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Chemistry Midterm Review

Total questions: 152

Worksheet time: 1hrs 29mins

Name
Class
Date
1.

Charge of an electron

a)

Positive

b)

Negative

c)

Neutral

2.

Charge of an proton

a)

Positive

b)

Negative

c)

Neutral

3.

Charge of a neutron

a)

Positive

b)

Negative

c)

Neutral

4.

How do you know the number of protons

a)

Atomic Number

b)

Mass Number

5.

Overall charge of an atom

a)

Positive

b)

Negative

c)

Neutral

6.

An atom with a charge.

a)

Ion

b)

Electrolyte

c)

Neutral

7.

How do you find the number of electrons in an atom

a)

Same as Mass

b)

8

c)

0

d)

Same as Atomic #

8.

How do you find the number of neutrons?

a)

0

b)

Same as protons

c)

Mass-Protons

d)

Protons - Electrons

9.

Isotopes have... (CHECK ALL THAT APPLY)

a)

Same number of protons

b)

Different number of neutrons

c)

Different number of electrons

d)

Different Masses

e)

Different Atomic Numbers

10.

Rutherford's Gold Foil...(Check all the apply)

a)

Atom is mostly empty space

b)

Small, dense, positively charged nucleus

c)

Electrons are surrounding the nucleus

d)

Some particles deflected (bounced back)

e)

Most particles passed through

11.

Have a mass of 1 amu... (check all that apply)

a)

Protons

b)

Neutrons

c)

Electrons

12.

Area of probability of finding an electron

a)

Orbit

b)

Orbital

c)

Nucleus

d)

Core

13.

Modern model of atom with electrons in orbitals

a)

Hard Sphere

b)

Rutherford

c)

Bohr

d)

Wave-Mechanical

14.

Which electrons have more energy?

a)

Shells closer to nucleus

b)

Shells further from nucleus

15.

Ground State --> Excited State

a)

Absorb Energy

b)

Release Energy

16.

Excited State --> Ground State

a)

Absorb Energy

b)

Release Energy (Light)

17.

Periodic Table organized in order of increasing...

a)

Atomic Mass

b)

Electronegativity

c)

Atomic Number

d)

Oxidation States

18.

Affinity (attraction) towards electron

a)

Electronegativity

b)

Ionization Energy

c)

Atomic Radius

d)

Atomic Mass

19.

Size of the atom

a)

Electronegativity

b)

Ionization Energy

c)

Atomic Radius

d)

Atomic Mass

20.

Amount of energy required to remove an electron

a)

Electronegativity

b)

Ionization Energy

c)

Atomic Radius

d)

Atomic Mass

21.

Where can you look up trends in Electronegativity, Ionization Energy, and Atomic Radius?

a)

Table A

b)

Table S

c)

Periodic Table

d)

Table I

22.

Left of Staircase (not H)

a)

Metal

b)

Nonmetal

c)

Metalloid

23.

Staircase

a)

Metal

b)

Nonmetal

c)

Metalloid

24.

Rightt of Staircase (plus H)

a)

Metal

b)

Nonmetal

c)

Metalloid

25.

Liquid at STP... (check all that apply)

a)

Hg

b)

H

c)

Si

d)

Br

e)

O

26.

Noble Gas

a)

Group 1

b)

Group 2

c)

Group 17

d)

Group 18

27.

Noble Gases have _____ valence electrons so they are ______.

a)

0, reactive

b)

8, reactive

c)

0, unreactive

d)

8, unreactive

28.

The # of Electrons SHARED in a single bond

a)

1

b)

2

c)

4

d)

6

29.

The # of Electrons SHARED in a double bond

a)

1

b)

2

c)

4

d)

6

30.

The # of Electrons SHARED in a triple bond

a)

1

b)

2

c)

4

d)

6

31.

The # of PAIRS of Electrons in a single bond

a)

1

b)

2

c)

4

d)

6

32.

Break Bonds...

a)

Absorb Energy

b)

Release Energy

33.

Form Bonds...

a)

Absorb Energy

b)

Release Energy

34.

