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Chemistry Final Review

Total questions: 100

Worksheet time: 2hrs 33mins

Name
Class
Date
1.

A chemical change occurs when a piece of wood ___.

a)

is cut

b)

is painted

c)

rots

d)

Review Please!

2.

the central part of an atom, containing protons and neutrons

a)

proton

b)

nucleus

c)

atom

d)

electron

e)

neutron

3.

the smallest particle of an element that retains the properties of that element

a)

proton

b)

nucleus

c)

atom

d)

electron

e)

neutron

4.

a positively charged subatomic particle

a)

proton

b)

nucleus

c)

atom

d)

electron

e)

neutron

5.

The nucleus of an atom is ___.

a)

positively charged and has more protons than neutrons

b)

negatively charged and has a low density

c)

the central core and is composed of protons and neutrons

6.

a negatively charged subatomic particle

a)

proton

b)

nucleus

c)

atom

d)

electron

e)

neutron

7.

a subatomic particle with no charge

a)

proton

b)

nucleus

c)

atom

d)

electron

e)

neutron

8.

What is the smallest particle of an atom?

a)

electron

b)

proton

c)

neutron

d)

Review Please!

9.

Of the elements Fe, Na, Pt, and Ar, which is a nonmetal?

a)

Fe

b)

Na

c)

Pt

d)

Ar

e)

Review Please!

10.

How many protons are in this ion?

a)

35

b)

36

c)

80

d)

45

e)

Review Please!

11.

How many neutrons are in this ion?

a)

35

b)

36

c)

80

d)

45

e)

Review Please!

12.

How many electrons are in this ion?

a)

35

b)

36

c)

80

d)

45

e)

Review Please!

13.

How many valence electrons are in this atom?

a)

3

b)

8

c)

2

d)

13

e)

Review Please!

14.

How many electron shells are in this atom?

a)

3

b)

8

c)

2

d)

13

e)

Review Please!

15.

Which of the following elements is in the same period as phosphorus?

a)

carbon

b)

magnesium

c)

oxygen

d)

Review Please!

16.

Which of the following elements has the smallest atomic radius?

a)

Bromine

b)

Chlorine

c)

Sulfur

d)

Review Please!

17.

How many valence electrons are in an atom of magnesium?

a)

2

b)

4

c)

3

d)

5

18.

How many valence electrons are in an atom of magnesium?

a)

2

b)

4

c)

3

d)

5

19.

Which of the following categories includes the majority of the elements?

a)

metals

b)

nonmetals

c)

liquids

d)

gases

e)

Review Please!

20.

Matter includes all of the following except

a)

air.

b)

smoke.

c)

light.

d)

water vapor.

21.

A student was cleaning out the laboratory refrigerator and stumbled across an unlabeled vial of a colorless liquid. In order to identify it, the student measured several of its properties. Which of the properties is an intensive property?

a)

the substance forms a white solid when added to vinegar

b)

the density of the substance is 0.742 g/mL

c)

the substance weighs 50.00 grams

d)

its volume is 67.0 mL

22.

After distilling a sample, you find that you have two distinct components. What can be said about the original sample?

a)

it is a compound

b)

it is an element

c)

it is a pure substance

d)

it is a mixture

23.

What is the relationship between wavelength and frequency of all waves on the electromagnetic spectrum?

a)

Wavelength and frequency are directly related.

b)

Wavelength and frequency are inversely related.

c)

Wavelength and frequency are unrelated.

d)

Wavelength and frequency are equal.

24.

The optical portion of the electromagnetic spectrum above represents visible light (red, orange, yellow, green, blue, indigo, and violet). Which statement is correct about the optical portion of the spectrum?

a)

The photons of red light have more energy than photons of violet light.

b)

The photons of red light have equal energy as photons of violet light.

c)

The photons of red light have less energy than photons of violet light.

d)

The photons of violet light have less energy than photons of red light.

25.

What atom matches this electron configuration?

1s2 2s2 2p6 3s2

a)

Magnesium

b)

Neon

c)

Aluminum

d)

Potassium

26.

