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Chemistry Chatper 3 Test

Total questions: 100

Worksheet time: 4hrs 22mins

Name
Class
Date
1.

What is the definition of a mole?

a)

The number of atoms in 12 grams of carbon-12

b)

The number of atoms in 1 gram of carbon-12

c)

The number of atoms in 6.022 x 10^23 grams of carbon-12

d)

The number of atoms in 1 gram of any element

2.

What is the molar mass of hydrogen?

a)

1.008 g

b)

12.01 g

c)

55.85 g

d)

16 g

3.

How do you calculate the molar mass of a compound?

a)

By adding up the molar masses of its component elements

b)

By dividing the molar mass of the compound by the number of moles

c)

By multiplying the molar mass of the compound by Avogadro's number

d)

By subtracting the molar mass of the compound from the molar mass of carbon-12

4.
The _______ describes the atoms in a compound.
a)
chemical equation
b)
chemical formula
c)
chemical symbol
d)
coefficient
5.
How many elements are in C6H12O6?
a)
1
b)
2
c)
3
d)
4
6.
How many atoms of carbon (C) are in C6H12O6?
a)
3
b)
6
c)
12
d)
24
7.
Which is the correct formula for:
 three hydrogen (H)
one sulfur (S)
four oxygen (O)
a)
H3SO4
b)
HSO4
c)
H4S3O
d)
H2O
8.
Numbers that precede symbols and formulas in a chemical equation are ____.
a)
catalysts
b)
coefficients
c)
superscripts
d)
subscripts
9.

How many Al atoms are in this compound? 4Al2O3

a)

2

b)

8

c)

6

d)

4

10.

How many F atoms are in this compound?

6MgF2

a)

2

b)

6

c)

8

d)

12

11.
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 
12.
When calculating the EF the mole ratio is given as follows:
H1O3.5
What will the EF be?
a)
H1O3.5
b)
HO3.5
c)
HO4
d)
H2O7
13.
Which of the following represents an empirical formula?
a)
H2O2
b)
HC2O4
c)
H2O6
d)
H12O48
14.

A number in front of a chemical formula in an equation that indicates how many molecules or atoms of each reactant and product are involved in a reaction.

a)

Coefficient

b)

Subscript

c)

Reactant

d)

Product

15.

A number in a chemical formula that tells the number of atoms in a molecule or the ratio of elements in a compound

a)

Coefficient

b)

Subscript

c)

Reactant

d)

Product

16.

A formula that shows the smallest whole-number mole ratio of the elements of a compound, and may or may not be the same as the actual molecular formula.

a)

Empirical Formula

b)

Molecular Formula

c)

Stoichiometry

d)

Chemical Reaction

17.

Gives the actual number of atoms of each element in a molecule of a compound.

a)

Empirical Formula

b)

Molecular Formula

c)

Stoichiometry

d)

Chemical Reaction

18.

The study of the amounts of reactants and products in chemical reactions(the study of chemical recipes)

a)

Empirical Formula

b)

Molecular Formula

c)

Stoichiometry

d)

Chemical Reaction

19.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
20.

What does the number 4 represent in 4 NH3?

a)

Subscript

b)

Superscript

c)

Coefficient

21.

What does the number 3 represent in 4 NH3?

a)

Subscript

b)

Superscript

c)

Coefficient

22.
Ionic compounds are bonds between
a)
Metals and Metals
b)
Metals and Nonmetals
c)
Nonmetals and Nonmetals
d)
None of the above
23.

The name of P2O5 is

a)

phosphorus oxide.

b)

phosphorus pentoxide.

c)

diphosphorus pentoxide.

d)

phosphorus (V) oxygen (II).

24.

Which is a binary compound?

a)

silver nitrate

b)

sodium chlorite

c)

potassium sulfide

d)

ammonium sulfate

25.

Positive ions are formed when an atom

a)

loses electrons.

b)

gains protons.

c)

gains electrons.

d)

loses protons.

26.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
27.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
28.
What is the name of C3Cl8 ?
a)
Carbon octachloride
b)
Tricarbon octachloride
c)
Carbon trichloride
d)
Octacarbon trichloride
29.
What is the chemical formula for Nitrogen triiodide?
a)
NI
b)
N3I
c)
NI3
d)
None of these
30.
What is the name of CO
a)
Carbon oxide
b)
Carbon dioxide
c)
Carbon monoxide
d)
Carbon II oxide
31.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
32.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
33.
Cations are...
a)
Positive
b)
Negative
c)
Neutral
d)
Purring
34.
Anions are...
a)
Positive
b)
Negative
c)
Neutral
d)
Crying
35.

