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INRS Final Chemistry Units 6-11 24-25

Total questions: 125

Worksheet time: 2hrs 9mins

Name
Class
Date
1.

Matter that has a definite volume and a definite shape is a __________.

a)

solid

b)

liquid

c)

gas

d)

plasma

2.

When two or more substances are physically combined, the result is a(n) ______.

a)

chemical change

b)

element

c)

compound

d)

mixture

3.

Three examples of physical changes are

a)

sawing wood, crushing a can, and burning a marshmallow

b)

burning of gasoline, rotting an egg, and exploding fireworks

c)

freezing of water, evaporation of gasoline, and rusting of a nail

d)

boiling of water, blowing up a balloon, and melting a candle

4.

In a solution, the substance that is being dissolved is the _______.

a)

solute

b)

solvent

c)

liquid

d)

gas

5.

Mrs. Joyner blends lemons, sugar, and water in a pitcher. She has made a ____________.

a)

compound

b)

substance

c)

homogeneous mixture

d)

heterogeneous mixture

6.

The Law of Conservation of Mass states

a)

Mass never stays constant

b)

Mass is always added during a chemical change

c)

Mass is always lost during a chemical change

d)

Mass is not lost or created during a chemical change

7.

Hydrogen, gold, and iron are all examples of

a)

homogeneous mixtures

b)

heterogeneous mixtures

c)

elements

d)

compounds

8.

The color of ink is a ___________.

a)

physical change

b)

physical property

c)

chemical change

d)

chemical property

9.

The atomic number of magnesium is 12. Therefore, its nucleus must contain

a)

6 protons and 6 neutrons

b)

6 protons and 6 electrons

c)

12 neutrons and no protons

d)

12 protons and no electrons

10.

An element with 5 protons, 6 neutrons, and 8 electrons has an atomic number of

a)

5

b)

6

c)

8

d)

11

11.

An element with 5 protons, 6 neutrons, and 8 electrons has a mass number of

a)

5

b)

6

c)

8

d)

11

12.

Atoms of the same element that have different numbers of neutrons are called

a)

molecules

b)

ions

c)

protons

d)

isotopes

13.

The majority of the mass of the atom is located in the _______ and the majority of the volume of the atom is located in the _______.

a)

Nucleus, electron cloud

b)

Nucleus, nucleus

c)

Electron cloud, nucleus

d)

Electron cloud, electron cloud

14.

Which statement about the arrangement of the periodic table is not true?

a)

Noble gases are in the group farthest to the right

b)

Metals are found on the left side of the periodic table

c)

Rare earth elements are in the first column on the left

d)

Transition metals are in the center of the periodic table

15.

Which of the following elements would be the most reactive?

a)

Iodine

b)

Silicon

c)

Silver

d)

Argon

16.

Which of the following elements would be the least reactive?

a)

Iodine

b)

Silicon

c)

Silver

d)

Argon

17.

The chemical bond formed when two atoms share electrons is called a(n) _______.

a)

Covalent bond

b)

Ionic bond

c)

Metallic bond

d)

Electron bond

18.

Which pair of atoms will combine with each other and form an ionic bond?

a)

C and O

b)

C and H

c)

Ca and Mg

d)

Ca and Br

19.

Which element is most likely to gain electrons in a chemical reaction?

a)

Kr

b)

K

c)

Br

d)

Ca

20.

Anions are formed by

a)

Losing electrons

b)

Gaining electrons

c)

Sharing electrons

d)

None of the above

21.

How does an atom of aluminum become an ion?

a)

It gains 3 electrons

b)

It gains 3 protons

c)

It loses 3 electrons

d)

It loses 3 neutrons

22.

How many electrons are shared between the hydrogen atoms in a molecule of H₂ gas?

a)

0

b)

1

c)

2

d)

4

23.

How many electrons are needed in the outer energy levels of most atoms for the atom to be chemically stable?

a)

2

b)

4

c)

6

d)

8

24.

The properties of a compound are _______ the properties of the elements that form it.

a)

Different from

b)

Similar to

c)

Identical to

d)

Derived from

25.

The burning of wood in a campfire that produces heat and light would be both an ____________ and an _______ reaction.

a)

exergonic; exothermic

b)

exergonic; endothermic

c)

endergonic; endothermic

d)

endergonic; exothermic

26.

