Download Honors Chemistry Semester 1 Exam Review

Chemistry Semester 2 Course Review
Name__________________________ Date___________ Per___
Italics indicate required honors extensions
Unit 9: Stoichiometry
Essential questions:

How does the amount of each reactant present at the start of a chemical reaction determine how much product forms?

How are balanced chemical equations used when solving stoichiometric problems?

What causes chemical reactions to stop?

What is a limiting reagent

What is the percent yield of a chemical reaction?
Key vocabulary:

reactant

product

stoichiometry

mole ratio




chemical reaction
limiting reactant
excess reactant
theoretical yield


actual yield
percent yield
Practice:
1. Differentiate between the significance of the coefficients in a balanced chemical equation and the significance of the subscripts in a
chemical formula. _________________________________________________________________________________________________
________________________________________________________________________________________________________________
________________________________________________________________________________________________________________
2.
State the Law of Conservation of Mass and explain its relationship to stoichiometry. ___________________________________________
________________________________________________________________________________________________________________
________________________________________________________________________________________________________________
________________________________________________________________________________________________________________
3.
mole-mole problem:
One disadvantage of burning propane (C3H8) is that carbon dioxide is one of the products. The released CO2 increases the
growing concentration of CO2 in the atmosphere. How many moles of carbon dioxide are produced when 10.0 moles of
propane are burned in excess oxygen on a gas grill?
4.
mole-mass problem:
Water decomposes to produce hydrogen gas and oxygen gas. How many grams of water would be required to
produce 10.0 moles of hydrogen gas?
5.
mass-mole problem:
If 25.0 grams of carbon dioxide are used in photosynthesis how many moles of glucose (C6H12O6) could be
Produced according to the following equation: 6CO2 + 6H2O  C6H12O6 + 6O2
6.
mass-mass problem:
One series of reactions that inflates air bags in automobiles is the decomposition of sodium azide (NaN3). Determine the
amount of N2 produced if 100.0 g of NaN3 is decomposed using the following unbalanced equation:
___NaN3  ___Na + ___N2
1
Chemistry Semester 1 Course Review
7.
8.
Name__________________________ Date___________ Per___
limiting reactant problem:
Nitrogen gas reacts with hydrogen gas to produce ammonia:
___N2 + ___H2  ___NH3
If 100.0 g of nitrogen gas reacts with 20.0 g of hydrogen gas what mass of ammonia will be produced?
*not balanced
Mass to mass and Percent Yield problem:
Iron reacts with oxygen to form Iron (III) oxide.
4Fe + 3O2  2Fe2O3.
a) If 200.0 g of iron reacts, what is the theoretical yield of iron (III) oxide?
b) If the actual yield is 205.4 g, what is the percent yield of the reaction?
Unit 10: States of Matter
Essential questions:

What is the relationship between temperature and kinetic energy?

How are degrees Celsius converting into Kelvin?

What are some examples of chemical properties? Physical properties?

What are some examples of some chemical changes? Physical changes?

How do intermolecular forces determine a substances state?

How do intermolecular forces determine the range of motion of particles in solids and liquids?

How do intermolecular forces determine the range of motion of particles in gases?

How are plasmas different from gases?

What makes matter change phase?

How does a phase change reach dynamic equilibrium?
Key vocabulary:

