blanks

A

same, different

133
Q

Resonance Structures

FC is constant across resonance structures

True or False

A

True

134
Q

Octet Rule Exceptions

When there is an odd number of valence electrons it is impossible for…

A

all atoms to have complete octets

135
Q

Octet Rule Exceptions

A radical species is a result of…

A

An unpaired electron from an odd number of valence electrons

136
Q

Octet Rule Exceptions

Which two elements will be octet difficent (have incomplete octets)

A

Al and B

Aluminium and Boron

137
Q

Octet Rule Exceptions

Which elements are eligable for valence shell expansion (expanded octet)?

A

Central elements with n ≥ 3, and empty d orbitals

Chem 0330 (1 decks)

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