wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

C-2 Review

Total questions: 94

Worksheet time: 1hrs 5mins

Name
Class
Date
1.
What is an ion?
a)
A Charged Atom
b)
A Large Atom
c)
A Small Atom
d)
A Cute Atom
2.
Barium atoms want to form...
a)
an anion
b)
a cation
c)
an onion
d)
a cuddly kitten friend
3.
An Arsenic atom wants to form...
a)
An anion
b)
A cation
c)
An onion
d)
A cuddly kitten friend
4.
Why are ions formed?
a)
To make our lives difficult
b)
Because atoms want 8 valence electrons
c)
Because atoms have the same number of protons and electrons
d)
Because atoms gained neutrons
5.
Cations are...
a)
Positive
b)
Negative
c)
Neutral
d)
Purring
6.
Anions are...
a)
Positive
b)
Negative
c)
Neutral
d)
Crying
7.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
8.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
9.
A Silicon atom wants...
a)
3 more electrons
b)
3 less electrons
c)
4 more or less electrons
d)
2 more electrons
10.
A Radium atom wants...
a)
One more electron
b)
One less electron
c)
Two more electrons
d)
Two less electrons
11.
Which particles change the charge in atoms when ions are formed?
a)
Protons
b)
Electrons
c)
Neutrons
d)
Kittens
12.
What is a Rubidium ion's symbol?
a)
Rb-
b)
Rb+
c)
Rb-2
d)
Rb+2
13.
What is the ionic symbol for a phosphorus atom?
a)
P-3
b)
P+3
c)
P-2
d)
P+2
14.
What is the ionic symbol for a Gallium atom?
a)
Ga+3
b)
Ga-3
c)
Ga+2
d)
Ga-2
15.
What is the ionic symbol for Selenium?
a)
Se-2
b)
Se+2
c)
Se-3
d)
Se+3
16.
Which of the following has a -1 charge? 
a)
Aluminum
b)
Bromine
c)
Calcium
d)
Potassium
17.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
18.

Why are ions formed?

a)

To make our lives difficult

b)

Because atoms want to be stable

c)

Because atoms have the same number of protons and electrons

d)

Because atoms gained neutrons

19.

Ionic bonds form between two ions that have

a)

negative charges

b)

positive charges

c)

opposite charges

20.
Cations are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
21.
Anions are _______ that form ____________ ions and __________ electrons.
a)
nonmetals, positive, lose
b)
nonmetals, negative, gain
c)
metals, positive, gain
d)
metals, positive, lose
22.

When an atom loses a valence electron, it becomes a(n) _____________ ion.

a)

positive

b)

negative

c)

neutral

23.

When an atom gains a valence electron, it becomes a(n) _____________ ion.

a)

positive

b)

negative

c)

neutral

24.
Where are metals located on the periodic table?
a)
Blue
b)
Green
c)
Red
25.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
26.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
27.
What is the charge of an atom that has gained one electron?
a)
-1
b)
-2
c)
+1
d)
+2
28.

Nonmetals are

a)

usually cations

b)

usually anions

29.

Metals are:

a)

Usually cations

b)

Usually anions

30.

Cations are _________________ and anions are _______________

a)

metals, nonmetals

b)

