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Semester 2 chem final exam review

Total questions: 150

Worksheet time: 5hrs 3mins

Name
Class
Date
1.
True or False
In a chemical reaction, no new atoms are created, and no atoms are destroyed. 
a)
true
b)
false
2.
A chemical change is different than a physical change because in a chemical change
a)
Chemicals are used
b)
Molecules do not physically touch
c)
A new substance is formed and in a physical change no new substance is formed
d)
The change can be seen but in a physical change it cannot
3.
The left side of the equation below is called
a)
Products
b)
Reactants
4.
The right side of the equation below is called the
a)
products
b)
reactants
5.
Which statement is not a description of a chemical reaction?
a)
A solid is dropped into a beaker of liquid and a gas is released.
b)
Two liquids are mixed in a beaker and a solid forms at the bottom of the beaker.
c)
A solid is dropped into a beaker of liquid and an explosion occurs.
d)
A liquid is heated in the sun and half of it evaporates.
6.
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 
7.
A chemical reaction that absorbs heat
a)
Single replacement
b)
Exothermic
c)
Endothermic
d)
Decomposition
8.
In a chemical reaction
a)
The atoms of the reactants always stay together to form the products
b)
The atoms of the reactants unbond, rearrange, and then rebond to form the products
c)
New atoms are formed which combine to make the products
d)
Some atoms disappear while others multiply to form the products
9.
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
10.
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
11.
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
12.

How many Carbons are present on the reactant side?

a)

1

b)

2

c)

3

d)

4

13.

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.

14.
Number of C's in 2Na₂CO₃
a)
1
b)
2
c)
3
d)
5
15.
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.
16.
Balance this equation,            
Al2O3 --> Al + O2 
a)
Cannot be balanced
b)
2Al2O3 --> 2Al+3O2 
c)
2Al2O3--> 4Al+3O2 
d)
3Al2O3--> 2Al+O2 
17.
a chemical reaction that releases energy by light or heat
a)
Endothermic Reaction
b)
Exothermic Reaction
c)
Diffusion
d)
Fission
18.
If reaction starts with 20g of reactants it should produce... 
a)
a total of 40g of product
b)
a total of 10g of product
c)
a total of 80 g of product
d)
a total of 20g of product
19.

What type of reaction is Fe + Cl2 → FeCl3

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

20.

What type of reaction is C2H2 + O2 → CO2 + H2O

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

21.

What type of reaction is Ag2O → Ag + O2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

22.

What type of reaction is C5H10 + O2 → CO2 + H2O

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

23.

What type of reaction is Zn + HCl → H2 + ZnCl2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

24.

What type of reaction is H2 + N2 → NH3

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

25.

What type of reaction is Fe + H2SO4 → H2 + FeSO4

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

26.

What type of reaction is Mg + Br2 → MgBr2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

27.

What type of reaction is K2CO3 → K2O + CO2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Combustion

e)

None of these

28.

Identify the type of reaction:

Zn(OH)2 + HNO3 ---> H2O + Zn(NO3)2

a)

single replacement

b)

combustion

c)

acid-base neutralization

d)

synthesis

e)

decomposition

29.
Ca(OH)2 is an example of a(n)
a)
Acid
b)
Base
c)
Neutral
30.
HBr is an example of a(n)
a)
Acid
b)
Base
c)
Neutral
31.
What are the products to a neutralization reaction?
a)
H2 + Ionic Salt
b)
H2O + Ionic Salt
c)
H3O+ + Ionic Salt
d)
OH- + Ionic Salt
32.
NH4NO3
a)
soluble
b)
insoluble
33.
NaCl
a)
soluble
b)
insoluble
34.
K2CO3
a)
soluble
b)
insoluble
35.
CaCO3
a)
soluble
b)
insoluble
36.

Determine the solubility for the substances at 55'C and arrange them in order from lowest to highest solubility.

a)

NaCl, NH4Cl, KBr, NaNO3

b)

NaCl, NH4Cl, NaNO3, KBr

c)

NH4Cl, NaCl, NaNO3, KBr

d)

NaNO3, KBr, NH4Cl, NaCl

37.

Identify if the following solution would be saturated, unsaturated, or supersaturated: 103 g KBr at 70'C.

a)

Unsaturated

b)

Saturated

c)

Supersaturated

38.

Identify how many grams of KNO3 is required to make a saturated solution at 40'C.

a)

50 g

b)

45 g

c)

60 g

d)

33 g

39.

How could you change a saturated solution to an unsaturated solution?

a)

Add solvent

b)

Add solute

40.