CANNOT be broken down by a chemical change

a)

Element

b)

Compound

c)

Mixture

d)

Solution

35.

Atoms are chemically combined in a fixed proportion that cannot be changed.

a)

Element

b)

Compound

c)

Mixture

d)

Solution

36.

Heterogeneous mixture

a)

Evenly mixed

b)

Unevenly mixed (has layers)

37.

Homogeneous mixture

a)

Evenly mixed

b)

Unevenly mixed (has layers)

38.

Solutions are...

a)

homogeneous mixtures

b)

heterogeneous mixtures

39.

Similar chemical properties

a)

Same number of neutrons

b)

Same number of valence electrons

c)

Same mass

d)

Same color

40.

Phase (solid/liquid/gas), Melting/Boiling point, Density

a)

Physical Properties

b)

Chemical Properties

41.

Phase Changes are...

a)

Physical Changes

b)

Chemical Changes

42.

Rusting, Oxidized, Reacts, Synthesized, Decomposed, Combusts

a)

Physical Changes

b)

Chemical Changes

43.

Metal/Nonmetal

a)

Ionic Bond

b)

Covalent Bond

44.

Two Nonmetals

a)

Ionic Bond

b)

Covalent Bond

45.

Electrons Shared

a)

Ionic Bond

b)

Covalent Bond

46.

Electrons Transfered

a)

Ionic Bond

b)

Covalent Bond

47.

Electrons shared equally

a)

Ionic Bond

b)

Nonpolar Covalent Bond

c)

Polar Covalent Bond

d)

Hydrogen Bond

48.

Electrons shared unequally

a)

Ionic Bond

b)

Nonpolar Covalent Bond

c)

Polar Covalent Bond

d)

Hydrogen Bond

49.

Bond polarity is determined by difference in...

a)

Ionization Energy

b)

Electronegativity

c)

Atomic Number

d)

Atomic Mass

50.

Which are forms of ENERGY? (CHECK ALL THAT APPLY!)

a)

Nuclear

b)

Electromagentic

c)

Thermal

d)

Temperature

e)

Chemical

51.

Real Gases are most like Ideal Gases at...

a)

Low Temperature & Low Pressure

b)

Low Temperature & High Pressure

c)

High Temperature & Low Pressure

d)

High Temperature & High Pressure

52.

Which phase is a mixture?

a)

s

b)

l

c)

g

d)

aq

53.

Temperature

a)

Average Potential Energy

b)

Average Kinetic Energy

c)

Average Atomic Mass

d)

Average Ionization Energy

54.

Separation based on particle size

a)

Distillation

b)

Evaporation

c)

Filtration

d)

Chromatography

e)

Electrolysis

55.

Separation based on boiling points

a)

Distillation

b)

Evaporation

c)

Filtration

d)

Chromatography

e)

Electrolysis

56.

Which is a property of a gas according to Kinetic Molecular Theory? (CHECK ALL THAT APPLY)

a)

Particles move in random straight line motion

b)

No attraction between gas particles

c)

Gas particles have negligible volume

d)

No loss of energy during collisions

57.

Definite shape and definite volume

a)

Solid

b)

Liquid

c)

Gas

58.

Indefinite shape and definite volume

a)

Solid

b)

Liquid

c)

Gas

59.

Indefinite shape and indefinite volume

a)

Solid

b)

Liquid

c)

Gas

60.

Melting/Fusion, Vaporization/Boiling, and Sublimation

a)

Endothermic with increasing entropy.

b)

Exothermic with increasing entropy.

c)

Endothermic with decreasing entropy.

d)

Exothermic with decreasing entropy.

61.

Condensation, Freezing, and Deposition

a)

Endothermic with increasing entropy.

b)

Exothermic with increasing entropy.

c)

Endothermic with decreasing entropy.

d)

Exothermic with decreasing entropy.

62.

Disorder of molecules / Randomness

a)

Heat of Reaction

b)

Activation Energy

c)

Entropy

d)

Electronegativity

63.

Which phase has the greatest disorder?

a)

s

b)

l

c)

g

d)

aq

64.

