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SS Morning Review

Total questions: 204

Worksheet time: 4hrs 38mins

Name
Class
Date
1.

What is the smallest unit of matter? It is composed of protons and neutrons, held together in the nucleus, and electrons around the nucleus in different electron orbitals, which form an electron cloud.

a)

cell

b)

nucleus

c)

atom

d)

electron

2.

What are any of the various self-contained units of matter or energy that are fundamental parts of all matter. These particles include electrons, protons, and neutrons.

a)

subatomic particles

b)

elements

c)

nucleus

d)

electron cloud

3.

What is a subatomic particle with a positive charge that is in the nucleus of an atom?

a)

neutron

b)

proton

c)

electron

d)

valence electron

4.

What is a subatomic particle without an electric charge, located in the nucleus of an atom?

a)

neutron

b)

proton

c)

electron

d)

valence electron

5.

What is a subatomic particle with a negative charge? It is found in the electron cloud surrounding the nucleus.

a)

neutron

b)

proton

c)

electron

d)

electron cloud

6.

What is the center of an atom containing protons and neutrons?

a)

nucleus

b)

neutron

c)

proton

d)

electron cloud

7.
Which subatomic particles are found in the nucleus of an atom?
a)
Protons and Electrons
b)
Protons and Neutrons
c)
Neutrons and Electrons
d)
Protons, Neutrons and Electrons
8.
What electrical charge does a proton have?
a)
+1
b)
0
c)
-1
d)
+2
9.

What mass does a neutron have?

a)

1 amu

b)

0 amu

c)

-1 amu

d)

+2 amu

10.
Complete the missing label on the diagram.
a)
Neutron
b)
Centre
c)
Nucleus
d)
Sub atomic particle
11.
Which particle is negatively charged?
a)
proton
b)
atom
c)
neutron
d)
electron
12.
In order for an atom to be neutral what has to be true?
a)
The atom has more protons than neutrons
b)
The atom has more neutrons than protons
c)
The atom has the same number of protons and neutrons
d)
The atom has the same number of protons and electrons
13.
What subatomic particles would you find in the nucleus of an atom?
a)
Protons only
b)
Protons and Neutrons
c)
Neutrons and Electrons
d)
Protons and Electrons 
14.

How many electrons does this atom have?

a)

2

b)

4

c)

6

d)

10

15.
Where is most of the mass in an atom located?
a)
in the nucleus
b)
in the protons
c)
in the neutrons
d)
in the electrons
16.

The smallest piece of an element:

a)

quark

b)

electron

c)

shell

d)

atom

17.

What is the name of group number 1?

a)

halogens

b)

noble gases

c)

alkali metals

d)

alkaline earth metals

18.

What is the name of group number 2?

a)

transition metals

b)

halogens

c)

metaloids

d)

alkaline earth metals

19.

where are the metaloids found

a)

far left, vertical

b)

stair step/diagonal

c)

far right horizontal

d)

at the bottom

20.

What group number are the halogens found?

a)

18 (8A)

b)

1

c)

2

d)

17 (7A)

21.

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

22.

A row on the Periodic Table of Elements

a)

family

b)

period

c)

row

d)

isotope

23.

___________ is a metal that is a liquid at room temperature.

a)

Platinum

b)

Water

c)

Tin

d)

Mercury

24.
__________ would have some characteristics of metals and some characteristics of nonmetals.
a)
Gold
b)
Sodium
c)
Arsenic
d)
Bismuth
25.

Which element is found in group 2, period 6?

a)

Oxygen (O)

b)

Barium (Ba)

c)

Selenium (Se)

d)

Carbon (C)

26.

Which halogen is found in period 4?

a)

Krypton (Kr)

b)

Xenon (Xe)

c)

Bromine (Br)

d)

Iodine (I)

27.

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)

28.

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

a)

group

b)

period

c)

family

d)

classification

29.

Name this group: These metals contain familiar metals such as gold, iron, and copper.

a)
b)
c)
d)
30.

an arrangement of the elements according to their atomic numbers so that elements with similar properties are in the same column and properties repeat from row to row

a)

Periodic Table of Elements

b)

Atomic Theory

c)

Isotopes

d)

Subatomic Particles

31.

one or two letters that represent the name of an element

a)

element name

b)

element symbol

c)

atomic number

d)

atomic mass

32.

a unique number for each element that equals the number of protons in an atom of that element

a)

element name

b)

element symbol

c)

atomic number

d)

atomic mass

33.

a grouping of elements based on similar properties, arranged by columns in the periodic table; also known as a group

a)

family

b)

period

c)

row

d)

isotope

34.

