Free Printable Chemistry Semester Knowledge Test

1.

Which of the following is true about compounds?

a)

They can be physically separated into their component elements

b)

They have compositions that vary

c)

They are substances

d)

They have properties similar to those of the component elements

2.

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

3.

Which state of matter has a definite volume and takes the shape of its container?

a)

Solid

b)

Liquid

c)

Gas

d)

Both b and c

4.

The smallest particle of an element that retains the properties of that element is a(n)___.

a)

Atom

b)

Electron

c)

Proton

d)

Neutron

5.

Which step in the scientific method requires you to use your senses to obtain information?

a)

Revising a hypothesis

b)

Designing an experiment

c)

Making an observation

d)

Stating a theory

6.

Isotopes of the same element have different ____.

a)

Numbers of neutrons

b)

Numbers of protons

c)

Numbers of electrons

d)

Atomic numbers

7.

According to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart as possible?

a)

Pairs of valence electrons

b)

Inner shell electrons

c)

Mobile electrons

d)

The electrons closest to the nuclei

8.

How many valence electrons are in an atom of phosphorous?

a)

2

b)

3

c)

4

d)

5

9.

Which of the following elements is a transition metal?

a)

Cesium

b)

Copper

c)

Tellurium

d)

Tin

10.

What is the formula for phosphoric acid?

a)

H₂PO₃

b)

H₃PO₄

c)

HPO₂

d)

HPO₄

11.

Which of the following is a physical change?

a)

Corrosion

b)

Explosion

c)

Evaporation

d)

Rotting of food

12.

All of the following are physical properties of matter except ____.

a)

Mass

b)

Color

c)

Melting point

d)

Ability to rust

13.

What is the electron configuration of potassium?

a)

1s² 2s² 2p² 3s² 3p² 4s¹

b)

1s² 2s² 2p¹⁰ 3s² 3p³

c)

1s² 2s² 3s² 3p⁶ 3d¹

d)

1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹

14.

The expression of 5008km in scientific notation is ___.

a)

5.008x10³ km

b)

50.08x10^-4 km

c)

5.008x10^-3 km

d)

5.008x10⁴ km

15.

What is the net charge of the ionic compound calcium fluoride?

a)

-2

b)

-1

c)

0

d)

+1

16.

What is the measurement 111.009mm rounded off to four significant figures?

a)

111mm

b)

111.0mm

c)

111.01mm

d)

110mm

17.

Which of the following elements has the smallest first ionization energy?

a)

Sodium

b)

Calcium

c)

Potassium

d)

Magnesium

18.

Which of the following is an example of a physical property?

a)

ability to rust

b)

color is red

c)

ability to catch fire

d)

ability to ripen

19.

Which of the following is a quantitative measurement?

a)

red apples

b)

orange solid

c)

26 degrees

d)

loud engines

20.

The one thing you change in a scientific experiment is known as the...

a)

constant

b)

independent variable

c)

dependent variable

d)

hypothesis

21.

In the laboratory, which of the following is NOT a rule to follow?

a)

wear goggles

b)

tie hair back

c)

read instructions

d)

taste chemicals

22.

Which of the following has three sig figs?

a)

0.2220

b)

220

c)

220.0

d)

0.220

23.

Which of the following is an example of a homogeneous mixture?

a)

salt water

b)

trail mix

c)

raw cake ingredients in a bowl

d)

sodium chloride

24.

If a ski pole is 5.0 ft in length, how long is it in mm?
1 ft = 12 in
1 inch = 2.54 cm
1 cm = 10 mm

a)

0.42 mm

b)

150 mm

c)

1500 mm

d)

11 mm

25.

1s²2s²2p⁶3s¹ is the electron configuration for _______________.

a)

sodium

b)

boron

c)

magnesium

d)

neon

26.

Which element in comparison to other elements has the greatest electronegativity?

a)

francium

b)

chlorine

c)

fluorine

d)

aluminum

27.

Which is the correct formula for the compound formed between beryllium and nitrogen?

a)

BeN

b)

Be₃N

c)

Be₃N₂

d)

Be₂N₃

28.

