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Modern Model of the Atom Review

Total questions: 258

Worksheet time: 5hrs 28mins

Name
Class
Date
1.

The distance between peaks of adjacent electromagnetic waves is called _____

a)

wavelength

b)

frequency

c)

energy

d)

amplitude

2.

What symbol is used to represent wavelength?

a)

ℓ

b)

w

c)

λ

d)

Λ

3.

What is the wavelength of the wave?

a)

3 cm

b)

6 cm

c)

12 cm

d)

18 cm

4.

Which wave has the longest wavelength?

a)
b)
c)
d)
5.

The number of waves that pass a fixed point in a given amount of time is the ...

a)

frequency

b)

wave speed

c)

amplitude

d)

wavelength

6.

The frequency of a wave measures:

a)

the length of the wave

b)

how many times a wave passes a point in a second

c)

how many times the waves oscillates back and forth

d)

the number of molecular collisions per second

7.

Which wave has the highest frequency? (Assume they all pass by in the same time period.)

a)
b)
c)
d)
8.

Frequency of light is ___ to wavelength.

a)

directly related

b)

inversely related

c)

not at all related

9.

As the frequency of an electromagnetic wave decreases, the wavelength decreases.

a)

True

b)

False

10.

The speed of electromagnetic radiation:

a)

depends on the form of radiation

b)

is always 3 x 108 m/s, regardless of the type

c)

decreases as distance increases

d)

is 6.626 x 10-34 J x s

11.

Energy and frequency of light are _____ related.

a)

directly

b)

inversely

c)

not at all

12.

When wavelength increases...

a)

energy decreases

b)

energy increases

13.

As wavelength decreases...

a)

energy increases

b)

energy decreases

14.

1 nanometer is equal to:

a)

1 billionth of a meter

b)

10 billionths of a meter

c)

1,000 meters

d)

1 million meters

15.

Which of the following describes a wave with a large wavelength?

Select all that apply

a)

high frequency

b)

low frequency

c)

high energy

d)

low energy

16.

The frequency of violet light is 7.5x1014 Hz. What is its wavelength?

a)

4.0x10-7 m

b)

4.0x107 m

c)

2.3 x1023 m

d)

2.3 x1023 Hz

17.

Violet light has a wavelength of

4.10 x 10-12 m. What is the frequency?

a)

1.23 x 10-3 Hz

b)

7.31 x 1019 Hz

c)

1.37 x 1012 Hz

d)

3.0 x 108 Hz

18.

The frequency of light is 7.14 x 1014 Hz. What is the wavelength?

a)

3.00 x 108 m

b)

4.20 x 10-7 m

c)

2.25 x 1023 m

d)

3.90 x 10-9 m

19.

The frequency of light is 7.14 x 1014 Hz. What is the energy?

a)

4.73 x 10-19 J

b)

1.20 x 10-48 J

c)

1.13 x 10-17 J

d)

4.97 x 10-49 J

20.

What is the frequency of ultraviolet light with a wavelength of 1.24 x 10-7 m?

a)

2.42 x 1015 Hz

b)

8.22 x 10-34 Hz

c)

3.00 x 108 Hz

d)

1.04 x 1013 Hz

21.

If an AM radio station broadcasts at

9.95 x 105 Hz, what is the wavelength of this radiation?

a)

6.59 x 10-28 m

b)

1.01 x 10-6 m

c)

3.32 x 10-3 m

d)

302 m

22.

A common infrared laser operates at 1.06 x 103 nm. What if the energy of a photon with this wavelength?

a)

7.02 x 10-40 J

b)

6.25 x 10-28 J

c)

3.54 x 10-15 J

d)

1.87 x 10-19 J

23.

A beam of light has a wavelength of 600 nm in air. What is the frequency of the light?

c = 3x108 m/s

1 nm = 1 x 10-9 m

a)

5 x 1014 Hz

b)

2 x 1014 Hz

c)

3 x 1014 Hz

d)

6 x 1014 Hz

24.

Find the frequency of an electromagnetic wave with a wavelength 2.75 × 10–8 m.

a)

1.10 Hz

b)

1.09 × 1016 Hz

c)

9.17 × 1015 Hz

d)

9.17 × 1016 Hz

25.

When bombarded with light, lithium emits a light with a frequency of 4.29 x 1014 Hz. Calculate the wavelength and use the chart to predict the color.

a)

blue

b)

green

c)

yellow

d)

red

26.

Calculate the energy of light with a frequency of 5.10 x 1014 Hz.

a)

3.38 x 10-19 J

b)

5.88 x 10-7 J

c)

9.62 x 1012 J

d)

1.04 x 10-13 J

27.

What is the frequency of infrared light with a wavelength of 1.05 x 10-6 m?

a)

6.96 x 10-40 Hz

b)

2.86 x 1014 Hz

c)

9.62 x 10-13 Hz

d)

2.55 x 10-19 Hz

28.

A violet spectral line of an element has a wavelength of 4.2 x 10-7 m. What is the frequency of the violet light?

a)

3.00 x 108 Hz

b)

6.63 x 10-34 Hz

c)

7.14 x 1014 Hz

d)

1.04 x 10-13 Hz

29.

