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Chemistry Semester 1 Review

Total questions: 202

Worksheet time: 2hrs 41mins

Name
Class
Date
1.

Chemistry is the study of...

a)

matter

b)

motion

c)

space

d)

energy

2.
a)

beaker

b)

flask

c)

test tube

d)

graduated cylinder

e)

micropipette

3.
a)

beaker

b)

flask

c)

test tube

d)

graduated cylinder

e)

micropipette

4.
a)

beaker

b)

flask

c)

test tube

d)

graduated cylinder

e)

micropipette

5.

In the laboratory, you should NOT...

a)

pour leftover chemicals back in the original container

b)

waft air towards your nose instead of sniff it directly

c)

wear goggles, gloves, aprons, and other protective equipment

d)

put broken glass in a specially-marked container

6.

Which branch of chemistry studies carbon-based molecules?

a)

organic chemistry

b)

inorganic chemistry

c)

analytical chemistry

d)

biochemistry

7.

A rule of nature that can usually be described by a mathematical formula is a(n)...

a)

law

b)

theory

c)

hypothesis

d)

observation

8.

A scientific explanation for something that has been extensively tested and has a massive amount of evidence for it is considered a(n)...

a)

law

b)

theory

c)

hypothesis

d)

observation

9.

A testable guess for why something may be is called a(n)...

a)

law

b)

theory

c)

hypothesis

d)

observation

10.

Which of these statements is true regarding experiments?

a)

the independent variable causes changes in the dependent variable

b)

the dependent variable causes changes in the independent variable

11.

Which group does NOT receive the independent variable so that we can compare results?

a)

control group

b)

experimental group

c)

dependent group

12.

For which two of these must you round to the appropriate number of sig figs?

a)

numbers found by calculation

b)

numbers found with a measuring tool

c)

numbers known to be exactly true

d)

numbers in conversion factors

13.

You measured 32.3 but your teacher said you should have got 35.0. What was your percent error?

a)

7.7%

b)

1.2%

c)

15.8%

d)

25.4%

14.

How many sig figs are in this number?

0.00501

a)

2

b)

3

c)

5

d)

6

15.

How many sig figs are in this number?

3.300 x 107

a)

2

b)

4

c)

6

d)

7

16.

Multiply and round to the correct number of sig figs:

23.22 x 8.1

a)

188.082

b)

188.08

c)

1.9 x 102

d)

188

17.

Add and round to the correct number of sig figs:

200.6 + 33.333

a)

233.933

b)

233.93

c)

233.9

d)

234

18.

What is the SI unit of temperature?

a)

°C

b)

°F

c)

K

d)

mol

19.

What is the SI unit of mass?

a)

kg

b)

L

c)

K

d)

m

20.

Which unit of distance is most appropriate for measuring the height of a person?

a)

cm

b)

μm

c)

km

d)

nm

21.

Which of these would change if you went higher in altitude?

a)

your mass

b)

your weight

c)

your height

22.

Absolute zero is the temperature where...

a)

all molecular motion freezes

b)

chemical reactions can happen spontaneously

c)

it's cold enough for nuclear fusion to occur

d)

all solids and liquids become gases

23.

Liters are a unit of...

a)

area

b)

volume

c)

density

d)

mass

24.

Density =

a)

mass / volume

b)

mass x volume

c)

mass x area

d)

mass / area

25.

Things will float on water if they are...

a)

more dense

b)

less dense

c)

hotter

d)

colder

26.

103

a)

kilo

b)

centi

c)

milli

d)

giga

e)

nano

27.

106

a)

kilo

b)

centi

c)

milli

d)

giga

e)

mega

28.

109

a)

hecto

b)

deca

c)

milli

d)

giga

e)

mega

29.

10-2

a)

hecto

b)

deca

c)

centi

d)

nano

e)

mega

30.

10-3

a)

hecto

b)

kilo

c)

milli

d)

nano

e)

mega

31.

1 mi = 1.6 km

How many km is 5.5 mi?

a)

8.8 km

b)

3.4 km

c)

0.29 km

d)

7.1 km

32.