Which is the correct name for the compound FeS?

a)

Iron Sulfide

b)

Iron (II) Sulfide

c)

Iron (I) Sulfide

d)

Iron (II) Sulfide (II)

29.

How many fluoride atoms would be present in one molecule of sulfur hexafluoride?

a)

6

b)

1

c)

2

d)

8

30.

The number that appears on the bottom right of a chemical symbol indicating how many atoms there are for that element.

a)

subscript

b)

superscript

c)

coefficient

d)

squared

31.

Which of these is a subatomic particle with a negative charge?

a)

photon

b)

ion

c)

neutron

d)

electron

32.

Which of these is an example of an element?

a)

nitinol

b)

iron

c)

water

d)

carbon dioxide

33.

Label the beaker, graduated cylinder, volumetric flask, funnel, and Erlenmeyer flask in the image

a)

beaker

b)

volumetric flask

c)

funnel

d)

Erlenmeyer flask

e)

graduated cylinder

1

2

3

4

5

1)

2)

3)

4)

5)

34.

What is the correct reading for the volume of liquid, in millileters (mL)

a)

20 mL

b)

25 mL

c)

24 mL

d)

24. 0mL

e)

24.00 mL

35.

Which of these is a chemical?

a)

wood

b)

water

c)

air

d)

light

36.

What is the best description of this particle?

a)

sodium electron

b)

sodium atom

c)

sodium molecule

d)

sodium ion

e)

sodium isotope

37.

All atoms are ____.

a)

positively charged, with the number of protons exceeding the number of electrons

b)

negatively charged, with the number of electrons exceeding the number of protons

c)

neutral, with the number of protons equaling the number of electrons

d)

neutral, with the number of protons equaling the number of neutrons

38.

The nucleus of an atom is ____.

a)

composed of protons and neutrons

b)

has more protons than neutrons

c)

contains protons and electrons

d)

consists of electron and neutrons

39.

Isotopes of the same element have different ____.

a)

positions on the periodic table

b)

chemical behavior

c)

atomic numbers

d)

mass numbers

40.

What is the maximum number of d orbitals in a principal energy level?

a)

1

b)

2

c)

3

d)

5

41.

What is the next atomic orbital in the series 1s, 2s, 2p, 3s, 3p?

a)

2d

b)

3d

c)

3f

d)

4s

42.

What is the number of electrons in the outermost energy level of an oxygen atom?

a)

2

b)

4

c)

6

d)

8

43.

What is the electron configuration of Fe?

a)

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁶

b)

1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁸

c)

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁸

d)

1s² 2s² 2p⁶ 3s² 3p⁴ 4s² 3d⁶

44.

How many protons, electrons, and neutrons does an atom with atomic number 50 and mass number 125 contain?

a)

50 protons, 50 electrons, 75 neutrons

b)

75 electrons, 50 protons, 50 neutrons

c)

120 neutrons, 50 protons, 75 electrons

d)

70 neutrons, 75 protons, 50 electrons

45.

In which of the following sets of elements are all members of the set in the same group (family) in the periodic table?

a)

N, P, and S

b)

F, Ne, and Na

c)

Ga, In, and Al

d)

Si, P, and S

46.

Which of the following elements is an alkaline earth metal?

a)

Se

b)

In

c)

Xe

d)

Ba

47.

In which of the following pairs of elements is one element a metalloid and one element a nonmetal?

a)

Hg and P

b)

Ge and F

c)

Pb and Bi

d)

As and Si

48.

Elements in the modern version of the periodic table are arranged in order of increasing__________?

a)

oxidation number

b)

atomic number

c)

atomic mass

d)

number of isotopes

49.

Which of the following has the smallest atomic radius?

a)

O

b)

Be

c)

Li

d)

Ne

50.

Of the following gives the correct order for the trend of decrease atomic radius?

a)

Ar > P > Si > Mg > Na

b)

Si > P > Ar > Na > Mg

c)

Na > Mg > Si > P > Ar

d)

Ar > Si > P > Na > Mg

51.

Luster is a property of ______________.

a)

Metal

b)

Nonmetal

c)

Metalloid

52.

Poor conductors of heat is a property or _______________.

a)

Metal

b)

Nonmetal

c)

Metalloid

53.

