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Atomic Structure, Waves, & Periodicity

Total questions: 134

Worksheet time: 2hrs 52mins

Name
Class
Date
1.

What is the atomic number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons in the energy levels

2.

What is the mass number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons and electrons in the atom

3.

What is the atomic number of this atom?

a)

1

b)

3

c)

4

d)

7

4.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

5.
Most of the mass in an atom is made up of _____________________?
a)
protons and electrons
b)
protons and neutrons
c)
neutrons and electrons
d)
electrons and quarks
6.
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
7.
What does the C represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
8.

What does the 6 represent?

a)

Atomic mass

b)

atomic number

c)

chemical symbol

d)

element name

9.
How is the number of neutrons in the nucleus of an atom calculated?
a)
Add the number of e- and p+ together
b)
Subtract the number of e- from p+
c)
Subtract the number of p+ from the mass number
d)
Add the mass number to the number of e-
10.
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 
11.
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
12.
If an atom has 12 positively charged subatomic particles, which of the following must it also have to be considered a neutral atom?
a)
12 neutrons
b)
12 electrons
c)
12 protons
d)
24 protons and neutrons
13.

An atom has 10 protons, 15 neutrons and 10 electrons what is its mass number.

a)

20

b)

10

c)

35

d)

25

14.

How many electrons does this atom have?

a)

2

b)

4

c)

6

d)

10

15.
The atomic number of an element that has 9 protons, 9 electrons, and 10 neutrons is _____.
a)
9
b)
10
c)
19
d)
28
16.
An element with a mass number of 11 and an atomic number of 5 has how many neutrons?
a)
11
b)
5
c)
6
d)
16
17.
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
18.
An atom has an atomic number of 15 and a mass number of 31. How many protons are there in the atom?
a)
15
b)
31
c)
16
d)
47
19.
What is the atomic number of the atom pictured? 
a)
9
b)
10
c)
18
d)
19
20.

Which of the following determines the identity of an element?

a)

number of protons

b)

atomic mass

c)

number of neutrons

d)

number of shells

21.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

22.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
23.
Value representing the number of protons in an element
a)
Atomic Mass
b)
Mass Number
c)
Valence Electrons
d)
Atomic Number
24.
Subatomic particles that are neutral in charge
a)
Neutrons
b)
Protons
c)
Nucleus 
d)
Electrons
25.
Which two subatomic particles make up the nucleus of an atom?
a)
Protons and Electrons
b)
Neutrons and Electrons
c)
Electrons and Protons
d)
Protons and Neutrons
26.
Where are the Electrons found in the structure of an atom?
a)
In the nucleus
b)
In spaces around the nucleus
27.

What is the mass number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons and electrons in the atom

28.
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
29.
What does the C represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
30.

What does the 6 represent?

a)

Atomic mass

b)

atomic number

c)

chemical symbol

d)

element name

31.
How is the number of neutrons in the nucleus of an atom calculated?
a)
Add the number of e- and p+ together
b)
Subtract the number of e- from p+
c)
Subtract the number of p+ from the mass number
d)
Add the mass number to the number of e-
32.
If an atom has 12 positively charged subatomic particles, which of the following must it also have to be considered a neutral atom?
a)
12 neutrons
b)
12 electrons
c)
12 protons
d)
24 protons and neutrons
33.

An atom has 10 protons, 15 neutrons and 10 electrons what is its mass number.

a)

20

b)

10

c)

35

d)

25

34.
The atomic number of an element that has 9 protons, 9 electrons, and 10 neutrons is _____.
a)
9
b)
10
c)
19
d)
28
35.
An element with a mass number of 11 and an atomic number of 5 has how many neutrons?
a)
11
b)
5
c)
6
d)
16
36.
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
37.
An atom has an atomic number of 15 and a mass number of 31. How many protons are there in the atom?
a)
15
b)
31
c)
16
d)
47
38.

Which of the following determines the identity of an element?

a)

number of protons

b)

atomic mass

c)

number of neutrons

d)

number of shells

39.
What is the atomic number of the atom pictured? 
a)
9
b)
10
c)
18
d)
19
40.

How many protons does indium have?

a)

49

b)

66

c)

114

d)

115

41.

Cations have what charge?

a)

+

b)

-

42.

Anions are what charge?

a)

+

b)

-

43.

Noble gases are...

a)

Happy and stable because they have full valence electrons

b)

Happy BUT UNSTABLE because they are gases

c)

Not happy because they don't want to be noble

d)

Not happy but stable because they are group number 18

44.

