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Grade 10 Chapter 7.1 and 7.2 Chemistry

Total questions: 115

Worksheet time: 2hrs 57mins

Name
Class
Date
1.

What is a positive ion called?

a)

anion

b)

cation

c)

isotope

d)

covalent

2.

What is a negative ion called?

a)

anion

b)

cation

c)

covalent

d)

isotope

3.

How many electrons would a Nitrogen ion gain/lose? If it has 5 valence electrons.

a)

lose 5

b)

gain 5

c)

lose 3

d)

gain 3

4.

What is the ion formed from Sulfur? If it has 6 valence electrons.

a)

S+2

b)

S-2

c)

S+6

d)

S-6

5.

How many electrons would a Calcium ion gain/lose? If it has 2 valence electrons.

a)

lose 1

b)

gain 1

c)

lose 2

d)

gain 2

6.

If an atom loses electrons, the charge will be positive.

a)

true

b)

false

7.

A Bromine ion gains 1 electron, which of the following is the correct symbol for a Bromine ion?

a)

Br-1

b)

Br+1

c)

Br+7

d)

Br-7

8.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
9.

An atom with 2 protons, 3 neutrons, and 4 electrons has a charge of ____.

a)

+2

b)

-2

c)

+3

d)

0

10.

If an element has 3 valence electrons, what charge will likely form on its ion ?

a)

+3

b)

+5

c)

-3

d)

-5

11.
Ions are: 
a)
atoms with a positive or negative charge
b)
atoms with no charge
c)
atoms with ONLY a positive charge
d)
atoms with ONLY a negative charge
12.

Na has 1 valence electron. It will have a charge of _______

a)

+1

b)

+2

c)

-1

d)

-2

13.

Be has 2 valence electron. It will have a charge of _______

a)

+1

b)

+2

c)

-1

d)

-2

14.

Ca has 2 valence electron. It will have a charge of _______

a)

+1

b)

+2

c)

-1

d)

-2

15.

Al has 3 valence electron. It will have a charge of _______

a)

+3

b)

-3

c)

+2

d)

-2

16.

P has 5 valence electron. It will have a charge of _______

a)

+3

b)

-3

c)

+2

d)

-2

17.

S has 6 valence electron. It will have a charge of _______

a)

-2

b)

-1

c)

+1

d)

+2

18.

Iodine has 7 valence electron. It will have a charge of _______

a)

-2

b)

-1

c)

+1

d)

+2

19.

F has 7 valence electron. It will have a charge of _______

a)

-2

b)

-1

c)

+1

d)

+2

20.

Oxygen has 6 valence electron. It will have a charge of _______.

a)

+1

b)

-1

c)

+2

d)

-2

21.
What is an ion?
a)
A Charged Atom
b)
A Large Atom
c)
A Small Atom
d)
A Cute Atom
22.
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
23.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
24.

What is the charge of a sodium ion?

a)

+2

b)

+1

c)

-1

d)

