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Worksheets

Quantum model & Periodicity

Total questions: 152

Worksheet time: 7hrs 33mins

Name
Class
Date
1.
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
2.
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
3.
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
4.
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
5.
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
6.
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
7.
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
8.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
9.
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
d)
All the arrows should be pointing up.
10.
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
11.
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
12.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
13.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
14.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
15.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
16.
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
d)
All the arrows should be pointing up.
17.
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
18.
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
19.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
20.
Which orbital shows a violation of the Aufbau Principle?
a)
A
b)
B
c)
C
d)
D
21.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
22.
Which element is depicted from this atomic orbital diagram?
a)
Carbon
b)
Nitrogen
c)
Oxygen
d)
Phosphorus
23.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
24.
An orbital can at most hold how many electrons?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
25.

Which of the following statements regarding electronic orbitals is/are correct?

a)

Each p-orbital can hold a maximum of six electrons.

b)

The 3p-orbitals have a higher energy level than the 3s-orbital.

c)

The three 3p-orbitals have slightly different energy levels.

d)

The 1s-orbital has the same size and shape as the 2s-orbital.

26.

What is the Aufbau principle?

a)

Within an energy level, s orbitals are the lowest energy, followed by p, d and then f. F orbitals are the highest energy for that level.

b)

The lower the principal quantum number (n) the lower the energy.

c)

All three.

d)

The Aufbau Principle states that electrons enter the lowest energy orbitals first.

27.

Identify the rule that is being violated

a)

Aufbau's Principle

b)

Hund's Rule

c)

Pauli's Exclusion Principle

d)

Heisenberg uncertainty principle

28.

What is incorrect about this orbital diagram?

a)

Both arrows in the filled 2p box should be pointing the same direction

b)

There is nothing incorrect with this diagram

c)

In the there should only be 1 arrow in the first 2p box and one in the 2nd 2p box

d)

All the arrows should be pointing the same direction.

29.

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)

Core Notation

30.

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

a)

Aufbau Principle

b)

Pauli's Exclusion Principle

c)

Hund’s Rule

d)

Noble gas notation

31.

Which rule is violated in the following orbital diagrams?

a)

Hund's Rule

b)

Aufbau Principle

c)

Pauli's Exclusion Principle

32.

Which rule is violated in the following orbital diagrams?

a)

Aufbau Principle

b)

Hund's Rule

c)

Pauli's Exclusion Principle

33.
Which type of orbital is shaped like a sphere?
a)
s orbital
b)
p orbital
c)
d orbital
d)
f orbital
34.

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

a)

2p

b)

2d

c)

4p

d)

4f

35.
Why is the 3rd energy able to fit more electrons?
a)
Because 3 is a sacred number, just look at it!
b)
Because the p-block that looks like it is part of the 3rd energy level is actually part of the 2nd energy level
c)
Because the d-block that looks like it is part of the 4th energy level is actually part of the 3rd energy level
d)
Because the third energy level has 7 s orbitals
36.
What is the electron configuration for F?
a)
1s2 2s2 3p5
b)
1s2 2s2 3d5
c)
1s2 2s2 2p5
d)
1s2 2p5
37.
What is the electron configuration for V?
a)
[Ne] 4s2 4d3
b)
[Ar] 4s2 4d3
c)
[Ne]4s2 3d3
d)
[Ar] 4s2 3d3
38.

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

a)

energy level

b)

s orbitals

c)

p orbitals

d)

the number of electrons

39.

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

a)

Chlorine

b)

Argon

c)

Fluorine

d)

Sulfur

e)

Bromine

40.

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

a)

5

b)

6

c)

8

d)

13

41.

What is the noble gas configuration for Cobalt?

a)

[Kr] 4s2 3d7

b)

[Kr] 4s2 4d7

c)

[Ar] 4s2 3d7

d)

[Ar] 4s2 4d7

42.

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

a)

[He] 3s2

b)

[Ne] 3s2

c)

[Ar] 3s2

d)

[Ar] 4s2

43.

The graph above shows the ionization energy values as the elements are arranged on the periodic table. Which conclusion cannot be drawn from the graph?

a)

The ionization energy drops significantly as you move down a group because the valence electrons are in a shell further from the nucleus.

b)

The ionization energy increases gradually as you move right across a period because the valence electrons are in a shell further from the nucleus.

c)

The ionization energy increases gradually as you move right across a period because you are adding more protons.

d)

The ionization energy increases when the valence electrons are more attracted to the nucleus.

