21.8: Exercises

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Write the chemical formula and Lewis structure of the following, each of which contains five carbon atoms:

an alkane
an alkene
an alkyne

What is the difference between the hybridization of carbon atoms’ valence orbitals in saturated and unsaturated hydrocarbons?

On a microscopic level, how does the reaction of bromine with a saturated hydrocarbon differ from its reaction with an unsaturated hydrocarbon? How are they similar?

On a microscopic level, how does the reaction of bromine with an alkene differ from its reaction with an alkyne? How are they similar?

Explain why unbranched alkenes can form geometric isomers while unbranched alkanes cannot. Does this explanation involve the macroscopic domain or the microscopic domain?

Explain why these two molecules are not isomers:

How does the carbon-atom hybridization change when polyethylene is prepared from ethylene?

Write the Lewis structure and molecular formula for each of the following hydrocarbons:

(f) 4-methyl-2-pentyne

10.

Write the chemical formula, condensed formula, and Lewis structure for each of the following hydrocarbons:

(f) 3,4-dimethyl-1-pentyne

11.

Give the complete IUPAC name for each of the following compounds:

12.

Give the complete IUPAC name for each of the following compounds:

13.

Butane is used as a fuel in disposable lighters. Write the Lewis structure for each isomer of butane.

14.

Write Lewis structures and name the five structural isomers of hexane.

15.

Write Lewis structures for the cis–trans isomers of

16.

Write structures for the three isomers of the aromatic hydrocarbon xylene, C₆H₄(CH₃)₂.

17.

Isooctane is the common name of the isomer of C₈H₁₈ used as the standard of 100 for the gasoline octane rating:

The hydrocarbon molecular structure shown includes C H subscript 3 C H C H subscript 2 C C H subscript 3. There is a C H subscript 3 group bonded to the second C atom in the chain (from left to right). There are two C H subscript 3 groups bonded above and below the fourth C atom in the chain.

What is the IUPAC name for the compound?
Name the other isomers that contain a five-carbon chain with three methyl substituents.

18.

Write Lewis structures and IUPAC names for the alkyne isomers of C₄H₆.

19.

Write Lewis structures and IUPAC names for all isomers of C₄H₉Cl.

20.

Name and write the structures of all isomers of the propyl and butyl alkyl groups.

21.

Write the structures for all the isomers of the –C₅H₁₁ alkyl group.

22.

Write Lewis structures and describe the molecular geometry at each carbon atom in the following compounds:

cis-3-hexene
cis-1-chloro-2-bromoethene
2-pentyne
trans-6-ethyl-7-methyl-2-octene

23.

Benzene is one of the compounds used as an octane enhancer in unleaded gasoline. It is manufactured by the catalytic conversion of acetylene to benzene:

Draw Lewis structures for these compounds, with resonance structures as appropriate, and determine the hybridization of the carbon atoms in each.

24.

Teflon is prepared by the polymerization of tetrafluoroethylene. Write the equation that describes the polymerization using Lewis symbols.

25.

Write two complete, balanced equations for each of the following reactions, one using condensed formulas and one using Lewis structures.

1 mol of 1-butyne reacts with 2 mol of iodine.
Pentane is burned in air.

26.

Write two complete, balanced equations for each of the following reactions, one using condensed formulas and one using Lewis structures.

2-butene reacts with chlorine.
benzene burns in air.

27.

What mass of 2-bromopropane could be prepared from 25.5 g of propene? Assume a 100% yield of product.

28.

Acetylene is a very weak acid; however, it will react with moist silver(I) oxide and form water and a compound composed of silver and carbon. Addition of a solution of HCl to a 0.2352-g sample of the compound of silver and carbon produced acetylene and 0.2822 g of AgCl.

What is the empirical formula of the compound of silver and carbon?
The production of acetylene on addition of HCl to the compound of silver and carbon suggests that the carbon is present as the acetylide ion, . Write the formula of the compound showing the acetylide ion.

29.

Ethylene can be produced by the pyrolysis of ethane:

How many kilograms of ethylene is produced by the pyrolysis of 1.000 10³ kg of ethane, assuming a 100.0% yield?

