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Chemistry Final Exam

Total questions: 75

Worksheet time: 2hrs 25mins

Name
Class
Date
1.

Which of the following best describes ionic bonding?

a)

Sharing of electrons between two atoms

b)

Transfer of electrons from one atom to another

c)

Sharing of a pair of electrons between multiple atoms

d)

Attraction between two non-metal atoms

2.

Which types of atoms typically undergo ionic bonding?

a)

Two non-metals

b)

Two metals

c)

A metal and a non-metal

d)

Noble gases

3.
K +  and  N-3
a)
KN
b)
KN3
c)
K3N3
d)
K3N
4.

What is a characteristic property of ionic compounds?

a)

High melting points

b)

Low boiling points

c)

Poor electrical conductivity in solid state

d)

Solubility in non-polar solvents

5.

Which of the following compounds is most likely to be ionic?

a)

CO2

b)

NaCl

c)

H2O

d)

CH4

6.

The formula unit of sodium fluoride is:

a)

NaF2

b)

NaF

c)

Na2F

d)

Na2F2

7.

The formula for aluminum oxide is:

a)

AlO

b)

AlO2

c)

Al2O3

d)

Al3O2

8.

What is the name of the compound with the formula FeCl3?

a)

Iron chloride

b)

Iron (II) chloride

c)

Iron (III) chloride

d)

Iron trichloride

9.

Identify Ammonium Sulfate

a)

NH4SO4

b)

(NH4)2(SO4)3

c)

(NH4)3(SO4)2

d)

(NH4)2SO4

10.

Name the ionic compound SnSe2

a)

Tin diselenide

b)

Tin (IV) Selenide

c)

Tin selenide

d)

Tin (II) triselenide

11.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
12.
magnesium sulfate
a)
MgSO4
b)
Mg(SO4)2
c)
Mg2SO4
13.

The polyatomic ion in KNO3 is:

a)

K+

b)

NO3-

c)

KNO3-

d)

NO2-

14.

Which of the following best describes covalent bonding?

a)

Transfer of electrons

b)

Sharing of electron pairs between atoms

c)

Formation of ions

d)

Metallic bonding

15.

Which types of atoms typically undergo covalent bonding?

a)

Metals and non-metals

b)

Metals

c)

Non-metals

d)

Noble gases

16.

What is the electronegativity difference for a non-polar covalent bond?

a)

0.0-0.4

b)

0.4-1.0

c)

1.0-2.0

d)

Greater than 2.0

17.

Which bond has the highest bond energy?

a)

C-C

b)

C=C

c)

C≡C

d)

C-H

18.

How many valence electrons are in a molecule of CO2?

a)

8

b)

16

c)

24

d)

32

19.

Since covalent compounds do not have free charges, they are

a)

good conductors

b)

poor conductors

c)

ionic

d)

metallic

20.

How do atoms achieve a full outer electron shell in covalent bonding?

a)

By losing electrons

b)

By gaining electrons

c)

By sharing electrons

d)

By transferring electrons

21.
tricarbon nonahydride
a)
CH9
b)
C3H9
c)
C3OH9
d)
C3(OH)9
22.
boron dibromide
a)
B2Br
b)
BBr2
c)
BBr
d)
B2Br2
23.

Silicon dioxide is the compound in sand. What is its formula?

a)

SO2

b)

NaO2

c)

SiO2

d)

SiO

24.

Which formula is for phosphorus trichloride?

a)

KCl3

b)

PCl3

c)

K3Cl

d)

P3Cl

25.

Which of the following pairs of elements is most likely to form a nonpolar covalent bond?

a)

H and O

b)

N and N

c)

Na and Cl

d)

C and O

26.

What is the molecular geometry of a molecule with 4 bonding pairs and no lone pairs on the central atom?

a)

Linear

b)

Bent

c)

Trigonal planar

d)

Tetrahedral

27.

What is the percent composition of carbon in CO2?

a)

27%

b)

33%

c)

44%

d)

66%

28.

How do you determine the percent composition of an element in a compound?

a)

By dividing the atomic mass of the element by the molar mass of the compound and multiplying by 100

b)

By dividing the number of atoms of the element by the total number of atoms in the compound

c)

By dividing the atomic number of the element by the total number of elements in the compound

d)

By dividing the molecular mass of the element by the molar mass of the compound and multiplying by 100

29.

What is the percent water in the hydrate CuSO4·5H2O?

a)

25%

b)

36%

c)

44%

d)

56%

30.

Which of the following compounds has the highest melting point?

a)

NaCl

b)

H2O

c)

CO2

d)

CH4

31.

An empirical formula represents:

a)

The actual number of atoms of each element in a molecule

b)

The simplest whole number ratio of atoms of each element in a compound

c)

The structural arrangement of atoms in a molecule

d)

The percent composition of a compound

32.

What is the empirical formula of a compound that is 40% sulfur and 60% oxygen by mass?

a)

SO2

b)

SO3

c)

S2O3

d)

S3O4

33.

If the empirical formula of a compound is CH2O and its molar mass is 180 g/mol, what is the molecular formula?

a)

CH2O

b)

C2H4O2

c)

C3H6O3

d)

C6H12O6

34.

Which of the following elements exists as a diatomic molecule?

a)

Boron

b)

Chlorine

c)

Neon

d)

Carbon

35.

What is the molecular formula of a compound with an empirical formula of CH and a molar mass of 78 g/mol?

a)

CH

b)

C2H2

c)

C6H6

d)

C3H3

36.