Which of the following is a Noble Gas?

a)

Na

b)

Mg

c)

Cl

d)

Ar

54.

Which of the following is a halogen?

a)

Kr

b)

Br

c)

Ca

d)

K

55.

Which of the following is an alkali earth metal?

a)

Kr

b)

Br

c)

Ca

d)

K

56.

How close a measurement is to the accepted value is called..

a)

Accuracy

b)

Precision

c)

Significant

d)

Estimate

57.

When a measurement is repeatable and consistent it is said to have...

a)

High precision

b)

Low precision

c)

High accuracy

d)

Low accuracy

58.

What does this bullseye demonstrate?

a)

High Accuracy & High Precision

b)

High Accuracy & Low Precision

c)

Low Accuracy & High Precision

d)

Low Accuracy & Low Precision

59.

Solve & Round to Correct Sig Figs.
4.5 + 4.32 =

a)

8.8

b)

8.7

c)

8

d)

8.0

60.

Calculate 12.47 m ÷ 3.2 s and give your answer with the correct number of significant figures.

a)

4 m/s

b)

3.9 m/s

c)

3.90 m/s

d)

3.897 m/s

61.

Calculate 0.020 cm x 50 cm x 11.1 cm and give your answer with the correct number of significant figures.

a)

10 cm³

b)

11.1 cm³

c)

11 cm³

d)

11. cm³

62.

Solve, and round using Sig Fig math rules:

12.5-mL + 20.05-mL + 2.69-mL

a)

35 mL

b)

35.2 mL

c)

35.24 mL

d)

35.240 mL

63.

Using correct sig figs, determine the density of an object with a mass of 10.0 grams and a volume of 5.0 mL.

a)

2.00 g/mL

b)

2.0 g/mL

c)

2 g/mL

d)

0.5 g/mL

64.

How would you write the following number using scientific notation?

45,800,000 mL

a)

$45.8\ \times10^6$

b)

$4.58\ \times10^7\ mL$

c)

$4.58\ \times10^7$

d)

$.458\ \times10^8\ mL$

65.

How would you write the following number using scientific notation?

0.004506 mL

a)

$4.506\times10^{-3}$

b)

$4.506\ \times10^3\ mL$

c)

$4.506\ \times10^{-3}\ mL$

d)

$4.5\ \times\ 10^{-3}\ mL$

66.

Calculate the volume of metal with a mass of 56.7 grams and a density of 4.67 grams per milliliter.

a)

12.1413276231 mL

b)

12.1 mL

c)

12.1

d)

$264.789\ \frac{g^2}{mL}$

67.

Convert from meters to cm: 9 meters

a)

900 cm

b)

90 cm

c)

0.9 cm

d)

0.09 cm

68.

1 L = _______ mL

a)

1

b)

10

c)

100

d)

1000

69.

3206 in = ________yd

a)

89 yd 2 in

b)

38472 yd

c)

267.167

d)

38472

70.

100 in = ______________ ft

a)

1,200

b)

5

c)

8.4

d)

8 ft 4 inches

71.

Which of the following atoms represents an isotope of the element Lithium?

a)

b)

c)

d)

72.

Chromium has 2 stable isotopes: Cr-52 and Cr-53. Chromium's atomic mass is 51.996. Which of chromium's 2 stable isotopes is the most abundant?

a)

Cr-52

b)

Cr-53

c)

Not enough information to be determined

d)

Cr-51

73.

Ling is trying to calculate the atomic mass for the element potassium (K). Potassium-39 has an atomic mass of 38.96371 and a percent abundance of 93.258%. Potassium-41 has an atomic mass of 40.96183 and a percent abundance of 6.730%. Which of the following is the correct way to calculate the atomic mass?

a)

(38.96371)(93.258) + (40.96183)(6.730)

b)

(38.96371 + 40.96183) / 2

c)

(38.96371)(.93258) + (40.96183)(0.6730)

d)

(38.96371)(0.93258) + (40.96183)(0.06730)

74.

Which symbol is written correctly?

a)

Au

b)

AU

c)

au

d)

ua

75.

Flourine

a)

Fl

b)

F

c)

fl

d)

Fe

76.

Phosphorus

a)

pH

b)

K

c)

P

d)

ph

77.

