Free Printable Chemistry Final Exam Study Guide

1.

Which of the following is a physical property?

a)

Explosive

b)

Combustible

c)

Melting point

d)

Ability to rust

2.

Which of the following is true about homogeneous mixture?

a)

They are known as solutions.

b)

They consist of two or more phases.

c)

They have compositions that never vary.

d)

They are always liquids.

3.

Which of the following is a mixture?

a)

Baking soda

b)

Mayonaise

c)

Sucrose

d)

Table salt

4.

Which of the following represents a compound?

a)

H

b)

H-3

c)

$H_2O$

d)

O-16

5.

Which of the following is a chemical property?

a)

Color

b)

Hardness

c)

Freezing point

d)

Ability to react with oxygen

6.

Which of the following is true for all chemical reactions?

a)

The total mass of the reactants increases.

b)

The total mass of the products is greater than the total mass of the reactants.

c)

The total mass of the products is less than the total mass of the reactants.

d)

The total mass of the reactants equals the total mass of the products.

7.

Which group of measurements is the most precise? (Each group of measurements is for a different object.)

a)

2 g, 3 g, 4 g

b)

2.0 g, 3.0 g, 4.0 g

c)

2 g, 2.5 g, 3 g

d)

1 g, 3 g, 5 g

8.

Three different people weigh a standard mass of 2.00 g on the same balance. Each person obtains a reading of 7.32 g for the mass of the standard. These results imply that the balance that was used is__.

a)

Accurate

b)

Precise

c)

Accurate and precise

d)

Neither accurate nor precise

9.

In the measurements 0.503 L, which digit is the estimated digit?

a)

5

b)

The 0 immediately to the left of 3

c)

3

d)

The 0 to the left of the 3

10.

Density is found by dividing___.

a)

Mass by volume

b)

Volume by mass

c)

Mass by area

d)

Area by mass

11.

What is the volume of 45.6 g of silver if the density of silver is 10.5 g/mL?

a)

0.23 mL

b)

4.34 mL

c)

479 mL

d)

none of the above

12.

Which of the following is necessary to calculate the atomic mass of an element?

a)

The atomic mass of carbon-12.

b)

The atomic number of the element.

c)

The relative masses of the element's protons and neutrons.

d)

The masses and relative abundance of each isotope of the element.

13.

What is the maximum number of f orbitals in any single energy level in an atom?

a)

1

b)

3

c)

5

d)

7

14.

How many valence electrons are in an atom of magnesium?

a)

2

b)

3

c)

4

d)

5

15.

Which of the following elements forms an ion with a 1- charge?

a)

Fluorine

b)

Hydrogen

c)

Potassium

d)

Sodium

16.

Under what conditions can potassium bromide conduct electricity?

a)

Only when melted.

b)

Only when dissolved.

c)

Only when it is in crystal form.

d)

Only when melted or dissolved in water.

17.

Aluminum is a group 3A metal. Which ion does Al typically form?

a)

$Al^{3-}$

b)

$Al^{3+}$

c)

$Al^{5-}$

d)

$Al^{5+}$

18.

Which of the following is a cation?

a)

$SO_3^{\ \ 2-}$

b)

Sulfate

c)

$Ca^{2+}$

d)

Chlorite

19.

In which of the following is the name and formula given correctly?

a)

Sodium oxide, NaO

b)

Barium nitride, BaN

c)

Cobaltous chloride, $CoCl_3$

d)

Stannic fluoride, $SnF_4$

20.

Which of the following combinations of symbol and explanation of symbol is correct when used in a

a)

(g), grams

b)

(l), liters

c)

(aq), dissolve in water

d)

(s), solid product

21.

Which field of science studies the composition and structure of matter?

a)

Physics

b)

Biology

c)

Chemistry

d)

Geology

22.

A theory is a__

a)

Proposed explanation for an observation.

b)

Well-tested explanation for a broad set of observations.

c)

Summary of the results of many observations.

d)

Procedure used to test a proposed explanation.

23.

Which of the following is a physical change?

a)

Corrosion

b)

Explosion

c)

Evaporation

d)

Rotting of food

24.

Which of the following is a heterogeneous mixture?

a)

Vinegar in water

b)

Milk

c)

Oil and vinegar

d)

Air

25.