In a chemical equation, the symbol that means dissolved in water is ___.

a)

(s)

b)

(l)

c)

(g)

d)

(aq)

27.

What type of reaction is the following chemical reaction? CH₃CH₂OH + 3O₂ → 2CO₂ + 3H₂O

a)

double-displacement

b)

single-displacement

c)

combustion

d)

synthesis

28.

Which chemical reaction represents a double displacement reaction?

a)

2Na + Cl₂ → 2NaCl

b)

NaOH + HCl → NaCl + H₂O

c)

Zn + 2HCl → ZnCl₂ + H₂

d)

2KClO₃ → 2KCl + 3O₂

29.

A teacher wants to demonstrate a chemical reaction for her students. Which activity below would best demonstrate a chemical reaction?

a)

Placing metal in an acid to create gas

b)

Measuring the densities of water and ice

c)

Melting a solid piece of aluminum

d)

Filling a balloon with helium gas

30.

Which of the following observations does NOT indicate that a chemical reaction has occurred?

a)

formation of a precipitate

b)

production of a gas

c)

state of matter change

d)

heat and light released

31.

A substance that is an ingredient in a chemical reaction is called a(n) __________.

a)

Catalyst

b)

Reactant

c)

Product

d)

Inhibitor

32.

Why does an increase in temperature result in an increase in reaction rate?

a)

It raises the activation energy

b)

It causes the molecules to increase in size

c)

It decreases the concentration of reactants

d)

It causes an increase in the number of particle collisions

33.

How many grams of KBr are needed to make a saturated solution in 100 g of water at 50°C?

a)

80 g

b)

90 g

c)

110 g

d)

60 g

34.

Would you classify a NaClO3 solution with a concentration of 120 g in 100 g of water at 10°C as saturated, unsaturated, or supersaturated?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

d)

Dilute

35.

Would you classify a KNO3 solution of 30 g in 100 g of water at 40°C as saturated, unsaturated, or supersaturated?

a)

Saturated

b)

Unsaturated

c)

Supersaturated

d)

Concentrated

36.

At what temperature is the solubility of KBr the same as that of KNO3?

a)

0°C

b)

35°C

c)

80°C

d)

60°C

37.

Label below which numbers represent solid, liquid, and gas on the heating curve of water.

a)

#1: solid, #3: liquid, #5: gas

b)

#1: gas, #3: solid, #5: liquid

c)

#1: liquid, #3: gas, #5: solid

d)

#1: solid, #3: gas, #5: liquid

38.

According to the heating curve graph, what takes longer:

heat of fusion (melting) or heat of vaporization (boiling)?

a)

Heat of fusion

b)

Heat of vaporization

c)

Both take the same amount of time

d)

Neither, they are instantaneous

39.

What is the group name for the element with the isotopic symbol ²⁰Na?

a)

Noble gases

b)

Halogens

c)

Alkali metals

d)

Transition metals

40.

If an atom has 3 neutrons and 2 electrons, which of the following is true about its atomic structure?

a)

It must be a noble gas

b)

It must have 2 protons

c)

It must have 3 protons

d)

It must have 5 protons

41.

Which model is commonly used to represent the arrangement of electrons in an atom, such as Magnesium-20?

a)

Lewis Dot Model

b)

Bohr Model

c)

Rutherford Model

d)

Quantum Mechanical Model

42.

An element is in the same family (group) as bromine (Br), but has fewer protons than magnesium (Mg). Which element is it?

a)

Fluorine (F)

b)

Chlorine (Cl)

c)

Iodine (I)

d)

Sodium (Na)

43.

Which element has 6 energy levels and 8 valence electrons?

a)

Neon (Ne)

b)

Argon (Ar)

c)

Radon (Rn)

d)

Xenon (Xe)

44.

What type of bond is formed between lithium and chlorine?

a)

Covalent bond

b)

Metallic bond

c)

Hydrogen bond

d)

Ionic bond

45.

Which diagram would best represent the electron arrangement for the compound formed between lithium and chlorine?

a)

Both atoms sharing electrons equally

b)

Lithium losing one electron and chlorine gaining one electron

c)

Both atoms gaining electrons

d)

Both atoms losing electrons

46.

