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Semester Two Review 2023-24

Total questions: 36

Worksheet time: 48mins

Name
Class
Date
1.

The atomic mass of an atom is equal to

a)

number of protons plus number of neutrons

b)

number of protons plus number of electrons

c)

number of electrons plus the number of neutrons

2.

Which part of an atom is used to identify it?

a)

number of protons

b)

number of neutrons

c)

number of electrons

3.

Calculation used to find the number of neutrons in an atom

a)

Mass Number- Atomic Number

b)

Atomic Number - Mass Number

c)

Mass Number - Electrons

d)

protons = electrons = neutrons

4.
The _________ of an element equals the number of protons in an atom of that element
a)
mass number
b)
atomic weight
c)
atomic number
d)
isotopes
5.

To convert from particles to moles, you should multiply by ....

a)
b)
c)
d)
6.

5.11 x 1023 atoms of lithium (Li) is equal to how many moles?

a)

1.18 moles

b)

0.351 moles

c)

1.34 moles

d)

0.849 moles

7.

0.50 moles of carbon (C) is equal to how many grams?

a)

6.0 grams

b)

12.0 grams

c)

8.0 grams

d)

14.0 grams

8.
What is the molar mass of AuCl3?
a)
96 g
b)
130 g
c)
232.5 g
d)
303.3 g
9.
magnesium carbonate
a)
Mg2C
b)
Mg2CO4
c)
Mg2(CO3)2
d)
MgCO3
10.
calcium phosphate
a)
CaPO4
b)
Ca2(PO4)3
c)
Ca3PO4
d)
Ca3(PO4)2
11.
Name the following ionic compound: Cr(NO2)3
a)
chromium nitrite
b)
chromium nitride
c)
chromium III nitride
d)
chromium III nitrite
12.
HNO2
a)
hydronitrogen
b)
hydrogen nitrogen oxygen
c)
nitrous acid
d)
nitric acid
13.
How many molecules are in 2.5 mol of NaCl?
a)
1.51x1023
b)
146
c)
4.15
d)
1.51x1024
14.

The compound with a pink square is known as a ___.

a)

Reactant

b)

Product

15.

Which type of reaction is shown?

a)

Combustion

b)

single replacement

c)

double replacement

d)

decomposition

16.

What type of reaction is shown?

a)

Decomposition

b)

Single replacement

c)

Combustion

d)

Combination (or Synthesis)

17.

What type of reaction is this?

a)

Combination (or Synthesis)

b)

Single replacement

c)

Double replacement

d)

Decomposition

18.

Which type of reaction is shown?

a)

Combustion

b)

Composition (or Synthesis)

c)

Decomposition

d)

Double replacement

19.

To balance this equation, what coefficient must be written in the blue box?

a)

1

b)

2

c)

3

d)

4

20.

What are the products of a combustion reaction?

a)

a single complex compound

b)

several simpler elements

c)

carbon dioxide and water

d)

carbon dioxide and hydrogen

21.

Which type of reaction is shown?

a)

Single replacement

b)

Double replacement

c)

Combustion

d)

Decomposition

22.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
23.

What is the empirical formula for C4H6?

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

24.
What is the best definition for subscript?
 
a)
The big number that tells you the number of molecules.
b)
The atomic number
c)
The little number that tells the number of atoms for each element.
25.
A chemical formula that shows the actual # and kinds of atoms present in one molecule of a compound is called_________
a)
ionic formula
b)
covalent formula
c)
empirical formula
d)
molecular formula
26.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
27.
2H2  +   O2  →  2H2O
How many moles of oxygen are consumed if 8 moles H2 are used?
a)
2
b)
4
c)
6
d)
8
28.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
29.
If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
a)
theoretical yield
b)
mole ratio
c)
actual yield
d)
percentage yield
30.

What is the amount of a product obtained from the actual performance of a chemical reaction called?

a)
mole ratio
b)
theoretical yield
c)
percentage yield
d)
actual yield
31.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
32.
What is the mole ratio of H2O to H3PO4 in the following chemical equation?   P4O10 + 6 H2O --> 4 H3PO4 
a)
6:4
b)
4:6
c)
1:3
d)
3:1
33.
When does a chemical reaction stop?
a)
When the lab is finished
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
34.
9. Complete the equation for the percent yield of a chemical reaction:
Percent yield=(________)÷(________)×100%
a)
actual yield; theoretical yield
b)
theoretical yield; actual yield
35.

A reactant that is leftover (not used up) after a chemical reaction stops

a)
stoichiometry
b)
mole ratio
c)
excess reactant
d)
limiting reactant
36.

Why is it important to identify the limiting reagent?

a)

The limiting reagent speeds up the reaction.

b)

The limiting reagent controls the amount of product formed.

c)

If there is no limiting reagent, the reaction will not occur.

d)

No stoichiometry calculations can be done without a limiting reagent.

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