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Chemistry Final Review

Total questions: 160

Worksheet time: 3hrs 14mins

Name
Class
Date
1.

Which has the SHORTEST wavelength and, therefore, the highest frequency/most energy

a)

Radio waves

b)

Ultraviolet Rays

c)

Gamma Rays

d)

X-rays

2.

Which has the LONGEST wavelength and, therefore, the lowest frequency/energy

a)

Gamma Rays

b)

Radio Waves

c)

Visible Light

d)

Infrared rays

3.

How much of the electromagnetic spectrum is visible?

a)

All of it

b)

None of it

c)

Most of it

d)

Only a small part

4.

Which section of the spectrum is the ONLY one we can see?

a)

X-rays

b)

Visible Light

c)

Gamma Rays

d)

Ultraviolet Rays

5.

As the frequency of an electromagnetic wave increases, the amount of energy in that wave...

a)

increases.

b)

decreases.

c)

stays the same.

6.

How are electromagnetic waves different from other waves? 

a)

They have very short wavelengths 

b)

They transmit energy instead of matter 

c)

They can travel through empty space

d)

They can change direction by reflection 

7.

Which EM waves are have the highest energy & are the most dangerous?

a)

radio

b)

gamma rays

c)

infrared

d)

x-rays

8.

Which type of electromagnetic wave travels fastest through a vacuum?

a)

radio

b)

gamma rays

c)

visible light

d)

They all travel at the same speed.

9.
which wavelength gives you sunburn? 
a)
radio 
b)
microwaves
c)
infra red 
d)
Ultra violet 
10.

Explain the structure of the atom

a)

There is a tiny nucleus and a large electron cloud filled with empty space

b)

There is a tiny nucleus and a tiny electron cloud

c)

The nucleus is bigger than the electron cloud

d)

The electron cloud is made of protons and electrons, the nucleus has neutrons

11.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
12.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
13.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
14.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
15.
What is the highest occupied energy level?
a)
1
b)
2
c)
3
d)
4
16.

What is an orbital?

a)

An orbital is a region in an atom where there is a high probability of finding electrons.

b)

An orbital is the path that planets follow around the sun.

c)

An orbital is a type of chemical bond between atoms.

d)

An orbital is a fixed position in space where electrons are always found.

17.

What is the electron cloud?

a)

A region around the nucleus of an atom where electrons are likely to be found

b)

A type of cloud found in the Earth's atmosphere

c)

A cloud made up of protons and neutrons

d)

A cloud that forms during a chemical reaction

18.

How many electrons can the f orbital hold?

a)

12

b)

10

c)

14

d)

8

19.

How many electrons can the 1st shell hold in total?

a)

1

b)

2

c)

3

d)

4

20.

What is the most stable arrangement of electrons in an atom's electron cloud called?

a)

Electron configuration

b)

Quantum mechanical model

c)

Bohr Model

d)

Shorthand notation

21.

Electrons act like _______ in addition to particles.

a)

waves

b)

particles

c)

atoms

d)

molecules

22.

What is the Aufbau principle in electron configurations?

a)

Electrons fill the highest energy orbital first.

b)

Electrons fill the lowest energy orbital first.

c)

Electrons fill orbitals randomly.

d)

Electrons fill orbitals based on atomic number.

23.

According to Hund’s rule, orbitals of equal energy each get ___ electron(s) before any orbital gets a second pair.

a)

1

b)

2

c)

3

d)

0

24.

What does the Pauli exclusion principle state about electrons in the same atom?

a)

They can have the same set of quantum numbers.

b)

No two electrons can have the same set of quantum numbers therefore must have opposite spins

c)

Electrons must have the same spin.

d)

Electrons must occupy different orbitals.