Identify a method to decrease the dissolving rate of a solution:

a)

decrease the temperature

b)

add KE

c)

stir the solution

d)

increase the temperature

41.

An aqueous solution is:

a)

any liquid with another compound dissolved in it.

b)

an ionic compound with water dissolved in it.

c)

water with another compound dissolved in it.

d)

none of the above

42.

Which of the following compounds is SOLUBLE?

a)

copper carbonate

b)

calcium carbonate

c)

potassium carbonate

d)

strontium carbonate

43.

In writing the chemical equation for a reaction that produces a precipitate, what abbreviation of the physical state must appear with one of the products?

a)

(s)

b)

(g)

c)

(l)

d)

(w)

44.

What would be the formula of the precipitate that forms when Pb(NO3)2 (aq) and K2SO4 (aq) are mixed?

a)

K(NO3)2

b)

PbSO4

c)

PbK2

d)

H2O

45.

Considering the following precipitation reaction:

Pb(NO3)2(aq) + 2KI(aq) → PbI2(s) + 2KNO3(aq)

Which compound would not form ions in the complete ionic equation?

a)

PbI2

b)

KNO3

c)

Pb(NO3)2

d)

KI

46.

When some ionic compounds form through reactions in solution, they fall out as a ___

a)

consolidated element

b)

heavy sludge

c)

dense discharge

d)

solid precipitate

47.

What is the net ionic equation for the reaction between K3PO4 (aq) and CuSO4 (aq)?

a)

2 K+(aq) + SO42-(aq) → K2SO4 (s)

b)

K+(aq) + SO42-(aq) → KSO4 (s)

c)

2 Cu2+(aq) + 3 PO43-(aq) → Cu3(PO4)2 (s)

d)

Cu2+(aq) + PO43-(aq) → CuPO4 (s)

48.

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

a)

Periodic Table

b)

Times Table

c)

6.02 X 1023

d)

The Mole

49.
The molar mass of an element is equal to its...
a)
Atomic mass
b)
Atomic number
c)
Oxidation number
d)
Valence electrons
50.
Mole in Chemistry is a(an)_______.
a)
unit
b)
animal
c)
number equals to 6.02
d)
number equals to 12
51.
What are the units for molar mass?
a)
grams
b)
amu
c)
grams/mole
d)
liters
52.
36.0 g of Be contains how many moles?
a)
0.25 mol
b)
4.0 mol
c)
45 mol
d)
320 mol
53.

How many moles are in 1459 grams of Na?

a)

63.46 moles

b)

60.36 moles

c)

10 moles

d)

1 mole

54.

How many grams are in 0.375 mol KBr

a)

39,10 g

b)

44.625 g

c)

0.003 g

d)

56.525 g

55.
How many grams are in 88.1 moles of magnesium?
a)
2141 g
b)
0.3 g
c)
30 g
d)
3.6 g
56.

What does the number 3 represent in 4NH3?

a)

Subscript

b)

Superscript

c)

Coefficient

57.

What does the number 4 represent in 4NH3?

a)

Subscript

b)

Superscript

c)

Coefficient

58.
What coefficient should be used to make the following equation balanced?
N2+O2--> _NO 
a)
1
b)
2
c)
3
d)
4
59.
What is the mole used for? 
a)
To measure the amount of grams in a substance
b)
To measure the amount of atoms or molecules in a substance
c)
To measure the amount of energy in a substance
d)
To measure the amount of bonding in a substance 
60.
How many atoms are in 1 mole of NaCl? 
a)
6.02 x 1023
b)
58 
c)
11
d)
17
61.

Why is the mole used to measure the atom?

a)

Atoms are extremely tiny particles, and their size varies from element to element

b)

Atoms are all the same size for every element

c)

Some atoms cannot be counted using the mole

d)

Tu eres loco, Senior Hagerman.

62.

The mole can be used to measure (SELECT ALL CORRECT ANSWERS)

a)

The amount of atoms

b)

The amount of molecules or compounds in a substance

c)

The amount of particles

d)

The amount of fission or fusion decay over time

63.

How many atoms are in 3 moles of ANY ELEMENT?

a)

Multiply 3 x 26.981 g/mol

b)

Multiply 3 x (6.02 x 1023) = 1.806 x 1024 atoms

c)

13 g/mol

d)

26.981 g/mol

64.