The characteristic color bands that a hot, dilute gas emits when viewed with a spectroscope are called...

a)

emission spectra

b)

absorption spectra

c)

continuous spectra

d)

black body radiation

30.

Emission of light from an atom occurs when an electron ___

a)

drops from a higher to a lower energy level

b)

jumps from a lower to a higher energy level

c)

orbits around the nucleus

d)

falls into the nucleus

31.

Which of the following correctly describes a wave with a short wavelength?

a)

high frequency

b)

high energy

c)

low frequency

d)

low energy

32.

Which drawing represents the process by which an emission line is formed?

a)
b)
c)
d)
33.

An electron in n=4 has _______ energy than an electron in n=2

a)

less

b)

more

c)

the same

34.

For an electron to change from ground state to an excited stated it must...

a)

absorb energy

b)

release energy

35.

Four gas spectra are given. What gases are in the unknown mixture?

a)

Gas B & Gas D

b)

Gas C & Gas B

c)

Gas A & Gas D

d)

Gas D & Gas C

36.

Who stipulated that electrons orbit the nucleus at fixed energies and distances?

a)

JJ Thomson

b)

John Dalton

c)

Ernest Rutherford

d)

Niels Bohr

37.

According to the Bohr Model, electrons are only found in specific orbits around the nucleus called __________________________

a)

energy levels

b)

electron lanes

c)

electron places

d)

atomic mass

38.

The lowest energy level an electron will occupy in an atom at an ordinary condition is called the ____.

a)

ground state

b)

excited state

c)

highest state

d)

minimum state

39.

When an electron absorbs enough energy, it jumps up to a higher level. This is called a(n)

a)

absorption state

b)

excited state

c)

emission state

d)

relaxation state

e)

ground state

40.

In the Bohr model, how do electrons travel?

a)

Electrons move in and out of the nucleus

b)

Electrons do not move

c)

Electrons move in circular orbits around the nucleus

d)

Electrons move in a straight line

41.

What is n defined as in the Bohr's atomic model?

a)

planetary orbit number

b)

principal quantum number

c)

principal quantum variable

d)

Bohr's number

42.

Emission spectra (bright line spectra) are created when electrons move from ___.

a)

higher to lower energy levels.

b)

lower to higher energy levels.

c)

s orbitals to p orbitals.

d)

one atom to a different atom.

43.

When an electron moves away from the nucleus, it

a)

moves to the ground state

b)

moves to an excited state

c)

gives off specific frequencies of light

d)

never returns

44.

When electrons fall from an excited state to their ground state,

a)

They absorb energy from the environment.

b)

They wobble back and forth.

c)

They emit specific frequencies of light.

d)

They spin out of orbit.

45.

The energy of a photon is directly proportional to the photon’s ........

a)

energy

b)

wavelength

c)

speed

d)

intensity

46.

What, besides light, behaves both like a particle and like a wave?

a)

an element

b)

a mole

c)

a chemical reaction

d)

an electron

47.

If an electron jumps from the n=4 level to the n=1 level, a photon of light will be ______.

a)

emitted

b)

absorbed

c)

both emitted and absorbed

d)

destroyed

48.

If an electron at n=1 _____ a photon of the right energy, it can jump outwards to n=3.

a)

emits

b)

absorbs

c)

emits and absorbs

d)

creates

49.

An electron falls from a high to low energy level. What happens?

a)

the electron lands in the nucleus

b)

the atom shrinks in size

c)

a photon of light is released

d)

a beam of radioactivity is released

50.

Emission of light from an atom occurs when an electron ___

a)

drops from a higher to a lower energy level

b)

jumps from a lower to a higher energy level

c)

orbits around the nucleus

d)

falls into the nucleus

51.

An electron cloud...

a)

represents a region of space where there is a 90% probability of finding an electron

b)
has uniform density
c)
can be called an orbital
d)
can only show where the electron is not located
52.
The Heisenberg Uncertainty Principle states
a)

velocity and position of an electron cannot be determined simultaneously

b)
a beam of light can interfere with the path and speed of an electron
c)
photons do not affect the position of an electron
d)
the velocity of a car cannot accurately be measured by a radar beam
53.

What shape are d orbitals?

a)

donut shaped

b)

spherical shaped

c)

dumbbell shaped

d)

flower shaped

54.

How many orbitals are present in a "p" sublevel?

a)

1

b)

3

c)

5

d)

7

55.

How many orbitals are present in an "f" sublevel?

a)

1

b)

3

c)

5

d)

7

56.
What is the shape of s orbitals?
a)
Dumbbell shaped
b)
Peanut shaped
c)
Spherical shaped
d)
Hybrid structure
57.

How is the modern model of the atom (aka the quantum mechanical model) different from Bohr's model of the atom?

a)

The modern model shows the probability of the electron's location.

b)

Bohr's model shows the probability of the electron's location.

c)

The modern model shows the exact location of the electron. 

d)

The modern model does not include a nucleus.

58.

