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Fall Semester Chemistry Review

Total questions: 75

Worksheet time: 6hrs 15mins

Name
Class
Date
1.
Which state of matter will hold its shape without a container?
a)
Solid
b)
Liquid
c)
Gas
d)
Plasma
2.
The kinetic theory states that the higher the temperature, the faster the 
a)
particles that make up a substance move
b)
bonds between atoms break down
c)
molecules of gas rush together
d)
lighter particles within a substance clump together
3.
What scientist is best known for his "Plum Pudding" model of the atom?
a)
J.J. Tomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
4.
Rutherford's gold foil experiment provided evidence that...
a)
Negative and positive charges are spread evenly throughout the atom.
b)
Alpha particles have a positive charge.
c)
Gold is not a dense as previously thought.
d)
There is a dense positively charged nucleus at the center of an atom.
5.

How many electrons are in an atom with an atomic number of 20, an atomic mass of 45, and a charge of +2?

a)

20

b)

10

c)

2

d)

18

6.
What particle provided the positive charge for an atom?
a)
proton 
b)
neutron
c)
electron
d)
nucleus
7.
Which particle does not contribute mass to the atom?
a)
Proton
b)
Neutron
c)
Electron
d)
Nucleus
8.

Which of the following families is the least electronegative?

a)

noble gases

b)

Halogens

c)

transition metals

d)

alkali metals

9.
Which element has the highest ionization energy?
a)
F
b)
Cl
c)
Br
d)
I
10.
Give the formula for oxygen dichloride
a)
OCl2
b)

O2Cl2

c)
OCl
d)
O2Cl
11.

Give the formula for copper(II) chloride

a)

CuCl2

b)

CuCl

c)

Cu2Cl

d)

Cu2Cl2

12.

Give the formula for magnesium carbonate

a)

Mg2C

b)

Mg2CO4

c)

Mg2(CO3)2

d)

MgCO3

13.

Name the compound:

CCl4

a)

carbon carbon tetraiodide

b)

carbon tetrachloride

c)

monocarbon tetrachloride

d)

water

14.

Name the compound:

Ba3(PO4)2

a)

tribarium diphosphate

b)

barium diphosphate

c)

barium phosphate

d)

barium phosphide

15.

Name the compound:

SnO2

a)

tin(II) oxide

b)

tin(IV)oxide

c)

tin(II)oxegen

d)

tin oxide

16.

What is the Law of Conservation of Mass?

a)

It states that no matter can be created or destroyed.

b)

It states that matter can be created or destroyed.

c)

It states that no sound can be created or destroyed.

17.
At the end of chemical reactions, what is the total mass of the reactants compared to the total mass of the products?
a)
the product is doubled
b)
the product is half the mass of the reactants
c)
the mass is the same
d)
the mass changes depending on the reaction
18.

Which of the following is an example of synthesis?

a)

2Na + Br2 --> 2NaBr

b)

2KClO3 --> 2KCl + 3O2

c)

2HgO + Cl2 --> 2HgCl + O2

d)

Cl2 + 2NaBr --> 2NaCl + Br2

19.
Which chemical reaction forms Carbon Dioxide and Water?
a)
Double Replacement
b)
Single Replacement
c)
Combustion
d)
Decomposition
20.
What coefficient should be used to make the following equation balanced?
N2+O2--> _NO 
a)
1
b)
2
c)
3
d)
4
21.
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
22.

How many grams are in 1.5 moles of O?

a)

9.0 x 1023 grams

b)

16 grams

c)

24 grams

d)

6.0 x 1023 grams

23.

How many moles are in 4.30 x 1024 molecules of H2O?

a)

6.02 x 1023

b)

7.14

c)

18.0

d)

129

24.

How many molecules are in 100. g of C6H12O6?

a)

180. g

b)

3.34 x 1023

c)

6.02 x 1023

d)

6.02 x 1025

25.
In the equation 2 Al2O3 --> 4 Al + 3 O2, what is the mole ratio of aluminum to oxygen?
a)
10:6 
b)
3:4
c)
4:3
d)
2:3
26.