1 m = 3.28 ft

Convert 3.0 x 108 m/s to ft/min

a)

5.9 x 1010 ft/min

b)

1.6 x 107 ft/min

c)

5.5 x 103 ft/min

d)

6.6 x 10-7 ft/min

33.

Which type of chart is best for showing changes in one variable?

a)

line graph

b)

bar graph

c)

circle graph

d)

scatterplot graph

34.

Which type of chart is best for percentages?

a)

line graph

b)

bar graph

c)

circle graph

d)

scatterplot graph

35.

This relationship is...

a)

directly proportional

b)

indirectly proportional

36.

The smallest piece of an element is a(n)...

a)

atom

b)

compound

c)

molecule

d)

formula unit

37.

Which subatomic particle has a positive charge?

a)

proton

b)

neutron

c)

electron

38.

Which subatomic particle has a negative charge?

a)

proton

b)

neutron

c)

electron

39.

Which subatomic particle has no charge?

a)

proton

b)

neutron

c)

electron

40.

Which subatomic particle determines atomic number? For example, H is 1.

a)

proton

b)

neutron

c)

electron

41.

How do you find atomic charge?

a)

p + e

b)

p - e

c)

n + p

d)

n - e

42.

How do you find atomic mass?

a)

p + e

b)

p - e

c)

n + p

d)

n - e

43.

Which particles are in the nucleus?

a)

proton

b)

neutron

c)

electron

44.

Which fundamental force holds particles in the nucleus together?

a)

strong nuclear force

b)

weak nuclear force

c)

electromagnetic force

d)

gravitational force

45.

Which fundamental force controls radioactive decay?

a)

strong nuclear force

b)

weak nuclear force

c)

electromagnetic force

d)

gravitational force

46.

Which fundamental force causes the attraction of opposite charges and repulsion of similar charges?

a)

strong nuclear force

b)

weak nuclear force

c)

electromagnetic force

d)

gravitational force

47.

How many neutrons does 17F- have?

a)

9

b)

8

c)

10

d)

1

48.

How many protons does 17F- have?

a)

9

b)

8

c)

10

d)

1

49.

How many electrons does 17F- have?

a)

9

b)

8

c)

10

d)

1

50.

CO2 changes from a solid to a gas.

a)

chemical change

b)

physical change

51.

Two atoms are crushed together with so much force that they combine into one larger atom.

a)

Nuclear fusion

b)

Nuclear fission

52.

One large atom breaks apart into smaller atoms

a)

Nuclear fusion

b)

Nuclear fission

53.

An atom has 11 protons, 12 neutrons, and 10 electrons. What is its atomic number?

a)

11

b)

23

c)

1-

d)

1+

54.

An atom has 11 protons, 12 neutrons, and 10 electrons. What is its mass number?

a)

11

b)

23

c)

12

d)

1+

55.

An atom has 11 protons, 12 neutrons, and 10 electrons. What is its charge?

a)

2-

b)

2+

c)

1-

d)

1+

56.

Which particle(s) are made of smaller particles called quarks?

a)

protons

b)

neutrons

c)

electrons

57.

12C and 12C are both carbon, but have different masses. They are...

a)

isotopes

b)

cations

c)

anions

d)

compounds

58.

Na+ and Ca2+ are both...

a)

isotopes

b)

cations

c)

anions

d)

compounds

59.

Cl- and O2- are both...

a)

isotopes

b)

cations

c)

anions

d)

compounds

60.

O2 is an...

a)

element

b)

compound

c)

homogeneous mixture

d)

heterogeneous mixture

61.

NaCl is a(n)...

a)

element

b)

compound

c)

homogeneous mixture

d)

heterogeneous mixture

62.

NaCl(aq) is a(n)...

a)

element

b)

compound

c)

homogeneous mixture

d)

heterogeneous mixture

63.

Trail mix is a(n)...

a)

element

b)

compound

c)

homogeneous mixture

d)

heterogeneous mixture

64.