During a phase change, temperature...

a)

increases, always.

b)

decreases, always.

c)

remains constant.

d)

increases or decreases depending on the change.

65.

"Substance" refers to... (CHECK ALL THAT APPLY)

a)

Element

b)

Compound

c)

Mixture

d)

Solution

66.

Strongest IMF

a)

van der Waals

b)

Dipole-Dipole

c)

Hydrogen Bonding

67.

Higher Boiling Point = _____ IMFs

a)

Stronger

b)

Weaker

68.

Isomers have...

a)

same molecular and structural formulas.

b)

different molecular and structural formulas.

c)

same molecular formula with different structural formulas.

d)

same structural formula with different molecular formulas.

69.

Symmetrical molecules are...

a)

Polar

b)

Nonpolar

70.

Asymmetrical molecules are...

a)

Polar

b)

Nonpolar

71.

Water molecules are...

a)

Polar

b)

Nonpolar

72.

What line segment represents when the substance is only in the solid state?

a)

A-B

b)

B-C

c)

C-D

d)

D-E

73.

Which segment(s) represent when a phase change is taking place? (Check all that apply)

a)

A-B

b)

B-C

c)

C-D

d)

D-E

e)

E-F

74.

In which segment(s) is the kinetic energy of the particles remaining constant?

a)

A-B

b)

B-C

c)

C-D

d)

E-F

e)

D-E

75.

What state(s) of matter are present at segment C-D?

a)

Solid-liquid

b)

Liquid

c)

Liquid-gas

d)

Gas-Solid

e)

Gas

76.
The phase change from water vapor to liquid water is known as...
a)
evaporation
b)
precipitation
c)
condensation
d)
sublimation
77.

In a solid, the particles

a)

have a rigid shape

b)

slide past one another

c)

overcome their strong attractions to each other

d)

move freely in any direction

78.

When solid changes to liquid, it is

a)

endothermic because energy is absorbed by the molecules

b)

exothermic because energy is absorbed by the molecules

c)

endothermic because energy is released by the molecules

d)

exothermic because energy is released by the molecules

79.
WHICH OF THESE DESCRIBES THE LAW OF CONSERVATION OF ENERGY?
a)
NO MACHINE IS 100% EFFICIENT
b)
ENERGY IS NEITHER CREATED OR DESTROYED
c)
THE ENERGY RESOURCES OF EARTH ARE LIMITED
d)
THE ENERGY OF A SYSTEM IS ALWAYS DECREASING
80.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

81.

According to the reference table, what is the boiling point of ethanoic acid at 80 kPa?

a)

28 oC

b)

100oC

c)

111oC

d)

125oC

82.
Matter is defined as anything that occupies space and has
a)
shape
b)
odor
c)
mass
d)
color
83.
Which substance cannot be decomposed by a chemical change?
a)
N₂O
b)
H₂O
c)
Ne
d)
HF
84.
Which statement describes a chemical property of iron?
a)
Iron is a shiny metal
b)
Iron can be flattened into sheets
c)
Iron can be drawn into a wire.
d)
Iron combines with oxygen to form rust
85.
Which is a characteristic of all mixtures?
a)
Their composition is in a fixed ratio
b)
They are homogeneous
c)
They are heterogeneous.
d)
Their composition can be varied.
86.
Which Kelvin temperature is equivalent to -24℃?
a)
297 K
b)
273 K
c)
249 K
d)
226 K
87.
Which substance can be decomposed by a chemical change?
a)
Cu
b)
Co
c)
C
d)
CH₄
88.
Which particle diagram above best represents a single element?
a)
A
b)
B
c)
C
d)
D
89.
Which particle diagram above best represents a single compound?
a)
A
b)
B
c)
C
d)
D
90.
Which particle diagram above best represents a mixture of elements?
a)
A
b)
B
c)
C
d)
D
91.
Which particle diagram above best represents a mixture of compounds?
a)
A
b)
B
c)
C
d)
D
92.
Rusting
a)
Physical
b)
Chemical
93.
Dissolving
a)
Physical
b)
Chemical
94.
Flammable
a)
Physical
b)
Chemical
95.
Heat is released.
a)
Endothermic
b)
Exothermic
96.
How would you separate a mixture of saltwater and sand?
a)
Filter out the sand, then evaporate the water leaving the salt behind.
b)
Evaporate the water leaving the sand and salt behind, then use a magnet to separate them.
c)
Evaporate the water leaving the sand and salt behind, then separate using filtration.
d)
Filter out the salt, then evaporate the water leaving the sand behind.
97.