How many moles are in 3.01 x 1023 atoms of magnesium?

a)

0.500 moles

b)

1.81 x 1046 moles

c)

5.00 x 1021 moles

d)

5.00 moles

65.
Using the balanced equation in question 1,
Mg(s)   +   HCl(aq)  -->   MgCl₂(aq)   +   H₂(g)
How many grams of HCl are consumed by the reaction of 2.50 moles of magnesium?
a)
5.00 g
b)
7.29
c)
182 g
d)
218 g
66.
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)
Ask for help
67.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of Mg to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
68.
2CO  +  O2  −-> 2CO2
How many liters of carbon dioxide are produced from 10L of carbon monoxide?
a)
10
b)
20
c)
1
d)
5
69.

2Al + 6HCl --> 2AlCl3 + 3H2

Aluminium reacts with hydrochloric acid. How many grams of aluminum are necessary to produce 11 L of hydrogen gas at STP?

a)

13

b)

8.8

c)

0.99

d)

1.0

70.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
71.
When does a chemical reaction stop?
a)
When the lab is finished
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
72.
Identify the limiting reagent when 6.00 g HCl combines with 5.00 g Mg to form MgCl2.
 
Mg +  2HCl --> MgCl2  +  H2   
 
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
73.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
74.
Fe (s) + S (l) --> FeS (s)  

In the experiment above, 7.62 g of Fe are allowed to react with 8.67 g of S.
How much FeS is formed?
a)
14.8 g
b)
12.2 g
c)
13.7 g
d)
19.9 g
75.
You need 2 pieces of bread, 1 tablespoon of peanut butter and 2 tablespoons of jelly to make a sandwich.  If you have 10 pieces of bread, 4 tablespoons of peanut butter and 20 tablespoons of jelly, what is the limiting reactant?
a)
bread
b)
jelly
c)
peanut butter
d)
sandwich
76.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
77.

Which of the following is CORRECT assumption of the kinetic molecular theory of gases?

a)

Collision between gas particles are inelastic

b)

Gas particles move around in an orderly manner

c)

Gases consists of closely spaced particles

d)

The average kinetic energy of the gas particle depends on the temperature

78.

The picture shows a paperclip floating when it is gently placed on water. What is the water characteristic that cause this?

a)

Surface tension

b)

Viscosity

c)

Polar molecule

d)

Diffusion

79.

Carbon has _______ electrons - the same number of bonds it can make.

a)

1

b)

2

c)

3

d)

4

80.

Organic compounds must have which two elements?

a)

Carbon and Oxygen

b)

Oxygen and hydrogen

c)

Carbon and Hydrogen

81.

Which of the following is an inorganic compound?

a)

C6H12O6

b)

H2O

c)

CH18

82.

The four organic molecules that are necessary for life are

a)

Oxygen, lipids, proteins and Carbohydrates

b)

Carbohydrates, proteins, lipids and nucleic acids

c)

Carbohydrates, minerals, proteins and liipids

83.

Organic compounds made only of the elements carbon and hydrogen are called...

a)

Hydrocarbons

b)

Carbohydrogens

c)

Carbohydrates

d)

Hydrocarbonates

84.

Which type of bonding is present within organic molecules?

a)

Covalent bond

b)

Ionic bond

c)

Metallic bond

d)

Hydrogen bond

85.

____________ groups are atoms, groups of atoms or bond that determine the characteristic of an organic compound.

a)

Aliphatic

b)

Aromatic

c)

Functional

d)

Hydrocarbon

86.

molecule with the same molecular structure but different structural formula

a)

fats

b)

lipids

c)

fossil fuels

d)

isomers

87.

Macromolecule that is made up of repeated structure called monomers

a)

protein

b)

amino acids

c)

polymer

88.

what are the outer most electrons called

a)

energy level

b)

valence

c)

valency

89.

Organic compounds that are made of only hydrogen and carbon atoms. They are found in many places, including crude oil and natural gas.

a)

Hydrocarbons

b)

Nucleic Acids

c)

Proteins

d)

Lipids/Fats

90.

They are the most abundant compounds found in living organisms, including polysaccharides which are polymers composed of many sugar building blocks. They are used by cells to get and store energy.

a)

Polymers

b)

Organic Compound

c)

Carbohydrates

d)

Carbon

91.

Without these, cells could not live. Long chains of carbon and hydrogen molecules creating fatty acids.

a)

Carbohydrates

b)

Organic Chemistry

c)

Proteins

d)

Lipids

92.

A molecule, made from joining together many small molecules called monomers.

a)

Lipids

b)

Polymers

c)

Carbohydrates

d)

Monomers

93.

The scientific study of the structure, properties, and reactions of carbon containing compounds.

a)

Organic Chemistry

b)

Organic Compounds

c)

Inorganic Compounds

d)

Chemical Formula

94.

