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Chemistry Final Exam Review

Total questions: 270

Worksheet time: 5hrs 57mins

Name
Class
Date
1.

(a)   is the study of the composition, structure, and properties of matter.

2.

(a)   are the building blocks of all things. They are the smallest unit of an element that retains the identity and properties of that element.

3.

Chemistry is a ____________________ science.

a)

physical

b)

social-behavioral

c)

political

d)

pseudo

4.

(a)   chemistry is the study of most carbon-containing compounds.

5.

(a)   is the study of the processes and substances occurring in living things.

6.

A (a)   is any substance with a definite composition.

7.

(a)   is research performed for the sake of knowledge itself.

8.

(a)   is the use of applied and basic research to produce goods for consumer use.

9.

All matter has ________________ and _____________________.

a)

mass

b)

volume

c)

color

d)

weight

e)

scent

10.

A(n) ______________________ cannot be broken down into smaller, stable parts.

a)

element

b)

compound

c)

molecule

d)

chemical

11.

A (a)   can be broken down into smaller, stable parts.

12.

A (a)   mixture is made when substances are evenly distributed throughout the mixture.

13.

(a)   properties are dependent on the amount of the substance present.

14.

__________________________ properties are related to the ability of a substance to undergo change.

a)

chemical

b)

physical

15.

Ice melting into water is an example of a...

a)

physical change

b)

chemical change

16.

Matter in the (a)   state has definite shape and definite volume.

17.

Matter in the (a)   state is in a high energy state where it has lost its electrons.

18.

Wood burning is an example of a _____________________ change.

a)

chemical

b)

physical

19.

All pure substances are ____________________.

a)

heterogeneous

b)

homogeneous

20.

What is the atomic number of Nitrogen?

(a)  

21.

I hand you a substance which is lustrous and conducts heat very well. What is it?

a)

A metal

b)

A nonmetal

c)

A metalloid

d)

A noble gas

22.

I show you a substance that does not react with other substances. What is it?

a)

A noble gas

b)

a metal

c)

a metalloid

d)

a nonmetal

23.

Group 18 elements are called (a)   gases.

24.

Malleability is a characteristic of (a)   .

25.

Starting substances in a reaction are called...

(a)  

26.

Factors in an experiment that do not change are called ______________________.

a)

controls

b)

variables

c)

experimental

d)

globular

27.

Once enough data is collected to back up a hypothesis, with rigorous testing and repeated confirmation of the hypothesis, the hypothesis becomes a _________________.

a)

theory

b)

law

c)

textbook

d)

discipline

28.

Mass is how much stuff is present. ____________________ is how much gravitational force acts on that matter.

a)

weight

b)

volume

c)

density

d)

terminal velocity

29.

Convert:

81 kg to grams

(a)  

30.

Convert:

22 mg to grams

(a)  

31.

_____________________ refers to the closeness of measures to the accepted value.

a)

accuracy

b)

precision

32.

Write 2.5×1072.5\times10^7 in expanded form.



(a)  

33.

8.2×10n=82 000 000 000 0008.2\times10^n=82\ 000\ 000\ 000\ 000 .
What is n?

(a)  

34.

(2.8×105)+(1.5×106)\left(2.8\times10^5\right)+\left(1.5\times10^6\right)  

a)

1.78×1061.78\times10^6  

b)

4.4×1054.4\times10^5  

c)

1.78×10−61.78\times10^{-6}  

d)

4.4×10114.4\times10^{11}  

35.

(3.1×104)×(2.8×106)\left(3.1\times10^4\right)\times\left(2.8\times10^6\right)  

a)

8.68×10108.68\times10^{10}  

b)

8.68×1028.68\times10^2  

c)

5.9×10105.9\times10^{10}  

d)

2.83×1062.83\times10^6  

36.

The SI Unit for temperature is...

(a)  

37.

The first step in the scientific method is to...

a)

ask a question

b)

form a hypothesis

c)

make an observation

d)

perform an experiment

38.

A testable statement is called a...

(a)  

39.

A theory explains why a phenomenon happens, whereas a

__________________ describes the phenomenon.

a)

law

b)

hypothesis

c)

guess

d)

postulate

40.

True or False:

The Imperial System is the system scientists use to communicate measurements.

a)

True

b)

False

41.

