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Final Review Spring 2023

Total questions: 77

Worksheet time: 1hrs 24mins

Name
Class
Date
1.
How do the following two elements bond together?
K1+  S2- 
a)
KS
b)
K8S
c)
K6S3
d)
K2S
2.
When an ionic compound is formed, its charge is 
a)
negative
b)
neutral (no charge)
c)
positive
3.
The proper formula for magnesium hydroxide:
a)
MgOH
b)
Mg2OH
c)
Mg(OH)2
d)
Mg2OH2
4.
Magnesium bromide is an ionic compound with the chemical formula MgBr₂.  What does the "2" tell you?
a)
There are 2 bromide ions for every magnesium ion
b)
Bromide has a 2- charge
c)
Bromide has a 2+ charge
d)
There are 2 magnesium ions to every bromide ion
5.
What do Roman Numerals represent in the name of a transition metal compound?
a)
how many atoms of the metal there are
b)
the oxidation number of the nonmetal
c)
the oxidation number of the metal
d)
the mass number
6.
Phosphorous trichloride
a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCL
7.

What letter on the diagram represents a gas?

a)

A

b)

B

c)

C

d)

D

8.

What is the boiling point of this substance at 1 ATM of pressure?

a)

40

b)

60

c)

100

d)

110

9.

Any substance that does not conduct electricity when in solution is called a(n) ―

a)

nonelectrolyte

b)

electrolyte

c)

conductor

d)

semiconductor

10.
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
11.
The red numbers in the image below represent ________
a)
subscripts
b)
coefficients
c)
I don't know, and don't want to try
d)
None of the answers are correct
12.

What is the right part of a chemical equation called...

H2 + O2 --> H2O

a)

Reactants

b)

Products

c)

Yields

d)

Chemical Equation

13.

What is the arrow in a chemical equation...

H2 + O2 --> H2O

a)

Reactants

b)

Products

c)

Yields

d)

Chemical Equation

14.
When balancing equations a ____ can be placed to the left of a formula of a substance to make the equations balanced
a)
charge
b)
subscript
c)
random number
d)
coefficient
15.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__Al + __O2--> __Al2O3
a)
4,1 --> 2
b)
4,3 --> 4
c)
3,4 --> 1
d)
4,3 --> 2
16.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__CH4 + __O2 --> __CO2+ __H2O
a)
2,1 --> 2,1
b)
1,2 --> 1,1
c)
1,2 --> 1,2
d)
1,2 --> 2,1
17.
AB + CD →AD + CB
a)
Double Replacement
b)
Single Replacement
c)
Synthesis
d)
Decomposition
18.
Identify this type of reaction,
Cl2 + 2KI -->  I2 + 2KCl
a)
Synthesis
b)
Single displacement
c)
Double displacement
d)
Decomposition
19.
2 AgNO3 + Cu --> Cu(NO3)2 + 2 Ag 
a)
single displacement
b)
double displacement
c)
decomposition
d)
synthesis
20.
Which of the following describes a precipitate?
a)
a liquid forms when a block of metal is heated
b)
a solid forms when one liquid is poured into another
c)
a gas forms when a solid is placed in a liquid
d)
bubbles form when an acid is poured on a rock
21.

What type of reaction is this?

2C5H10 + 15O2 → 10CO2 + 10H2O

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

22.

N2 + 3H2 → 2NH3


How many moles of H2 is needed to react with 2 moles of N2?

a)

6

b)

3

c)

2

d)

1

23.

Where are the numbers for a mole ratio found?

a)

They are part of the chemical formulas for the reactants / products.

b)

They are given in the problem.

c)

They are found on the periodic table for those elements.

d)

They are found as coefficients in the reaction's balanced chemical equation.

24.

2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

New problem: How many moles of ethane (C2H6) are required to produce 13.5 moles of water from the above reaction?

a)

4.5 mol C2H6

b)

27 mol C2H6

c)

40.5 mol C2H6

d)

81 mol C2H6

e)

162 mol C2H6

25.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
26.
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
27.

A sample contains 36.95 g of mercury (Hg) and 13.05 g of chlorine (Cl). What is the empirical formula for this compound?

a)

HgCl2

b)

Hg3Cl

c)

Hg17Cl36

d)

HgCl

28.

Which of the following is NOT a unit used to express concentration?

a)

Molality

b)

Molarity

c)

Mass percent

d)

Density

29.
The pH of a solution is tested, and it is found to be a basic solution. Of the following choices, what could the pH have been?
a)
3
b)
9
c)
7
d)
5
30.
When dissolved in water, acids produce:
a)
bases
b)
salts
c)
hydrogen ions
d)
hydroxide ions
31.

The pH actually measures:

a)

the strength of an acid.

b)

the strength of hydrogen ions.

c)

the concentration of hydrogen ions.

d)

the strength of a base.