-2

25.
Group 17 always has ions with a charge of 
a)
+1
b)
+2
c)
-1
d)
-2
26.
What charge will an Oxygen ion have? 
a)
+1
b)
-1
c)
+2
d)
-2
27.
If an element has 3 valence electrons, what charge will likely form on its ion ?
a)
+3
b)
+5
c)
-3
d)
-5
28.
Which of the following has a -3 charge?
a)
Boron
b)
Fluorine
c)
Nitrogen
d)
Neon
29.
charge of lithium ion
a)
-2
b)
-1
c)
+1
d)
+2
30.
charge of beryllium ion
a)
-2
b)
-1
c)
+1
d)
+2
31.
Which of the following has a -1 charge? 
a)
Aluminum
b)
Bromine
c)
Calcium
d)
Potassium
32.
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
33.
Cations are...
a)
Positive
b)
Negative
c)
Neutral
d)
Purring
34.
Anions are...
a)
Positive
b)
Negative
c)
Neutral
d)
Crying
35.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
36.
Which particles change the charge in atoms when ions are formed?
a)
Protons
b)
Electrons
c)
Neutrons
d)
Kittens
37.
What is the ionic symbol for a Caesium atom?
a)
Cs+
b)
Cs-
c)
Cs+2
d)
Cs-2
38.
Make sure you get enough Potassium in your diet!
a)
Huh?
b)
K
c)
I <3 bananas
d)
Sure
39.
Metals tend to 
a)
gain electrons
b)
lose electrons
40.
If my charge becomes 2+ what does that say about me?
a)
I am stealing 2 electrons
b)
I am losing 2 electrons
c)
I am in period 2
d)
I have an atomic # of 2
41.
If I gain electrons I become
a)
Positive because I've added to my atom
b)
negative because I've added electrons
c)
same because i'm balanced
d)
equal because now I have electrons
42.
When metals bond with non-metals they form what type of bonds
a)
covalent
b)
ionic
c)
cooperative
d)
lewis
43.
How do the following two elements bond together?
Na1+  F1-         
a)
NaF
b)
NaF3
c)
Na3F
d)
Na1F2
44.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
45.
How do the following two elements bond together?
K1+  S2- 
a)
KS
b)
K8S
c)
K6S3
d)
K2S
46.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
47.
PbS2
a)
lead sulfide
b)
lead sulfur
c)
lead II sulfide
d)
lead IV sulfide
48.
AgF
a)
silver fluoride
b)
silver fluorine
c)
monosilver monofluoride
d)
silver monofluorine
49.
When a nonmetal gains electrons, it becomes this type of ion.
a)
Anion
b)
Cation
50.
When a metal loses electrons, it becomes this type of ion.
a)
anion
b)
cation
51.
When an ionic compound is formed, its charge is 
a)
negative
b)
neutral (no charge)
c)
positive
52.
What is the formula for magnesium chloride?
a)
MgCl
b)
Mg2Cl
c)
MgCl2
d)
Mg(ClO3)2
53.
The chemical formula for an ionic compound of potassium and oxygen is
a)
KO.
b)
K2O.
c)
K2O2.
d)
KO2.
54.
The first step in naming an ionic compound is always...
a)
Naming the anion
b)
Changing the ending to -ide
c)
Naming the cation
d)
Writing the cation charge
55.
Name the following ionic compound: BeCl2
a)
beryllium chlorine
b)
beryllium II chloride
c)
beryllium chloride
d)
beryllium dichloride
56.
How many valence electrons does a bromine atom have?
a)
1
b)
2
c)
6
d)
7
57.
What is the correct formula for the compound, lithium oxide?
a)
LiO
b)
Li2O
c)
LiO2
d)
Li2O2
58.
What is the charge on the simple (single atom) ion that sulfur forms?
a)
1-
b)
2+
c)
3+
d)
2-
59.
What is the formula for the compound formed by magnesium ions and nitrogen ions?
a)
MgN
b)
Mg2N3
c)
Mg3N2
d)
MgN3
60.
How many valence electrons for Ca?
a)
1
b)
2
c)
3
d)
4
61.
How many valence electrons for S?
a)
8
b)
7
c)
6
d)
4
62.
How many valence electrons for Ne?
a)
8
b)
7
c)
6
d)
4
63.
How many valence electrons for Potassium?
a)
1
b)
2
c)
6
d)
4
64.

How many valence electrons does an atom need to have a stable electron configuration?

a)

2

b)

4

c)

6

d)

8

65.
If an atom does not have a stable octet, what will it do?
a)
form bonds with other atoms
b)
nothing
c)
fall apart
d)
gain or lose protons
66.
Which type of bond transfers electrons?
a)
ionic
b)
covalent
c)
metallic
67.
What ion does a sulfur atom form
a)
+1
b)
+2
c)
-1
d)
-2
68.
What will be the chemical formula for 
K+1 and Cl-1
a)
KCl
b)
K2Cl
c)
KCl2
d)
KCl3
69.
What will be the chemical formula for 
Li+1 and S-2
a)
LI2S
b)
LiS2
c)
LiCl
d)
Li3Cl
70.
What will be the chemical formula for 
Ca+2  and Br-1
a)
CaBr2
b)
Ca2Br
c)
CaBr
d)
CaBr3
71.
What will be the chemical formula for 
K and N
a)
K3N
b)
KN
c)
KN3
d)
K2N
72.
What are electrons in the outermost energy level called?
a)
valence electrons
b)
bonus electrons
c)
protons
d)
orbitals
73.
What ion does a Ca atom form
a)
+1
b)
+2
c)
-1
d)
-2
74.
What ion does a Nitrogen atom form
a)
-3
b)
+2
c)
+3
d)
-1
75.
What is the correct term for "atom with more protons than electrons"?
a)
positive ion (cation)
b)
negative ion (anion)
c)
neutral atom
d)
stable atom
76.
What is the correct term for "atom with more electrons than protons"?
a)
positive ion (cation)
b)
negative ion (anion)
c)
neutral atom
d)
stable atom
77.

Which groups tend to not form ions? Check all that apply

a)

1A

b)

4A

c)

3A

d)

7A

e)

8A

78.
Mg2+ and Cl- create...
a)
Mg2Cl
b)
MgCl2
c)
Mg2Cl2
d)
MgCl
79.
H+ and S2- create...
a)
H2S
b)
HS2
c)
H2S2
d)
HS
80.
Ca2+ and N3- create...
a)
Ca2N3
b)
Ca3N2
c)
CaN3
d)
Ca2N
81.
Li+ and P3- create...
a)
Li3P
b)
LiP3
c)
LiP
d)
Li2P
82.

Pb4+ and O2- create...

a)

Pb2O

b)

PbO2

c)

Pb2O2

d)

PbO

83.

Na+ and Cl- create...

a)

Na2Cl

b)

NaCl2

c)

Na2Cl2

d)

NaCl

84.

K+ and S2- create...

a)

K2S

b)

KS2

c)

K2S2

d)

KS

85.

Mg2+ and O2- create...

a)

Mg2O3

b)

MgO2

c)

MgO

d)

Mg2O

86.

