Types of Compounds
Practice Test
1.
What is the formula for the binary compound of potassium and chlorine?
a.
KCl2
b.
KCl
c.
K2ClO3
d.
KHCl
2.
What is the formula for lithium carbonate?
a.
LiCO
b.
Li
3
CO
2
c.
LiCO
3
d.
Li
2
CO
3
3.
The charge on an ion formed from an atom is called the _____________ of the atom.
a.
reaction capacity
b.
atomic radius
c.
oxidation number
d.
charge
4.
Which of the following is the formula for nitric acid?
a.
HNO3
b.
HNO2
c.
HN
d.
HNO
5.
Which of these is NOT a binary compound?
a.
potassium iodide
b.
carbon dioxide
c.
water
d.
aluminum nitrate
6.
The formulas O
2
, P
4
, and S
8
show that oxygen, phosphorus, and sulfur are _______________.
a.
hydrates
b.
diatomic
c.
ionic elements
d.
molecular elements
7.
These elements commonly have more than one positive oxidation number.
a.
alkaline earths
b.
transition elements
c.
noble gases
d.
alkali metals
8.
Compounds that contain water are called __________.
a.
anhydrous
b.
aluminates
c.
hydrates
d.
aqueous
9.
What is the formula for the binary compound that forms when potassium and sulfur react?
a.
K
2
SO
4
b.
KS
2
c.
K
2
S
d.
KS
10.
What is the oxidation number of Group 17 nonmetals?
a.
-1
b.
1
c.
0
d.
3
11.
Fluorine atoms tend to react to form _______ ions.
a.
1-
b.
7+
c.
3+
d.
5-
12.
Calcium atoms tend to react to form _______ ions.
a.
4-
b.
6-
c.
2+
d.
1+
13.
What is the formula for sulfur trioxide?
a.
SO
b.
S
3
O
c.
SO
3
2-
d.
SO
3
14.
What is the name of the molecular compound NO
2
?
a.
dinitrogen dioxide
b.
nitrogen dioxide
c.
nitrogen dioxygen
d.
nitrite
15.
Name the molecular compound represented by the formula PF
5
.
a.
phosphorus(V) fluorine
b.
phosphate
c.
phosphorus fluorine
d.
phosphorus pentafluoride
16.
Iron atoms commonly react to form __________ ions.
a.
1+ and 2+
b.
2+ and 4+
c.
2+ and 3+
d.
3+ and 4+
17.
Name the ionic compound represented by the formula Mg(OH)
2
.
a.
manganese hydroxide
b.
magnesium hydroxide
c.
magnesium hydrate
d.
magnesium oxide
18.
These types of compounds make eggshells brittle.
a.
covalent
b.
molecular
c.
network
d.
ionic
19.
Diatomic oxygen and ozone are _____________.
a.
different elements
b.
ionic
c.
allotropes
d.
isotopes
20.
In aqueous solution, H
2
SO
4
is called _______________.
a.
hydrogen sulfite
b.
nitric acid
c.
hydrogen sulfur oxide
d.
sulfuric acid
21.
C
5
H
12
is the formula for the hydrocarbon _____________.
a.
pentane
b.
hexane
c.
carbon hydride
d.
methane
22.
The sum of the charges in an ionic compound must equal ________.
a.
positive eight
b.
positive one
c.
zero
d.
negative eight
23.
If each carbon atom can form four bonds, why doesn't a two-carbon alkane have eight hydrogen atoms?
a.
Alkanes have functional groups bonded to carbon atoms.
b.
Alkanes have double bonds leaving fewer bonds available for hydrogen atoms.
c.
Each of the carbon atoms must bond to the other carbon atom as well as to hydrogen atoms.
d.
Alkanes have triple bonds between carbons and so can only bond with one hydrogen atom each.
24.
Which of these formulas does not represent a polyatomic ion?
a.
CN
-
b.
NO
2
-
c.
PO
4
3-
d.
CO
25.
The formula for a covalent compound is called a _______________.
a.
covalent code
b.
macromolecule
c.
molecular formula
d.
covalent formula