(a)   data is descriptive and tells the characteristics of the system we are studying.

42.

(a)   are often used to communicate theories, explaining how a phenomenon works and how data or events are related.

43.

(a)   are the SI unit for the intensity of light.

44.

(a)   is a derived unit of length, width, and height multiplied together.

45.

(a)   is a derived SI unit with mass divided by volume.

46.

First person to propose the concept of an atom

a)

Rutherford

b)

Democritus

c)

Dalton

d)

Bohr

47.

These particles are found in the nucleus

a)

protons and electrons

b)

nucleus and neutrons

c)

protons and neutrons

d)

electrons and neutrons

48.

Rutherford experimented with ____

a)

Gold foil and alpha particles

b)

Cathode rays and alpha particles

c)

electron and alpha particles

d)

gold foil and cathode rays

49.

Thomson Experimented with ______

a)

Gold Foil

b)

alpha particles

c)

cathode rays

d)

protons

50.
Which scientist developed the atomic theory?
a)
JJ Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
James Chadwick
51.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

52.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
53.
Subatomic particles that are neutral in charge
a)
Neutrons
b)
Protons
c)
Nucleus 
d)
Electrons
54.
Where electrons are likely to be found as they travel around the nucleus
a)
Nucleus
b)
Electron Cloud
c)
Within a Proton
d)
Within a Neutron
55.

John Dalton stated:

a)

Atoms are tiny, invisible particles.

b)

Atoms of one element are all the same.

c)

Atoms of different elements are different.

d)

Compounds form by combining atoms.

e)

All of the statements listed.

56.

What is the smallest unit of matter? It is composed of protons and neutrons, held together in the nucleus, and electrons around the nucleus in different electron orbitals, which form an electron cloud.

a)

cell

b)

nucleus

c)

atom

d)

electron

57.

What is the number of protons in the nucleus of an atom that determines the chemical properties of an atom?

a)

mass number

b)

atomic mass

c)

atomic number

d)

atomic symbol

58.

What is the mass number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons and electrons in the atom

59.

Protium, Deuterium and Tritium are isotopes of the element Hydrogen.


Why does Tritium have a greater mass number than both Protium and Deuterium?

a)

It has more protons

b)

It has more neutrons

c)

It is electrically neutral

d)

It has more electrons

60.

What is the mass number of an atom that contains 9 protons, 10 neutrons, and 9 electrons?

a)

9

b)

10

c)

18

d)

19

61.

What is true about the carbon atom depicted in the image?

a)

This carbon atom has 13 protons

b)

There are 13 subatomic particles in the electron cloud

c)

The mass number of this carbon atom is 13

d)

The atomic number of this carbon atom is 13

62.

All the isotopes of a particular element will always have the same -

a)

Atomic number

b)

Mass number

c)

Number of neutrons

d)

Total number of subatomic particles

63.

These three isotopes of carbon have different -

a)

Atomic numbers

b)

Mass numbers

c)

Numbers of protons

d)

Symbols

64.
How many molecules are in 2.5 mol of NaCl?
a)
1.51x1023
b)
146
c)
4.15
d)
1.51x1024
65.
What is the mass of one mole of aluminum?
a)
26.982 g
b)
13 g
c)
53.985 g
d)
14 g
66.
How many moles are in 16.94g of water?
a)
16.94
b)
0.9403
c)
305.2
d)
1.063
67.
What is Avogadro's Number?
a)
6 x 1023
b)
6 x 103
c)
600
d)
6.0
68.
How many moles are in 6 x 1023 molecules of H2O?
a)
1
b)
2
c)
6
d)
600
69.

The mass of one mole of an element is equal to

a)

its atomic number from the periodic table, but in amus.

b)

its atomic mass from the periodic table, but in amus.

c)

its atomic mass from the periodic table, but in grams.

d)

its atomic number from the periodic table, but in grams.

70.

What is the mass of 1.2 x 1024 atoms of C?

a)

2.0 grams

b)

24 grams

c)

0.17 grams

d)

1.4 x 1025 grams

71.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
72.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
73.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the there should only be 1 orbital in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
74.
The blue section of the wave is measuring _________________.
a)
wavelength
b)
crest
c)
trough
d)
amplitude 
75.