Phase change going from Liquid to Solid...

a)

Melting

b)

Freezing

c)

Condensation

d)

Sublimation

95.

Phase change going from a Gas to a Liquid...

a)

Sublimation

b)

Deposition

c)

Ionization

d)

Condensation

96.

Phase change going from a Solid to a Gas...

a)

Deposition

b)

Sublimation

c)

Condensation

d)

Recombination

97.

Are the particles moving faster or slower as time goes on?

a)

Faster

b)

Slower

98.
All changes in the state of matter of a substance requires
a)
vibration
b)
water
c)
permission
d)
energy
99.
The phase change from water vapor to liquid water is known as...
a)
evaporation
b)
precipitation
c)
condensation
d)
sublimation
100.

A student measures the pressure and volume of an empty water bottle to be 1.4 atm and 2.3 L. She then decreases the pressure to 0.65 atm. What is the new volume?

a)

2.1 L

b)

5.0 L

c)

8.2 L

d)

3.9 L

101.

A student inflates a balloon with helium then places it in the freezer. The student should expect

a)

the balloon's volume to increase

b)

the balloon's volume to decrease

c)

the balloon's moles to increase

d)

the balloon's moles to decrease

102.
Which of the following would increase the (gas) pressure of a system?
a)
Increase the Temperature
b)
Pump in more gas
c)
Decrease the volume
d)
All of these
103.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
104.
What about gases can be measured?
a)
Pressure and Volume
b)
Temperature, Volume, and Pressure
c)
Volume and Temperature
d)
Pressure, Temperature, Volume, and Moles
105.
What is 50 °C in Kelvin?
a)
223
b)
323
c)
100
d)
50
106.

Determine the temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure.

a)

0 K

b)

107 K

c)

207 K

d)

307 K

107.

Pressure is

a)

defined as the mass that an object exerts when at rest.

b)

not a measurable in gases.

c)

defined as the number of moles of substance divided by the mass of the substance.

d)

created by the force of the gas particles impacting the walls of the container.

108.
You have 20 g of water with specific heat of 4.18 J/gŸ°C.  The temperature changes from 25° C to 20° C.  How much heat energy (Q) moves from the water to the surroundings?
a)
418 Joules
b)
209 J
c)
83 J
d)
4.18 J
109.
Calculate the heat absorbed by 105.0 grams of water when it is heated to cook spaghetti. The initial temperature of the water is 20.0°C, and the final temperature of the water is 99.0°C. The specific heat of water is 4.18 J/g•°C.
a)
8778 J/g°C
b)
0.0005 J/g°C
c)
34673 J/g°C
d)
43451.1 J/g°C
110.
What does temperature measure?
a)
Heat
b)
ºC
c)
Kinetic Energy
d)
Thermal Energy
111.
Is photosenthysis an Exothermic or an Endothermic reaction?
a)
Endothermic
b)
Exothermic
112.
What letter represents the activation energy?
a)
A
b)
B
c)
C
d)
D
113.
What type of reaction is this?
a)
Endothermic
b)
Exothermic
114.
According to the Law of Conservation of Energy, energy cannot be _________ or ____________. 
a)
destroyed, destroyed
b)
created, saved
c)
created, destroyed
d)
lost, found
115.

What is kinetic energy?

a)

moving energy

b)

potential energy

c)

stored energy

d)

renewable energy

116.

What is potential energy?

a)

moving energy

b)

stored energy

c)

renewable energy

d)

non renewable energy

117.
Increase in temperature of the reactants can do one of the following
a)
Slow collision frequency
b)
Allow less effective collision between the particles
c)
Cause particles to lose speed
d)
Increase collision between the particles thus increasing the rate.
118.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
119.
Which factors increase the rate of a reaction.
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of these
120.
A ______________ is a substance that increases the rate of a reaction without being used up during the reaction. 
a)
catalyst
b)
product
c)
reactant
d)
solute
121.

(NH4)2SO4 + Ba(NO3)2 → 2NH4NO3 + BaSO4

What would happen if we increased the concentration of (NH4)2SO4?

a)

More product would be produced

b)

Less (NH4)2SO4 would participate in the reactions

c)

There would be less collisions between

(NH4)2SO4 and Ba(NO3)2

d)

There would be more Ba(NO3)2 particles to react

122.

In which container would you expect a higher reaction rate, and why? (Note: The number of particles is the same in both containers.)

a)

The left would have a higher reaction rate because it has a greater volume and more collisions will happen.

b)

The right would have a higher reaction rate because it has a greater volume and more collisions will happen.

c)

The left would have a higher reaction rate because it has a lesser volume and more collisions will happen.

d)

The right would have a higher reaction rate because it has a lesser volume and more collisions wil happen.

