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Chemistry Final Exam Review

Total questions: 95

Worksheet time: 1hrs 18mins

Name
Class
Date
1.

Which subatomic particle differs between isotopes of the same element?

a)

Protons

b)

Electrons

c)

Neutrons

d)

Nucleus

2.

Carbon-14 has how many neutrons?

a)

6

b)

12

c)

8

d)

14

3.

Which pair are isotopes of the same element?

a)

12C and 14C

b)

16O and 16N

c)

19F and 20Ne

d)

23Na and 24Mg

4.

Atomic size increases as you move:

a)

Down a group

b)

Across a period left to right

c)

Up a group

d)

Toward fluorine

5.

Which element has the highest electronegativity?

a)

Sodium

b)

Calcium

c)

Fluorine

d)

Iodine

6.

A magnesium ion has a charge of:

a)

-1

b)

+2

c)

-2

d)

+1

7.

Which element forms a –3 ion?

a)

Calcium

b)

Oxygen

c)

Nitrogen

d)

Sodium

8.

An O²⁻ ion has how many electrons?

a)

6

b)

8

c)

10

d)

12

9.

How many electron shells are in a Bohr model of sulfur?

a)

1

b)

2

c)

3

d)

4

10.

How many dots are in the Lewis structure of chlorine?

a)

5

b)

7

c)

8

d)

6

11.

Which is a shared property of metals and nonmetals?

a)

Good conductors

b)

Form compounds

c)

High luster

d)

Malleability

12.

Which element is a nonmetal?

a)

Sulfur

b)

Iron

c)

Magnesium

d)

Aluminum

13.

What is the electron configuration of oxygen?

a)

1s² 2s² 2p⁶

b)

1s² 2s² 2p⁴

c)

1s² 2s² 2p²

d)

1s² 2p⁴

14.

How many valence electrons does nitrogen have?

a)

6

b)

5

c)

3

d)

7

15.

Which element is in group 2 and period 6?

a)

Boron

b)

Barium

c)

Calcium

d)

Strontium

16.

How many valence electrons do alkali metals have?

a)

1

b)

2

c)

7

d)

8

17.

What is the molar mass of CO₂?

a)

28 g/mol

b)

44 g/mol

c)

12 g/mol

d)

32 g/mol

18.

How many moles are in 18 grams of water (H₂O)?

a)

1

b)

0.5

c)

2

d)

3

19.

How many atoms are in 1 mole of any substance?

a)

3.01 × 10²²

b)

6.02 × 10¹⁹

c)

6.02 × 10²³

d)

1.00 × 10⁶

20.

What type of reaction is 2Na + Cl₂ → 2NaCl?

a)

Synthesis

b)

Decomposition

c)

Combustion

d)

Double replacement

21.

In CH₄ + 2O₂ → CO₂ + 2H₂O, which is a product?

a)

CH₄

b)

O₂

c)

CO₂

d)

H₂

22.

What is the atomic number of carbon?

a)

6

b)

12

c)

14

d)

8

23.

The mass number of an atom is the sum of:

a)

Protons and neutrons

b)

Protons and electrons

c)

Neutrons and electrons

d)

Electrons only

24.

What is the formula for aluminum oxide?

a)

AlO

b)

Al2O3

c)

Al3O2

d)

Al2O3

25.

What is the formula for calcium chloride?

a)

CaCl

b)

CaCl2

c)

Ca2Cl

d)

Ca2Cl3

26.

What type of bond is formed between two nonmetals?

a)

Covalent

b)

Ionic

c)

Metallic

d)

Polar

27.

Which is an ionic compound?

a)

CO2

b)

NaCl

c)

H2O

d)

O2

28.

How many hydrogen atoms are in H3PO4?

a)

3

b)

4

c)

1

d)

7

29.

What coefficient balances this equation: __H₂ + O₂ → H₂O?

a)

1

b)

2

c)

4

d)

3

30.

Which molecule is polar?

a)

CO₂

b)

CH₄

c)

H₂O

d)

Cl₂

31.

What shape is a molecule with 4 bonds and no lone pairs?

a)

Tetrahedral

b)

Bent

c)

Linear

d)

Trigonal planar

32.

Which statement describes conservation of mass?

a)

Mass of reactants = mass of products

b)

Matter is destroyed in reactions

c)

Mass increases during reactions

d)

Mass is only conserved in physical changes

33.

