Free Printable Exam Review/Class

1.

atomic number

a)

number of protons/stands for an element

b)

number of neutrons

c)

number of electrons

d)

number of protons and neutrons

2.

mass number

a)

number of protons

b)

number of electrons

c)

number of protons and electrons

d)

number of protons and neutrons

3.

atomic symbol

a)

capital letter

b)

lowercase letter

c)

2 capital letters

d)

2 lowercase leters

4.

Which of the following reactions is a combustion reaction ?

a)

MgCO3 + O2 → MgO + CO2

b)

C3H8 + 5O2 → 3CO2 + 4H2O

c)

6CO2 + 6H2O → C6H12O6 + 6O2

d)

6CO2 + 6H2O → C6H12O6 + 6O2

5.

Which of the following is a decomposition reaction?

a)

MgCo3 --> MgO + CO2

b)

SO3 + H2O --> H2SO4

c)

2 Mg + O2 --> 2MgO

6.

What is the atomic mass of this element?

a)

20

b)

60

c)

40

d)

41

7.

What is the symbol of this element?

a)

Calcium

b)

P

c)

Ca

d)

C

8.

The characteristics or properties of metals include

a)

shiny and solid

b)

ductile and malleable

c)

lose electrons

d)

all of the above

9.

Water is an element?

a)

true

b)

false

10.

A molecule is

a)

a singular particle of a particular element

b)

another name for an element

c)

2 or more atoms that are combined

11.

Gold is an example of a(n)

a)

pure element

b)

pure compound

c)

pure mixture

12.

What is the number of protons that the element in this image contain?

a)

14

b)

7

c)

15

d)

18

13.

"C" is the element symbol for which element?

a)

calcium

b)

carbon

c)

chlorine

d)

cadmium

14.

True or False? Neutrons have a negative charge

a)

True

b)

False

15.

A _________ is a substance made of two or more DIFFERENT elements chemically combined.

a)

mixture

b)

compound

c)

substance

16.

anions are _____ ions.

a)

positive

b)

negative

c)

neutral

17.

What charge will a Beryllium ion have?

a)

+

b)

2+

c)

2-

d)

-

18.

What charge will a sulfide ion have?

a)

3+

b)

2+

c)

2-

d)

3-

19.

What charge will a nitride ion have?

a)

3+

b)

2+

c)

2-

d)

3-

20.

what charge will an aluminum ion have?

a)

3+

b)

2+

c)

2-

d)

3-

21.

How many valence electrons does Lithium have?

a)

1

b)

2

c)

3

d)

4

22.

How many valence electrons does magnesium have?

a)

1

b)

2

c)

12

d)

24

23.

How many valence electrons does Carbon have?

a)

4

b)

12

c)

6

d)

14

24.

How many valence electrons does Sulfur

a)

16

b)

32

c)

6

d)

3

25.

How many valence electrons does Krypton have?

a)

36

b)

18

c)

8

d)

4

26.

If an atom has 3 valence electrons, what charge will it have as an ion?

a)

+3

b)

-3

c)

+5

d)

-5

27.

If an element gains 1 electron, what charge will it have?

a)

+1

b)

-1

c)

+7

d)

-7

28.

Group 17 always has ions with a charge of

a)

+1

b)

+2

c)

-1

d)

-2

29.

Beryllium will ____ valence electrons when forming an ionic bond.

a)

lose 4

b)

gain 4

c)

lose 2

d)

gain 2

30.

Why are ions charged particles?

a)

The number of electrons does not equal the number of protons.

b)

The number of protons does not equal the number of neutrons.

c)

The number of neutrons does not equal the number of electrons.

d)

The electric charges of the electrons and protons cancel each other out.

31.

Where are metals located on the periodic table?

a)

Blue

b)

Green

c)

Red

32.

Where are the nonmetals located on the periodic table?

a)

Blue

b)

Red

c)

Green

33.

What charge will an Oxygen ion have?

a)

+1

b)

-1

c)

+2

d)

-2

34.

What is the charge of a sodium ion?

a)

+2

b)

+1

c)

-1

d)

-2

35.

Which of the following has a -3 charge?

a)

Boron

b)

Fluorine

c)

Nitrogen

d)

Neon

36.

Anions are...

a)

Positive

b)

Negative

c)

Neutral

d)

Crying

37.

What is the ionic symbol for a Gold ion?

a)

Au⁺

b)

Au^-

c)

Au⁺²

d)

Au^-2

38.