When an iron nail is ground into powder, its mass___.

a)

Stays the same

b)

Decreases

c)

Increases

d)

Cannot be determined

26.

The chief advantage of the metric system over other systems of measurement is that it___.

a)

has more units

b)

is in the multiples of 10

c)

is in the multiples of 15

d)

is derived from nature itself

27.

Which of the following is true about subatomic particles?

a)

Electrons are negatively charged and are the heaviest subatomic particle.

b)

Protons are positively charged and the lightest subatomic particle.

c)

Neutrons have no charge and are the lightest subatomic particle.

d)

The mass of the neutron nearly equals the mass of a proton.

28.

The particles that are found in the nucleus of an atom are___.

a)

neutrons and electrons

b)

electrons only

c)

protons and neutrons

d)

protons and electrons

29.

The nucleus of an atom is

a)

the central core and is composed of protons and neutrons.

b)

positively charged and has more protons than neutrons.

c)

negatively charged and has a high density.

d)

negatively charged and has a low density.

30.

The atomic number of an element is the total number of which particles in the nucleus?

a)

neutrons

b)

protons

c)

electrons

d)

protons and electrons

31.

An element has an atomic number of 76. The number of protons and electrons in a neutral atom of the element are___.

a)

152 protons and 76 electrons

b)

76 protons and 0 electrons

c)

38 protons and 38 electrons

d)

76 protons and 76 electrons

32.

Isotopes of the same element have different

a)

number of neutrons.

b)

number of protons.

c)

number of electrons.

d)

atomic numbers.

33.

Which of the following sets of symbols represents isotopes of the same element?

a)

91 92 93

J J J 42 42 42

b)

50 50 50 L L L 19 19 19

c)

84 86 87 M M M 38 38 38

d)

138 133 133

Q Q Q

59 59 59

34.

According to the aufbau principle

a)

an orbital may be occupied by only two electrons.

b)

electrons in the same orbital must have opposite spins.

c)

electrons enter orbitals of highest energy first.

d)

electrons enter orbitals of lowest energy first.

35.

Which color of visible light has the shortest wavelength?

a)

yellow

b)

green

c)

blue

d)

violet

36.

Which of the following electromagnetic waves have the highest frequencies?

a)

ultraviolet light waves

b)

X-rays

c)

microwaves

d)

gamma rays

37.

How are the frequency and wavelength of light related?

a)

They are inversely proportional to each other.

b)

Frequency equals wavelength divided by the speed of light.

c)

Wavelength is determined by dividing frequency by the speed of light.

d)

They are directly proportional to each other.

38.

The modern periodic table is arranged in order of increasing atomic___.

a)

mass

b)

charge

c)

number

d)

radius

39.

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

a)

metalloids

b)

liquids

c)

metals

d)

nonmetals

40.

Which of the following elements is a transition metal?

a)

cesium

b)

copper

c)

tellurium

d)

tin

41.

What is the charge of a cation?

a)

a positive charge

b)

no charge

c)

a negative charge

d)

The charge that depends on the size of the nucleus.

42.

What is the element with the highest electronegativity value?

a)

cesium

b)

helium

c)

calcium

d)

fluorine

43.

How does calcium obey the octet rule when reacting to form compounds?

a)

It gains electrons.

b)

It gives up electrons.

c)

It does not change its number of electrons.

d)

Calcium does not obey the octet rule.

44.

Which of the following occurs in an ionic bond?

a)

Oppositely charged ions attract.

b)

Two atoms share two electrons.

c)

Two atoms share more than two electrons.

d)

Like-charged ions attract.

45.

Alloys are important because

a)

their properties are often superior to those of their component elements.

b)

they never corrode.

c)

they are less expensive to produce than their component elements.

d)

their properties are a blend of their component elements.

46.

Which of the following particles are free to drift in metals?

a)

protons

b)

electrons

c)

neutrons

d)

cations

47.

What characteristic of metals makes them good electrical conductors?

a)

They have mobile valence electrons.

b)

They have mobile protons.

c)

They have mobile cations.

d)

Their crystal structures can be rearranged easily.

48.

