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Semester 2 Chemistry Review

Total questions: 116

Worksheet time: 1hrs 22mins

Name
Class
Date
1.
The energy of an object as it is in motion is defined as
a)
Kinetic Theory
b)
Kinetic energy
c)
Potential energy
d)
Electric energy
2.
The random molecular motion of a substance is greatest when the substance is
a)
condensed
b)
frozen
c)
gas
d)
a liquid
3.
What is 50 C in Kelvin?
a)
223
b)
323
c)
100
d)
50
4.
What will happen to the volume of a gas under constant temperature if the pressure increases?
a)
Increase
b)
Decrease
c)
Nothing
d)
Explosion!
5.
If you increase the pressure of a constant volume of gas, what will happen to the temperature?
a)
Increase
b)
Decrease
c)
Stay the same
d)
It will Blow Up
6.
What is the device that measures atmospheric pressure?
a)
Aerometer
b)
Annemeter
c)
Barometer
d)
Humidity Detector
7.
The kinetic theory states
a)
Particles won't move if you don't apply energy to it.
b)
Particles only move in liquids and gases.
c)
Particles are always in motion.
d)
At the same temperature the object that has the most mass heats quicker.
8.
Gas molecules can easily be compressed  because ___________. 
a)
gas molecules are soft
b)
gas molecules are far apart
c)
gas molecules follow the shape of the container
9.
Gas particles have the ________ kinetic energy because they move the fastest.
a)
least
b)
most
10.
The higher the average kinetic energy the __________________ 
a)
the higher the volume
b)
the higher the mass
c)
the higher the temperature
d)
the higher the density
11.
How do gas molecules move? 
a)
in an orderly fashion 
b)
constantly and randomly
c)
in straight line paths
d)
in a circular motion
12.
Gases are described as having a 
a)
definite shape and indefinite volume
b)
indefinite shape and indefinite volume
c)
definite shape and definite volume
d)
indefinite shape and definite volume
13.
Collisions between gas particles are said to be "elastic" because _________________________.
a)
they have a stretchy waistband
b)
kinetic energy is lost between particles
c)
kinetic energy is not lost between particles and is instead transferred
d)
particles move in a straight line
14.
Which of the following explains why gases are less dense than solids?
a)
Gases have faster moving particles that are very close together.
b)
Gases have slow moving particles that are very close together.
c)
Gases have faster moving particles that are far apart.
d)
Gases have slow moving particles that are close together.
15.
The intermolecular forces between gas molecules are 
a)
very strong
b)
extremely important
c)
not significant at normal temperatures and pressures
16.
A gas will always _____________ to fill its container.
a)
expand
b)
contract
c)
heat up
d)
cool down
17.
Gases are the only phase of matter that is ________________ because there is a large amount of space between molecules.
a)
Differential
b)
fluid
c)
Compressible
d)
molar
18.
The key word for pressure is 
a)
motion
b)
collisions
c)
concentration
d)
energy
19.
Higher pressure means ______________ collisions between gas particles and the walls of their container.
a)
more
b)
less
c)
faster
d)
harder
20.
How do you convert degrees C to K?
a)
Add 273
b)
Subract 273
c)
call 911
21.
STP stands for
a)
Significant Technology Problems
b)
Sulfur Technecium  and Phosphorous
c)
Solid Tectonic Placebo
d)
Standard Temperature and Pressure
22.
Pressure is caused by ______.
a)
gravity.
b)
gas molecules colliding with each other.
c)
gas molecules colliding with surfaces of the container.
d)
gas molecules reacting with each other.
23.
What is the symbol for heat?
a)
q
b)
H
c)
J
d)
∘C
24.
The heat required to raise the temperature of a SUBSTANCE by 1∘C
a)
calorie
b)
joule
c)
specific heat
d)
4.184 J
25.
Chemical reactions where both q and H are negative are considered
a)
spontaneous
b)
nonspontaneous
c)
exothermic
d)
endothermic
26.
Chemical reactions that absorb energy are called
a)
endothermic
b)
fast
c)
slow
d)
exothermic
27.
Formula for solving specific heat problems
a)
q = mcΔT
b)
H = ΔH x moles
c)
H = ΔH x grams
d)
products - reactants
28.
Formula for solving phase change problems
a)
q = mcΔT
b)
grams x moles x ΔH 
c)
H = ΔH x grams
d)
products - reactants
29.
What is the symbol for enthalpy?
a)
H
b)
S
c)
G
d)
q
30.
Energy can not be created or destroyed, it can only be transferred refers to the....
a)
law of conservation of energy
b)
law of conservation of mass
c)
life facts
d)
law of conservation of chemistry
31.
Which direction does heat flow?
a)
hot to cold
b)
cold to hot
32.
Temperature is __________, but heat is_______________. 
a)
the average kinetic energy; transfer of energy
b)
transfer of energy; the average kinetic energy 
c)
a measure of heat; how much temperature a substance has
d)
how much heat a substance has; measure of temperature
33.

