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Chemistry Exam 2

Total questions: 94

Worksheet time: 47mins

Name
Class
Date
1.

Which observation does NOT indicate that a chemical reaction has occurred?

a)

formation of a precipitate

b)

production of a gas

c)

evolution of heat and light

d)

change in total mass of substances

2.

A solid produced by a chemical reaction in solution that separates from the solution is called...

a)

a precipitate

b)

a reactant

c)

a molecule

d)

the mass of the product

3.

What is the small whole number that appears in front of a formula in a chemical equation?

a)

a subscript

b)

a superscript

c)

a ratio

d)

a coefficient

4.

To balance a chemical equation, it may be necessary to adjust the...

a)

coefficients

b)

subscripts

c)

formulas of the products

d)

number of products

5.

According to the law of conservation of mass, the total mass of the reacting substance is...

a)

always more than the total mass of the products

b)

always less than the total mass of the products

c)

sometimes more and sometimes less than the total mass of the products

d)

always equal to the total mass of the products

6.

A chemical equation is balanced when the...

a)

coefficients of the reactants equal the coefficients of the products

b)

same number of each kind of atom appears in the reactants and in the products

c)

products and reactants are the same chemicals

d)

subscripts of the reactants equal the subscripts of the products

7.

In an equation, the symbol for a substance in water solution is followed by...

a)

( L ) - cursive and lowercase L

b)

( g )

c)

( ag )

d)

( s)

8.

A chemical formula written over the arrow in a chemical equation signifies...

a)

a byproduct

b)

the formation of a gas

c)

a catalyst for the reaction

d)

an impurity

9.

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

10.

Which coefficients correctly balance the formula equation:

CaO + H2O---> Ca(OH)2?

a)

2, 1, 2

b)

1, 2, 3

c)

1, 2, 1

d)

1, 1, 1

11.

What is the balanced equation for the combustion of sulfur?

a)

S(s) + O2(g)---> SO(g)

b)

S(s) + O2(g)---> SO2(g)

c)

2S(s) + 3O2(g)--->SO3(s)

d)

S(s) + 2O2(g)---> SO4^2(aq)

12.

In what kind of reaction do two or more substances combine to form a new compound?

a)

decomposition reaction

b)

ionic reaction

c)

double - replacement reaction

d)

synthesis reaction

13.

In what kind of reaction does one element replace a similar element in a compound?

a)

single - replacement reaction

b)

double - replacement reaction

c)

decomposition reaction

d)

ionic reaction

14.

In what kind of reaction does a single compound produce two or more simpler substances?

a)

decomposition reaction

b)

synthesis reaction

c)

single - replacement reaction

d)

ionic reaction

15.

In what kind of reaction do the ions of two compounds exchange places in aqueous solution to form two new compounds?

a)

synthesis reaction

b)

double - replacement reaction

c)

decomposition reaction

d)

combustion reaction

16.

The reaction:

Mg(s) + 2HCl(aq)---> H2(g) + MgCl2(aq)

is a...

a)

composition reaction

b)

decomposition reaction

c)

single - replacement reaction

d)

double - replacement reaction

17.

The reaction:

2HgO(s)--->2Hg(L) + O2(g)

is a(n)

a)

single - replacement reaction

b)

synthesis reaction

c)

ionic reaction

d)

decomposition reaction

18.

The decomposition of a substance by an electric current is called...

a)

electrolysis

b)

conduction

c)

ionization

d)

transformation

19.

What is the name of a list of elements arranged according to the ease with which they undergo certain chemical reactions?

a)

reactivity list

b)

reaction sequence

c)

activity series

d)

periodic list

20.

What can be predicted by using an activity series?

a)

whether a certain chemical reaction will occur

b)

the amount of energy released by a chemical reaction

c)

the electronegativity values of elements

d)

the melting points of elements

21.

Which branch of chemistry deals with the mass relationships of elements in compounds and the mass relationships among reactants and products in chemical reactions?

a)

qualitative analysis

b)

entropy

c)

chemical kinetics

d)

stoichiometry

22.