30.

Why do the compounds hexane, hexanol, and hexene have such similar names?

31.

Write condensed formulas and provide IUPAC names for the following compounds:

ethyl alcohol (in beverages)
methyl alcohol (used as a solvent, for example, in shellac)
ethylene glycol (antifreeze)
isopropyl alcohol (used in rubbing alcohol)
glycerine

32.

Give the complete IUPAC name for each of the following compounds:

(a)

This shows a C H subscript 3 group bonded to a C H group. The C atom in the C H group is bonded above to an O H group. The C in the C H group is also bonded below to a C H subscript 2 group. The C H subscript 2 group is bonded below to a C H subscript 3 group.

(b)

This shows a C H subscript 3 group bonded to a C atom. The C atom is bonded to an O H group and an I atom. It is also bonded to a second C atom. This second C atom is bonded above and below to a C H subscript 3 group. The second C atom is bonded to a C H subscript 2 group with is bonded to a C H subscript 3 group.

(c)

33.

Give the complete IUPAC name and the common name for each of the following compounds:

(a)

This shows a C H subscript 3 group bonded to a C H subscript 2 group. This C H subscript 2 group is bonded to an O atom which is also bonded to a C H subscript 2 group. This C H subscript 2 group is bonded to a C H subscript 2 group. This C H subscript 2 group is bonded to a C H subscript 2 group. This C H subscript 2 group is bonded to a C H subscritp 3 group. All bonds are in a straight line.

(b)

This shows a C H subscript 3 group bonded to a C H subscript 2 group. This C H subscript 2 group is bonded to an O atom. This O atom is bonded to a C H subscript 2 group which is also bonded to another C H subscript 2 group. This C H subscript 2 group is bonded to a C H subscript 3 group. All bonds are in a straight line.

(c)

This figure shows a C H subscript 3 group bonded to an O atom. This O atom is bonded to a C H subscript 2 group which is also bonded to another C H subscript 2 group. This C H subscript 2 group is bonded to a C H subscript 3 group. All bonds are in a straight line.

34.

Write the condensed structures of both isomers with the formula C₂H₆O. Label the functional group of each isomer.

35.

Write the condensed structures of all isomers with the formula C₂H₆O₂. Label the functional group (or groups) of each isomer.

36.

Draw the condensed formulas for each of the following compounds:

dipropyl ether
2,2-dimethyl-3-hexanol
2-ethoxybutane

37.

MTBE, Methyl tert-butyl ether, CH₃OC(CH₃)₃, is used as an oxygen source in oxygenated gasolines. MTBE is manufactured by reacting 2-methylpropene with methanol.

Using Lewis structures, write the chemical equation representing the reaction.
What volume of methanol, density 0.7915 g/mL, is required to produce exactly 1000 kg of MTBE, assuming a 100% yield?

38.

Write two complete balanced equations for each of the following reactions, one using condensed formulas and one using Lewis structures.

propanol is converted to dipropyl ether
propene is treated with water in dilute acid.

39.

Write two complete balanced equations for each of the following reactions, one using condensed formulas and one using Lewis structures.

2-butene is treated with water in dilute acid
ethanol is dehydrated to yield ethene

40.

Order the following molecules from least to most oxidized, based on the marked carbon atom:

41.

Predict the products of oxidizing the molecules shown in this problem. In each case, identify the product that will result from the minimal increase in oxidation state for the highlighted carbon atom:

(a)

(b)

The left side of a reaction and arrow are shown. The arrow is labeled with an O in brackets. To the left of the arrow is a molecular structure. It shows a C H subscript 3 group bonded up and to the right to a C H subscript 2 group bonded down and to the right to a C H subscript 2 group which is bonded up and to the right to an O H group. The C in the second C H subscript 2 group is red.

(c)

42.

Predict the products of reducing the following molecules. In each case, identify the product that will result from the minimal decrease in oxidation state for the highlighted carbon atom:

(a)

The left side of a reaction and arrow are shown. The arrow is labeled with an R in brackets. To the left of the arrow is a molecular structure that shows a central, red C atom. This C atom is bonded to a C H subscript 3 group, and H atom, and an O atom. It forms a double bond with the O atom.

