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Ionic Bonding Test

Total questions: 139

Worksheet time: 7hrs 13mins

Name
Class
Date
1.

How many CORE ELECTRONS does Chlorine have?

a)

2

b)

4

c)

8

d)

10

e)

17

2.

How many VALENCE ELECTRONS does Chlorine have?

a)

2

b)

7

c)

8

d)

10

e)

17

3.

Ionic bonds are formed when electrons get

a)

Shared between two atoms

b)

Removed from both atoms

c)

Transferred from one atom to another

d)

Added to both atoms

4.

How many valence electrons does Mg have? (use the PTable)

a)

1

b)

2

c)

3

d)

4

e)

5

5.

How many valence electrons does Po (Polonium) have? (Use your PTable)

a)

2

b)

4

c)

6

d)

8

6.

Ionic bonds typically form between

a)

A metal and a nonmetal

b)

Two nonmetals

c)

Two metals

d)

A metalloid and a metal

7.

Atoms are most stable when their outer shell is complete.

a)

True

b)

False

8.

Why do elements form chemical bonds?

a)

Because they're friendly

b)

To create a new element

c)

To become stable

d)

Because they all need to gain more electrons

9.

What is the correct formula for Sodium Chloride?

a)

SCl

b)

NaCl

c)

SC

d)

NaCl2

10.

Name this ionic compound: Al2O3

a)

Dialuminum oxide

b)

Aluminum oxygen

c)

Oxygen Aluminide

d)

Aluminum oxide

11.

If you were to draw the lewis dot structure for Germanium (Ge), how many dots would you put around it?

a)

2

b)

4

c)

6

d)

8

12.

Cations _______ electrons, becoming _______ charged.

a)

Gain; positively (+)

b)

Gain; negatively (-)

c)

Lose; positively (+)

d)

Lose; negatively (-)

13.

Anions ____ electrons, becoming _____ charged.

a)

Gain; positively (+)

b)

Gain; negatively (-)

c)

Lose; positively (+)

d)

Lose; negatively (-)

14.

Write the chemical formula for K and Br (potassium bromide).

a)

KBr

b)

K2Br

c)

KBr3

d)

KBr2

15.

Write the chemical formula for Na and S (sodium sulfide).

a)

NaS

b)

S2S2

c)

Na2S

d)

NaS2

16.

Metals (like Na) typically _____ electrons in the formation of ionic bonds.

a)

Gain

b)

Lose

c)

Keep the same

17.

Nonmetals (like Cl) typically ____ electrons when they form ionic bonds.

a)

Gain

b)

Lose

c)

Keep the same

18.

Why are there two sodiums (Na), in the formation of this ionic compound?

a)

There always has to be 2 metals

b)

The overall charge needs to add up to 4

c)

The overall charge has to be 0

d)

It needs to have more metal atoms than nonmetal

19.

Using the model for the formation of Scandium Fluoride (an ionic compound), write the chemical formula.

a)

Sc3F

b)

Sc3F3

c)

Sc+3F-1

d)

ScF3

20.

Using the model, write the chemical formula for an ionic compound that has Mg and Cl.

a)

MgCl2

b)

Mg2Cl2

c)

Mg+2Cl-1

d)

Mg2Cl2

21.

Ionic bonds are formed between...

a)

Non - metals

b)

A metal and a non-metal

c)

Metals

22.

Which of the below is an ionic compounds?

a)

Ni

b)

MgCl2

c)

H2O

d)

CH4

23.

How is an ionic bond formed?

a)

Sharing of electrons

b)

Delocalised electrons

c)

Transfer of electrons

24.

An example of an ionic compound is Sodium Chloride, which is made from Na+ and Cl- ions. Why do these ions form an ionic bond?

a)

They have like charges

b)

They are from the same group

c)

They are from the same period

d)

They have opposite charges

25.
In the chemical formula for an ionic compound, which item is written first?
a)
positive ion
b)
negative ion
c)
subscript
d)
the female
26.

