Question: For gasoline, isooctane, 2,2,4-trimethylpentane

> Why is the staggered conformation of ethane more stable than the eclipsed conformation?

> Name each of the following compounds: a. с. H;C CH3 Br b. CH3 d. CH3 В Br

> Draw the structures of each of the following compounds: a. trans-1,4-Dimethylcyclooctane b. cis-1,3-Dichlorocyclohexane c. cis-1,3-Dibromocyclobutane

> Explain how Rutherford concluded that the atom is principally empty space.

> What are the weak interactions that maintain the tertiary structure of a protein?

> Which of the following names are correct and which are incorrect? If incorrect, write the correct name. a. 1,4,5-Tetrabromocyclohexane b. 1,3-Dimethylcyclobutane c. 1,2-Dichlorocyclopentane d. 3-Bromocyclopentane

> How many isomers of dibromocyclobutane can you construct? As in Question 10.83, use a set of molecular models to construct the isomers and then draw them. Question 10.83: How many geometric and structural isomers of dichlorocyclopropane can you constru

> Draw each of the following cycloalkanes: a. 1,2,3-Trichlorocyclopropane b. 1,1-Dibromo-3-chlorocyclobutane c. 1,2,4-Trimethylcycloheptane d. 1,2-Dichloro-3,3-dimethylcyclohexane

> Name each of the following cycloalkanes, using the IUPAC system: a. b. c. d. Br Br Br CI ICH3 H,C Cl CH3

> How do linear, continuous-chain alkanes differ from branched-chain alkanes?

> How does the general formula of a cycloalkane compare with that of an alkane?

> What are the potential advantages and disadvantages of breeder reactors?

> Draw the structures of the following compounds. Are the names provided correct or incorrect? If they are incorrect, give the correct name. a. 1,4-Dimethylbutane b. 1,2-Dichlorohexane c. 2,3-Dimethylbutane d. 1,2-Diethylethane

> What is the OH2 concentration of each solution in Question 8.71? Question 8.71: a. 1.0 × 10-6 M b. 1.0 × 10-8 M c. 5.6 × 10-4 M

> Which of the following structures are incorrect? Describe the problem in those that are incorrect. a. CH3CH(CH3)2CH2CH3 b. CH3(CH2)5CH3 c. CH2CH2C(CH3) CH2CH2CH3 d. CH3CH2CH(CH3)3CH3

> The enzyme aconitase catalyzes the isomerization of citrate into isocitrate. Discuss the two reactions catalyzed by aconitase in terms of the chemistry of alcohols and alkenes.

> Which of the following pairs of molecules are identical compounds? Which are constitutional isomers? a. CH3CH2CH(CH3) CH2CH3 CH3C(CH3)2CH2CH2CH3 b. CH3CH2CH2CH2C(CH3)2CH2CH(CH3) CH3 CH3CH(CH3) CH2CH2C(CH3)2CH2CH2CH3

> Which of the following pairs of compounds are identical? Which are constitutional isomers? Which are completely unrelated? a. b c. d. Br Br CH;CH,CHCH3 and CH;CHCH,CH3 Br CH3 CH3 CH;CH,CHCH,CHCH3 and CH,CHCH,CHCH,CH, Br Br Br CH,ČCH,CH, and BrĊCH,

> Name all of the isomers that you obtained in Question 10.63. Question 10.63: Draw a complete structural formula for each of the straight-chain isomers of the following alkanes: a. C4H9Br b. C4H8Br2

> Name the following using the IUPAC Nomenclature System: a. b. c. d. CI CH,CHCHCH,CH3 Cl CH3 CH;CH,CCH,CHCH3 1. 1. ČH, ČH3 CH, CH3 CH,CH,CHCHCHCH3 CH3 Br CHCH,CH,CH- Br

> Provide the IUPAC name for each of the following compounds: a. b. CH3CHClCH2CH2CH2Cl c. CH;CH,CHCH,CHCH,CH3 ČH3 ČH; ČH,CH3 CH3 CH3C Br CH3

> Provide the IUPAC names for the products of the reactions in Question 10.5. Question 10.5: Write a balanced equation for each of the following reactions. Show all possible products. a. the monobromination of propane b. the monochlorination of butane c.