Which is the electron configuration for an oxygen atom?

a)

1s22s22p63s23p64s2

b)

1s22s22p6

c)

1s22s22p4

d)

1s22s22p63s23p6

27.

How many valence electrons are represented here?

a)

7

b)

2

c)

5

d)

8

28.

What is this element?

1s22s22p63s23p6

4s23d104p6

a)

Argon

b)

Bromide

c)

Selenium

d)

Krypton

29.

Which is the correct Lewis structure for Nitrogen?

a)
b)
c)
d)
30.

A _______ is a neutral group of atoms that are held together by covalent bonds.

a)

Molecule

b)

Compound

c)

Substance

31.

Chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet (8) of electrons in its highest occupied energy level.This is called the:

a)

O'doyle Rules

b)

Valence Rule

c)

Aqua Rule

d)

Octet Rule

32.

Properties of Metals:

a)

They generally have high melting points.

b)

They are all liquids at room temperature except mercury

c)

They are bad conductors of heat and electricity.

d)

They are malleable & ductile

33.
Which state of matter is represented here?
a)
Solid
b)
Liquid
c)
Gas
34.
Describe how particles in a gas behave.
a)
They don't move at all.
b)
They vibrate.
c)
They move rapidly.
d)
They move moderately and vibrate
35.
What kind of intermolecular force is shown here?
a)
hydrogen bonding
b)
London dispersion
c)
network covalent
d)
electrostatic (ionic)
36.
Which kind of intermolecular force is shown here?
a)
electrostatic (ionic)
b)
network covalent
c)
London dispersion
d)
dipole-dipole
37.
Which letter represents the energy needed to start the reaction?
a)
A
b)
B
c)
C
d)
D
38.
Which formula represents enthalpy?
a)
C-A
b)
A-C
c)
D-A
d)
A-D
39.
Which of the following solutions is more concentrated?
a)
A
b)
B
c)
Cannot determine
d)
They are equal
40.
Which of the following solutions is more concentrated?
a)
A
b)
B
c)
Cannot determine
d)
They are the same
41.
Where would the level of A have to be for the reaction to be endothermic?
a)
Just where it is now
b)
Below where it is now
c)
At the same level as C
d)
Above the level of C
42.
Endothermic reactions feel
a)
hot
b)
cold
c)
nice
d)
sleepy
43.

A 4.0 g sample of iron was heated from 0°C to 20.°C. It absorbed 35.2 J of energy as heat. What is the specific heat of this piece of iron?

a)

2816 J/gxC

b)

2.27 J/gxC

c)

2.27 J/g

d)

0.44 J/gxC

44.

Name the compound Fe(NO3)2.

a)

Iron (II) Nitrate

b)

Iron (II) Nitrite

c)

Iron (III) Nitrate

d)

Iron (III) nitride

45.

For the reaction represented by the equation 2H2 + O2 ® 2H2O, how many grams of water are produced from 6.00 mol of hydrogen?

a)

2

b)

6

c)

54

d)

108

46.

The electron configuration of an element is [Kr] 4d6 5s1. To what group does this element belong?

a)

4

b)

5

c)

7

d)

9

47.

Which coefficients correctly balance the formula equation

NH4NO2(s)® N2(g) + H2O(l)?

a)

1 2 2

b)

1 1 2

c)

2 1 1

d)

2 2 2

48.

What is the formula for the compound formed by calcium ions and chloride ions?

a)

CaCl

b)

Ca2Cl

c)

CaCl3

d)

CaCl2

49.

The energy required to remove an electron from an atom is the atom's

a)

electron affinity

b)

electron energy

c)

electronegativity

d)

ionization energy

50.

In the reaction represented by the equation 2Al2O3 ® 4Al + 3O2, what is the mole ratio of aluminum to oxygen?

a)

10:6

b)

3:4

c)

2:3

d)

4:3

51.

According to the kinetic-molecular theory, particles of matter

a)

are in constant motion

b)

have different shapes

c)

have different colors

d)

are always fluid

52.

