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Chemistry Honors Sem 1 Final Exam review

Total questions: 124

Worksheet time: 3hrs 6mins

Name
Class
Date
1.
Which type(s) of substances are considered pure substances?
a)
Elements only
b)
Compounds only
c)
Mixtures only
d)
Elements and compounds
2.
Which of the following requires a physical change to separate?
a)
Element
b)
Compound
c)
Mixture
3.
Which type of substance cannot be broken down into simpler substances?
a)
Element
b)
Compound
c)
Mixture
4.
What is true about a solution?
a)
Solutions are not mixtures.
b)
Solutions are mixtures.
c)
All mixtures are solutions.
5.

Sweet Tea, everything is mixed evenly and looks the same.

a)

Heterogeneous Mixture

b)

Homogeneous Mixture

6.

Oil and Water

a)

Element

b)

Compound

c)

Homogeneous Mixture

d)

Heterogeneous Mixture

7.
Water (H2O) freezing is an example of:
a)
A chemical change
b)
A physical change
8.
A compound consists of two or more elements bound together.
a)
True
b)
False
9.
A chemical change always results in the formation of a:
a)
explosion
b)
big mess
c)
new substance
d)
new state of matter
10.

True or False: A compound can be broken down further into elements

a)

True

b)

False

11.

True or False: An Element can be broken down into smaller atoms

a)

True

b)

False

12.
Solids are described as having a 
a)
definite shape and indefinite volume
b)
indefinite shape and indefinite volume
c)
definite shape and definite volume
d)
indefinite shape and definite volume
13.
Liquids are described as having a 
a)
definite shape and indefinite volume
b)
indefinite shape and indefinite volume
c)
definite shape and definite volume
d)
indefinite shape and definite volume
14.
Gases are described as having a 
a)
definite shape and indefinite volume
b)
indefinite shape and indefinite volume
c)
definite shape and definite volume
d)
indefinite shape and definite volume
15.
A substance that has a definite shape and volume.
a)
evaporation
b)
gas
c)
liquid
d)
solid
16.

What is an example of a color change as an indicator for a chemical reaction?

a)

Solid to liquid transformation

b)

No change in color

c)

Solid to gas transformation

d)

Colorless to colored solution

17.

What is the evidence of a gas being released during a chemical reaction?

a)

Change in color

b)

Formation of bubbles or change in volume

c)

Increase in temperature

d)

Formation of solid particles

18.

How does a change in temperature indicate a chemical reaction?

a)

Change in temperature indicates the phase of the moon

b)

Change in temperature indicates the number of people in a room

c)

Change in temperature indicates the stock market performance

d)

Change in temperature indicates the occurrence of a chemical reaction.

19.
A change where one or more new substances are created.
a)
Physical Change 
b)
Chemical Change 
20.
Which of the following is NOT an example of a physical change?
a)
crumpled paper
b)
pencil sharpening
c)
shrunken clothing
d)
rust
21.
When you break a cracker into pieces it is a...
a)
Chemical change
b)
Physical change
22.
A solid piece of chocolate is melted and changed to liquid form. Which property of the piece of chocolate will remain the same?
a)
Texture
b)
Temperature
c)
Shape
d)
 Mass
23.
Freezing Juice?
a)
Physical Change
b)
Chemical Change
24.

Benjamin, Ethan, and Emma are studying different properties of materials. They come across a property that doesn't change even if the amount of material changes. Which of the following is an example of such an intensive property?

a)

Volume

b)

Mass

c)

Density

d)

Size

25.

Which of the following is an example of an extensive property?

a)

Temperature

b)

Color

c)

Length

d)

Boiling Point

26.

What is an intensive property?

a)

A property that depends on the quantity of matter

b)

A property that does not depend on the quantity of matter

c)

A property that changes according to conditions

d)

A property that is additive for subsystems

27.

What is an extensive property?

a)

A property that depends on the quantity of matter

b)

A property that does not depend on the quantity of matter

c)

A property that changes according to conditions

d)

A property that is additive for subsystems

28.

Zoe, Maya, and Charlotte are studying for their chemistry exam. They come across a question asking for an example of an extensive property. Which of the following options should they choose?

a)

Refractive Index

b)

Melting Point

c)

Weight

d)

Hardness

29.