Polar covalent bond

dispersion force

dipole-dipole force

hydrogen bond

viscosity

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


surface tension
melting point
vaporization
evaporation
vapor pressure




boiling point
freezing point
condensation
deposition
Practice:
1.
Place a check in the box if the description applies to solids, liquids and/or gases. Each characteristic may apply to 1, 2 or all 3 states:
Solids
Liquids
Gases
Highly compressible
Fluid
Takes the shape of its container
Fills the volume of its container
Particles are far apart from one another
Molecules are moving
2
Physical Science Semester 1 Course Review
2.
Name__________________________ Date___________ Per___
Fill in the chart below: (a thru f)
a.
b.
Gases
c.
Liquids
d.
e.
Solids
f.
3.
Which of the above (a thru f) are exothermic? ________________________
4.
Which of the above (a thru f) are endothermic? ________________________
5.
Water boils when the ____________ pressure is equal to the __________________ pressure.
6.
How are temperature and the kinetic energy of molecules related?
________________________________________________________________________________________________________________
________________________________________________________________________________________________________________
7.
What is plasma? __________________________________________________________________________________________________
8.
Put hydrogen bonds, dispersion forces and dipole-dipole forces in order of how strong they are and give an example of each
type of attraction.
________________________________________________________________________________________________________________
________________________________________________________________________________________________________________
________________________________________________________________________________________________________________
________________________________________________________________________________________________________________
________________________________________________________________________________________________________________
________________________________________________________________________________________________________________
9.
Why do polar compounds tend to have higher melting boiling points than nonpolar compounds? ________________________________
____________________________________________________________________________________________________________________
____________________________________________________________________________________________________________________
Unit 11: Gases
Essential questions:

What is absolute zero?

How does the kinetic molecular theory explain the behavior of gases?

How are pressure units converted?

What is Daltons Law of partial pressures?

Why are they called Laws and not theories?

How are temperature, pressure and volume related?

What is Standard temperature and pressure?

How can the volume, pressure or temperature of a gas be calculated?

Can the amount of moles of a gas be related to the pressure, volume and temperature of the sample?

Do gases always follow the idea gas law?

How can balanced equations be used to calculate the volume of gases formed in chemical reactions?
Key vocabulary:

Kinetic molecular theory

elastic collision

temperature



pressure
absolute zero
combined gas law



molar volume
ideal gas law
ideal gas constant
3
Chemistry Semester 1 Course Review
Name__________________________ Date___________ Per___
Practice:
1. List the five main assumptions of the kinetic-molecular theory.
Spacing and particle size _________________________________________________________________________
Attraction/repulsion ____________________________________________________________________________
Movement ____________________________________________________________________________________
Collision type__________________________________________________________________________________
Temperature __________________________________________________________________________________
2.
What causes the pressure of a gas inside of a container? ____________________________________________
3.
What is the combined gas law? ________________________________________________________________
4.
What are Standard Temperature and Pressure?_____________________________________________________
5.
If the temperature of a weather balloon is increased how does the volume of the balloon change? _______________________________
6.
Combined gas law: A gas at 110 kPa and 30.0 oC fills a flexible container with an initial volume of 2.00 L. If the temperature is raised to
80.0 oC and the pressure is increased to 440 kPa, what will be the new volume?
7.
Combined gas law: What is the volume at STP :of a 125.0 mL of a gas at 1.50 atm and 100.0 oC
8.
Ideal gas law: What are the values (with units) for R, the ideal gas constant?
9.
Ideal gas law: Calculate the number of moles of gas contained in a 3.0 L vessel at 300. K with a pressure of 1.50 atm.
10. Molar volume: Hydrogen gas reacts with oxygen gas to produce water at STP. How many liters of hydrogen gas are required to produce
25.0 grams of water?
____H2 + ____O2  ____H2O
11. John puts 1250 PSI of Oxygen, 780 PSI of Nitrogen and 550 PSI if Helium in a SCUBA tank.
What is the total pressure?
12. Under what conditions do gases follow the Ideal gas Law? _____________________________________________________
Unit 12: Solutions
Essential questions:

What factors affect the formation of solutions?

How is concentration of a solution calculated using molarity?

How does a solution become saturated or supersaturated?

What factors affect the solubility of gases and solids in liquids?

What's the difference between strong, weak, and nonelectrolytes?

