Unit A: Chemical Change

Chapter and Unit Review Questions

Chapter 1 Review Questions

Knowledge

1.	An atom has an atomic mass of 9.01 and an atomic number of 4.
	a.	Determine the identity of the atom.
	b.	Determine the number of neutrons the atom has.
	c.	Draw a Bohr diagram for the atom.
	d.	Draw a Lewis dot diagram for the atom.
	e.	Determine the number of valence electrons this atom has.
	f.	Write the symbol of the ion for this atom. Explain the reason for the net charge on this ion.

2.	An atom has an atomic mass of 32.06 and an atomic number of 16.
	a.	Determine the identity of the atom.
	b.	Determine the number of neutrons in the most common form of the atom.
	c.	Draw a Bohr diagram for the atom.
	d.	Draw a Lewis dot diagram for the atom.
	e.	Determine the number of valence electrons this atom has.
	f.	Write the symbol of the ion for this atom. Explain the reason for the net charge on this ion.

3.	Consider the following compounds. carbon tetrachloride, CCl₄(l) hydrogen fluoride, HF(g) potassium iodide, KI(s) magnesium oxide, MgO(s)
	a.	Which compounds are ionic and which are molecular?
	b.	Draw Lewis dot diagrams of the individual atoms that comprise these compounds.
	c.	Draw diagrams to illustrate the bonding between particles in each of the four compounds.

A fireproof safe contains an ionic compound, CaCO₃(s), between the inside and outside layers of metal. The particles of this compound do not respond to the heat released by a fire the same way the particles in the metal do. Explain how these different responses to heat are due to the different forms of chemical bonds in these materials. Describe how the presence of the CaCO₃(s) in the safe’s construction protects the contents against damage from the heat.

Classify each substance as being either a molecular compound or an ionic compound. Determine whether it will dissolve in water and whether it is classified as an electrolyte or a non-electrolyte.

	a.	NaF(s)
	b.	CH₄(g)
	c.	Li₂O(s)
	d.	AlCl₃(s)
	e.	C₅H₁₂(l)

6.	Define dissociation. Use a diagram to explain why NaCl(s) will dissociate when placed in water.
7.	Describe the differences between the changes that occur to solute particles that form a solution by undergoing dissociation and to the changes that occur to solute particles that form a solution but do not dissociate.
8.	Give two reasons why a concentrated solution of sulfuric acid is more dangerous than a dilute solution of sulfuric acid.
9.	Explain why it is a common safety procedure to flush skin with plenty of water when it comes into contact with a concentrated acid.

Applying Concepts

10.

You dissolve 280 g of sucrose (table sugar), C₁₂H₂₂O₁₁(s), in 2.00 L of water.

	a.	Determine the number of moles of sugar in this solution.
	b.	Calculate the molar concentration of this solution.

11.

You dissolve 16.0 g of potassium sulfate, K₂SO₄(s), in 500 mL of water.

	a.	Determine the number of moles of potassium sulfate in this solution.
	b.	Calculate the molar concentration of this solution.

12.

A solution contains 100 ppm of lead. Determine the mass of lead present in 0.500 kg of the solution.

13.

While visiting an ocean beach in Nova Scotia, you notice the following sign above the sinks in the changing room.

If someone was to ignore this sign and drink 250 g of water, they would consume about 9.5 ×10^–6 g of arsenic. Calculate the concentration of the arsenic in this water in parts per million.

The maximum acceptable level of arsenic in drinking water is 0.025 ppm. Drinking water with an arsenic concentration of 60 ppm is lethal. Use this information and your answer to question 13.a. to determine if drinking a cup of water from this tap would be lethal.

There are places on Earth where the only drinking water available to people contains high levels of arsenic. Use the Internet to locate a place where the arsenic contamination of drinking water creates major health problems for the population. What is the source of the arsenic contamination in this place?

Arsenic has been used as a poison for centuries. Use the Internet to survey the evidence that suggests that Napoleon Bonaparte was poisoned with arsenic while imprisoned on the tiny island of St. Helena.

14.

Determine how many moles of solute are dissolved in each of the following solutions.

	a.	a 250-mL solution of sucrose, C₁₂H₂₂O₁₁(aq), with a concentration of a 0.500 mol/L
	b.	a 5.00-L solution of potassium sulfate, K₂SO₄(aq), with a concentration of 0.0250 mol/L

15.

Determine the number of moles of solute and the mass of the solute dissolved in each of the following solutions.

	a.	a 250-mL solution of sucrose, C₁₂H₂₂O₁₁(aq), with a concentration of 0.146 mol/L
	b.	a 4.00-L solution of potassium sulfate, K₂SO₄(aq), with a concentration of 0.150 mol/L

16.