Lead Chloride is an ionic compound, made up from Pb2+ ions and Cl- ions. Which is the correct formula for this compound?

a)

PbCl3

b)

PbCl

c)

PbCl4

d)

PbCl2

27.

Which of the following is true for ionic bonding & ionic compounds? (3 correct statements)

a)

They must be made of ions with like charges.

b)

The negative ion must be written first.

c)

Compounds must have an overall charge of zero.

d)

They are made of metals and nonmetals.

e)

The positive ion must be written first.

28.

Which properties are all characteristics of ionic compounds?

a)

solids with high melting and boiling points

b)

soft solids which are highly malleable

c)

when solid, the ions are held in place so the compounds cannot conduct electricity

d)

conduct electricity when dissolved or molten

29.

What properties does an ionic compound have?

a)

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

b)

A high melting point and it conducts electricity when molten or dissolved

c)

A high boiling point and it conducts electricity when solid

30.

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

31.

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.

32.

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 which require a large amount of heat energy to overcome these strong bonds.

d)

They have weak bonds which require a little amount of heat energy to overcome these weak bonds.

33.

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.

34.

Be and F can combine to form BeF2, an ionic compound. Select ALL the true statements.

a)

Each Be atom loses two electrons from the outer shell.

b)

Each F atom gains two electrons from Be.

c)

The force holding the ionic compound together is electrostatic attraction.

d)

Each F ion has a charge of -1

35.

Select all the true statements:

a)

Each outer shell electron in Cl is represented by a cross.

b)

In Na, the total charge is -2.

c)

Na+ and Cl- are held together by electrostatic attraction.

d)

Na+ has a full outer shell of electrons.

36.

Match the following to form true statements:

a)

When solid, ionic compounds

1.

cannot conduct electricity

b)

When melted ionic compounds

2.

can conduct electricity

c)

Ionic compounds have

3.

high melting and high boiling points

d)

There are many strong bonds

4.

between ions in an ionic compound.

e)

Elements in group 1 of the periodic table form ions

5.

with a charge of 1+

37.

Sodium Oxide is Na2O. Meaning there are 2 Na present for every O in the ionic compound. As the Oxygen ion has a charge of -2, what charge does each Sodium ion have?

a)

-1

b)

-2

c)

+2

d)

+1

38.

This is an image of the giant ionic lattice representing Sodium Chloride, what is represented by the +?

a)

Cl ion

b)

Cl atom

c)

Na atom

d)

Na ion

39.

What is the correct formula for aluminium oxide? Aluminium is in group 3 and oxygen is in group 6.

a)

Al₂O₃

b)

AlO

c)

AlO₄

d)

Al₂O

e)

Al₃O₂

40.

Which of the following is NOT a property of ionic compounds?

a)

They conduct electricity when molten

b)

They conduct electricity when in solution

c)

They have high boiling points

d)

