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CEM 141 > Chapter 2 > Flashcards

Chapter 2 Flashcards

1
Q

What is light?
A. A wave
B. A particle
C. Both
D. Neither

A

C.

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2
Q

_______ is the height of peaks (________).

A

Amplitude, intensity

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3
Q

λ = wavelength (m), wavelength is …

A

The distance between two identical points

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4
Q

ν = frequency (Hz = s^-1), frequency is …

A

The number of wavelengths per second

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5
Q

Wavelength and frequency are related by _________: c = λ × v

A

The speed of light

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6
Q

_______ = c = 3.00 × 10^8 m s^-1

A

Speed of light

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7
Q

________ – increases as frequency increases (and wavelength decreases).

A

Energy of light

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8
Q

Let’s say we have 2 objects 1 m apart (10^0 m). How far apart would 2 objects be that were 10^1 m apart?
A. 1 m
B. 10 m
C. 20 m
D. 100 m
E. 1000 m

A

B.

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9
Q

Let’s say we have 2 objects 1 m apart (10^0 m). How far apart would 2 objects be that were 10^2 m apart?
A. 1 m
B. 10 m
C. 20 m
D. 100 m
E. 1000 m

A

D.

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10
Q

Let’s say we have 2 objects 1 m apart (10^0 m). How far apart would 2 objects be that were 10^3 m apart?
A. 1 m
B. 10 m
C. 20 m
D. 100 m
E. 1000 m

A

E.

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11
Q

Which e/m radiation has wavelengths on the order of the sizes of atoms?
A. Radiowaves (λ ≈ m)
B. Microwaves (λ ≈ cm)
C. X-rays (λ ≈ nm)
D. Gamma rays (λ ≈ pm)

A

C.

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12
Q

Determine the wavelength of an X-ray with a frequency of 3.0 × 10^18 Hz in meters. (c = 3.0 × 10^8 m/s).
A. 1.0 × 10^–10 m
B. 9.0 × 10^26 m
C. 9.0 × 10^–19 m
D. 1.0 × 10^–1 m

A

A

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13
Q

Which has the longest wavelength?
A. X-rays
B. Visible
C. Infrared

A

C.

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14
Q

Which has the highest frequency?
A. X-rays
B. Visible
C. Infrared

A

A.

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15
Q

Which has the highest energy?
A. X-rays
B. Visible
C. Infrared

A

A.

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16
Q

Many metals emit _________ when electromagnetic radiation shines on the surface.

A

Electrons

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17
Q

When you increase the intensity of UV light …
A. The number of electrons emitted increases
B. The number of electrons emitted decreases
C. There’s no change
D. There’s zero electrons are emitted

A

A.

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18
Q

When you keep the intensity the same and increase the wavelength (decreasing the frequency) to the blue …
A. The number of electrons emitted increases
B. The number of electrons emitted decreases
C. There’s no change
D. There’s zero electrons are emitted

A

C.

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19
Q

When you keep the intensity the same and increase the wavelength (decreasing the frequency) into the yellow …
A. The number of electrons emitted increases
B. The number of electrons emitted decreases
C. There’s no change
D. There’s zero electrons are emitted

A

D.

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20
Q

When you keep the yellow light and increase the intensity …
A. The number of electrons emitted increases
B. The number of electrons emitted decreases
C. There’s no change
D. There’s zero electrons are emitted

A

D.

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21
Q

If the frequency of the light is above the threshold frequency, _________ from the metal.

A

Electrons are emitted

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22
Q

If the frequency of the light is below the threshold frequency, _________.

A

No electrons are emitted

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23
Q

Einstein postulated that light must come in packets of energy (or particles or quanta) – called …

A

Photons

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24
Q

The energy of light depends on the __________, not on the intensity.

A

Frequency

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25
Q

E/m radiation is a ______ - ______ effect.

A

Particle, photoelectric

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26
Q

Each photon has a definable energy (______).