Electrons fill energy levels and sublevels _____ in energy first.

a)

lower

b)

higher

76.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
77.
How many valence electrons does phosphorus have?
a)
5
b)
2
c)
8
d)
15
78.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
79.

Which shows the correct orbital diagram for Cobalt?

a)
b)
c)
d)
80.

What element's orbital notation is pictured here?

a)

Ar

b)

Br

c)

Cu

d)

Cl

81.
Which letter represents wavelength?
a)
A
b)
B
c)
C
d)
D
82.
Which wave has a greater frequency?
a)
A
b)
B
83.

If a wave has a greater frequency, what happens to the wavelength?

a)

increases

b)

decreases

c)

stays the same

84.

If a wave has a greater frequency, what happens to number of waves per second?

a)

increases

b)

decreases

c)

stays the same

85.

What property does the orange arrow (A) represent?

a)

Crest

b)

Trough

c)

Wavelength

86.

What property does the green arrow (B) represent?

a)

Crest

b)

Trough

c)

Wavelength

87.
In a vacuum, all electromagnetic waves have the same
a)
wavelength
b)
frequency
c)
speed
d)
amplitude
88.
which of the following does NOT belong in the electromagnetic spectrum:
a)
X-ray
b)
sound wave
c)
ultra violet rays
d)
microwaves
89.
The distance from one point to the next corresponding point on a wave is called the ________________.
a)
waveform
b)
peak
c)
amplitude
d)
wavelength
90.
Which kind of wave has the greatest frequency?
a)
gamma rays
b)
infrared
c)
ultraviolet
d)
microwaves
91.

What model of the atom replaced Bohr's model?

a)

Heisenberg's model

b)

Thomson's model

c)

Rutherford's model

d)

Quantum Mechanical model

92.

Who proposed that electrons are only found in specific, discrete circular orbits around the nucleus?

a)

Albert Einstein

b)

Erwin Schrodinger

c)

Ernest Rutherford

d)

Niels Bohr

93.

Who used theoretical calculations and experimental results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom?

a)

JJ Thomson

b)

Niels Bohr

c)

Erwin Schrodinger

d)

James Chadwick

94.

If n = 3, what is the maximum number of electrons that can fit in this shell?

a)

2

b)

8

c)

18

d)

32

95.

How many d orbitals make up the d subshell?

a)

1

b)

5

c)

3

d)

7

96.

What orbital is shown in the picture?

a)

s orbital

b)

p orbital

c)

d orbital

d)

f orbital

97.

What is the difference in a 1s orbital and a 2s orbital?

a)

The shape of the orbital

b)

The size of the orbital

c)

The number of electrons it can hold

d)

None of the above

98.

Which quantum number represents the shape of the orbital?

a)

principal quantum number

b)

azimuthal (angular momentum) quantum number

c)

magnetic quantum number

d)

spin quantum number

99.

What states that every orbital of a subshell must be singly occupied before any orbital can have a pair?

a)

Pauli exclusion principle

b)

Hund's rule

c)

Aufbau principle

d)

None of the above

100.

This states that no two electrons will have the same 4 quantum numbers in an atom or molecule. The two electrons of the same orbital must have opposite spin states.

a)

Pauli exclusion principle

b)

Hund's rule

c)

Aufbau principle

d)

None of the above

101.

What states that electrons fill the lowest energy orbitals/levels first before occupying higher energy levels?

a)

Pauli exclusion principle

b)

Hund's rule

c)

Aufbau Principle

d)

None of the above

102.

How many electrons can be held in the first energy level?

a)

2

b)

8

c)

6

d)

10

103.

How many energy levels are currently present on the periodic table?

a)

18

b)

7

c)

6

d)

4

104.

How many orbitals are there in a p-sublevel?

a)

1

b)

3

c)

5

d)

7

105.

What sublevels are present in the 5th energy level of an atom?

a)

s

b)

p and d

c)

d and f

d)

s p and d

e)

s p d and f

106.

How many orbitals are there in a d-sublevel?

a)

10

b)

6

c)

3

d)

5

107.

Magnesium is placed in the ____ energy level on the periodic table.

a)

1st

b)

5th

c)

3rd

d)

24th

e)

12th

108.

The area on the far right of the periodic table is known as the ____ block.

a)

s

b)

p

c)

d

d)

f

109.