A student finds the density of an aluminum block to be 2.873 g/cm³. Using the information on Table S, calculate the student’s percent error. (Round to 2 decimal places.)

(a)  

98.

Which of the following statement(s) is/are true.

a)

The molecules in a gas take up a negligible amount of space in relation to the container they occupy.

b)

Collisions are elastaic, so energy is gained or lost when molecules collide.

c)

The molecules are in constant, linear motion.

d)

All are true

99.

Which of the following are ways in which a REAL gas deviates from an IDEAL gas?

(CHECK ALL THAT APPLY)

a)

Real Gases have weak intermolecular forces

b)

Real Gases are not compressible.

c)

Real Gases do occupy some volume.

d)

Real Gases do not travel in random straight line motion.

100.

Which of the following would behave most like an Ideal Gas?

a)

Ar (g)

b)

Ne (g)

c)

H2 (g)

d)

O2 (g)

101.

For all gas law problems, temperature MUST be converted into...

a)
Celsius
b)
Kelvin
c)

Fahrenheit

d)

Just use the unit from the problem.

102.

Which gas law is represented by the graph?

a)

Boyle's Law

b)

Charles's Law

c)

Lussac's Law

d)

Combined Gas Law

103.

Which gas law is represented by the graph?

a)

Boyle's Law

b)

Charles's Law

c)

Lussac's Law

d)

Combined Gas Law

104.

Which gas law is represented by the graph?

a)

Boyle's Law

b)

Charles's Law

c)

Lussac's Law

d)

Combined Gas Law

105.

Standard Pressure (include unit)

(a)  

106.

Standard Pressure (include unit)

(a)  

107.

Standard Temperature

(a)  

108.

Standard Temperature

(a)  

109.

Which of the following are "subatomic particles?" (CHECK ALL THAT APPLY)

a)

Protons

b)

Electrons

c)

Cations

d)

Neutrons

e)

Anions

110.

What is the overall charge of the NUCLEUS ofan atom?

a)

Neutral

b)

Positive

c)

Negative

d)

It depends.

111.

What is the overall charge of an ATOM?

a)

Positive

b)

Negative

c)

Neutral

d)

It depends

112.

Where are protons found?

a)

In the Nucleus

b)

Orbiting the Nucleus

113.

Where are neutrons found?

a)

In the Nucleus

b)

Orbiting the Nucleus

114.

Where are electrons found?

a)

In the Nucleus

b)

Orbiting the Nucleus

115.

Decide if each of the following is true of CATIONS or ANIONS.

Categorize the following

Positively charged

Lost Electrons

Negatively charged

Gained Electrons

Larger than the atom of that element.

Smaller than the atom of that element.

More protons than electrons.

More electrons than protons.

CATION
ANION
116.

The weighted average of all naturally occurring isotopes of a given element.

a)

Average Atomic Mass

b)

Atomic Number

c)

Atomic Mass Number

117.

Which of the following is MOST ABUNDANT?

A = 24%

B = 47%

C = 13%

D = 16%

a)

A

b)

B

c)

C

d)

D

118.

The outermost shell of electrons is called the (a)   shell.

119.
Question Image

Match the number with its value.

a)

Ground state electron configuration.

1.

2-8-18-7

b)

Atomic Number

2.

35

c)

Average Atomic Mass

3.

79.904

120.

How many valence electrons does Bromine have in its ground state?

a)

2

b)

8

c)

18

d)

7

121.

How many shells of electrons does Bromine have in the ground state?

a)

2

b)

4

c)

1

d)

7

122.

