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Chemistry Chapter 3 Practice Test

Total questions: 63

Worksheet time: 3hrs 9mins

Name
Class
Date
1.

What is the average atomic mass of Neon?

a)

10 amu

b)

20.18 amu

c)

10.18 amu

d)

22.18 amu

2.
How many protons are in Beryllium?
a)
4
b)
9
c)
5
d)
2
3.
How many neutrons are in a Gold atom?
a)
79
b)
196
c)
118
d)
275
4.
How many electrons does a Copper atom have?
a)
63
b)
29
c)
92
d)
34
5.
Where is most of the mass of the atom contained?
a)
In the protons
b)
In the neutrons
c)
In the electron cloud
d)
In the nucleus
6.
Which particle has a similar mass to a proton?
a)
Electron
b)
Neutron
c)
Photon
d)
Marble
7.
Which atomic particle has a positive charge?
a)
Proton
b)
Neutron
c)
Electron
8.
Which subatomic particle has a neutral charge?
a)
Proton
b)
Neutron
c)
Electron
9.

A mole of potassium contains 6.022 x 1023 _____.

a)

atoms

b)

formula units

c)

ions

d)

molecules

10.
Molar mass is in units of ________.
a)
grams
b)
grams/mole
c)
mole
d)
moles/gram
11.
Which compound has the smallest molar mass?
a)
CO
b)
CO2
c)
H2O
d)
H2O2
12.
Which represents the greatest mass of sulfur?
a)
1 gram of sulfur
b)
1 atom of sulfur
c)
0.5 mole of sulfur
d)
6.02 x 1023 atoms of sulfur
13.
How many grams are in 1.2 x 1024 atoms of C?
a)
28 grams
b)
24 grams
c)
6.02 grams
d)
1.2 grams
14.
What is the mass of 2.50 mol of Helium gas He?
a)
40 g
b)
10 g
c)
16 g
d)
32 g
15.

How many water molecules are in 5.2 moles of water?

a)

6.02 x 1023 molecules

b)

5.2 molecules

c)

3.1304 x 1024 molecules

d)

8.638 x 10-24 molecules

16.

Calculate the number of moles copper (II) sulfate in 320g of CuSO4.

a)

2 moles

b)

4 moles

c)

6 moles

d)

8 moles

17.

Calculate the number of moles of carbon dioxide contained in 11g of CO2.

a)

0.25 mol

b)

0.5 mol

c)

11 mol

d)

44 mol

18.

Who is the early Greek philosopher that coined the term atoms?

a)

Democritus

b)

Aristotle

c)

J.J. Thomsen

d)

Rutherford

19.

Which subatomic particle was found using the cathode ray?

a)

protons

b)

neutrons

c)

electrons

d)

megatrons

20.

Isotopes have the same number of _________ but different number of __________

a)

electrons ; protons

b)

protons ; electrons

c)

neutrons ; protons

d)

protons ; neutrons

21.

Which two particles have about the same mass?

a)

electrons & protons

b)

protons & neutrons

c)

electrons & neutrons

d)

positrons & neutrons

22.

When writing an isotope in symbolic notation, what does the top number represent?

a)

number of protons

b)

number of electrons

c)

mass number

d)

number of neutrons

23.

If a cathode ray contains electrons, which way would the ray bend?

a)

towards a positively charged plate

b)

towards a negatively charged plate

c)

it would not bend

d)

backwards

24.

Which scientist described a positively charged core ("nucleus") in the middle of a lot of empty space?

a)

Chadwick

b)

Thomson

c)

Rutherford

d)

Bohr

25.

Which scientist described an atom made of a solid positively charge substance with electrons dispersed throughout it?

a)

Rutherford

b)

Thomson

c)

Chadwick

d)

Bohr

26.

What are the components (parts) of an atom?

a)

protons

b)

neutrons

c)

electrons

d)

positrons

27.

Which scientist discovered the first subatomic particle, the electron?

a)

Rutherford

b)

Democritus

c)

Thomson

d)

Bohr

28.

Milikan used the oil drop experiment to discover what about the electron?

a)

melting point

b)

velocity

c)

charge

d)

boiling point

29.

Which is an example, that proved part of Dalton's atomic theory incorrect?

a)

atoms are small

b)

isotopes

c)

law of conservation of mass

d)

bonds break and recombine

30.

How many atoms are in this molecule of AgBr2?

a)

1

b)

2

c)

3

d)

4

31.

The law of __________ states that a compound is always composed of the same elements in the same proportion by mass

a)

conservation of mass

b)

conservation of energy

c)

definite proportions

d)

multiple proportions

32.
The smallest particle of an element that retains the properties of that element
a)
protons
b)
neutron
c)
electron
d)
atom
33.
A subatomic particle with no charge
a)
proton
b)
neutron
c)
electron
d)
atom
34.
Atoms with the same number of protons, but a different number of neutrons
a)
isotope
b)
atomic mass
c)
mass number
d)
atomic mass unit
35.
The total number of protons and neutrons in an atom
a)
isotope
b)
atomic mass
c)
mass number
d)
atomic mass unit
36.
The number of protons in the nucleus of an element
a)
atomic number
b)
atomic mass
c)
mass number
d)
atomic mass unit
37.