What properties of solutions are colligative properties?
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Chemistry Semester 1 Course Review







Name__________________________ Date___________ Per___
How does an increase in vapor pressure affect the colligative properties of a solution?
How would an equation be written for the dissociation of ionic solutes in water?
Why does oil not dissolve in water according to the factors that affect solubility?
How does an increase in temperature and pressure of a solution affect the solubility of the solute?
How does polarity of the solute and solvent affect the solubility of a solution?
Compare, contrast, and provide examples of suspensions, colloids, and solutions similar and different.
What does a solubility curve represent?
Key vocabulary:

solution

soluble

insoluble

solvation (hydration)

“like dissolves like”

solubility










saturated solution
unsaturated solution
supersaturated solution
concentration
molarity
colligative properties
suspension
colloids
electrolyte
nonelectrolyte
Practice:
1. In general, what two classes of materials will dissolve in water? __________________________________________
2.
Which is more concentrated, 10.0 grams of sugar in 100.0 mL of water or 10.0 grams of sugar in 125.0 mL of water?
________________________________________________________________________________________________
Why? ___________________________________________________________________________________________
3.
If a crystal of solute was added to each of the following types of solutions, what would happen?
unsaturated_______________________ saturated___________________ supersaturated ____________________
4.
What three classes of compounds are electrolytes? ___________________________________________________________
5.
Give two examples of nonelectrolytes. _____________________________________________________________________
6.
According to Reference Table G, which solution is
saturated at 30°C?
(1) 12 grams of KClO3 in 100 grams of water
(2) 12 grams of KClO3 in 200 grams of water
(3) 30 grams of NaCl in 100 grams of water
(4) 30 grams of NaCl in 200 grams of water
7.
According to Reference Table G, the solubility of which
compound is least affected by a change in temperature?
________
5
Chemistry Semester 1 Course Review
8.
Fill out the chart to show how the addition of a solute to a solvent will affect the melting point (MP) and the boiling point (BP) of the
solution, and why these temperatures are affected.
Condition Required to change the
phase of the pure liquid
Affect of adding solute
9.
Name__________________________ Date___________ Per___
Boiling Point
Melting point
__________ pressure is equal to
__________ pressure
Kinetic energy of particles
overcomes ____________
attractive forces present in the solid
state.
Boiling Point is ______________
because the number of solvent
particles at the surface is reduced
thereby lowering the vapor
pressure requiring a/an
__________ in temperature to
achieve atmospheric pressure.
Melting point is _____________
because solute particles dirupt
interparticle attractive forces
allowing melting to occur at a
_______ temperature.
A 100.5 mL intraveneous (IV) solution contains 5.10 g glucose (C6H12O6). What is the molarity of this solution?
10. How many grams of sodium hydroxide are required to prepare 500.0 mL of a 2.00 M solution?
11. Solubility of solids and gases:
Factors that affect solvation rate of SOLIDS in liquids:
Temperature of the solution increases
The mixture is stirred
The solid is broken into smaller pieces
Factors that affect solubility of GAS in a liquid:
Temperature of the solution increases
The pressure over the gas is decreased
The pressure over the gas is increased
The rate of the solvation...(Circle your choice)
Increases
Decreases
Increases
Decreases
Increases
Decreases
The solubility of the gas in the liquid…(Circle choice)
Increases
Decreases
Increases
Decreases
Increases
Decreases
Unit 13: Thermochemistry
Essential questions:

What are some types of renewable and nonrenewable energy resources?

What is energy and how is it measured?

What is the difference between temperature and heat energy?

What is an endothermic process and what is the sign for ΔH for the process? What is an exothermic process and what is the sign for ΔH
for the process?

What is the SI unit for energy?

How are system, surroundings, and universe defined in thermochemistry?

How is the Law of Conservation of Energy applied using calorimetry?