The f-block on the periodic table can hold ___ elements.

a)

3

b)

6

c)

18

d)

14

e)

10

110.

Which sublevels are present in n=3?

a)

s

b)

s and p

c)

s and d

d)

s p d and f

e)

s p and d

111.

How many total electrons can fit in the d-sublevel?

a)

2

b)

18

c)

10

d)

14

112.

How many atoms are in a single row of the p-block of the periodic table?

a)

1

b)

3

c)

10

d)

5

e)

6

113.

Electrons prefer to be in...

a)

third energy level

b)

highest energy level

c)

2nd energy level

d)

lowest possible energy level

114.

How many electrons could fit in a HALF full d-sublevel?

a)

2

b)

10

c)

5

d)

6

115.

Bohr's model of the atom is sometimes called the planetary model. If the atoms is like a solar system, what is analogous to the sun?

a)

energy levels

b)

electrons

c)

neutrons

d)

the nucleus

116.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

117.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
118.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
119.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
120.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
121.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
122.

I am a metal


I am in group 2


I am in period 6


I am…

a)

Mo

b)

Re

c)

S

d)

Ba

123.

I am a nonmetal


I am in period 2


I am in group 16/6A

a)

Ba

b)

Si

c)

Ba

d)

O

124.

Find an element with similar chemical properties to Barium (Ba).

a)

Ca an Ra, because they are in the same group and have similar chemical properties.

b)

Cs and La, b/c they are in the same period number.

c)

Ca and Y, b/c they are 90 degree angle and have similiar properties.

125.
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.
126.
_______________ developed the first periodic table and arranged the elements in order of increasing atomic mass.
a)
Stevie Wonder
b)
Sasha Vujacic
c)
Dmitri Mendeleev
d)
James Mosely
127.
Mendeleev classified elements based on not only atomic mass but what else?                                                   
a)
reactivity
b)
boiling points
c)
physical properties only 
d)
 chemical & physical properties
128.
What does the 6 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
129.
What does 12.011 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
130.
What does the C represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
131.

Periodic law states that the elements are arranged according to their atomic ________ so that elements with similar chemical properties are in the same ________ and properties repeat periodically.

a)

numbers, rows

b)

masses, rows

c)

masses, column

d)

numbers, column

132.

Which element is found in group 2, period 6?

a)

Oxygen (O)

b)

Barium (Ba)

c)

Selenium (Se)

d)

Carbon (C)

133.

Which halogen is found in period 4?

a)

Krypton (Kr)

b)

Xenon (Xe)

c)

Bromine (Br)

d)

Iodine (I)

134.

Which element has similar chemical properties as sodium but has 7 energy levels?

a)

Francium (Fr)

b)

Cesium (Cs)

c)

Rubidium (Rb)

d)

Potassium (K)

135.

Find these groups: Locate Lanthanides and Actinides.

a)
b)
c)
d)
136.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
137.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
138.
Electronegativity is...
a)
the ability of an atom to attract/ accept electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
139.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
140.
Cations are...
a)
Positive
b)
Negative
c)
Neutral
d)
Purring
141.
Anions are...
a)
Positive
b)
Negative
c)
Neutral
d)
Crying
142.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
143.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
144.
Which particles change the charge in atoms when ions are formed?
a)
Protons
b)
Electrons
c)
Neutrons
d)
Kittens
145.
How many total electrons does Mg+2 (a magnesium ion) have?
a)
10
b)
12
c)
14
d)
22
146.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
147.
What do we call a covalent bond where electrons are shared UNEVENLY or UNEQUALLY?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
148.
What type of bond is shown in this image?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
149.
Are the atoms more stable when they are bonded together or when they are apart? 
a)
Bonded Together
b)
Apart
150.

What is it called if there are three-pairs of electrons being shared?

a)

Triple Bond

b)

Three Single Bonds

c)

Tribond

d)

Double and Single Bond Combo

151.
How many electrons are shared in a double bond?
a)
2
b)
4
c)
6
d)
8
152.
Ionic bonds form between two ions that have...
a)
ionic compounds
b)
negative charges
c)
positive charges
d)
opposite charges
153.

