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Bohr models, electron configurations, and periodic trends

Total questions: 139

Worksheet time: 7hrs 29mins

Name
Class
Date
1.

Select the two statements that are TRUE:

a)

Electrons release energy when they move to a higher energy state

b)

Electrons release energy when they move to a lower energy state

c)

Electrons absorb energy when they move to a higher energy state

d)

Electrons absorb energy when they move to a lower energy state

2.

Compare the energy released when an electron moves down 6 energy levels vs. 4 levels.

a)

More energy is released when it moves down 4 levels

b)

Less energy is released when it moves down 4 levels

c)

The same amount of energy is release if the electron started in the same level

d)

The same amount of energy is release if the electron ended in the same level

3.

During a flame test, ions of a specific metal are heated in a flame. A characteristic color of light is emitted by these ions in the flame when the electrons _______________.

a)

Gain energy as they return to their ground state

b)

Gain energy as they move to their excited state

c)

Emit energy as they return to their ground state

d)

Emit energy as they move to their excited state

4.

If a light wave has a frequency of 2.0 hz, what is the wavelength?

a)

1.3 x 10^-33 hz

b)

1.5 x 10^8 hz

c)

6.0 x 10^8 hz

d)

7.0 x 10^-9 hz

5.

How much energy is in a photon with a frequency of 3.0 hz?

a)

2.0 x 10^-33 J

b)

2.2 x 10^-34 J

c)

4.5 x 10^-33 J

d)

9.0 x 10^8 J

6.

How much energy is in a photon with a wavelength of 0.50 m?

a)

6.0 x 10^8 J

b)

1.5 x 10^8 J

c)

4.0 x 10^-25 J

d)

9.9 x 10^-26 J

7.

In the Bohr model of the atom, in which orbit is an electron in its lowest energy state?

a)

in the orbit closest to the nucleus

b)

in the orbit farthest from the nucleus

c)

in the electron cloud

d)

midway between two orbits

8.

All of the elements in a period (row) have the same number of (a)   .

Choose from the below words
protons
energy levels
valence electrons
electrons
9.

All of the elements in a group (column) have the same number of (a)   . (except He)

Choose from the below words

electrons

protons

energy levels

valence electrons
10.

What is the Bohr Model of Carbon in the ground state?

a)

6 protons, 6 neutrons, 6 electrons with 2 in the first shell and 4 in the second shell

b)

6 protons, 6 neutrons, 6 electrons with 4 in the first shell and 2 in the second shell

c)

6 protons, 6 neutrons, 6 electrons with 3 in the first shell and 3 in the second shell

d)

6 protons, 6 neutrons, 6 electrons with 1 in the first shell and 5 in the second shell

11.

The lowest energy state of an atom is called its:

a)

ground state

b)

ionized state

c)

initial energy state

d)

final energy state

12.

Which of the transitions below for a hydrogen

atom involves the least energy?

a)

𝑛= 5 𝑡𝑜 𝑛 = 3

b)

𝑛 = 5 𝑡𝑜 𝑛 = 4

c)

𝑛 = 2 𝑡𝑜 𝑛 = 5

d)

𝑛I= 4 𝑡𝑜 𝑛 = 7

13.

A photon has a frequency of 4,3 x 1014 Hz, the energy of this photon is ___________ _J and the wavelength is ______nm

a)

2.8 x 10-19 and 7 x 10-7

b)

2.8 and 700

c)

2.8 x 10-19 and 700

d)

2.8 and 7

14.

A photon has a frequency of 4.3 x 1014 Hz, the energy of this photon is ___________ _J and the wavelength is ______m

a)

2.8 x 10-19 and 7 x 10-7

b)

2.8 and 700

c)

2.8 x 10-19 and 700

d)

2.8 and 7

15.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
16.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
17.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
18.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
19.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
20.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
21.
What do you start electron configuration with?
a)
1s2
b)
1d10
c)
1f14
d)
1p6
22.
What is this element?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
23.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
24.
There are 4 different types of subshells s,p,d,f
a)
true
b)
false
25.
Which electron configuration belongs to Copper (Cu)?
a)
1s2 2s2 2p6 3s2 3p6 4s2 3d8
b)
1s2 2s2 2p6 3s2 3p6 4s2 3d9
c)
1s2 2s2 2p6 3s2 3p6 4s2 3d10
26.
Identify the Electron Configuration for Aluminum (Al)
a)
1s2 2s2 2p6 3s2 3p1
b)
1s2 2s2 2p6 3s2 3p3
c)
1s2 2s2 2p6 3s2 4p1
27.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
28.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
29.

How many electrons can the d sublevel (the d orbitals) hold?

a)

14

b)

10

c)

2

d)

6

30.