A

E = hν

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27
Q

If the photon has enough energy, it can eject _______.

A

One electron

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28
Q

What is the energy of a photon of frequency 4.0 × 1018 s–1 (in the X-ray part of the spectrum)?
Constant: h = 6.626 × 10–34 J s
A. 2.6 × 108 J
B. 2.6 × 10–15 J
C. 1.7 × 10–52 J
D. 6.0 × 1051 J

A

B.

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29
Q

What is the wavelength of a photon with an energy of 6.2 × 10^–8 J?
Constants: c = 3.0 × 10^8 m/s, h = 6.626 × 10–34 J s
A. 3.2 × 10^–34 m
B. 3.2 × 10^18 m
C. 3.2 × 10^–18 m
D. 9.4 × 10^25 m

A

C.
SLIDE 40

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30
Q

A covalent bond between two H atoms (in H2) requires 7.2 × 10^–19 J of energy to break, causing the molecule to fall apart. What frequency of light does this correspond to? Constants: c = 3.0 × 10^8 m/s, h = 6.626 × 10^–34 J s
A. 1.1 × 10^15 s–1
B. 9.2 × 10^–16 s–1
C. 4.8 × 10^–52 s–1

A

A.
SLIDE 41

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31
Q

A covalent bond between two H atoms (in H2) requires 7.2 × 10^–19 J of energy to break, causing the molecule to fall apart.
What is the wavelength? Constants: c = 3.0 × 10^8 m/s, h = 6.626 × 10^–34 J s
A. 3.6 × 10^6 m
B. 3.3 × 10^23 m
C. 2.8 × 10^–7 m

A

C.
SLIDE 42

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32
Q

A covalent bond between two H atoms (in H2) requires 7.2 × 10–19 J of energy to break, causing the molecule to fall apart. What is the wavelength in nm?
A. 280 nm
B. 2.8 × 10 –16 nm
C. 2.8 × 10 –7 nm

A

A.
SLIDE 42

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33
Q

________ is important at very small scales.

A

Wave-particle duality

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34
Q

The ________ is the same whether that element is on Earth, in the Sun, or in a galaxy light years away.

A

Spectrum of an element

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35
Q

The next model of the atom was developed by …

A

Niels Bohr

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36
Q

(Bohr Model)
Electrons move in ______ around nucleus.

A

Orbits

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37
Q

(Bohr Model)
The energies of electrons in atoms are …

A

Quantized

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38
Q

(Bohr Model)
The energy of the photons corresponds to the ________ in energy between the orbits.

A

Difference

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39
Q

(Bohr Model)
An _______ moves to higher energy orbit when a ______ is …

A

Electron, photon, absorbed

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40
Q

A ______ is _______ when an _______ moves to lower energy orbit.

A

Photon, emitted, electron

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41
Q

Bohr’s model (electrons moving in defined orbits around nucleus at known energy levels) only works for …

A

Hydrogen

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42
Q

A better way to represent the transitions of electrons upon absorbing or emitting photons is with …

A

Energy Diagrams

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43
Q

Each energy level has a ________, the higher the number the higher the _______.

A

Quantum number, energy

44
Q

Energy levels are NOT ______ (they represent ______ only)

A

Orbits, energy

45
Q

Electrons transition between energy levels by _________ or _______ photons with energies equal to the exact difference in energy between the two levels.

A

Absorbing, emitting

46
Q

Which color photon is emitted when an electron moves from level 2🡪1?
A. Green
B. Orange

A

B.

47
Q

Which photon is absorbed when an electron moves from level 1🡪3?
A. Green
B. Orange

A

A.

48
Q

Is the same amount of energy required to move an electron from n=2 to n=3?
A. Yes
B. No

A

B.

49
Q

Which of the following transitions for an electron in a hydrogen atom would release the largest amount of energy?
A. n = 3 → n = 2
B. n = 4 → n = 2
C.n = 1 → n = 4
D. n = 2 → n = 1

A

D.

