Wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Fall Review (On level)

Total questions: 99

Worksheet time: 4hrs 33mins

Name
Class
Date
1.

Isotopes of an element contain an equal number of protons but a different number of ____________________.

a)

neutrons

b)

electrons

c)

atomic numbers

2.

How many protons are in the isotope pictured above?

a)

29

b)

34

c)

63

d)

92

3.

The mass number of an isotope is made up of which subatomic particles?

a)

protons and electrons

b)

protons and neutrons

c)

electrons and neutrons

d)

protons, neutrons and electrons

4.

The atomic number of an element is the total number of which subatomic particle found in the nucleus?

a)

Electron

b)

Neutron

c)

Proton

d)

Neutrons + Protons

5.

An unknown element has two naturally occurring isotopes. One has a mass of 10.01 amu and % abundance of 19.8%. The other has a mass of 10.99 amu and % abundance of 80.2%. Calculate the atomic mass.

a)

1079.6

b)

107.95 amu

c)

21 amu

d)

10.8 amu

6.

Element X has 13 neutrons with a mass number of 28. Element Y has 13 protons. These elements are:

a)

Different elements

b)

Isotopes

7.

What does the 6 represent?

a)

Atomic mass

b)

atomic number

c)

chemical symbol

d)

element name

8.

What is the mass number?

a)

35

b)

18

c)

17

d)

52

9.

A carbon atom contains 4 electrons. What is the net charge of the atom?

a)

  • +10

b)

  • +2

c)

  • -2

d)

0

10.

How many neutrons?

a)

35

b)

18

c)

17

d)

52

11.

What is the mass number of the atom shown in the Bohr model?

a)

11

b)

12

c)

23

d)

Can't be determined

12.
What is the mass number of this atom?
a)
1
b)
3
c)
4
d)
7
13.
What is the atomic number of this atom?
a)
2
b)
4
c)
6
d)
none of the above
14.
How many valence electrons?
a)
2
b)
3
c)
5
d)
10
15.
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
16.

On the periodic table, Groups are

a)

Horizontal rows

b)

Vertical columns

17.

On the periodic table, Periods are

a)

Horizontal rows

b)

Vertical columns

18.

The innermost energy level has a maximum of how many electrons?

a)

1

b)

2

c)

6

d)

8

19.

Which Bohr model represents Neon?

a)
b)
c)
d)
20.

Which 3 things are always equal for an atom?

a)

Electrons, protons, and neutrons

b)

Atomic number, protons, electrons

c)

Mass number, atomic number, protons

d)

Atomic number, neutrons, electrons

21.
What is the formula to solve for the neutron?
a)
Mass + Atomic Number= Neutrons
b)
Mass x Atomic Number = Neutrons
c)
Mass - Atomic Number = Neutrons
d)
Mass + Number of Protons = Neutron
22.
How many neutrons does the an element with an atomic number of 3 and a mass of 6.9 contain?
a)
6.9
b)
4
c)
3
d)
7
23.
Can you round the atomic mass?
a)
Yes, always round the mass
b)
No, never round the mass
c)
Depends on which element
d)
Only round if the number increases
24.
An atom with 19 protons, and 19 electrons and a mass of 39 has how many neutrons?
a)
19
b)
39
c)
20
d)
58
25.

What do the elements highlighted orange have in common?

a)

The same number of protons

b)

The same number of valence electrons

c)

The same number of neutrons

d)

The same number of electrons shells

26.
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
27.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
28.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
29.

Calculate the wavelength of the yellow light emitted by the street light, if the frequency of the radiation is 5.10x1014Hz.

a)

5.12 x 10-7m

b)

5.88 x 10-7 m

c)

4.20 x 1014m

d)

3.0 x 108m

30.

Energy is measured in........

a)

Wavelength

b)

Meters

c)

Joules

d)

Frequency

31.

Calculate the wavelength of blue light emitted by a mercury lamp with a frequency of 6.88 x 1014 Hz.

a)

3.44 x 10-6m

b)

4.36 x 10-7m

c)

3.0 x 108 m

d)

633 m

32.