25.
The Periodic Table of the Elements is useful for revealing patterns and trends in the elements. Which statement accurately describes a pattern in the size of atomic radii in the Periodic Table of the Elements?
a)
Atomic radii decrease from left to right across a period and decrease from top to bottom in a group.
b)
Atomic radii increase from left to right across a period and increase from top to bottom in a group.
c)
Atomic radii decrease from left to right across a period and increase from top to bottom in a group.
d)
Atomic radii increase from left to right across a period and decrease from top to bottom in a group.
26.
The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?

a)
W
b)
X
c)
Y
d)
Z
27.
Fluorine, chlorine, bromine, and iodine all have the same number of valence electrons and have a tendency to gain electrons. Which element has the greatest ionization energy and electronegativity?
a)
fluorine
b)
chlorine 
c)
bromine 
d)
iodine 
28.

Based on their locations in the periodic table, which element has chemical properties most similar to those of calcium, Ca?

a)

beryllium, Be

b)

potassium, K

c)

titanium, Ti

d)

yttrium, Y

29.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more neutrons
30.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
31.

What BEST DESCRIBES the process by which an atom or a molecule acquires a negative or positive charge by gaining or losing electrons?

a)

Polarity

b)

Affinity

c)

Ionization

d)

Discharge

32.

What BEST DESCRIBES a positively charged ion?

a)

Proton

b)

Atom

c)

Anion

d)

Cation

33.

What BEST DESCRIBES an arrangement of elements in a particular form, figure, or combination?

a)

Illusion

b)

Crystal lattice

c)

Configuration

d)

Stability

34.

Valence electrons are easier to remove when there are more inner shell electrons to weaken the attraction of the nucleus. This is called....

a)

Valence Electron Protection

b)

Electron Shielding

c)

Ionization Energy

d)

Electron Affinity

35.

Using the following table as a guide, which set of elements are organized from the lowest ionization energy to the highest?

a)

H, Na, Rb, Cs

b)

Cs, Rb, Na, H

c)

F, C, Be, Li

d)

O, S, Te, Po

36.

The distance between the center of the nucleus to the outer boundary of the highest energy level electron cloud is defined as...

a)

Atomic Radius

b)

Atomic Mass

c)

Atomic Number

d)

Electronegativity

37.

What best describes electronegativity?

a)

The shielding of valence electrons from the nucleus by inner shell electrons

b)

The amount of energy needed to remove an electron from an atom.

c)

The amount of energy released when an electron is added to an atom.

d)

A chemical property of an atom to attract electrons while bonded in a compound.

38.

Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.

a)

Decreases, increases

b)

Increases, increases

c)

Increases, decreases

d)

Stays the same, increases

39.

Which element has the highest electronegativity?

a)

Mg

b)

Al

c)

Si

d)

P

40.

Ionization energy __________ from left to right within a period and __________ from top to bottom within a group.

a)

Decreases, increases

b)

Increases, increases

c)

Increases, decreases

d)

Stays the same, increases

41.

Which element has the lowest electronegativity?

a)

Strontium

b)

Calcium

c)

Magnesium

d)

Beryllium

42.
This is a correct dot diagram for nitrogen (N)
a)
true
b)
false
43.
This is the correct dot diagram for nitrogen (N)
a)
true
b)
false
44.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
45.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
46.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
47.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
48.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
49.
What element has the valence shell configuration
3s2 3p2
a)
Al
b)
B
c)
Si
d)
Ga
50.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
51.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
52.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
53.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
54.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

55.

Which of the following is not a sublevel

a)

s

b)

p

c)

n

d)

f

e)

d

56.
Which of the following is the correct electron configuration for a carbon atom?
a)
1s2 2s2 2p6 3s2 3p2
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p2
d)
1s2 2s2 2p6 3s2 3p6 4s2 4p2
57.
Which of the following elements is a noble gas?
a)
1s2 2s2
b)
1s2 2s2 2p5
c)
1s2 2s2 2p6 3s2 3p6
d)
1s2 2s2 2p6 3s1
58.

Typically, atoms are more stable when they are

a)

bonded together

b)

apart from each other

59.

A single covalent bond involves the sharing of

a)

only one electron.

b)

two electrons.

c)

three electrons.

d)

a variable number of electrons, which depends on the bonding atoms.