Which indicates a chemical reaction occurred?

a)

Formation of a gas

b)

Melting

c)

Dissolving sugar

d)

Evaporation

34.

Will zinc replace copper in a single replacement reaction?

a)

Yes

b)

No

c)

Only in acidic solution

d)

Only with heat

35.

Which particle diagram represents a gas?

a)

Widely spaced dots

b)

Closely packed and vibrating dots

c)

Dots in a fixed position

d)

Randomly arranged solids

36.

A single covalent bond contains:

a)

One pair of electrons

b)

Two pairs

c)

Three pairs

d)

Four pairs

37.

What happens to average kinetic energy when a substance is heated?

a)

Increases

b)

Decreases

c)

Stays the same

d)

Disappears

38.

A substance with high specific heat:

a)

Heats up quickly

b)

Heats slowly

c)

Has high density

d)

Is a metal

39.

How much heat is absorbed by 10 g of water heated 10°C? (c = 4.18 J/g°C)

a)

41.8 J

b)

418 J

c)

4.18 J

d)

4180 J

40.

Which is an exothermic process?

a)

Freezing

b)

Boiling

c)

Melting

d)

Evaporation

41.

In an endothermic reaction:

a)

Heat is released

b)

Heat is absorbed

c)

Temperature decreases

d)

Bonds are formed

42.

A catalyst works by:

a)

Increasing the energy of reactants

b)

Lowering activation energy

c)

Raising temperature

d)

Adding mass to the product

43.

Which element has 2 valence electrons and forms a +2 ion?

a)

Calcium

b)

Nitrogen

c)

Fluorine

d)

Potassium

44.

What’s the correct name for KCl?

a)

Potassium dichloride

b)

Potassium chloride

c)

Potassium monochloride

d)

Kalium chloride

45.

What type of bond exists in H₂O?

a)

Ionic

b)

Polar covalent

c)

Metallic

d)

Nonpolar covalent

46.

Which element is in Period 3, Group 17?

a)

Oxygen

b)

Fluorine

c)

Chlorine

d)

Bromine

47.

Which formula represents dinitrogen tetroxide?

a)

N₂O

b)

NO₂

c)

N₂O₃

d)

N₂O₄

48.

Which reaction type is NaOH + HCl → NaCl + H₂O?

a)

Synthesis

b)

Single replacement

c)

Double replacement

d)

Decomposition

49.

How many total atoms are in Al₂(SO₄)₃?

a)

A) 7

b)

B) 10

c)

C) 17

d)

D) 12

50.

Which change is physical, not chemical?

a)

Burning

b)

Melting

c)

Rusting

d)

Reacting with acid

51.

Which of these samples shown best represents an element?

a)

A

b)

B

c)

C

d)

D

52.
a)

Compound

b)

Mixture of elements and compounds

c)

Mixture of elements

d)

Mixture of compounds

53.

This picture represents which of the following?

a)

element

b)

compound

54.
SeCl4
a)
selenium chloride
b)
monoselenium tetrachloride
c)
selenium tetrachloride
d)
monoselenium chloride
55.

Which type of intermolecular force is present in nonpolar molecules?

a)

London dispersion forces

b)

Dipole-dipole interactions

c)

Hydrogen bonding

d)

Ionic interactions

56.

What is the strongest intermolecular force that occurs between polar molecules (no F, O, N bonded to H)?

a)

London dispersion forces

b)

Dipole-dipole interactions

c)

Hydrogen bonding

d)

Ionic interactions

57.

Which type of intermolecular force is strongest?

a)

London dispersion forces

b)

Dipole-dipole interactions

c)

Hydrogen bonding

d)

Ionic interactions

58.
Which has a pH below 7?
a)
Acid
b)
Base
59.

What turns clear in the presence of phenolphthalein?

a)
Acid
b)
Base
60.
Turns litmus red
a)
Acids
b)
Bases
c)
All
61.

What pH is the strongest base?

a)

1

b)

7

c)

4

d)

14

62.
Which of the following is most likely to be basic:
a)
Lemon juice
b)
Vinegar
c)
Laundry detergent
d)
Coke
63.
Tastes Sour
a)
Acids
b)
Bases
c)
Salts
d)
All
64.
Which of these pH values would indicate that a solution is a weak base?
a)
4
b)
5.6
c)
8
d)
13
65.
When dissolved in water, acids produce:
a)
bases
b)
salts
c)
hydrogen ions
d)
hydroxide ions
66.
Which type of ion does a base produce when it is dissolved in water?
a)
oxide
b)
oxygen
c)
hydrogen
d)
hydroxide
67.