44.
The bar graph above represents four elements and their respective ionization energies. Based on the organization of the modern periodic table, how would these elements be found on the periodic table?
a)
They are in the same period with W being furthest left.
b)
They are in the same period with W being furthest right.
c)
They are in the same group with W being furthest to the bottom.
d)
They are in a diagonal line with W being at the bottom right.
45.
Which of the following is true for alkaline earth metals as their atomic number increases?
a)
The atomic radius decreases.
b)
Ionization energy decreases.
c)
The number of valence electrons increases.
d)
The Coulombic attraction increases.
46.
Which of the following sequences corresponds to a correct trend in ionization energy?
a)
Cl > S > P > Al
b)
Sr > Ca > Mg > Be
c)
Rb > K > Na > Li
d)
Rb > Sr > I > Xe
47.
Which of the following is true about a sulfur atom and a chlorine atom?
a)
Sulfur is larger and has higher ionization energy.
b)
Sulfur is larger and has lower ionization energy.
c)
Sulfur is smaller and has higher ionization energy.
d)
Sulfur is smaller and has lower ionization energy.
48.
The graph above shows the ionization energy values as the elements are arranged on the periodic table. Which conclusion cannot be drawn from the graph?
a)
The ionization energy drops significantly as you move down a group because the valence electrons are in a shell further from the nucleus.
b)
The ionization energy increases gradually as you move right across a period because the valence electrons are in a shell further from the nucleus.
c)
The ionization energy increases gradually as you move right across a period because you are adding more protons.
d)
The ionization energy increases when the valence electrons are more attracted to the nucleus.
49.
The bar graph above represents four elements and their respective ionization energies. Based on the organization of the modern periodic table, how would these elements be found on the periodic table?
a)
They are in the same period with W being furthest left.
b)
They are in the same period with W being furthest right.
c)
They are in the same group with W being furthest to the bottom.
d)
They are in a diagonal line with W being at the bottom right.
50.
Which of the following is true for alkaline earth metals as their atomic number increases?
a)
The atomic radius decreases.
b)
Ionization energy decreases.
c)
The number of valence electrons increases.
d)
The Coulombic attraction increases.
51.
Which of the following sequences corresponds to a correct trend in ionization energy?
a)
Cl > S > P > Al
b)
Sr > Ca > Mg > Be
c)
Rb > K > Na > Li
d)
Rb > Sr > I > Xe
52.
Which of the following is true about a sulfur atom and a chlorine atom?
a)
Sulfur is larger and has higher ionization energy.
b)
Sulfur is larger and has lower ionization energy.
c)
Sulfur is smaller and has higher ionization energy.
d)
Sulfur is smaller and has lower ionization energy.
53.
Which element has the greater ionization energy?
a)
Strontium
b)
Boron
54.
Which element has the greater ionization energy?
a)
Lead
b)
Silicon
55.
Put the following in order of increasing ionization energy:Neon, Lithium, Carbon
a)
Lithium, Carbon, Neon
b)
Carbon, Lithium, Neon
c)
Neon, Carbon, Lithium
d)
Lithium, Neon, Carbon
56.
Put the following in order of increasing ionization energy:Strontium, Aluminum, Indium
a)
Strontium, Indium, Aluminum
b)
Strontium, Aluminum, Indium
c)
Indium, Aluminum, Strontium
d)
Aluminum, Indium, Strontium
57.
Put the following in order of increasing ionization energy:Tellurium, Sulfur, Selenium
a)
Tellurium, Sulfur, Selenium
b)
Selenium, Sulfur, Tellurium
c)
Sulfur, Selenium, Tellurium
d)
Tellurium, Selenium, Sulfur
58.
Put the following in order of increasing ionization energy:Cobalt, Tungsten, Ruthenium
a)
Tungsten, Ruthenium, Cobalt
b)
Cobalt, Tungsten, Ruthenium
c)
Ruthenium, Cobalt, Tungsten
d)
Cobalt, Ruthenium, Tungsten
59.
Put the following in order of increasing ionization energy:Sodium, Oxygen, Boron
a)
Sodium, Boron, Oxygen
b)
Oxygen, Boron, Sodium
c)
Sodium, Oxygen, Boron
d)
Oxygen, Sodium, Boron
60.
What is ionization energy?
a)
Energy needed to destroy an atom
b)
Energy required to remove an electron
c)
Energy needed to split an electron
d)
Energy required to add an electron
61.
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. 
62.

As you look down a group, ionization energy and electronegativity

a)

increases

b)

decreases

63.