Name the following compounds. FeO

Hint: Iron can be a +2 or +3

a)

Iron(III) oxide

b)

Iron(II) oxide

c)

Iron dioxide

d)

Iron monoxide

47.

Name the following compounds. Be₃P₂

a)

Triberyllium diphosphide

b)

Beryllium diphosphide

c)

Beryllium phosphide

d)

Beryllium(II) phosphide

48.

Name the following compounds. P₄O₆

a)

Tetraphosphorus hexoxide

b)

Tetraphosphorus pentoxide

c)

Phosphorus trioxide

d)

Phosphorus hexoxide

49.

Give the correct chemical formula for the following names. Ammonium sulfide

a)

(NH₄)₂S

b)

NH₄S

c)

NH₄₂S

d)

(NH₄)S₂

50.

Give the correct chemical formula for the following names. Tetracarbon decahydride

a)

C4H12

b)

C10H4

c)

C4H10

d)

C₁₀H₁₀

51.

Give the correct chemical formula for the following names. Manganese (II) chloride

a)

MnCl

b)

Mn₂Cl

c)

Mn₂Cl₃

d)

MnCl₂

52.

Balance and classify the following chemical reaction: ____AlBr₃ + ____K → ____KBr + ____Al

a)

1, 3, 3, 1

b)

2, 3, 3, 2

c)

3, 2, 2, 3

d)

2, 1, 1, 2

53.

What are the correct coefficients to balance the reaction: N₂ + O₂ → N₂O₅?

a)

2 N₂ + 5 O₂ → 2 N₂O₅

b)

1 N₂ + 2 O₂ → 1 N₂O₅

c)

2 N₂ + 2 O₂ → 2 N₂O₅

d)

1 N₂ + 5 O₂ → 2 N₂O₅

54.

Balance the following equation: CH₄ + O₂ → CO₂ + H₂O. What are the correct coefficients?

a)

1 CH₄ + 2 O₂ → 1 CO₂ + 2 H₂O

b)

2 CH₄ + 1 O₂ → 2 CO₂ + 2 H₂O

c)

1 CH₄ + 1 O₂ → 1 CO₂ + 1 H₂O

d)

1 CH₄ + 3 O₂ → 2 CO₂ + 2 H₂O

55.

Calculate the density of the rectangular prism

a)

2 g/cm3

b)

4 g/cm3

c)

6 g/cm3

d)

8 g/cm3

56.

What is the density of the sphere, if its mass is 50 g?

a)

40 grmL\frac{40\ gr}{mL}  

b)

65mLg\frac{65mL}{g}  

c)

2 gcm3\frac{2\ g}{cm^3}  

d)

25gmL\frac{25g}{mL}  

57.

24 g of magnesium reacts with 38 g of fluorine to produce ______ g of magnesium fluoride

a)

14

b)

24

c)

38

d)

62

58.
How many protons are in this element?
a)
79
b)
196
c)
117
d)
Cannot be determined
59.
How many electrons does potassium K contain? (click to see image)
a)
19
b)
39
c)
20
d)
40
60.

How many neutrons does an Oxygen atom have?

a)

8

b)

16

c)

24

d)

7.999

61.
Which subatomic particles are found in the nucleus of an atom?
a)
Protons and Electrons
b)
Protons and Neutrons
c)
Neutrons and Electrons
d)
Protons, Neutrons and Electrons
62.
What electrical charge does a proton have?
a)
+1
b)
0
c)
-1
d)
+2
63.
The total number of protons and neutrons in an atom is called the...
a)
Atomic number
b)
Proton number
c)
Mass number
d)
Weight number
64.

In an atom, the number of protons is equal to the number of ____________.

a)

energy levels

b)

neutrons

c)

neurons

d)

electrons

65.
These will determine what element an atom is. 
a)
number of neutrons
b)
number of electrons
c)
number of atoms 
d)
number of protons 
66.
What element is represented in this Bohr Model? 
a)
Carbon
b)
Hydrogen
c)
Aluminum
d)
Lithium
67.

Which is an atom of this element?

a)
b)
c)
d)
68.

Which group of elements have one valence electron(s)?

a)

Group 13

b)

Group 2

c)

Group 18

d)

Group 1

69.