Anions

a)

Gain electrons, has an overall positive charge

b)

Lose electrons, has an overall positive charge

c)

Lose electrons, has an overall negative charge

d)

Gain electrons, has an overall negative charge

154.

Cations

a)

Gain electrons, has an overall positive charge

b)

Lose electrons, has an overall positive charge

c)

Lose electrons, has an overall negative charge

d)

Gain electrons, has an overall negative charge

155.

When an ionic bond is formed, electrons are _____.

a)

gained

b)

lost

c)

shared

d)

gained or lost

156.

How many valence electrons do MOST atoms need to be stable?

a)

123

b)

8

c)

as many as there are protons

157.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
158.
What elements have zero electronegativity?
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
159.

Which bond shares electrons evenly?

a)

non polar Covalent

b)

Polar Covalent

c)

Ionic

160.

What does the word "polar" refer to?

a)

together, mutually, in common

b)

valence electrons

c)

an atom or molecule with a net electric charge due to the loss or gain of one or more electrons.

d)

To have a positive and negative end like a magnet

161.

The difference in electronegativity affects the type of bond will be formed. What type of bond would be formed with a difference of 0.3?

a)

Covalent

b)

Polar Covalent

c)

Ionic

162.

The difference in electronegativity affects the type of bond will be formed. What type of bond would be formed with a difference of 2.0?

a)

Covalent

b)

Polar Covalent

c)

Ionic

163.

A metallic bond is a bond between ________.

a)

nonmetals

b)

metals

c)

transition metals

d)

metalloids

164.

Which of the following is NOT a property of metals?

a)

Hard

b)

Can conduct electricity

c)

Very brittle (breaks easily)

d)

Malleable (can bend without breaking)

165.

What is meant by the term "sea of electrons"?

a)

It's what we call all the free floating electrons in a metal.

b)

It's what we call electrons that are floating in a liquid.

c)

It's the total number of electrons in a metal atom.

d)

It's the total number of electrons in the ocean.

166.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Linear
167.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
168.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
169.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
170.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
171.
What does the Roman Numeral in the name of a multivalent compound represent?
a)
the charge on the anion
b)
the charge on the cation
c)
the number of cations
d)
the number of metal ions
172.
What type of compound is Ca3N2?
a)
covalent
b)
simple ionic
c)
polyatomic ionic
d)
multivalent ionic
173.
Carbon monoxide is a deadly gas produced from incomplete combustion. What type of compound is it?
a)
covalent
b)
simple ionic
c)
polyatomic ionic
d)
multivalent ionic
174.
What type of compound is KNO3?
a)
covalent
b)
simple ionic
c)
polyatomic ionic
d)
multivalent ionic
175.

What is the name of CuCl2?

a)

copper (II) chloride

b)

copper chloride

c)

copper monochloride

d)

copper (I) chloride

176.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
177.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
178.
What is the name of Br6F10 ?
a)
Bromium fluoride
b)
Hexabromine fluoride
c)
Bromium decafluoride
d)
none of the above
179.

What is the mass in grams of 5.90 mol octane (C8H18)?

a)

673 g

b)

0.0512 g

c)

389 g

d)

E) 3.55 x 1024 g

180.
How many moles are present in 32.3 grams of carbon dioxide (CO2)?
a)
44.01 moles
b)
1421.52 moles
c)
32.3 moles
d)
0.73 moles
181.

What is the oxidation state of Cl in ClO- ?

a)

0

b)

+1

c)

-1

d)

+2

182.

What is the oxidation state of Pb in PbO ?

a)

+2

b)

+4

c)

0

d)

-2

183.

S in HSO4- ?

a)

+5

b)

-6

c)

+6

d)

+2

184.

What is the oxidation state of Cu in Cu2+?

a)

-1

b)

-2

c)

+2

d)

0

185.

What is the molar mass of PbSO4?

a)

303.27 g/mol

b)

255.27 g/mol

c)

163.87 g/mol

d)

372.27 g/mol

186.

Shivani measures out 6.0 moles of epsom salt (MgSO4) to put in her bath. How many grams of MgSO4 went in the bath?

a)

3.6 x 1024 g

b)

720 g

c)

0.050 g

d)

340 g

187.

Determine the mass of 4.20 moles of C6H12

a)

353 g

b)

0.0499 g

c)

337 g

d)

2.53 x 1024 g

188.