Choose the correct shortcut configuration for iodine.

a)

[Ar]4s24d104p5

b)

[Kr]5s24d105p5

c)

[Xe]5s25d105p5

d)

none of the above

31.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

32.

Which area on the periodic table represents the electrons in the "d" sublevel (d orbitals)?

a)

representative elements

b)

columns 3-8

c)

rare earth elements

d)

transition elements

33.

Which periodic table family below has their last, most energetic electron in their electron configuration in the s-block?

a)

Alkaline Earth

b)

Halogens

c)

Noble Gases

d)

Transition Metals

34.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
35.

Each orbital can hold how many electrons?

a)

5

b)

4

c)

8

d)

2

36.
How many half-filled orbitals would silicon contain?
a)
0
b)
2
c)
1
d)
3
37.

What is incorrect about this orbital diagram?

a)

Both arrows in the 2p box should be pointing up

b)

There is nothing incorrect with this diagram

c)

In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box pointing in the same direction.

d)

All the arrows should be pointing up.

38.

In an electron configuration, what follows 4s?

a)

4p

b)

3d

c)

4s

d)

2f

39.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
40.
What is the noble gas configuration for beryllium?
a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
41.
What is the abbreviated electron configuration for barium?
a)
[Xe] 6s2
b)
[Rn] 6s2
c)
[Ar] 4s2 3d10 4p5
d)
[He] 2s2 3p1
42.
What is the noble gas configuration for Neon?
a)
[Ne]
b)
[He]2s22p6
c)
[F]2p1
d)
[Ne]2s21p6
43.

Choose the Noble Gas that you would use to begin the shorthand configuration of the following element.

Iron

a)

[He]

b)

[Ne]

c)

[Ar]

d)

[Kr]

44.

Choose the Noble Gas that you would use to begin the shorthand configuration of the following element.

Plutonium (Pu)

a)

[Xe]

b)

[Ne]

c)

[Rn]

d)

[Kr]

45.

What is the shorthand configuration for Tin?

a)

[Xe]5s24d105p2

b)

[Xe]5s24d105p2

c)

[Kr]5p2

d)

[Kr]5s24d105p2

46.

What is the shorthand configuration for Lead?

a)

[Xe]6s24f145d106p2

b)

[Xe]6s25d106p2

c)

[Rn]6s25d106p2

d)

[Rn]6s24f145d106p2

47.

A substance with characteristics of metals and nonmetals.

a)

metalloid

b)

element

c)

compound

d)

atom

48.

What orbital is shown in the picture?

a)

s orbital

b)

p orbital

c)

d orbital

d)

f orbital

49.

Which quantum number represents the shape of the orbital?

a)

principal energy (n)

b)

angular momentum (l)

c)

magnetic (m)

d)

spin

50.

Which quantum number represents the orientation of the orbital?

a)

principal quantum number

b)

azimuthal (angular momentum) quantum number

c)

magnetic quantum number

d)

spin quantum number

51.

When atoms _____________ energy, their electrons move to higher energy levels. These electrons _____________ energy by emitting light when they return to lower energy levels.

a)

lose, absorb

b)

absorb, lose

c)

lose, lose

d)

absorb, absorb

52.

Which form of radiation has the highest frequency?

a)

radio waves

b)

ultraviolet

c)

x-ray

d)

gamma

53.
An electron cloud
a)
represents a 50% 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
54.
The quantum numbers describe all the characteristics of an electron except
a)
orbital shape
b)
velocity 
c)
energy level
d)
magnetic spin
55.
The n quantum number gives information about
a)
Size and Energy of the energy level
b)
orientation of the orbital
c)
spin of the electron
d)
shape of the orbital
56.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
57.
How many electrons can the f sublevel hold?
a)
14
b)
10
c)
6
d)
4
58.
Which main energy level is furthest from the nucleus ?
a)
1
b)
2
c)
3
59.

Put the visible light colors in order from lowest energy to highest energy

a)
Violet, Blue, Green, Orange, Yellow, Red
b)
Red, Yellow, Green, Orange, Violet, Blue
c)
Red, Orange, Yellow, Green, Blue, Violet
d)
Blue, Violet, Green, Yellow, Orange, Red
60.

Each element produces its own pattern of emission spectra lines because each element has its own distinct

a)

Speed of light

b)

Electron configuration

c)

Number of neutrons

d)

None of these

61.

If an electron moves from n=4 to n=2 it ____

a)

absorbs energy

b)

emit energy

62.

Which of the following states that electrons occupy orbitals of lowest energy first?

a)

Hund’s Rule

b)

Aufbau Principle

c)

Pauli Exclusion Principle

63.