The "3" in 3H2O is a...

a)

coefficient that indicates how many molecules are present

b)

coefficient that indicates how many atoms are in each molecule

c)

subscript that indicates how many molecules are present

d)

subscript that indicates how many atoms are in each molecule

65.

The "2" in 3H2O is a...

a)

coefficient that indicates how many molecules are present

b)

coefficient that indicates how many atoms are in each molecule

c)

subscript that indicates how many molecules are present

d)

subscript that indicates how many atoms are in each molecule

66.

Which of these is NOT one of the 7 diatomic elements?

a)

O2

b)

F2

c)

N2

d)

S2

67.

Covalent bonds form...

a)

formula units

b)

molecules

68.

Ionic bonds form...

a)

formula units

b)

molecules

69.

In NaCl(aq), what is the solute?

a)

H2O

b)

NaCl(aq)

c)

NaCl

70.

In NaCl(aq), what is the solvent?

a)

H2O

b)

NaCl(aq)

c)

NaCl

71.

A homogeneous mixture with metals is called a(n)...

a)

aqueous solution

b)

colloid

c)

alloy

d)

formula unit

72.

Which of these is NOT a physical property?

a)

color

b)

melting point

c)

density

d)

reactivity

73.

Temperature is the average ___ of a substance's particles.

a)

kinetic energy

b)

potential energy

c)

density

d)

reactivity

74.

Has definite shape and volume

a)

solid

b)

liquid

c)

gas

d)

plasma

75.

Has definite volume, but not shape

a)

solid

b)

liquid

c)

gas

d)

plasma

76.

Does not have definite shape or volume; atoms have no charge

a)

solid

b)

liquid

c)

gas

d)

plasma

77.

Does not have definite shape or volume; free-flying charged particles

a)

solid

b)

liquid

c)

gas

d)

plasma

78.

When particles are arranged in orderly patterns, the substance is called a(n)...

a)

crystal

b)

amorphous solid

c)

colloid

d)

alloy

79.

solid to liquid

a)

melting

b)

freezing

c)

vaporization

d)

sublimation

e)

condensation

80.

liquid to solid

a)

melting

b)

freezing

c)

vaporization

d)

sublimation

e)

condensation

81.

liquid to gas

a)

deposition

b)

freezing

c)

vaporization

d)

sublimation

e)

condensation

82.

gas to liquid

a)

deposition

b)

freezing

c)

vaporization

d)

sublimation

e)

condensation

83.

gas to solid

a)

deposition

b)

melting

c)

vaporization

d)

sublimation

e)

condensation

84.

solid to gas

a)

deposition

b)

melting

c)

vaporization

d)

sublimation

e)

condensation

85.

gas to plasma

a)

deposition

b)

ionization

c)

recombination

d)

sublimation

e)

condensation

86.

Adding solute to a liquid will...

a)

decrease its melting point but increase its boiling point

b)

decrease its melting point and boiling point

c)

increase its melting point and boiling point

d)

increase its melting point but decrease its boiling point

87.

At higher altitudes, boiling occurs at ___ temperatures due to the ___ air pressure.

a)

higher; increased

b)

lower; increased

c)

higher; decreased

d)

lower; decreased

88.

A chemical that assists in a chemical reaction, but is not chemically changed, is called a(n)...

a)

alloy

b)

catalyst

c)

formula unit

d)

colloid

89.

Which law requires that you must end a chemical reaction with the same number of atoms you started with?

a)

law of conservation of mass

b)

law of conservation of momentum

c)

2nd law of thermodynamics

d)

1st law of motion

90.

In this reaction, what coefficient belongs in front of O2?

CH4 + O2 → H2O + CO2

a)

none (implied 1)

b)

2

c)

3

d)

4

91.

In this reaction, what coefficient belongs in front of AlBr3?

AlBr3 + K2SO4 → KBr + Al2(SO4)3

a)

none (implied 1)

b)

2

c)

3

d)

6

92.

Light behaves like a...

a)

particle

b)

wave

c)

particle and wave simultaneously

93.

Light behaves like a...

a)

particle

b)

wave

c)

particle and wave simultaneously

94.