Valence electrons means..

a)

Electrons inside the atoms

b)

Electrons on the outer most energy level

c)

Electrons with no charge

d)

Electrons that are stable

45.

Element Chlorine [Cl] at group #17 have how many valence electrons?

a)

6

b)

7

c)

17

d)

5

46.

Element Chlorine [Cl] will make a(n)...

a)

Cation

b)

Anion

47.

Anions will

a)

lose electrons

b)

gain electrons

48.

Cations will

a)

Lose electrons

b)

Gain electrons

49.

Isotopes behave chemically the same as other same elements

a)

True

b)

False

50.

Isotopes behave physically same with other same elements

a)

True

b)

False

51.

This isotope have how many neutrons?

a)

26

b)

12

c)

14

d)

16

52.

Which of the Chlorine [Cl] is heavier?

a)

Cl-37

b)

Cl-35

53.

For Cl 37, what does the 37 represent?

a)

Number of Protons

b)

Number of Neutrons

c)

Number of Electrons

d)

Atomic Mass Number

54.

Which element is located at period 4 group 6? [click the picture to zoom in]

a)

Cr

b)

Sg

c)

Hf

d)

Ta

55.

What is the planetary model also known as?

a)

Thomson model

b)

Plum pudding model

c)

Bohr model

d)

Nuclear model

56.

Which scientist proposed the Nuclear Model by doing the Gold Foil Experiment?

a)

Rutherford

b)

J.J. Thomson

c)

Bohr

d)

Dalton

57.

Protons are...

a)

Positive charge

b)

Negative charge

c)

Neutral/No charge

58.

Electrons are...

a)

Positive charge

b)

Negative charge

c)

Neutral/No charge

59.

Neutrons are...

a)

Positive charge

b)

Negative charge

c)

Neutral/No charge

60.

Which particles are NOT inside the nucleus of atoms?

a)

Protons

b)

Electrons

c)

Neutrons

61.

What particles determine the mass number?

a)

Protons and electrons

b)

Electrons and neutrons

c)

Protons and neutrons

d)

Protons, neutrons, and electrons

62.

What is the mass number of bromine?

a)

35

b)

45

c)

80

d)

79.904

63.

The atomic number is equal to _.

a)

the number of protons

b)

the number of neutrons only

c)

the total number of protons and neutrons

d)

the number of protons, neutrons, and electrons

64.

How many neutrons does this bromine atom have?

a)

35

b)

45

c)

80

d)

115

65.

What is the mass number of this Neon atom?

a)

10

b)

11

c)

21

d)

20

66.

How many electrons does this magnesium ion have?

a)

24

b)

12

c)

10

d)

14

67.

What changes when an atom becomes an ion?

a)

The number of electrons

b)

The number of protons

c)

The number of neutrons

d)

Both the number of neutrons and electrons

68.

How many neutrons does this Neon atom have?

a)

21

b)

11

c)

10

d)

12

69.

What happened to this Magnesium atom to make it an ion?

a)

It LOST electrons

b)

It GAINED electrons

c)

It GAINED protons

d)

It LOST protons

70.

What is the atomic number of this element?

a)

12

b)

24

c)

23

d)

35

71.

Adding or subtracting neutrons makes the element change into

a)

an ion

b)

a mixture

c)

an isotope

d)

a neutral atom

72.

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

a)

+1

b)

0

c)

-1

d)

-2

73.
The atomic mass is equal to _.
a)
the number of protons only
b)
the number of neutrons only
c)
the total number of protons and neutrons
d)
the number of protons, neutrons, and electrons.
74.

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

a)

26

b)

55.845

c)

56

d)

30

75.
How many neutrons does B (Boron) contain?
a)
5
b)
11
c)
6
d)
10.811
76.
Which wave has a greater frequency?
a)
A
b)
B
77.

State whether true or false.

Every element has its own unique atomic line spectra.

a)

True

b)

False

78.

Wavelength and Frequency are related in that...

a)

they are always the same

b)

when one increases, the other decreases (inversely proportional)

c)

there is no correlation

d)

they both vary in an irregular pattern

79.

What particles in the heated compounds are responsible for the production of the colored light?

a)

proton

b)

neutron

c)

electron

d)

proton and neutron

80.

What subatomic particle is responsible for the spectral lines seen in emission spectra diagrams?

a)

electrons

b)

protons

c)

neutrons

81.

Each element on the periodic table can be identified by its

a)

classification as a solid, liquid or gas.

b)

location on the table.

c)

ability to react to form compounds.

d)

unique spectral "fingerprint."