> Draw each of the following compounds using structural formulas: a. 1,1,1-Trichlorodecane b. 1,2-Dibromo-1,1,2-trifluoroethane c. 3,3,5-Trimethylheptane d. 1,3,5-Trifluoropentane

> Draw each of the following using line formulas: a. Dichlorodiiodomethane b. 1,4-Diethylcyclohexane c. 2-Iodo-2,4,4-trimethylpentane

> Name each of the compounds in Question 10.50b. Question 10.50b: b. CH3CH2CH2CH2CH3 CH3(CH2)8CH3 CH3(CH2)6CH3

> What would the physical state of each of the compounds in Question 10.50 be at room temperature? Question 10.50: Based on intermolecular forces, rank the following compounds from highest to lowest melting points: a. decane propane methane ethane b. CH3

> Verify your answer to Question 5.45 by calculating the temperature needed to double the volume of the gas. Question 5.45: The temperature of a gas is raised from 258C to 508C. Will the volume double if mass and pressure do not change? Why or why not?

> Describe the relationship between the length of hydrocarbon chains and the melting points of the compounds.

> Why do linear alkanes have higher melting and boiling points than branched-chain alkanes?

> Describe London dispersion forces.

> The following is the structure of the pain reliever ibuprofen, found in Advil. Circle and label the functional groups of the ibuprofen molecule. OH Ibuprofen

> Folic acid is a vitamin required by the body for nucleic acid synthesis. The structure of folic acid is given below. Circle and identify as many functional groups as possible. H,NN N CH,NH- -NH–CHCH,CH,COOH OH ČOOH Folic acid

> Classify each of the carbon atoms in the following structures as primary, secondary, tertiary, or quaternary. a. CH3CH2C(CH3)2CH2CH3 b. CH3CH2CH2CH2CH(CH3) CH(CH3) CH3 c. d.

> What is the major structural feature that distinguishes between saturated and unsaturated hydrocarbons?

> Of the classes of compounds listed in Question 10.35, which are saturated? Which are unsaturated? Question 10.35: Give the general formula for each of the following: a. An alkane b. An alkyne c. An alkene d. A cycloalkane e. A cycloalkene

> Convert the following condensed formulas into structural formulas: a. CH3CH(CH3) CH(CH3) CH(CH3) CH2CH3 b. CH3C(CH3)2CH(CH2CH3) CH2CH2CH3

> Using the octet rule, explain why carbon forms four bonds in a stable compound.

> How do soaps assist in the removal of oil and grease from clothing?

> Convert the following line formulas into condensed formulas: b. а. d. с.

> Convert the following structural formulas into line formulas: a. b. c. H. H H-C-H Н-С-Н H H H H ннн H-C-H H Н-С—Н H H H H-C-H H нн H-C=C-C-C=Ċ-C=Ċ-Ċ-C=Ċ-H нн H H H H-C-H H-C-H H H. нн H HÇ=C-C-Ç=C-H H H Н-С—Н H

> Condense each of the following structural formulas: H H Н-С—Н H-C-H H ннн H H а. Н—С—С С-С—С—Н b. Н—С—С С-Н ннннн H Н-С—Н H H. Н-С—Н H нннн ннн I III нн Н-С—Н H H H H нн Н-С—н H H

> What results would the student expect if the sample in Question 10.1 were an inorganic compound? What results would the student expect if it were an organic compound? Question 10.1: A student is presented with a sample of an unknown substance and asked

> Describe what is meant by the term nuclide.

> Is the roentgen unit used in the measurement of alpha particle radiation? Why or why not?

> Which of the compounds in Question 10.12 would be soluble in water? Question 10.12: Based on intermolecular forces or ionic interactions, rank the following compounds from highest to lowest melting points: a. H2O2 CH4 KCl b. C6H14 C18H38 NaCl

> Based on intermolecular forces or ionic interactions, rank the following compounds from highest to lowest melting points: a. H2O2 CH4 KCl b. C6H14 C18H38 NaCl

> Why would a Geiger counter be preferred to film for assessing the immediate danger resulting from a spill of some solution containing a radioisotope?

> Give all the possible monochlorinated products for the following reaction: Name the products, using IUPAC nomenclature. Light CH,CH(CH,)CH,CH, + Cl, ?

> Calculate the number of mol corresponding to: a. 15.0 g NH3 b. 16.0 g O2

> Why are ionic substances more likely to be water-soluble?

> Suggest a protocol for radioactive waste disposal.

> Would the use of concrete rather than wood paneling help to protect workers in other parts of the clinic? Why?

> Would wearing a lab apron lined with thin sheets of lead have a positive effect? Why?

> Would wearing gloves have any significant effect? Why?

> Why do high-altitude jet flights increase a person’s exposure to background radiation?

