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WorksheetsSpring Semester
Total questions: 60
Worksheet time: 2hrs 18mins
Name
Class
Date
1.
The first step in naming an ionic compound is always...
a)
Naming the anion (non-metal)
b)
Changing the ending to -ide
c)
Naming the cation (metal)
d)
Writing the cation charge
2.
What is the correct formula for the compound, lithium oxide?
a)
LiO
b)
Li2O
c)
LiO2
d)
Li2O2
3.
What is the formula for manganese(III) oxide?
a)
MgO
b)
Mg2O3
c)
MnO
d)
Mn2O3
4.
From the following ionic compounds, choose the name-formula pair that is not correctly matched.
a)
sodium sulfide Na2S
b)
ammonium nitrate
NH4NO3
NH4NO3
c)
sodium sulfate
Na2SO3
Na2SO3
d)
calcium oxide CaO
5.
Name the following ionic compound: Cr(NO2)3
a)
chromium nitrite
b)
chromium nitride
c)
chromium III nitride
d)
chromium III nitrite
6.
Which of the following combinations would need roman numerals in the name?
a)
potassium + fluorine
b)
beryllium + oxygen
c)
boron + iodine
d)
silver + oxygen
7.
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
8.
The name of the compound Ca3(PO4)2
a)
calcium phosphate
b)
tricalcium diphosphate
c)
calcium phosphorus oxide
d)
calcium phosphide
9.
Group 15 elements form what type of charge?
a)
-1
b)
-3
c)
+3
d)
15
10.
When adding a subscript to a polyatomic ion, you should...
a)
multiply any subscripts on the polyatomic ion by the subscript you are adding
b)
put parentheses around the polyatomic ion before adding a subscript
c)
write the new subscript next to any subscripts on the polyatomic ion
d)
put the polyatomic ion in square brackets before adding the subscript
11.
Ionic Formula -
strontium iodide
strontium iodide
a)
SrI
b)
SrI2
c)
Sr2I
d)
StI2
12.
Identify the type of chemical reaction being represented in the following equation:
MgCO3 --> MgO + CO2
MgCO3 --> MgO + CO2
a)
combustion
b)
synthesis
c)
decomposition
d)
single
13.
Identify the type of chemical reaction being represented in the following equation:
C3H6O + O2 --> CO2 + H2O
C3H6O + O2 --> CO2 + H2O
a)
combustion
b)
synthesis
c)
single
d)
double
14.
Identify the type of chemical reaction being represented in the following equation:
MgSO4 + KNO3 --> Mg(NO3)2 + K2SO4
MgSO4 + KNO3 --> Mg(NO3)2 + K2SO4
a)
combustion
b)
decomposition
c)
single
d)
double
15.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
16.
hydrobromic acid
a)
HBrO3
b)
HBr
c)
HBr2
d)
HBrO
17.
H2SO4
a)
hydrosulfuric acid
b)
sulfuric acid
c)
sulfurous acid
d)
hydrosulfurous acid
18.
Ca+2, O-2
a)
CaO
b)
OCa
c)
Ca-2O+2
d)
Ca2O2
19.
K+, O-2
a)
KO
b)
K2O
c)
K-2O2
d)
O2K
20.
What is the correct formula for phosphorous trichloride?
a)
P₃Cl
b)
PCl₃
c)
KCl₃
d)
K₃Cl
21.
Two elements react to form one product is an example of which type of chemical reaction?
a)
combustion
b)
decomposition
c)
synthesis
d)
single replacement
22.
Which type of reaction takes place in the presence of oxygen and produces carbon dioxide and water?
a)
double replacement
b)
decomposition
c)
combustion
d)
single replacement
23.
What kind of reaction is this:
CaCO3 + Ag2SO4 → CaSO4 + Ag2CO3
CaCO3 + Ag2SO4 → CaSO4 + Ag2CO3
a)
Decomposition
b)
Single Replacement
c)
Double Replacement
d)
Combustion
24.
If an element is diatomic it should have a subscript of___
a)
2, always
b)
2, only when it is by itself
c)
it shouldn't have a subscript, it should have a coefficent
25.
when calcium carbonate reacts with silver sulfate, it produces calcium sulfate and silver carbonate. what is the correct balanced equation for this reaction
a)
Ca2CO3 + AgSO4 → CaSO4 + Ag2CO3
b)
CaCO3 + Ag2SO4 → Ca2SO4 + AgCO3
c)
CaCO3 + Ag2SO4 → CaSO4 + Ag2CO3
d)
Ca2CO3 + Ag2SO4 → Ca2SO4 + Ag2CO3
26.
in a reaction, aqueous barium chloride reacts with aqueous potassium carbonate to produce solid barium carbonate and aqueous potassium chloride. what is the correct balanced equation.
a)
Ba2Cl(aq) + KCO3(aq) --> BaCO3(s) + KCl(aq)
b)
BaCl2(aq) + K2CO3(aq) --> BaCO3(s) + 2KCl(aq)
c)
BaCl(aq) + K2CO3(aq) --> BaCO3(s) + K2Cl(aq)
d)
Ba2Cl2(aq) + KCO3(aq) --> Ba2CO3(s) + KCl2(aq)
27.
Which conversion factor should be used to solve the following, "How many moles in 28 grams of CO2?"
a)
1 mol = 22.4 L
b)
1 mol = 44.01 g
c)
1 mol = 6.02x1023 atoms
d)
more than one
28.
Which expression below show the correct method of determining the percent composition of Sodium in Na2CO3?
a)
%Na = (22.99g/106g) x 100
b)
%Na = (22.99g/106) / 100
c)
%Na = (45.98g/106g) x 100
d)
%Na = (106/45.98g) x 100
29.