Determine the volume of solution required for the following situations.

	a.	You wish to obtain 3.89 g of sucrose, C₁₂H₂₂O₁₁(s), from a 0.0675-mol/L sugar solution.
	b.	You wish to prepare a 6.26-g potassium sulfate solution, K₂SO₄(aq), with a concentration of 0.0250 mol/L.

17.

An amount of sucrose, C₁₂H₂₂O₁₁(s), is needed to prepare 500 mL of a sugar solution with a concentration of 0.783 mol/L.

	a.	Calculate the number of moles of sucrose that will be needed for this solution.
	b.	Calculate the mass of sucrose required to make this solution.

18.

An amount of sodium chloride, NaCl(s), is needed to prepare 1.25 L of a salt solution with a concentration of 0.750 mol/L.

	a.	Calculate the number of moles of sodium chloride that will be needed for this solution.
	b.	Calculate the mass of sodium chloride required to make this solution.

19.	While removing rust from the bumper of a vintage automobile, a can containing 95.0 mL of an acid-based rust remover is left out in the hot sun. After some time, 15.0 mL of the water evaporates from this can. If the acid’s original concentration was 2.30 mol/L, determine the new concentration of the acid.
20.	While cleaning a toilet, 150 mL of disinfectant solution is poured into a toilet containing 750 mL of water. If the initial concentration of the disinfectant was 3.40 mol/L, determine the new concentration of the solution.

Use the following information to answer questions 21 to 27.

Case Study: The Chemistry of Shampoo

Despite claims from the manufacturers, shampoo cannot enliven, nourish, or revive hair. This is because the part of hair that appears above the scalp is basically a shaft of protein molecules produced by cells in the scalp. Individual hairs are lubricated and protected by a natural oil, called sebum, which is produced by tiny glands located at the base of each hair. Unfortunately, sebum naturally tends to collect dirt as well as residues from hair-care products. The goal of shampoo is to remove the oily layer of sebum and any dirt that this layer may have accumulated on the shafts of the hairs. The challenge is that this oily layer must be removed in the watery environment of the shower. Water is a poor solvent for oil.

Shampoo manufacturers have solved this problem by including detergent substances in their products. Detergents are a type of surfactants—short for “surface active agents.” The detergent property of the solutions removes the oil, and the surfactant property means that the shampoo will rinse out of the hair easily in water.

Surfactants work because one end of these long molecules consists of a tail of hydrocarbons that can attach itself to oily substances. At the other end of these molecules is a head that can be ionized and, therefore, be attracted to water molecules. If the head of the surfactant carries a negative charge, it is called anionic. If the head carries a positive charge, the surfactant is called cationic. Shampoos usually consist of a group of anionic surfactants mixed with other ingredients in a water-based solution.

INGREDIENTS IN BRAND X SHAMPOO

Name of Ingredient	Volume (mL)	Function
water	109.3	acts to dissolve other ingredients
ammonium lauryl sulfate solution	109.0	anionic surfactant
ammonium laureth sulfate solution	106.5	anionic surfactant
ammonium dodecylbenzene sulfonate solution	12.0	anionic surfactant
lauramide DEA solution	10.5	high-foaming surfactant
dimethicone solution	2.0	a coating that replaces the sebum, providing shine and easy combing
disodium EDTA solution	0.7	preservative to keep shampoo from “spoiling”
Total	350.0

Shampoos work because the tail of the surfactant molecule secures itself to the oily layer of sebum while the anionic head attracts water molecules. When you rinse out the shampoo, the sebum is also washed away.

21.	Identify an ingredient in the shampoo that could be classified as the solvent.
22.	Identify an ingredient in the shampoo that could be classified as a solute.
23.	Explain how neutral water molecules could be attracted to the charged head of an anionic surfactant. Draw a diagram to support your answer.

24.

Calculate the percent by volume concentration of the following ingredients in the shampoo.

	a.	ammonium lauryl sulfate solution
	b.	ammonium laureth sulfate solution
	c.	ammonium dodecylbenzene sulfonate solution
	d.	dimethicone solution

25.	The main protein in hair is keratin. An interesting property of keratin in hair is that its molecular structure tends to have a high percentage of negative charges on its outer surface. This means that the outer surface of each shaft of hair tends to have a slightly negative charge.

	a.	Explain how the slightly negative charge along the length of a hair actually assists in the rinsing of the anionic surfactants from the hair after shampooing.
	b.	Explain why dry hair tends to stand up and “fly away” after it has been combed.

26.	Use your understanding of the properties of different groups of molecules to explain the following statement from the information box: “Water is a poor solvent for oil.”

27.