The middle conversion factor is the

a)

mole ratio of C2H18 to CO2

b)

molar mass of CO2

c)

molar mass of O2

d)

combination lock of your locker

68.

Given the unbalanced equation: Na2O + H2O →\rightarrow NaOH

How many grams of NaOH is produced from 120 grams of Na2O?

a)

120 g NaOH

b)

62 g NaOH

c)

1.94 g NaOH

d)

155 g NaOH

69.

Which atom has the following configuration?

1s22s22p63s23p64s23d104p6

a)

Argon

b)

Krypton

c)

Selenium

d)

Bromide

70.

What is the electron configuration for iron (atomic number 26)?

a)

1s22s22p63s23p64s23d6

b)

1s22s22p63s23p64s23d10

c)

[Xe]3d10

d)

1s22s22p63s23p64s2

71.

The Law of Conservation of Mass States

a)

Energy cannot be created nor destroyed, it can only change form.

b)

Mass cannot be created nor destroyed, it can only change form.

c)

Mass can be created or destroyed, it cannot change form.

72.

How many atoms are in the products below?
4Fe +3O2 → 2Fe2O34Fe\ +3O_{2\ }\rightarrow\ 2Fe_2O_3  

a)

7

b)

10

c)

17

d)

20

73.
A 55-gram egg is placed in a pot. After the egg is boiled, which is most likely the mass of the egg?
a)
50 
b)
55 
74.
In a reaction A + B ----> C,  reactant A has 5g and product  C has 9g. How many grams does reactant B should have? 
a)
4g
b)
5g
c)
9g
d)
14g
75.

Determine the molecular geometry of the given structure.

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Trigonal Planar

d)

Tetrahedral

76.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Linear
77.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
78.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

79.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
80.
Energy due to motion is ____________ energy. 
a)
Potential 
b)
Energy
c)
Kinetic
d)
Friction
81.
If a chemical reaction is EXOTHERMIC, the temperature would....
a)
Stay the same
b)
Increase
c)
Decrease
82.

What energy is stored and waiting to be used?

a)

Kinetic Energy

b)

Potential Energy

83.
In an endothermic reaction, heat is ...
a)
taken in or absorbed
b)
given out or released 
84.
In an exothermic reaction, heat is ...
a)
taken in or absorbed
b)
given out or released
85.
What is true of this reaction?
a)
Equal amounts of energy were released and absorbed
b)
The reaction released more energy than it absorbed
c)
The reaction absorbed more energy than it released
86.
Convert 17 m to cm:
a)
0.17 cm
b)
0.017 cm
c)
1,700 cm
d)
170 cm
87.
Convert 8 kilometers to meters
a)
800 m
b)
80,000 m
c)
8,000 m
d)
.008 m
88.

How does a catalyst work in speeding up a reaction?

a)

By lowering the activation energy or reaction

b)

by giving them more energy

c)

by making them more available

89.

Why does breaking up a solid reactant increase the rate of reaction?

a)

it creates more solid

b)

it creates more energy

c)

it increases the total surface area

d)

it increases the concentration

90.

Between which two points is the gas heating up?

a)

A ----> B

b)

B <---- C

c)

C ----> D

d)

D ----> E

e)

E ----> F

91.

What type of reaction is this?

a)

Exothermic

b)

Endothermic

c)

Energy Producing

d)

No way to tell

92.

The graph above is from which type of reaction?

a)

Endothermic reaction

b)

Exothermic reaction

93.

Which of the following energy changes corresponds to the activation energy required for the forward reaction to take place?

a)

A

b)

C

c)

B

d)

E

94.

Hydrogen and oxygen molecules combine to form water molecules as shown in the reaction below. Given the molecules provided, which of the following is true about the products of this reaction? 

a)

2 H2O molecules are produced, O2 is the limiting reactant

b)

4 H2O molecules are produced, H2 is the limiting reactant

c)

4 H2O molecules are produced, O2 is the limiting reactant

d)

6 H2O molecules are produced, H2 is the limiting reactant

95.

Draw the products (notes/whiteboard) that can be formed from the reactants shown. Then identify the limiting and excess reactants.

a)

Fe is limiting and S is excess.

b)

S is limiting and Fe is excess.

c)

FeS is both limiting and excess.

d)

There is no limiting or excess reactants.

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