Which group of elements are the most reactive metals?

a)

Group 2

b)

Group 1

c)

Group 13

d)

Group 18

70.

Which group of elements are the most reactive nonmetals?

a)

Group 2

b)

Group 1

c)

Group 18

d)

Group 17

71.

Which group of elements are nonreactive due to already being chemically stable?

a)

Group 17

b)

Group 1

c)

Group 2

d)

Group 18

72.

What are the horizontal rows on the periodic table called?

a)

Valence electrons

b)

Elements

c)

Periods

d)

Groups

73.

Which classification of elements are malleable, ductile, shiny, silvery solids and good conductors of heat and electricity?

a)

Transition metals

b)

Metalloids

c)

Nonmetals

d)

Metals

74.

Which classification of elements are gases or dull brittle solids and poor conductors?

a)

Transition metals

b)

Metals

c)

Nonmetals

d)

Metalloids

75.

Which classification of elements are solids, semi-conductors, physcial properties like metals, and chemical properties like nonmetals?

a)

Transition metals

b)

Metals

c)

Nonmetals

d)

Metalloids

76.

Match the following group names:

a)

Group 1

1.

Alkali metals

b)

Group 2

2.

Alkaline earth metals

c)

Group 3

3.

Rare earth metals

d)

Group 17

4.

Halogens

e)

Group 18

5.

Noble gases

77.

How many valence electrons does group 13 have?

a)

1

b)

2

c)

3

d)

12

78.

What are the red elements (those on the left)?

a)

metals

b)

nonmetals

c)

metalloids

79.

What are the yellow "stair-step" elements?

a)

metals

b)

nonmetals

c)

metalloids

80.

What element is in Group 13, Period 4?

a)

Aluminum

b)

Gallium

c)

Silicon

d)

Germanium

81.

What element is in Group 2, Period 5?

a)

Rubidium

b)

Strontium

c)

Cerium

d)

Barium

82.
Negative ions are called
a)
Cations
b)
Electrons
c)
Anions
d)
Neutrons
83.
When an atom loses a valence electron, it becomes a(n) _____________ ion.
a)
positive
b)
negative
c)
neutral
d)
polyatomic
84.

What class of elements tends to gain electrons?

a)

metals

b)

nonmetals

c)

metalloids

d)

Noble Gas

85.

Match the charge with the groups.

a)

-1

1.

Group 17

b)

-3

2.

Group 15

c)

-2

3.

Group 16

86.

Match the charge with the groups.

a)

+1

1.

Group 1

b)

+2

2.

Group 2

c)

+3

3.

Group 3

87.

Usually a _________ bond forms between metals and non metals.

a)

covalent

b)

coordinate covalent

c)

metallic

d)

ionic

88.

Which type of bonding does the image best represent?

a)

Ionic

b)

Covalent

c)

Metallic

89.

Which term best matches the following definition?

Definition: the tendency of an atom to prefer to have a full valence shell.

a)

Octet Rule

b)

Valence Shell

c)

Molecule

d)

Compound

e)

Chemical Bond

90.

Which term best matches the following definition?

Definition: the glue that holds atoms together in molecule or compounds.

a)

Octet Rule

b)

Valence Shell

c)

Molecule

d)

Compound

e)

Chemical Bond

91.

Which term best matches the following definition?

Definition: a group of atoms bonded together; at least two atoms bonded together.

a)

Octet Rule

b)

Valence Shell

c)

Molecule

d)

Compound

e)

Chemical Bond

92.

Which term best matches the following definition?

Definition: at least two different elements (type of atom) bonded together.

a)

Octet Rule

b)

Valence Shell

c)

Molecule

d)

Compound

e)

Chemical Bond

93.

What type of bonding in carbon dioxide (made of molecules containing CO2)?

a)

Metallic

b)

Covalent

c)

Ionic

94.

What type of bonding in sodium fluoride (made of the compound containing NaF)?

a)

Metallic

b)

Covalent

c)

Ionic

95.

Classify:

2H2 + O2 ---->2H2O

a)

synthesis reaction

b)

decomposition reaction

c)

single replacement reaction

d)

double replacement reaction

96.

Classify:

Mg + 2HCl ----> MgCl2 + H2

a)

synthesis reaction

b)

decomposition reaction

c)

single replacement reaction

d)

double replacement reaction

97.