A

a)

wavelength

b)

frequency

c)

amplitude

d)

crest

e)

trough

95.

C

a)

wavelength

b)

frequency

c)

amplitude

d)

crest

e)

trough

96.

B

a)

wavelength

b)

frequency

c)

amplitude

d)

crest

e)

trough

97.

D

a)

wavelength

b)

frequency

c)

amplitude

d)

crest

e)

trough

98.

As wavelength gets longer...

a)

frequency and energy both increase

b)

frequency and energy both decrease

c)

frequency increases; energy decreases

d)

frequency decreases; energy increases

99.

How bright or luminous a light appears is caused by...

a)

frequency

b)

amplitude

c)

number of photons

100.

The intensity of a light's color is caused by...

a)

frequency

b)

amplitude

c)

number of photons

101.

The color or hue of light is caused by...

a)

frequency

b)

amplitude

c)

number of photons

102.

When the crests of two waves perfectly overlap, they ___ due to ___.

a)

get stronger; constructive interference

b)

get weaker; constructive interference

c)

get stronger; destructive interference

d)

get weaker; destructive interference

103.

Particles of light are called

a)

photons

b)

positrons

c)

neutrinos

d)

muons

104.

Light is a type of ___ radiation

a)

electromagnetic

b)

gravitational

c)

conductive

d)

colloidal

105.

Of the visible colors, red light has the...

a)

longest wavelength and highest frequency

b)

longest wavelength and lowest frequency

c)

shortest wavelength and highest frequency

d)

shortest wavelength and lowest frequency

106.

Which type of EM radiation has the longest wavelengths, which makes them good for long-distance communications?

a)

radio

b)

infrared

c)

ultraviolet

d)

gamma

107.

Which type of EM radiation has wavelengths in the mm-cm range, which makes them good for vibrating molecules?

a)

X-rays

b)

microwaves

c)

ultraviolet

d)

gamma

108.

Which type of EM radiation is do we release from our body heat? This is detectable by night- and heat-vision cameras.

a)

radio

b)

infrared

c)

ultraviolet

d)

gamma

109.

Which type of EM radiation includes "black light" and the rays that cause sunburns?

a)

X-rays

b)

microwaves

c)

ultraviolet

d)

infrared

110.

Which type of EM radiation is more ionizing than UV but less ionizing than gamma?

a)

X-rays

b)

microwaves

c)

radio

d)

infrared

111.

Which type of EM radiation has the shortest wavelength and is most energetic?

a)

X-rays

b)

microwaves

c)

radio

d)

gamma

112.

Electricity is the flow of...

a)

electrons

b)

protons

c)

neutrons

d)

photons

113.

Metals are good at conducting electricity because...

a)

the electrons don't belong to any one atom

b)

the weak attraction between cation and anions

c)

they have more protons to repel electrons

d)

metals are polar

114.

If all electrons are in the lowest possible energy levels and orbitals, the atom is in the...

a)

ground state

b)

excited state

c)

spectral state

d)

catalyst state

115.

If an atom absorbs energy and jumps into a higher energy level, the atom is in the...

a)

ground state

b)

excited state

c)

spectral state

d)

catalyst state

116.

When atoms absorb energy, their...

a)

protons go up energy levels

b)

protons go down energy levels

c)

electrons go up energy levels

d)

electrons go down energy levels

117.

Atoms release photons when...

a)

protons go up energy levels

b)

protons go down energy levels

c)

electrons go up energy levels

d)

electrons go down energy levels

118.

The study of how atoms absorb and emit light is called...

a)

cosmology

b)

spectroscopy

c)

organic chemistry

d)

astrology

119.

The Heisenberg Uncertainty Principle says it's not possible to know both the position and momentum of an electron because...

a)

observing them causes them to move

b)

they only exist theoretically

c)

they're too small too be able to detect

d)

they can spontaneously break into quarks

120.

Although this is how atoms are usually drawn, what's wrong with this depiction? Check all that apply.

a)

Electrons don't orbit like planets. They move around in random directions.

b)

The nucleus is very, very, very tiny compared to the electron cloud.

c)

Electrons orbitals aren't always circular; they can have weird shapes.

d)

Electrons are much, much smaller than protons and neutrons.

