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Unit 7 Review: Ionic Compounds

Total questions: 65

Worksheet time: 2hrs 43mins

Name
Class
Date
1.
What is the formula for aluminum fluoride?
a)
AlF
b)
Al2F3
c)
AlF3
d)
Al3F2
2.
A chemical bond resulting from the electrostatic attraction between positive and negative ions is called a(n)
a)
covalent bond.
b)
ionic bond.
c)
charged bond.
d)
dipole bond.
3.
How many valence electrons does a bromine atom have?
a)
1
b)
2
c)
6
d)
7
4.
AgF
a)
silver fluoride
b)
silver fluorine
c)
monosilver monofluoride
d)
silver monofluorine
5.
When metals bond with non-metals they form what type of bonds
a)
covalent
b)
ionic
c)
cooperative
d)
lewis
6.
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
7.
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
8.
Metals tend to 
a)
gain electrons
b)
lose electrons
9.
What is the correct formula for the compound, lithium oxide?
a)
LiO
b)
Li2O
c)
LiO2
d)
Li2O2
10.
What do Roman Numerals represent in the name of a transition metal compound?
a)
how many atoms of the metal there are
b)
the oxidation number of the nonmetal
c)
the oxidation number of the metal
d)
the mass number
11.
The name for CrN:
a)
Chromium nitride
b)
Chromium (I) nitride
c)
Chromium (III) nitride
d)
Chromium nitride (III)
12.

The charge of Fe in Fe2O3:

a)

+2

b)

+3

c)

+1

d)

-2

13.

The charge of copper in Cu2S:

a)

+1

b)

+2

c)

-1

d)

-2

14.

What is the charge of Gold in the formula AuO2?

a)

+2

b)

+1

c)

+4

d)

(II)

15.

The name of Cu₃N₂ is

a)

copper (III) nitride

b)

copper (II) nitride

c)

copper nitride

d)

tricopper dinitride

16.
Nonmetals tend to 
a)
gain electrons
b)
lose electrons
17.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
18.
PbS2
a)
lead sulfide
b)
lead sulfur
c)
lead II sulfide
d)
lead IV sulfide
19.
When a nonmetal gains electrons, it becomes this type of ion.
a)
Anion
b)
Cation
20.
When a metal loses electrons, it becomes this type of ion.
a)
anion
b)
cation
21.
The proper formula for magnesium hydroxide:
a)
MgOH
b)
Mg2OH
c)
Mg(OH)2
d)
Mg2OH2
22.

Which of the following combinations would need roman numerals in the name?

a)

strontium + fluorine

b)

boron + oxygen

c)

silver + iodine

d)

titanium + oxygen

23.
Name the following ionic compound: Cr(NO2)3
a)
chromium nitrite
b)
chromium nitride
c)
chromium III nitride
d)
chromium III nitrite
24.
Which of the following is NOT an ionic compound:
a)
CaO
b)
NaOH
c)
BaCl2
d)
Br2
25.
What is the formula for calcium carbonate?
a)
CaCO
b)
CaCO2
c)
CaCO3
d)
Ca3CO3
26.
Name this compound: 
NH4F
a)
Ammonia fluoride
b)
Ammonium fluorite
c)
Ammonia fluorate
d)
Ammonium fluoride
27.
The chemical formula of iron (III)bromide is
a)
FeBr
b)
Fe(III)Br
c)
FeBr₃
d)
Fe₂Br₃
28.
When naming ionic compounds you always write the name of the positive element  _______ .
a)
first
b)
second
c)
with "ide"
d)
with a prefix
29.
In most cases, when naming you change the ending of the second element to ________.
a)
-ate.
b)
-ite.
c)
-ide.
d)
-ine.
30.
What is the formula for calcium phosphide?
a)
CaP
b)
Ca2P3
c)
Ca3P2
d)
Ca2P
31.
The chemical formula for an ionic compound of potassium and oxygen is
a)
KO.
b)
K2O.
c)
K2O2.
d)
KO2.
32.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

33.