Manufacturers are required to list the ingredients in shampoo in order of decreasing concentration. However, they are not required to state numerical values for the concentration of each ingredient because this would reveal the exact recipe of the shampoo—something considered to be a trade secret. Locate a bottle of shampoo in your home.

	a.	List the first three ingredients on your bottle of shampoo.
	b.	How many ingredients are listed in total?
	c.	Suggest some of the tests that would have to be performed on each of these ingredients before they could be approved for use in shampoo.

Chapter 2 Review Questions

Knowledge

1.	For each of the following reactions, state whether oxidation or reduction will occur, determine the number of electrons gained or lost, and write a balanced half-reaction.

	a.	Sn⁴⁺(aq) Sn²⁺(aq)
	b.	Na⁺(aq) Na(s)
	c.	S(s) S^2–(aq)
	d.	2 F^–(g) F₂(aq)
	e.	As(s) As^3–(aq)
	f.	Gold atoms convert into gold ions.
	g.	Nitride ions convert into nitrogen gas.

Using the activity series, write the oxidation half-reaction that describes each of the following changes.

	a.	An atom of lithium reacts to form a lithium ion.
	b.	An atom of copper reacts to form a copper(II) ion.

3.	Examine the following balanced chemical equations: Mg(s) + Cl₂(g) MgCl₂(s) 2 Ni(s) + O₂(g) 2 NiO(s) Ag₂S(s) + Ca(s) CaS(s) + 2 Ag(s)
	a.	Identify the chemical substances being oxidized.
	b.	Identify the chemical substances being reduced.
	c.	Identify any ions that do not undergo oxidation or reduction during the reaction (spectators).

4.	Refer to the balanced chemical equations in question 3.

	a.	Determine the number of electrons gained by each atom or ion.
	b.	Determine the number of electrons lost by each atom or ion.

5.	Determine whether the following substances could undergo oxidation, reduction, or both.

	a.	lithium atom, Li(s)
	b.	hydride ion, H^–(aq)

Applying Concepts

6.	If you place a strip of aluminium metal into hydrochloric acid, you will obtain hydrogen gas. The balanced chemical equation that describes this process is 2 Al(s) + 6 HCl(aq) 2 AlCl₃(aq) + 3 H₂(g)

	a.	State the chemical substance that is gaining electrons. Provide a reason for your choice.
	b.	State the chemical substance that is losing electrons. Provide a reason for your choice.
	c.	State the chemical substance that is neither gaining nor losing electrons. Provide a reason for your choice.
	d.	State the atom or ion that is being oxidized.
	e.	How many moles of aluminium metal are required to make 300 mol of hydrogen gas?
	f.	How many moles of hydrochloric acid are required to make 300 mol of hydrogen gas?

7.	Balance the following reactions.

	a.	HCl(aq) + Zn(s) ZnCl₂(aq) + H₂(g)
	b.	Pb(NO₃)₂(aq) + Cu(s) Cu(NO₃)₂(aq) + Pb(s)
	c.	AgNO₃(aq) + Cu(s) Cu(NO₃)₂(aq) + Ag(s)
	d.	AuCl₃(aq) + Zn(s) ZnCl₂(aq) + Au(s)

8.	Aspirin, C₉H₈O₄(s), is easily made by reacting salicylic acid, C₇H₆O₃(aq), and acetic anhydride, C₄H₆O₃(s). This is described by the chemical reaction 2 C₇H₆O₃(aq) + C₄H₆O₃(s) 2 C₉H₈O₄(s) + H₂O(l) You have 3.56 mol of acetic anhydride.

	a.	How many moles of aspirin could you produce?
	b.	How many moles of water will this reaction produce?
	c.	How many moles of salicylic acid will you need?

Cement is primarily made up of a substance called quicklime, CaO(s). Quicklime is created by using heat to decompose limestone, CaCO₃(s). A by-product of this reaction is carbon dioxide, CO₂(g). The balanced chemical reaction that describes this process is

CaCO₃(s)

CaO(s) + CO₂(g)

In the process of making quicklime, a factory releases 7.13 × 10⁵ mol of carbon dioxide into the air every day.

	a.	How many moles of quicklime is the factory producing every day?
	b.	How many moles of limestone is the factory using every day?
	c.	Explain how your answer makes sense by describing what is occurring to the limestone at the atomic scale.

Use the following information to answer questions 10 to 13.

The process of producing copper metal from ores containing copper involves a step in which air is blown over molten copper(I) sulfide in a conversion furnace. The product that emerges from this furnace is called blister copper, because its surface is blistered by the escaping sulfur dioxide gases as the sulfur solidifies. The equations describing the reactions that occur as air is blown over the molten copper(I) sulfide to produce pure copper are as follows:

Reaction 1: 2 Cu₂S(l) + 3 O₂(g)

2 Cu₂O(l) + 2 SO₂(g)
Reaction 2: 2 Cu₂O(l) + Cu₂S(l)

6 Cu(l) + SO₂(g)

10.	Consider each substance described in Reactions 1 and 2. Classify each substance as being an ionic compound, a molecular compound, or a pure metal.