Rb+ and P3- create...

a)

Rb3P

b)

RbP3

c)

RbP

d)

Rb2P

87.

Ca2+ and F- create...

a)

Ca2F2

b)

Ca3F

c)

CaF2

d)

Ca2F

88.

Al3+ and P3- create...

a)

Al3P

b)

AlP3

c)

AlP

d)

Al2P

89.

Ba2+ and Cl- create...

a)

Ba2Cl

b)

BaCl2

c)

Ba2Cl2

d)

BaCl

90.

Sr2+ and I- create...

a)

Sr2I

b)

SrI2

c)

Sr2I2

d)

SrI

91.

H+ and N3- create...

a)

H3N

b)

HN2

c)

H2N2

d)

HN

92.

Ba2+ and P3- create...

a)

Ba2P3

b)

Ba3P2

c)

BaP3

d)

Ba2P

93.

Lithium and Fluorine create...

a)

LiF

b)

LiF2

c)

Li2F

d)

Li2F2

94.

Potassium and Sulfur create...

a)

KS

b)

KS2

c)

K2S

d)

K2S2

95.
The force that holds two atoms together; may form by the attraction of a positive ion for a negative ion or by sharing electrons.
a)
chemical bond
b)
ionic compound
c)
metallic bond
d)
formula unit
96.
A 3-D geometric arrangement of particles in which each positive ion is surrounded by negative ions and each negative ion is surrounded by positive ions; vary in shape due to sizes and relative numbers of the ions bonded
a)
crystal lattice
b)
electron sea model
c)
lattice energy
d)
delocalized electron
97.
An ionic compound whose aqueous solution conducts electric current.
a)
electrolyte
b)
crystal lattice
c)
formula unit
d)
lattice energy
98.
The simplest ratio of ions represented in an ionic compound.
a)
formula unit
b)
ionic compound
c)
chemical bond
d)
metallic bond
99.
The electrostatic force that holds oppositely charged particles together in an ionic compound.
a)
ionic bond
b)
formula unit
c)
chemical bond
d)
metallic bond
100.
Compounds that contain ionic bonds.
a)
ionic compounds
b)
ionic bonds
c)
formula unit
d)
chemical bond
101.
The energy required to separate one mole of the ions of an ionic compound, which is directly related to the size of the ions bonded and is also affected y the charge of the ions.
a)
lattice energy
b)
alloy
c)
oxidation number
d)
delocalized electron
102.

The following properties are all characteristics of ionic compounds EXCEPT

a)

high melting and boiling points

b)

soft

c)

crystal lattice structure

d)

conduct electricity when dissolved in water

103.
Which of the following is a property of an ionic compound?
a)
high melting point
b)
soft
c)
malleable
d)
liquid at room temperature
104.

What type of forces hold on an ionic lattice together?

a)

Electrostatic attraction forces

b)

Covalent bond

c)

Metallic bond

d)

Van der Waals forces

105.

What properties does an ionic compound have?

a)

A low boiling point and it conducts electricity when dissolved in water

b)

A high melting and it conducts electricity when liquid

c)

A high boiling point and it conducts electricity when solid

106.

Ionic compounds conduct electricity when dissolved in water. Which statement below best explains the property?

a)

Ions are free to move.

b)

Electrons are free to move.

c)

Bonds are strong.

d)

There are weak intermolecular forces of attraction.

107.

Which three of the following are features of ionic compounds? (click 3 boxes)

a)

They have bonds between metals and non-metals.

b)

They have bonds between two non-metals.

c)

They form simple molecular structures.

d)

They form giant ionic lattices.

e)

They involve the transfer of electrons.

108.

Ionic compounds form giant ionic lattices. What forces hold the giant ionic lattices together?

a)

strong frictional forces between the surfaces of the atoms

b)

strong magnetic forces of attraction between the poles of ions

c)

strong electrostatic forces of attraction between oppositely charged ions

109.

Why do ionic compounds have high melting and boiling points?

a)

Their ions are free to move.

b)

Their ions are held in fixed positions.

c)

They have many strong bonds.

d)

They have many weak bonds.

110.

True or false? Ionic compounds have high melting points.

a)

true

b)

false

111.

True or false? Ionic compounds have low boiling points.

a)

true

b)

false

112.

True or false? Ionic compounds conduct electricity when they are in their solid state.

a)

true

b)

false

113.

Why do ionic compounds NOT conduct electricity when they are in their solid state?

a)

Their ions are free to move.

b)

Their ions are held in fixed positions.

c)

Their electrons are free to move

d)

Their electrons are held in a fixed state

114.

Why do ionic compounds conduct electricity when they are molten or dissolved?

a)

Their ions are free to move.

b)

Their ions are held in fixed positions.

c)

Their electrons are free to move

d)

Their electrons are held in a fixed state

115.

Magnesium oxide is insoluble in water. Can magnesium oxide conduct electricity?

Select yes or no and a reason.

a)

Yes

b)

No

c)

Magnesium oxide can be heated so that it melts and conducts electricity.

d)

Magnesium oxide doesn't dissolve, so it stays in its solid state and doesn't conduct electricity.

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