What is specific heat capacity? Why does it take more heat to change the temperature of water compared to metals?
Key vocabulary:

thermochemistry

absolute zero

calorie



joule
energy
law of conservation of energy



heat
specific heat
calorimeter
6
Chemistry Semester 1 Course Review



surroundings
system
universe
Name__________________________ Date___________ Per___



endothermic
exothermic
renewable energy source


nonrenewable energy source
chemical potential energy
Practice:
1. What is the derived unit for specific heat? ___________
2.
Select the word in the parenthesis that makes the statement true: An object with a higher specific heat requires (more / less) heat to
raise its temperature.
3.
How many kJ are equal to 500.0 calories?
4.
What is the SI unit for energy/heat? __________
5.
Select the word in the parenthesis that makes the statement true: An (endothermic/exothermic) reaction releases heat so the container
would feel (warm/cold) while an (endothermic/exothermic) reaction absorbs heat from the surroundings so the container would feel
(warm/cold).
6.
Select all the phrases in the parenthesis that make the
statement true: The flat lines on a heating curve represent
(a temperature change/ a constant temperature/ a change
of state).
7.
Select all the phrases in the parenthesis that make the
statement true: The sloped lines on a heating curve
represent (a temperature change/ a constant
temperature/ a change of state).
8.
Select all the phrases in the parenthesis that make the
statement true: It takes longer for substances to (melt /
boil) because the heat of vaporization is (higher / lower)
than the heat fusion.
9.
When a hot object is put in cooler water, what will happen to the temperature of the object? ____________ to the temperature of the
water?_____________
10. Convert 25oC to Kelvin. _________
Convert 25K to oC. __________
11. Why are there no negative temperatures in the Kelvin system? __________________________________________
12. Which statement describes characteristics of an endothermic reaction?
__The sign of H is positive, and the products have less potential energy than the reactants.
__The sign of H is positive, and the products have more potential energy than the reactants.
__The sign of H is negative, and the products have less potential energy than the reactants.
__The sign of H is negative, and the products have more potential energy than the reactants.
13. Select all the phrases in the parenthesis that make the statement true: The average kinetic energy of a substance’s molecules (increases
/ decreases) as it cools from 273K to 263K?
14. Select all the phrases in the parenthesis that make the statement true: Solid X is placed in contact with solid Y. Heat will flow
spontaneously from X to Y when (X is 20°C and Y is 20°C / X is 10°C and Y is 5°C / X is -25°C and Y is -10°C / X is 25°C and Y is 30°C).
15. What is the total number of joules of heat energy absorbed by 15 grams of water when it is heated from 30°C to 40°C?
7
Chemistry Semester 1 Course Review
Name_________________________
16. The heat of fusion of a compound is 30 joules per gram. What is the total number of joules of heat that must be absorbed by a 15.0 gram
sample to change the compound from a solid to a liquid at its melting point?
17. Salt A and salt B were dissolved separately in 100 mL beakers of water. The water temperatures were measured and recorded as shown
in the table below:
Salt A:
Salt B:
initial water temp.
25.1°C
25.1°C
final water temp.
30.2°C
20.0°C
Select all the phrases in the parenthesis that make the statement
true:
The dissolving of (only salt A was endothermic/ only salt B was
exothermic/ both salt A and salt B were endothermic/
salt A was exothermic and the dissolving of salt B was endothermic).
Unit 14: Acids and Bases
Essential questions:

What is the definition of an acid? Base?

What are the properties of acids? Bases?

What is the purpose of an indicator? Give an example.

What are some common acids and bases?

What is pH? What is the pH range of an acid? Of a base? Of a neutral?

How can you identify a neutralization reaction?

How does a scientist use a titration experiment to calculate the concentration of an unknown solution?