The letter, C, is a ... of carbon.

a)

Name

b)

Nickname

c)

Chemical Symbol

d)

Pseudonym

35.

Find these groups: Locate Lanthanides and Actinides.

a)
b)
c)
d)
36.

Name this family: This family contains an element known for its role in the chemistry of life.

a)

Nitrogen family

b)

Carbon family

c)

Halogen family

d)

Noble gases

37.

Find this family: This family contains nitrogen and phosphorus.

a)
b)
c)
d)
38.

Name this family: This family contains an element necessary for water and we need it to breathe.

a)

Oxygen family

b)

Halogen family

c)

Carbon family

d)

Nitrogen family

39.

Find this family: This family contains very reactive nonmetals like fluorine and chlorine.

a)
b)
c)
d)
40.

Name this group: These elements, also known as inert gases, tend to be nonreactive.

a)

Halogen family

b)

Noble gases

c)

Carbon family

d)

Nitrogen family

41.
Which of the following atomic symbols for bromine is written correctly?
a)
bR
b)
BR
c)
Br
d)
br
42.
How many significant figures: 216 m
a)
1
b)
2
c)
3
d)
0
43.
How many significant figures: 2016 m
a)
1
b)
2
c)
3
d)
4
44.
How many significant figures: 153.0 mL
a)
1
b)
2
c)
3
d)
4
45.
How many significant figures: 0.012 km
a)
1
b)
2
c)
3
d)
4
46.
How many significant figures: 1000 mL
a)
1
b)
2
c)
3
d)
4
47.
How many significant figures: 100.000 cL
a)
1
b)
3
c)
5
d)
6
48.
How many significant figures: 0.001 g
a)
4
b)
3
c)
2
d)
1
49.
How many significant figures: 4.20 cm
a)
1
b)
2
c)
3
d)
4
50.
How many significant figures: 0.010 L
a)
1
b)
2
c)
3
d)
4
51.

How many significant figures: 450 m

a)

3

b)

2

c)

1

d)

0

52.
How many sig figs are there?
100000000
a)
1
b)
9
c)
10
53.
How many sig figs are there?
0.000008
a)
1
b)
2
c)
6
d)
7
54.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

55.

What is the atomic number of Barium, Ba? (enlarge the periodic table)

a)

20

b)

38

c)

56

d)

88

56.

How many protons are in a sodium atom, Na? (tap to enlarge the periodic table)

a)

Sodium has 1 proton.

b)

Sodium has 3 protons.

c)

Sodium has 11 protons

57.

Atoms of the same element which have a different number of neutrons are called _________________.

a)

ions

b)

isotopes

c)

quarks

d)

molecules

58.

Which subatomic particle has a negative charge in the atom?

a)

proton

b)

neutron

c)

electron

d)

quark

59.

How many neutrons does C-14 contain? (tap to enlarge the image)

a)

6

b)

7

c)

14

d)

8

60.

ALL atoms of the same element have:

a)

same number of proton

b)

same number of nucleon

c)

different number of neutron

d)

different number of electron

61.
If X is the symbol for an element, which of the following two symbols represent    isotopes of the same element?     I. 7735X  II. 7733X  III. 8137X  IV. 8135 X
a)
I and II
b)
III and IV
c)
I and IV
d)
I and III
62.
How many neutrons does the isotope below have?     89 36Kr
a)
53
b)
36
c)
89
d)
125
63.
Four isotopes of lead include lead-204, lead-206, lead-207, and lead-208.  The average atomic mass of lead is 207.2.  Which isotope of lead is likely to be the most abundant.
a)
204
b)
206
c)
207
d)
208
64.
Which subatomic particles contribute the most to the mass of an atom?
a)
Protons, Neutrons, Electrons
b)
Protons only
c)
Protons and Electrons
d)
Protons and Neutrons
65.
The number of protons is equal to 
a)
the atomic number
b)
the number of neutrons
c)
the energy levels
d)
the periodic table groups
66.

If an atom has 12 neutrons and 11 protons, what is its atomic mass?

(a)  

67.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
68.
Calculate the average atomic mass of silver.
a)
106.38649amu
b)
111.91896amu
c)
107.8677amu
d)
121
69.
An element has two naturally occurring isotopes. One is 10.013 amu and is 19.9% abundant. The other is 11.01 amu and is 80.1% abundant. What is the average atomic mass? What element is it?
a)
9.012, Beryllium
b)
12.011, Carbon
c)
6.941, Lithium
d)
10.812, Boron
70.
Oxygen has 8 protons. What is oxygen's atomic number?
a)
16
b)
8
c)
15.999
d)
0
71.