The weighted average of the masses of the isotopes of an element

a)

atomic number

b)

average atomic mass

c)

mass number

d)

atomic mass unit

38.

One-twelfth the mass of a carbon-12 atom

a)

atomic number

b)

average atomic mass

c)

mass number

d)

atomic mass unit

39.
Dalton said that atoms are indivisible and all atoms of an element are identical.  It is now known that
a)
all of Dalton's hypotheses are correct
b)
atoms of an element can have different number of protons
c)
atoms are divisible
d)
atoms of an element are not identical, but must have the same mass
40.
Which of these is true about subatomic particles
a)
Electrons are negatively charged and are the heaviest subatomic particle
b)
Protons are positively charged and the lightest subatomic particle
c)
Neutrons have no charge and are the lightest subatomic particle
d)
The mass of a neutron nearly equals the mass of a proton
41.
The particles found in the nucleus are
a)
neutrons and electrons
b)
electrons only
c)
protons and neutrons
d)
protons and electrons
42.
The atomic number of an element is the total number of which particles?
a)
neutrons
b)
protons
c)
electrons
d)
protons and electrons
43.
An element has an atomic number of 66.   The number of protons and electrons in a neutral atom of the element are ____. 
a)
66 protons and 33 electrons 
b)
33 protons and 33 electrons 
c)
66 protons and 0 electrons 
d)
66 protons and 66 electrons 
44.
The sum of the protons and neutrons equals the 
a)
atomic number
b)
nucleus number
c)
mass number
d)
atomic mass
45.

Using the periodic table, determine the number of neutrons in Sulfur-32

a)

8

b)

16

c)

32

d)

48

46.
Which of the following equals one atomic mass unit
a)
The mass of one electron
b)
The mass of one helium-4 atom
c)
The mass of one carbon-12 atom
d)
one-twelfth the mass of a carbon-12 atom
47.
What is the atomic number for an element with 85 neutrons and a mass number of 128?
a)
85
b)
128
c)
213
d)
43
48.
What is the molar mass of GaI3?
a)
196.62 g/mol
b)
450.42 g/mol
c)
336.06 g/mol
d)
4.5042 g/mol
49.

How many moles are in 8.31 x 1024 silver atoms

a)

5.00 x 1048 moles

b)

13.80 moles

c)

1.38 x 1049 moles

d)

1.38 moles

50.
What is the mass of 3.18 x 1025 atoms of Pd?
a)
52.82 grams
b)
5620 grams
c)
1.78 x 1047 grams
d)
.496 grams 
51.
If silver contained 63.45% silver-107 and 36.55% silver-109, its atomic mass would be
a)
107.73 g/mol
b)
108.27 g/mol
c)
109.45 g/mol
d)
10773.1 g/mol
52.
How many neutrons are in Bromine-84
a)
35 neutrons
b)
49 neutrons
c)
84 neutrons
d)
79.90 neutrons
53.

Thomson concluded that cathode rays have a negative charge. Why did his experiment lead him to this conclusion?

a)

Opposite charges attract

b)

Like charges attract

c)

Opposite charges repel

d)

Like charges repel

54.

What did Thomson call his model of the atom?

a)

The electronegativity model

b)

The plum pudding model

c)

The Thomson model

d)

The cathode ray model

55.

Which of the following is NOT a conclusion reached in Rutherford's experiment?

a)

Atoms are mostly empty space.

b)

Atoms have a dense center with a positive charge.

c)

All atoms are identical.

d)

The area surrounding the nucleus contains the electrons.

56.

In his experiment, Rutherford concluded that atoms have a nucleus because

a)

most of the particles went straight through the foil.

b)

some of the particles were deflected near the front of the screen.

c)

some of the particles were deflected back towards the alpha source.

d)

not enough information is given.

57.
What is the mole used for? 
a)
To measure the amount of grams in a substance
b)
To measure the amount of atoms or molecules in a substance
c)
To measure the amount of energy in a substance
d)
To measure the amount of bonding in a substance 
58.
Avogadro's number of representative particles is equal to one_____.
a)
kilogram
b)
gram
c)
kelvin
d)
mole
59.

What is Avogadro's Number?

a)

6.022 x 1023

b)

- 6.022 1023

c)

6.022 x 1022

d)

6,022,000,000,000

60.

A mole of Neon contains

6.022 x 1023 _____.

a)

atoms

b)

formula units

c)

ions

d)

molecules

61.
Where do you look to calculate the molar mass?
a)
avogadros number
b)
periodic table 
62.

What is the molar mass of one molecule of Nitrogen N2?

a)

14.01 amu

b)

14.01 g/mol

c)

28.02 g/mol

d)

28.02 amu

63.

What is the molar mass of Carbon Dioxide (CO2)?

a)

12 amu

b)

12 g/mol

c)

44 g/mol

d)

44 amu

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