A balanced chemical equation allows one to determine the...

a)

mole ratio of any two substances in the ratio

b)

energy released in the reaction

c)

electron configuration of all elements in the reaction

d)

mechanism involved in the reaction

23.

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 

24.

According to kinetic - molecular theory, gases condense into liquids because of...

a)

gravity

b)

atmosphere pressure

c)

forces between molecules

d)

elastic collisions

25.

According to kinetic - molecular theory, which substances are made of particles?

a)

ideal gases only

b)

all gases

c)

all matter

d)

all matter except solids

26.

If two moving steel balls collide, their total energy after the collision is the sane as before. This is an example of...

a)

Boyle's law

b)

the law of gravity

c)

an elastic collision

d)

both Boyle's law and Charles's law

27.

Which is an example of gas diffusion?

a)

inflating a flat tire

b)

the odor of perfume spreading throughout a room

c)

a cylinder of oxygen stored under high pressure

d)

All of the above

28.

By which process do gases take the shape of their container?

a)

evaporation

b)

expansion

c)

adhesion

d)

diffusion

29.

If a gas with an odor is released in a room, it quickly can be detected across the room because it...

a)

diffuses

b)

is dense

c)

is compressed

d)

condenses

30.

Which is an example of effusion?

a)

air slowly escaping from a pinhole in a tire

b)

the aroma of a cooling pie spreading across a room

c)

helium dispersing into a room after a balloon pops

d)

oxygen and gasoline fumes mixing in an automobile carburetor

31.

What happens to the volume of a gas during compression?

a)

the volume increases

b)

the volume decreases

c)

the volume remains constant

d)

it is impossible to tell because all gases are different

32.

Pressure is the force per unit...

a)

volume

b)

surface area

c)

length

d)

depth

33.

What is the SI unit of force?

a)

torr

b)

pascal

c)

pound

d)

newton

34.

What instrument measures atmospheric pressure?

a)

barometer

b)

manometer

c)

vacuum pump

d)

torrometer

35.

If the temperature of a container of gas remains constant, how could the pressure of the gas increase?

a)

the mass of the gas molecules increases

b)

the diffusion of the gas molecules increases

c)

the size of the container increases

d)

the number of gas molecules in the container increases

36.

The standard molar volume of a gas as STP is...

a)

22.4 L

b)

g/22.4 L

c)

g - mol wt/22.4 L

d)

1 L

37.

The compressibility of a liquid is generally...

a)

less than that of a gas

b)

more than that of a gas

c)

equal to that of a gas

d)

zero

38.

What is vaporization?

a)

the process by which a liquid changes to a gas

b)

the process by which a solid changes to a gas

c)

both are correct

d)

neither is correct

39.

What is the physical change of a liquid to a solid by the removal of heat?

a)

solidification

b)

particle arrangement

c)

freezing

d)

both, solidification and freezing

40.

Forces holding particles together are the strongest in a...

a)

solid

b)

liquid

c)

gas

d)

vapor

41.

The rate of diffusion in solids is very low because the...

a)

particles are not free to move about

b)

surfaces of solids usually connect gases

c)

attractive forces are weak

d)

melting points are high

42.

Compared with gases, solids are...

a)

more easily compressed

b)

more likely to diffuse

c)

lower in density

d)

incompressible

43.

Which of the following properties do solids share with liquids?

a)

fluidity

b)

definite shape

c)

definite volume

d)

slow rate of diffusion

44.

Compared with a crystalline solid, the particles in an amorphous solid...

a)

occur in a random pattern

b)

occur in a definite, three - dimensional arrangement

c)

consist of molecular sheets

d)

have a more complex unit cell

45.

Which of the following is an amorphous solid?

a)

ice

b)

diamond

c)

graphite

d)

glass

46.

Which of the following is a crystalline solid?

a)

a plastic milk container

b)

a quartz rock

c)

a glass bottle

d)

a three - dimensional glass cube

47.