50
Q

Can a hydrogen atom absorb or emit every wavelength of light in the visible spectrum?
A. Yes
B. No

A

B.

51
Q

________, all matter has wave properties and, therefore, a wavelength λ.

A

de Broglie

52
Q

________ – λ is much smaller than the object - no effect on properties

A

Macroscopic objects

53
Q

____________ – λ similar in size to the object - affects properties

A

Atomic-scale objects (such as electrons)

54
Q

What is the wavelength of an electron moving at 2.65 × 10^6 m s–1?

Useful Information:
λ = h/(mv)
h = 6.626 × 10^–34 J s
1 J = 1 kg m2 s–2
Mass of an electron is 9.1 × 10^−31 kg

A

2.75 x 10^-10 m

55
Q

Is the wavelength of a human (10–37 m) comparable to the size of a human (1-2 m)?
A. Yes
B. No

A

B.

56
Q

What is the evidence that electrons are waves?
Diffraction and interference pattern of waves of ______ and ______.

A

Light, electrons

57
Q

When electrons are used in the double slit experiment, they show an _______.

A

Interference pattern

58
Q

Are electrons circling around the nucleus in orbits?
A. Yes
B. No
C. Sometimes
D. In the H atom, but no other atoms

A

B.

59
Q

________: regions of space where electrons with a certain quantized energy have a high probability of being found.

A

Atomic orbitals

60
Q

Each orbital can be described by a set of ________ (n, l, ml) that are derived from quantum mechanical calculations.

A

Quantum numbers

61
Q

A fourth quantum number, ______ , describes the electron spin.

A

m(sub)s

62
Q

There ______ s orbital in a “set” or subshell.

A

Is only one

63
Q

The ______ the principal quantum number, the ______ the orbital and the ______ the energy.

A

Larger, larger, higher

64
Q

In a set of p orbitals, there ______ orbitals.

A

Are three

65
Q

In a set of d orbitals, there ______ orbitals.

A

Are five

66
Q

How many orbitals are in the electron cloud of one atom?
A. Only the s orbital
B. Only one p orbital
C. Only the d orbitals
D. All of the orbitals (all s, p, d, etc.) overlap within the electron cloud.

A

D.

67
Q

We often refer to elements by the location of their electrons in the ________ (_______)

A

Outermost orbitals, valence electrons

68
Q

________ are …
- A closed shell of electrons is very stable – they don’t participate in reactions.
- To identify: use the last noble gas (group 18, eg Ne or Xe) and any full d shell (transition metals).

A

Core electrons

69
Q

________, these are the electrons that determine reactivity!

A

Valence electrons

70
Q

Write the electron configuration for
carbon and label the core and valence electrons …

A

1s^2 2s^2 2p^2
-core–valence–

71
Q

Write the electron configuration for
chlorine and label the core and valence electrons…

A

1s^2 2s^2 2p^6 3s^2 3p^5
——–core———-valence—

72
Q

What is the core/valence electron configuration of O?
A. [He] 2s^2 2p^4
B. [Ne] 2s^2 2p^4
C. [Ne] 2s^2 2p^1
D. [He] 2s^2

A

A.

73
Q

How many core and valence
electrons does N have?
A. 2 core, 5 valence
B. 5 core, 2 valence
C. 4 core, 3 valence

A

A.

74
Q

How many valence electrons does P have? How about As? And Sb?

A

5, 5, 5

75
Q

How many core and valence electrons does Si have?
A. 10 core, 4 valence
B. 4 core, 10 valence
C. 12 core, 2 valence

A

A.

76
Q

How many valence electrons does C have? How about Ge? And Sn?