How many moles are in 98.3 grams of aluminum hydroxide, Al(OH)3?

a)

1.26 moles

b)

0.8 moles

c)

7,670 moles

d)

1.63 x 10-22 moles

189.

What is the molar mass of table salt (NaCl)? Read all options! Be careful!

a)

58.44 amu

b)

35.45 g/mol

c)

22.99 g/mol

d)

58.44 g/mol

190.
What is Avogadro's Number? 
a)
6.02 x 1023
b)
- 6.02 1023
c)
6.02 x 1022
d)
6,020,000,000,000
191.

Formula mass of CO2

a)

44g/mol

b)

44 amu

c)

28g/mol

d)
28g
192.
Formula mass of KBr
a)
119
b)
117g
c)
54
d)
62g
193.

What is the percent by mass of magnesium in MgO?

a)

20%

b)

40%

c)

50%

d)

60%

194.

What is the percent by mass of fluorine in CaF2 (gram-formula mass = 78 g/mol)?

a)

24%

b)

49%

c)

49%

d)

65%

195.
How many atoms of iodine are in a mole of iodine?
a)
53
b)
63.55g
c)
126.9
d)
6.02 x 1023
196.
What coefficient should be used to make the following equation balanced?
N2+O2--> _NO 
a)
1
b)
2
c)
3
d)
4
197.

Which equation is balanced?

a)

PbO2 + 2H2

b)

SO2 + H20 --> H2SO4

c)

2Na + 2H2O --> 2NaOH + H2

198.
How many HCl molecules do you need to balance this equation? 
Mg +  __HCl --->  MgCl2 + H2
a)
1
b)
2
c)
3
d)
4
199.

What law governs the balancing of chemical equations?

a)

Law of Energy

b)

Law of Conservation of Matter/Mass

c)

Law of Gravity

d)

Law of Matter Movement

200.

Balance this equation

_Al +_HCl --> _H2 +_AlCl3

a)

2,6,3,2

b)

it's already balanced

c)

4,12,3,4

d)

2,1,4,5

201.

What are the coefficients that would properly balance this equation?

__Ca + __H2O --> __Ca(OH)2 + __H2

a)

2,1 --> 2,1

b)

1,2 --> 1,1

c)

1,2 --> 2,4

d)

1,2 --> 2,1

202.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__CO + __Fe2O3--> __Fe + __CO2
a)
3,1 --> 2,3
b)
3,2 --> 1,1
c)
3,2 --> 2,4
d)
3,2 --> 2,1
203.

What are the coefficients that would properly balance this equation?

__AgNO3 + __H2S --> __Ag2S+ __HNO3

a)

2,1 --> 1,2

b)

1,2 --> 1,1

c)

1,2 --> 1,2

d)

1,2 --> 2,1

204.

What are the coefficients that would properly balance this equation?

__H2 + __S --> __H2S

a)

1,1 --> 1

b)

2,2 --> 2

c)

1,2 --> 1

d)

1,2 --> 2

205.

What are the coefficients that would properly balance this equation?

__Al + __O2--> __Al2O3

a)

4,1 --> 2

b)

4,3 --> 4

c)

3,4 --> 1

d)

4,3 --> 2

206.

Determine the coefficients to make the following equation balanced?

__N2 + __O2--> __NO

a)

1, 1, 1

b)

1, 1, 2

c)

2, 2, 2

d)

1, 2, 2

207.

Determine the coefficients to balance the equation.

__Al +__HCl --> __H2 +__AlCl3

a)

2,6,3,2

b)

it's already balanced

c)

4,12,3,4

d)

2,1,4,5

208.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

209.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

210.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

211.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

212.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

213.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

214.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

215.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

216.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

217.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

218.

A list of elements that organizes them in order of their reactivity is called

a)

Negativity Series

b)

Netflix Series

c)

Activity Series

d)

Displacement Series

219.
Based on the activity series, will this reaction occur?
Ni (s) + H2O (l) →
a)
Yes
b)
No
220.
Based on the activity series, will this reaction occur?
Au (s) + HCl (l) →
a)
Yes
b)
No
221.

Predict the product(s) of this reaction (don't worry about balancing):

Li + H2O →

a)

Li2O + H2

b)

LiO + H2

c)

LiOH + H2

d)

Li(OH)2

222.