(b)

The left side of a reaction and arrow are shown. The arrow is labeled with an R in brackets. To the left of the arrow is a molecular structure that shows a central, red C atom. This C atom is bonded to 2 C H subscript 3 groups, and it forms a double bond with an O atom.

(c)

The left side of a reaction and arrow are shown. The arrow is labeled with an R in brackets. To the left of the arrow is a molecular structure which shows a central, red C atom which is bonded to a C H subscript 3 group, and O H group, and forms a double bond with an O atom.

43.

Explain why it is not possible to prepare a ketone that contains only two carbon atoms.

44.

How does hybridization of the substituted carbon atom change when an alcohol is converted into an aldehyde? An aldehyde to a carboxylic acid?

45.

Fatty acids are carboxylic acids that have long hydrocarbon chains attached to a carboxylate group. How does a saturated fatty acid differ from an unsaturated fatty acid? How are they similar?

46.

Write a condensed structural formula, such as CH₃CH₃, and describe the molecular geometry at each carbon atom.

(f) formaldehyde

47.

Write a condensed structural formula, such as CH₃CH₃, and describe the molecular geometry at each carbon atom.

2-propanol
acetone
dimethyl ether
acetic acid
3-methyl-1-hexene

48.

The foul odor of rancid butter is caused by butyric acid, CH₃CH₂CH₂CO₂H.

Draw the Lewis structure and determine the oxidation number and hybridization for each carbon atom in the molecule.
The esters formed from butyric acid are pleasant-smelling compounds found in fruits and used in perfumes. Draw the Lewis structure for the ester formed from the reaction of butyric acid with 2-propanol.

49.

Write the two-resonance structures for the acetate ion.

50.

Write two complete, balanced equations for each of the following reactions, one using condensed formulas and one using Lewis structures:

ethanol reacts with propionic acid
benzoic acid, C₆H₅CO₂H, is added to a solution of sodium hydroxide

51.

Write two complete balanced equations for each of the following reactions, one using condensed formulas and one using Lewis structures.

1-butanol reacts with acetic acid
propionic acid is poured onto solid calcium carbonate

52.

Yields in organic reactions are sometimes low. What is the percent yield of a process that produces 13.0 g of ethyl acetate from 10.0 g of CH₃CO₂H?

53.

Alcohols A, B, and C all have the composition C₄H₁₀O. Molecules of alcohol A contain a branched carbon chain and can be oxidized to an aldehyde; molecules of alcohol B contain a linear carbon chain and can be oxidized to a ketone; and molecules of alcohol C can be oxidized to neither an aldehyde nor a ketone. Write the Lewis structures of these molecules.

54.

Write the Lewis structures of both isomers with the formula C₂H₇N.

55.

What is the molecular structure about the nitrogen atom in trimethyl amine and in the trimethyl ammonium ion, (CH₃)₃NH⁺? What is the hybridization of the nitrogen atom in trimethyl amine and in the trimethyl ammonium ion?

56.

Write the two resonance structures for the pyridinium ion, C₅H₅NH⁺.

57.

Draw Lewis structures for pyridine and its conjugate acid, the pyridinium ion, C₅H₅NH⁺. What are the hybridizations, electron domain geometries, and molecular geometries about the nitrogen atoms in pyridine and in the pyridinium ion?

58.

Write the Lewis structures of all isomers with the formula C₃H₇ON that contain an amide linkage.

59.

Write two complete balanced equations for the following reaction, one using condensed formulas and one using Lewis structures.

Methyl amine is added to a solution of HCl.

60.

Write two complete, balanced equations for each of the following reactions, one using condensed formulas and one using Lewis structures.

Ethylammonium chloride is added to a solution of sodium hydroxide.

61.

Identify any carbon atoms that change hybridization and the change in hybridization during the reactions in Exercise 20.26.

62.

Identify any carbon atoms that change hybridization and the change in hybridization during the reactions in Exercise 20.39.

63.

Identify any carbon atoms that change hybridization and the change in hybridization during the reactions in Exercise 20.51.

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