What are the causes and environmental effects of acid rain?
Key vocabulary:

acidic solution

Arrhenius acid

Arrhenius base

basic solution

Bronsted-Lowry acid

Bronsted-Lowry base

conjugate acid

conjugate base

conjugate acid-base pair









strong acid
weak acid
strong base
weak base
ion product constant for water
pH
pOH
acid-base indicator
buffer
Practice:
1. List at least 5 properties of acid and bases in the table:
Acid









end point
equivalence point
neutralization reaction
salt
titration
monoprotic
diprotic
acid rain
Base











8
Chemistry Semester 1 Course Review
2.
3.
Name_________________________
Compare and contrast the Arrhenius and Bronsted-Lowry:
Arrhenius
Bronsted-Lowry
Differentiate between strong and weak acids and bases (i.e. What makes an acid strong?) __________________________
________________________________________________________________________________________________
4.
Conjugate acid/base pairs - Using the equation below, label the: acid, base, conjugate acid, conjugate base
NH3
+
H2O
-->
NH4+
+
OH-
5.
[H+], [OH-], pH, pOH Fill in the chart below:
[H+]
[OH-]
pH
pOH
acid/base
1.0 X 10-3M
2.0 X 10-3M
5
12.2
6.
Predict the products for this neutralization reaction: HCl + NaOH --> _________ + __________
7.
The data collected from a laboratory titration are used to calculate the (chose one)
(1) rate of a chemical reaction
(3) concentration of a solution
(2) heat of a chemical reaction
(4) boiling point of a solution
8.
A student completes a titration by adding 12.0 milliliters of NaOH(aq) of unknown concentration to 16.0 milliliters of
0.15M HCl(aq). What is the molar concentration of the NaOH(aq)?
9.
Acids react with many metals. What will be the second product of the reaction below?
HCl + Mg ---> MgCl2 (aq) + ________(g)
10.
Which of these pH numbers indicates the highest level of acidity? (a) 5
11.
A solution with a pH of 2.0 has a hydrogen ion concentration ten times greater than a solution with a pH of:
(a) 1.0 (b) 3.0 (c) 0.20 (d) 20
12.
Which compound is an Arrhenius acid? (1) H2SO4
13.
According to one acid-base theory, water acts as an acid when an H2O molecule
(1) accepts an H+
(2) donates an H+
(3) accepts an H-
(2) KCl
(b) 8
(3) NaOH
(c) 10
(d) 12
(4) NH3
(4) donates an H-
9
Chemistry Semester 1 Course Review
14.
Name_________________________
Given the reaction:
HCl(aq) + LiOH(aq) → HOH(ℓ) + LiCl(aq)
The reaction is best described as:
(1) neutralization
(2) synthesis
15.
(3) decomposition (4) oxidation-reduction
What are some possible sources of the acids in the atmosphere that contribute to acid rain? ______________________
_______________________________________________________________________________________
Unit 15: RedOx
Essential questions:

What types of reactions are also classified as redox reactions?

What happens during oxidation and reduction?

How are oxidation numbers assigned?

How are half-reactions classified as oxidation or reduction?
Key vocabulary:

Redox

Oxidation



Reduction
Oxidizing Agent
Reducing Agent
Practice:
1. What happens during oxidation? _______________________________________
2. What happens during reduction? _______________________________________
3. List several common redox reactions: _________________________________________________________________________________
________________________________________________________________________________________________________________
4.
5.
Half reactions: Write the correct half reaction in the space provided.
Br + 1 e-  Br –
Mg 
a. Oxidation Half reaction ________________________________
Mg +2 + 2 e-
b.
Reduction Half reaction ________________________________
c.
Balance the equation. __________________________________________
Put it all together. Show the oxidation number of each element:
K(s)
____
+
Br2 (g)
____

KBr (s)
___ ____
a.
Which substance is oxidized? _________
b.
Which substance is reduced? _________
c.
What is the oxidizing agent? _________
d.
What is the reducing agent? _________
e.
Balance the equation. __________________________________________
Unit 16: Reaction Rates
Essential questions:

What factors impact the rate of a chemical reaction, and how is the rate changed for each factor?

How are endothermic and exothermic reactions represented in an energy diagram?

What is a catalyst? How does a catalyst work?

What is a reversible reaction?