82.
Which elements are in the unknown sample?
a)
A and B
b)
B and C
c)
A and D
d)
B and D
83.

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

a)

Hydrogen only

b)

Hydrogen & Helium

c)

Calcium only

d)

Hydrogen & Calcium

84.
_____________________light is the only type of EM wave detected by the human eye.
a)
Red
b)
Gamma
c)
Microwave
d)
Visible
85.
Calculate the wavelength of light that has a frequency of 5.2 x 1012 Hz. 
a)
5.8 x 10 -5 m
b)
5.8 x 10 -7 m
c)
5.19 x 10 14 m
d)
1.56 x 10 23 m
86.
High frequency waves have _________ wavelengths.
a)
varying
b)
long
c)
the same
d)
short
87.
If an AM radio station broadcasts at
9.95 x 105 Hz, what is the wavelength of this radiation?
a)
6.59 x 10-28 m
b)
1.01 x 10-6 m
c)
3.32 x 10-3 m
d)
302 m
88.
The distance between two crests or two troughs of a wave is called:
a)
frequency
b)
amplitude
c)
wavelength
d)
hertz
89.
An argon ion laser emits light at 488 nm. What is the frequency of this radiation? (1 nm = 1x10-9m)
a)
4.07 x 10-19 Hz
b)
6.15 x 1014 Hz
c)
1.46 x 102 Hz
d)
2.05 x 106 Hz
90.
A common infrared laser operates at 1.06 x 103 nm. What is the energy of a photon with this wavelength? (1 nm = 1x10-9m)
a)
7.02 x 10^-40 J
b)
6.25 x 10^-28 J
c)
3.54 x 10^-15 J
d)
1.87 x 10^-19 J
91.
Which wave in the diagram has the greatest frequency?
a)
1
b)
2
c)
3
d)
4
92.
Which wave in the diagram has the greatest wavelength?
a)
1
b)
2
c)
3
d)
4
93.
What is the frequency of a photon whose energy is 3.4x10-19J?
a)
8.8x1026 Hz
b)
5.1x1014 Hz
c)
1.9x10-15 Hz
d)
2.3x10-52 Hz
94.

Periodic law states that repeating patterns of chemical properties form when you arrange elements by their:

a)

average atomic mass

b)

atomic number

c)

ion charge

d)

electron configuration

95.

A horizontal row in the periodic table is called a:

a)

group

b)

period

c)

family

d)

row

96.

A vertical column in the periodic table is called a:

a)

group

b)

period

c)

family

d)

row

97.

How many protons does oxygen have?

a)

8

b)

16

c)

32

d)

4

98.

How many electrons does oxygen have when it is neutral?

a)

8

b)

16

c)

32

d)

4

99.

How many valence electrons does oxygen have?

a)

2

b)

8

c)

6

d)

18

100.

How many electrons does oxygen want to gain?

a)

1

b)

2

c)

3

d)

4

101.

Based on oxygen's location on the periodic table, predict its electronegativity:

a)

low electronegativity

b)

medium electronegativity

c)

high electronegativity

d)

no electronegativity

102.

Based on oxygen's location on the periodic table, predict its relative atomic size:

a)

small

b)

medium

c)

large

d)

no size

103.

What type of element is oxygen?

a)

metal

b)

nonmetal

c)

metalloid

d)

transition metal

104.

Which of these is the correct electron configuration for oxygen?

a)

1s2 2s2 2p11s^2\ 2s^2\ 2p^1

b)

2p22p^2

c)

1s2 2s2 2p41s^2\ 2s^2\ 2p^4

d)

2p42p^4

105.

Which of these is the correct orbital diagram for oxygen?

a)
b)
c)
d)
106.

Which of these best describes the periodic trends for electronegativity:

a)

Increases across a period and down a group

b)

Increases across a period and up a group

c)

increases across a period and down a group with a drop-off at the halogens

d)

increases across a period and up a group with a drop-off at noble gases

107.

The trends on the periodic table are dependent on..

a)

how attracted a valence electron is to the nucleus

b)

how attracted valence electrons are to each other

c)

how attracted a valence electrons is to a non valence electron

d)

how attracted a non valence electron is to the nucleus

108.

What makes a valence electron more attracted to the nucleus?

a)

less distance between the nucleus and having less protons

b)

less distance between the nucleus and having more protons

c)

more distance between the nucleus and having less protons

d)

more distance between the nucleus and having more protons

e)

less distance and having more valence electrons

109.

What is the tendency of an atom to attract electrons towards itself in a bond?

a)

atomic radius

b)

ionization energy

c)

shielding

d)

Electronegativity

110.