60.

The measure of an atom’s ability to attract electrons is its

a)

electronegativity

b)

polarization.

c)

ionization

d)

electron affinity

61.

Atoms that are bonded with an electronegativity difference of 0 to 0.3 are generally considered to be

a)

negatively charged compounds.

b)

nonpolar-covalent compounds.

c)

polar-covalent compounds.

d)

ionic compounds.

62.

When an atom completely gives up its valence electrons to another atom, they form a bond that is considered to be

a)

purely ionic.

b)

partially ionic.

c)

polar-covalent.

d)

nonpolar-covalent.

63.

You can estimate the degree to which a bond between two atoms is ionic or covalent by calculating the

a)

distance between the atoms’ nuclei.

b)

difference in the atoms’ electronegativities.

c)

atoms’ atomic radii.

d)

number of atoms in the compound.

64.

An ionic bond results from the electrical attraction between

a)

a cation and an anion

b)

two anions

c)

two cations

d)

three or more cations and neutral molecules

65.

What is transferred in an ionic bond?

a)

proton

b)

electron

c)

neutron

d)

energy level

66.

Covalent bonds result from two or more atoms

a)

combining their nucleii

b)

combining their inner electron shells

c)

transfer all valence electrons

d)

sharing valence electrons to achieve an octet

67.

The EN of Fluorine is 4.0; the EN of Cesium is 0.7; what is the EN difference?

a)

3.3

b)

4.7

c)

there is no difference

d)

0.33

68.

Usually a _________ bond forms between metals and non metals.

a)

covalent

b)

coordinate covalent

c)

metallic

d)

ionic

69.

Usually a ___________ bond forms between two or more nonmetals.

a)

covalent

b)

ionic

c)

coordinate covalent

d)

metallic

70.

The type of bonding one would expect to occur between atoms in a 14K gold ring would be

a)

ionic

b)

covalent

c)

metallic

d)

coordinate coordinate bond

71.

Which term best matches the following definition?

Definition: the tendency of an atom to prefer to have a full valence shell.

a)

Octet Rule

b)

Valence Shell

c)

Molecule

d)

Compound

e)

Chemical Bond

72.

Which type of bonding does the image best represent?

a)

Ionic

b)

Covalent

c)

Metallic

73.

Which type of bonding does the image best represent?

a)

Ionic

b)

Covalent

c)

Metallic

74.

Which type of bonding does the gif best represent?

a)

Ionic

b)

Covalent

c)

Metallic

75.

What type of bonding is present in an Iron nail (made of Fe atoms)?

a)

Metallic

b)

Covalent

c)

Ionic

76.

What type of bonding is present in an silver ring nail (made of Ag atoms)?

a)

Metallic

b)

Covalent

c)

Ionic

77.

What type of bonding in carbon dioxide (made of molecules containing CO2)?

a)

Metallic

b)

Covalent

c)

Ionic

78.

What type of bonding in ozone (made of molecules containing O3)?

a)

Metallic

b)

Covalent

c)

Ionic

79.

What type of bonding in sodium fluoride (made of the compound containing NaF)?

a)

Metallic

b)

Covalent

c)

Ionic

80.

What type of bonding in magnesium cloride (made of the compound containing MgCl2)?

a)

Metallic

b)

Covalent

c)

Ionic

81.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

82.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

83.
H2O
a)
Polar 
b)
Nonpolar 
84.

Which bond involves an unequal sharing of electrons?

a)

Ionic bond

b)

Nonpolar covalent bond

c)

Polar covalent bond

d)

Metallic bond

85.