The greater the average kinetic energy of the particles in a sample of matter,

a)

the higher the temperature is.

b)

the lower the termperature is.

c)

the more energy is absorbed by the sample in the form of heat.

d)

the less energy is released by the sample in the form of heat.

53.

ΔH is always positive for a

a)

spontaneous reaction

b)

non spontaneous reaction

c)

exothermic reaction

d)

endothermic reaction

54.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
55.
The formula of calcium phosphate is 
a)
CaPO4
b)
Ca2(PO4)3
c)
Ca3PO4
d)
Ca3(PO4)2
56.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
57.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
58.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
59.

The diagram provided here shows the reactants and the products of a common chemical reaction. The line on the graph behind them represents the energy of the system as the reaction progresses. Which of the following conclusions is best supported by the information provided?

a)

This is a fast reaction.

b)

This is a slow reaction.

c)

This reaction is endothermic.

d)

This reaction is exothermic.

60.

You can speed up a reaction by... (choose all that apply)

a)

adding an inhibitor

b)

adding a catalyst

c)

cooling the reaction

d)

heating the reaction

e)

increasing the surface area

61.

If a reaction is endothermic

a)

the system is losing energy

b)

the system is gaining energy

c)

the universe is losing energy

d)

the universe is gaining energy

62.

Complete this sentence: Atomic radius ____ from left to right across a period and ____ from top to bottom down a group on the periodic table.

a)

increases, decreases

b)

increases, increases

c)

decreases, decreases

d)

decreases, increases

63.

Complete this sentence: Ionization energy ____ from left to right across a period and ____ from top to bottom down a group on the periodic table.

a)

increases, decreases

b)

increases, increases

c)

decreases, decreases

d)

decreases, increases

64.

Complete this sentence: Metallic character ____ from left to right across a period and ____ from top to bottom down a group on the periodic table.

a)

increases, decreases

b)

increases, increases

c)

decreases, decreases

d)

decreases, increases

65.

Complete this sentence: Electronegativity ____ from left to right across a period and ____ from top to bottom down a group on the periodic table.

a)

increases, decreases

b)

increases, increases

c)

decreases, decreases

d)

decreases, increases

66.

Complete this sentence: Electron affinity ____ from left to right across a period and ____ from top to bottom down a group on the periodic table.

a)

increases, decreases

b)

increases, increases

c)

decreases, decreases

d)

decreases, increases

67.
The right of the arrow is called?
a)
Reactant 
b)
Product
c)
Yields
68.
The left of the arrow is called?
a)
Reactant
b)
Product
c)
Yields
69.
H
H2
NaCl
Cl
O2
List the correct answers in order.
a)
molecule, compound, molecule, element,molecule
b)
element, molecule, compound, compound, molecule
c)
element, molecule, compound, element, molecule
d)
Compound, element, ,molecule, vector, roger
70.
Boiling point, Freezing point, creating a mixture, can be separated, change in state, are all what type of property?
a)
Chemical
b)
Physical
71.
Which of the following is not a chemical property?
a)
Reactivity
b)
Flammability
c)
Half Life
d)
Shape
72.
The easiest way to tell if a change is physical or chemical is to ask yourself?
a)
Did it break?
b)
Did it change color?
c)
Did it create a new substance?
d)
Did it look cool?
73.
List the coeffecieints in order.
a)
4,3,2
b)
2,2,3
c)
4,2,3
d)
1,2,3
74.
List the subscripts in the product only.
a)
2
b)
2,2,3
c)
2,3
d)
4,3,2,
75.
Water = 1 Oxygen + 2 Hydrogen.  Pick the correct formula.
a)
H2O2
b)
HO
c)
H2O
d)
2 H2O2
76.
3 molecules of water = 1 Oxygen + 2 Hydrogen.  Pick the correct formula to represent 3 molecules of water.
a)
H2O
b)
2H2 +  O2
c)
2H2O2
d)
3H2O
77.
Balanced or Unbalanced?
a)
Balanced
b)
Unbalanced
78.
Balanced or Unbalanced?
a)
Balanced
b)
Unbalanced
79.
Balanced or Unbalanced?
a)
Balanced
b)
Unbalanced
80.
Type of reaction?
a)
Sythesis
b)
Double replacement
c)
Single replacement
d)
Combustion
81.
Type of reaction?
a)
Decomposition
b)
Single replacement
c)
Double replacement
d)
Combustion
82.
Type of reaction?
a)
Sythesis
b)
Decomposition
c)
Combustion
d)
Single Replacement
83.
Type of reaction?
a)
Sythesis
b)
Decomposition
c)
Single Replacement
d)
Double replacement
84.