What is the molar mass of Hydrogen Peroxide (H2O2)?
a)
48 g/mole
b)
34.02 g/mole
c)
36.5 g/mole
d)
35.5 g/mole
30.
What are the units for molar mass?
a)
grams
b)
amu
c)
grams/mole
d)
liters
31.
How many molecules are in 2.5 mol of NaCl?
a)
1.51x1023
b)
146
c)
4.15
d)
1.51x1024
32.
Find the percent composition of hydrogen in (NH4)2S.
a)
11.8%
b)
41.1%
c)
47.1%
33.
Which of the following has more molecules a mole of CO2 or a mole of H2O?
a)
CO2 has more
b)
H2O has more
c)
They have the same
d)
Impossible to compare
34.
Which of the following does NOT describe a mole?
a)
6.02x1023
b)
Abbreviation for molecule
c)
The number of atoms present in 12 g of carbon-12
d)
Avogadro's Number
35.
What is the mass of one mole of aluminum chloride?
a)
62.43g
b)
116.40g
c)
133.33g
d)
97.89g
36.
What is the molar mass of B2(CO3)3?
a)
81.63 g/mol
b)
94.84 g/mol
c)
38.82 g/mol
d)
201.65 g/mol
37.
How many grams are in 1.2x1024 molecules of carbon monoxide?
a)
28 grams
b)
56 grams
c)
6.02 grams
d)
1.2 grams
38.
How many molecules are in 9.44 moles of AlCl3?
a)
1.57x10-23 molecules AlCl3
b)
5.68x1024 molecules AlCl3
c)
0.705 molecules AlCl3
d)
1.25x1023 molecules AlCl3
39.
All of the following are empirical formulas EXCEPT
a)
C3H8
b)
Na2SO4
c)
N2O4
d)
Al3(SO4)2
40.
Which of the following is the correct empirical formula for C4H10
a)
C2H5
b)
CH2.5
c)
C8H20
d)
C4H10
41.
Determine the empirical formula for a compound with 87.1% Ag and 12.9% S.
a)
AgS2
b)
Ag3S5
c)
Ag2S
d)
Ag4S2
42.
The empirical formula of a substance is CH2O. Its molar mass is 180.0. What is the molecular formula?
a)
C6H12O6
b)
C4H8O4
c)
C8H16O8
d)
C2H4O2
43.
Epinephrine (adrenaline) is a hormone secreted into the bloodstream in times of stress. It contains 59.00% C, 6.62% H, 26.20% O, 7.65%N and has a molar mass of 183 g/mol. What is its molecular formula?
a)
C9H12NO3
b)
C5H11N3O2
c)
C8H12NO2
d)
C7H9N2O
44.
Is the empirical formula of a substance ever the same as the molecular formula for a substance?
a)
Always
b)
Sometimes
c)
Never
45.
What is the mass of 1.2 moles of IrI3?
a)
570 g
b)
690 g
c)
320 g
d)
957 g
46.
What is the molar mass of (NH4)2O?
a)
34 g/mol
b)
33 g/mol
c)
49 g/mol
d)
52 g/mol
47.
Find the grams of 0.75 moles of (NH4)3PO4?
a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g
48.
A formula with the lowest whole # ratio of elements in a compound is called
a)
empirical formula
b)
chemical formula
c)
covalent formula
d)
molecular formula
49.
A chemical formula that shows the actual # and kinds of atoms present in one molecule of a compound is called_________
a)
ionic formula
b)
covalent formula
c)
empirical formula
d)
molecular formula
50.
KMnO4
a)
Empirical
b)
Molecular
51.
Na2S2O3
a)
Empirical
b)
Molecular
52.
What is the molecular formula of a compound with an empirical formula of C2OH4 and a molar mass of 88 grams per mole?
a)
C2O4H8
b)
C8O2H4
c)
C4O2H8
d)
C4O8H2
53.
What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.
a)
K2SO4
b)
K8SO16
c)
K8S4O8
d)
K8S4O16
54.
Find the percent composition of N2S2.
a)
N: 69.6% S: 30.4%
b)
N:36% S: 75.6%
c)
N: 96.6% S: 3.4%
d)
N: 30.4% S: 69.6%
55.
Find the percent composition of Cu in CuBr2 .
a)
28.45%
b)
32.85%
c)
17.78%
d)
68.10%
56.
What is the percent composition of S in the formula (NH4)2S ?
a)
12.05%
b)
19.30%
c)
47.11%
d)
56.18%
57.
29.0 g of Argon combine completely with 4.30 g of Sulfur. What is the percent composition of Argon and Sulfur?
a)
87.09% Argon, 12.9% Sulfur
b)
12.9% Argon, 87.09% Sulfur
c)
80% Argon, 20% Sulfur
d)
35% Argon, 65% Sulfur
58.
222.6 g of Sodium combine completely with 77.4 g of Oxygen. What is percent composition of Sodium and Oxygen?
a)
25% Sodium, 74.2% Oxygen
b)
15% Sodium, 85% Oxygen
c)
74.2% Sodium, 25.8% Oxygen
d)
90% Sodium, 10% Oxygen
59.
How many moles are in 987g of Ra(OH)2
a)
38 moles Ra(OH)2
b)
30 moles (OH)2
c)
3.8 moles Ra(OH)2
d)
260 moles Ra(OH)2
60.
How many moles are in 4.5x1024 particles?
a)
7.5 particles
b)
7.5 mol
c)
2.7x1048 mol
d)
2.7x1048 particles
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