What does the Pauli Exclusion Principle state?

a)

An orbital can only hold a maximum of 2 electrons, each with opposite spins

b)

An orbital can hold a minimum of 6 electrons, each with opposite spins

c)

An orbital can hold a maximum of 6 electrons, each with the same spin

d)

An orbital can hold a maximum of 2 electrons, each with the same spin

64.

Which of the following is NOT a possible pair of quantum numbers?

a)

2p

b)

2d

c)

4p

d)

4f

65.

What does the 1 in "1s" stand for?

a)

energy level

b)

s orbitals

c)

p orbitals

d)

the number of electrons

66.

What element has the electron configuration 1s2 2s2 2p6 3s2 3p5?

a)

Chlorine

b)

Argon

c)

Fluorine

d)

Sulfur

e)

Bromine

67.

How many electrons are in 1s2 2s2 2p4?

a)

5

b)

6

c)

8

d)

13

68.

What is the noble gas configuration for Cobalt?

a)

[Kr] 4s2 3d7

b)

[Kr] 4s2 4d7

c)

[Ar] 4s2 3d7

d)

[Ar] 4s2 4d7

69.

What is the noble gas configuration for 1s2 2s2 2p6 3s2?

a)

[He] 3s2

b)

[Ne] 3s2

c)

[Ar] 3s2

d)

[Ar] 4s2

70.

Which of the following will have similar properties to 1s2 2s2 2p6 3s2 3p2?

a)

carbon

b)

calcium

c)

chlorine

d)

cesium

71.
Question Image

Match the parts of the electron configuration to what it represents.

a)

1

1.

Energy Level

b)

s

2.

Orbital

c)

2

3.

Electrons

72.

Finish the electron configuration for chlorine:

1s2 2s2 (a)   3s2 3p6

73.

Match the group to the configuration that it ends with.

a)

s1

1.

alkali metals

b)

s2

2.

alkaline earth metals

c)

p5

3.

halogens

d)

p6

4.

noble gases

74.

How many electrons can the second energy level hold?

a)

18

b)
2
c)
8
d)

6

75.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
76.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the there should only be 1 orbital in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
77.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
78.
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
79.
All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Core Notation
80.
An electron occupies the lowest energy orbital that can receive it.
a)
Hund’s rule
b)
Pauli exclusion principle
c)
Bohr model of the atom
d)
Aufbau principle
81.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Hund's
b)
Aufbau's
c)
Pauli's Exclusive
82.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Aufbau's
b)
Hund's
c)
Pauli exclusive
83.
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
84.

Which shows the correct orbital diagram for Cobalt?

a)
b)
c)
d)
85.

This shape is that of a/n:

a)

s orbital

b)

p orbital

c)

d orbital

d)

f orbital

86.
How many electrons can the p sublevel hold?
a)
14
b)
10
c)
2
d)
6
87.

Which element is the least reactive?

a)

Li

b)

Ne

c)

B

d)

C

88.
Elements which are shiny, conduct electricity and heat are called
a)

metal

b)

nonmetal

c)

metalloid

d)

nonexistent

89.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
90.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
91.
The groups of the period table tell us:
a)
Number of electron shells
b)
Number or electrons
c)
Number of protons
d)
Number of valence electrons
92.

What is the name of group number 1?

a)

halogens

b)

noble gases

c)

alkali metals

d)

alkaline earth metals

93.

What is the name of group number 2?

a)

transition metals

b)

halogens

c)

metaloids

d)

alkaline earth metals

94.

where are the metaloids found

a)

far left, vertical

b)

stair step/diagonal

c)

far right horizontal

d)

at the bottom

95.

What group number are the halogens found?

a)

18 (8A)

b)

1

c)

2

d)

17 (7A)

96.

Periodic law states that the elements are arranged according to their atomic ________ so that elements with similar chemical properties are in the same ________ and properties repeat periodically.

a)

numbers, rows

b)

masses, rows

c)

masses, column

d)

numbers, column

97.

A row on the Periodic Table of Elements

a)

family

b)

period

c)

row

d)

isotope

98.

Which element has similar chemical properties as sodium but has 7 energy levels?

a)

Francium (Fr)

b)

Cesium (Cs)

c)

Rubidium (Rb)

d)

Potassium (K)

99.

Elements that have the same number of energy levels are said to be in the same ______.

a)

group

b)

period

c)

family

d)

classification

100.

Which of the following groups would be the most REACTIVE METALS?

a)

b)

c)

d)

101.

Which has the greater Electronegativity: 
Cl or Al?

a)
Cl
b)
Al
102.