For an endothermic reaction, the surroundings feel

a)

warm

b)

cold

34.

For an exothermic reaction, the SYSTEM feels

a)

warm

b)

cold

35.
Temperature is measured in 
a)
joules
b)
grams
c)
degrees Celcius
d)
Kelvin
36.
The variable C stands for what
a)
heat 
b)
mass
c)
specific heat
d)
change in temperature
37.
For the formula:
 Q= m c ∆T
The  units for specific heat are:
a)
g /J C
b)
°C/g J
c)
kJ/g
d)
J/g°C
38.
What is the symbol for entropy?
a)
H
b)
S
c)
q
d)
E
39.
The randomness or disorder of a system
a)
heat (q)
b)
enthalpy (H)
c)
entropy (S)
d)
temperature (T)
40.
A reaction that occurs without outside intervention is considered
a)
spontaneous
b)
exothermic
c)
endothermic
d)
nonspontaneous
41.
The study of heat changes that accompany chemical reactions and phase changes
a)
energy
b)
chemistry
c)
work
d)
thermochemistry
42.
Entropy increases from solid, liquid to gas. Why?
a)
Molecular disorder increases
b)
Molecular randomness decreases
c)
Molecules are more energetic
d)
Molecules are more reactive
43.
What phase change brings an increase in entropy?
a)
g->s
b)
l->s
c)
l->g
d)
g->l
44.
As NaCl dissolves according to the equation
NaCl(s) → Na+(aq) + Cl-(aq), the entropy of the system 
a)
Increases
b)
Decreases
c)
Remains the same
45.
Spontaneous reactions are driven by
a)
increasing enthalpy and increasing entropy.
b)
decreasing enthalpy and decreasing entropy.
c)
increasing enthalpy and decreasing entropy.
d)
decreasing enthalpy and increasing entropy.
46.
Which one of these would result in a decrease in entropy?
a)
A solid solute dissolves in water.
b)
A gas is released.
c)
A liquid freezes.
d)
A liquid boils.
47.
What is a substance that is dissolved in another substance? 
a)
solution
b)
solute
c)
solvent
d)
compound
48.
What is a solvent?
a)
The substance that does the dissolving in a solution.
b)
The substance that is being dissolved in a solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
49.
In the above picture, a powder is about to be poured into the liquid. Which of the following should be done to make this powder dissolve faster?

a)
stir the powder in the liquid
b)
freeze the mixture
c)
add more powder to the liquid
d)
store the mixture in a dark place
50.
A solution that is considered dilute would be....
a)
Dark in color
b)
Have a strong scent
c)
Have a large amount of solute
d)
Have a small amount of solute
51.

At high pressure, gases are

a)

more soluble

b)

less soluble

c)

insoluble

52.

Which of the following increases the rate of dissolving?

a)

Agitation

b)

Increasing Temperature

c)

Decreasing particle size

d)

All of the above

53.

Which of the following is present in larger quantity in a solution

a)

Solvent

b)

Solute

c)

solution

d)

Non of the above

54.

As temperature increases, the solubility of solid solute

a)

increases

b)

decreases

55.

How does temperature affect the rate of dissolving?

a)

by increasing the kinetic energy

b)

by decreasing the particle size

c)

by increasing collisions between particles

d)

Both increasing kinetic energy and collisions

56.

A student is dissolving sugar in water to make candy. She notices that sugar lumps are forming at the bottom of the pan. What could she do to help more of the sugar dissolve?

a)

heat the solution

b)

cool the solution

c)

add more sugar to the pan

d)

take some water out of the pan

57.

Which of the following increases the rate at which a solid solute will dissolve in a beaker of water?

a)

placing the beaker in a bucket of ice

b)

adding the solute slowly into the beaker

c)

crushing the solute before placing it into the beaker

d)

agitating the beaker before placing the solute

58.
Which solute does not increase in solubility as temperature rises?
a)
NH3
b)
NaNO3
c)
KNO3
d)
NaCl
59.
You and your friend have a contest to see who can make iced tea the fastest. Which of the following would NOT help you win?
a)
Cooling the water
b)
Using smaller crystals
c)
Heating the water
d)
Stirring quickly
60.
How does a solution become supersaturated?
a)
dissolve lots of solvent in it.
b)
dissolve a little solute in it. 
c)
dissolve more solute than you should be able to. 
d)
dissolve a super amount of solvent in it. 
61.
Which solute is the least soluble at 90 ⁰C?
a)
SO2
b)
KClO3
c)
KI
d)
HCl
62.
When no more sugar will dissolve in a glass of water, the solution is
a)
unsaturated
b)
saturated
c)
supersaturated
d)
suspended
63.
Which of the following usually makes a substance dissolve faster in a solvent?
a)
agitating the solution
b)
increasing the particle size of the solute
c)
lowering the temperature
d)
decreasing the number of particles
64.
A solute that contains polar molecules will dissolve in a solvent that contains
a)
nonpolar molecules
b)
polar molecules
c)
covalent molecules
d)
equal-sized molecules
65.
A _______ solution contains more solute than would normally dissolve at a certain temperature.
a)
unsaturated
b)
suspended
c)
saturated
d)
supersaturated
66.
What does it mean to be "Soluble" ?
a)
Capable of being a solid.
b)
To have soul.
c)
Capable of being dissolved.
d)
To sink.
67.