123.
2SO2(g)+O2(g)⇌2SO3(g)
Removing O2(g) will
a)
shift equilibrium right
b)
shift equilibrium left
c)
decrease temperature
d)
have no change
124.
2SO2(g)+O2(g)⇌2SO3(g)
Adding SO2(g) will
a)
shift equilibrium right
b)
shift equilibrium left
c)
increase rate of reaction
d)
have no change
125.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
126.
For the reaction...
heat  +  N2  +  O2  ↔  2NO
If the heat is added to the chemical system, the equilibrium will shift _______.
a)
left
b)
right
c)
left and right
d)
neither left nor right
127.

What is the formula for phosphorous acid?

a)

H3PO4

b)

H2PO4

c)

H3P

d)

H3PO3

128.

What is the formula for nitric acid?

a)

HNO2

b)

HNO3

c)

HNO4

d)

H2NO3

129.

Name this acid with the formula HF

a)

hydrofluoric acid

b)

hypofluoric acid

c)

hydrogen fluorine acid

d)

fluoric acid

130.

H3PO4

a)

hydrophsophorus acid

b)

phosphoric acid

c)

hydrogen phosphorous

d)

phosphori hydroxide

131.
Mg(OH)2
a)
magnesium hydroxide acid
b)
hydromagnesium acid
c)
magnesium oxygen hydride
d)
magnesium hydroxide
132.

A substance that is 3 on the pH scale would be a(n):

a)

acid

b)

base

c)

neutral

d)

solute

133.
Human blood has a pH between 7.35 and 7.45. Which of the following best describes human blood?
a)
strongly acidic
b)
slightly acidic
c)
strongly basic
d)
slightly basic
134.

What is the molarity of a solution with 0.25 mol of HNO3 dissolved in 1.5 L of solution?

a)

6.0 M

b)

0.17 M

c)

0.38 M

d)

2.5 M

135.

What is the pH of a solution with a pOH of 5.75?

a)

1.35

b)

5.60

c)

8.25

d)

10.5

136.

What is the [H+] for a solution with a pH of 2.5?

a)

3.2x10-3 M

b)

4.6x10-4 M

c)

3.2x103 M

d)

9.3x105 M

137.

Which is NOT true about indicators?

a)

They each have a certain pH where they change color

b)

They come in a variety of colors

c)

They are useful in titrations

d)

They neutralize acids and bases

138.

What are the products when hydrobromic acid is mixed with sodium hydroxide

a)

H2O and NaBr

b)

HBr and NaOH

c)

OBr and NaH

d)

Na and BrOH

139.

Water has a neutral because

a)

it has more H+ ions than OH-

b)

it has more OH- ions than H+

c)

it does not produce any ions

d)

it has an equal amount of H+ and OH- in solution

140.

What is the [H+] if the pH is 4.0?

a)

1.0 x 10-10 M

b)

1.0 x 10-14 M

c)

1.0 x 10-4 M

d)

1.0 x 10-7 M

141.

What is the [OH-] if the [H+] is 1.0 x 10-3M?

a)

1.0 x 10-3 M

b)

1.0 x 10-14 M

c)

6.02 x 10-23 M

d)

1.0 x 10-11 M

142.

What is the oxidation number of chlorine in HClO?

a)

0

b)

-1

c)

+1

d)

+5

143.

Reduction is the ___________ of electrons.

a)

loss

b)

gain

c)

sharing

d)

transfer

144.

What is the oxidation number of nitrogen in N2?

a)

-3

b)

0

c)

+4

d)

-1

145.

The sum of the oxidation numbers in SCN- is equivalent to

a)

0

b)

-1

c)

+1

d)

+3

146.

What is the oxidation number of iodine in KIO3?

a)

0

b)

-1

c)

+5

d)

+1

147.

Which of the following represents oxidation?

a)

C → CH4

b)

Fe3+ → Fe2+

c)

Cl2 → 2Cl-

d)

Zn → ZnO

148.
Which of the following represents reduction?
a)
C →  CO
b)
N2 →  NH3
c)
Zn  →   Zn2+ 
d)
H2 →  H2O
149.

In the reaction Zn + 2HCl --> ZnCl2 + H2

which element, if any, is oxidized?

a)

Zinc

b)

Hydrogen

c)

Chlorine

d)

None

150.
In the reaction
2Ca(s) + O2(g) --> 2CaO(s), calcium is __________
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above

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