What is the noble gas configuration for beryllium?

a)

[He]1s²

b)

[He]2s²

c)

[Li]2s¹

d)

[Li]2s²

78.

What is the noble gas configuration for phosphorus?

a)

[Ar] 3p⁵

b)

[He] 3s² 3p⁵

c)

[Ne] 3s² 3p³

d)

[Na] 3s² 3p⁵

79.

[Ne]3s²3p¹is the noble gas configuration for which element?

a)

scandium

b)

boron

c)

nitrogen

d)

aluminum

80.

What atom matches this electron configuration?
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰

a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

81.

[He]2s²2p⁴ is the noble gas configuration for which element?

a)

oxygen

b)

sulfur

c)

phosphorus

d)

fluorine

82.

If n = 2, what are the allowed values of l ? Select all that apply.

a)

0

b)

1

c)

2

d)

3

83.

Which of the following is incorrect about the quantum variable m, or m_l?

a)

m = -l...l

b)

the value for p is -1, 0, 1

c)

when l is 2, there are 5 values for m

d)

the value is either +1/2 or -1/2

84.

Which of the following sets of quantum numbers (n, l, ml, and ms) describes the valence electron of Na?

a)

2, 1, 0, -½

b)

2, 0, 0, -½

c)

3, 1, 1, +½

d)

3, 0, 0, +½

85.

How many electrons are in 1s² 2s² 2p⁴?

a)

5

b)

6

c)

8

d)

13

86.

Orbital sublevels, or l, represents:

a)

orbital color

b)

orbital shape

c)

electron spin

d)

energy level

87.

The spin of an electron is represented by this variable:

a)

n

b)

m

c)

L

d)

m_s

88.

Which element is this?

a)

Nickel

b)

Neon

c)

Sodium

d)

Nitrogen

89.

What is the atomic number of this atom?

a)

2

b)

4

c)

6

d)

8

90.

Which has more energy?

a)

radio/tv waves

b)

infrared

91.

What is the correct order of the visible light spectrum starting with the longer wavelength?

a)

Red, yellow, orange, blue, violet, indigo

b)

Violet, indigo, blue, green, yellow, orange, red

c)

Green, yellow, blue, indigo, red, orange

d)

Red, orange, yellow, green, blue, indigo, violet

92.

Why were there blank spaces left in Mendeleev's periodic table?

a)

He didn't know what to put there.

b)

Undiscovered elements not yet known.

c)

Multiple elements could have fit

d)

He forgot to add the elements in.

93.

In the modern periodic table elements are arranged by:

a)

atomic mass

b)

atomic number

c)

valence electrons

d)

number of isotopes

94.

The first usable modern periodic table was developed by

a)

Dmitri Mendeleev

b)

Glenn Seaborg

c)

John Newlands

d)

Johan Dobereiner

95.

Which of the following will have a higher electronegativity than arsenic (As)?

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

96.

A substance that is dull, brittle, and a nonconductor would be classified as a

a)

metal

b)

nonnmetal

c)

metalloid

d)

metallica

97.

As you move across the periodic table from left to right, the atomic radius decreases. This is because -

a)

the number of protons increases, so attraction to electrons increases

b)

the number of energy levels increases

c)

the number of electrons increases

d)

the atomic mass increases

98.

What is the charge on an Aluminium ion?

a)

3

b)

+3

c)

+2

d)

+1

99.

A(n) _________ is an ion with a positive (+) charge.

a)

anion

b)

cation

c)

ion

d)

solute

100.

What is the ionic compound formed between Ba and P?

a)

Ba₂P₃

b)

Ba₃P₂

c)

BaP

d)

Ba₂P₂

101.

Atoms gain or lose electrons to become stable by satisfying this rule.

a)

Lewis Structure rule

b)

Periodic Law

c)

octet rule

d)

Ionic Law

102.

Magnesium bromide is an ionic compound with the chemical formula MgBr₂. What does the "2" tell you?

a)

There are 2 bromide ions for every magnesium ion

b)

Bromide has a 2- charge

c)

Bromide has a 2+ charge

d)

There are 2 magnesium ions to every bromide ion

103.