Silver

(a)

39.

Xenon

(a)

40.

Potassium

(a)

41.

How many valence electrons does this Nitrogen atom have?

a)

15

b)

5

c)

2

d)

3

42.

How many valence electrons does Magnesium(Mg) have?

a)

1

b)

2

c)

3

d)

4

43.

How many valence electrons does this Nitrogen atom have?

a)

7

b)

5

c)

15

d)

2

44.

How many protons does Lead(Pb) have?

a)

207

b)

82

c)

14

d)

124

45.

Which is the correct molecular structure for carbon dioxide (CO₂)?

a)

b)

c)

d)

46.

What is the correct Lewis Dot Structure for ammonia NH₃?

a)

b)

c)

d)

47.

According to the octet rule most elements need _______ valence electrons.

a)

2

b)

8

c)

6

d)

18

48.

Hydrogen needs _____ electrons in its valence shell to be stable.

a)

4

b)

6

c)

8

d)

2

49.

Metals and nonmetals form which kind of bond?

a)

Polar covalent

b)

Ionic

c)

Non-polar covalent

d)

Metallic

50.

What coefficients does ____H2 + ____O2 -> ____H2O need to be balanced?

a)

1,1,1

b)

2,2,2

c)

2,1,2

d)

none of the above

51.

How many hydrogen atoms?

a)

1

b)

2

c)

6

d)

not enough information

52.

What type of reaction follows the form AX + BY -> AY + BX?

a)

single replacement cationinc

b)

double replacement

c)

synthesis

d)

decomposition

53.

When balancing a combustion reaction what atoms do we balance second?

a)

hydrogen

b)

water

c)

carbon

d)

oxygen

54.

A double replacement reaction produces either, a gas, water, or a ______________.

a)

precipitate

b)

isotopes

c)

compounds

d)

new elements

55.

What happens to the atoms in a chemical reaction?

a)

they are created

b)

they are converted to energy

c)

they are destroyed

d)

they are rearranged

56.

Balance the equation ___Fe(s) + ___CuSO4(aq) -> ____FeSO4(aq) + ____Cu(s)

a)

1,2,2,1

b)

2,3,6,3

c)

2,4,2,4

d)

already balnced

57.

How many nitrogen atoms are on the reactants side of 3Mg(NO3)2 + 2K3PO4 -> Mg3(PO4)2 + 6KNO3?

a)

6

b)

3

c)

18

d)

1

58.

$Balance\ the\ equation\ Fe_3O_4+H_2->Fe+H_2O.$

a)

3,1,4,2

b)

1,4,3,4

c)

2,8,6,8

d)

none of the above

59.

What forces us to balance chemical equations?

a)

The Law of Balanced Equations

b)

The Law of Conservation of Mass

c)

The Law of Conservation of Energy

d)

The Law of Science

60.

Mg₃N₂ --> Mg + N₂

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

61.

K + Li₂O --> K₂O + Li

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

62.

Al₂O₃ --> Al + O₂

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

63.

C₂H₆ + O₂ --> CO₂ + H₂O

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

64.

NO + O₂ --> NO₂

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

65.

Na₂CO₃ + HCl --> NaCl + H₂O + CO₂

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

66.

What type of chemical reaction is shown in the image?

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

67.

C₆H₁₂O₆ + O₂ --> CO₂ + H₂O

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

68.

Fe + CuNO₃ --> Cu + Fe(NO₃)₂

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

69.

What type of chemical reaction is shown in the image?

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

70.

What molecule could this be?

a)

H₂O

b)

CCl₄

c)

PCl₅

d)

NaCl

71.

What is the VSEPR theory used to predict?

a)

Bond Strength

b)

Polarity

c)

Molecular Shape

d)

Electronegativity

72.

Classify the following molecule.

a)

polar

b)

nonpolar

73.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

74.

Electronegativity is a measurement of the ability of a nucleus to:

a)

attract bonding electrons

b)

attract other nuclei

c)

attract electrons in the non-valence energy levels

75.

Classify the following as polar or nonpolar: SiO₂

a)

polar

b)

nonpolar

76.

The force of attraction between oppositely charged particles is a(n):

a)

ionic bond

b)

valence electron

c)

metallic bond

d)

lewis dot diagram

77.

A covalent bond is:

a)

shared electrons

b)

bonding 2 nonmetals

c)

a transfer of electrons

d)

a charged particle

78.