What is the frequency of light with a wavelength of

4.8 x 10-7 meters?

a)

5.34 x 10-9 Hz

b)

3.0 x 108 Hz

c)

3.21 x 1017 Hz

d)

6.25 x 1014 Hz

33.

The unit of measure for frequency is?

a)

Seconds

b)

Meters

c)

Hertz

d)

Liters

34.

What does "h" stand for?

a)

Speed of Light

b)

Plank's Constant

c)

Speed of Sound

d)

Constant Energy

35.

What is the unit of Energy?

a)

J

b)

Hz

c)

nm

d)

s

36.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
37.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
38.
In the correct Lewis structure for water, how many unshared pairs of electrons will oxygen have?
a)
1
b)
4
c)
3
d)
2
39.
Which of the following elements will NOT be surrounded by an octet of electrons in a correctly drawn Lewis structure?
a)
carbon
b)
oxygen
c)
chlorine
d)
hydrogen
40.
What is the first thing you need to do when drawing Lewis Structures?
a)
Draw your bonds
b)
Count the number of valence electrons
c)
Subtract to make the valence number even
d)
Add to make the valence number even
41.
After drawing in your bonds, what do you do if you don't have enough electrons to get each atom to its octet?
a)
Place dots until everything has eight
b)
Place dots only around the terminal atoms
c)
Add a multiple bond
d)
Have eight only around the central atom
42.
In a Lewis structure, what do you do  with the total number of valence if your ion is 2- charged?
a)
Add 2 to the valence number
b)
Subtract 2 from the valence number
c)
Multiply the valence number by 2
d)
Divide the valence number by 2
43.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
44.

What is a Bohr Model?

a)

a simplified representation of an atom

b)

vertical column in periodic table

c)

horizontal row in periodic table

d)

Only shows the element symbol and it's outer most electron shell

45.

What are the names of the 2 models that we have been using?

a)

Bohr and Newton Structures

b)

Lewis and Caroll Models

c)

Bohr Model & Lewis Dot Structure

d)

Element & Atom structures

46.

Electron live in something called __________.

a)

nucleus

b)

orbits

c)

Shells or Energy levels

d)

Valences

47.

How many electrons can go in the Second energy level?

a)

2

b)

8

c)

18

d)

32

48.

What is a Lewis Dot Structure?

a)

It shows all of the particles in the atom.

b)

Contains protons and neutrons

c)

Only shows the element symbol and it's outer most electron shell

d)

Contains protons and electrons

49.

What is the chart called where all the elements are organized?

a)

Periodic Table

b)

Valence Chart

c)

Bohr Chart

d)

Lewis Chart

50.
A covalent bond is
a)
a bond that shares electrons metallicaly
b)
A bond that shares electrons with non metals
c)
Metalloids bonding
d)
metals and nonmetals bonding
51.
Choose the correct IUPAC formula for the compound lead(II) bromite.
a)
Pb(BrO3)2
b)
Pb(BrO2)
c)
Pb(BrO2)2
d)
Pb(BrO3)
52.
Recall that the ions in ionic compounds combine to form the simplest ratio that gives an overall neutral charge.  What would this ratio be between magnesium and nitride ions?
a)
Mg2N3
b)
Mg3N2
c)
MgN
d)
Mg2N2
53.
An element, X, with the general valence electron configuration 2s22p5 will form what compound with magnesium?  What is the identity of element X?
a)
MgX
The identity of X is oxygen.
b)
XMg
The identity of X is oxygen.
c)
MgX2 
The identity of X is fluorine.
d)
X2Mg
The identity of X is fluorine.
54.
Arsenic pentafluoride is an extremely dangerous toxin, mainly poisoning liver cells. It has an apparent smell that is similar to vinyl chloride gas.  What is the IUPAC name for arsenic pentafluoride?
a)
As5F
b)
AsF5
c)
AsF3
d)
As3F
55.
Choose the pair of names and formulas that do NOT match.
a)
Cl2O7 : dichlorine heptoxide
b)
NO : nitrogen monoxide
c)
N2O5 : dinitrogen pentoxide
d)
SO3 : monosulfur trioxide
56.
Potassium cyanide is highly toxic. The moist solid emits small amounts of hydrogen cyanide due to hydrolysis, which smells like bitter almonds. Not everyone, however, can smell this; the ability to do so is a genetic trait. What is the IUPAC formula for potassium cyanide?
a)
KCN
b)
K(CN)2
c)
K2(CN)
d)
K2(CN)2
57.