11.	Every 1000 kg of ore mined from Kidd Creek Mine in Ontario typically contains about 18 kg of copper and 58 g of silver.

	a.	Determine the percentage of the ore that contains copper.
	b.	Determine the concentration of the silver in the ore in parts per million.
	c.	Explain the statement, “Percentage and parts per million are actually very similar methods for communicating parts of a whole. In fact, percentage could also be called parts per hundred to help people see the similarities.”

12.	A copper refining operation uses about 34.4 mol of oxygen every second in the refining of copper(I) sulfide.

	a.	Determine the number of moles of copper(I) sulfide required for this reaction every second.
	b.	Determine the number of moles of copper(I) oxide produced by this reaction every second.

13.

Sulfur dioxide has been shown to cause a number of health and environmental problems. The mining industry has responded by reducing their emissions of sulfur dioxide. This is done by capturing some of the sulfur dioxide produced and converting it into sulfuric acid. Despite these efforts, in Canada about 40% of all sulfur dioxide emissions come from the mineral sector. Use the Internet to determine any health and environmental problems caused by the release of sulfur dioxide.

14.	A small coffee cup has a volume of 250 mL. The density of gold is 19.4 g/mL.

	a.	Use the density of gold as a conversion factor to determine the total mass of the fine grains of gold that could fill a coffee cup.
	b.	Use the Internet to find the current world price for a gram of gold. Use your answer from question 14.a. to calculate the current value (in Canadian dollars) of a small coffee cup filled with fine grains of gold.
	c.	As indicated by your answer to question 14.a., gold is a very dense substance. Explain how this property can be used to separate particles of gold from small grains of sand and other minerals when streambed deposits are swirled with water in a shallow container. This process is called panning for gold.

15.	Describe how an activity series could be used to

	a.	determine the reactivity of various metals
	b.	determine the reactivity of various metal ions
	c.	determine whether a particular combination of a metal and a solution containing a metal ion would spontaneously react

16.

Use the activity series for metals and metal ions to complete the following table. Indicate whether a spontaneous reaction or a non-spontaneous reaction will occur with each combination.

Metal	Metal Ion
Metal	Al³⁺(aq)	Zn²⁺(aq)	Sn²⁺(aq)
Al(s)
Zn(s)
Sn(s)

17.	Use your knowledge of reduction and oxidation to explain what occurs to a metal when it corrodes and the techniques that protect metals from corrosion.

18.

Draw a voltaic cell that consists of nickel and magnesium electrodes, each within a solution of its metal ion. Label the cathode, anode, positive and negative electrodes, electrolytes, flow of electrons through the external circuit, and flow of ions through the salt bridge. Assume the salt bridge contains a solution of potassium nitrate, KNO₃(aq).

19.

A voltaic cell is described by the following cell notation:

Al(s) | Al³⁺(aq) | | Fe²⁺(aq) | Fe(s)

Draw a detailed diagram of this voltaic cell. Include labels for the direction of the flow of electrons, anions, and cations within the cell. Assume the salt bridge contains a solution of potassium nitrate, KNO₃(aq).

20.	Compare the voltaic cells in questions 18 and 19. Identify which voltaic cell would produce the higher output on the voltmeter. Concisely explain your reasoning.

21.	Devices like watches, pacemakers, and hearing aids require cells that are very small. In these applications, a miniature mercury button cell is often used.

Although the chemical reactions within these cells are complex, they can still be categorized as oxidation and reduction:

Reaction 1: Zn(s) + 2 OH^–(aq)

ZnO(s) + H₂O(l) + 2e^–
Reaction 2: HgO(s) + H₂O(l) + 2e^–

Hg(l) + 2 OH^–(aq)

	a.	Classify Reaction 1 as being either an oxidation or a reduction reaction. Support your answer.
	b.	Is the powdered zinc in contact with the steel top acting as the anode or the cathode in this cell?
	c.	Classify Reaction 2 as being either an oxidation or a reduction reaction. Support your answer.
	d.	Is the powdered HgO(s) in contact with the steel bottom acting as the anode or the cathode in this cell?
	e.	Would electrons leave the top or the bottom of this cell to flow through an external circuit.

22.	Zinc is electroplated over iron metal to prevent the corrosion of iron nails. This process is called galvanizing. Explain how the zinc acts to protect the iron.

23.	Refer to the diagram on the right.
	a.	Identify the type of cell depicted as either voltaic or electrolytic.
	b.	Describe the importance of the power source to the chemical change that occurs in the cell.
	c.	Determine the direction of electron flow in this cell.
	d.	Identify the half-reaction that occurs at the cathode of this cell.