Which of the following states that it is impossible to know both the position and velocity of an electron at the same time?

a)
Hund's Rule
b)
Heisenberg Uncertainty Principle
c)
Aufbau Principle
d)
Pauli Exclusion Principle
59.
Which of the following correctly describes the electron cloud model?
a)
Electrons do not follow fixed orbits, but are found more frequently in areas around the nucleus.
b)
Electrons are found in fixed orbitals around a positive nucleus.
c)
All of an atom's mass is concentrated in the electron cloud around the nucleus.
d)
Electrons are evenly embedded throughout a positively charged sphere.
60.

Which shape represents the shape of an "s" orbital?

a)
b)
c)
d)
61.

Which shape represents the shape of an "p" orbital?

a)
b)
c)
d)
62.

Bohr proposed that an electron is found only in specific circular paths, or orbits, around the nucleus.

a)

True

b)

False

63.

This shape represent which orbital?

a)

s

b)

p

c)

d

64.

These shapes represent which orbital?

a)

s

b)

p

c)

d

65.

What is the lowest energy state of an atom called?

a)

the ground state

b)

the excited state

c)

the solid state

d)

the chaotic state

66.

In the figure, why are there dots beyond the "boundary" of the atomic orbital?

a)

the boundary encloses the volume in which the electron is found 90% of the time

b)

the boundary is three-dimensional, while the picture shows only two dimensions

c)

experimental error

d)

the boundary encloses the volume in which the electron is found 50% of the time

67.

PET scans for medical imaging usually involve a small amount of radioactive decay, producing a gamma ray with a frequency of 1.24x1020 Hz. How much energy does a single photon of this radiation have?

a)

8.22 x 10-14 J

b)

5.34 x 10-54 J

c)

1.24 x 10-20 J

d)

2.42 x 10-12 J

68.

Bohr's model of the atom proposed that ______.

a)

the nucleus spins

b)

neutrons move around the nucleus

c)

electrons move around the nucleus in fixed certain orbits at certain allowed distances

d)

neutrons do not exist, but are just paired protons and electrons

69.

Energy levels in Bohr's model of an atom could be described as ...

a)

Orbits with fixed energies where an electron moves around an atom at only certain distances from the nucleus

b)

Orbits with a wide range of energies where an electron moves around an atom

c)

Orbits with fixed energies where an electron moves around an atom at any distance from the nucleus

d)

Orbits with a wide range of energies where an electron moves around an atom at any distance from the nucleus

70.

Emission of light from an atom occurs when an electron

a)

drops from a higher to a lower energy level.

b)

jumps from a lower to a higher energy level.

c)

moves along its atomic orbit

d)

is ejected from the nucleus

71.
If an electron moves from n=5 to n=2 ...
a)
it absorbs energy
b)
it releases energy
72.

Four gas spectra are given. What gases are in the unknown mixture?

a)

Gas B & Gas D

b)

Gas C & Gas B

c)

Gas A & Gas D

d)

Gas D & Gas C

73.
If an electron moves from n=2 to n=4 ...
a)
it absorbs energy
b)
it releases energy
74.

Which of the following electron transitions emits light with the SHORTEST wavelength?

a)

n = 4 to n = 3

b)

n = 4 to n = 2

c)

n = 4 to n = 1

d)

n = 3 to n = 2

75.

Heisenberg's uncertainty principle states that _____ cannot BOTH be known simultaneously.

a)

wavelength and distance

b)

position and momentum

c)

charge and displacement

d)

atomic radius and frequency

76.

The region outside the nucleus where an electron can most probably be found is called a(n) ___.

(Select all that apply)

a)

orbit

b)

orbital

c)

quantum

d)

electron configuration

77.

How many atomic orbitals make up an s-sublevel?

a)

5

b)

10

c)

2

d)

1

e)

6

78.

The quantum number "n" represents:

a)

electron spin

b)

orbital

c)

sublevel

d)

primary energy level

79.

Which of the following represents an s orbital?

a)
b)
c)
d)
80.

Which of the following represents a p orbital?

a)
b)
c)
d)
81.

How many orbitals are present in a p-sublevel?

a)

1

b)

3

c)

5

d)

7

82.

How many orbitals are there in a d-sublevel?

a)

10

b)

6

c)

3

d)

5

83.

Which of the following represents a d orbital?

a)
b)
c)
d)
84.

What is the maximum number of electrons that can occupy an orbital?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

85.

All orbitals of equal energy (degenerate orbitals) are occupied by one electron before any single orbital is occupied by a second electron.

a)

Aufbau Principle

b)

Pauli's Exclusion Principle

c)

Hund’s Rule

d)

Parity Principle

86.

Identify the rule that is being violated

a)

Aufbau Principle

b)

Hund's Rule

c)

Pauli's Exclusion Principle

d)

Heisenberg uncertainty principle

87.
What is the Pauli Exclusion Principle?
a)
An atomic orbital can only hold a maximum of 2 electrons, each with opposite spins
b)
An atomic orbital can hold a minimum of 6 electrons, each with opposite spins
c)
An atomic orbital can hold a maximum of 6 electrons, each with the same spin
d)
An atomic orbital can hold a minimum of 2 electrons, each with opposite spins
88.

