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Unit 2- Atomic Structure

Total questions: 126

Worksheet time: 3hrs 4mins

Name
Class
Date
1.
Which of the following is NOT a subatomic particle?
a)
Proton
b)
Neutron
c)
Photon
d)
Electron
2.
Which subatomic particle has a positive charge?
a)
Proton
b)
Neutron
c)
Electron
3.
Which subatomic particle has a negative charge?
a)
Proton
b)
Neutron
c)
Electron
4.
Which subatomic particle is neutral?
a)
Proton
b)
Neutron
c)
Electron
5.
Which subatomic particles are NOT located in the nucleus?
a)
Protons
b)
Neutrons
c)
Electrons
6.
The atomic number of an element is the same as the number of ________ in the nucleus.
a)
Protons
b)
Neutrons
c)
Protons + Neutrons
d)
Electrons
7.
Atoms of the same element with different numbers of neutrons are called
a)
Ions
b)
Isotopes
c)
Iotas
d)
Introns
8.
The mass of a proton is the same as the mass of a 
a)
neutron
b)
electron
9.
The mass number of an isotope is equal to the number of ______ in an atom.
a)
Protons
b)
Neutrons
c)
Protons + Neutrons
d)
 Electrons
10.
The mass listed on the periodic table for each element is known as the 
a)
average atomic mass
b)
atomic mass
c)
atomic weight
d)
weighted mass
11.

To calculate average atomic mass, you need

a)

the atomic mass of each isotope

b)

the percent abundance of each isotope

c)

the atomic mass and percent abundance of each isotope

d)

to find the average of the atomic masses of each isotope

12.

Which subatomic particle determines the identity of an element?

a)

protons

b)

neutrons

c)

electrons

13.

Which TWO subatomic particles determine the charge of an atom?

a)

protons

b)

neutrons

c)

electrons

14.

What is the relative mass of an electron?

a)

1 amu

b)

0 amu

15.

An element has two isotopes, one with a mass of 39 and one with a mass of 41. If the average mass is 40.6, which isotope is more abundant?

a)

mass of 39

b)

mass of 41

c)

they are both equally abundant

16.
The area of the atom where protons and neutrons are found
a)
Electron Cloud
b)
Nucleus
c)
Energy Level
17.
The horizontal rows of the periodic table
a)
Groups
b)
Periods
c)
Families
18.
The vertical rows of the periodic table, also called families
a)
Groups
b)
Periods
c)
Rows
19.
A design of an atom showing the nucleus as well as the electrons their designated orbits
a)
Periodic Table
b)
Bohr Model
c)
Electron Cloud
20.
What is similar between the elements in the same group?
a)
They have the same atomic mass.
b)
They have the same energy levels.
c)
They have the valence electrons.
21.
If an element has 14 protons, 15 neutrons, and 14 electrons, what is that elements atomic mass
a)
28
b)
14
c)
29
22.
What element does the Bohr Model represent?
a)
Nitrogen
b)
Potassium
c)
Sodium
23.
Which other element has the same number of valence electrons as chlorine?
a)
Sodium
b)
Bromine
c)
Oxygen
24.
Alkaline Earth Metals...
a)
are semiconductors
b)
are the most reactive type of elements
c)
have two valence electrons
25.
What is the name of this element?
a)
Helium
b)
Hydrogen
c)
Argon
d)
Silver
26.
What is the name of this element?
a)
Lithium
b)
Boron
c)
Carbon
d)
Neon
27.
What is the mass number of this atom?
a)
1
b)
3
c)
4
d)
7
28.
What is the atomic number of this atom?
a)
2
b)
4
c)
6
d)
none of the above
29.
What group does this element belong to?
a)
Group 1: Alkali metals
b)
Group 18: Noble Gases
c)
Group 2: Alkaline-Earth Metals
d)
Group 17: Halogens
30.
How many valence electrons?
a)
2
b)
3
c)
5
d)
10
31.
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
32.

What is this element?

a)

Beryllium (atomic #4)

b)

Boron (atomic #5)

c)

Carbon (atomic #6)

d)

Nitrogen (atomic #7)

33.

How many valence electrons?

a)

2

b)

3

c)

4

d)

5

34.

What group does this element belong to?

a)

1

b)

2

c)

17

d)

18

35.

How many valence electrons?

a)

2

b)

4

c)

6

d)

8

36.

Which Bohr model represents Neon?

a)
b)
c)
d)
37.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
38.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
39.
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.
40.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
41.
Which orbital shows a violation of the Aufbau Principle?
a)
A
b)
B
c)
C
d)
D
42.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
43.