121.

Which orbital has 1 sublevel and holds 2 electrons?

a)

s

b)

p

c)

d

d)

f

122.

Which orbital has 3 sublevels and holds 6 electrons?

a)

s

b)

p

c)

d

d)

f

123.

Which orbital has 5 sublevels and holds 10 electrons?

a)

s

b)

p

c)

d

d)

f

124.

Which orbital has 7 sublevels and holds 14 electrons?

a)

s

b)

p

c)

d

d)

f

125.

1s2 2s2 2p6

a)

O

b)

C

c)

Na +

d)

Br -

126.

Fe

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d6

b)

1s2 2s2 2p6 3s2 3p6 4s2 4p6

c)

1s2 2s2 3s2 4s2 4s2 3p6 46

d)

1s2 2s2 3s2 4s2 4s2 3p6 3d10

127.

N

a)

1s ↑↓ 2s ↑↓ 2p ↑↓ ↑

b)

1s ↑↓ 2s ↑↓ 2p ↑ ↑ ↑

c)

1s ↑↓ 2s ↑↓ 2p ↓↓↓

d)

1s ↑ 2s ↑ 2p ↑ ↑ ↑ 3s ↑ 3p ↑

128.

[Ar] 4s1

a)

K

b)

Kr

c)

Cl

d)

Na

129.

Which type of metals have valence electrons in the d orbital?

a)

transition metals

b)

alkali metals

c)

alkaline earth metals

d)

basic metals

130.

Which type of metals have valence electrons in the s1 orbital?

a)

transition metals

b)

alkali metals

c)

alkaline earth metals

d)

basic metals

131.

Which type of metals have valence electrons in the s2 orbital?

a)

transition metals

b)

alkali metals

c)

alkaline earth metals

d)

basic metals

132.

What charge do ions of alkali metals form?

a)

1+

b)

2+

c)

1-

d)

2-

133.

What charge do ions of halogens form?

a)

1+

b)

2+

c)

1-

d)

2-

134.

Which chemical family is the LEAST reactive?

a)

noble gases

b)

halogens

c)

alkali metals

d)

transition metals

135.

Which of these chemical families is the MOST reactive?

a)

noble gases

b)

basic metals

c)

halogens

d)

transition metals

136.

Which element is in period 3, group 2?

a)

Mg

b)

Y

c)

B

d)

Li

137.

Electrons in the outermost energy shell are called...

a)

valence electrons

b)

ground-state electrons

c)

catalyst electrons

d)

ionic electrons

138.

Which element has 6 valence electrons?

a)

C

b)

O

c)

N

d)

Ne

139.

Which element forms a 3- charge?

a)

C

b)

O

c)

N

d)

B

140.

According to the octet rule, most atoms want 8...

a)

valence electrons

b)

orbitals

c)

neutrons

d)

energy levels

141.

Which elements cannot conduct electricity?

a)

metals

b)

nonmetals

c)

metalloids or semimetals

142.

Which family consists of mostly man-made radioactive elements?

a)

transition metals

b)

halogens

c)

actinides

d)

alkaline earth metals

143.

Dots in a Lewis structure represent...

a)

valence electrons

b)

atomic charge

c)

atomic number

d)

energy levels

144.

In which type of bond are electrons shared evenly between two nonmetals?

a)

polar covalent

b)

nonpolar covalent

c)

ionic

d)

metallic

145.

In which type of bond are electrons shared between two nonmetals, but not evenly?

a)

polar covalent

b)

nonpolar covalent

c)

ionic

d)

metallic

146.

In which type of bond does a metal give electrons away to a nonmetal?

a)

polar covalent

b)

nonpolar covalent

c)

ionic

d)

metallic

147.

In which type of bond do electrons move freely amongst all atoms?

a)

polar covalent

b)

nonpolar covalent

c)

ionic

d)

metallic

148.

Which type of bond will form in SO2?

a)

single covalent

b)

double covalent

c)

triple covalent

d)

ionic

149.

