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Worksheets

Chemistry

Total questions: 29

Worksheet time: 37mins

Name
Class
Date
1.

What is the molar mass of 98 gm of H3PO4?

a)

1

b)

2

c)

5

d)

6

2.

An electron is

a)

positively charged

b)

neutral

c)

negatively charged

3.
What is the molar mass of table salt (NaCl)?
a)
116.886 g/mol
b)
35.453 g/mol
c)
22.990 g/mol
d)
58.443 g/mol
4.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
5.

Which of the following is needed to determine the molar mass of a molecule?

a)

Types of elements in the molecule

b)

Quantity of elements in the molecule

c)

Mass of the elements in the molecule

d)

All are correct and needed.

6.
Which would have more atoms?
a)
1 mole of Li
b)
1 mole of Au
c)
1 mole of Si
d)
None, all are equal
7.
The relative atomic mass is the average mass of an atom compared to 
a)
the mass of a carbon-12 atom.
b)
1/12 the mass of a carbon-12 atom
c)
the mass of a hydrogen atom
d)
1/12 the mass of a hydrogen atom
8.
The relative molecular mass of a compound is equal to the sum of its
a)
Atomic mass
b)
Atomic number
c)
Oxidation number
d)
Valence electrons
9.
What is the relative atomic mass of sodium?
a)
11
b)
23
c)
46
d)
64
10.
What is the relative molecular mass of fluorine gas, F2?
a)
19
b)
38
c)
9
d)
18
11.
What is the unit of relative molecular mass?
a)
kilogram
b)
gram
c)
gram per mole (g/mol)
d)
no units
12.
The formula of a compound is M(OH)2. Given that the Mr of the compound is 98, calculate the Ar of M.
a)
32
b)
64
c)
81
d)
94
13.

Find Atomic Mass: What is the mass of one mole of Lithium (Li)?

a)

6.9 grams

b)

14.0 grams

c)

22.9 grams

d)

56.9 grams

14.
Which of the following is NOT a subatomic particle?
a)
Proton
b)
Neutron
c)
Photon
d)
Electron
15.
Atoms of the same element with different numbers of neutrons are called
a)
Ions
b)
Isotopes
c)
Iotas
d)
Introns
16.
The mass listed on the periodic table for each element is known as the 
a)
average atomic mass
b)
atomic mass
c)
atomic weight
d)
weighted mass
17.
Which of the following elements has 13 electrons?
a)
Nitrogen
b)
Aluminum
c)
Silicon
d)
Phosphorus
18.

Each element is defined by the number of

a)

Atoms

b)

Isotopes

c)

Neutrons

d)

Protons

e)

Nuclei.

19.

The atomic mass of an element is the ___.

a)

average of the mass number and the atomic number for the element

b)

weighted average of the masses of the isotopes of the element

c)

total mass of the isotopes of the element

d)

total number of subatomic particles in the nucleus

20.

calculate the relative atomic mass for Ammonium nitrate

a)

80.0

b)

79

c)

60

d)

65

21.

Each element is defined by the number of

a)

Atoms

b)

Isotopes

c)

Neutrons

d)

Protons

e)

Nuclei.

22.

The atomic mass number of a specific element is determined by the:

a)

number of protons in its nucleus

b)

number of neutrons plus protons in its nucleus

c)

number of neutrons plus electrons in its nucleus

d)

number of electrons in its outermost shell

e)

total number of neutrons orbiting the nucleus

23.

Molality (m) = moles of solute / _________________________.

a)

kilogram of solvent

b)

kiloliter of solvent

c)

kilometer of solvent

d)

ounces of solvent

24.

What is the molality of a solution made by dissolving 2 moles of NaOH in 400 grams of water?

a)

5 mol/kg. solvent

b)

4 mol/kg solvent

c)

3 mol/kg. solvent

d)

2.5 moles /kg solvent

25.

molality is defined as ________________________

a)

the moles of solute per kilogram of solvent

b)

moles of solute per liter of solution

c)

mass of solute/ mass of solution

d)

mass of solute/ mass of solvent X 100

26.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
27.
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
28.

A solution that is considered unsaturated would _____.

a)

be dark in color.

b)

have a strong scent.

c)

have a large amount of solute.

d)

have a small amount of solute.

29.

What is the molality of a solution made by dissolving 2 moles of NaOH in 400 grams of water?

a)

5 mol/kg. solvent

b)

4 mol/kg solvent

c)

3 mol/kg. solvent

d)

2.5 moles /kg solvent

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