Chapter 3 Review Questions

Knowledge

Complete the following table.

Name of Compound	Chemical Formula	Condensed Structural Diagram	Alkane, Alkene, or Alkyne
3,4-diethylhexane
3-methyl-4-propyloctane
2,2-dimethylbutane
	C₅H₈(l) (unbranched)
3-ethyl-1-pentene
3-hexene
3-octyne
2-ethyl-4-methyl-1-pentene
	C₇H₁₄(l) (unbranched)

2.	Compare and contrast a continuous-chain alkane with a branched alkane.

3.	a.	Draw complete structural diagrams for 2-methyl-2-butene and 3-methyl-2-pentene.
	b.	Show how the name describes the features and structure of these two molecules.
	c.	Which molecule would have the higher boiling and melting point?

4.	Draw a diagram of a fractional distillation column. Label the following items on your diagram. furnace residue fractions with higher boiling points fractions with lower boiling points long-chained hydrocarbons small-chained hydrocarbons gaseous hydrocarbons

5.	Outline the changes that occur to the molecules of petroleum that undergo the process of fractional distillation.

Applying Concepts

6.	The following compounds are named incorrectly. Draw a complete structural diagram of the compound, and name it correctly.

	a.	1-methylbutane
	b.	2-ethylpentane
	c.	2-ethyl-2-propylhexane
	d.	4-butyl-2-methylhexane
	e.	2-propyl-butane
	f.	3-ethyl-2-propyl-5-hexyne
	g.	2-ethyl-3,4-dimethyl-3-octene

7.	Explain why the compound 2-methyl-1-propyne cannot exist.

8.	Write the balanced chemical equation for the following reactions.

	a.	the combustion of 2-pentyne
	b.	the combustion of 5,5-diethyl-2,2-dimethyloctane
	c.	the hydrogenation of 2-butene
	d.	the hydrogenation on 2-methyl-3-hexyne
	e.	the cracking of octane to produce two-carbon and three-carbon molecules
	f.	the cracking of hexene into two three-carbon molecules

9.	Draw a series of structural diagrams to illustrate the polymerization of each of these starter compounds.

	a.	ethene
	b.	propene

Use the following information to answer questions 10 and 11.

Each of these foods could be used as a dessert in a typical “brown bag” lunch.

The following labels describe the contents of the granola bar, the two chocolate cookies with vanilla filling, and a small rolled cake with filling.

10.	Identify which of these foods would be the healthiest choice if you want to reduce the risks associated with heart disease? Concisely support your answer.

11.	One of the ingredients listed on these labels is trans fat.

	a.	Describe the process of how industrially produced trans fat is made.
	b.	Describe the similarities in terms of structure and in terms of properties between saturated fat and trans fat.
	c.	What recommendation do most nutritionists make in terms of the amount of trans fat you should have in your diet?

Case Study: The Life Cycle of a 2-L Pop Bottle

12.

The starting point in the life cycle of a 2-L pop bottle is petroleum. During the refining processes, the naptha fraction from a fractional distillation tower is passed on to another pressurized tower where the molecules from the naptha fraction are broken down into smaller molecules. Further fractional distillation is used to produce ethene.

	a.	Sketch a labelled diagram illustrating the production of ethene from petroleum.
	b.	Sketch a diagram of an ethene molecule, and write its molecular formula.

13.

The ethene is shipped to a manufacturing facility where it is polymerized into polyethylene terephthalate, which is often shortened to PET or PETE. This is the material used to make 2-L pop bottles. The first step in making the bottles involves heating PETE and pouring it into a mould to make a small, plastic tube called a parison or a preform.

	a.	Use the Internet to determine how a parison or preform is made into a 2-L pop bottle.
	b.	How do preforms help reduce the costs of shipping empty bottles to the factories where the beverages are made?

Every product made from PETE is identified with the code on the left. This code is used to identify the type of plastic so recyclers can properly sort the plastics before the plastics are reclaimed and made into the next generation of products.

There are, in fact, a total of six plastics that are commonly used in packaging, each identified with its own plastic recyling code. Each of these plastics has properties that determine the type of packaging applications to which it is best suited.

14.

Copy the following table into your notebook. Add as many rows as necessary.

Plastic Recycling Code	Full Name of Plastic	Properties	Packaging Applications	Products Made from Recycling This Plastic
	polyethylene terephthalate

	a.	Use the Internet to collect information to complete the first row of the chart for PETE. Repeat this process to complete the five other rows with information for each of the other types of common plastic packaging.
	b.	Look around your home and find specific products that are packaged in each of the six types of plastic packaging. Look on the bottom of plastic containers for the plastic recycle code that will be stamped on the bottom. Add your results to the second last column.

