Question: Why do linear alkanes have higher melting

> Provide the complete IUPAC name for each of the compounds in Question 11.3. Question 11.3: In each of the following pairs of molecules, identify the cis-isomer and the trans-isomer. H H H CH CH3 а. C=C C=C CH;CH, CH,CH3 CH;CH2 H Br, b. Br. CH3 C=C

> What is meant by a geometric isomer?

> Describe the major differences between ionic and covalent bonds.

> Arrange the following groups of molecules from the highest to the lowest melting points. b.

> Convert the condensed structures in Question 10.33 into line formulas. Question 10.33: a. CH3CH2CH2OH b. CH3CH2CH2NH2 c. d. // e. f. CH3CH2OCH2CH3 g. CH3CH2CH2I CH;CH,CH,C=0 CH;CH,CH,C=0 ОН

> What are the bond angles in ethyne?

> Convert the following condensed formulas into structural formulas: a. CH3CH2CH(CH2CH3) CH2CH2CH3 b. CH3CH(CH3) CH(CH3) CH2CH2CH2CH3

> What are the bond angles in ethene?

> What are the characteristic functional groups of alkenes and alkynes?

> Convert the structural formulas in Question 10.22 into condensed formulas. Question 10.22: 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

> Draw each of the following compounds: a. 2,3-Dichlorotoluene b. 3-Bromoaniline c. 1-Bromo-3-ethylbenzene d. o-Nitrotoluene e. p-Xylene f. o-Dibromobenzene

> Is the final product in each of the reactions in Question 11.19 an aldehyde or a ketone? Question 11.19: Write equations for the complete hydration of each of the following alkynes: a. H3CC———CH b. H3CC———CCH2CH3

> Name the following compounds using the IUPAC Nomenclature System: a. CH3C———CCH2CH3 b. CH3CH2CHBrCHBrCH2C———CH c. CH3CH(CH3) CCl—— C(CH3) CH(CH3)2 d. CH3CH(CH2CH3) C———CCHClCH3

> A bacterial culture is given 14C-labeled pyruvate as its sole source of carbon and energy. The following is the structure of the radiolabeled pyruvate. CH3-C*-C-o

> Write an equation for the hydration of each of the following alkenes. Predict the major product of each of the reactions. a. CH2——CHCH2CH2CH3 b. CH3CH2CH2CH—— CHCH3 c. CH3CHBrCH2CH—— CHCH2Cl d. CH3CH2CH2CH2CH2CH—— CHCH3

> Using the IUPAC Nomenclature System, name each of the products and reactants in the reactions described in Question 11.13. Question 11.13: Write a balanced equation for the addition of bromine to each of the following alkenes. Draw the products and rea

> Using the IUPAC Nomenclature System, name each of the products and reactants in the reactions described in Question 11.11. Question 11.11: Write balanced equations for the complete hydrogenation of each of the following alkynes: a. H3CC ———CCH3 b. H3C

> Write balanced equations for the hydrogenation of 1-butene and cis-2-butene. CH-(CH,-CH=CH-(CH,) -CH2 CH,CH),-CH,-CH (CH,)- CH2 зн, 200°С, CH 25 рsі, metal catalyst CH3-(CH2-CH=CH-(CH2)7 + CH(CH2)7-CH-CH-(CH2) CH CH3-(CH2-CH=CH-(CH2)7 -CH2 CHCH2),-C

> Write a balanced equation for the complete combustion of each of the following: a. pentane b. hexane c. octane d. ethane

> Explain why halogenation of an alkane is a substitution reaction.

> What is meant by free rotation around a carbon-carbon single bond? Why can’t conformations be separated from one another?

> 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.

> 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

> For gasoline, isooctane, 2,2,4-trimethylpentane, is the standard of excellence. Write a balanced equation for the complete combustion of isooctane.

> 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