They are insoluble in water

41.
In the chemical formula for an ionic compound, which item is written first?
a)
positive ion
b)
negative ion
c)
subscript
d)
the female
42.
Magnesium bromide is an ionic compound with the chemical formula MgBr₂.  What does the "2" tell you?
a)
There are 2 bromide ions for every magnesium ion
b)
Bromide has a 2- charge
c)
Bromide has a 2+ charge
d)
There are 2 magnesium ions to every bromide ion
43.
Which of the following is a characteristic property of ionic compounds?
a)
They form hard, brittle crystals with characteristic shapes
b)
They have low melting points
c)
They have low boiling points
d)
They contain no charged particles
44.
In what form can an ionic compound conduct electricity?
a)
when dissolved in water
b)
as a solid
c)
as a crystal
d)
when warmed slightly
45.
Which is the correct name for CaBr2?
a)
Calcium Bromine
b)
Bromine Calcium
c)
Calcium Bromide
d)
Carbon and Bromine
46.
What is the formula of Sodium oxide?
a)
Na2O
b)
NaO2
c)
Na2O2
d)
Na2O
47.
What is the formula of calcium oxide?
a)
CaO2
b)
CaO
c)
Ca2O
d)
CO
48.
An ionic bond is the attraction between:
a)
oppositely charged ions
b)
similarly charged ions
c)
neutral ions
d)
neutral atoms
49.
What is the formula for magnesium phosphide?
a)
Mg3P2
b)
Mg2P3
c)
Mg2(PO4)3
d)
Mg3(PO4)2
50.
Write the formula for barium + nitrogen
a)
Ba2N3
b)
Ba3N2
c)
BaN
d)
BaN3
51.
Write the correct chemical formula for Ag +  and  Br -
a)
AgBr
b)
silver bromide
c)
Ag2Br2
d)
gold bromide
52.
What is the formula for tin (II) nitride?
a)
Sn3N2
b)
SnN2
c)
Sn3N
d)
SnN
53.
Name the following ionic compound: MgSO4
a)
magnesium sulfoxide
b)
magnesium sulfide
c)
magnesium sulfate
d)
magnesium oxide
54.
If copper (II) and phosphate bond together, the resulting chemical formula would be:
a)
Cu2(PO4)3
b)
CuPO4
c)
Cu3(PO4)2
d)
Cu3PO4
55.

What is the chemical name for Cu(OH)3

a)

Copper Hydroxide

b)

Copper Hydroxide III

c)

Copper III Hydroxide

d)