nonmetals, metals

31.
What are ionic bonds?
a)
Valence electrons transferred between atoms
b)
Inner most electrons transferred between atoms
c)
Sharing electrons
32.
Atoms that gain electrons become...
a)
negatively charged
b)
positively charged
c)
remain neutrally charged
d)
21
33.
if METALS are more likely to LOSE electrons, they will form ...
a)
anions
b)
neutral atoms
c)
positive ions
d)
negative ions
34.
If an aluminum atom has 13 protons (+) and 10 electrons (-), what is it's charge?
a)
Al3+
b)
Al13+
c)
Al10+
d)
Al10-
35.
Which is most likely to form a negative ion?
a)
an element from group 17
b)
a metal
c)
an element from group 1
d)
an element with atoms that have eight valence electrons
36.
How many valence electrons does Lithium have?
a)
1
b)
2
c)
3
d)
4
37.
How many valence electrons does magnesium have?
a)
1
b)
2
c)
12
d)
24
38.
Which group is very nonreactive?
a)
Noble Gases
b)
Halogens
c)
Alkali Metals
d)
Transition Metals
39.
How many valence electrons do all elements in the Carbon family have?
a)
6
b)
5
c)
4
d)
7
40.
Ionic bonds occur between...
a)
A metal and a nonmetal
b)
Two metals
c)
Two nonmetals
d)
Two gases
41.
In a bond between Sodium and Chlorine, what will the final charges on each ion be?
a)
Sodium -1, Chlorine +2
b)
Sodium +2, Chlorine -1
c)
Sodium +1, Chlorine -1
d)
Sodium -2, Chlorine +2
42.
What bond involves the sharing of electrons?
a)
Ionic
b)
Transitive
c)
Covalent
43.
What types of elements are involved in a covalent bond?
a)
A nonmetal and a metal
b)
Two nonmetals
c)
Gases Only
d)
Metalloids Only
44.
What would the correct chemical formula be for Magnesium + Chlorine?
a)
MgCl
b)
MgCl2
c)
Mg2Cl
d)
2MgCl
45.
What would the correct formula be for Hydrogen + Hydrogen?
a)
2H
b)
H2
46.

Why do elements bond?

a)

To be friends

b)

To create a new element

c)

To become stable

d)

To get bigger

47.
What kind of bond forms when atoms exchange electrons?
a)
ionic
b)
covalent
c)
artificial
d)
univalent
48.
If an atom loses two electrons what charge will it have?
a)
-2
b)
-1
c)
+1
d)
+2
49.

The octet rules states that most elements want to have _____ valence electrons.

a)

2

b)

4

c)

6

d)

8

50.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
51.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
52.
Predict the bond that will form between Sr and S.
a)
Ionic
b)
Covalent
53.

Chemical bond is ...

a)

the physical mixing of two different atoms.

b)

the force that holds two atoms together

c)

the energy used up when two atoms combined.

d)

the temperature that changes the phase of matter.

54.

Which of the following atoms is most likely to bond with another atom?

a)
b)
c)
d)
55.

How many valence electrons does Oxygen (O) have?

a)

6

b)

8

c)

15

d)

16

56.

What does the number 3 represent in 4NH3?

a)

Subscript

b)

Superscript

c)

Coefficient

57.

What does the number 4 represent in 4NH3?

a)

Subscript

b)

Superscript

c)

Coefficient

58.

How many Nitrogen (N) atoms are in 4NH3?

a)

4

b)

1

c)

3

d)

12

59.

How many Hydrogen (H) atoms are in 4NH3?

a)

4

b)

1

c)

3

d)

12

60.

How many total molecules is 4NH3?

a)

4

b)

1

c)

3

d)

12

61.

How many total atoms make up 4NH3?

a)

4

b)

16

c)

3

d)

12

62.

In the equation shown, what are the reactant(s)?

a)

N2 + H2

b)

NH3

63.

In the equation shown, what are the product(s)?

a)

N2 + H2

b)

NH3

64.

Is this equation balanced?

a)

Yes

b)

No

65.

Is this equation balanced?

a)

Yes

b)

No

66.

Is this equation balanced?

a)

Yes

b)

No

67.

To balance an equation you should:

a)

ONLY change subscripts.

b)

ONLY change coefficients.

c)

Change BOTH subscripts and coefficients.

68.

Which of the following is a chemical reaction?

a)

Sodium and chlorine atoms bond to form salt molecules.

b)

Ice melts to form water.

c)

Carbon dioxide freezes to form dry ice.

d)

Salt and water mix to form salt water.

69.

Identify the Reactants in this equation.

a)

A

b)

B

70.

What is a chemical equation?

a)

Describes the number of elements in a compound.

b)

One or two letters that represent the elements on the periodic table.

c)

The number to the lower right of an element that shows the number of atoms bonded.

d)

A written description of a chemical reaction.

71.