True or False: The smaller the difference in electronegativity, the more polar the bond

a)

True

b)

False

86.
Electronegativity is the...
a)
energy needed to remove the outermost electron.
b)
ability of an atom to attract electrons from another atom.
87.
Which of these statements describes the basic idea of the Valence Shell Electron Pair Repulsion (VSEPR) theory?
a)
There is always an octet of electrons around an atom in a molecule.
b)
Shared and unshared electron pairs repel each other as much as possible.
c)
Electrons are attracted to the nucleus of the central atom.
d)
Molecules repel one another due to intermolecular forces.
88.
The name of FeCl₂ is
a)
iron chloride
b)
iron (II) chloride
c)
iron (I) chloride
d)
iron dichloride
89.
What is the correct name for P₃Cl₆?
a)
Potassium chloride
b)
Phosphorous chloride
c)
Triphosphorous hexachloride
d)
Tetraphosphorous heptachloride
90.
What is the correct formula for dinitrogen tetroxide?
a)
N₃O₃
b)
(N₂)₂(O₄)₃
c)
N₂O₄
d)
N₄O₂
91.
What is the correct name for SO₂?
a)
Sulfur oxide
b)
Sulfite
c)
Sulfur dioxide
d)
Sulfur II Oxide
92.

What is the charge on the nitrogen in: NaN3

a)

1+

b)

1-

c)

3+

d)

3-

e)

None of these.

93.

Name the following compound: Zn3N2

a)

zinc nitride

b)

trizinc dinitride

c)

zinc (III) nitride

d)

zinc (II) nitide

e)

zinc nitrogen

94.
calcium phosphate
a)
CaPO4
b)
Ca2(PO4)3
c)
Ca3PO4
d)
Ca3(PO4)2
95.
barium hydroxide
a)
Ba(OH)2
b)
Ba2OH
c)
BaOH
d)
Ba2OH
96.
Fe(NO3)2
a)
iron nitrate
b)
iron dinitrate
c)
iron(II) nitrate
d)
iron(I) nitrate
97.
What is the name of C3Cl8 ?
a)
Carbon octachloride
b)
Tricarbon octachloride
c)
Carbon trichloride
d)
Octacarbon trichloride
98.
write the formula of the compound formed between elements below:
Be     F
a)
BeF2
b)
Be2F
c)
BeF
d)
F2Be
99.
write the formula of the compound formed between elements below:
Ca   NO2
a)
Ca(NO2)2
b)
Ca(NO2)
c)
CaNO2 2
d)
CaNO2
100.
write the name for the following compound:
(NH4)3PO4
a)
ammonium phosphate
b)
ammonium phosphite
c)
ammonium phosphide
d)
triammonium phosphite
101.
The name of Cu₃N₂ is
a)
copper (III) nitride
b)
copper (II) nitride
c)
copper nitride
d)
tricopper dinitride
102.

What is the correct formula for the compound calcium carbide?

a)

CaC

b)

Ca2C

c)

CaC2

d)

Ca2C4

103.
Name the following ionic compound: LiNO3
a)
lithium nitrate
b)
lithium III nitrate
c)
lithium nitride
d)
lithium oxide
104.

Name the following compound: AlCl3

a)

aluminum chlorine

b)

aluminum trichloride

c)

aluminum chloride

d)

aluminum (III) chloride

e)

None of these.

105.

Name the following compound: Na2S

a)

sodium sulfide

b)

disodium sulfide

c)

sodium sulfur

d)

sodium monosulfide

e)

None of these.

106.

Name the following compound: CuCl2

a)

copper chlorine

b)

copper (I) chloride

c)

copper (II) chloride

d)

copper dichloride

e)

None of these.

107.

What is the formula for: magnesium sulfide

a)

MgS

b)

Mg2S2

c)

MnS

d)

MgS2

e)

None of these.

108.

What is the formula for: silver oxide

a)

AgO2

b)

AgO

c)

Ag2O

d)

SiO2

e)

None of these.

109.

What is the formula for: aluminum phosphide

a)

AlP

b)

AlP3

c)

Al3P3

d)

Al3P2

e)

None of these.

110.

What is the formula for: potassium fluoride

a)

KF

b)

KFl

c)

K2F2

d)

K2F

e)

None of these.

111.