Copper I Hydroxide III

56.
This type of model shows only the valence electrons of an element? 
a)
Bohr diagram 
b)
Childers model
c)
Lewis-dot diagram 
d)
What is a valence electron again?
57.
Which of the following combinations would need roman numerals in the name?
a)
potassium + fluorine
b)
beryllium + oxygen
c)
boron + iodine
d)
silver + oxygen
58.
What is the formula for aluminum sulfide?
a)
Al2S3
b)
Al3S2
c)
Al2SO4
d)
AlS
59.
What is the name for CaS?
a)
calcium sulfate
b)
calcium sulfide
c)
calcium monosulfide
d)
monocalcium monosulfide
60.
What is the name for LiI?
a)
lithium oxide
b)
lithium iodide
c)
lithium monoiodide
d)
monolithium iodide
61.
Refer to the image. Which diagrams correctly represent the transfer of electrons in ionic bonding?
a)
Diagram 3 and 4
b)
Diagram 1 and 2
c)
Diagram 1 and 4
d)
Diagram 2 and 3
62.
What is the correct name of CaBr2?
a)
calcium bromine
b)
calcium baride
c)
monocalcium dibromide
d)
calcium bromide
63.
In the compound aluminum oxide, which is the cation?
a)
Al+3
b)
Al
c)
O-2
d)
O
64.
For the ions shown in the cartoon,  the strongest force of attraction would be formed between.
a)
Li + and F -
b)
Na + and Cl -
c)
Cs + and F -
d)
Cs + and Br -
65.
Which of the following is NOT a property of ionic compounds?
a)
They conduct electricity when molten
b)
They conduct electricity when in solution
c)
They have high boiling points
d)
They are insoluble in water
66.
A(n) _________ is an ion with a positive (+) charge.
a)
anion
b)
cation
c)
ion
d)
solute
67.
Magnesium bromide is an ionic compound with the chemical formula MgBr₂.  What does the "2" tell you?
a)
There are 2 bromide ions for every magnesium ion
b)
Bromide has a 2- charge
c)
Bromide has a 2+ charge
d)
There are 2 magnesium ions to every bromide ion
68.
Which of the following is a characteristic property of ionic compounds?
a)
They form hard, brittle crystals with characteristic shapes
b)
They have low melting points
c)
They have low boiling points
d)
They contain no charged particles
69.
Nitrogen will ____ electrons when forming an ionic bond.
a)
gain 1
b)
lose 1
c)
gain 3
d)
lose 3
70.
What is the formula of Sodium oxide?
a)
Na2O
b)
NaO2
c)
Na2O2
d)
Na2O
71.
Elements in Group 1 lose one electron to form ions with a(n) _________________ charge.
a)
1+
b)
2+
c)
0
d)
1-
72.
Definition: the electrostatic attraction between positive and negative ions in a compound
a)
chemical bond
b)
atomic bond 
c)
covalent bond
d)
ionic bond
73.
Alkali metal elements will tend to become an ion with a charge of _____
a)
1+
b)
1-
c)
2+
d)
2-
74.
Definition: the simplest whole number ratio of atoms or ions of the elements in anionic compound
a)
formula unit
b)
atomic unit 
c)
chemical unit
d)
ionic unit
75.
Pure ionic compounds are _____
a)
electrically neutral
b)
charged positively
c)
charged negatively
d)
strongly charged
76.
The most common model of ions shows them as spheres arranged in a regular three-dimensional pattern called _____
a)
a crystal lattice
b)
a wireframe lattice
c)
a crystal cube
d)
an ordered pair
77.
Concerning their physical properties, ionic substances are often _____
a)
hard and brittle
b)
soft and brittle
c)
hard and malleable
d)
soft and malleable
78.
A group 16 element will tend to become an ion with a charge of _____
a)
1+
b)
1-
c)
2+
d)
2-
79.
Predict the charge on the most stable ion formed by calcium
a)
1+
b)
1-
c)
2+
d)
2-
80.
Predict the charge on the most stable ion formed by phosphorus
a)
1+
b)
1-
c)
2+
d)
3-
81.
Name this compound:
NiPO4
a)
Nickel (I) phosphate
b)
Nickel (II) phosphate
c)
Nickel (IV) phosphate
d)
Nickel (III) phosphate
82.
calcium hydroxide
a)
Ca2OH
b)
CaOH2
c)
Ca(OH)2
d)
correct answer is not given
83.