Predict the product(s) of this reaction (don't worry about balancing):

Mg + HCl →

a)

MgHCl

b)

MgCl2 + H2

c)

MgCl2 + H

d)

MgCl + H2

223.

Predict the product(s) of this reaction (don't worry about balancing):

SrI2 +Br2→

a)

Sr + I2Br2

b)

SrBr + I2

c)

SrBr2 + I2

d)

Sr + IBr2

224.
Predict the product(s) of this reaction (don't worry about balancing):
C12H22O11 + O2 →
a)
CO + HO
b)
CO2
c)
CO2 + H2O
d)
H2O
225.

Based on the activity series, which metal could X represent in the reaction below?

X + Ca (NO3)2 --> Ca + X (NO3)2

a)

Ba

b)

Fe

c)

Mg

d)

Zn

226.

For the following balanced chemical equation

2K + F2 --> 2KF

how many moles of KF are present?

a)

2 mol of KF

b)

1 mol KF

227.

6.0 mol of aluminium reacts with oxygen to form aluminium oxide. What is the amount of oxygen, in mol, needed for complete reaction?

4Al(s) + 3O2(g) → 2Al2O3(s)

a)

1.5

b)

3.0

c)

4.5

d)

6.0

228.

Nitrogen reacts with hydrogen to give ammonia, NH3 in a closed container. How many moles of H2 are needed to produce 25 mol of NH3?

N2 + 3H2 → 2NH3

a)

A) 12.5

b)

B) 25

c)

C) 37.5

d)

D) 50

e)

E) 62.5

229.
The ______________ yield is the maximum amount of product possible in a reaction. This determines the amount of product that should be produced in a perfect setting
a)
Percent
b)
actual
c)
stoichiometry
d)
theoretical
230.

When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

231.
7. The amount of product that actually forms when a chemical reaction is carried out in a laboratory is called the _________ yield.
a)
actual
b)
theoretical
c)
percent
232.
CH4  +  2O2  →  CO2  +  2H2O
24 grams of CH4 was added to the above reaction. Calculate the theoretical yield of CO2.
a)
66 grams
b)
132 grams
c)
33 grams
d)
8.72
233.
P4 + 6Cl2 --> 4PCl3 
The reaction of 75.0g P4 with excess chlorine gas produces 110g PCl3 in lab. Find the theoretical yield and calculate percent yield for the reaction. 
a)
78%
b)
64%
c)
27%
d)
33%
234.

This is what you call a reactant that you have enough of. The one that DOES NOT run out.

a)

Limiting Reactant

b)

Excess Reactant

c)

Highly Reactant

d)

Super Reactant

235.
The limiting reactant
a)
slows the reaction down
b)
is used up first
c)
is the reactant that is left over
d)
controls the speed of the reaction
236.

Using the following equation:

Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)

How many moles of iron can be made from 6 moles H2 and excess Fe2O3?

a)

4 moles Fe

b)

6 moles Fe

c)

9 moles Fe

d)

2 moles Fe

237.

How much water can be made if 8 moles of NH3 react with 6 moles of NO?

4NH3+6NO --> 5N2 + 6H2O

a)

5 moles

b)

6 moles

c)

12 moles

d)

18 moles

238.

What is the molar mass of Ca(OH)2

a)

58.1g/mol

b)

84.0g/mol

c)

74.1g/mol

239.

What is the first thing you must do to solve a stoichiometry problem?

a)

Write a Balanced Equation

b)

Panic

c)

Write an Unbalanced Equation

d)

Avogadro's Number

240.

How many moles are in 45.6 g Ca?

a)

0.879mol Ca

b)

1.14mol Ca

c)

1.50mol Ca

d)

0.62 mol Ca

241.

How many grams are in one mole of Nitrogen gas (N2)?

a)

14.0

b)

28.0

c)

14.011

d)

28.50

242.

Balance this reaction: ____ LiNO3 + ____ MgF2 ----> ____ Mg(NO3)2 + ____ LiF

a)

1,1,1,1

b)

1,2,1,1

c)

2,1,1,2

d)

2,1,2,1

243.

How many O atoms are in Al2(CO3)3?

a)

2

b)

3

c)

6

d)

9

244.