Name the molecule in the picture

a)

calcium carbonate

b)

carbonic acid

c)

sodium chloride

d)

nicolodium chloride

58.

How many Aluminum atoms are in Al2O3?

a)

3

b)

5

c)

2

d)

1

59.
What kind of bond forms when atoms share electrons?
a)
ionic
b)
covalent
c)
artificial
d)
univalent
60.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
61.
Why do atoms share electrons?
a)
To attain the electron configuration of a noble gas.
b)
To become ions and take a charge
c)
to increase the mass
d)
it's a nice thing to do.
62.
When an atom loses an electron, it becomes a:
a)
positive ion
b)
negative ion
c)
neutral ion
d)
neutral atom
63.

Does CuS have a covalent bond or ionic bond?

a)

Covalent

b)

Ionic

64.

Does HS have a covalent bond or an ionic bond?

a)

Covalent

b)

Ionic

65.

If Sulfur has 6 valence electrons, what is its oxidation number?

a)

-2

b)

+2

c)

-6

d)

+6

66.

What is the number of electrons MOST atoms want in their valence orbital?

a)

2

b)

6

c)

8

d)

16

67.
What is an interaction that holds 2 atoms together called?
a)
Chemical Bond
b)
Covalent Bond
c)
Ionic Bond
d)
Metallic Bond
68.

What is the name for Fe2S3?

a)

Iron sulfide

b)

Diiron trisulfide

c)

Iron (II) sulfide

d)

Iron (III) sulfide

69.

What is the name of CO?

a)

Carbon oxide

b)

Monocarbon monoxide

c)

Carbon monoxide

d)

Carbon dioxide

70.

What is the formula for dichlorine heptoxide?

a)

Cl2O6

b)

Cl2O7

c)

ClO5

d)

Cl2O9

71.

What is the name of H2SO4?

a)

Hydrosulfuric acid

b)

Sulfuric acid

c)

Sulfurous acid

d)

Hydrogen Sulfate

72.

What is the name of NaOH?

a)

Sodium hydrogen oxide

b)

Sodium acid

c)

Sodium hydroxide

d)

Sodium oxalic acid

73.

What is the formula for calcium hydroxide?

a)

CaOH

b)

Ca(OH)2

c)

Ca2OH

d)

HCa

74.
What two elements make up water?
a)
Helium and oxygen
b)
Hydrogen and oxygen
c)
helium and carbon
d)
oxygen and carbon
75.
What word describes when water is attracted to other substances?
a)
cohesion
b)
adhesion
c)
capillary action
d)
surface tension
76.
When water molecules stick easily to other water molecules, this is called what?
a)
cohesion
b)
adhesion
c)
solution
d)
polar molecule
77.

The __________________ is a property of a system in which two points have opposite characteristics, such as charges (positive/negative) or magnetic poles.

a)

polarity

b)

opposites

c)

cohesion

d)

adhesion

78.
Which end of the water molecule has a slightly positive charge?
a)
the oxygen end
b)
the hydrogen end
c)
both ends are slightly positive
d)
neither end is positive
79.
In a covalent bond, one or more electrons are? 
a)
shared 
b)
lost 
c)
gained 
d)
transferred 
80.
The fact that ice floats on liquid water is due to the fact that water's solid is ___________ than it's liquid form
a)
less polar
b)
more polar
c)
less dense
d)
more dense
81.
A high specific heat means...
a)
It heats up quickly with energy added
b)
It requires more energy to change temperature
82.
How does capillary action happen?
a)
water is polar
b)
it drags other water molecules up the tubes
c)
it sticks to the tubes
d)
ALL OF THESE REASONS
83.
Which water quality indicator will be most impacted by burning fossil fuels and air pollution?
a)
nitrates
b)
pH (water will be more acidic)
c)
Dissolved oxygen
d)
turbidity
84.
Water is a universal solvent because it...
a)
It can be found anywhere
b)
It freezes when it gets cold
c)
floats when frozen
d)
Dissolves most substances
85.
Which of the following is LEAST likely to dissolve in water?
a)
nonpolar fats and oils
b)
polar sugar molecules
c)
salt made of a positive sodium ion and a negative chloride ion
d)
all of the substances will dissolve easily in water
86.