What is the charge on a lithium atom that loses 1 electron?

a)

+1

b)

0

c)

-1

d)

-2

72.

What is the atomic number of Fe? (click to see image)

a)

26

b)

55.845

c)

56

d)

30

73.
a)
2
b)
8
c)
3
d)
13
74.
a)
12
b)
7
c)
8
d)
14
75.

Valence electrons are in the...

a)

Innermost energy level of the atom.

b)

Middle energy level of the atom.

c)

Outermost energy level of the atom.

d)

energy levels of the atom.

76.

How many valence electrons does Helium have?

a)

1

b)

2

c)

3

d)

4

e)

5

77.

Convert 6 m to cm

a)

60 cm

b)

600 cm

c)

6000 cm

d)

0.6 cm

78.

Convert 210 mm to cm

a)

2.1 cm

b)

21 cm

c)

210 cm

d)

2100 cm

79.

Convert 5.3 km to m

a)

53 m

b)

530 m

c)

5300 m

d)

53000 m

80.

Convert 0.84 m to cm

a)

0.084 cm

b)

0.0084 cm

c)

8.4 cm

d)

84 cm

81.

Convert 54,000 mm to km

a)

0.054 km

b)

0.54 km

c)

5.4 km

d)

54 km

82.

Convert 0.067 km to mm

a)

67 mm

b)

670 mm

c)

6700 mm

d)

67000 mm

83.

Convert 3000 g to kg

a)

0.3 kg

b)

3 kg

c)

30 kg

d)

300 kg

84.

Convert 5 kg to g

a)

50 g

b)

500 g

c)

5000 g

d)

50000 g

85.

Convert 560 g to kg

a)

56 kg

b)

5.6 kg

c)

0.56 kg

d)

0.056 kg

86.

Convert 35,000 mg to kg

a)

0.035 kg

b)

0.35 kg

c)

3.5 kg

d)

35 kg

87.

Convert 9.48 kg to g

a)

94.8 g

b)

948 g

c)

9480 g

d)

94800 g

88.

Convert 256 g to kg

a)

25.6 kg

b)

2.56 kg

c)

0.256 kg

d)

0.0256 kg

89.

Convert 2000 ml to l

a)

20 l

b)

2 l

c)

20000 l

d)

200 l

90.

Convert 500 cl to l

a)

50 l

b)

5 l

c)

5000 l

d)

50000 l

91.

Convert 45,000 ml to l

a)

4500 l

b)

450 l

c)

45 l

d)

4.5 l

92.

Convert 65 l to ml

a)

650 ml

b)

6500 ml

c)

65000 ml

d)

650000 ml

93.

Convert 525 ml to cl

a)

52.5 cl

b)

5.25 cl

c)

0.525 cl

d)

0.0525 cl

94.

Convert 465,400 ml to l

a)

46540 l

b)

4654 l

c)

465.4 l

d)

46.54 l

95.
If the exponent on your power of 10 is positive, is your number larger or smaller than 10?
a)
Larger
b)
Smaller
96.
7.82 x 10-6 is an example of scientific notation. The exponent of -6 tells you your number will be very ________.
a)
Large
b)
Small
c)
Basic
97.
Change from standard form to scientific notation: 12,000,000
a)
12.0  x  107
b)
0.12  x  107
c)
1.2  x  106
d)
1.2  x  107
98.
Change from standard form to scientific notation:  450,000
a)
4.5  x  105
b)
45  x  105
c)
4.5  x  104
d)
4.5  x  106
99.
Change from standard form to scientific notation:  0.000398
a)
39.8  x  10-5
b)
3.98  x  10-5
c)
3.98  x  10-4
d)
39.8  x  10-6
100.
Change from standard form to scientific notation: 0.004078
a)
4.078  x  10-3
b)
4.078  x  103
c)
40.78  x  10-4
d)
.4078  x  10-2
101.
125,678,000: Change to scientific notation
a)
1.25678  x  1012
b)
.125678  x  10-9
c)
12.5678  x  108
d)
1.25678  x  108
102.
Try to change the number back to standard form:  6.79  x  104
a)
679,000
b)
6,790
c)
67,900
d)
6,790,000
103.
Try to change the number back to standard form: 3.97  x  10-2
a)
0.000397
b)
0.0397
c)
0.0000397
d)
0.397
104.
The factor multiplied by a power of 10 in scientific notation needs to be greater than or equal to one but less than ___________?
a)
1
b)
10
c)
100
d)
1,000
105.