An atom with 2 protons, 3 neutrons, and 4 electrons has a charge of ____.

a)

+2

b)

-2

c)

+3

d)

0

36.

How many protons, neutrons, and electrons?

a)

proton = 6, neutron = 4, electron = 1

b)

proton = 4, neutron = 4, electron = 5

c)

proton = 1, neutron = 6, electron = 10

d)

proton = 4, neutron = 2, electron = 3

37.

A Bromine ion gains 1 electron, which of the following is the correct symbol for a Bromine ion?

a)

Br-1

b)

Br+1

c)

Br+7

d)

Br-7

38.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
39.
What is the oxidation number of Fe in FeO?
a)
+1
b)
-1
c)
+2
d)
-2
40.

What is the oxidation number of O in elemental O2 ?

a)

0

b)

-2

c)

+1

d)

+2

41.

What is the oxidation number of Na in Na+ ?

a)

0

b)

+1/2

c)

+1

d)

-1

42.
What is the oxidation number of Br in BrO3-1?
a)
+3
b)
-2
c)
+5
d)
+2
43.
What is the oxidation number of Sn in SnO2?
a)
+1
b)
+4
c)
+2
d)
-2
44.
If an atom loses electrons during a chemical reaction, the atom was:
a)
Oxidized
b)
Reduced
c)
Neutralized
d)
Precipitated
45.

What is the oxidation number of H in H2O?

a)

-1

b)

+1

c)

+2

d)

-2

46.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

47.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

48.

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

49.

Name the following ionic compound: Cs2S

a)

cesium sulfide

b)

cesium sulfate

c)

cesium II sulfate

d)

cesium II sulfide

50.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

51.

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

a)

potassium + fluorine

b)

beryllium + oxygen

c)

boron + iodine

d)

gold + oxygen

52.

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

53.

When naming a compound, which of these is written first?

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

54.

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

55.

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

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

56.

What is the name of the compound Sc(OH)3?

a)

Scandium (III) hydroxide

b)

Scandium (I) hydroxide

c)

Scandium (II) hydroxide

d)

Scandium hydroxide

57.

The name of the compound Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

58.

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

a)

potassium + fluorine

b)

beryllium + oxygen

c)

boron + iodine

d)

lead + oxygen

59.

What is the correct molecular formula for barium hydroxide?

a)

Ba(OH)2

b)

Ba2OH

c)

BaOH

d)

Ba2OH

60.
What is the formula for copper(I) sulfate?
a)
CuSO3
b)
CuSO4
c)
Cu2SO3
d)
Cu2SO4
61.

Metals tend to __________.

a)

gain electrons

b)

lose electrons

62.

Nonmetals tend to ______.

a)

gain electrons

b)

lose electrons

63.

Which neutral atom would form a cation?


Choose all that apply.

a)

Potassium (K)

b)

Oxygen (O)

c)

Neon (Ne)

d)

Barium (Ba)

64.

Which neutral atom would form an anion?


Choose all that apply.

a)

Helium (He)

b)

Magnesium (Mg)

c)

Oxygen (O)

d)

Fluorine (F)

65.

In ionic compounds, the oxidation number is ______ as the charge of the ion.

a)

the same

b)

different

66.

Elements in the same group have the same oxidation number.

a)

True

b)

False

67.

Elements in group 2 (2A) have what oxidation number?

a)

+2

b)

+1

c)

-2

d)

-3

68.

When naming an ionic compound, which name stays exactly as it is?

a)

The cation

b)

The anion

69.
The formula of calcium phosphate is 
a)
CaPO4
b)
Ca2(PO4)3
c)
Ca3PO4
d)
Ca3(PO4)2
70.
What is the formula for manganese(III) oxide?
a)
MgO
b)
Mg2O3
c)
MnO
d)
Mn2O3
71.
What is the name of Al(NO3)3?
a)
Aluminum trinitrate
b)
Monoaluminum nitrate
c)
Aluminum (III) nitrate
d)
Aluminum Nitrate
72.
ammonium phosphate
a)
(NH4)3PO4
b)
NPO4
c)
NH4PO4
d)
NH4(PO4)3
73.
The formula for copper (II) hydroxide is
a)
Cu(II)OH
b)
Cu(OH)2
c)
Cu2OH
d)
CuOH2
74.
The chemical formula for tin (IV) oxide is written
a)
Sn2O4
b)
Ti2O4
c)
SnO2
d)
TiO2
75.