Which of the following was a conclusion of Rutherford's Gold Foil Experiment? (CHECK ALL THAT APPLY!)

a)

Nucleus is small and dense.

b)

Electrons are negatively charged.

c)

Neutrons are inside the nucleus.

d)

The atom is mostly empty space.

e)

Nucleus is positively charged.

123.

What happened to the particles that the nucleus was bombarded with in the Gold Foil Experiment?

a)

All bounced back.

b)

All passed through.

c)

Some passed through, but most bounce back.

d)

Some bounced back, but most passed through.

124.

Area of probability of finding an electron.

(a)  

125.

How do electrons move away from the nucleus into higher energy levels?

a)

Absorb energy.

b)

Release energy.

126.

How do electrons move toward the nucleus to lower energy levels?

a)

Absorb energy.

b)

Release energy.

127.

  • Electron configuration when electrons have absorbed energy and electrons have moved into higher energy levels.

a)

Excited State

b)

Ionized State

c)

Ground State

d)

Unstable State

128.

Which could be a possible excited state of the Magnesium atom? (CHECK ALL THAT APPLY!)

a)

2-8-2

b)

1-9-2

c)

2-7-3

d)

2-8-1-1

129.

What form of energy do electrons give off as they fall from the excited state back down to the ground state?

(a)  

130.

The unique set of colors/wavelengths given off by each element as the electrons fall back down to the ground state.

a)

Absorption Spectra

b)

Reflection Spectra

c)

Transmission Spectra

d)

Bright Line Spectra

131.

Which gases are present in the mixture? (CHECK ALL THAT APPLY!)

a)

A

b)

B

c)

C

d)

D

132.

Match the following

a)

Alkali Metals

1.

Group 1

b)

Alkaline Earth Metals

2.

Group 2

c)

Transition Metals

3.

Group 3-12

d)

Halogens

4.

Group 17

e)

Noble Gases

5.

Group 18

133.

Good Conductor

a)

Metal

b)

Nonmetal

134.

Ductile and Malleable

a)

Metal

b)

Nonmetal

135.

Brittle

a)

Metal

b)

Nonmetal

136.

Luster (Shiny)

a)

Metal

b)

Nonmetal

137.

Good Insulator

a)

Metal

b)

Nonmetal

138.

Number of Valence Electrons in Group 16 elements.

a)

2

b)

4

c)

6

d)

8

139.

Which element has properties most similar to those of Nitrogen?

a)

Lithium

b)

Oxygen

c)

Arsenic

d)

Hydrogen

140.

Which element has properties most similar to those of Potassium?

a)

Lithium

b)

Oxygen

c)

Arsenic

d)

Magnesium

141.

Cl2

a)

Solid

b)

Liquid

c)

Gas

142.

P

a)

Solid

b)

Liquid

c)

Gas

143.

H2

a)

Solid

b)

Liquid

c)

Gas

144.

Hg

a)

Solid

b)

Liquid

c)

Gas

145.

Hg

a)

Metal

b)

Nonmetal

c)

Metalloid

146.

O2

a)

Metal

b)

Nonmetal

c)

Metalloid

147.

Ge

a)

Metal

b)

Nonmetal

c)

Metalloid

148.

As

a)

Metal

b)

Nonmetal

c)

Metalloid

149.

Which group has the most reactive metals?

a)

Group 1

b)

Group 2

c)

Group 17

d)

Group 18

150.

As the temperature of a liquid increases, its vapor pressure...

a)

increases.

b)

decreases.

c)

remains the same.

d)

must be 0.

151.

Identify the classification of the element based on its properties.

a)

High conductivity and low electronegativity.

1.

Metal

b)

Low Conductivity and high electronically.

2.

Nonmetal

c)

Both metallic and nonmetallic properties.

3.

Metalloid

152.

Identify the bond type based on elemental classification.

a)

Metal ONLY

1.

Metallic

b)

Metal/Nonmetal

2.

Ionic

c)

Two Different Nonmetals

3.

Polar Covalent

d)

Two of the Same Nonmetals

4.

Nonpolar Covalent

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