Which of the following is an example of an intensive property?

a)

Luster

b)

Ductility

c)

State of Matter

d)

Odor

30.

What is a physical property?

a)

A property of a substance that can be observed without changing the substance

b)

A property of a substance that can only be observed by changing the substance

c)

A property of a substance that is related to its reactivity

d)

A property of a substance that is related to its flammability

31.

Which of the following is an example of a physical property?

a)

Color change

b)

Gas production

c)

Density

d)

Temperature change

32.

What is a chemical property?

a)

A property of a substance that can be observed without changing the substance

b)

A property of a substance that can only be observed by changing the substance

c)

A property of a substance that is related to its reactivity

d)

A property of a substance that is related to its flammability

33.

Which of the following is an example of a chemical property?

a)

Color change

b)

Gas production

c)

Density

d)

Temperature change

34.
Is a a rusting bicycle a chemical or physical change?
a)
chemcial
b)
physical
35.
Dissolving a solid into a liquid is a ___.
a)
physical change
b)
chemical change
36.

Which of the following are physical properties or changes?

a)

Burning

b)

Breaking glass

c)

Melting Ice

d)

Ice feels slippery

37.

What is the name of element with atomic number 3?

a)

helium

b)

sodium

c)

potassium

d)

lithium

38.

What is the atomic mass of oxygen?

a)

18.00

b)

17.00

c)

15.00

d)

16.00

39.
Name group 1 on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
noble gases
noble gases
d)
halogens
40.
Name group 2 on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
noble gases
d)
transition metals
41.
Name group 18 on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
transition metals
d)
noble gases
42.
Name groups 3 - 12 on the periodic table.
a)
noble gases
b)
halogens
c)
metalloids
d)
transition metals
43.
Name group 17 on the periodic table.
a)
transition metals
b)
metalloids
c)
halogens
d)
alkali metals
44.
Which group has the most reactive nonmetals?
a)
alkali metals
b)
noble gases
c)
metalloids
d)
halogens
45.
Where are the nonmetals located on the periodic table?
a)
top left corner
b)
bottom left corner
c)
top right corner
d)
bottom left corner
46.
Name the group that contains inert (nonreactive) elements.
a)
noble gases
b)
halogens
c)
alkali metals
d)
alkaline earth metals
47.
Elements in the same ________ are more chemically similar.
a)
group
b)
period
c)
club
d)
table
48.
The majority of elements on the periodic table are
a)
man made.
b)
nonmetals.
c)
metals.
d)
gases.
49.

The identity of an element on the periodic table is determined by the number of _______.

a)

protons

b)

neutrons

c)

electrons

d)

ions

50.

An atom that has the same number of protons but different numbers of neutrons is an _______________.

a)

isotope

b)

ion

c)

molecule

d)

awesome atom

51.

The current periodic table is arranged by..

a)

Atomic number

b)

Atomic mass

c)

Alphabetically

d)

Oldest to Newest

52.

What atomic particle determines the element?

a)

protons

b)

neutrons

c)

electrons

d)

nucleus

53.

(challenge) An atom has 10 protons and 10 electrons. What happens to the charge if you add 1 more electron?

a)

It becomes a negative ion

b)

It becomes a positive ion

c)

nothing changes

d)

It becomes a different element

54.

An atom of HELIUM has 2 protons. If you add 1 more proton, what happens?

a)

It becomes an ion

b)

It becomes a different kind of element

c)

Nothing

55.

Challenge: What is the charge of an atom with 3 protons and 2 electrons?

a)

0 (neutral)

b)

+1

c)

-1

56.

How many neutrons does lithium have?

a)

3

b)

4

c)

6

d)

7

57.

Calculate the average atomic mass of the element iron (Fe) using the following data:

[Isotope / % abundance]

[Iron 54 / 6% ] [Iron 56 / 92% ] [ Iron 57 / 2% ]

a)

53.7 amu

b)

54.9 amu

c)

5592.0 amu

d)

55.9 amu

58.
What are ionic bonds?
a)
valence electrons transferred between atoms
b)
Inner most electrons transferred between atoms
59.
Why do ionic bonds form?
a)
so the number of protons equals the number of electrons
b)
to fill the outermost energy level
c)
so an atom can become unstable
60.
An atom that has gained or lost electrons is called ...
a)
a winner
b)
an isotope
c)
an ion
d)
a loser
61.
Mg2+ and Cl- create...
a)
Mg2Cl
b)
MgCl2
c)
Mg2Cl2
d)
MgCl
62.
Ca2+ and N3- create...
a)
Ca2N3
b)
Ca3N2
c)
CaN3
d)
Ca2N
63.