No two electrons in the same atom can have the same four quantum numbers.

a)

Aufbau principle

b)

Pauli exclusion principle

c)

Hund’s rule

d)

Noble gas notation

89.

Which electron configuration shows a violation of Hund's Rule?

a)

A

b)

B

c)

C

d)

D

90.

Which electron configuration shows a violation of Pauli's Exclusion Principle?

a)

A

b)

B

c)

C

d)

D

91.

What is the maximum number of electrons that a d sublevel can hold?

a)

14

b)

10

c)

2

d)

6

92.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
93.

Identify the element for

[Xe] 6s2 4f14 5d4

a)

Cobalt

b)

Iron

c)

Tungstun

94.

What is the noble gas configuration for boron?

a)

[He]1s22s2

b)

[He]2s22p2

c)

[He]2s22p1

d)

[Li]2s22p1

95.

What is the maximum number of orbitals allowed in the 4th energy level (n=4)?

a)

4

b)

8

c)

16

d)

32

96.

Q3. If n = 3, what are the allowed values of ℓ? (Select all that apply)

a)

0

b)

1

c)

2

d)

3

e)

4

97.

The angular momentum quantum number ℓ represents:

a)

orbital color

b)

orbital shape

c)

electron spin

d)

energy level

98.

Which of the following sublevels is not allowed?

(Select all that apply)

a)

2p

b)

3d

c)

2d

d)

5f

e)

3f

99.

For ℓ = 2, select all the possible values of m:

a)

-2

b)

-1

c)

0

d)

1

e)

2

100.

The major difference(s) between a 1s orbital and a 2 s orbital is that

(select all that apply)

a)

the 2 s orbital is at a higher energy level.

b)

the 2s orbital has a slightly different shape.

c)

the 1 s orbital can have only one electron.

d)

the 2s orbital can hold more electrons.

e)

the 2s orbital has a larger average radius

101.

For a principle quantum number, "n", equal to 2, what is the total electron capacity of that level?

a)

2

b)

4

c)

8

d)

16

102.

Which of the following sets of quantum numbers are allowed?

a)

n=3, ℓ = 3, m = 1, s = -½

b)

n=5, ℓ = 4, m = -2, s = +½

c)

n=4, ℓ = 1, m = 0, s = -½

d)

n=7, ℓ = 2, m = +3, s = +½

e)

n=6, ℓ = 7, m = -2, s = +½

103.

Is this the correct Lewis dot diagram for Boron?

a)

Yes

b)

No

104.

Which of the following is the correct Lewis dot diagram for magnesium?

a)
b)
c)
d)
105.

How many electrons should sodium, atomic number 11, have around its Lewis dot model?

a)

1

b)

2

c)

3

d)

4

106.

This is the correct dot diagram for nitrogen, group 15.

a)

true

b)

false

107.

The outer most electrons are called...

a)

valence electrons

b)

heavy electrons

c)

emission electrons

d)

Excited electrons

108.

Elements in the same column of the periodic table always have the same # of _______ as one another.

a)

Protons

b)

Neutrons

c)

Electrons

d)

Valence Electrons

109.

How many valence electrons does phosphorus have?

a)

31

b)

5

c)

15

d)

4

110.

What is the shape of a d orbital?

a)
b)
c)
d)
111.

A p sublevel contains (a)   orbitals.

112.

What is the shape of an s orbital?

a)
b)
c)
d)
113.

Identify the element with the following ground state electron configuration:

1s22s22p63s2

a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

114.

Which of the following sublevels has the highest energy?

a)

2p

b)

2s

c)

3p

d)

1s

115.

Which element is represented by this ground state electron configuration?

a)

neon

b)

fluorine

c)

magnesium

d)

argon

116.

What rule states that electrons fill orbitals in order of increasing energy?

a)

Hund’s Rule

b)

Aufbau Principle

c)

Pauli Exclusion Principle

117.

An f sublevel contains (a)   orbitals.

118.

Which guideline (the Aufbau principle, Hund’s rule or the Pauli exclusion principle) is violated in the electron configuration shown here?

a)

Aufbau principle

b)

Hund's rule

c)

Pauli Exclusion Principle

119.

A d sublevel contains (a)   orbitals.

120.

What is the shape of a p orbital?

a)
b)
c)
d)
121.
What is the Pauli Exclusion Principle?
a)
An atomic orbital can only hold a maximum of 2 electrons, each with opposite spins
b)
An atomic orbital can hold a minimum of 6 electrons, each with opposite spins
c)
An atomic orbital can hold a maximum of 6 electrons, each with the same spin
d)
An atomic orbital can hold a minimum of 2 electrons, each with opposite spins
122.

Which electron configuration shows a violation of the Pauli Exclusion Principle?

a)

A

b)

B

c)

C

d)

D

123.

Which of the following electron configurations do NOT follow the Aufbau principle? (Select all that apply)

a)
b)
c)
d)
e)
124.