What does the Roman numeral in parentheses mean on some transition metals?

a)

the number of atoms

b)

the number of ions

c)

the number of ionic charge

79.

What part of the atom is responsible for chemical bonding?

a)

protons

b)

neutrons

c)

electrons

80.

Which of these is a characteristic of ionic compounds?

a)

They are gases at room temperature.

b)

They conduct an electric current when melted or dissolved.

c)

They have low melting points.

d)

They have the weakest bonds.

81.

What type of bonds equally share electrons?

a)

ionic

b)

polar covalent

c)

nonpolar covalent

82.

Ionic bond is present in which of the following species:

a)

O₂

b)

CHCl₃

c)

NaBr

d)

CCl₄

83.

Among the following compounds identify the compound that has all three bonds (ionic, covalent and

coordinate bond)

a)

Ammonia

b)

Ammonium chloride

c)

Sodium hydroxide

d)

Calcium chloride

84.

The type of bonding in HCl molecule is:

a)

Polar covalent bond

b)

Pure covalent

c)

Non-polar

d)

Hydrogen bonding

85.

Formation of a compound through ionic bond ____________ the ionization energy of the metal ion.

a)

Does not depends on

b)

Depend on

c)

Is independent regarding

d)

May or may not depend on

86.

Why do atoms share electrons in covalent bonds?

a)

To increase their atomic numbers

b)

To attain a noble-gas electron configuration

c)

To become more polar

d)

To becomes ions and attract each other

87.

Valency of aluminum is:

a)

2

b)

3

c)

4

d)

5

88.

Identify the molecule with a single covalent bond.

a)

CO₂

b)

CO

c)

Cl₂

d)

N₂

89.

A _________ is a solid that forms during a chemical reaction.

a)

precipitate

b)

solute

c)

solvent

d)

gas

90.

2H₂ + O₂ → 2H₂O
How many moles of oxygen are consumed if 8 moles H₂ are used?

a)

2

b)

4

c)

6

d)

8

91.

2 KClO₃ → 2 KCl + 3 O₂
How many moles of oxygen are produced when 6.7 moles of KClO₃ decompose completely?

a)

6.7 mol

b)

1.0 mol

c)

10.05 mol

d)

4.5 mol

92.

Stoichiometry is -

a)

a balanced reaction with the same number of elements on both sides of the reaction

b)

Calculating moles

c)

using the balanced reaction and moles to calculate amounts needed and used

d)

percentage yield

93.

What are the coefficients to balance the following:

Fe + CuCl₂ --> Cu + FeCl₃

a)

1,1,1,1

b)

2,3,3,2

c)

3,2,3,2

d)

4,6,6,4

94.

What is a Excess Reagent?

a)

amount you end with

b)

what you run out of first

c)

what you have left over

d)

what you start with

95.

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

96.

What is the first thing you must do to solve a stoichiometry problem?

a)

Write a Balanced Equation

b)

Panic

c)

Write an Unbalanced Equation

d)

Ask for help

97.

2H₂ + O₂ → 2H₂O
How many moles of water can be produced if 8 moles H₂ are used?

a)

4 moles

b)

8 moles

c)

16 moles

d)

2 moles

98.

What is the molar mass of Helium?

a)

4.00g/mol

b)

1.00g/mol

c)

2.00g/mol

d)

6.00g/mol

99.

How many molecules are there in 4.00 moles of glucose? C6H12O6?

a)

72g

b)

$2.408\ \times\ 10^{24}$

c)

22.4L

d)

4.56

100.

What is the volume of 0.05mol of Neon gas at STP?

a)

1.12L Ne

b)

102g Ne

c)

47L Ne

d)

100 mol Ne

101.

Which term describes a solution in which there is less than the maximum amount of solute dissolved for the given temperature?

a)

Unsaturated

b)

Saturated

c)

Concentrated

d)

Supersaturated

102.

The ___ is the thing being dissolved.

a)

solute

b)

solvent

c)

mixture

d)

suspension

103.

Besides stirring, which of the following should be done to make this powder dissolve faster in the liquid?

a)

Add heat to the liquid

b)

Cool the liquid in a freezer

c)

Add more powder to the liquid

d)

Store the mixture in a dark place

104.

Since "like dissolves like", water and oil will not mix because

a)

both of them are polar

b)

both of them are nonpolar

c)

oil is polar and water is nonpolar

d)

oil is nonpolar and water is polar

105.