The reaction between hydrogen gas and oxygen gas to form water is written as:

a)

H2 + O2 → H2O

b)

2H2 + O2 → 2H2O

c)

2H + O → H2O

37.

Balance the equation: ___Al + ___O2 → ___Al2O3

a)

1, 1, 1

b)

2, 3, 1

c)

4, 3, 2

d)

3, 2, 1

38.

Which type of reaction is represented by the equation 2H2 + O2 → 2H2O?

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

39.

How many moles of H2O are produced when 2 moles of H2 react with 1 mole of O2?

a)

1 mole

b)

2 moles

c)

3 moles

d)

4 moles

40.

In the reaction N2 + 3H2 → 2NH3, the mole ratio of N2 to NH3 is:

a)

1:1

b)

1:2

c)

1:3

d)

2:3

41.

How many grams of H2O are produced from 8 grams of H2 in the reaction 2H2 + O2 → 2H2O?

a)

72 grams

b)

36 grams

c)

18 grams

d)

54 grams

42.

How many grams of CO2 are produced from 44 grams of O2 in the reaction C + O2 → CO2?

a)

44.0 grams

b)

88.0 grams

c)

22.5 grams

d)

60.5 grams

43.

If the theoretical yield of a product is 20 grams and the actual yield is 16 grams, what is the percent yield?

a)

75%

b)

80%

c)

85%

d)

90%

44.
4 Al + 3 O2 –> 2 Al2O3  How much aluminum would be needed to completely react with 45 grams of O2?
a)
1.05 moles
b)
3.75 moles
c)
1.875 grams
d)
1.875 moles
45.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
46.
How many grams are in 7.8 moles of NaCl?
a)
476grams
b)
460 grams
c)
452 grams
d)
462 grams
47.
Balance the following reaction :
 
CaC₂(s)   +   H₂O(l)   -->   C₂H₂(g)   +   Ca(OH)₂(aq)
a)
1,2,2,2
b)
1,2,1,1
c)
2,1,1,1
d)
2,1,2,1
48.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
49.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
50.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
51.
2 KClO3 → 2 KCl + 3 O2
How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?
a)
6.7 mol
b)
1.0 mol
c)
10.1 mol
d)
4.5 mol
52.
 SiO2 + 3C → SiC + 2CO
I need to add 8 moles of Carbon to the reaction. How many grams of Carbon should I weigh?
a)

96 g

b)
0.67 g
c)
2.67 g
d)
48 g
53.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
54.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)  
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
55.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

56.

What is the shape of a CH2Cl2 molecule?

a)

Linear

b)

Trigonal planar

c)

Tetrahedral

d)

Octahedral

57.

Which geometric molecular shape is shown?

a)

trigonal planar

b)

linear

c)

bent

d)

trigonal pyramidal

58.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
59.
What is the empirical formula of the following molecular formula:  C3H6
a)
C3H6
b)
CH2
c)
C2H4
d)
CH3
60.

You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.

a)

SO

b)

SO2

c)

SO3

d)

SO4

61.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
62.
What is the percent composition by mass of oxygen in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
63.
What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?
a)
CH2O
b)
C2H4O2
c)
C4H8O4
d)
C6H12O6
64.
Glycerol has a molar mass of 92.09g/mol. Its percent composition is: 39.12% C, 8.75% H, and 51.12% O. What is the molecular formula for glycerol?
a)
C2H3O2
b)
CH2O
c)
C2H4O2
d)
C3H8O3
65.
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
66.

Determine the amount of moles in CuBr that are in 276.9 g of the compound.

a)

3.2 mol

b)

1.7 mol

c)

2.1 mol

d)

1.9 mol

67.

Determine the number of moles of Mg3P2 that are in 583 g of the compound.

a)

2.9 mol

b)

6.1 mol

c)

4.3 mol

d)

1.7 mol

68.

What is the molar mass of NaCl?

a)

49.46 g/mol

b)

58.44 g/mol

c)

152.92 g/mol

d)

161.90 g/mol

69.

What is the molar mass of MgF2?

a)

62.31 g/mol

b)

67.62 g/mol

c)

43.31 g/mol

d)

86.62 g/mol

70.

What is the molar mass of Al(NO3)3?

a)

62.01 g/mol

b)

88.99 g/mol

c)

151.00 g/mol

d)

213.01 g/mol

71.

What is the molar mass of (NH4)2S?

a)

57.18 g/mol

b)

68.17 g/mol

c)

32.07 g/mol

d)

17.04 g/mol

72.
What molecular shape is the structure shown here? (BCl3)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
73.
Which of the following equations are correctly balanced?
a)
12CO2 +H2O --> C6H12O6 + O2
b)
CO2 + 9H2O --> C6H12O6 + O2
c)
CO2 + H2O --> 3C6H12O6 + O2
d)
6CO2 + 6H2O --> C6H12O6 + 6O2
74.
Which of the following is an unbalanced equation?
a)
CaCO3 --> CaO + CO2
b)
PbO2 + 2H2-->2Pb + H2O
c)
2Na+ 2H2O-->2NaOH + H2
d)
CS2 + 2O2 --> CO2 + 2SO2
75.

Balanced this equation:

Sb2S3 + O2 ---> Sb + SO2

a)

It is balanced.

b)

Sb2S3 + O2 ---> 2Sb + SO2

c)

Sb2S3 + 3O2 ---> 2Sb + 3SO2

d)

3Sb2S3 + 3O2 ---> 2Sb + SO2

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