Which has the greater Electronegativity: 
N or C?

a)
C
b)
N
103.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
104.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
105.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
106.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
107.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
108.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
109.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)

the number of protons and electrons increases, so attraction to electrons increases

b)
the number of energy levels increases
c)

just the number of electrons increases

d)
the atomic mass increases
110.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
111.

Put in order from biggest to smallest (decreasing atomic radius)

a)

Calcium

b)

Iron

c)

Zinc

d)

Bromine

e)

Krypton

1)
2)
3)
4)
5)
112.

Which of these is a distinguishing property for the noble gases?

a)

Soft - can cut with a plastic knife

b)

Unreactive - don't give or receive electrons

c)

Shiny - exhibits luster

d)

Poor conductors of electricity

113.

An unknown element is observed to be shiny, malleable, ductile, and is found to conduct heat and electricity very well. What group might this element fall into?

a)

Alkali metals

b)

Alkali earth metals

c)

Transition metals

d)

Non-metals

114.

Which of these are not good conductors of heat & electricity?

a)

metalloids

b)

alkali earth metals

c)

transition metals

d)

non-metals

115.

The shaded elements here are known as the...

a)

Noble Gases

b)

Halogens

c)

Non-Metals

d)

Transition Metals

116.

The elements in the d-block of the periodic table are known as...

a)

Alkali metals

b)

Transition metals

c)

Noble gases

d)

non-metals

117.

Most of the elements on the periodic table are...

a)

Metals

b)

Non-metals

118.

As you look down a group, ionization energy and electronegativity

a)

increases

b)

decreases

119.

As you look from left to right across a period, ionization energy and electronegativity both

a)

increase

b)

decrease

120.

Which element has the greater ionization energy?

a)

Magnesium (Mg)

b)

Phosphorus (P)

121.

Which element has the greater ionization energy?

a)

Iodine (I)

b)

Chlorine (Cl)

122.
List the following in order of weakest to strongest ionization energy.
P, Cs, Co, Sr
a)
P, Co, Sr, Cs
b)
Cs, Sr, Co, P
c)
Sr, Cs, Co, P
d)
P, Co, Cs, Sr
123.

What color of the rainbow has the longest wavelength?

a)

red

b)

blue

c)

green

d)

violet

124.

Pick the sentence that best describes the relationship between wavelength and energy of light.

a)

As the wavelength gets longer the energy of light increases.

b)

As the wavelength gets shorter the energy of light increases.

c)

A photon with a long wavelength will have high energy.

d)

These are not related.

125.

The colors emitted by an element (Emission spectra) are

a)

Unique to that type of element

b)

The same for every element

c)

Depends on the amount of energy in the element

d)

Elements do not emit colors

126.

An electron that jumps multiple orbitals compared to an electron that jumps only one will release

a)

a shorter wavelength of color

b)

a longer wavelength of color

c)

no wavelengths of color

d)

all the wavelengths of color

127.

True or False: The ground state is the highest energy state of an atom.

a)

True

b)

False

128.

Diagram below shows

a)

Continuous spectrum

b)

Absorption spectrum

c)

Emission Line spectrum

d)

Absorption Line spectrum

129.

A particle of light is called a...

a)

Photoelectron

b)

Photon

c)

Proton

d)

Electron

130.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

131.
Which light equation would be used to calculate the energy of light that has a frequency of
a)
a.
b)
b.
c)
c.
d)
d.
132.
The waves with the largest wavelengths are which type of waves?
a)
Gamma rays
b)
Visible light
c)
Radio waves
d)
X-rays
133.
The theory of wave-particle duality states that all matter has properties of
a)
neither a particle nor a wave.
b)
both a particle and a wave.
c)
just a wave and not a particle.
d)
just a particle and not a wave.
134.

Which wave has a higher frequency?

a)

A

b)

B

135.

A certain photon of light has a wavelength of 4.22x10-7nm. What is the frequency?

a)

7.11x1014 Hz

b)

7.11Hz

c)

1.41x10-15 Hz

d)

-1.41x1015 Hz

136.
What does the letter 'h' represent in the formula E = hv?
a)
Planck's constant
b)
Hydrogen
c)
Energy
137.

What is the energy of a quantum of light with a frequency of 7.39x1014Hz.(E=Hv)

a)

4.88x1019 J

b)

4.88x10-19 J

c)

2.22x1023 J

d)

2.22x10-23 J

138.

What is the wavelength for a quantum of light with energy of 7.56x10-19J?

a)

2.62x10-7m

b)

2.62x107m

c)

2.64x10-45m

d)

2.64x1045m

139.

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

a)

frequency

b)

wave speed

c)

amplitude

d)

wavelength

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