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

a)

increase

b)

decrease

64.

Which element has the greater ionization energy?

a)

Magnesium (Mg)

b)

Phosphorus (P)

65.

Which element has the greater ionization energy?

a)

Iodine (I)

b)

Chlorine (Cl)

66.

Which has the greater electronegativity:

N or C?

a)

C

b)

N

67.

Which has the greater electronegativity:

Cl or Al?

a)

Cl

b)

Al

68.
What elements have zero electronegativity?
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
69.
Which has the greater EN: 
N or C?
a)
C
b)
N
70.
Which has the greater EN: 
H or F?
a)
H
b)
F
71.
Put these in increasing order:
F, N, B
a)
B < N < F
b)
B < F < N
c)
N < F < B
d)
F < N < B
72.
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. 
73.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
74.
The element with the lowest electronegativity in Period 3 is - 
a)
Na
b)
Cl
c)
Ar
d)
Mg
75.
 Which of the following generally applies to the noble gases? 
a)
high ionization energy, low electronegativity, high reactivity
b)
high ionization energy, high electronegativity, high reactivity
c)
low ionization energy, low electronegativity, low reactivity
d)
high ionization energy, low electronegativity, low reactivity 
76.
Elements closer to the noble gases have stronger attraction for electrons.
a)
True
b)
False
77.
Chlorine and Fluorine are both very electronegative, as they are both missing a single electron from their valence energy level.  Why is Fluorine more electronegative than Chlorine? 
a)
Fluorine has less energy levels.
b)
Chlorine has more electrons in its outer shell
c)
Fluorine has more protons.
d)
None of these
78.
What elements have zero electronegativity?
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
79.
What is ionization energy?
a)
Energy needed to destroy an atom
b)
Energy required to remove an electron
c)
Energy needed to split an electron
d)
Energy required to add an electron
80.

As you look down a group, ionization energy and electronegativity

a)

increases

b)

decreases

81.

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

a)

increase

b)

decrease

82.

Which element has the greater ionization energy?

a)

Magnesium (Mg)

b)

Phosphorus (P)

83.

Which element has the greater ionization energy?

a)

Iodine (I)

b)

Chlorine (Cl)

84.
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
85.

As you look from left to right across a period, electronegativity

a)

increases

b)

decreases

86.

Who developed the Periodic Table?

a)

Mendeleev, who was a chemist and teacher

b)

Pavlov, who was a teacher and physchologist

c)

Ladahoff, who was a teacher and biologist

87.
The tendency of an atom to attract electrons and acquire a negative charge
a)
electronegativity
b)
charge
c)
bonding ability
d)
electron configuration
88.
A negatively charged subatomic particle that exists in various energy levels outside the nucleus of an atom
a)
neutron
b)
electron
c)
proton
d)
subatomic particle
89.
Which element has the greater ionization energy?
a)
Lead
b)
Silicon
90.
Put the following in order of increasing ionization energy:Neon, Lithium, Carbon
a)
Lithium, Carbon, Neon
b)
Carbon, Lithium, Neon
c)
Neon, Carbon, Lithium
d)
Lithium, Neon, Carbon
91.

As you look down a group, ionization energy and electronegativity

a)

increases

b)

decreases

92.
What is ionization energy?
a)
Energy needed to destroy an atom
b)
Energy required to remove an electron
c)
Energy needed to split an electron
d)
Energy required to add an electron
93.

Which element has the greater ionization energy?

a)

Magnesium (Mg)

b)

Phosphorus (P)

94.

Which element has the greater ionization energy?

a)

Iodine (I)

b)

Chlorine (Cl)

95.

As you look from left to right across a period, electronegativity

a)

increases

b)

decreases

96.
Which of these elements has the highest ionization energy?
a)
Lithium (Li)
b)
Potassium (K)
c)
Francium (Fr)
d)
Sodium (Na)
97.
Which of these elements has the lowest ionization energy?
a)
Oxygen (O)
b)
Boron (B)
c)
Carbon (C)
d)
Fluorine (F)
98.

The energy it takes to remove one electron from an atom

a)

Atomic Radii

b)

Ionization Energy

c)

Electron Affinity

d)

Ionic Radius

99.

Electron affinity trends is . . . .

a)

generally increases across a period, and a trend of decreasing electron affinity going down groups would be expected.

b)

generally decreases across a period, and a trend of decreasing electron affinity going down groups would be expected.

c)

generally increases across a period, and a trend of increasing electron affinity going down groups would be expected.

d)

generally decreases across a period, and a trend of increasing electron affinity going down groups would be expected.