What is the formula for: tin (II) bromide

a)

SnBr2

b)

SnBr

c)

Sn2Br

d)

TiBr2

e)

None of these.

112.
What is the name of Ca(NO3)2
a)
calcium nitrite
b)
calcium II nitrate
c)
calcium nitrate
d)
carbon nitrate
113.
What is the name of the compound with the formula FePO4?
a)
iron phosphate
b)
iron (II) phosphate
c)
iron (IV) phosphate
d)
iron (III) phosphate
114.
True or False
In a chemical reaction, no new atoms are created, and no atoms are destroyed. 
a)
true
b)
false
115.
The left side of the equation below is called
a)
Products
b)
Reactants
116.
The right side of the equation below is called the
a)
products
b)
reactants
117.
A number in front of a chemical formula in an equation that indicates how many molecules or atoms of each reactant and product are involved in a reaction.
a)
Coefficient
b)
reactant
c)
subscript
d)
product 
118.
Which of the following answers will balance the equation below?
__K + __Br2 --> __KBr
a)
2, 1, 1
b)
2, 3, 2
c)
2, 1, 2
d)
1, 2, 3
119.
If the reactants on the left side of a chemical equation are C₃H₈ + 5O₂, the products in a balanced equation could be
a)
4CO₂ + 3H₂O
b)
3CO₂ + 4H₂O
c)
2CO₂ + 3H₂O
d)
3CO + 4H₂O
120.
Which of the following options correctly balances the equation below?
__HNO2 + __O2 --> __HNO3
a)
4, 1, 4
b)
1, 2, 1
c)
1, 2, 1
d)
2, 1, 2
121.

How many Carbons are present on the reactant side?

a)

1

b)

2

c)

3

d)

4

122.

How many Hydrogens are on the product side of this chemical equation?

a)

1

b)

2

c)

3

d)

4

123.

Is this chemical equation balanced? Why or why not? Choose the BEST answer.

a)

Yes, the amount of atoms for each element are equal on both the reactant and product side.

b)

No, the carbons are not the same number on both the reactant and product side.

c)

No, neither the carbons or hydrogens are the same amount on both the reactant and product side.

d)

No, none of the elements (carbon, hydrogen, or oxygen) are the same amount on both the reactant and product side.

124.
Number of C's in 2Na₂CO₃
a)
1
b)
2
c)
3
d)
5
125.
Which of the following shows the correct way to balance the chemical equation?
Fe + O2 -> Fe2O3
a)
4Fe + 3O2 -> 2Fe2O3
b)
2 Fe + 3O2 -> Fe2O6
c)
4 Fe + O6 -> 2Fe2O3
d)
None of the options are correctly balanced.
126.
Balance this equation,            
Al2O3 --> Al + O2 
a)
Cannot be balanced
b)
2Al2O3 --> 2Al+3O2 
c)
2Al2O3--> 4Al+3O2 
d)
3Al2O3--> 2Al+O2 
127.
Coal contains carbon and other elements. Carbon dioxide forms when coal burns in the presence of oxygen. Which of these is the best evidence that a chemical reaction occurs when coal burns?
a)
The shape of the coal changes
b)
Oxygen is present
c)
A new substance is produced
d)
Coal is made up of more than one element
128.
Is burning wood a chemical or physical change?
a)
chemical
b)
physical
129.
Is glass breaking a chemical or phyiscal change?
a)
chemical
b)
physical
130.
CxHy +O2 --> H2O + CO2
a)
Decomposition
b)
Double replacement
c)
Combustion
d)
Single Replacement
131.
One reactant into several products.
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
132.
One element replaces another in a compound.
a)
Synthesis
b)
Combustion
c)
Single Replacement
d)
Double Replacement
133.
This pictures simulates what type of reaction?
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
134.
KOH + H3PO4 --> K3PO4 + H2O
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
135.
Si + S8 --> Si2S4
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
136.
Pb(NO3)2 --> PbO + NO2 + O2
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Combustion
137.