What was the basis for Dalton's atomic theory?

a)

The law of conservation of mass and the law of constant composition

b)

The discovery of subatomic particles and isotopes

c)

The law of definite proportions

d)

The rearrangement of atoms in a chemical reaction

64.

According to Dalton's atomic theory, all matter is made of ________.

a)

Molecules

b)

Protons, neutrons, and electrons

c)

Atoms

d)

Subatomic particles

65.

Which scientist performed the gold foil experiment?

a)

Democritus

b)

Dalton

c)

Thompson

d)

Rutherford

66.

Which scientist discovered that the atom was mostly empty space?

a)

Democ

b)

Dalton

c)

Thompson

d)

Rutherford

67.

Which scientist proposed the Plum Pudding Model?

a)

Democritus

b)

Dalton

c)

Thompson

d)

Rutherford

68.

Who discovered the first subatomic particle, the electron?

a)

Ernest Rutherford

b)

J. J. Thomson

c)

Cricket Media

d)

Newsela staff

69.

What did Rutherford theorize about the center of an atom?

a)

The center of an atom was made of negatively charged electrons

b)

The center of an atom was mostly empty space

c)

The center of an atom was a dense nucleus surrounded by light, fast-moving electrons

d)

The center of an atom was 10,000 times smaller than the size of the atom

70.

Bohr discovered that electrons are located in

a)

the nucleus

b)

inside protons

c)

electron cloud

d)

circular orbits around the nucleus

71.

What element has this electron configuration?

a)

boron

b)

carbon

c)

nitrogen

d)

oxygen

72.

Which element is represented by this electron configuration?

a)

neon

b)

sodium

c)

magnesium

d)

aluminum

73.

Which element is represented by this orbital notation?

a)

neon

b)

sodium

c)

magnesium

d)

aluminum

74.

Which of the following is the orbital notation for oxygen?

a)
b)
c)
d)
75.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
76.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
77.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
78.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
79.
What noble gas should be used to write the shorthand configuration for Te?
a)
Ar
b)
Kr
c)
Xe
d)
Sb
80.

What is the trend of atomic radius across periods in the periodic table?

a)

decreases

b)

fluctuates

c)

increases

d)

remains constant

81.

Explain the trend of atomic radius down a group in the periodic table.

a)

The atomic radius fluctuates

b)

The atomic radius increases

c)

The atomic radius decreases

d)

The atomic radius remains constant

82.

Compare the atomic radius of lithium and fluorine. Which is larger?

a)

Helium

b)

They are the same

c)

Fluorine

d)

Lithium

83.

Which trend correctly describes the change in ionization energy across a period in the periodic table?

a)

Ionization energy decreases from left to right.

b)

Ionization energy increases from left to right.

c)

Ionization energy remains constant across a period.

d)

Ionization energy first increases, then decreases across a period.

84.

What happens to the ionization energy as you move down a group in the periodic table?

a)

It increases because the atomic radius decreases.

b)

It decreases because the atomic radius increases.

c)

It remains constant because the number of protons remains the same.

d)

It increases because the electron shielding effect decreases.

85.

How does the atomic radius of an atom relate to its ionization energy?

a)

Larger atomic radius means higher ionization energy.

b)

Smaller atomic radius means higher ionization energy.

c)

Atomic radius has no relation to ionization energy.

d)

Larger atomic radius means lower ionization energy, but only in metals.

86.
a)

Metal

b)

Nonmetal

c)

Metalloid

87.
a)

Metal

b)

Nonmetal

c)

Metalloid

88.
a)

Metal

b)

Nonmetal

c)

Metalloid

89.
a)

Metal

b)

Nonmetal

c)

Metalloid

90.
a)

Metal

b)

Nonmetal

c)

Metalloid

91.
a)

Metal

b)

Nonmetal

c)

Metalloid

92.

