name: period: chemistry i honors semester 2 exam...

Name: ___________________________________________________________________ Period: __________

CHEMISTRY I HONORS SEMESTER 2 EXAM REVIEW

1 L. Tait

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. 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? ___C3H8 + ___O2 ___CO2 + ___H2O

4. 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? ___H2O ___H2 + ___O2

5. 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. One series of reactions that inflates air bags in automobiles is the decomposition of sodium azide (NaN3). Determine the amount in grams of N2 produced if 100.0 g of NaN3 is decomposed using the following unbalanced equation: ___NaN3 ___Na + ___N2

Chemistry Semester 2 Exam Review Last Name_________________________ Per___

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7. 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?

8. 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?


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Unit10: 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

surface tension

melting point

vaporization

evaporation

vapor pressure

boiling point

freezing point

condensation

deposition

Practice: 9. 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

10. Fill in the chart below with the appropriate phase change: (a thru f)

a.

b. c.

d. e.

f.

11. Which of the above (a thru f) are exothermic? ___________________Which of the above (a thru f) are endothermic? ___________________

12. Water boils when the ____________ pressure is equal to the __________________ pressure.

13. How are temperature and the kinetic energy of molecules related? _____________________________________________________________

____________________________________________________________________________________________________________________

14. What is plasma? ______________________________________________________________________________________________________

____________________________________________________________________________________________________________________

Gases Liquids Solids


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15. 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.

____________________________________________________________________________________________________________________

____________________________________________________________________________________________________________________

____________________________________________________________________________________________________________________

____________________________________________________________________________________________________________________

____________________________________________________________________________________________________________________

16. Why do polar compounds tend to have higher melting boiling points than nonpolar compounds?

____________________________________________________________________________________________________________________

____________________________________________________________________________________________________________________

____________________________________________________________________________________________________________________

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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 Practice: 17. List the five main assumptions of the kinetic-molecular theory.

Spacing and particle size ________________________________________________________________________________________________

Attraction/repulsion ___________________________________________________________________________________________________

Movement __________________________________________________________________________________________________________

Collision type_________________________________________________________________________________________________________

Temperature _________________________________________________________________________________________________________

18. What causes the pressure of a gas inside of a container? ______________________________________________________________________

19. What is the combined gas law? __________________________________________________________________________________________

20. What are Standard Temperature and Pressure?_____________________________________________________________________________

21. If the temperature of a weather balloon is increased how does the volume of the balloon change?____________________________________

22. 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?

23. What is the volume of a 125.0 mL of a gas at 1.50 atm and 100.0 oC at STP?

24. What are the values (with units) for R,the ideal gas constant? 25. Calculate the number of moles of gas contained in a 3.0 L vessel at 300.K with a pressure of 1.50 atm.


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26. 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

27. John puts 1250 PSI of Oxygen, 780 PSI of Nitrogen and 550 PSI if Helium in a SCUBA tank. What is the total pressure?

28. Under what conditions do gases follow the Ideal gas Law?_____________________________________________________________________


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Unit 12: Solutions Essential questions:

What factors affect the formation of solutions?

How is the 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?

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: 29. In general, what two classes of materials will dissolve in water? ________________________________________________________________

30. 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? _______________________________________________________________________________________________________________

31. Solubility of solids and gases:

Factors that affect solvation rate of SOLIDS in liquids: The rate of the solvation...(Circle your choice)

Temperature of the solution increases Increases Decreases

The mixture is stirred Increases Decreases

The solid is broken into smaller pieces Increases Decreases

Factors that affect solubility of GAS in a liquid: The solubility of the gas in the liquid…(Circle your choice)

Temperature of the solution increases Increases Decreases

The pressure over the gas is decreased Increases Decreases

The pressure over the gas is increased Increases Decreases

32. If a crystal of solute was added to each of the following types of solutions, what would happen?

unsaturated___________________________ saturated___________________________ supersaturated ___________________________

33. What three classes of compounds are electrolytes? _________________________________________________________________________

34. Give two examples of nonelectrolytes. ____________________________________________________________________________________


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35. According to Reference Table G, which solution is

saturated at 30°C? (circle one)

(a) 12 grams of KClO3 in 100 grams of water

(b) 12 grams of KClO3 in 200 grams of water

(c) 30 grams of NaCl in 100 grams of water

(d) 30 grams of NaCl in 200 grams of water

36. According to Reference Table G, the solubility of

which compound is least affected by a change in

temperature? _____________

37. 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.

Boiling Point Melting point

Condition Required to change the

phase of the pure liquid

__________ pressure is equal to

__________ pressure

Kinetic energy of particles

overcomes ____________

attractive forces present in the solid

state.

Affect of adding solute

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

disruptinter-particle attractive

forces allowing melting to occur at a

_______ temperature.

38. A 100.5 mL intravenous (IV) solution contains 5.10 g glucose (C6H12O6). What is the molarity of this solution? 39. How many grams of sodium hydroxide are required to prepare 500.0 mL of a 2.00 M solution?


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Unit 13: Thermochemistry& Reaction Rates 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?

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? Key vocabulary:

thermochemistry

absolute zero

calorie

joule

energy

law of conservation of energy

heat

specific heat

calorimeter

surroundings

system

universe

endothermic

exothermic

renewable energy source

nonrenewable energy source

chemical potential energy

Collision Theory

Reaction Rate

Concentration

Surface Area

Catalyst

Molecular Clocks

Practice: 40. What is the derived unit for specific heat? ___________

41. 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.