How many moles of H2O are produced by 4.8 moles of O2?

2H2 +O2 --> 2H2O

a)

9.6 mol H2O

b)

317 mol H2O

c)

906 mol H2O

d)

3.7 mol H2O

27.

From the reaction: B2H6 + 3O2 --> 2HBO2 + 2H2O

What mass of O2 will be needed to burn 36.1 g of B2H6?

a)

62.6 g O2

b)

3.91 mol of O2

c)

125 g O2

28.
How many liters of NH3 are needed to react completely with 30.0L of NO at STP?
4NH3+6NO --> 5N2 + 6H2O
a)
5.0 L
b)
20.0 L
c)
7.5 L
d)
120.0 L
29.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
30.

You have a gas that has a pressure of 2 atm and a volume of 10L. What would be the new volume if the pressure was changed to 1 atm?

a)

5 L

b)

20 L

c)

It would stay at 10L

d)

1 L

31.
In the ideal gas law, which variable represents the gas constant?
a)
n
b)
R
c)
T
d)
V
32.

A gas has a volume of 55.0L at a temperature of 55.0 degrees Celsius. What temperature will the gas be if the volume increased to 76.0 L?

a)

453 K

b)

275 K

c)

502 K

d)

353 K

33.

How many significant figures does 1.90 have?

a)

3

b)

2

c)

6

d)

1

34.

Round 0.010229 to four sig figs

a)

1022

b)

1023

c)

0.01023

d)

0.0102

e)

0.01022

35.
Solve & Round to Correct Sig Figs.
100 / 2.0 = 
a)
50
b)
50.
c)
50.0
d)
50.00
36.
Multiply (2.45 x 104) x (8.78 x 106) and express in scientific notations.
a)
2.15 x 1011
b)
2.15 x 1014
c)
2.10 x 1014
d)
2.10 x 1015
37.
Which of the following is correct scientific notation?
a)
20.35 x 104
b)
.2035 x 104
c)
2035 4
d)
2.035 x104
38.

What is the molarity of 4.0 grams of sodium chloride in 3,800 mL of solution?

a)

0.018 M

b)

0.0011 M

c)

1.052 M

d)

0.062 M

39.
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
40.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
41.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
42.

What element is on period 4 group 10?

a)

Db

b)

Ni

c)

Pd

d)

Ti

43.

Molar mass of NaOH is ______________________

a)

40.00 grams/mol

b)

50.00 grams/mol

c)

45.00 grams/mol

d)

38.00 grams/nol

44.
The variable that a scientist changes in a scientific experiment is called the:
a)
Independent
b)
Dependent
c)
Control
d)
Constant
45.
The alkali metals have how many valence electrons?
a)
1
b)
2
c)
7
d)
8
46.
Which particles give the identity of an atom?
a)
Protons
b)
Neutrons
c)
Electrons
d)
Valence electrons
47.
Which type of bond uses the transfer of electrons?
a)
covalent bonds
b)
ionic bonds
c)
metallic bonds
d)
all chemical bonds
48.
Isotopes are elements that have variations in the number of:
a)
electrons
b)
neutrons
c)
protons
d)
ions
49.

Covalent bonds form when

a)

the electronegativity difference between two atoms is very large.

b)

electrons are completely transferred between two atoms.

c)

pairs of electrons are shared between two atoms.

d)

ions are held together by opposite charges.

