Question: In each of the following reactions, identify

> Reactions in which one or more are transferred between species are called oxidation–reduction reactions.

> Explain the difference between somatic damage from radiation and genetic damage. Which type causes immediate damage to the exposed individual?

> Although aluminum is one of the most abundant metals on earth, its price until the 1890s made it a “precious metal” like gold and platinum. Why?

> How does an electrolysis cell differ from a galvanic cell?

> What is meant by a nuclear bombardment process? Give an example of such a process, and describe what the net result of the process is.

> The “Chemistry in Focus” segment Stainless Steel: It’s the Pits discusses the fact that stainless steel can corrode if there is a deficit of chromium. How does chromium protect stainless steel?

> Pure iron ordinarily rusts quickly, but steel does not corrode nearly as fast. How does steel resist corrosion?

> In a breeder nuclear reactor, nonfissionable is converted to fissionable .

> is the process of returning metals to their natural state—the ores from which they were originally obtained. This process involves of the metal.

> What are some advantages of using lithium ion batteries in electrical devices? What is a disadvantage?

> Write the chemical equation for the overall cell reaction that occurs in a lead storage automobile battery. What species is oxidized in such a battery? What species is reduced? Why can such a battery be “recharged”?

> Consider the oxidation–reduction reaction Zn(s) + Pb2+(aq) Zn2+(aq) + Pb(s) Sketch a galvanic cell that uses this reaction. Which metal ion is reduced? Which metal is oxidized? What half-reaction takes place at the anode in the

> Consider the oxidation–reduction reaction Al(s) + Ni2+(aq) Al3+(aq) + Ni(s) Sketch a galvanic cell that makes use of this reaction. Which metal ion is reduced? Which metal is oxidized? What half- reaction takes place at the anode in

> What type of reaction takes place at the cathode in a galvanic cell? At the anode?

> In which direction do electrons flow in a galvanic cell, from anode to cathode or vice versa?

> In each of the following reactions, identify which element is being oxidized and which is being reduced by assigning oxidation numbers. a. 4KClO3(s) + C6H12O6(s) / 4KCl(s) + 6H2O(l) + 6CO2(g) b. 2C8H18(l) + 25O2(g) / 16CO2(g) + 18H2O(l) c. PCl3(g) + Cl2

> During nuclear , a large nucleus is transformed into lighter nuclei. During nuclear , small nuclei are combined to make a heavier nucleus. Both processes release energy, but nuclear

> How do the forces that hold an atomic nucleus together compare in strength with the forces between atoms in a molecule?

> Nitric acid is a very strong acid, but is also a very strong oxidizing agent, and generally behaves as the latter. It will dissolve many metals. Balance the following oxidation–reduction reactions of nitric acid. a. Cu(s) + HNO3(aq) Cu2+(

> Each of the following nuclides is known to undergo radioactive decay by production of an alpha particle, /. Write a balanced nuclear equation for each process. a. / b. / c. /

> Each of the following nuclides is known to undergo radioactive decay by production of a beta particle, /. Write a balanced nuclear equation for each process. a. /C b. / c. /

> Complete each of the following nuclear equations by supplying the missing particle. a. 80 201

> How is 6 14

> Naturally occurring magnesium consists primarily of three isotopes, of mass numbers 24, 25, and 26. How many protons does each of these nuclides contain? How many neutrons does each of these nuclides contain? Write nuclear symbols for each of these isoto

> Technetium-99 has been used as a radiographic agent in bone scans ( 43 99

> Although naturally occurring potassium consists mostly of the isotope of mass number 39 (93.25%), isotopes of mass number 41 (6.73%) and 40 (0.01%) also are present. Write the nuclear symbol for each of the isotopes of potassium. How many neutrons are pr

> In each of the following reactions, identify which element is being oxidized and which is being reduced by assigning oxidation states. a. 2Cu(s) + S(s) / Cu2S b. 2Cu2O(s) + O2(g) / 4CuO(s) c. 4B(s) + 3O2(g) / 2B2O3(s) d. 6Na(s) + N2(g) / 2Na3N(s)

> The following isotopes (listed with their half-lives) have been used in the medical and biologic sciences. Arrange these isotopes in order of their relative decay activities: 3H (12.2 years), 24Na (15 hours), 131I (8 days), 60Co (5.3 years), 14C (5730 ye

> Consider the isotopes of radium listed in Table 19.3. Which isotope is most stable against decay? Which isotope is “hottest”? From table 19.3: Half-life Nuclide 12 days 깰Ra 3.6 days 224 껍Ra 15 days Ra 225 276Ra 16

> Although magnesium metal does not react with water at room temperature, it does react vigorously with steam at higher temperatures, releasing elemental hydrogen gas from the water. Mg(s) + 2H2O(g) Mg(OH)2(s) + H2( g) Identify which e