What do molecular clocks have to do with reaction rates?
10
Chemistry Semester 1 Course Review
Key vocabulary:

Collision Theory

Reaction Rate
Name________________________ Date___________ Per___




Concentration
Surface Area
Catalyst
Molecular Clocks
Practice:
1. What do molecular clocks have to do with reaction rates?
______________________________________________________________________________________
2.
How does each factor affect the rate of a chemical reaction?
Factors that affect reaction rate:
Concentration of the reactants increases
Concentration of the reactants decreases
Temperature increases
Temperature decreases
An inhibitor is added
A catalyst is added
The pressure of a reactant gas is increased
The pressure of a reactant gas is decreased
The rate of the reaction…. (Circle your choice)
Increases
Decreases
Increases
Decreases
Increases
Decreases
Increases
Decreases
Increases
Decreases
Increases
Decreases
Increases
Decreases
Increases
Decreases
3.
Draw and label the following reaction diagrams. Be sure to label the activation energy (∆Ea) and the change in heat (∆H) on each
diagram:
Exothermic
Exothermic with a Catalyst
Endothermic
4.
Fill in the missing terms: A _______________ speeds up a reaction by lowering the ________________ ______________
Unit 17: Nuclear Chemistry
Essential questions:

What happens when an unstable nucleus decays?

How is the structure of atoms altered during fission and fusion?

How are nuclear reactions classified and balanced?

What is the difference between a chemical reaction and a nuclear reaction?

How does nuclear chemistry explain the natural world and affect your life? (fission and fusion in nature, half-life in fossil dating and
molecular clocks and tumor location, nuclear reactions in fire detectors, cancer treatment, and power production)

What are the impacts on the environment from nuclear production?

How is a graph used to determine the half-life of a radioactive isotope or how much radioisotope will be present in a sample after a given
time period?
Key vocabulary:

Fission

Fusion

Radioactive Decay



Radioactive isotope
(Radioisotope)
Alpha radiation
Beta radiation




Gamma radiation
Half-life
Radioisotope tracer
Exponential decay
11
Chemistry Semester Course Review
Name__________________________ Date___________ Per___
Practice:
1. Compare and contrast alpha, beta and gamma radiation:
Attribute
Alpha radiation
Symbols
Beta radiation
Gamma radiation
Mass
Charge
Penetrating ability
2.
Compare radioactive decay, nuclear fission and nuclear fusion:
Comparison Category
Radioactive decay
Nuclear fission
Nuclear fusion
Define
Natural occurrences
Technological uses
3.
4.
Yucca Mountain is the proposed site for a national repository for high level nuclear waste generated from military functions, nuclear medicine,
nuclear power, and nuclear research. Identify 3 characteristics of this site that make it suitable for this purpose:
a.
______________________________________________________________________________________________
b.
______________________________________________________________________________________________
c.
______________________________________________________________________________________________
What are the advantages and disadvantages of using nuclear power plants to generate electricity?
Advantages
Disadvantages
12
Chemistry Semester Course Review
5.
Name__________________________ Date___________ Per___
Compare and contrast nuclear reactions and chemical reactions:
Comparison Category
Nuclear reactions
Chemical reactions
Fundamental Forces Responsible
Subatomic particles affected
Relative amount of energy released
Current applications as an energy
source
Future applications as energy source
6.
In the nucleus, why don’t the positive protons fly apart from electrostatic repulsion? _______________________________________________
____________________________________________________________________________________________________________________
7.
8.
Balance the following nuclear reactions:
 _____ +
a.
99 Tc
43
b.
239 Pu
94
c.
239 Np
93


4
2He
0 e
-1
d.
42 K
19
+ _____
e.
1 H
1
239 Pu
94

+
0 e
-1
3 H
1

+ _____
_____
+ _____
Interpret the graph to answer the questions:
a.
What is the initial mass? __________________
b.
What is the half-life? __________________
c.
What mass remains after 3.0 half-lives? ___________
d.
What mass remains after 10 time units? __________
e.
After how many half-lives will 200 pounds remain?
___________
13