Gas grills use propane fuel. The combustion of propane is represented in this equation:

C3H8 + 5O2 ----> 3CO2 + 4H2O. How many grams of propane will burn when 36.0 moles of water are formed?

a)

0.500 g C3H8

b)

9.00 g C3H8

c)

318 g C3H8

d)

397 g C3H8

245.
CH4 + 2O2 --> 2H2O + CO2
What is the mass of CO2 produced when 35g of O2 reacts? 
a)
1.09 g
b)
24.1 g
c)
28.2 g
d)
44.0 g
246.

What is the mass of 0.75 moles of (NH4)3PO4?

a)

0.0044 g

b)

91 g

c)

110 g

d)

74 g

247.
2H2  +   O2    −−〉 2H2O
How many grams of H2O can be produced from 3.91 g of O2? 
a)
1.905
b)
4.4
c)
2.2
d)
1.1
248.

2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

Ethane (C2H6) combusts in the above reaction. What is the mole ratio of ethane to oxygen gas?

a)
b)
c)
d)
249.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
250.

How many moles of glucose, C6H12O6 can be "burned" biologically when 10.0 mol of oxygen is available? C6H12O6 (s) + 6O2 (g) → 6CO2 (g) + 6H2O(l)

a)

A- 0.938 mol

b)

B- 1.67 mol

c)

C- 53.3 mol

d)

D- 60.0 mol

251.

Which state of matter has both definite shape and definite volume?

a)

Gas

b)

Liquid

c)

Solid

252.
What happens when my glass of water is sitting in the sun and disappears into a gas?
a)
evaporation
b)
burning
c)
melting
d)
freezing
253.
How is a gas defined?
a)
Indefinite shape, indefinite volume
b)
Definite shape, definite volume
c)
Found in stars
d)
Definite volume, indefinite shape
254.
What term describes a solid changing to a gas?
a)
Deposition
b)
Sublimation
c)
Evaporation
d)
Freezing
255.
Particles of a liquid
a)
are tightly packed together and stay in a fixed position.
b)
have no viscosity.
c)
decrease in volume with increasing temperature.
d)
are free to move around one another but still touch.
256.
Particles (molecules) in a ______________________ have more energy than the other states of matter.
a)
gas
b)
solid
c)
liquid
257.
The state of matter that has no definite size or shape is
a)
Solid
b)
Liquid
c)
Gas
258.
Which state of matter has the lowest compressibility?
a)
Solid
b)
Liquid
c)
Gas
d)
Plasma
259.
When a gas changes directly to a solid, the process is known as what?
a)
Sublimation
b)
Condensation
c)
Deposition
d)
Evaporation
260.

Which is not true about the liquid state of matter?

a)

The liquid state has a definite volume and a definite shape.

b)

The liquid state takes on the shape of its container.

c)

The liquid state has a definite volume and an indefinite shape.

d)

The particles in a liquid can easily move past each other.

261.

Which process could cause a material to change state from gas to liquid?

a)

Adding heat

b)

Adding energy

c)

Removing particles

d)

Removing energy

262.
A gas
a)
has a definite shape but no definite volume
b)
has a definite volume but no definite shape
c)
has fast-moving particles
263.
Boiling
a)
liquid to gas
b)
gas to solid
c)
gas to liquid
d)
solid to liquid
264.
What are the states of matter?
a)
solid, liquid, and juice
b)
solid and liquid
c)
solid and gas
d)
solid, liquid, and gas
265.
The molecules in the picture are tightly held together with little movement. They have shape and energy.  Therefore, the picture represents _________.
a)
solid
b)
liquid
c)
gas
d)
plasma
266.

This type of soilds have ordered internal structures.

a)

Crystalline solids

b)

Amorphous solids

c)

Pseudo solids

d)

Supercooled liquids

267.

What is an amorphous solid?

a)

Solid that does not has ordered internal structure

b)

Solid that has a crystal lattice

c)

Solid that cannot change its state

268.
Which form of matter does not take the shape of its container?
a)
liquid
b)
gas
c)
solid
d)
air
269.
______________________ takes place when a liquid changes to a solid.
a)
freezing
b)
melting
c)
boiling
d)
sublimation
270.
a)
It remains the same.
b)
It changes greatly.
c)
It changes minimally.
d)
Unable to tell.

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