> Radioactive molybdenum-99 is used to produce the tracer isotope, technetium-99m. Write a nuclear equation for the formation of molybdenum-99 from stable molybdenum- 98 bombarded with neutrons.

> Describe an application of each of the following isotopes: a. iodine-131 b. thallium-201

> Describe how medically useful isotopes may be prepared.

> Calculate the number of ATP molecules produced by the complete b-oxidation of eicosanoic acid.

> Describe how radioactive tracers are used in the diagnosis of disease.

> What type of nuclear reaction fuels our solar system?

> In what way are beta particles and positrons similar?

> Why are cadmium rods used in a fission reactor?

> What are the major disadvantages of a fission reactor for electrical energy production?

> Which type of nuclear process combines small nuclei to release energy?

> What property of carbon enables us to assess the age of a painting?

> The hydronium ion concentration in the blood of three different patients was: Patient.. [H3O1] A.. 5.0 x 10-8 B. 3.1 x10-8 C.. 3.2 x 10-8

> A patient receives 9.0 ng of a radioisotope with a half-life of 12 h. How much will remain in the body after 2.0 days, assuming that radioactive decay is the only path for removal of the isotope from the body?

> Would you predict lithium-9 to be stable? Explain your reasoning.

> Note the major accomplishment of each of the following: a. Thomson b. Rutherford c. Geiger d. Bohr

> Would you predict cobalt-59 to be stable? Explain your reasoning.

> Phosphorus-31, known to bioaccumulate in the liver, decays by beta emission. Write a balanced nuclear equation for this process.

> Cobalt-60 has a half-life of 5.3 years. How many half-lives occur after 21.2 years?

> Explain why the binding energy of a nucleus is expected to be large.

> Element 106 was named seaborgium (Sg) in honor of Glenn T. Seaborg, a pioneer in the discovery of lanthanide and actinide elements. Seaborgium-263 decays by alpha emission. Write a balanced nuclear equation for this process.

> Write a balanced nuclear equation for positron emission by manganese-52.

> Write a balanced nuclear equation for alpha decay of bismuth-212.

> Element 109 was synthesized by bombarding bismuth-209 with iron-58. Write the equation for this process if one product is a neutron.

> Complete the following nuclear equation: ? −−−→ (90 ^ 214) Th + (2 ^4) HE

> Complete the following nuclear equation: (78 ^ 190) Pt −−−→ a + ?

> a. Write the sequence of steps that would be followed for one round of b-oxidation of hexanoic acid. b. Calculate the number of ATP molecules produced by complete b-oxidation of hexanoic acid.

> Complete the following nuclear equation: (92 ^ 238) U + (7 ^14) N−−−−→?6(0 ^1) n

> Write a nuclear equation to represent radium-226 decaying to radon-222 plus an alpha particle.

> Samarium-147 is one of many rare earth isotopes that undergo alpha decay. Write a balanced nuclear equation for this process.

> How many protons and neutrons are contained in each of the three isotopes of carbon?

> How many protons and neutrons are contained in the nucleus of uranium-235?

> Write the nuclear symbol for carbon-14.

> Rank the four major types of radiation in order of size, speed, and penetrating power.

> What is the major difference between beta and gamma radiation?

> Write the nuclear symbol for a beta particle.

> We can control the rate of chemical reactions. Can we control the rate of natural radiation?

> Observed increases in global temperatures are caused by elevated levels of carbon dioxide. Is this statement a theory or a scientific law? Explain your reasoning.

> What are the major differences between alpha particles and gamma radiation?

> What is the composition of a positron?

> What is alpha decay?

> How does the energy of gamma radiation compare with that of other regions of the electromagnetic spectrum?

> A buffer solution is prepared in such a way that the concentration of propanoic acid is 2.00 3 1021 M and the concentration of sodium propanoate is 4.00 3 1021 M. If the buffer equilibrium is described by Ka = 1.34 × 10-5 use the Henderso

> Barium-131 is a radioisotope used to study bone formation. A patient ingested barium-131. How much time will elapse until only one-fourth of the barium-131 remains, assuming that none of the isotope is eliminated from the body through normal processes? T

> Calculate the pH of a buffer system containing 1.0 M NH3 and 1.0 M NH4Cl. (Ka of NH4+, the acid in this system, is 5.6 × 10-10.)

> What is the pH of the solution described in Question 8.101? Question 8.101: What is [H3O+] for a buffer solution that is 0.200 M in acid and 0.500 M in the corresponding salt if the weak acid Ka = 5.80 × 10-7?