This orbital diagram represents

a)

Sodium

b)

Magnesium

c)

Aluminum

d)

Iron

44.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
45.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
46.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
47.
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
48.
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
49.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
50.

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

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

51.

What is this element?

1s22s22p63s23p64s23d104p6

a)

Argon

b)

Krypton

c)

Selenium

d)

Bromide

52.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
53.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
54.

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

a)

representative elements

b)

columns 3-8

c)

rare earth elements

d)

transition elements

55.
How many electron can be found in a p orbital?
a)
2
b)
3
c)
4
d)
6
56.
What is the electronic configuration of iron?
a)
1s22s22p63s23p64s23d6
b)
1s22s22p63s23p63d8
c)
1s22p63s23p64s23d6
d)
1s22s22p63s23p64s13d6
57.

How many valence electrons does the element have?

(a)  

58.

How many valence electrons does the element have?

(a)  

59.

How many valence electrons does the element have?

(a)  

60.

How many valence electrons does the element have?

1s22s22p63s23p64s23d10

(a)  

61.

How many valence electrons does the element have?

1s2 2s2 2p6 3s2

(a)  

62.

How many valence electrons does the element have?

1s22s22p63s23p64s23d104p6

(a)  

63.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
64.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
65.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
66.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
67.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
68.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
69.
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
70.
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
71.
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)
72.
Electronegativity is...
a)
the ability of an atom to attract/ accept 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.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
74.
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
75.
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.
76.
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
77.
How many valence electrons are in an atom of Ar?
a)
2
b)
8
c)
4
d)
1
78.
How many valence electrons are in an atom of K?
a)
3
b)
8
c)
4
d)
1
79.
The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?

a)
W
b)
X
c)
Y
d)
Z
80.

This model this model was the first to show a nucleus, consisting of protons and neutron. Electrons surround the nucleus but are not shown in distinct energy levels.

a)

The "Rutherford Model" of the atom

b)

The "Plum Pudding Model" of the atom

c)

The "Quantum Mechanical Model" of the atom

81.

This model was developed after J.J. Thompson discovered electrons, a particle smaller than an atom. It shows electrons floating freely in a positive region.

a)

The "Plum Pudding Model" of the atom

b)

The "Rutherford Model" of the atom

c)

Democritus's model of the atom

d)

The "Quantum Mechanical Model" of the atom

82.
Ernest Rutherford discovered that atoms were mostly _________________. 
a)
negatively charged
b)
positively charged
c)
electrons
d)
empty space. 
83.
In the gold foil experiment, most of the positively charged alpha particles passed through the gold foil, but some were deflected or bounced back.  What did we conclude because of this?  
a)
Atoms are small indivisible spheres
b)
Atoms are mostly empty space with a small, dense, positive center
c)
Atoms have negatively charged particles which orbit the nucleus
d)
Light is a wave, not a particle
84.

Who was the first to propose that matter consist of indivisible particle of matter called atoms?

a)

John Dalton

b)

Aristotle

c)

Democritus

d)

Plato

85.

The cathode-ray tube was used to discover the ____ by ____.

a)

electron by Thomson

b)

electron by Dalton

c)

proton by Thomson

d)

proton by Dalton

e)

electron by Rutherford

86.

An atom is electrically neutral because

a)

the numbers of protons and neutrons are equal.

b)

the numbers of protons and electrons are equal.

c)

neutrons balance the protons and electrons.

87.

Which of the following statements is correct?

a)

Protons are positively charged and neutrons are negatively charged.

b)

Protons are negatively charged and electrons are positively charged.

c)

Protons are positively charged and electrons are negatively charged.

88.

Which model of the atom is denoted as the "plum pudding" model?

a)

A

b)

B

c)

C

d)

D

e)

E

89.

Chadwick is credited with discovering which part of the atom?

a)

nucleus

b)

protons

c)

electrons

d)

neutrons

90.

Who is credited with developing model D?

a)

Thomson

b)

Dalton

c)

Bohr

d)

Rutherford

91.

Dalton's model of the atom is represented by which letter?

a)

A

b)

B

c)

C

d)

D

e)

E

92.

What is the heaviest atom that can be formed through nuclear fusion in the core of stars?

(a)  

93.

What is the name of the process that forms elements Helium through Iron?

(a)  

94.

This model this model was the first to show a nucleus, consisting of protons and neutron. Electrons surround the nucleus but are not shown in distinct energy levels.

a)

The "Rutherford Model" of the atom

b)

The "Plum Pudding Model" of the atom

c)

The "Quantum Mechanical Model" of the atom

95.