What is Avogadro's number?

a)

6.02 x 1023

b)

1 mole

c)

600 million

d)

6.02

76.

How many moles are in 6.02 x 1023 molecules of H2O?

a)

1 mole

b)

2 moles

c)

6.02 moles

d)

602000000000000000000000 moles

77.

One mole of carbon dioxide (CO2) contains 6.02 x 1023 _____.

a)

atoms

b)

formula units

c)

ions

d)

molecules

78.

How many moles are in 8.30 X 1023 molecules of H2O?

a)

1.38 X 1023 moles H2O

b)

1.38 moles H2O

c)

2 moles H2O

d)

1 mole H2O

79.

How many molecules are there in 31.8 moles of water?

a)

5.28 x 10-23 molecules

b)

1.91 x 1025 molecules

c)

5.28x 10-25 molecules

d)

1.91 x 1023 molecules

80.

What is the conversion factor that should be used to determine how many molecules are there in 4.00 moles of glucose, C6H12O6?

a)
b)
c)
d)
81.

Which has the most particles?

a)

1 mole H2

b)

1 mole Na1+

c)

1 mole Al(OH)3

d)

These are all the same

82.

Why is the mole used in chemistry?

a)

The mass of atoms is in AMUs which is too hard to convert to grams.

b)

A dozen is not a scientific amount.

c)

Chemists needed to make chemistry easier to understand.

d)

It makes counting large numbers of small particles easier.

83.

How many moles there are in 5.68 x 1024 formula units of AlCl3?

a)

3.42 x 1024 moles

b)

9.44 x 1024 moles

c)

9.44 moles

d)

3.42 moles

84.

How many moles are in 4.5 x 1024 atoms of lithium?

a)

2.71 x 1048 particles

b)

7.47 moles

c)

7.47 x 1024 atoms

d)

2.71 moles

85.

How is moles abbreviated?

a)

M

b)

m

c)

mol

d)

ml

86.

How many moles of Na contain 1.45 x 1021 atoms of Na?

a)

8.73 x 1044 moles

b)

8.73 moles

c)

0.00241 moles

d)

2.41 x 1044 moles

87.

How many atoms are in 2 moles of water?

HINT: Remember mole is just a unit of measurement

a)

1.204x1024

b)

6.02x1023

c)

12.04x1023

d)

12.04x1024

88.

Calculate the Molar Mass for CaCl

a)

75.53 mol/g

b)

75.53 g/mol

c)

35.45 g/mol

d)

40.08 g/mol

89.
What is the molar mass of NaCl?
a)
58.45g/mol
b)
28g/mol
c)
12g/mol
d)
6.02 x 1023
90.
What is the molar mass of C2H4O2?
a)
40g
b)
50g
c)
60g
d)
68g
91.
How do we get mass from moles?
a)
multiply by avogadro's number
b)
multiply by molar mass
c)
divide by avogadro's number
d)
divide by molar mass
92.
What would be the mass of 1.5mol H2O
a)
20
b)
27
c)
32
d)
40
93.
What is the mass of 0.75 moles of (NH4)3PO4?
a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g
94.

How many particles (Molecules) would be in 8.4 moles of Octane (C8H18)?

a)
5.77 x 1023
b)
5.04 x 1024
c)
5.77 x 1026
d)
5.04 x 1023
95.
How many molecules are in 32.4 grams of phosphorous pentoxide?
a)
1.76 x 1023 molecules
b)
0.29 moles
c)
1.76 x 1022 molecules
d)
0.29 molecules
96.
The molar mass of an element is the mass of one ____ of the element.
a)
atom
b)
molecule
c)
mole
d)
gram
97.
What is the molar mass of Carbon Dioxide (CO2)?
a)
12 amu
b)
12 g
c)
44 g
d)
44 amu
98.
What is the mass of one mole of Al2(SO4)3?
a)
75.04 g
b)
342.14 g 
c)
75.04 mol
d)
342.14 mol
99.
How many molecules are present in 25 g of NaBr?
a)
102.96 molecules
b)
0.24 molecules
c)
1.45x1023 molecules
d)
2.34 x 1020molecules
100.
What is the mass of 54.3x1045molecules of BeO?
a)
3.27x1070 g
b)
9.01 x1022g
c)
2.25 x1024 g
d)
1.31 x1069g

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