Which substance is least soluble at 0 ºC?

a)

KI

b)

KNO3

c)

KClO3

d)

Ce2(SO4)3

68.

Which of the following will dissolve most rapidly?

a)

sugar cubes in cold water

b)

sugar cubes in hot water

c)

powdered sugar in cold water

d)

powdered sugar in hot water

69.

The ability of an atom to attract the shared electrons in a covalent bond is called its _____.

a)

Electronegativity

b)

Polarizability

c)

Electron affinity

d)

Nuclear charge

70.

Which formula represents a polar molecule containing polar covalent bonds?

a)

NaCl

b)

CH4

c)

NH3

d)

F2

71.

Which of the following is soluble in water?

a)

sodium nitrite (NaNO3)

b)

Gold (Au)

c)

Benzene (C6H6)

d)

Carbon Tetrabromide (CBr4)

72.

What compounds are soluble in water? (select ALL that apply)

a)

Polar Covalent Compounds

b)

Pure Metals

c)

Non polar Covalent Compounds

d)

Ionic Compounds

73.

When you add a solute, such as salt, to a solution, what happens to its boiling point?

a)

increases the boiling point

b)

decreases the boiling point

c)

depends on the solute added

d)

does not change

74.

The phrase 'like dissolves like' refers to molecules with similar _______ and _______.

a)

size and polarity

b)

size and elements

c)

polarity and elements

d)

elements and charges

75.

Which of the following is a polar molecule?

a)

CF4

b)

OF2

c)

CS2

d)

F2

76.

Which of the following in NOT a solution?

a)

tap water

b)

brass

c)

pure nitrogen

d)

air

77.

Which of the following would decrease the freezing point of water the greatest? (think dissociation factor)

a)

C6H12O6

b)

NaCl

c)

Li2CO3

d)

KI

78.

How do you determine if a substance is polar or non polar?

a)

determine total electrons

b)

draw Lewis structure and determine symmetry

c)

look and guess polarity

79.
Le Chatelier's Principle states that if a chemical system at equilibrium is stressed,
a)
the system will adjust to increase the stress
b)
the system will adjust to reduce the stress
c)
the system will not adjust
80.
How do catalysts increase the rate of reaction?
a)
The frequency of collisions is the increased
b)
The activation energy is lowered
c)
The energy of collisions is increased
d)
Both the frequency and energy of collisions is increased
81.
For the reaction...
SO2 + O2  <−>  SO3
If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.
a)
left
b)
right
c)
left and right 
d)
neither left nor right
82.
For the reaction...
SO2 + O2 <−>  SO3
If the equilibrium shifts to the right, the concentration of O2 will ___________.
a)
increase
b)
decrease
c)
remain the same
d)
double
83.
For the reaction...
SO2 + O2 <−>  SO3
If the concentration of O2 is increased, the equilibrium of the reaction will shift ___________.
a)
left
b)
right
c)
left and right
d)
neither left nor right
84.
What is the proper K for the following reaction? 
   2 NO(g)  +  O2(g) ↔ 2 NO2(g)
a)
K = [NO2]2 / [NO]2[O2]
b)
K =  [NO]2[O2] / [NO2]2
c)
K = [NO]2[O2][NO2]2
d)
K = 2[NO][O2] / 2[NO2]
85.
What kind of reaction is this?
a)
Endothermic
b)
Exothermic
c)
Equilibrium
d)
Can not be determined
86.
Which best defines "reaction rate"?
a)
Concentration change per unit time
b)
How long a reaction takes
c)
Adding a catalyst
d)
Combining reactants with products
87.
Activation energy is required to start a chemical reaction. What is activation energy?
a)
The energy needed for a reaction to occur
b)
The minimum amount of energy needed for a reaction to potentially occur
c)
The energy added by a catalyst
d)
The energy possessed by the products
88.
Decreasing the particle size increases the reaction rate because
a)
It makes particles move faster
b)
It increases the likelihood of collisions with the correct geometry
c)
It decreases the surface area available to react
d)
It increases the number of collisions
89.
In an endothermic reaction the products have 
a)
more energy than the reactants
b)
less energy than the reactants
c)
the same energy as the reactants
d)
no energy
90.
Which factor does NOT change the speed of a chemical reaction?
a)
Pressure
b)
Concentration
c)
Temperature
d)
Particle Size
91.