A system is in equilibrium when...

a)

no physical or chemical changes are occurring

b)

the physical changes counteract the chemical changes

c)

opposing physical or chemical changes occur at equal rates

d)

only physical changes are occurring

48.

A volatile liquid...

a)

has strong attractive forces between particles

b)

evaporates readily

c)

has an order

d)

is ionic

49.

What is the process of a substance changing from a solid to a vapor without passing through the liquid phase?

a)

condensation

b)

evaporation

c)

sublimation

d)

vaporization

50.

A phase diagram indicates the conditions under which...

a)

the various states of a substance exist

b)

amorphous solids become crystalline

c)

Le Chatelier's principle no longer applies

d)

all vapors become flammable

51.

The triple point of a substance is the temperature and pressure conditions at which...

a)

density is greatest

b)

states of a substance coexist at equilibrium

c)

equilibrium cannot occur

d)

kinetic energy is at a minimum

52.

What is the critical pressure?

a)

the pressure at which all substances are solids

b)

the pressure at which the attractive forces in matter break down

c)

the highest pressure under which a solid can exist

d)

the lowest pressure under which a substance can exist as a liquid at the critical temperature

53.

Why are water molecules polar?

a)

they contain two kinds of atoms

b)

the electrons in the covalent bonds spend more time closer to the oxygen nucleus

c)

the hydrogen bonds are weak

d)

they have covalent bonds

54.

Why is ice less dense than liquid water?

a)

the molecules in liquid water can crowd together more compactly than in ice

b)

liquid water's energy level is lower than that of ice

c)

liquid water molecules are farther apart than the molecules in ice

d)

liquid water has fewer chemical impurities than ice has

55.

In ice, what holds H2O molecules together?

a)

ionic bonds

b)

dispersion interaction forces

c)

hydrogen bonds

d)

oxygen - oxygen bonds

56.

What is the boiling point of water at standard pressure?

a)

100C

b)

112C

c)

212C

d)

200C

57.

At about what temperature does water reach its maximum density?

a)

0C

b)

2C

c)

4C

d)

6C

58.

Acids taste...

a)

sweet

b)

sour

c)

bitter

d)

salty

59.

Acetic acid is formed in significant quantities in...

a)

lemons

b)

vinegar

c)

sour milk

d)

apples

60.

Acids generally release H2gas when they react with...

a)

nonmetals

b)

semimetals

c)

active metals

d)

inactive metals

61.

Acids make litmus paper turn...

a)

red

b)

yellow

c)

blue

d)

black

62.

Acids react with...

a)

bases to produce salts and water

b)

salts to produce bases and water

c)

water to produce bases and salts

d)

neither bases, salts, nor water

63.

Aqueous solutions of acids...

a)

always have Faraday properties

b)

conduct electricity

c)

have very high boiling points

d)

cannot be prepared

64.

Which acid is used in batteries?

a)

hydrochloric acid

b)

phosphoric acid

c)

nitric acid

d)

sulfuric acid

65.

What acid is produced in the stomach?

a)

hydrochloric acid

b)

phosphoric acid

c)

nitric acid

d)

sulfuric acid

66.

What is an Arrhenius acid?

a)

a chemical compound that increases the concentration of hydrogen ions in aqueous solution

b)

a chemical compound that increases the concentration of hydroxide ions in aqueous solution

c)

a chemical compound that decreases the concentration of hydrogen ions in aqueous solution

d)

a chemical compound that decreases the concentration of hydroxide ions in aqueous solution

67.

What is an Arrhenius base?

a)

a chemical compound that increases the concentration of hydrogen ions in aqueous solution

b)

a chemical compound that increases in concentration of hydroxide ions in aqueous solution

c)

a chemical compound that decreases in concentration of hydrogen ions in aqueous solution

d)

a chemical compound that decreases in concentration of hydroxide ions in aqueous solution

68.

A substance that ionizes nearly completely in aqueous solutions and produces H3O^+ is a...

a)

weak base

b)

strong base

c)

weak acid

d)

strong acid

69.