Which of the following is true for ionic bonding & ionic compounds?

a)

They must be made of ions with like charges.

b)

The negative ion must be written first.

c)

Compounds must have an overall charge of zero.

d)

They are made of metals and nonmetals.

e)

The positive ion must be written first.

104.

Metals tend to

a)

gain electrons

b)

lose electrons

105.

What is the charge of ion "X" in CaX?

a)

+1

b)

-1

c)

+2

d)

-2

106.

How many covalent bonds can Hydrogen make?

a)

1

b)

2

c)

3

d)

4

107.

Put a rectangle around the electron(s) that are important for covalent bonding.

A

B

C

D

108.

How many valence electrons?

a)

4

b)

2

c)

6

d)

8

109.

How many covalent bonds can Oxygen make?

a)

4

b)

2

c)

6

d)

8

110.

How many covalent bonds can Nitrogen make?

a)

2

b)

3

c)

5

d)

8

111.

The covalent molecule among the following is

a)

NaCl

b)

NH₃

c)

CaO

d)

KF

112.

Which of the following is the correct Lewis dot structure for a molecule of fluorine, F₂?

a)

b)

c)

d)

113.

CHCl₃ has how many double bonds?

a)

0

b)

1

c)

2

d)

3

114.

What two types of atoms make a covalent bond?

a)

2 Nonmetals

b)

1 Nonmetal and 1 Metal

c)

2 Metals

d)

2 Noble Gases

115.

What molecule could this be? (Each purple cloud represents a lone pair of electrons.)

a)

CO₂

b)

NH₃

c)

H₂S

d)

CH₄

116.

Match the following shapes to their Names

a)

1.

Trigonal Planar

b)

2.

Tetrahedral

c)

3.

Trigonal Pyrimidal

d)

4.

Linear

e)

5.

Bent

117.

What is the Molecular Geometry?

a)

Trigonal Bipyramidal

b)

Tetrahedral

c)

Quadralateral

d)

Pentahedral

118.

CH₄ is

a)

polar

b)

non-polar

119.

NH₃ is

a)

polar

b)

non-polar

120.

Electronegativity _______ across a period and ______ down a group.

a)

increases, increases

b)

increases, decreases

c)

decreases, increases

d)

decreases, decreases

121.

Non-polar molecules can have polar covalent bonds.

a)

True

b)

False

122.

The electrons in an ionic molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

123.

In a polar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

124.

Order the types of bonds based on the charge of their molecules. (lowest amount of charge to greatest)

a)

Polar Covalent --> Ionic --> Nonpolar Covalent

b)

Ionic --> Nonpolar Covalent --> Polar Covalent

c)

Ionic --> Polar Covalent --> Nonpolar Covalent

d)

Nonpolar Covalent --> Polar Covalent --> Ionic

125.

Write the formula for the ionic compound potassium oxide.

a)

KO

b)

K₃O

c)

K₂O₂

d)

K₂O

126.

What is the name of the polyatomic ionic compound NH₄NO₃?

a)

Calcium Carbonate

b)

Ammonium Nitrate

c)

Potassium Sulfate

d)

Sodium Chloride

127.

Write the formula for the polyatomic ionic compound calcium phosphate.

a)

Ca₃(PO₄)₂

b)

Ca₃(PO₄)₃

c)

Ca₂(PO₄)₃

d)

Ca(PO₄)₃

128.

What is the name of the transition metal ionic compound FeCl₃?

a)

Iron(III) chloride

b)

Ferric chloride

c)

Iron(IV) chloride

d)

Iron(II) chloride

129.

Write the formula for the transition metal ionic compound copper(II) sulfate.

a)

Cu₂SO4

b)

CuSO₄

c)

CuS₂O₄

d)

Cu₂(SO₄)₃

130.

Write the formula for the ionic compound aluminum nitride.

a)

AlNi

b)

Al₃N₂

c)

AlN

d)

Al₂N₃

131.

What is the name of the transition metal ionic compound CuSO₄?

a)

Copper(I) sulfate

b)

Copper(II) sulfate

c)

Copper(III) sulfate

d)

Copper(IV) sulfate

132.