Which coefficients go in the blanks to balance this chemical equation?

a)

4, 3, 2

b)

2, 3, 1

c)

1, 1, 1

d)

3, 2, 4

85.

What type of reaction is this? (select all that apply)

Cl₂(g) + 2KBr(aq) → 2KCl(aq) + Br₂(l)

a)

Single Replacement

b)

Redox

c)

Double Replacement

d)

Neutralization

86.

What is the mass of 4.55 mol of C2H6?

a)

0.151 g

b)

115 g

c)

137 g

d)

661 g

87.

What's the mole ratio of C to CS2 according to the balanced chemical equation?

a)

5 mol C / 1 mol CS2

b)

1 mol C / 5 mol CS2

c)

2 mol C / 4 mol CS2

d)

2 mol C / 5 mol CS2

88.

A scientist calculates the theoretical yield of an experiment to be 25.70g. They recover 12.76g. What is their percent yield?

a)

49.65%

b)

50.35%

c)

65.21%

d)

34.79%

89.

A scientist calculates the theoretical yield of an experiment to be 91.80g. They recover 65.89*g. What is their percent yield?

a)

71.78%

b)

28.22%

c)

84.22%

d)

16.78%

90.

82.3 g of Mg reacts with 57.9 g of N2 to form Mg3N2. Which is the limiting reagent?

a)

Mg

b)

N2

c)

Mg3N2

91.

940.6g of CoF3 react with 428.7 g of SF4 to form SF6 and CoF2. Which is the limiting reagent?

a)

CoF3

b)

SF4

c)

SF6

d)

CoF2

92.

What is 81.4 °F in K?

a)

301 K

b)

286 K

c)

81.4 K

d)

209 K

93.

What happens to the particles of an IDEAL gas when they collide?

a)

The bounce off each other without losing any energy. The collisions are perfectly elastic. 

b)

The bounce off each other and lose some energy. The collisions are inelastic. 

c)

They stick together and go the same direction.

d)

They chemically react.

94.

Which postulate of kinetic molecular theory disproves the following statement:

The size of the gas molecules directly affects the volume of the ideal gas.

a)

A gas consists of individual particles in constant and random motion.

b)

The volume of the individual gas molecules is small when compared to the distance between them.

c)

Collisions between molecules are perfectly elastic.

d)

The pressure of the gas is due entirely to the force of the collisions of the gas particles with the walls of the container.

95.

Which of the following equations illustrates an endothermic reaction?

a)

SO2 + 33.5 J --> S + O2

b)

2CO + O2 --> 2CO2 + 58 kJ

96.

ΔH is negative when...

a)

a reaction is exothermic and heat energy is absorbed from surroundings

b)

a reaction is exothermic and heat energy is released into the surroundings

c)

a reaction is endothermic and heat energy is absorbed from surroundings

d)

a reaction is endothermic and heat energy is released into the surroundings

97.

In an exothermic reaction, what is being transformed into thermal energy?

a)

Light energy of reactants

b)

Kinetic energy of reactants

c)

Chemical energy of reactants

d)

Light energy of products

98.

What are weak acids according to the Arrhenius definition?

a)

They retain most of their OH- in solution

b)

They give up most of their OH- in solution

c)

They retain most of their H+ in solution

d)

They give up most of their H+ in solution

99.

What addition to the end of a compound in a reaction indicates that it is a solid?

a)

(aq)

b)

(g)

c)

(s)

d)

(l)

100.

What is an electrolyte?

a)

A nonmetal that conducts electricity.

b)

A metal that conducts electricity.

c)

An ion that conducts electricity.

d)

A metalloid that conducts electricity.

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