Which of the following is not a correct designation for a sublevel?

a)

zz

b)

p

c)

d

d)

f

125.
There are 4 different types of subshells (orbitals) s,p,d,f.
a)
true
b)
false
126.

Each orbital can hold how many electrons?

a)

5

b)

4

c)

8

d)

2

127.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
128.
How many electrons can the s sublevel hold?
a)
14
b)
10
c)
2
d)
6
129.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
130.

Write the electron configuration

a)

1s22s22p6

b)

1s12s12p3

c)

1s22s22p63s2

d)

1s22s22p63s3

131.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
132.
Electrons are paired based on their spin directions, clockwise and counterclockwise, is what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
133.

Which orbital shows a violation of Hund's Rule (bunk bed rule)?

a)

A

b)

B

c)

C

d)

D

134.

Which orbital shows a violation of the Pauli Exclusion Principle (2 electrons with opposite spins)?

a)

A

b)

B

c)

C

d)

D

135.

Which orbital shows a violation of the Aufbau Principle (lowest levels filled first)?

a)

A

b)

B

c)

C

d)

D

136.

Write the electron configuration for the element.

a)

1s12s12p33s1

b)

1s22s22p53s1

c)

1s2s2p3s

d)

1s22s22p63s1

137.

This orbital diagram represents:

a)

C (6)

b)

B (5)

c)

N (7)

d)

O (8)

138.

What is the next orbital filled after 4s?

a)

5s

b)

3d

c)

4p

d)

3p

139.

What is the next orbital filled after 4d?

a)

6p

b)

5d

c)

5p

d)

4f

140.

What is the correct electron configuration for Phosphorus (15)?

a)

1s22s22p63s23p4

b)

1s22s22p63s23d3

c)

1s22s22p63s23p3

d)

1s2s2p3s3p

141.

What is the correct electron configuration for Titanium (22)?

a)

1s22s22p63s23p4

b)

1s22s22p63s23p64s23d2

c)

1s22s22p63s23p64s24p2

d)

1s22s22p63s23p64s24d2

142.
Which is associated with more energy? 
a)
2p
b)
2s
c)
3p
d)
1s
143.

What is the maximum number of electrons that can occupy a p sublevel?

(a)  

144.

What is the maximum number of orbitals allowed in the 6th energy level (n=6)?

a)

9

b)

16

c)

26

d)

36

e)

72

145.
According to the Aufbau Principle, which sublevel should starting filling with electrons after 5s?
a)
6s
b)
5p
c)
4d
d)
3f
146.
Identify the following element:
1s22s22p63s23p64s23d10
a)
nickel
b)
copper
c)
zinc
d)
gallium
147.
Identify the element whose electron configurations ends with 5p3
a)
As
b)
Te
c)
Sb
d)
Sn
148.

Which of the following statements is true about the 3s and the 4s sublevels?

(Select all that apply)

a)
These sublevels have the same energy
b)
These sublevels are the same distance from the nucleus
c)
These sublevels hold different amounts of electrons
d)
These sublevels have the same shape
e)

The 4s orbital has more energy than the 3s orbital

149.

Which of the following sets of quantum number is NOT allowed?

a)

{ n=3, l=2, m=+1, s=-1/2 }

b)

{ n=5, l=3, -m=1, s=+1/2 }

c)

{ n=12, l=1, m=+2, s=+1/2 }

d)

{ n=7, l=6, m=-5, s=-1/2 }

150.

Which of the following states that each electron in an atom can be described by a unique set of quantum numbers?

a)
Hund's Rule
b)
Heisenberg Uncertainty Principle
c)
Aufbau Principle
d)
Pauli Exclusion Principle
151.
According to the Aufbau Principle, which sublevel should starting filling with electrons before the 3p sublevel?
a)
3s
b)
2p
c)
4s
d)
4p
152.
How many valence electrons are in an atom of sulfur?
a)
2
b)
4
c)
6
d)
8
153.

How many unpaired electrons are in an atom of strontium?

a)
0
b)
1
c)
2
d)
3
154.

How many unpaired electrons are in an atom of germanium?

(Hint: write an electron configuration)

a)
2
b)
3
c)
4
d)
5
155.

This element is in the period three. It has one unpaired electron in its highest occupied sublevel and it has 3 valence electrons. What is the identity of this element

(a)  

156.

This element is in period 5 of the periodic table. It has 2 valence electrons and 2 unpaired electrons. Its average atomic mass is greater than 100 amu.

Identify this element.

a)
Sr
b)
Zr
c)
Pd
d)
Sn
157.

What atom matches this electron configuration?

1s22s22p63s23p64s23d3

a)

Vanadium

b)

Copper

c)

Nickel

d)

Germanium

158.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
159.

Each element on the periodic table can be identified by its

a)

classification as a solid, liquid or gas.

b)

location on the table.

c)

ability to react to form compounds.

d)

unique spectral "fingerprint."

160.

When an electron returns to ground state from an excited state, the atom will

a)

emit energy

b)

absorb energy

c)

rotate

d)

wiggle

161.