The correct formula for MnO4 -  and  Ca+2
a)
(MnO4)2Ca
b)
MnO4Ca2
c)
Ca2MnO4
d)
Ca(MnO4)2
84.
The name of FeCl₂ is
a)
iron chloride
b)
iron (II) chloride
c)
iron (I) chloride
d)
iron dichloride
85.
Which of the following combinations would need roman numerals in the name?
a)
potassium + fluorine
b)
beryllium + oxygen
c)
boron + iodine
d)
lead + oxygen
86.
lithium permanganate
a)
LiMnO4
b)
MnO4Li
c)
Li4MnO
d)
correct answer is not given
87.
calcium phosphate
a)
Ca3P2O8
b)
Ca2(PO4)3
c)
CaPO4
d)
correct answer is not given
88.
Cu2CO3
a)
copper carbonate
b)
copper (II) carbonate
c)
copper (I) carbonate
d)
copper carbon oxide
89.
iron (II) sulfate
a)
FeSO4
b)
Fe4(SO4)2
c)
FeSO2
d)
correct answer is not given
90.
copper (II) hydroxide
a)
CuOH2
b)
Cu2OH
c)
Cu(OH)2
d)
correct answer is not given
91.
Chlorine and Flourine will form an ionic bond together since they are in the same group.
a)
True
b)
False
92.
Magnesium and Sulfur would probably be able to form an ionic bond.
a)
True
b)
False
93.
Mg3N2
a)
Magnesium Nitride
b)
Trimanganese dinickel
c)
Magnesium (I) Nitride
94.
How many electrons will sulfur lose or gain when forming an ion?
a)
lose 2
b)
gain 2
c)
gain 6
d)
lose 6
95.
FeBr is called
a)
iron bromine
b)
iron (I) bromine
c)
iron bromide
d)
iron (I) bromide
96.
Calcium Nitride 
a)
CaN
b)
Ca3N2
c)
Ca2N3
d)
Ca2N
97.
AlF3
a)
Aluminum (I) fluride
b)
Aluminum (II) fluride
c)
Aluminum (III) fluoride
d)
aluminum fluroide
98.
TiCl2
a)
Tin(I) Chloride
b)
Titanium (I) Chloride
c)
Titanium (II) Chloride
d)
Titanium (I) Chloride 
99.
Na2S
a)
Sodium Sulfide
b)
Sodium Sulfate
c)
Sodium Sulfite
d)
Disodium Sulfide
100.
Atoms that lose electrons become...
a)
negatively charged (anion)
b)
postively charged (cation)
c)
remain neutral, no charge
d)
losers
101.
Why are ions charged particles?
a)
The number of electrons does not equal the number of protons.
b)
The number of protons does not equal the number of neutrons.
c)
The number of neutrons does not equal the number of electrons.
d)
The electric charges of the electrons and protons cancel each other out.
102.
Which of the following is NOT a characteristic of IONIC COMPOUNDS?
a)
High melting point
b)
Conducts electricity
c)
Strong bonds
d)
Low boiling points
103.
Which two elements could form an ionic compound?
a)
#6 carbon and #8 oxygen
b)
#1 hydrogen and #7 nitrogen
c)
#3 lithium and #9 fluorine
d)
#5 boron and #10 neon
104.
Which of the following compounds is not an ionic compound?
a)
barium oxide
b)
lithium oxide
c)
carbon dixoide
d)
calcium chloride
105.
Which statement about energy and ionic bonds is true?
a)
It takes energy to form a negative ion.
b)
Halogens need the most energy to become ions.
c)
It takes energy to remove valence electrons from an atom.
d)
It takes more energy to gain two electrons than one.
106.
In which of the following elements is the valence electron farthest from the nucleus?
a)
#3 lithium
b)
#11 sodium
c)
#19 potassium
d)
#37 rubidium
107.
What is the chemical name for NH4Cl?
a)
Nitrogen Hydrogen Chloride
b)
Nitrogen Tetrahydrogen Chloride
c)
Ammonium Chloride
d)
Ammounium Calcide
108.
What is the name for Al(CN)3?
a)
Aluminum Cyanide
b)
Aluminum Carbon Nitrogen
c)
Aluminum Tricarbon trinitride
d)
Aluminum Tricarbonitride
109.
A mixture of two or more metals is called:
a)
mixture
b)
solution
c)
compound
d)
alloy
110.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
111.
acetate
a)
C2H3O21-
b)
C3H2O31-
c)
C2H2O31-
d)
C3H3O21-
112.
phosphate
a)
PO32-
b)
PO33-
c)
PO42-
d)
PO43-
113.
chlorate
a)
ClO21-
b)
ClO31-
c)
ClO41-
d)
ClO1-
114.
cyanide
a)
CN2-
b)
CN1-
c)
CN21-
d)
CNO1-
115.
ammonium
a)
NH41+
b)
NH42+
c)
NH31+
d)
NH32+
116.
nitrite
a)
N3-
b)
NO21-
c)
NO31-
d)
N2O1-
117.