Name the ionic compound SnSe2

a)

Tin diselenide

b)

Tin (IV) Selenide

c)

Tin selenide

d)

Tin (II) triselenide

34.

Which of these combinations is a metallic compound made of?

a)

Metal and Metal

b)

Nonmetal and Nonmetal

c)

Metal and Nonmetal

d)

Cation and Cation

35.

Which of these combinations is a covalent compound made of?

a)

Metal and Metal

b)

Nonmetal and Nonmetal

c)

Metal and Nonmetal

d)

Cation and Cation

36.

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

37.

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

38.

When naming a compound, what must the last part be?

a)

the element with "ide" at the end

b)

the element with the ending "ite"

c)

the name of the element

d)

the element with "ide" at the end, unless its a polyatomic ion

39.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

40.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)
pairs of electrons are shared between two nonmetal atoms.
d)
two nonmetal atoms are attracted to each other by opposite charges.
41.
An ionic bond forms when 
a)
Valence electrons are shared
b)
a sea of mobile electrons surround the cations
c)
valence electrons are transferred between atoms
d)
none of the above
42.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
43.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
44.
Predict the bond that will form between Sr and S.
a)
Ionic
b)
Covalent
45.
What is a valence electron?
a)
an electron that is found in the outermost shell of an atom. 
b)
an electron found in the innermost shell of an atom.
c)
an electron found in the middle shell.
46.
A positively or negatively charged particle.
a)
covalent bond
b)
compound
c)
ion
d)
chemical bond
47.
Tells what elements a compound contains and the number of those atoms.
a)
compound
b)
ion
c)
chemical formula
d)
ionic bond
48.
Force that holds together atoms in a substance.
a)
compound
b)
ion
c)
chemical bond
d)
ionic bond
49.

Can NEVER conduct electricity

a)

ionic

b)

covalent

c)

metallic

50.

Have high melting & boiling points

a)

ionic

b)

covalent

c)

metallic

51.

CAN conduct electricity when dissolved in water

a)

ionic

b)

covalent

c)

metallic

52.

crystalline structure of alternating positive and negative charges

a)

ionic

b)

covalent

c)

metallic

53.

are a "sea" of electrons

a)

ionic

b)

covalent

c)

metallic

54.
All solids at room temperature
a)
ionic compounds
b)
covalent compounds
55.
When dissolved in water, the solution is a good conductor of electricity.
a)
ionic compounds
b)
covalent compounds
56.
usually soft
a)
ionic compounds
b)
covalent compounds
57.

Why do metals conduct electricity?

a)

They are shiny

b)

The electrons are delocalised and able to move

c)

The electrons are held tightly within the lattice

d)

The electrons are shared between two metal ions

58.

Which of these are considered properties of metals? (choose ALL that apply)

a)

brittleness

b)

low melting point

c)

luster (shininess)

d)

malleability

e)

ductility

59.

Why do metallic compounds conduct electricity as solids?

a)

core electrons are mobile, allowing electricity to flow through the metal

b)

valence electrons are mobile, allowing electricity to flow through the metal

c)

protons are mobile, allowing electricity to flow through the metal

d)

the metal cations are mobile, allowing electricity to flow through the metal

60.

Which of the following is a covalent compound?

a)

CaO

b)

NaCl

c)

CaCl2

d)

CH4

61.
How do the following two elements bond together?
K1+  S2- 
a)
KS
b)
K8S
c)
K6S3
d)
K2S
62.

Which particle is responsible for bonding?

a)

Protons

b)

Electrons

c)

Neutrons

d)

Nucleus

63.

Which of the following is true about Ionic Bonds? (select ALL TRUE options)

a)

High melting point

b)

Low melting point

c)

Can dissolve in water

d)

Cannot dissolve in water

e)

Can conduct electricity

64.

Why do atoms form bonds?

a)

to attain a noble gas configuration

b)

to increase their mass

c)

to increase their atomic number

d)

to attain an alkali metal configuration

65.
Some are solids, some are liquids, and some are gases at room temperature.
a)
ionic compounds
b)
covalent compounds

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