Which type of bond will form in MgO?

a)

single covalent

b)

double covalent

c)

triple covalent

d)

ionic

150.

Which type of bond will form in CH4?

a)

single covalent

b)

double covalent

c)

triple covalent

d)

ionic

151.

Which type of bond will form in N2?

a)

single covalent

b)

double covalent

c)

triple covalent

d)

ionic

152.

Which ionic compound will form between K and N?

a)

KN

b)

K3N

c)

KN3

d)

KN2

153.

Which ionic compound will form between Ni2+ and PO43- ?

a)

NiPO4

b)

Ni2PO4

c)

Ni3PO8

d)

Ni3(PO4)2

154.

What charge does Cu have in CuBr?

a)

1+

b)

2+

c)

3+

d)

4+

155.

SO42- is a(n)...

a)

cation

b)

polyatomic ion

c)

acid

d)

base

156.

CaO

a)

calcium oxide

b)

calcium (II) oxide

c)

calcium monoxide

d)

monocalcium monoxide

157.

NO2

a)

nitrogen oxide

b)

nitrogen dioxide

c)

mononitrogen dioxide

d)

nitrogen oxide (II)

e)

nitrogen dioxate

158.

NiCl

a)

nickel chloride

b)

nickel (I) chloride

c)

nickel monochloride

d)

nickel chlorite

e)

nickel chlorate

159.

sodium chlorite

a)

NaClO

b)

NaClO2

c)

NaCl

d)

Na(ClO2)2

160.

hydrogen nitrate is also called

a)

nitric acid

b)

hydronitric acid

c)

nitrous acid

d)

hyponitrous acid

161.

hydrogen sulfite is also called

a)

sulfuric acid

b)

hydrosulfuric acid

c)

sulfurous acid

d)

persulfous acid

162.

hydrogen chloride is also called

a)

chloric acid

b)

hydrochloric acid

c)

chlorous acid

d)

hypochlorous acid

163.

Why do molecules form predictable shapes?

a)

electrons around the atoms repel each other

b)

protons in the nuclei repel each other

c)

positively charged nuclei attract electrons

d)

partial charges attract each other

164.

When drawing molecules in 3D, darkened triangles mean...

a)

the atom is pointing towards you

b)

the atom is pointing away from you

c)

the atom is in the same plane as the central atom

165.

When drawing molecules in 3D, dotted lines mean...

a)

the atom is pointing towards you

b)

the atom is pointing away from you

c)

the atom is in the same plane as the central atom

166.

In AXE format, X represents...

a)

how many atoms are bonded to the central atom

b)

how many central atoms are present

c)

how many lone pairs are around the central atom

d)

how many lone pairs are on the surrounding atoms

167.

In AXE format, E represents...

a)

how many atoms are bonded to the central atom

b)

how many central atoms are present

c)

how many lone pairs are around the central atom

d)

how many lone pairs are on the surrounding atoms

168.

What is the AXE of this molecule?

a)

AX3E2

b)

AX5

c)

AX2E3

d)

AX3

169.

What is the steric number of this molecule?

a)

2

b)

3

c)

5

d)

4

170.

What is the electron domain geometry of this molecule?

a)

trigonal planar

b)

trigonal bipyramidal

c)

T-shaped

d)

trigonal pyramidal

171.

What is the molecular geometry of this molecule?

a)

trigonal planar

b)

trigonal bipyramidal

c)

T-shaped

d)

trigonal pyramidal

172.

Which element has the highest electronegativity?

a)

F

b)

P

c)

He

d)

Cs

173.

How strongly an atom pulls on electrons of other atoms is called...

a)

electronegativity

b)

polarity

c)

ionicity

d)

covalence

174.

In H2O which atoms are partially positive?

a)

H

b)

O

175.

In HF, the dipole line points towards...

a)

F, which is δ-

b)

F, which is δ+

c)

H, which is δ-

d)

H, which is δ+

176.

Overall, CO2 is a(n) ___ molecule.

a)

polar

b)

nonpolar

c)

ionic

d)

metallic

177.