A farmer is looking to use ammonium phosphate as a fertilizer for his crops. Which of the following represents the chemical formula for ammonium phosphate?

a)

(NH4)3PO4

b)

NPO4

c)

NH4PO4

d)

NH4(PO4)3

118.

In a chemistry lab, you are tasked with creating a compound consisting of zinc and fluoride. Which of the following formulas represents zinc fluoride correctly?

a)

ZnF2

b)

ZnF

c)

Zn2F

d)

Zn2F4

119.

A chemist is working on a project that involves the use of aluminum sulfite. Which of the following represents the correct chemical formula for aluminum sulfite?

a)

Al2(SO3)3

b)

Al2(SO4)3

c)

AlSO3

d)

Al3(SO3)2

120.

A chemist is working on a project that involves the synthesis of silver phosphide. Which of the following chemical formulas represents silver phosphide?

a)

Ag3P

b)

Ag3PO4

c)

Ag3PO3

d)

AgP

121.

In an industrial setting, a worker needs to identify the chemical compound labeled as Ca(CN)2 in the storage area. What is the correct identification?

a)

Calcium Cyanide

b)

Calcium Dicyanide

c)

Calcium Dicarbon Dinitrogen

d)

Calcium Thiocyanate

122.

In a chemistry lab, a student is tasked with identifying the compound Sr(OH)2. What is its common name?

a)

Strontium Hydroxide

b)

Strontium Hydride

c)

Strontium Dihydroxide

d)

Strontium Dioxygen Dihydride

123.

A chemist is working on a project that involves the use of iron(II) carbonate. What is the correct formula for iron(II) carbonate?

a)

Fe2CO3

b)

FeCO3

c)

Fe2CO2

d)

FeCO4

124.

In a chemistry lab, you're given a compound labeled NaBr. What is the name of this compound?

a)

Bromide sodide

b)

Sodium bromide

c)

Sodium bromate

d)

Sodium bromite

125.

A chemist is analyzing a white powder in the lab and determines its chemical formula to be NH4F. What is the name of this compound?

a)

Ammonia fluoride

b)

Ammonium fluorite

c)

Ammonia fluorate

d)

Ammonium fluoride

126.

While studying geology, you come across a mineral sample in a limestone cave. The guide tells you it's composed of CaCO3. What is the name of this compound?

a)

Calcium carbon oxide

b)

Calcium(II) carbonate

c)

Calcium carbonate

d)

Carbonate(I) calcide

127.

A chemist is labeling containers for a new laboratory setup and comes across a bottle containing KF. What should the label read?

a)

Potassium fluoride

b)

Potassium fluorite

c)

Fluorine potasside 

d)

Potassium fluorate

128.

A chemist is working on a solution that requires magnesium hydroxide. Which of the following represents the correct chemical formula they should use?

a)

MgOH₂

b)

Mg(OH)₂

c)

Mg(OH)

d)

MgH₂

129.

Imagine you are working in a laboratory and analyzing the composition of minerals. You come across a sample labeled as iron (II) oxide. What is the charge on the iron in this compound?

a)

2+

b)

2-

c)

1+

d)

1-

e)

None of these.

130.

In a chemistry lab, you come across a compound labeled
Na2S. What is the NAME of this compound?

a)

sodium (II) sulfide

b)

sodium sulfide

c)

disodium sulfide

d)

sodium sulfur

131.

In the process of manufacturing semiconductors, a technician needs to know the correct formula for calcium arsenide. Which of the following is it?

a)

Ca3As2

b)

CaAs2

c)

Ca3As

d)

Ca3Ar2

132.

A chemist is working on a project that involves the use of iron(II) carbonate. What is the correct formula for iron(II) carbonate that the chemist should use?

a)

Fe2CO3

b)

FeCO3

c)

Fe2CO2

d)

FeCO4

133.

Imagine you're a scientist observing alkali metals in a lab. When these metals form an ion, what charge do they typically have?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

134.

Imagine you are a scientist working in a lab and you're examining the properties of elements. When you observe the alkaline earth metals on the periodic table, what charge do they typically have when they form an ion?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

135.

Imagine you are a scientist analyzing the chemical properties of elements. When you examine the halogens in the periodic table, what charge do they typically have upon forming an ion?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

136.

In a chemistry lab, a student is asked to determine the ion that Nitrogen, N, will most likely form. Which ion will Nitrogen form?

a)

N

b)

N-3

c)

N-5

d)

N+5

137.
What is the charge on a noble gas & why?
a)
0; they don't exchange electrons
b)
+1; they give away an electron
c)
-1; they gain an electron
d)
1; they form only single bonds
138.
An ionic bond is the attraction between:
a)
oppositely charged ions
b)
similarly charged ions
c)
neutral ions
d)
neutral atoms
139.
Ionic bonds form because
a)
Two ions of the same charge are attracted to each other
b)
Two ions of different charges are attracted to each other
c)
Two atoms share their electrons
d)
Two or more atoms share protons

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