How are reaction rates determined?

a)

experimentally by measuring the temperature

b)

experimentally by measuring the concentration

c)

calculations using the temperature

d)

calculations using the concentrations

92.

SELECT ALL THAT APPLY!

What needs to happen for a reaction to occur...

a)

reactants must collide

b)

collisions must be in the correct orientation

c)

collisions must have enough energy

d)

reactants must be at the correct temperature

93.

What is a temporary, unstable arrangement of atoms in which old bonds are breaking and new bonds are forming?

a)

activation energy

b)

activated complex

c)

state of energy

d)

state of complexity

94.

What is the nature of a reactant?

a)

its reactivity

b)

how it is produced in nature

c)

its natural reaction

d)

how it creates reactants

95.

What does Ksp stand for?

a)

Solubility product constant

b)

Kitchen standard procedure

c)

Solubility product changes

d)

Insolubility product constant

e)

(Delta)G

96.
Which of the following is NOT true at equilibrium?
a)
The forward and reverse reactions proceed at the same rate.
b)
The concentrations of reactants and products do not change.
c)
The concentration of the reactants is equal to the concentration of the products.
d)
The forward and reverse reactions continue to occur.
97.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If  O2 is removed, the  concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
98.
N2O4(g) ↔ 2 NO2(g)
What is the concentration equilibrium constant expression?
a)
Kc = [NO2]2/[N2O4]
b)
Kc = [N2O4]/[NO2]2
c)
Kc = [N2O4]2/[NO2]
d)
Kc = [NO2]/[N2O4]2
99.
Keq < 1
a)
There are more products than reactants when the reaction reached equilibrium.
b)
There are more reactant than products when the reaction reached equilibrium.
c)
The amount of reactants is equal to the amount of products.
100.
Holly has an unknown substance in a beaker. She wants to determine the relative pH of the unknown substance. She places a piece of blue litmus paper into the substance, and the litmus paper stays blue.
The substance in the beaker
a)
is a base.
b)
has a neutral pH.
c)
is an acid.
d)
does not have a pH.
101.
The pH of a solution is tested, and it is found to be a basic solution. Of the following choices, what could the pH have been?
a)
3
b)
9
c)
7
d)
5
102.
Many cleaning solutions are bases. Which of the following is a property of most bases?
a)
feels slippery
b)
white color
c)
can only be liquid
d)
tastes sour
103.
Which of the following word pairs correctly completes the sentence below?
_______ are corrosive substances characterized as having a strong smell, a sour taste, and a _______.
a)
Acids; pH less than 7
b)
Acids; pH greater than 7
c)
Bases; pH greater than 7
d)
Bases; pH less than 7
104.
Tastes bitter.
a)
Acids
b)
Bases
c)
Salts
d)
All
105.
When dissolved in water, acids produce:
a)
bases
b)
salts
c)
hydrogen ions
d)
hydroxide ions
106.
Which type of ion does a base produce when it is dissolved in water?
a)
oxide
b)
oxygen
c)
hydrogen
d)
hydroxide
107.
A hydrogen ion, H+, is the same as a(n):
a)
neutron
b)
electron
c)
proton
d)
hydroxide ion
108.
A compound that changes color when it is in contact with an acid or base is called______________
a)
Acid
b)
Base 
c)
Neutral
d)
Indicator
109.
On the pH scale what numbers are bases?
a)
8-14
b)
0-7
c)
7
d)
1
110.
The pH scale measures...
a)
...the strength of an acid.
b)
...the strength of hydrogen ions.
c)
...the concentration of hydrogen ions.
d)
...the concentration of an acid
111.
Acid + base --> ?
a)
salt + hydrogen gas + water
b)
salt + carbon dioxide + water
c)
salt + water
d)
salt only
112.
What does a pH scale do?
a)
Tells you if a substance is an acid.
b)
Tells you if a substance is a base.
c)
Measures the strength or weakness of an acid or base.
d)
All of these are true.
113.
A(n) ______ is a substance with a pH less than 7
a)
Acid
b)
Alkaline
c)
Base
d)
Buffer
114.
A neutralization reaction will (almost) always produce...
a)
water & salt
b)
water
c)
salt
d)
water & carbon
115.

Complete the following reaction:

HCl + Mg(OH)2 -->

a)

MgCl2 + H2O

b)

Mg +H2O

c)

MgCl2 + H2

d)

MgCl2 + H2O + CO2

116.

What is the endpoint of a titration

a)

point of neutralization in a titration; pH = 7

b)

point where the moles of the ions are equal to each other

c)

When the volume of base in the burette is used up

d)

When there is no acid, only base

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