15.

Although it is possible to recycle most types of plastics, in reality only items marked with recycling codes 1 and 2 are actively recycled. Since there is no market for plastic packages marked with numbers 3 through 6, these items end up in landfills. This is part of the reason why less than 5% of all plastics are recycled, compared to 34% for paper, 22% for glass, and 30% for metals. In addition, these three materials can be recycled into similar products many times over, while plastics usually have only a single re-use.

	a.	Why is it especially important for recycled plastics to be made into items that will have a relatively long, useful life?
	b.	In the ecological slogan, “Reduce, Re-use, Recycle,” it is the last word that tends to get the most attention. Explain why reducing the consumption of plastic is the most effective way to help the environment in the long term. You will explore these ideas in more detail in Unit D.

Unit A Review Questions

1.	Which term—solution, solute, or solvent—best matches each of the following substances?

	a.	sucrose (table sugar)
	b.	water
	c.	sports drink

Use the following list to answer questions 2.a. and 2.b.

	I.	hydrogen peroxide, H₂O₂(aq)
	II.	hydrochloric acid, HCl(aq)
	III.	salt water, NaCl(aq)
	IV.	ammonia, NH₃(aq)

	a.	The two electrolyte solutions are __________ and __________.
	b.	The two non-electrolyte solutions are __________ and __________.

3.	At the particle level, describe how water molecules act to change the structure of the crystals of a solid ionic compound to form an electrolytic solution.

4.	Use a simple, labelled diagram to highlight the main features of each of the following types of solutions.

	a.	an electrolytic solution
	b.	a non-electrolytic solution
	c.	a concentrated solution
	d.	a dilute solution

Read the following descriptions of four chemical reactions.

Reaction A: Copper sheets oxidize and lose their shine.
Reaction B: Hydrogen ions in solution react to form a molecule of hydrogen gas.
Reaction C: Iron metal rusts to form iron(II) oxide.
Reaction D: A nickel(II) ion is electroplated at the cathode of an electrolytic cell.

Complete the following chart for each of the reactions.

Reaction	Half-Reaction for the First Element Mentioned	Oxidation or Reduction	Number of Electrons Gained or Lost
A
B
C
D

6.	In this unit you made an extensive use of the activity series for metals and metal ions. Summarize the uses of this activity series.

7.	Examine the following balanced chemical equation: 2 Mg(s) + O₂(g) 2 MgO(s)

	a.	Identify the chemical substance being oxidized.
	b.	Identify the chemical substance being reduced.
	c.	Identify any spectators.
	d.	Determine the number of electrons gained by each atom or ion.
	e.	Determine the number of electrons lost by each atom or ion.

8.	Examine the following balanced chemical equation: 2 Ag(s) + H₂SO₄(l) Ag₂SO₄(aq) + H₂(g)

	a.	Identify the chemical substance being oxidized.
	b.	Identify the chemical substance being reduced.
	c.	Identify any spectators.
	d.	Determine the number of electrons gained by each atom or ion.
	e.	Determine the number of electrons lost by each atom or ion.

9.	Determine whether the following species could undergo oxidation, reduction, or both.

	a.	a hydrogen ion, H⁺(aq)
	b.	a gold ion, Au⁺(aq)
	c.	a silver ion, Ag⁺(aq)

10.

Complete the following table.

Name of Compound	Chemical Formula	Condensed Structural Diagram	Alkane, Alkene, or Alkyne	Saturated or Unsaturated
2,2-dimethylpentane
4-propyloctane
3-octene
	C₇H₁₂(l)
2-ethyl-1-hexene
	CH₄(g)

11.	Draw the condensed structural diagram for 4,4-diethyl-2-hexyne. Describe the process used to draw the diagram.

12.	Complete each of the following calculations by showing all of your steps.

	a.	Calculate the molar concentration of a solution prepared by adding 150 mL of water to 25.4 g of silver nitrate, AgNO₃(aq).
	b.	Calculate the number of moles of solute dissolved in 0.050 L of a 0.392-mol/L silver nitrate solution, AgNO₃(aq).
	c.	The maximum concentration of lead in drinking water is 0.010 ppm. A 4.00-kg sample of contaminated well water was found to have twice this concentration of lead. Calculate the mass of the lead dissolved in the water.
	d.	In addition to copper, trace amounts of other metals are often recovered at copper mines. The concentration of silver found in the ore of a copper mine is 58 ppm. Calculate the mass of ore that would have to be mined to yield 1.00 kg of silver.

