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Unit 5: Ionic Bonding Review

Total questions: 45

Worksheet time: 1hrs 20mins

Name
Class
Date
1.

In an ionic bond, the ions are held together because...

a)

the positive nucleus of each ion attracts the other ion's negatively charged electrons

b)

the ions have opposite charges

c)

as the electron moved from one atom to another it pulled the atom along with it

d)

electrons are being shared

2.

Which element(s) will lose valence electrons to form an ion? Check all that apply.

a)

Phosphorus

b)

Iron

c)

Barium

d)

Neon

3.

Which element(s) will form negative ions? Check all that apply.

a)

Potassium

b)

Sulfur

c)

Iodine

d)

Magnesium

4.

Which of the following pairs of elements could NOT react to form an ionic compound?

a)

Carbon and Oxygen

b)

Potassium and Fluorine

c)

Silver and Oxygen

d)

Aluminum and Chlorine

5.
Nitrogen will form which of the following ions?
a)
N
b)
N-3
c)
N-5
d)
N+5
6.
Beryllium will ____ valence electrons when forming an ionic bond.
a)
lose 4
b)
gain 4
c)
lose 2
d)
gain 2
7.
In the compound aluminum oxide, which is the cation?
a)
Al+3
b)
Al
c)
O-2
d)
O
8.
What determines how ionic bonds will form?
a)
Number of protons
b)
Mass of the atom
c)
Number of total electrons
d)
Number of valence electrons
9.
Boron will ____ valence electrons when forming an ionic bond.
a)
lose three
b)
gain three
c)
lose 5
d)
gain 5
10.
What type of bond is this? Lithium with Fluorine?
a)
ionic
b)
covalent
11.
How many electrons are needed in the outer energy levels of an atom to be stable?
a)
2
b)
4
c)
6
d)
8
12.
What is the ionic compound formed between K and F?
a)
KF
b)
K2F
c)
KF2
d)
K2F2
13.
What is the ionic compound formed between Ba and P?
a)
Ba2P3
b)
Ba3P2
c)
BaP
d)
Ba2P2
14.
Atoms gain or lose electrons to become stable by satisfying this rule.
a)
Lewis Structure rule
b)
Periodic Law
c)
octet rule
d)
Ionic Law
15.

Which pair of elements should form an ionic bond?

a)

Carbon and Oxygen

b)

Sodium and Fluorine

c)

Iron and Chromium

d)

Xenon and Silicon

16.
Mg2+ and Cl- create...
a)
Mg2Cl
b)
MgCl2
c)
Mg2Cl2
d)
MgCl
17.

Potassium and Sulfur create...

a)

KS

b)

KS2

c)

K2S

d)

K2S2

18.
Ca2+ and N3- create...
a)
Ca2N3
b)
Ca3N2
c)
CaN3
d)
Ca2N
19.

What are the necessary conditions for an ionic bond to form between atoms?

a)

One atom must have a high ionization energy and the other a high electron affinity.

b)

One atom must have a low ionization energy and the other must have a low electron affinity.

c)

One must have a low ionization energy and the other a high electron affinity.

d)

Both atoms must have a high electron affinity.

20.

What ultimately lowers the chemcial potential energy between atoms, giveing them both more stability?

a)

The Gravitational Force

b)

The Electrostatic Force.

c)

The Strong Force.

d)

The Weak Force.

21.
Where are the transition metals found on the periodic table?
a)
The first 5 elements
b)
The bottom two rows
c)
Group 3-12
d)
Row 3-12
22.
What is a transition metal?
a)
They are elements that charges vary and are represented by roman numerals during nomenclature.
b)
A type of squirrel.
c)
Elements that are not defined as metals or nonmetals.
d)
A metal with no charge.
23.
What is one way to recognize a transition metal?
a)
If it has a roman numeral
b)
it says that it is a transition metal
c)
you cant recognize it
d)
it has 4 elements
24.
Name the compound using appropriate rules:
FeCl3
a)
Chloride Iron
b)
Iron III Chloride
c)
Chloride III Iron
d)
I have no clue
25.
Which of these combinations is an ionic compound made of?
a)
Metal and Metal
b)
Nonmetal and Nonmetal
c)
Metal and Nonmetal
d)
Cation and Cation
26.

What is the name of the following formula: Cu3N

a)

copper nitride

b)

copper (iii) nitride

c)

copper (i) nitride

d)

copper (iii) nitrogen (i)

27.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

28.

When naming ionic compounds with transition metals you need to include roman numerals to show the _____ of the metal..

a)

atomic number

b)

mass number

c)

charge

d)

ionization energy

29.
The oxidation number for Fe in Fe2O3:
a)
+2
b)
+3
c)
+1
d)
-2
30.
The name of Cu₃N₂ is
a)
copper (III) nitride
b)
copper (II) nitride
c)
copper nitride
d)
tricopper dinitride
31.
In most cases, when naming you change the ending of the second element to ________.
a)
-ate.
b)
-ite.
c)
-ide.
d)
-ine.
32.
An ionic compound made of copper (Cu2+) and oxygen would be named
a)
copper oxygen.
b)
copper oxide.
c)
dicopper oxide.
d)
copper(II) oxide.
33.
Because the overall charge in a compound must be ____________, the charge of iron in Fe2O3 can be calculated as 3+.
a)
2+
b)
1+
c)
0
d)
1-
34.
Name that Ion
Cu+2
a)
Iron(III)
b)
colbalt(II)
c)
copper(II)
d)
cadmium
35.

In the compound TiO2, titanium has a charge of ______. Hint: The charge on "O" is -2. Use the charge on oxygen to determine the charge on Ti.

a)

4+

b)

2+

c)

2-

d)

4-

36.

LiNO3

a)

lithium nitrate

b)

lithium(III) nitrate

c)

lithium nitride

d)

lithium oxide

37.

MgSO4

a)

magnesium sulfoxide

b)

magnesium sulfide

c)

magnesium sulfate

d)

magnesium oxide

38.

Na2(SO4)

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

39.

Sc(OH)3

a)

Scandium(III) hydroxide

b)

Scandium(I) hydroxide

c)

Scandium(II) hydroxide

d)

Scandium hydroxide

40.

Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

41.

CaCO3

a)

Calcium carbon oxide

b)

Calcium(II) carbonate

c)

Calcium carbonate

d)

Carbonate(I) calcide

42.

Li2CO3

a)

lithium carbonate

b)

lithium(I) carbonate

c)

lithium carbon trioxide

d)

monolithium carbonate

43.

CoCO3

a)

Cobalt(II) carbonate

b)

Cobalt(I) carbonate

c)

Cobalt carbonate

d)

Cobalt(III) carbonate

44.

TiPO4

a)

Titanium(III) phosphate

b)

Titanium(II) phosphate

c)

Titanium(I) phosphate

d)

Titanium phosphate

45.

Ni3(PO4)2

a)

Nickel(II) phosphate

b)

Nickel(I) phosphate

c)

Nickel(III) phosphate

d)

Nickel phosphate

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