> Iron ores, usually oxides of iron, are converted to the pure metal by reaction in a blast furnace with carbon (coke). The carbon is first reacted with air to form carbon monoxide, which in turn reacts with the iron oxides as follows: F2O3(s) + 3CO(g)

> Pennies in the United States consist of a zinc core that is electroplated with a thin coating of copper. Zinc dissolves in hydrochloric acid, but copper does not. If a small scratch is made on the surface of a penny, it is possible to dissolve away the z

> Write a balanced nuclear equation showing the bombardment of /with deuterium atoms (the isotope of hydrogen with A = 2, /) to produce /and an alpha particle.

> Write a balanced nuclear equation showing the bombardment of / with alpha particles to produce /and a neutron.

> What does a gamma ray represent? Is a γ ray a particle? Is there a change in mass or atomic number when a nucleus produces only a γ ray?

> What does a nuclear transformation represent? How is a nuclear transformation performed?

> Complete each of the following nuclear equations by supplying the missing particle. a. 89 210

> In each of the following reactions, identify which element is being oxidized and which is being reduced by assigning oxidation numbers. a. 2Al(s) + 3S(s) Al2S3(s) b. CH4( g) + 2O2( g) CO2( g) + 2H2O( g) c. 2Fe2O3(s) +

> For each of the following oxidation–reduction reactions, identify which element is being oxidized and which is being reduced. a. Cl2( g) + I2( g) 2ICl( g) b. Cl2( g) + 2Li(s) 2LiCl(s) c. 2Na(s) + 2H2O( l )

> Complete each of the following nuclear equations by supplying the missing particle. a. ? 2 4

> Complete each of the following nuclear equations by supplying the missing particle. a. 88 226

> Which of the following nuclear processes results in a decrease in the neutron-to-proton ratio? Justify your answer. a. ß-particle production b. Positron production c. Electron capture d. α-particle production e. γ-ray production

> Give the nuclear symbol for each of the following. a. a beta particle b. an alpha particle c. a neutron d. a proton

> What is the oxidation state of manganese in each of the following substances? a. MnCl2 b. KMnO4 c. MnO2 d. Mn(C2H3O2)3

> What is the oxidation state of nitrogen in each of the following substances? a. N2 b. NH3 c. NO2 d. NaNO3

> Naturally occurring sulfur consists primarily (94.9%) of the isotope with mass number 32, but small amounts of the isotopes with mass numbers 33, 34, and 36 also are present. Write the nuclear symbol for each of the isotopes of sulfur. How many neutrons

> What do we mean when we say a nucleus has undergone an electron capture process? What type of electron is captured by the nucleus in this process?

> Because the chemistry of an atom is determined by the number and arrangement of its , the properties of the nucleus do not strongly affect the chemical behavior of an atom.

> What is a decay series?

> When a nucleus emits a neutron, does the atomic number of the nucleus change? Does the mass number of the nucleus change? Explain.

> When a nucleus emits a beta particle, by how many atomic mass units does the mass of the nucleus change? By how many units does the atomic number of the nucleus change? Explain.

> For the nuclide
, identify the mass number and the atomic number.

> What is meant by saying an element exists in several isotopic forms? Do isotopes of a given element have similar chemical properties? Explain.

> The sum of the numbers of neutrons and protons is the .

> What does the atomic number of an atom represent?

> How large is a typical atomic nucleus, and how does the size of the nucleus of an atom compare with the overall size of the atom?

> The major use of alkanes has been in reactions, as a source of heat and light.

> Tetraethyl lead, (C2H5)4Pb, was added to gasoline in the past as a(n) agent.

> Kerosene may be converted to gasoline by , which means that the larger, heavier kerosene components are broken down by heat into smaller, lighter gasoline fragments.

> The “Chemistry in Focus” segment Do We Age by Oxidation? discusses antioxidants. What does it mean for a chemical to be an antioxidant? How would it work chemically?

> The positions of substituents along the hydrocarbon framework of a molecule are indicated by the of the carbon atom to which the substituents are attached.

> For a branched hydrocarbon, the root name for the hydrocarbon comes from the number of carbon atoms in the continuous chain in the molecule.

> The systematic names of all saturated hydrocarbons have the ending added to a root name that indicates the number of carbon atoms in the molecule.

> Structural isomerism occurs when two molecules have the same number of each type of atom but exhibit different arrangements of the between those atoms.

> Alkanes in which the carbon atoms form a single unbranched chain are said to be alkanes.

> The general orientation of the four pairs of electrons around the carbon atoms in alkanes is .

> A carbon compound containing a carbon–carbon double or triple bond is said to be .