The higher the ionization energy...

a)

the more attracted the valence electron is to the nucleus so it is harder to remove

b)

the less attracted the valence electron is to the nucleus so it is easier to remove

c)

the more attracted the valence electron is to another electron, so it is harder to remove

d)

the more repelled a valence electron is to another electron, so it is easier to remove

111.

Why does ionization energy decrease going down a group?

a)

Adding more energy levels makes the ve- further from the nucleus so it is easier to remove

b)

There are more valence electrons in the outer shell so the ve- is easier to remove

c)

There are more protons in the nucleus so the ve- is easier to remove

d)

There are less protons in the nucleus so the ve- is easier to remove

112.
Why does electronegativity increase across a period?
a)
Adding more energy levels makes the ve- further from the nucleus
b)
There are more valence electrons in the outer shell
c)
There are more protons  in the nucleus
d)
There are less protons in the nucleus
113.
Which is smaller... Mg or Mg2+ ?
a)
Mg because it gains an energy level
b)
Mg due to extra electron repulsion
c)
Mg2+ because of extra electron repulsion
d)
Mg2+ because it loses an energy level
114.
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
115.
List the following from largest to smallest atomic radius.
P, Cs, Co, Sr
a)
P, Co, Sr, Cs
b)
P, Cs, Co, Sr
c)
Cs, Sr, Co, P
d)
Sr, Cs, Co, P
116.

Why doesn't having more protons increase the attraction down a column?

a)

there are more valence electrons in the outermost energy level

b)

actually, there aren't more protons in the nucleus down the column

c)

as energy levels are added, non-valence electrons block the extra protons from attracting ve-

d)

more neutrons block the extra protons

117.

What happens to atomic radius across a period?

a)

the atoms get bigger because the nucleus is bigger as more protons are added

b)

the atoms get bigger because there are more ve-

c)

the atoms get smaller because with more attraction to the extra protons, the e- cloud moves closer to the nucleus

d)

the atoms get bigger because there are more energy levels

118.

Element Z has more protons than element Y, but both have 4 energy levels. Which statement is true?

a)

Y is smaller and would attract electrons more in a bond

b)

Y is bigger and would attract electrons more in a bond

c)

Z is smaller and would attract electrons more in a bond

d)

Z is bigger and would attract electrons more in a bond

119.

Nitrogen is a _ so it will _ electrons when forming an ion.

a)

metal, lose

b)

metal, gain

c)

nonmetal, lose

d)

nonmetal, gain

120.

Nitrogen will gain _ ve- to have a charge of _.

a)

5 , -5

b)

3, +3

c)

3, -3

d)

5, +5

121.

Which of the following lose all their ve- when forming an ion?

a)

metals

b)

nonmetals

c)

metalloids

d)

depends on how many ve- the element has

122.

Which has a higher electronegativity.. Rb or Sr?

a)

Rb, because with more p+ in its nucleus it attracts e- more

b)

Sr, because with more p+ in its nucleus it attracts e- more

c)

Rb, because with more nrg levels the ve- are closer to/ more attracted to the nucleus

d)

Sr, because with more nrg levels the ve- are closer to/ more attracted to the nucleus

123.

Which has a higher ionization energy.. N or As?

a)

N, because with more p+ in its nucleus it attracts e- more making them harder to remove.

b)

As, because with more p+ in its nucleus it attracts e- more making them harder to remove.

c)

As, because with less nrg levels the ve- are closer to/ more attracted to the nucleus making them harder to remove.

d)

N, because with less nrg levels the ve- are closer to/ more attracted to the nucleus making them harder to remove.

124.

Look at the bohr models of Li and Be. Imagine the first valence electron was already removed from both atoms, and now you are going to remove the second valence electron. The energy required to remove the second valence electron is called second ionization energy. Would lithium or beryllium have a higher second ionization energy ?

a)

Li, because it has more protons

b)

Be, because it has more protons

c)

Li, because the second valence electron comes from an energy level closer to the nucleus

d)

Be, because the second valence electron comes from an energy level closer to the nucleus

e)

Li, because the beryllium has two valence electrons that repel each other

125.
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
126.
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. 
127.
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
128.

Which of the following elements has the smallest atomic radius?

a)

Sulfur

b)

Chlorine

c)

Aluminum

d)

Sodium

129.

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)

130.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
131.
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
132.

Across a period from left to right , atomic radius

a)

decreases

b)

increases

c)

increases, then decreases

d)

decreases, then increases

133.
Why does it take energy to remove electrons?
a)
Because it is attracted to the nucleus
b)
Because it is attracted to other electrons
c)
Because it is trapped in an orbital
d)
Because it does not want to move 
134.
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

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132 questions

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130 questions

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130 questions

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Worksheet

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