100.

The amount of energy released when an electron is added to a neutral atom to form a negative ion

a)

Atomic Radii

b)

Ionization Energy

c)

Electron Affinity

d)

Oxidation Number

101.

Ionization energy trends is . . . .

a)

becomes greater down and to the right of the periodic table.

b)

becomes greater up and to the right of the periodic table.

c)

becomes greater up and to the left of the periodic table.

d)

becomes greater down and to the left of the periodic table.

102.

Which of the given atoms has the lowest electron affinity?

a)

Sr

b)

Be

c)

Ca

d)

Ra

103.

List the following atoms in order of increasing ionization energy: Li, Na, C, O, F.

a)

Li<Na<C<O<F

b)

Na<Li<C<O<F

c)

F<O<C<Li<Na

d)

Na<Li<F<O<C

104.

When the atomic radius increases, electron affinity

a)

Decreases

b)

Increases

c)

Neutral

d)

No effect

105.
Which atom would require the most energy to remove an electron?
a)
Ar
b)
Cl
c)
I
d)
Xe
106.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
107.

Which of the following atoms would have the largest second ionization energy?

a)

Cl

b)

S

c)

Ca

d)

Na

108.

The distance between nucleus and outermost shell occupied electron

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

109.

The energy it takes to remove one electron from an atom

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

110.

The tendency of an atom to attract a shared pair of electrons

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

111.

The amount of energy released when an electron is added to a neutral atom to form a negative ion

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

112.

The degree of oxidation (loss of electrons) of an atom in a chemical compound

a)

Atomic Radii

b)

Ionization Energy

c)

Electronegativity

d)

Electron Afinity

e)

Oxidation Number

113.

Atomic radii trends is . . . .

a)

generally decrease along each period of the table, from the alkali metals to the noble gases; and increase down each group.

b)

generally increase along each period of the table, from the alkali metals to the noble gases; and increase down each group.

c)

generally increase along each period of the table, from the alkali metals to the noble gases; and decrease down each group.

d)

generally decrease along each period of the table, from the alkali metals to the noble gases; and decrease down each group.

114.

Ionization energy trends is . . . .

a)

becomes greater up and to the right of the periodic table.

b)

becomes greater down and to the right of the periodic table.

c)

becomes greater up and to the left of the periodic table.

d)

becomes greater down and to the left of the periodic table.

115.

Electronegativity trends is . . . .

a)

increases on passing from left to right along a period, and decreases on descending a group.

b)

increases on passing from left to right along a period, and increases on descending a group.

c)

decreases on passing from left to right along a period, and decreases on descending a group.

d)

decreases on passing from left to right along a period, and increases on descending a group.

116.

Electron affinity trends is . . . .

a)

generally increases across a period, and a trend of decreasing electron affinity going down groups would be expected.

b)

generally decreases across a period, and a trend of decreasing electron affinity going down groups would be expected.

c)

generally increases across a period, and a trend of increasing electron affinity going down groups would be expected.

d)

generally decreases across a period, and a trend of increasing electron affinity going down groups would be expected.

117.

Metallic character trends is . . . .

a)

decrease going across a period and tends to increase going down a group.

b)

increase going across a period and tends to increase going down a group.

c)

decrease going across a period and tends to decrease going down a group.

d)

increase going across a period and tends to decrease going down a group.

118.

Which element has bigger atomic radii?

a)

Beryllium is bigger than Fluorine

b)

Oxygen is bigger than Sulphur

c)

Litihium is bigger than Sodium

d)

Phosphorus is bigger than Bromine

119.

Which element has smaller atomic radii?

a)

Beryllium is smaller than Fluorine

b)

Sulphur is smaller than Oxygen

c)

Litihium is smaller than Sodium

d)

Potassium is smaller than Bromine

120.

Which element has higher ionization energy?

a)

Chlorine is higher than Sodium

b)

Phosphorus is higher than Nitrogen

c)

Silicon is higher than Carbon

d)

Magnesium is higher than Aluminium

121.

Which element has lower ionization energy?

a)

Chlorine is lower than Sodium

b)

Phosphorus is lower than Nitrogen

c)

Carbon is lower than Silicon

d)

Aluminium is lower than Magnesium

122.

Which element has higher electronegativity?

a)

Fluorine is higher than Oxygen

b)

Potassium is higher than Sodium

c)

Aluminium is higher than Boron

d)

Phosphorus is higher than Chlorine

123.