Molarity is ...

a)

grams of solute/deciliters of solvent.

b)

grams of solute/liters of solution.

c)

moles of solute/liters of solution.

d)

moles of solute/milliliters of solvent.

106.

If more solvent is added to a solution:

a)

its molarity decreases

b)

its molarity increases

c)

it becomes more concentrated

d)

it will saturate out

107.

What is the universal solvent?

a)

salt

b)

sugar

c)

water

d)

ice

108.

A mixture with more solute dissolved in the solvent than is usually soluble is called:

a)

concentrated

b)

supersaturated

c)

saturated

d)

unsaturated

109.

When you have added as much solute as can dissolve in the solvent, the solution is called:

a)

concentrated

b)

supersaturated

c)

saturated

d)

unsaturated

110.

Kool-Aid - Powder, sugar, and water
Identify the solvent

a)

water

b)

powder

c)

sugar

d)

powder and sugar

111.

salt water is a

a)

compound

b)

element

c)

heterogeneous mixture

d)

solution

112.

Solubility refers to the ____ of solute that can dissolve in a certain volume or mass of solvent, at a certain temperature.

a)

Mean

b)

Range

c)

Amount

d)

Mode

113.

What does it mean to dilute a solution?

a)

lower the concentration of solute per solvent

b)

increase the concentration of solute per solvent

114.

Which of the following is the Dilution Formula?

a)

V₁M₁ = V₂M₂

b)

M = m/V

c)

V = mT

d)

PV = nRT

115.

A dilution is when

a)

solute is added to the volume of solution

b)

water is added to the volume of solution

c)

solute is removed from the volume of solution

d)

water is removed from the volume of solution

116.

How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?

a)

27.8 mL

b)

27.78 mL

c)

2.8 mL

d)

278 mL

117.

Which of the following has the MOST surface area?

a)

A single 5 gram ice cube

b)

5 grams of crushed ice

c)

5 grams of shaved ice

118.

a)

Monatomic Element

b)

Compound

c)

Mixture

d)

Diatomic Element

119.

Classify the picture with the correct label.

a)

Element

b)

Compound

c)

Mixture of Compounds

d)

Mixture of Elements

120.

Which unit is used to measure mass in the metric system?

a)

Pound

b)

Slug

c)

Ounce

d)

Gram

121.

Based on the image, what is the mass of the object being measured?

a)

500.10 grams

b)

501.00 grams

c)

510.00 grams

d)

600 grams

122.

This is the smallest particle into which an element can be divided and still be the same substance.

a)

Mixture

b)

Compound

c)

Element

d)

Atom

123.

The smallest particle in a chemical element or compound that has the chemical properties of that element or compound

a)

atom

b)

molecule

c)

element

d)

compound

124.

An empirical formula:

a)

is the simplest whole-number ratio of moles of elements in the compound,

b)

is a formula that calculates the coefficients of a compound in a balanced equation.

125.

Which pair has the same empirical formula?

a)

NaCrO₄ and Na₂Cr₂O₇

b)

C₂H₄O₂ and C₆H₁₂O₆

c)

C₃H₆O₃ and C₂H₆O₂

d)

CH₄ and C₂H₆

126.

What is the empirical formula if you have 36.84% nitrogen and 63.16% oxygen?

a)

NO

b)

N₂O₄

c)

N₂O₃

d)

N₂O₅

127.

What is the percent by mass of chlorine in NaCl?

a)

39%

b)

61%

c)

35%

d)

65%

128.

What is the percent composition of a compound that contains 40.8 g carbon and 54.4 g oxygen?

a)

42.9 %; 57.1% oxygen

b)

52.9 %; 57.1% oxygen

c)

42.9 %; 45.23% oxygen

d)

55.9 %; 99.1% oxygen

129.

What is the percent composition of S in the formula (NH₄)₂S ?

a)

12.05%

b)

19.30%

c)

47.11%

d)

56.18%

130.

In chemistry, a "mole" is:

a)

The mass of an atom

b)

a large number used to count particles

c)

based on the volume of a substance

131.

The number 6.02 x 10²³ is called...

a)

Obama's number

b)

Bohr's number

c)

Trump's number

d)

Avogadro's number

132.

We use the periodic table to calculate...

a)

mass

b)

molar mass

c)

moles

Exam Review/Class

Total questions: 132

Worksheet time: 2hrs 39mins

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