13.	Ammonia is a very useful reagent for many reactions. One way of making ammonia is to react nitrogen gas with hydrogen gas. N₂(g) + 3 H₂(g) 2 NH₃(g) You have 20.0 mol of nitrogen.

	a.	How many moles of ammonia could you make?
	b.	How many moles of hydrogen gas would you require to react with the nitrogen?

Use the following information to answer questions 14 to 18.

Case Study: The Chemistry of Hair Conditioners

When you rinse shampoo out of your hair, you also remove oils that act to protect your hair. A hair conditioner replaces these oils with a protective coating. Although some hair conditioners are applied and then left on wet hair, most conditioners are also rinsed out of the hair. How can the protective coating be left on the hair when the other ingredients of the conditioner are rinsed away?

Part of the answer to this question is found in the structure of hair itself. The main protein in hair is keratin. An interesting property of the keratin in hair is that its molecular structure tends to have a high percentage of negative charges on its outer surface. This means that the outer surface of each shaft of hair tends to have a slightly negative charge, even after it’s been washed with shampoo.

This is why the manufacturers of hair conditioners use substances in their products called surfactants—short for “surface active agents.”

As the following example indicates, conditioners usually consist of a group of cationic surfactants mixed with other ingredients in a water-based solution.

INGREDIENTS IN BRAND Y HAIR CONDITIONER

Ingredient	Volume (mL)	Function
water	465.5	acts to dissolve the other ingredients
cyclomethicone and dimethiconol solution	10.5	an oil soluble blend of compounds that holds silicone in solution until it can be released onto the hair
distearyldiammonium chloride solution	7.0	cationic surfactant—helps second ingredient attach to hair
cetyl alcohol solution	6.0	ingredients work to keep the oil-based and water-based parts of the solution from separating
sorbitan oleate solution	5.0
stearyl alcohol solution	4.0
polysorbate-85 solution	2.0
Total	500.0

The cationic surfactants play a key role in hair conditioners. The charged head of the surfactant is attracted to the hair while the long tail helps carry the oil-based ingredients that give the hair its shine.

14.	Identify the ingredient in the hair conditioner that could be classified as the solvent.

15.	Identify an ingredient in the hair conditioner that could be classified as a solute.

16.	Explain how neutral water molecules could be attracted to the charged head of a cationic surfactant. Sketch and label a diagram to support your answer.

17.	As explained in the information, the outer surface of a hair has a slight negative charge.

	a.	Explain the significance of the charge along the length of the hair to the action of the cationic surfactants in bringing a new protective coating to a hair.
	b.	Explain why conditioned hair is less likely to stand on end and “fly away.”

18.	Calculate the percent by volume concentration of the following ingredients in the hair conditioner.

	a.	distearyldiammonium chloride
	b.	cetyl alcohol
	c.	polysorbate-85

19.	Balance each of the following reactions.

	a.	SnCl₂(aq) + Al(s) AlCl₃(aq) + Sn(s)
	b.	Au(NO₃)₃(aq) + Ag(s) AgNO₃(aq) + Au(s)
	c.	HNO₃(aq) + Cu(s) Cu(NO₃)₂(aq) + H₂(g)
	d.	Zn(s) + H₂SO₄(aq) H₂(g) + ZnSO₄(aq)

20.	If you react chlorine gas with sodium metal, you can produce sodium chloride. Cl₂(g) + 2 Na(s) 2 NaCl(s)

	a.	State the chemical substance that is being oxidized.
	b.	State the chemical substance that is being reduced.
	c.	Determine the number of electrons transferred in the reaction.
	d.	If 75.0 mol of sodium reacted with a sufficient amount of chlorine gas, how many moles of chlorine gas will be required?

21.	A student performed an experiment on platinum metal and collected the following data: Pt(s) + Ag⁺(aq) no reaction Pt(s) + Fe²⁺(aq) no reaction According to the data, where should solid platinum, Pt(s), and its ion, Pt²⁺(aq), appear in the activity series for metals and metal ions?

22.	Use the activity series to predict whether each combination of reactants will result in a spontaneous reaction.

	a.	copper metal and chromium(II) ion
	b.	zinc metal and hydrochloric acid
	c.	silver metal and nitric acid
	d.	silver ion and nickel metal

23.	List some of the methods used to prevent the corrosion of metals. Briefly explain how these methods prevent the oxidation of the metal being protected.

24.	An automobile manufacturer plans to build a corrosion-proof body for a car. The car’s body will be made entirely from plastic. Will the use of plastic in the car’s body prevent damage from corrosion? Suggest advantages and disadvantages of this design.

25.

The following cell notation describes a voltaic cell:

Mg(s) | Mg²⁺(aq) | | Ag⁺(aq) | Ag(s)

Draw a diagram of this voltaic cell. Label the anode, cathode, voltmeter, and salt bridge. Also label the direction of the flow of electrons, anions, and cations within the cell. Assume that potassium nitrate, KNO₃(aq), is used in the salt bridge.