50.
Which of the following is a chemical change?
a)
Iron rusting 
b)
Glass breaking
c)
Clothing ripping
d)
Hair cut
51.

If a sample has a mass of 1.25 x 102 g and a volume of 50. mL, what is its density? Is it a physical or chemical property?

a)

0.40 g/mL; physical

b)

0.40 g/mL; chemical

c)

2.5 g/mL; physical

d)

2.5 g/mL; chemical

52.
What is the volume occupied by 51.0 g of NH3 gas at STP?
a)
0.439 L
b)
22.8 L
c)
67.2 L
d)
91.9 L
53.

Which of these are pure substances?

a)
A only
b)
A and C
c)
D and A
d)
A and B
54.
 68 cm = ___________ mm
a)
0.68
b)
6.8
c)
68
d)
680
55.
This bullseye demonstrates...
a)
High Accuracy & High Precision
b)
High Accuracy & Low Precision
c)
Low Accuracy & High Precision
d)
Low Accuracy & Low Precision
56.
The students measured length during a science experiement, they got 12 cm. But the actual measurement was 14.25 cm. What was the percent error?
a)
15.79%
b)
18.75%
c)
2.25%
d)
18%
57.
Separating mixtures based on boiling points.
a)
Desalination
b)
Distillation
c)
Decantation
d)
Condensation
58.

24.1% of all the isotopes of a an element have a mass of 75.23 amu, 48.7% have a mass of 74.61 amu, and 27.2% have a mass of 75.20 amu. What is the average mass of this element?

a)
74.92 amu
b)
24.97 amu
c)
75.01 amu
d)
74.51 amu
59.
Solve this equation for beta decay.
614C = ___ + -10e
a)
410Be
b)
714N
c)
210He
d)
613C
60.

If 10.0 mg of iodine 131 is given to a patient, how much is left after 24 days? The half-life of iodine-131 is 8 days.

a)
1.25mg
b)
1.25g
c)
10g
d)
10mg
61.

When an atom _______________ _____________, its electrons can use this energy to move to a higher energy level.

a)

releases energy

b)

absorbs energy

c)

emits radiation

d)

gets rid

62.
What is the basis of a metallic bond?
a)
the attraction of neutral metal atoms.
b)
the attraction between protons and neutrons.
c)
the attraction between positive metal ions and interlocking electrons.
d)
the attraction between positive metal ions and free floating electrons.
63.
N2, Cl2, and O2 are all 
a)
diatomic molecules.
b)
ionic bonds.
c)
of equal mass.
d)
solids.
64.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
65.

According to the kinetic molecular theory, all collisions between gas molecules are inelastic; all kinetic energy is lost.

a)

True

b)

False

66.

How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?

a)

27.8 mL

b)

.278 mL

c)

2.8 mL

d)

278 mL

67.

How much water must be added to prepare a 0.2M dilute solution KBr? Your stock solution is 100 mL of 1.5M KBr.

a)

175 mL

b)

750 mL

c)

650 mL

d)

13.3 mL

68.

Which is the correct set of acid properties:

a)

sour taste, corrosive, change litmus from red to blue

b)

sour taste, corrosive, change litmus from blue to red

c)

sweet taste, slippery, change litmus from blue to red

d)

sour taste, slippery, change litmus from blue to red

69.

Which of the following statements is true concerning acids and bases?

a)

acids and bases don't react with each other

b)

acids mixed with bases neutralize each other

c)

acids mixed with bases make stronger bases

d)

acids mixed with bases make stronger acids

70.

Is pure water acidic, basic, or neutral?

a)

Acidic

b)

Basic

c)

Neutral

71.

The pH scale is a range from:

a)

1 - 7

b)

0 - 14

c)

1 - 5

d)

1 - 14

72.

If the [H3O+] of a solution is 1 x 10-3 M, the pH is

a)

11

b)

-3

c)

3

d)

1

73.

Oranges have a [H3O+] of 1.7 x 10-2 M. Their pOH is

a)

1.77

b)

12.23

c)

10.91

d)

3.09

74.

Eggs have a pOH of 5.4. Eggs are a(n) __________.

a)

acid

b)

base

c)

neutral

d)

metal

75.

A solution of KOH is 1.0 x 10-5 M. What is the [H+] concentration?

a)

5

b)

9

c)

1.0 x 10-9

d)

1.0 x 10-5

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