> Figure 20.3 shows the structures of the hydrocarbons propane and butane. Discuss the arrangement of the electron pairs around each of the carbon atoms in these molecules. Are these molecules linear? Why or why not? From figure 20.3: 109.5° H H H H.

> The first “organic” compound to be synthesized in the laboratory, rather than being isolated from nature, was , which was prepared from .

> For the polymeric substances nylon and Dacron, sketch representations of the repeating unit in each.

> Does an oxidizing agent donate or accept electrons? Does a reducing agent donate or accept electrons?

> What are some applications of the common polymer polyvinyl chloride (PVC)?

> The “Chemistry in Focus” segment Mother of Invention discusses Stephanie Kwolek and the invention of Kevlar. Is Kevlar a copolymer or a homopolymer?

> What is condensation polymerization, and how does it differ from addition polymerization? Give an example of a common condensation polymer.

> One type of polymerization reaction in which the monomers “add together” to form the polymer (and no other products are formed) is called a(n) polymerization.

> What, in general terms, is a polymer? What is a monomer?

> Draw a structural formula for each of the following: a. methyl butanoate b. ethyl acetate c. o-chlorobenzoic acid d. 2,2-dimethyl-3-chloro-butanoic acid

> Give the systematic name for each of the following organic acids: a. CH,-CH,-CH-C CH, HO CH,-C b. CH, c. CH,-CH,-ċ–CH,-C HO. CH3 CH, c-CH,-Ċ-CH, d. Но ČH, CI

> What two main functional groups are in acetylsalicylic acid (aspirin)?

> Which of the following molecules are saturated? a. CH3-CH3 b. CH2=CH2 c. CH3-CH2-CH2-CH3 d. CH3-CH2-CH=CH2

> From what two families of organic compounds are esters synthesized? Give a specific example of a reaction in which an ester is formed, and indicate how the name of the ester in your example is derived from the compounds used to synthesize it.

> Does an oxidizing agent increase or decrease its own oxidation state when it acts on another atom? Does a reducing agent increase or decrease its own oxidation state when it acts on another substance?

> Complete the following equations with the structural formula of the principal organic product. / Mild oxidation а. CH, — CH, —CH,—CH,—Он Strong oxidation b. CH, — CH, —CH,—ОН

> Are carboxylic acids typically strong acids or weak acids? Write an equation showing the acid CH3CH2COOH ionizing in water.

> Draw the structure of the group that characterizes organic (carboxylic) acids. Give the general condensed formula for an organic acid.

> Draw structural formulas for each of the following aldehydes and ketones. a. dimethyl ketone b. 3-methyl-2-butanone c. propanal d. 2,2-dimethyl-3-pentanone

> Give the systematic name for each of the following aldehydes or ketones. CH3 a. CH,-CH- CH,-C-C H CH3 CH, b. CH,-CH- c-CH-CH, CH, Ö CH, CH, CI c. CH,-C-ČH-CH, d. CH,-C H.

> Provide an alternative name for the compound 2-butanone.

> Aldehydes and ketones both contain the carbonyl group, yet the properties of these two types of compounds are different enough that they are classified separately. Without looking back at the text, draw the structures of the ketone and the aldehyde that

> Write equations showing the oxidation of a primary alcohol and the oxidation of a secondary alcohol to produce an aldehyde and a ketone, respectively. Indicate the structure of each alcohol and of the principal organic products of the oxidations.

> Which of the following molecules are unsaturated? a. CH3-CH2-CH2-CH3 b. CH3-CH=CH-CH3 c. CH3-C (C-CH3 d. CH3-CH2-CH3

> What is acetone commonly used for in industry? What compound gives rancid butter its unpleasant odor?

> What is an oxidizing agent? What is a reducing agent?

> What functional group is common to both aldehydes and ketones?

> What is the simplest aromatic alcohol commonly called? What is it mostly used for in the United States?

> Write the equation for the fermentation of glucose to form ethanol. Why can’t ethanol solutions of greater than about 13% concentration be made directly by fermentation? How can the ethanol content be increased beyond this level in beverages?

> Is 1-pentanol a primary, secondary, or tertiary alcohol? Why or why not?

> Give the systematic name for each of the following alcohols. Indicate whether the alcohol is primary, secondary, or tertiary. CH,-CH3 а. CH —CH, —с-сн,—сH, ÓH CH3 CH3 b. CH;-CH-CH-CH-CH3 CH3 c. CH3-CH-CH,-C-CH3 CH3 d. CH;-CH-CH,-C-CH,-OH CH3 CH3

> Distinguish among primary, secondary, and tertiary alcohols. Give a structural formula for an example of each type.

> Draw the Lewis structures for carbon dioxide and carbon monoxide.