3 Pb + 2 H3PO4 ----> 3 H2 + 1 Pb3(PO4)2

a)

Synthesis (or combination)

b)

Decomposition

c)

Single replacement

d)

Double replacement

138.

Combustion reactions will always involve

a)

Oxygen and a solid

b)

Liquid nitrogen and heat

c)

Oxygen and heat/energy

d)

CO and H2O

139.

Which type of chemical reaction has the following configuration?


Hydrocarbon + Oxygen --> Carbon Dioxide + Water


CxHy + O2 --> CO2 + H2O

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

140.

What type of chemical reaction has the following configuration?


Compound --> Substance + Substance


AB --> A + B

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

141.

Select each compound that can be produced by combustion reactions. (more than 1 answer)

a)

Oxygen

b)

Carbon Dioxide

c)

Water

d)

Glucose

e)

Carbon

142.

Classify the following chemical reaction


BaCl2(aq) + K2CrO4(aq) --> BaCrO4(s) + 2KCl(aq)




a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

143.

Classify the following chemical reaction.


Si(s) + 2Cl2(g) --> SiCl4(l)

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

144.

Classify the follow chemical reaction.


2C6H6(l) + 15O2 --> 6H2O(l) + 12CO2(g)

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

145.

What type of chemical reaction is when a single compound is broken down into two or more products?

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

146.

Identify the type of chemical reaction picture above

a)

Composition/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

147.
What is the molar mass of NaOH?
a)
40 g/mol
b)
38.989 g/mol
c)
23.998 g/mol
d)
57.004 g/mol
148.
What is the molar mass of AuCl3?
a)
96 g
b)
130 g
c)
232.5 g
d)
303.3 g
149.
How many molecules of sugar (C6H12O6) are in a mole?
a)
24 molecules
b)
180 molecules
c)
180 g
d)
6.02 x 1023 molecules
150.
What is the mass of 0.89 mol of CaCl2?
a)
111 grams
b)
0.008 grams
c)
98.9 grams
d)
none of the choices
151.
Which conversion factor should be used for the following question " How many molecules are there in 4.00 moles of glucose, C6H12O6? 
a)
1 mole = 78.12 g
b)
1 mole = 22.4 L 
c)
1 mol = 6.02x 1023 particles 
d)
more than one
152.

How many moles are in 19.82 g Mg? 

Mg= 24.31g

a)
1.226mol Mg
b)

481.82 mol Mg

c)

1.00mol Mg

d)

 0.815 mol Mg

153.

Determine the molar mass for carbon tetrachoride (CCl4)

C= 12.01g

Cl=35.45g

a)

153.81 g/mol

b)

141.8 g/mol

c)

189.35 g/mol

d)

47.46 g/mol

154.

What is the mass in grams of 2.3456 moles of W?

W= 183.84

a)

431.22 grams

b)

6.02 grams

c)

207.2 grams

d)

486.01 grams

155.

How many moles are in 1459 grams of Na?

Na= 22.99g

a)

63.46 moles

b)

60.36 moles

c)

10 moles

d)

1 mole

156.

What is the molar mass of Aluminum Sulfide?

Al= 26.98

S=32.07

a)

150.17 g/mol

b)

59.05 g/mol

c)

138.23 g/mol

d)

75.27 g/mol

157.

How many grams are in 0.523 mol of AlPO4?

a)

63.78 g

b)

38.68 g

c)

47.23 g

d)

55.43 g

158.

How many moles are in 100 g of carbon dioxide, CO2?

a)

2.27 mol

b)

2.36 mol

c)

3.51 mol

d)

1.49 mol

159.

Find the molar mass for NaOH

The following is the Atomic Mass from the Period Table

Na= 22.99g

O=16g

H=1.01g

a)

40 g

b)

40 moles

c)

17 g

d)

17 moles

160.

When looking for Molar mass, where do you look for the Atomic Mass?

a)

Periodic Table

b)

Guess

c)

6.02 X 1023

d)

The Mole

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