The line emission spectrum shown below happens when...

a)

an electron transitions from lower to higher energy level.

b)

an electron transitions from higher to lower energy level.

c)

an electron travels in a fixed circular orbit

162.
Which elements are in the unknown sample?
a)

A

b)

B

c)

C

d)

D

163.

Which element(s) is/are found in the star's spectra below? (Select all that apply)

a)

Hydrogen

b)

Helium

c)

Calcium

164.

The figure shows different possible transitions of electrons as they move from higher energy states to lower energy states. Which transition will produce the spectrum line with the LOWEST wavelength in this element's atomic spectrum?

a)

E

b)

F

c)

B

d)

A

165.

Oxygen is perhaps the most important atom on Earth. Which of the following electronic transitions in the oxygen atom will result in light emission?

a)

n=1→n=2n=1\rightarrow n=2  

b)

n=1→n=3n=1\rightarrow n=3  

c)

n=3→n=2n=3\rightarrow n=2  

d)

n=2→n=3n=2\rightarrow n=3  

166.

What is the frequency for a sodium lamp that has a wavelength of 598 nm?

(1 nm = 10-9 m)

a)

5.01 x 1014 Hz5.01\ x\ 10^{14}\ Hz  

b)

179 Hz

c)

1.99 x 10−15 Hz1.99\ x\ 10^{-15}\ Hz  

d)

5.01 x 105 Hz5.01\ x\ 10^{5\ }Hz  

167.

Blue light has a wavelength of 400. nm. What is the frequency of this radiation? What is the energy of this radiation?

a)

 7.5 x 1014 Hz and 7.5 x 105 J\ 7.5\ x\ 10^{14}\ Hz\ and\ 7.5\ x\ 10^5\ J  

b)

7.5 x 105 Hz and   1.13 x 1048 J7.5\ x\ 10^5\ Hz\ and\ \ \ 1.13\ x\ 10^{48}\ J  

c)

7.5 x 1014 Hz and 4.97 x 10−19 J7.5\ x\ 10^{14\ }Hz\ and\ 4.97\ x\ 10^{-19}\ J  

d)

120 Hz and 2.65 x 10−40 J120\ Hz\ and\ 2.65\ x\ 10^{-40}\ J  

168.
Emission of light from an atom occurs when an electron
a)
drops from a higher to a lower energy level.
b)
   jumps from a lower to a higher energy level.   
c)
   moves within its atomic orbital.
d)
falls into the nucleus.
169.

The picture shows an atom in the ground state absorbing energy and the electron jumps to the excited state. Which state has higher energy?

a)

Ground State

b)

Excited State

170.

How many valence electrons are represented in this depiction of an atom?

(a)  

171.

How many d orbitals are present in a d sublevel?

(a)  

172.

How many p orbitals are present in a p sublevel?

(a)  

173.

What is incorrect about this electron configuration?

a)

Both arrows in the 2p sublevel should be pointing up

b)

There is nothing incorrect with this diagram

c)

In the 2p sublevel there should only be 1 electron in the first 2p box and one in the 2nd 2p box, with the same spin as the arrow in the first box

d)

All the arrows should be pointing up.

e)

In the 2p sublevel there should only be 1 electron in the first 2p box and one in the 2nd 2p box, with the opposite spin to the arrow in the first box

174.

Which electron configuration shows a violation of the Pauli Exclusion Principle?

a)
b)
c)
d)
175.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

176.

How many valence electrons should an atom of lithium have in its Lewis dot diagram?

a)

1

b)

2

c)

3

d)

4

177.

How many valence electrons should an atom of oxygen have in its Lewis dot diagram?

a)

5

b)

6

c)

7

d)

8

178.

How many valence electrons should an atom of magnesium have in its Lewis dot diagram?

a)

1

b)

2

c)

3

d)

4

179.

This is a correct Lewis dot diagram for nitrogen (N)

a)

true

b)

false

180.

This is a correct Lewis dot diagram for carbon (C)

a)

true

b)

false

181.

This is a correct Lewis dot diagram for neon (Ne)

a)

true

b)

false

182.

How many electrons should an atom of boron have in its Lewis dot diagram?

a)

1

b)

2

c)

3

d)

4

183.

How many valence electrons does an atom of chlorine (Cl) have?

(a)  

184.

How many valence electrons does carbon (C) have?

(a)  

185.
Which of these elements has 8 valence electrons?
a)
P
b)
Be
c)
O
d)
Ar
186.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
187.

How many orbitals are available to hold electrons in the 6th energy level (n=6)?

a)

9

b)

16

c)

26

d)

36

188.

If n = 2, what is the maximum number of electrons allowed in that energy level?

a)
2
b)
4
c)
8
d)
16
189.

How many valence electrons are in an atom of sulfur?

(a)  

190.

How many unpaired electrons are in an atom of strontium?

(Hint: draw an electron configuration using arrows and boxes)

a)
0
b)
1
c)
2
d)
3
191.

What is the maximum number of electrons allowed in the 4th energy level (n=4)?

a)

4

b)

8

c)

16

d)

32

192.

How many valence electrons does an atom of aluminum have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

193.