32.
The amount of solute actually dissolved in a given amount of solvent.
a)
dilution
b)
concentration
c)
saturated solution
d)
supersaturated mixture
33.
__________ are made up of solutes and solvents.
a)
Solutions
b)
Suspensions
c)
Heterogeneous Mixtures
d)
Pure Substances
34.
The pH scale is a range from:
a)
1-7
b)
0-14
c)
1-5
d)
1-20
35.
A(n) _______ is a substance with a pH greater than 7.
a)
Base
b)
Acid
c)
Buffer
d)
Water
36.

What is present in aqueous solutions of an acid or alkali that allow them to conduct electricity?

a)

mobile electrons

b)

mobile ions

c)

mobile atoms

d)

mobile molecules

37.
The limiting reactant
a)
slows the reaction down
b)
is used up first
c)
is the reactant that is left over
d)
controls the speed of the reaction
38.

This is what you call a reactant that you have enough of. The one that DOES NOT run out.

a)

Limiting Reactant

b)

Excess Reactant

c)

Highly Reactant

d)

Super Reactant

39.

Water molecule are polar molecule so, in a solution of water, the water molecules attract eachother by

a)

covalent bond

b)

Hydrogen bond, it's a type of Van Der Waals force

c)

ionic bond

40.

Ice float on water because the ice is less dense that liquid water.

a)

True

b)

False

41.

Polar molecules will dissolve in other polar molecules and nonpolar molecules will dissolve in other nonpolar molecules.

a)

True

b)

False

42.

2Na + 2H2O → 2NaOH+ H2

Assuming H2O is in excess, how many grams of hydrogen can be produced with 120 g of Na?

a)

5.2 g

b)

2.6 g

c)

690 g

d)

45 g

43.
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
44.
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
45.
What is the molar mass of CO2?
a)
12
b)
16
c)
32
d)
44
46.
Molar mass is in units of ________.
a)
grams
b)
grams/mole
c)
mole
d)
moles/gram
47.

The pH actually measures:

a)

the strength of an acid.

b)

the strength of hydrogen ions.

c)

the concentration of hydrogen ions.

d)

the strength of a base.

48.
The amount of solute actually dissolved in a given amount of solvent.
a)
dilution
b)
concentration
c)
saturated solution
d)
supersaturated mixture
49.
What does it mean to dilute a solution?
a)
lower the concentration of solute per solvent
b)
increase the concentration of solute per solvent
50.

What is the overall charge of the ionic compound NaCl

a)

+1

b)

+2

c)

+3

d)

0

51.
What formula results when Ca+2  and  Br- ions bond?
a)
Ca2Br2
b)
CaBr
c)
Ca(br)2
d)
CaBr2
52.

What kind of Ion does Aluminum form?

a)

Al+3Al^{+3}  

b)

Al−3Al^{-3}  

c)

Al−1Al^{-1}  

d)

Al+2Al^{+2}  

53.

Anions gain...

a)

Their onions

b)

respect

c)

electrons

d)

binaries

54.

Losing electrons makes an atom more

a)

of a loser

b)

positively charged

c)

forgetful

d)

than enough

55.

Which two elements would NOT form an ionic bond?

a)

calcium and lithium

b)

calcium and oxygen

c)

lithium and oxygen

d)

calcium and carbon

56.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
57.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
58.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
59.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
60.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
61.
In this molecule, each OXYGEN makes how many bonds?
a)
1
b)
2
c)
3
d)
4
62.
In this molecule, each HYDROGEN makes how many bonds?
a)
1
b)
2
c)
3
d)
4
63.
In this molecule, each CARBON makes how many bonds?
a)
1
b)
2
c)
3
d)
4
64.

Which of the following compounds has only single bonds?

a)

I only

b)

II only

c)

III only

d)

I and III

e)

III and IV

65.
Which of the following is the correct Lewis structure for CH2O?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
66.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
67.

Which atom will never be in the middle of a Lewis Dot structure?

a)

N

b)

C

c)

H

d)

P

68.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
69.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
70.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
71.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Linear
72.
Choose the correct shape for this molecule:
a)
Tetrahedral
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
73.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
74.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
75.

What is the concentration of a solution in parts per million if 0.02 grams of NaCl is dissolved in 1000 grams of solution?

a)

2 ppm

b)

20 ppm

c)

200 pm

d)

0.2 ppm

76.

A 2400.-gram sample of an aqueous solution contains 0.012 gram of NH3. What is the concentration of NH3 in the solution, expressed as parts per million?

a)

5.0 ppm

b)

15 ppm

c)

20. ppm

d)

50. ppm

77.

Which unit can be used to express the concentration of a solution?

a)

mols/L

b)

m/s

c)

g/mol

d)

amu

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