Which of these combinations is an ionic compound made of?

a)

Metal and Metal

b)

Nonmetal and Nonmetal

c)

Metal and Nonmetal

d)

Cation and Cation

93.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

94.

What is the what charge of lead in the compound: lead(IV) iodide

a)

+1

b)

+4

c)

+6

d)

-1

95.

Name the ionic compound, CaCO3

a)

calcium carbide

b)

calcium carbon trioxide

c)

calcium carbon oxide

d)

calcium carbonate

96.

Name the ionic compound, FeBr3

a)

Iron (II) bromide

b)

Iron (III) bromide

97.

What is the correct name for (NH4)2S

a)

Ammonium sulfate

b)

Nitrogen octhydrogen sulfide

c)

Ammonium sulfide

98.

What is the name of the compound P4S10

a)

phosphorous sulfide

b)

tetraphosphide decasulfate

c)

phosphorous decasulfate

d)

tetraphosphorous decasulfide

99.

What is the chemical formula of sulfur hexabromide?

a)

SBr₆

b)

S₆Br

c)

S(VI)Br

d)

SBr4

100.

Chlorous acid has the formula

a)

HClO3

b)

HClO2

c)

HClO

d)

HCl

101.

Name this acid: HNO2

a)

hydronitrous acid

b)

hydrogen nitrogen oxygen

c)

nitrous acid

d)

hyponitrous acid

102.

Name this acid: H2SO4

a)

hydrogen sulfate

b)

hydrosulfuric acid

c)

sulfuric acid

d)

sulfurous acid

103.

Name this acid with the formula HF

a)

hydrofluoric acid

b)

hypofluoric acid

c)

hydrogen fluorine acid

d)

fluoric acid

104.
diphosphorus pentoxide
a)
P2O5
b)
PO5
c)
P5O2
d)
P2O6
105.

How many different elements are present in H2C2H3O2?

a)

1

b)

2

c)

3

d)

4

106.

What is the total number of atoms in this chemical formula? C8H3NaBr12C_8H_3NaBr_{12}  

a)

18

b)

12

c)

25

d)

24

107.
The number of Na's in Na₂CO₃
a)
1
b)
2
c)
3
d)
6
108.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
109.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms

b)

The difference in the electronegativities of the two atoms

c)

The charges of the atoms

d)

None of the Above

110.

Which bond shares electrons unevenly?

a)

Covalent

b)

Polar Covalent

c)

Ionic

111.

Which bond involves "stealing" electrons?

a)

Covalent

b)

Polar Covalent

c)

Ionic

112.

The direction of the dipole arrow in this image tells us that

a)

H is the more electronegative atom in the bond

b)

Cl is the more electronegative atom in the bond

c)

H is the more polar atom in the bond

d)

Cl is the more polar atom in the bond

113.
What molecular shape is the structure shown here? (NH4+)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
114.

What molecular geometry is the structure shown here? (BCl3)

a)

linear

b)

trigonal planar

c)

tetrahedral

d)

trigonal pyramidal

115.

What molecular geometry is the structure shown here? (H2O)

a)

tetrahedral

b)

trigonal planar

c)

bent

d)

trigonal pyramidal

116.

Molecular shape for SCl2

a)

linear

b)

bent

c)

tetrahedral

d)

trigonal pyramidal

117.

Molecular shape for CO32-

a)

trigonal planar

b)

bent

c)

trigonal pyramidal

d)

tetrahedral

118.

Molecular shape for SiCl4

a)

trigonal bipyramidal

b)

bent

c)

trigonal pyramidal

d)

tetrahedral

119.

Choose the correct shape for this molecule:

a)

Trigonal planar

b)

Linear

c)

Bent

d)

Tetrahedral

120.

What shape will this molecule be?

a)

linear

b)

bent

c)

tetrahedral

d)

trigonal pyramidal

121.

A diatomic molecule is made of two atoms of the same element.

a)

True

b)

False

122.

Name the compound as ionic or molecular:

PF4

a)

ionic

b)

molecular

123.

Name the compound as ionic or molecular:

CH4

a)

ionic

b)

molecular

124.

What is a molecular compound composed of? Choose the BEST answer

a)

Polyatomic ions only

b)

A metal + a non-metal

c)

a non-metal

  • + a non-metal

d)

Covalently bonded compounds

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