26.

The diagram shows a voltaic cell that a student set up in a lab.

Observations from this cell:

The voltage output is zero.
The solution of Cu(NO₃)₂(aq) is becoming less blue as time goes by.
The mass of the zinc electrode has increased since the experiment began.

	a.	Suggest a reason for the change in the mass of the zinc electrode in the cell.
	b.	Suggest a reason why the cell was not able to produce a voltage.

27.

Locate the video clip called “Career Profile: Ceramic Artist” on the Science 20 Textbook CD. This segment describes how chemistry is used by a potter to create works of art. Watch this video, and then answer the following questions.

	a.	Describe the chemical composition of the clay used by a ceramic artist.
	b.	List the compounds used to give colour to a glaze.
	c.	Consider the list that you generated in 27.b. Identify the category of matter that applies to all the compounds on your list.
	d.	Describe how the compounds used in glazes are prepared to be applied to the clay body.

28.

Some specialized electrical devices, such as pacemakers, require a miniature cell that can maintain a constant voltage throughout its useful lifetime. In these devices, silver-zinc button cells are often used.

Although the chemical reactions within these cells are complex, they can still be categorized as oxidation and reduction.

Oxidation and Reduction in a Miniature Silver-Zinc Button Cell

Reaction 1: Ag₂O(s) + H₂O(l) + 2e^–

2 Ag(s) + 2 OH^–(aq)
Reaction 2: Zn(s) + 2 OH^–(aq)

ZnO(s) + H₂O(l) + 2e^–

	a.	Classify Reaction 1 as being either an oxidation or a reduction reaction. Support your answer.
	b.	Is the powdered Ag₂O(s) in contact with the steel bottom acting as the anode or the cathode in this cell?
	c.	Classify Reaction 2 as being either an oxidation or a reduction reaction. Support your answer.
	d.	Is the powdered zinc, Zn(s), in contact with the steel top acting as the anode or the cathode in this cell?
	e.	Would electrons leave the top of this cell and flow through an external circuit or would they leave the bottom of this cell?

Use the following information to answer questions 29 to 31.

Although a single zinc chloride cell can provide 1.5 V, smoke detectors require a higher voltage. For applications such as this, the six cells are combined in a single package to provide 9.0 V of output. Refer to the cross sectional diagram given.
Each cell within this device adds energy to the current of electrons that flows to the circuitry of the smoke detector. The chemical reactions that occur within each cell are summarized as follows:

Oxidation and Reduction Within Each Cell

Oxidation Reaction: Zn(s)

Zn²⁺ + 2e^–
Reduction Reaction: 2 NH₄⁺(aq) + 2 MnO₂(s) + 2e^–

Mn₂O₃(s) + 2 NH₃(g) + H₂O(l)

29.	Identify the proper name for the type of device shown in the illustration.

30.	Consider the oxidation reaction that occurs within each cell.

	a.	Use this reaction to determine whether the zinc electrode is acting as the anode or the cathode.
	b.	Carefully examine the cross sectional diagram. Explain how this diagram verifies your answer to question 29.a.

31.	Consider the reduction reaction that occurs within each cell.

	a.	Explain why both the manganese and the ammonium are considered to be reduced in this reaction.
	b.	If the reduction half-reaction for the manganese(IV) oxide were to be placed in the activity series for metals and metal ions, would it appear above or below the reduction half-reaction for zinc? Explain.

32.	Draw an electrolytic cell that would be able to plate nickel onto an iron drill bit. In your diagram include the following: electrolyte solution and label its contents anode cathode power source direction for electron flow

33.	The compound 3-ethyl-3-methyl-2-pentyne cannot exist. Use the name of the compound to draw a condensed structural diagram that will explain why this compound could never exist.

34.	a.	Write a balanced chemical equation to show one possibility in the cracking of decane.
	b.	Properly name the products of your cracking reaction.

35.	Write a balanced chemical equation to describe each reaction.

	a.	the combustion of butane
	b.	the combustion of 2,2-dimethylhexane
	c.	the hydrogenation of 3-hexene

36.	Draw a series of diagrams to illustrate the polymerization of 2-butene.

37.	Many nutritionists recommend sardines as a healthy food. Although this food is a good source of many important nutrients, it is not a perfect food due to the presence of some less desirable substances.

	a.	Saturated and unsaturated fats are listed in the nutrition facts. Explain what these terms mean in terms of the carbon chains that make up these substances.
	b.	Identify at least two items listed in the nutrition facts that indicate that this is a healthy food choice.
	c.	Identify at least two items listed in the nutrition facts that are less desirable because they are not associated with good health.