Which atom has the largest atomic radius?

a)

potassium

b)

rubidium

c)

francium

d)

cesium

106.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
107.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
108.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
109.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
110.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
111.
Order the following in increasing atomic radii: 
Ra, Be, Ca, Rb, H
a)
Ra, Be, Rb, H, Ca
b)
Rb, H, Ca, Be, Ra
c)
Ra, Rb, Ca, Be, H
d)
H, Be, Ca, Rb, Ra
112.
The more protons there are, the  ____ .
a)
Weaker the pull
b)
Smaller the electrons
c)
Stronger the pull
d)
The bigger the electrons
113.
Which one has the largest radius?
a)
Lithium (Li, atomic #3)
b)
Boron (B, atomic #5)
c)
Neon (Ne, atomic #10)
d)
Nitrogen (N, atomic #7)
114.

What is the atomic radius?

a)

The distance from the nucleus to the outer boundary of an atom

b)

The distance from one side of an atom to the other side

c)

The distance around the atom

d)

The distance between atoms in the gas phase

e)

The distance between atoms in the solid phase

115.

Which of the following elements would be smaller: indium or gallium?

a)

indium

b)

gallium

c)

both atoms are the same size

d)

cannot be determined

e)

the sizes can vary

116.

Which of the following elements would be larger: potassium or cesium?

a)

potassium

b)

cesium

c)

both atoms are the same size

d)

cannot be determined

e)

the sizes can vary

117.

Which of the following elements would be the largest: copper, zinc, silver or cadmium?

a)

copper

b)

zinc

c)

silver

d)

cadmium

e)

cannot be determined

118.

Why is iodine larger than bromine?

a)

iodine has a greater number of electrons than bromine

b)

iodine has a greater number of protons than bromine

c)

iodine has more occupied energy levels and greater shielding than bromine

d)

iodine has more neutrons than bromine

e)

iodine has more valence electrons than bromine

119.

Which has the highest ionization energy?

a)

Arsenic

b)

Iron

c)

ZInc

d)

Cobalt

120.

Which has a lower ionization energy?

a)

Lithium

b)

Cesium

c)

Sodium

121.

Ionization energy __________ as you do across a period

a)

has no pattern

b)

stays the same

c)

decreases

d)

increases

122.

Select all that explain the ionization energy trend within periods

a)

electrons are closer to the nucleus

b)

their is a weak pull between electrons from the nucleus, making them easily moveable

c)

feel more of a pull from nucleus, making them harder to move

d)

electrons are further from the nucleus

123.

Ionization energy (a)   as you go down a group.

124.

Explain why ionization energy decreases as you go down a group.

a)

Outer electrons are further away from the nucleus you go down a group

b)

Electrons feel less pull from the nucleus as you go down a group

c)

Electrons are easier to remove as you go down a group

d)

All of the above

125.

What is Ionization energy?

a)

The energy used in a chemical reaction

b)

Potential energy

c)

The energy it takes to remove one electron from an atom or ion in its gaseous state

126.

Which of the following lists the atoms in order of increasing Ionization energy?

a)

calcium, iron, copper

b)

copper, iron, calcium

c)

calcium, copper, iron

d)

iron, copper, calcium

127.

Which element has a higher electronegativity value?

a)

Niobium

b)

Tin

c)

Cadmium

d)

Iodine

128.

Which element has a lower electronegativity value?

a)

Calcium

b)

Barium

129.

Electronegativity (a)   as you go down a group.

130.

Electronegativity trends are the same as:

a)

Atomic radius trends

b)

Ionization energy trends

c)

Both of these

d)

None of these

131.

What does electronegativity do as you go across a period?

a)

decrease

b)

no pattern

c)

stay the same

d)

increase

132.

As you move across a period, the outer electrons are ________ to the nucleus, so the nucleus of the atom is ________ to attract electrons in a bond.

a)

closer, more able

b)

closer, less able

c)

further, less able

d)

further, more able

133.

Do noble gases have electronegativity values?

a)

yes

b)

no

134.

Why does electronegativity decrease as you go down a group?

a)

As you go down a group, the outer electrons are further away from the nucleus

b)

As you go down a group, the nucleus is less able to attract electrons in a bond

c)

Both of these

d)

None of these

135.