Classify:

2HCl + 2NaOH -----> NaCl + H2O

a)

synthesis reaction

b)

decomposition reaction

c)

single replacement reaction

d)

double replacement reaction

98.

Classify:

CH4 + O2 → CO2 + H2O

a)

single replacement

b)

double replacement

c)

synthesis

d)

combustion

99.

An _______ reaction is when more energy is released than is absorbed. This energy can be in the form of light, heat, electricity, etc.

a)

endothermic

b)

endergonic

c)

exothermic

d)

exergonic

100.

An _______ reaction is when more thermal energy is absorbed than is released.

a)

endothermic

b)

endergonic

c)

exothermic

d)

exergonic

101.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
102.
Increase in temperature of the reactants can do one of the following
a)
Slow collision frequency
b)
Allow less effective collision between the particles
c)
Cause particles to lose speed
d)
Increase collision between the particles thus increasing the rate.
103.
What type of reaction is this?
a)
Endothermic
b)
Exothermic
104.
How would this reaction be classified?
2Na + Cl2 → 2NaCl + 25kJ energy
a)
Exothermic
b)
Endothermic
c)
Isothermic
d)
None of the above
105.

What ions are there more of in acidic solutions?

a)

H+ (really H3O+)

b)

OH-

106.

Which one of the following is NOT a property of acids.

a)

Tastes sour

b)

Corrodes metals

c)

Conduct electricity

d)

Turns red litmus paper blue

107.

Which one of these substances will have a NEUTRAL pH?

a)

Lemon juice

b)

Coffee

c)

Bleach

d)

Water

108.

Acids have a pH of _______________.

a)

below 7

b)

above 7

c)

exactly 7

109.

Which of the following pH values represents a base?

a)

2.1

b)

4.6

c)

6.8

d)

8.1

110.

KOH is ...

a)

an acid

b)

a base

c)

a salt

d)

an ionic compound

111.

The table shows the pH of several solutions. Which solution is the most acidic?

a)

milk

b)

water

c)

bleach

d)

vinegar

112.
Turns litmus red
a)
Acids
b)
Bases
c)
All
113.

Hydrochloric acid

a)

HClHCl  

b)

HNO3HNO_3  

c)

H2SO4H_2SO_4  

d)

H3PO4H_3PO_4  

114.

Which statement best describes the difference between nuclear fusion and nuclear fission?

a)

Fusion splits atoms, fission combines them

b)

Fusion combines atoms, fission splits them

c)

Both fusion and fission split atoms

d)

Both fusion and fission combine atoms

115.

Which type of nuclear radiation is being emitted here?

a)

Alpha

b)

beta

c)

gamma

d)

none

116.
Positively charged particles that consist of two protons and two neutrons are called
a)
alpha particles
b)
beta particles
c)
gamma rays
d)
neutron emissions
117.
In order of most to least penetrating radiation we have
a)
Alpha , Beta,  Gamma
b)
Beta , Gamma , Alpha
c)
Gamma, Beta, Alpha
d)
Gamma, Alpha, Beta
118.
What is the formula for Boyle's Law?
a)
P1V1=P2V2
b)
P1V1/P2V2
c)
P1V2=P2V1
d)
P1/V1=P2/V2
119.
What is the formula Charles' Law?
a)
V = T
b)
VT = VT
c)
T1 / V1 = T2 / V2
d)
V1 / T1 = V2 / T2
120.

Three gases are mixed together in a container with a total pressure of 4.8 atm. If two of the gases have pressures of 1.2 atm and 1.5 atm, what is the pressure of the third gas?

a)

2.5 atm

b)

1.8 atm

c)

2.1 atm

d)

1.3 atm

121.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
122.

Avogadro's number (6.02x1023) of particles is equal to one_____.

a)
kilogram
b)
gram
c)
kelvin
d)
mole
123.
Where do you look to calculate the molar mass?
a)
avogadros number
b)
periodic table 
124.
What is the molar mass of one molecule of Nitrogen N2?
a)
14.01 amu
b)
14.01 g
c)
28.02 g
d)
28.02 amu
125.

Find the mass of 3.6 mol of Au.

a)

843.6 g

b)

709.2 g

c)

435.9 g

d)

196.9 g

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