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

a)

True

b)

False

96.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
97.
Line emission spectrum shown below happens when
a)
Electron transition from lower to higher energy level.
b)
Electron transition from higher to lower energy level.
c)
Electron exist in fixed energy states
d)
Electron transition between different energy levels.
98.
Why are line emission spectra of elements called "atomic fingerprints"?
a)
They are all the same
b)
They are all unique
c)
They are all similar
d)
They all contain colored light
99.

All stars are composed of a mixture of elements. When these elements are heated they emit specific amounts of electromagnetic radiation, known as an emission spectrum. Each element emits a unique, identifiable, spectrum.


Using the Bright-line emission spectrum chart below, identify the elements present in this modeled star (found in the line labeled “mixture”).

a)

Lithium and cadmium are in the mixture. Strontium is not in the mixture.

b)

Lithium and strontium are in the mixture. Cadmium is not in the mixture

c)

Cadmium and strontium are in the mixture. Lithium is not in the mixture

d)

All of the shown elements are present in the mixture.

100.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

101.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

102.
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
103.

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

a)

Hydrogen only

b)

Hydrogen & Helium

c)

Calcium only

d)

Hydrogen & Calcium

104.

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

a)

absorbs energy

b)

releases energy

105.

Look carefully at the picture. It shows an electron in the excited state on the left, and the electron returning to its ground state on the right. When the electron return to the ground state it emits a_______________________.

a)

blast of cold air

b)

electrostatic charge

c)

proton

d)

photon (light)

106.

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

107.

An atom that has gained or lost electrons in an attempt to become stable/bond with another atom.

a)

Normal/Neutral Atom

b)

Ion

c)

Isotope

108.

Atoms of the same element that have different mass than expected because they have a different number of neutrons.

a)

Neutral Atom

b)

Ion

c)

Isotope

d)

Cation

109.

If an ion has a positive charge you would __________ the charge number from the number of protons to figure out how many electrons there are.

a)

subtract

b)

add

c)

multiply

d)

divide

110.

If an ion has a negative charge you would __________ the charge number to the number of protons to figure out how many electrons there are.

a)

Add

b)

Subtract

c)

Divide

d)

Multiply

111.

If an atom has 9 protons and 10 electrons it has a charge of ____.

a)

0

b)

-1

c)

+1

d)

-2

112.

If an atom has 4 protons and 2 electrons it has a charge of ____.

a)

0

b)

-2

c)

+2

d)

+1

113.

If an atom has a charge of +3 and an atomic number of 5 it should have _______ electrons.

a)

1

b)

2

c)

3

d)

4

114.

If an atom has a charge of -2 and an atomic number of 16 it should have _______ electrons.

a)

14

b)

16

c)

18

d)

20

115.

If an atom has a charge of 0 (neutral) and an atomic number of 8 it should have ____ electrons.

a)

0

b)

8

c)

7

d)

9

116.

How many protons does this isotope of titanium have?

a)

22

b)

26

c)

48

d)

70

117.

How many neutrons are in an atom of carbon-14?

a)

6

b)

8

c)

10

d)

14

118.

If X is the symbol for an element, which TWO of the following symbols represent isotopes of the same element?

I. 7735X

II. 7733X

III. 8137X

IV. 8135 X

a)

I

b)

II

c)

III

d)

IV

119.

Chromium has four naturally occurring isotopes (chromium-50, chromium-52, chromium-53, and chromium-54). What is the average atomic mass of Chromium?

a)

4

b)

51.996

c)

52.25

d)

Not enough information was given.

120.

An element has three isotopes. Given the abundances and relative masses, calculate the average atomic mass and determine (from the periodic table) which element it is.


Abundances | Relative masses

0.005% | 234.04 amu

0.720% | 235.04 amu

99.275% | 238.05 amu

a)

Uranium (#92, Atomic Mass: 238.03 amu)

b)

Fluorine (#9, Atomic Mass: 19.00 amu)

c)

Mercury (#89, Atomic Mass: 200.59 amu)

d)

Polonium (#84 209 amu)

121.
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
122.

Rubidium has two naturally occurring isotopes, 85Rb (relative mass 84.9118 amu) and 87Rb (relative mass 86.9092 amu). The abundance of 87Rb is 27.8%, If rubidium has an average atomic mass of 85.47 amu, what is the % abundance of 85Rb (in percent)?

a)

27.9%

b)

72.1%

c)

74.63%

d)

34.29%

123.

What is the number of neutrons?

(a)  

124.

If you have 10 protons and 9 neutrons, what would the mass number be?

(a)  

125.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
126.

How many neutrons does this isotope of titanium have?

(a)  

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