Which element has lower electronegativity?

a)

Fluorine is lower than Oxygen

b)

Potassium is lower than Sodium

c)

Boron is lower than Aluminium

d)

Chlorine is lower than Phosphorus

124.

Which element has higher electron affinity?

a)

Bromine is higher than Calsium

b)

Chlorine is higher than Fluorine

c)

Magnesium is higher than Beryllium

d)

Sodium is higher than Aluminium

125.

Which element has lower electron affinity?

a)

Bromine is lower than Calsium

b)

Chlorine is lower than Fluorine

c)

Berylliumis lower than Magnesium

d)

Aluminium is lower than Sodium

126.

Which element is more metallic?

a)

Sodium is more metallic than Aluminium

b)

Fluorine is more metallic than Beryllium

c)

Potassium is more metallic than Lithium

d)

Chlorine is more metallic than Silicon

127.

Which element is less metallic?

a)

Sodium is less metallic than Aluminium

b)

Beryllium is less metallic than Fluorine

c)

Lithium is less metallic than Potassium

d)

Chlorine is less metallic than Silicon

128.
The concept of shielding happens because of
a)
attraction between nucleus and valence electrons
b)
attraction between nucleus and core electrons
c)
repulsion between valence electrons and other valence electrons
d)
repulsion between core electrons and valence electrons
129.
How many SHIELDING electrons are there in this atom? 1s2 2s22p6
a)
2
b)
4
c)
6
d)
8
130.
How many SHIELDING electrons are there in this atom?
1s2 2s22p6 3s23p6 4s2
a)
2
b)
4
c)
10
d)
18
131.
Shielding electrons are: 
a)
Electrons in the highest energy level
b)
Electrons in the lower energy levels
c)
Electrons that just come and go - they don't stay with the atom
d)
Electrons that are excited
132.
Valence electrons are: 
a)
Electrons in the highest energy level
b)
Electrons closest to the nucleus
c)
Electrons that just come and go - they don't stay with the atom
d)
Electrons that are excited
133.
Shielding electrons causes the force of attraction to the nucleus to 
a)
increase
b)
decrease
134.
The effective nuclear charge is _____ the actual nuclear charge
a)
the same as
b)
less than
c)
greater than
135.
When a new energy level is added to the atom, shielding
a)
increases
b)
decreases
136.
In moving from left to right across a period on the periodic table, the effective nuclear charge
a)
increases
b)
decreases
c)
stays the same
137.
In moving from top to bottom down a group on the periodic table,
a)
shielding increases
b)
shielding decreases
138.
How many shielding electrons does carbon have? (hint: write its configuration first)
a)
1
b)
2
c)
3
d)
4
139.
How many valence electrons does carbon have?
a)
3
b)
4
c)
5
d)
6
140.
As you go down a group, the amount of shielding....
a)
increases
b)
decreases
c)
stays the same
141.
As you go across a period, the amount of shielding...
a)
Increases
b)
decreases
c)
stays the same
142.
What is the Nuclear charge of yttrium? 
a)
40
b)
41
c)
38
d)
39
143.
What is EFFECTIVE nuclear charge
a)
The charge that actually matters
b)
The sharge of an element
c)
The charge felt by the valence electrons
d)
The charge felt by the inner orbital electrons
144.
As you move down a group, the effective nuclear charge....
a)
increase
b)
decreases
c)
stays the same
145.
As you move across a period, the effective nuclear charge...
a)
increases
b)
decreases
c)
stays the same
146.
Which of the following elements has the most "shielding" electrons?
a)
Nitrogen
b)
Phosphorus
c)
Arsenic
d)
Bismuth
147.
Which of the following elements has the most "shielding" electrons?
a)
Neon
b)
flourine
c)
oxygen
d)
They have the same
148.
Which of the following elements has the highest effective nuclear charge?
a)
Indium
b)
Antimony
c)
tellerium
d)
Tin
149.
Which of the following elements has a greater effective nuclear charge?
a)
Radium
b)
Francium
c)
copernicium
d)
actinium
150.
Which of the following elements has the lowest amount of shielding electrons?
a)
Argon
b)
Neon
c)
Helium
d)
Radon
151.
Which of the following elements has the lowest amount of shielding electrons?
a)
Hafnium
b)
Titanium
c)
Zirconium
d)
Rutherfordiu
152.
In the following configuration, which electrons are the shielding electrons? 1s2 2s2 2p6 3s2 3p4
a)
1s2 2s2 2p6
b)
3s2 3p4
c)
1s2 2s2
d)
2s2 2p6 3s2 3p4

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