Which of the following compounds contains the lead (II) ion?

a)

$PbO$

b)

$PbCl_4$

c)

$Pb_2O$

d)

$Pb_2S$

49.

What is the ending for the names of all binary compounds, both ionic and molecular?

a)

-ide

b)

-ite

c)

-ade

d)

-ate

50.

Which of the following correctly shows a prefix used in naming binary compounds with its corresponding number?

a)

deca-, 7

b)

nona-, 9

c)

hexa-, 8

d)

octa-, 4

51.

In the chemical equation $H_2O_2\ \left(aq\right)\ =\ H_2O\ \left(l\right)\ +O_2\ \left(g\right),\$ the $O_2$ is a ___.

a)

catalyst

b)

solid

c)

product

d)

reactant

52.

This symbol for reversible reactions indicates that___.

a)

heat must be applied

b)

an incomplete combustion reaction has occured

c)

a gas is formed by the reaction

d)

the reaction is reversible

53.

A catalyst is

a)

the product of a combination reaction.

b)

not used up in a reaction.

c)

one of the reactants in single-replacement reactions.

d)

a solid product of a reaction.

54.

What are the coefficients that will balance the skeleton equation below?

$N_2+H_2\rightarrow NH_3$

a)

1,1,2

b)

1,3,3

c)

3,1,2

d)

1,3,2

55.

Chemical equations must be balanced to satisfy

a)

the law of definite proportions.

b)

the law of multiple proportions.

c)

the law of conservation of mass.

d)

Avogadro's principle.

56.

In order to predict whether or not a single-replacement reaction takes place, you need to consult a chart that shows the

a)

periodic table.

b)

activity series of metals.

c)

common polytomic ions

d)

ionic charges of representative elements.

57.

The products of a combustion reaction include

a)

water, carbon dioxide, and carbon monoxide.

b)

hydrogen, water, and carbon dioxide.

c)

hydrogen and carbon monoxide.

d)

hydrogen and water.

58.

The reaction $2Fe\ +\ 3Cl_2\ \rightarrow\ 2FeCl_3$ is an example of which type of reaction?

a)

combustion reaction

b)

single-replacement reaction

c)

combination reaction

d)

decomposition reaction

59.

The equation $2C_3H_7OH\ +\ 9O_2\ \rightarrow\ 6CO_2\ +\ 8H_2O$ is an example of which type of reaction?

a)

combustion reaction

b)

single-replacement reaction

c)

double-replacement reaction

d)

decomposition reaction

60.

The variable that is observed during an experiment is called what type of variable?

a)

independent

b)

manipulated

c)

controlling

d)

responding

61.

An example of an extensive property of matter is

a)

temperature.

b)

pressure.

c)

mass.

d)

hardness.

62.

Which state of matter takes both the shape and volume of its container?

a)

solid

b)

liquid only

c)

gas only

d)

both b and c

63.

Which of the following can be classified as a mixture?

a)

pure water

b)

pure air

c)

pure nitrogen

d)

pure gold

64.

The closeness of a measurement to its true value is a measure of its___.

a)

precision

b)

accuracy

c)

responsibility

d)

usefulness

65.

Which of the following measurements contains two significant figures?

a)

0.004 00 L

b)

0.004 04 L

c)

0.000 44 L

d)

0.004 40 L

66.

How many significant figures are in the measurement 0.003 4 kg?

a)

two

b)

four

c)

five

d)

This cannot be determined.

67.

What does the number 84 in the name of krypton-84 represent?

a)

the atomic number

b)

the mass number

c)

the sum of the protons and electrons

d)

twice the number of protons.

68.

Using the periodic table, determine the number of neutrons in $16_O$ .

a)

4

b)

8

c)

16

d)

24

69.

To what category of elements does an element does an element belong if it is a poor conductor of electricity?

a)

transition elements

b)

metalloids

c)

nonmetals

d)

metals

70.

How does atomic radius change from left to right across a period in the periodic table?

a)

It tends to decrease.

b)

It tends to increase.

c)

It first increases, then decreases.

d)

It first decreases, then increases.

71.

The octet rule states that, in chemical compounds, atoms tend to have___.

a)

the electron configuration of a noble gas

b)

more protons than electrons

c)

eight electrons in their principal energy level

d)

more electrons than protons

72.