The hydrogen atoms in a water molecule are ________________ charged.

a)

not

b)

negatively

c)

neutrally

d)

positively

87.

A paperclip floating on water is an example of what property of water?

a)

capillary action

b)

surface tension

c)

universal solvent

d)

specific heat index

88.
Ability to rust is this type of property:
a)
Physical property
b)
Chemical property
89.

A beaker cracks while heating. What is the best immediate action to take?

a)

Turn off heat and inform the teacher

b)

Continue heating and observe carefully

c)

Add cold water to cool the beaker

d)

Pick it up quickly with bare hands

90.

In a chemistry lab, what is the primary purpose of Personal Protective Equipment (PPE) such as goggles, gloves, and lab coats?

a)

To identify students by class section and seating chart

b)

To speed up procedures by reducing cleanup time

c)

To prevent exposure to chemical hazards and physical injury

d)

To improve experimental accuracy and reaction yield

91.

What is ionization energy?

a)

The amount of energy required to remove an electron from a gaseous atom.

b)

The energy released when an electron is added to a gaseous atom.

c)

The energy required to add a neutron to a nucleus.

d)

The energy needed to split a molecule into atoms.

92.

Describe the ionization energy trend from the Periodic Table.

a)

I.E. decreases down a group and increases across a period.

b)

I.E. increases down a group and decreases across a period.

c)

I.E. remains constant down a group and increases across a period.

d)

I.E. decreases down a group and remains constant across a period.

93.

Explain why it requires more energy to remove each subsequent electron after the first. It always requires more energy to remove a 2nd or 3rd electron because they are more attracted to a positive ion than a neutral atom.

a)

Because the electrons are more attracted to a positive ion than a neutral atom.

b)

Because the electrons are less attracted to a positive ion than a neutral atom.

c)

Because the electrons are equally attracted to a positive ion and a neutral atom.

d)

Because the electrons are not attracted to a positive ion at all.

94.

There is a very large increase of ionization energy whenever an electron is removed from an atom/ion that is ____.

a)

iso electronic with a noble gas.

b)

in a high energy state.

c)

part of a covalent bond.

d)

in a metallic state.

95.

If an atom loses electrons, it becomes a negative ion.

(a)  
Choose from the below words
True
False
96.

Which of the following factors does not directly influence the ionization energy of an atom?

a)

Atomic radii

b)

Nuclear charge

c)

Shielding effect

d)

Neutrons

97.

Which element has the greatest ionization energy: Aluminum (Al)    or    Chlorine (Cl)?

a)

Aluminum (Al)

b)

Chlorine (Cl)

98.
Which of these elements has the lowest ionization energy?
a)
Oxygen (O)
b)
Boron (B)
c)
Carbon (C)
d)
Fluorine (F)
99.
Which of these elements has the highest ionization energy?
a)
Lithium (Li)
b)
Potassium (K)
c)
Francium (Fr)
d)
Sodium (Na)

Similar Resources on Wayground

Unit 1 Atomic Theory Review

102 questions

Unit 1 Atomic Theory Review

quiz

Worksheet

•

10th Grade

Chemistry CSEC MC

100 questions

Chemistry CSEC MC

quiz

Worksheet

•

9th - 12th Grade

Summer 2021 Chemistry Final

100 questions

Summer 2021 Chemistry Final

quiz

Worksheet

•

11th Grade

CH 2: Chemistry for A&P

100 questions

CH 2: Chemistry for A&P

quiz

Worksheet

•

9th - 12th Grade

Ionic and Covalent Bonds

104 questions

Ionic and Covalent Bonds

quiz

Worksheet

•

9th - 12th Grade

3.2 PRACTICE TEST

100 questions

3.2 PRACTICE TEST

quiz

Worksheet

•

10th Grade

General Chemistry Concepts

100 questions

General Chemistry Concepts

quiz

Worksheet

•

9th - 11th Grade

Chemistry Final

100 questions

Chemistry Final

quiz

Worksheet

•

8th Grade - University