42. How many kJ are equal to 500.0 calories?

43. What is the SI unit for energy/heat? __________

44. 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).

45. 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).

46. 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).

47. 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.

48. When a hot object is put in cooler water, what will happen to the temperature of the object? ____________ To the temperature of the

water?_____________

49. Convert 25oC to Kelvin. _________ Convert 25K to oC. __________


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50. Why are there no negative temperatures in the Kelvin system? ________________________________________________________________

51. Which statement describes characteristics of an endothermic reaction? (check one)

____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.

52. 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.

53. 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).

54. What is the total number of joules of heat energy absorbed by 15 grams of water when it is heated from 30.0°C to 40.0°C?The specific heat of

water is 4.184 J/g°C.

55. The heat of fusion of water is 6.01 kilojoules per mole. What is the total number of kilojoules of heat that must be absorbed by a 15.0 gram

sample to change the compound from a solid to a liquid at 0°C?

56. 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:

initial water temp. final water temp.

Salt A: 25.1°C 30.2°C

Salt B: 25.1°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).

57. How does each factor affect the rate of a chemical reaction?

Factors that affect reaction rate: The rate of the reaction…. (Circle your choice)

Concentration of the reactants increases Increases Decreases

Concentration of the reactants decreases Increases Decreases

Temperature increases Increases Decreases

Temperature decreases Increases Decreases

An inhibitor is added Increases Decreases

A catalyst is added Increases Decreases

The pressure of a reactant gas is increased Increases Decreases

The pressure of a reactant gas is decreased Increases Decreases

58. 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

59. Fill in the missing terms: A _______________ speeds up a reaction by lowering the ________________ ______________


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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

end point

equivalence point

neutralization reaction

salt

titration

monoprotic

diprotic

acid rain

Practice: 60. List at least 5 properties of acid and bases in the table:

Acid Base

61. Acids react with many metals. What will be the second product of the reaction below?

HCl + Mg ---> MgCl2 (aq) + ________(g)

62. Which of these pH numbers indicates the highest level of acidity? (a) 5 (b) 8 (c) 10 (d) 12

63. 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

64. Compare and contrast the Arrhenius and Bronsted-Lowry:

Arrhenius Bronsted-Lowry

65. Differentiate between strong and weak acids and bases (i.e. what makes an acid strong?) ___________________________________________

________________________________________________________________________________________________________________________


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66. Conjugate acid/base pairs - Using the equation below, label the: acid, base, conjugate acid, conjugate base

NH3 + H2O -->NH4+ + OH-

67. [H+], [OH-], pH, pOH Fill in the chart below:

[H3O+] [OH-] pH pOH acid/base

1.0 X 10-3M

2.0 X 10-3M

5.2

12.2

68. Predict the products for this neutralization reaction: HCl + NaOH --> _________ + __________

69. The data collected from a laboratory titration are used to calculate the (chose one)

(1) rate of a chemical reaction

(2) heat of a chemical reaction

(3) concentration of a solution

(4) boiling point of a solution

70. 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)?

71. Which compound is an Arrhenius acid? (1) H2SO4 (2) KCl (3) NaOH (4) NH3

72. 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- (4) donates an H-

73. Given the reaction: HCl(aq) + LiOH(aq) → HOH(ℓ) + LiCl(aq)

The reaction is best described as: (circle one)

(1) neutralization (2) synthesis (3) decomposition (4) oxidation-reduction

74. What are some possible sources of the acids in the atmosphere that contribute to acid rain?_________________________________________

____________________________________________________________________________________________________________________


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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: 75. What happens during oxidation? _______________________________________

76. What happens during reduction? _______________________________________

77. List several common redox reactions: _________________________________________________________________________________

________________________________________________________________________________________________________________

78. Half reactions: Write the correct half reaction in the space provided.

Br + 1 e- Br – Mg Mg +2 + 2 e-

a. Oxidation Half reaction ________________________________

b. Reduction Half reaction ________________________________

c. Balance the equation. __________________________________________

79. 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. __________________________________________________


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Unit 16: 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

Practice: 80. Compare and contrast alpha, beta and gamma radiation:

Attribute Alpha radiation Beta radiation Gamma radiation

Symbols

Mass

Charge

Penetrating ability

81. Balance the following nuclear reactions:

a. 𝑇𝑐4399 _______ + 𝑒−1

0

b. 𝑃𝑢94239 𝐻𝑒2

4 + _______

c. 𝑁𝑝93239 𝑃𝑢94

239 + _______

d. 𝐾1942 𝑒−1

0 + _______

e. 𝐻11 + 𝐻1

3 _______

82. In the nucleus, why don’t the positive protons fly apart from electrostatic repulsion? _______________________________________________

____________________________________________________________________________________________________________________

83. Compare radioactive decay, nuclear fission and nuclear fusion:

Comparison Category Radioactive decay Nuclear fission Nuclear fusion

Define

Natural occurrences

Technological uses


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84. What are the advantages and disadvantages of using nuclear power plants to generate electricity?

Advantages Disadvantages

85. 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

86. 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 half-lives? __________

e. After how many half-lives will 200. pounds remain?

___________ (show calculation)

name: period: chemistry i honors semester 2 exam...

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