Elements in the same column of the periodic table always have the same number of _______ as one another.

a)

protons

b)

neutrons

c)

occupied energy levels

d)

valence electrons

194.
How many valence electrons are found in atoms of group 14?
a)
4
b)
3
c)
14
d)
16
195.
Which group has the greatest number of valence electrons?
a)
1
b)
14
c)
18
d)
16
196.

This could be the Lewis dot diagram of

a)

P

b)

Ar

c)

Na

d)

B

197.

The elements in this group all have 5 valance electrons.

a)

Group 5

b)

Group 15

c)

Group 3

d)

Group 18

198.

How many valence electrons are present in an atom of Na?

(a)  

199.

How many valance electrons does iodine have?

a)

6

b)

16

c)

7

d)

17

200.

The outermost electrons in an atom are referred to as ___.

a)

valence electrons

b)

inner electrons

c)

emission electrons

d)

excited electrons

e)

core electrons

201.

This could be the Lewis dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

202.

This could be the Lewis dot diagram of

a)

Ne

b)

Si

c)

Al

d)

Be

203.

For a principle quantum number, "n", equal to 7, what is the maximum number of electrons that can occupy that energy level?

(a)  

204.

Is the 5p orbital permitted?

a)

Yes

b)

No

205.

For a p sublevel, "ℓ" equals ____.

a)

0

b)

1

c)

2

d)

3

206.

What is the correct designation for an orbital which has an n=4 and ℓ= 2?

a)

4s

b)

4d

c)

4p

d)

4f

207.

For a principle quantum number, "n", equal to 6, is it possible for "ℓ" to be equal to 7?

a)

Yes

b)

No

208.

What is the correct designation for an orbital which has an "n" value of 3 and an "ℓ" value of 1?

a)

3p

b)

3s

c)

3d

d)

3f

209.

How many sublevels are at the 3rd energy level?

a)

1

b)

3

c)

4

d)

8

210.

What is the maximum number of electrons that could be at the 2nd energy level?

a)

1

b)

2

c)

8

d)

16

211.

If quantum number "n" = 3, what are the possible values for "ℓ"?

a)

0, 1, 2, 3, 4...

b)

-1, -2, -3

c)

0, 1, 2

d)

1, 2

212.

What information does "ℓ" provide about an orbital?

a)

the shape of the orbital

b)

the energy level of the orbital

c)

the size of the orbital

d)

the number of orbitals in a sublevel

213.

In the Bohr model, how do electrons travel?

a)

Electrons move in and out of the nucleus

b)

Electrons do not move

c)

Electrons move in circular orbits around the nucleus

d)

Electrons move in a straight line

214.

The principal quantum number, n, defines

a)

energy level or shell of the electron

b)

probable distance of the electrons from the nucleus

c)

Shape of orbital

d)

Both energy level or shell of the electron and probable distance of the electrons from the nucleus

215.

The magnetic quantum number m determines

a)

number of orbitals

b)

their orientation within a subshell

c)

Both number of orbitals and their orientation within a subshell

d)

the energy of an orbital

216.

What is the selection rule for the magnetic quantum number, m ?

a)

n-1

b)

0 to +l

c)

-l ..... 0 ..... +l

d)

any integer from 1 to infinity

217.

The energy levels in an atom are equally spaced.

a)

True

b)

False

218.

Contains 7 orbitals with a maximum capacity of 14electrons

a)

s sublevel

b)

d sublevel

c)

f sublevel

219.

The principal quantum number always equals the number of sublevels within that principal energy level.

a)

True

b)

False

220.

How many orbitals are in the third principal energy level?

a)

3

b)

6

c)

9

d)

2

221.

Which of the following is an allowed excited state for an atom?

a)

He: 1s2

b)

H: 1d1

c)

1Na:1s2 2s2 2p6 3d1

d)

Ne: 1s2 2s2 2p5 3s1

e)

He: 1s1 2f1

222.

What types of orbitals are found in the principal energy level n = 5?

a)

s orbital

b)

s,p orbital

c)

s,p,d orbitals

d)

s, p, d, and f orbitals

223.

For a neutral atom with the electron configuration of 1s2 2s2 2p5 3s1 which statement is false?

a)

the atomic number is ten

b)

the 1s and 2s orbitals are filled

c)

the atom is in the ground state

d)

the atom is in the excited state

224.

Which orbital designation has the highest energy?

a)

2s

b)

2p

c)

3d

d)

4s

225.

Which of the following electron transitions emits light with the LONGEST wavelength?

a)

n = 4 to n = 3

b)

n = 4 to n = 2

c)

n = 4 to n = 1

d)

n = 3 to n = 2

226.

What is the maximum number of electrons allowed in the 6th energy level (n=6)?

a)

9

b)

16

c)

26

d)

36

e)

72

227.

For an s sublevel, "ℓ" equals ____.

a)

0

b)

1

c)

2

d)

3

228.

For a d sublevel, "ℓ" equals ____.

a)

0

b)

1

c)

2

d)

3

229.

For an f sublevel, "ℓ" equals ____.

a)

0

b)

1

c)

2

d)

3

230.