What is the electron configuration of the oxide ion $\left(O^{2-}\right)$ ?

a)

$1s^22s^22p^4$

b)

$1s^22s^22p^6$

c)

$1s^22s^2$

d)

$1s^22s^22p^2$

73.

Write the formula for the compound barium oxide.

(a)

74.

Write the electron configuration diagram that shows the transfer of electrons that takes place to form the compound sodium fluoride. Include the electron configurations of the ions formed.

a)

$Na\ \left(1s^22s^22p^63s^1\right)\ +F\left(1s^22s^22p^5\right)\ =\ Na^+F^-\left(1s^22s^22p^6\right)$

b)

$Na^+\left(1s^22s^22p^6\right)$

c)

$F^-\left(1s^22s^22p^6\right)$

75.

Give the electron configuration for a neutral atom of chlorine.

a)

$1s^22s^22p^63s^23p^5$

b)

$1s^22s^22p^5$

c)

$1s^22s^22p^63s^23p^6$

d)

$1s^22s^22p^4$

76.

Which group in the periodic table is know as the noble gases?

(a)

77.

Balance the following equation.

$C_3H_6\ +\ O_2\ \rightarrow\ CO\ +\ H_2O$

a)

C = 3

H = 6

O = 2

b)

C = 1

H = 2

O = 2

c)

C = 3

H = 6

O = 6

d)

C = 3

H = 6

O = 6

78.

Use the periodic table to determine the number of neutrons on nitrogen - 14

(a)

79.

Compare the compositions, properties and bonding of ionic and molecular compounds.

a)

Most ionic compounds are crystalline solids at room temperature.

b)

High melting points.

c)

Can conduct electric current when melted or dissolved in water.

d)

Composed of a metal and a nonmetal.

80.

Explain the steps / process of Scientific method. Why is it important that we follow the scientific method when performing a lab experiment? What is the difference between independent and dependent variable?

a)

Observation / Problem

b)

Hypothesis

c)

Experiment

d)

Conclusion

e)

Theory / Natural Law

81.

Describe the five types of chemical reactions and how each is identified based its chemical equation. What is the law of Conservation of Mass? Why is it important to remember when dealing with chemical equations?

a)

Synthesis / Combination:

$A\ +\ B\ \rightarrow\ AB$

b)

Decomposition:

$AB\ \rightarrow\ A\ +\ B$

c)

Single Displacement:

$AB\ +\ C\ \rightarrow\ AC\ +\ B$

d)

Double Displacement:

82.

Describe five types of chemical reactions and how each is identified based on its chemical equation. What is the law of Conservation of Mass? Why is it important to remember when dealing with chemical equations?

a)

Synthesis / Combination: $A\ +\ B\ \rightarrow\ AB$

b)

Decomposition: $AB\ \rightarrow\ A\ +\ B$

c)

Single Displacement: $AB\ +\ C\ \rightarrow\ AC\ +\ B$

d)

Double Displacement: $AB\ +\ CD\ \rightarrow\ AD\ +\ BC$

e)

Combustion: $C_xH_y\ +\ O_2\ \rightarrow\ CO_2\ +\ H_2O$ Mass can neither be created nor destroyed.

83.

What are the trends observed periodic properties (Atomic radius, ionization energy and electronegativity) ?

Explain the reason for these trends. Give an example for each.

(a)

84.

Distinguish between metals, non metals, and metalloids. Give examples for each. What are their properties and how are they arranged in the periodic table?

a)

Metals are generally good conductors of heat and electric current. Copper and Silver

b)

Nonmetals are poor conductors of heat and electric current. Nitrogen and Oxygen

c)

Metalloids have properties that are similar to those of metals and nonmetals. Boron and Silicon

85.

State and illustrate the three laws used in writing electron configuration for an element by taking Chlorine and Aluminum as examples.

a)

The Aufbau Principle: Each electron occupies the lowest energy orbital

b)

Pauli Exclusion Principle: A maximum of two electrons may occupy a single orbital, if the electrons have opposite spins.

c)

Hund's Rule: Single electrons with the same spin must occupy each equal-energy orbital.

Chemistry Final Exam Study Guide

Total questions: 85

Worksheet time: 45mins

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