______ is the end result of a chemical reaction. (Right Side)

a)

Product

b)

Deleting atoms and matter

c)

Subscript

d)

Reactant

72.

What does the Law of Conservation of Matter state?

a)

Matter cannot be created or destroyed in a chemical reaction, it just changes into something new/changes form.

b)

Matter can only be lost in a chemical reaction.

c)

Matter can only be gained in a chemical reaction.

d)

Matter can be gained and lost in a chemical reaction.

73.

Given the equation:

2Na + S --> Na2S

Name the reactant(s).

a)

Na only

b)

S only

c)

Na2S

d)

2Na + S

74.
Given the equation:
2Na + S --> Na2S
Name the product(s).
a)
Na only
b)
S only
c)
Na2S only
d)
Na and S
75.

Is the equation balanced?: 2H2O + O2 --> 4MgO + 3Fe

a)

yes

b)

no

76.
2 NaBr + 1 Ca(OH)2 ----> 1 CaBr2 + 2 NaOH
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
77.
2 NH3+ 1 H2SO4 ----> 1 (NH4)2SO4
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
78.
3 Pb + 2 H3PO4 ----> 3 H2 + 1 Pb3(PO4)2
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
79.
1 Li3N + 3 NH4NO3 ----> 3 LiNO3 + 1 (NH4)3N
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
80.
3 HBr + 1 Al(OH)3 ----> 3 H­2O + 1 AlBr3
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
81.
Pb + FeSO4 ----> PbSO4 + Fe
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
82.
CaCO3 ----> CaO + CO2
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
83.
P4 +  3 O2 ----> 2 P2O3
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
84.
2 AgNO3 + Cu ----> Cu(NO3)2 + 2 Ag
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
85.
O3  ----> O. + O2
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
86.
Increase in temperature of the reactants can do one of the following
a)
Slow collision frequency
b)
Allow less effective collision between the particles
c)
Cause particles to lose speed
d)
Increase collision between the particles thus increasing the rate.
87.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
88.
Which factors increase the rate of a reaction.
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of these
89.
Smaller particle size allows for a _________ surface area to be exposed for the reaction.
a)
larger
b)
smaller
90.
Increasing the concentration of the reactants will slow down the reaction.
a)
false 
b)
true
91.
Why does a higher temperature increase the rate of a reaction?
a)
it increases both the frequency and energy of particle collisions
b)
it only increases the frequency of particle collisions
c)
it only increases the energy of particle collisions
d)
it reduces the activation energy of the reaction
92.
Products will form faster if____________
a)
the particle size of the reactants are larger.
b)
temperature is decreased.
c)
concentration of the reactants are increased.
d)
the reaction is not stirred.
93.
Which of these will NOT speed up the rate of reaction between a strip of magnesium and hydrochloric acid?
a)
tightly coil up the strip of magnesium
b)
cut up the strip of magnesium
c)
increase the concentration of the hydrocholoric acid
d)
increase the temperature of the hydrocholoric acid
94.

Name the compound AlBr3

a)

aluminum bromide

b)

aluminum tribromide

c)

aluminum bromine

d)

aluminum boride

Similar Resources on Wayground

Earth & Space Ch. 1-3

91 questions

Earth & Space Ch. 1-3

quiz

Worksheet

•

8th Grade

MYP Semester 1 Final

90 questions

MYP Semester 1 Final

quiz

Worksheet

•

10th - 12th Grade

Unit 3 review (P)

92 questions

Unit 3 review (P)

quiz

Worksheet

•

8th Grade

Chemistry Exam Review

90 questions

Chemistry Exam Review

quiz

Worksheet

•

10th - 12th Grade

Biology Fall Final

90 questions

Biology Fall Final

quiz

Worksheet

•

10th Grade

Unit 2 Atoms

93 questions

Unit 2 Atoms

quiz

Worksheet

•

8th Grade

Ch. 19 - Chemical Reactions

89 questions

Ch. 19 - Chemical Reactions

quiz

Worksheet

•

8th - 12th Grade

E/S Q1 Review

90 questions

E/S Q1 Review

quiz

Worksheet

•

9th Grade