What is the selection rule for the angular magnetic quantum number, ℓ ?

a)

0, ..., n-1

b)

0 to n

c)

-l ..... 0 ..... +l

d)

any integer from 1 to infinity

231.

If n = 3, can ℓ = 3?

a)

yes

b)

no

232.

If n = 6, can ℓ = 3?

a)

yes

b)

no

233.

What information does "m" provide about an orbital?

a)

the shape of the orbital

b)

the energy level of the orbital

c)

the size of the orbital

d)

the number of orbitals in a sublevel

234.

What information does "n" provide about an orbital?

a)

the shape of the orbital

b)

the energy level of the orbital

c)

the size of the orbital

d)

the number of orbitals in a sublevel

235.

If ℓ = 6, can m= 3?

a)

yes

b)

no

236.

If ℓ = 2, can m= 3?

a)

yes

b)

no

237.

If ℓ = 4, can m= -2?

a)

yes

b)

no

238.

Is a 3f orbital allowed?

a)

yes

b)

no

239.

Is a 8f orbital allowed?

a)

yes

b)

no

240.

What rule is not being followed in the electron configuration shown here?

a)

Pauli Exclusion Principle

b)

Hund's rule

c)

Aufbau principle

d)

There are no errors in this electron configuration

241.

What rule is not being followed in the electron configuration shown here?

a)

Pauli Exclusion Principle

b)

Hund's rule

c)

Aufbau principle

d)

There are no errors in this electron configuration

242.

What rule is not being followed in the electron configuration shown here?

a)

Pauli Exclusion Principle

b)

Hund's rule

c)

Aufbau principle

d)

There are no errors in this electron configuration

243.

What is the ground state electron configuration for a neutral atom of beryllium, using noble gas notation?

a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
244.

What is the ground state electron configuration for a neutral atom of cobalt, using noble gas notation?

a)

[Kr] 4s2 3d7

b)

[Kr] 4s2 4d7

c)

[Ar] 4s2 3d7

d)

[Ar] 4s2 4d7

245.
[He]2s22p4 is the noble gas configuration for which element?
a)
oxygen
b)
sulfur
c)
phosphorus
d)
fluorine
246.

Using noble-gas notation, calcium is represented by [Ar]4s2. How many electrons does calcium have?

a)

18

b)

20

c)

22

d)

24

247.

What is the correct noble-gas notation for the electron configuration for a ground state neutral atom of chlorine? 

a)

[Ar]3s2 3p5

b)

[Ne]3s2 3p4

c)

[Ar]3s2 3p4

d)

[Ne]3s2 3p5

248.

Which element is represented by this orbital notation?

a)

carbon

b)

nitrogen

c)

oxygen

d)

fluorine

249.

What is the ground state electron configuration for a neutral atom of sulfur, using noble gas notation?

a)

[Ar] 3p4

b)

[Ne] 3p4

c)

[Ne] 3s23p4

d)

[He] 3s23p4

250.

Which element below matches this noble gas configuration? [Kr] 5s2 4d2

a)

titanium

b)

calcium

c)

zirconium

d)

hafnium

251.

What is the ground state electron configuration for a neutral atom of osmium, using noble gas notation?

a)

[Xe] 6s2 5d6

b)

[Xe] 6s2 4f14 5d6

c)

[Rn] 6d6

d)

[Kr] 5s2 4d6

252.

What is the ground state electron configuration for a neutral atom of bromine, using noble gas notation?

a)
[Ar] 4s2 3d10 4p5
b)
[Kr] 3s2 3p5
c)
[Ne] 3s2 3p5
253.

What is the ground state electron configuration for a neutral atom of strontium, using noble gas notation?

a)
[Ar] 3s2 3p6 4s2 
b)
[Xe] 3s2 3p6 4s2 
c)
[Kr] 5s2 
254.

What is the ground state electron configuration for a neutral atom of tin, using noble gas notation?

a)
[Kr] 5s2 4d10 5p1
b)
[Kr] 5s2 4d10 5p2
c)
[Kr] 5s2 4d10 5p3
255.

Match the following rules for electron configurations with their descriptions

a)

Aufbau principle

1.

sublevels must be filled in order of increasing energy

b)

Hund's rule

2.

for p, d and f sublevels, put 1 e- in each orbital spin aligned before pairing any e-

c)

Pauli exclusion principle

3.

two electrons may share an orbital, but they must have opposite spins

256.

Match the following orbitals with their shapes

a)
1.

s orbital

b)
2.

p orbital

c)
3.

d orbital

d)
4.

f orbital

257.

An s sublevel contains ​ ​​ (a)   orbital. A p sublevel contains ​ (b)   orbitals. A d sublevel contains ​ (c)   orbitals. An f sublevel contains ​ (d)   orbitals.

Choose from the below words
1
3
5
7
2
6
10
14
258.

An s sublevel can hold a maximum of ​ ​​ 2 electrons. A p sublevel can hold a maximum of ​ (a)   electrons. A d sublevel can hold a maximum of ​ ​ (b)   electrons. An f sublevel can hold a maximum of ​ ​ (c)   electrons.

Choose from the below words
6
10
14
2
1
3
5
7