Which is the correct order of electronegativity from lowest to highest?

a)

Zinc, Nickel, Iron, Scandium

b)

Iron, Nickel, Zinc, Scandium

c)

Scandium, Iron, Nickel, Zinc

d)

Scandium, Iron, Zinc, Nickel

136.

Electronegativity is the ability of an atom to attract electrons in a physical bond.

a)

false

b)

true

137.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
138.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
139.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
140.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
141.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
142.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
143.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
144.
What is this element? 
1s22s22p63s23p6
4s23d104p6
a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
145.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
146.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
147.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
148.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
149.
How many valence electrons does phosphorus have?
a)
5
b)
2
c)
8
d)
15
150.
What element has the valence shell configuration
3s2 3p2
a)
Al
b)
B
c)
Si
d)
Ga
151.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
152.
What noble gas should be used to write the shorthand configuration for Te?
a)
Ar
b)
Kr
c)
Xe
d)
Sb
153.
Identify the element in Period 5 that has 1 valence electron?
a)
Rb
b)
Nb
c)
Ag
d)
Sb
154.
What element in Period 4 has 5 valence electrons?
a)
Zr
b)
As
c)
V
d)
Sb
155.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
156.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
157.
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
158.
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
159.
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
160.
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
161.
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
162.
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
163.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
164.
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.
165.
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
166.
An orbital can at most hold how many electrons?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
167.

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.

168.

Identify the rule that is being violated

a)

Aufbau's Principle

b)

Hund's Rule

c)

Pauli's Exclusion Principle

d)

Heisenberg uncertainty principle

169.

What is the noble gas configuration for Neon?

a)

[Ne]

b)

[He]2s22p6

c)

[F]2p1

d)

[Ne]2s21p6

170.
What is the noble gas configuration for beryllium?
a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
171.
What is the noble gas configuration for boron?
a)
[He]1s22s2
b)
[He]2s22p2
c)
[He]2s22p1
d)
[Li]2s22p1
172.
What is the noble gas configuration for Sulfur?
a)
[Ar] 3p4
b)
[He] 3s2 3p4
c)
[Ne] 3s2 3p4
d)
[Na] 3s2 3p4
173.
What is the noble gas configuration for phosphorus?
a)
[Ar] 3p5
b)
[He] 3s2 3p5
c)
[Ne] 3s2 3p3
d)
[Na] 3s2 3p5
174.
[He]2s22p4 is the noble gas configuration for which element?
a)
oxygen
b)
sulfur
c)
phosphorus
d)
fluorine
175.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
176.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
177.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
178.
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.
179.
 The diagram above represents two electrons with 
a)
a. opposite spins.
b)
 b. the same spin.
c)
c. different energies.
d)
d. different energy levels.
180.
Identify the element for
[Xe] 6s2 4f14 5d4
a)
Cobalt
b)
Iron
c)
Tungstun
181.
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
182.
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
183.
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
184.
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
185.
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
186.
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
187.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
188.
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.
189.
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
190.
An orbital can at most hold how many electrons?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
191.

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.

192.

Identify the rule that is being violated

a)

Aufbau's Principle

b)

Hund's Rule

c)

Pauli's Exclusion Principle

d)

Heisenberg uncertainty principle

193.

What is the noble gas configuration for Neon?

a)

[Ne]

b)

[He]2s22p6

c)

[F]2p1

d)

[Ne]2s21p6

194.
What is the noble gas configuration for beryllium?
a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
195.
What is the noble gas configuration for boron?
a)
[He]1s22s2
b)
[He]2s22p2
c)
[He]2s22p1
d)
[Li]2s22p1
196.
What is the noble gas configuration for Sulfur?
a)
[Ar] 3p4
b)
[He] 3s2 3p4
c)
[Ne] 3s2 3p4
d)
[Na] 3s2 3p4
197.
What is the noble gas configuration for phosphorus?
a)
[Ar] 3p5
b)
[He] 3s2 3p5
c)
[Ne] 3s2 3p3
d)
[Na] 3s2 3p5
198.
[He]2s22p4 is the noble gas configuration for which element?
a)
oxygen
b)
sulfur
c)
phosphorus
d)
fluorine
199.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
200.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
201.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
202.
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.
203.
 The diagram above represents two electrons with 
a)
a. opposite spins.
b)
 b. the same spin.
c)
c. different energies.
d)
d. different energy levels.
204.
Identify the element for
[Xe] 6s2 4f14 5d4
a)
Cobalt
b)
Iron
c)
Tungstun

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