Which intermolecular force is weakest? It's caused by an attraction between temporary partial charges caused by from the random positions of electrons.

a)

london dispersion forces

b)

dipole-dipole interactions

c)

hydrogen bonds

178.

Which intermolecular force is the second strongest and exists between partial charges of polar molecules with small electronegativity differences?

a)

london dispersion forces

b)

dipole-dipole interactions

c)

hydrogen bonds

179.

Which intermolecular force is the strongest and exists between partial charges of extremely polar molecules?

a)

london dispersion forces

b)

dipole-dipole interactions

c)

hydrogen bonds

180.

Water is cohesive and adhesive due to its...

a)

hydrogen bonding

b)

covalent bonding

c)

ionic bonding

d)

metallic bonding

181.

If a solute is aqueous, that means it is...

a)

dissolved in water

b)

a precipitate

c)

insoluble in water

d)

hydrophobic

182.

An insoluble chemical is produced when two solutions are mixed. This is called a(n)...

a)

hydrophilic substance

b)

precipitate

c)

aqueous solution

d)

catalyst

183.

Water cannot mix with substances that are...

a)

hydrophobic

b)

hydrophilic

c)

ionic

d)

covalent

184.

A chemical that has polar and nonpolar sides and can force water and oil to mix is called a(n)...

a)

catalyst

b)

emulsifier

c)

precipitate

d)

coefficient

185.

Which chemicals produce an H+ ion when dissolved in water?

a)

acids

b)

bases

c)

precipitates

d)

emulsifiers

186.

Which chemicals produce an OH- ion when dissolved in water?

a)

acids

b)

bases

c)

precipitates

d)

emulsifiers

187.

Alkaline is another word for...

a)

acidic

b)

basic

c)

aqueous

d)

hydrophobic

188.

Which of these is the strongest base?

a)

pH 3

b)

pH 5

c)

pH 7

d)

pH 9

e)

pH 11

189.

Which of these is the strongest acid?

a)

pH 3

b)

pH 5

c)

pH 7

d)

pH 9

e)

pH 11

190.

Pure water is perfectly neutral. What pH is neutral?

a)

pH 3

b)

pH 5

c)

pH 7

d)

pH 9

e)

pH 11

191.

An acid-base neutralization reaction always produces... (Check all that apply)

a)

H2O

b)

a salt

c)

CO2

d)

O2

e)

an organic compound

192.

A combustion reaction always produces... (Check all that apply)

a)

H2O

b)

a salt

c)

CO2

d)

O2

e)

an organic compound

193.

The reactants of a combustion reaction are always... (Check all that apply)

a)

H2O

b)

a salt

c)

CO2

d)

O2

e)

an organic compound

194.

Chemicals that change color in the presence of an acid or base are called...

a)

indicators

b)

catalysts

c)

precipitates

d)

emulsifiers

195.

The energy required to start a chemical reaction is called...

a)

activation energy

b)

precipitation energy

c)

catalytic energy

d)

emulsifying energy

196.

2Na + Cl2 → 2NaCl

a)

synthesis

b)

decomposition

c)

single-replacement

d)

double-replacement

e)

combustion

197.

Acid-base neutralization reactions are a type of...

a)

synthesis

b)

decomposition

c)

single-replacement

d)

double-replacement

e)

combustion

198.

HgSe → Hg + Se

a)

synthesis

b)

decomposition

c)

single-replacement

d)

double-replacement

e)

combustion

199.

Mg + CuS → Cu + MgS

a)

synthesis

b)

decomposition

c)

single-replacement

d)

double-replacement

e)

combustion

200.

LiF + NaCl → LiCl + NaF

a)

synthesis

b)

decomposition

c)

single-replacement

d)

double-replacement

e)

combustion

201.

CH4 + 2O2 → 2H2O + CO2

a)

synthesis

b)

decomposition

c)

single-replacement

d)

double-replacement

e)

combustion

202.

HCl + NaOH → H2O + NaCl

a)

synthesis

b)

decomposition

c)

single-replacement

d)

double-replacement

e)

combustion

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