Strong acids are...

a)

strong electrolytes

b)

weak electrolytes

c)

nonelectrolytes

d)

nonionized

70.

Which of the following is a triprotic acid?

a)

H2SO4

b)

CH3COOH

c)

HCl

d)

H3PO4

71.

Which of the following is a diprotic acid?

a)

H2SO4

b)

CH3COOH

c)

HCl

d)

H3PO4

72.

A Bronsted - Lowry acid is...

a)

an electron - pair acceptor

b)

an electron - pair donor

c)

a proton acceptor

d)

a proton donor

73.

A Bronsted - Lowry base is a(n)...

a)

producer of OH^- ions

b)

proton acceptor

c)

electron - pair donor

d)

electron - pair acceptor

74.

A Lewis acid is...

a)

an electron - pair acceptor

b)

an electron - pair donor

c)

a proton acceptor

d)

a proton donor

75.

Which acid definition is the broadest?

a)

traditional

b)

Lewis

c)

Bronsted - Lowry

d)

Faraday

76.

A Lewis base is a(n)...

a)

producer of OH^- ions

b)

proton acceptor

c)

electron - pair donor

d)

electron - pair acceptor

77.

An electron - pair donor is a...

a)

traditional base

b)

Bronsted - Lowry acid

c)

Bronsted - Lowry base

d)

Lewis base

78.

An electron - pair acceptor is a...

a)

Bronsted - Lowry base

b)

Lewis acid

c)

Lewis base

d)

traditional acid

79.

A conjugate base is the species that...

a)

remains after a base has given up a proton

b)

is formed by the addition of a proton to a base

c)

is formed by the addition of a proton to an acid

d)

remains after an acid has given up a proton

80.

A conjugate acid is the species that...

a)

remains after a base has given up a proton

b)

is formed by the addition of a proton to a base

c)

is formed by the addition of a proton to an acid

d)

remains after an acid has given up a proton

81.

The conjugate of a strong base is a...

a)

strong acid

b)

weak acid

c)

strong base

d)

weak base

82.

The conjugate of a strong acid is a...

a)

strong acid

b)

weak acid

c)

strong base

d)

weak base

83.

The conjugate of a weak base is a...

a)

strong acid

b)

weak acid

c)

strong base

d)

weak base

84.

The conjugate of a weak acid is a...

a)

strong acid

b)

weak acid

c)

strong base

d)

weak base

85.

An amphoteric species is one that reacts as a(n)...

a)

acid only

b)

base only

c)

acid or base

d)

none of the above

86.

What is neutralization?

a)

an acid - base reaction that does not include dissocation of ions

b)

a reaction of hydronium ions and hydroxide ions to form a salt

c)

a reaction of hydronium ions and hydroxide ions to form water molecules

d)

a reaction of hydronium ions and hydroxide ions to form water molecules and a salt

87.

How many covalent bonds can a carbon atom usually form?

a)

2

b)

3

c)

4

d)

5

88.

What do all organic compounds contain?

a)

hydrogen

b)

water

c)

oxygen

d)

carbon

89.

Which of the following is an alkane?

a)

propyne

b)

propane

c)

propene

d)

propyl bromide

90.

Hydrocarbons in which carbon atoms form only single bonds are arranged in a ring are called...

a)

cycloalkanes

b)

alkynes

c)

alkenes

d)

aromatic hydrocarbons

91.

Which hydrocarbons have double covalent bonds?

a)

alkanes

b)

alkenes

c)

alkynes

d)

aromatic hydrocarbons

92.

Which hydrocarbons have triple covalent bonds?

a)

alkanes

b)

alkynes

c)

alkenes

d)

aromatic hydrocarbons

93.

Why are functional groups important?

a)

the properties of functional groups help to systematically classify compounds

b)

reactions of a compound involve the bonds within a functional group

c)

both are correct

d)

neither is correct

94.

Carboxylic acids are...

a)

weak acids

b)

strong acids

c)

sometimes weak bases

d)

amphoteric

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