Which of the following is the correct name for the chemical formula Ca(NO₂)₂?

a)

cadmium nitride

b)

calcium nitrate

c)

calcium nitrite

d)

cadmium nitrite

133.

Fe⁺³combines with S^-2to form

a)

Fe⁺⁴(S)^-3

b)

Fe²S⁴

c)

Fe₂S₃

d)

Fe³S²

134.

What is formula for Chromium II Bromide?

a)

ChBr

b)

Cr₂Br

c)

CrBr₂

d)

CrBr

135.

Question 1: Convert 25 liters of CO2 to moles.

a)

3.50 moles

b)

2.75 moles

c)

1.25 moles

d)

0.568 moles

136.

Question 6: Convert 3 grams of H2 to moles.

a)

0.15 moles

b)

1.5 moles

c)

0.05 moles

d)

0.5 moles

137.

What should go in the question mark spot?

$57.2\ grams\ NiS\ \times\ \frac{1\ mol}{?}=0.63\ mol$

a)

$6.02x10^{23}\ mc$

b)

1 mole

c)

90.75 grams

d)

57.2 grams

138.

How many moles are in $3.92x10^{23}$ molecules of $CaF_2$ ?

Which part of the setup is incorrect?

$3.92x10^{23}\ molecules\ \times\ \frac{1\ mole}{78.08\ g}$

a)

$3.92x10^{23}\ molecules$

b)

1 mole

c)

78.08 g

139.

How many grams are in 2.9 moles of $SiCl_4$ ? Fill in the missing information.

$2.9\ mol\ \times\ \frac{?\ grams}{1\ mole}=492.68\ g\ SiCl_4$

(a)

140.

What is the molar mass of Al₂(CO₃)₃?

a)

113.97 g/mol

b)

137.99 g/mol

c)

233.99 g/mol

d)

185.99 g/mol

141.

If you're starting with 82.21 grams of PH₃ and you want to convert to moles, what would go on the bottom of the conversion fraction?

$82.21\ grams\ \times\frac{ }{??????????????????}$

a)

1 mol

b)

33.994 grams

c)

6.02x10²³ mc

d)

82.21 grams

142.

Question 2: What is the volume in liters of 64 grams of H2O, given that one mole of any gas at STP occupies 22.4 liters?

a)

33.6 liters

b)

116.8 liters

c)

5.6 liters

d)

79.84 liters

143.

Question 9: Determine the volume in liters of 4 grams of CO2 at STP.

a)

0.0896 liters

b)

0.06 liters

c)

0.12 liters

d)

0.0045 liters

144.

How many molecules of diphosphorus pentachloride are in exactly 1 mole of P₂Cl₅?

a)

2 atoms

b)

5 atoms

c)

2 moles

d)

5 moles

e)

6.022 x 10²³ molecules

145.

Which type of particles are used for covalent (molecular) compounds?

a)

atoms

b)

molecules

c)

formula units

146.

What id the molar mass of UF₆?

a)

101 g/mol

b)

238 g/mol

c)

257 g/mol

d)

352 g/mol

147.

Which of the following dimensional analysis setups will correctly convert 27.76 g of Li to atoms of Li?

a)

A

b)

B

c)

C

d)

D

148.

Why is the mole used in chemistry?

a)

The mass of atoms is in AMUs which is too hard to convert to grams.

b)

A dozen is not a scientific amount.

c)

Chemists needed to make chemistry easier to understand.

d)

It makes counting large numbers of small particles easier.

149.

What is the molar mass of Magnesium Oxide (MgO)? Please round your answer to two decimal places with NO UNITS!

(a)

150.

How many particles is .5 moles of a substance?

a)

$3.01\ \times\ 10^{23}\ molecules$

b)

$6.02\ \times\ 10^{23}\ molecules$

c)

$8.31\ \times\ 10^{-25}\ molecules$

d)

$5.0\ \times\ 10^{22}\ molecules$

151.

How many molecules are in 84.0 g of C₅H₅N?

a)

4.00 x 10²⁷ molecules

b)

6.40 x 10²³ molecules

c)

1.10 x 10^-20 molecules

d)

5.06 x 10²⁵ molecules

Chemistry Semester Knowledge Test

Total questions: 151

Worksheet time: 4hrs 11mins

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