A

4, 4, 4

77
Q

(___________)
Originally developed by Mendeleev
On basis of experimental behavior and repeating (periodic) patterns
He left spaces for undiscovered elements
Originally on basis of increasing atomic mass - then on atomic number
Really electron organization explains repeating patterns

A

Periodic Table

78
Q

What is the electron configuration for Br?
A. [Ar] 4s2 4p5
B. [Ar] 4s2 3d10 4p5
C. [Kr] 4p5

A

B.

79
Q

How many core and valence electrons does Br have?
A. 18 core and 17 valence
B. 28 core and 7 valence
C. 35 core and 0 valence

A

B.

80
Q

We are making the claim that electrons are in orbitals with quantized energies.
What is the evidence for this?

A

Periodic trends

81
Q

The atomic radius of Na is ________ than that of Li.
A. larger
B. smaller
C. no different

A

A.

82
Q

The atomic radius of Ne is ________ than that of Li.
A. larger
B. smaller
no different

A

B.

83
Q

What happens to the force (F) if q1 or q2 increases?
A. increase
B. decrease
C. stays same

A

A.

84
Q

What happens to the force as r increases?
A. increase
B. decrease
C. stays same

A

B.

85
Q

The atomic radius represents the state where the _______________ between the electrons and protons are _____ to the _________________ between the electrons.

A

Forces of attraction, equal to, forces of repulsion

86
Q

Effective nuclear charge _________ across a row.

A

Increases

87
Q

What happens to the attractive force across a row?
A. increases
B. decreases
C. stays same

A

A.

88
Q

Which of the following has the smallest atomic radius?
A. Ar
B. Al
C. Ga
D. Kr

A

A.

89
Q

If an electron is removed from an atom, what is the charge of the ion?
A. Neutral
B. Positive
C. Negative
D. It depends on the element

A

B.

90
Q

The outermost electron is removed resulting in a cation. Cations are ___________ charged.

A

Positively

91
Q

Which has a larger radius?
A. Li
B. Li+
C. Same

A

A.

92
Q

If an electron is added to an atom, what is the charge of the ion?
A. Neutral
B. Positive
C. Negative
D. It depends on the element

A

C.

93
Q

An electron is added to the next available (lowest energy) orbital. Anions are ________ charged.

A

Negatively

94
Q

Which has the largest radius?
A. F
B. F–
C. Same

A

B.

95
Q

Which is larger? Na+ or F–
A. Na+
B. F–
C. Same

A

C.

96
Q

_________: energy required to remove an electron from an atom in the gas phase.

A

Ionization Energy

97
Q

Compare Li and Na. Which is easier to remove an electron from?
A. Li
B. Na
C. Same

A

B.

98
Q

The ionization energy of Na is __________ than that of Li.
A. larger
B. smaller

A

B.

99
Q

Compare Li and Ne. Which is it easier to remove an electron from?
A. Li
B. Ne
C. Same

A

A.

100
Q

The ionization energy of Ne is _________ than that of Li.
A. larger
B. smaller

A

A.

101
Q

(Trends Down a Group)
Atomic radius ________, ionization energy ________.

A

Increases, decreases

102
Q

(Trends Across a Row)
Atomic radius ________, ionization energy ________.

A

Decreases, increases

103
Q

The trends in radius and IE are _________ but caused by the same phenomenon – the _________.

A

Inversely related, effective nuclear charge

104
Q

Which ionization energy is largest?
A. First IE: Mg (g) 🡪 Mg^+ (g) + e^-

B. Second IE: Mg^+ (g) 🡪 Mg^2+ (g) + e^-

C. Third IE: Mg^2+ (g) 🡪 Mg^3+ (g) + e^-

A

C.

105
Q

IE1 1,012 kJ/mol
IE2 1,900 kJ/mol
IE3 2,910 kJ/mol
IE4 4,960 kJ/mol
IE5 6,270 kJ/mol
IE6 22,200 kJ/mol
IE7 26,345 kJ/mol
Which element in period three would most likely show this trend in ionization energies?
A. Mg
B. Al
C. Si
D. P
E. S

A

D.

CEM 141 (7 decks)

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