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20.7: Exercises

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    1.

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

    1. an alkane
    2. an alkene
    3. an alkyne
    2.

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

    3.

    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?

    4.

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

    5.

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

    6.

    Explain why these two molecules are not isomers:

    Two structural formulas are shown. In the first, a chain of six carbon atoms with a single double bond between carbons two and three counting right to left across the molecule is shown with twelve total H atoms bonded. H atoms are bonded at each end of the molecule as well as above. H atoms are also bonded below all C atoms except those involved in the double bond. In the second structure, a hydrocarbon chain of five C atoms connected by single bonds is shown. A single C with three attached H atoms is bonded beneath the second carbon counting right to left across the molecule.

    7.

    Explain why these two molecules are not isomers:

    Two structural formulas are shown. In the first, a horizontal hydrocarbon chain consisting of six singly bonded C atoms is shown. Each C atom has an H atom bonded above and below it. The two C atoms on either end of the chain each have a third H atom bonded to them. In the second structure, a horizontal hydrocarbon chain composed of five C atoms connected by single bonds is shown with a sixth C atom singly bonded beneath the right-most C atom. The first C atom (from left to right) has three H atoms bonded to it. The second C atom has two H atoms bonded to it. The third C atom has two H atoms bonded to it. The fourth C atom has two H atoms bonded to it. The fifth C atom has two H atoms bonded to it. The C atom bonded below the fifth C atom has three H atoms bonded to it.

    8.

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

    9.

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

    1. (f) 4-methyl-2-pentyne
    10.

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

    1. (f) 3,4-dimethyl-1-pentyne
    11.

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

    1. (c)

      This structure shows a hydrocarbon chain composed of C H subscript 3 C H C H subscript 2 C H subscript 3 with a C H subscript 3 group attached beneath the second C atom counting left to right.

      (d)

      (e)

      This structure shows a horizontal chain composed of C H subscript 3 C F C H subscript 2 C H subscript 2 C H subscript 2 C H subscript 3 with a C H subscript 2 C H triple bond C H group attached beneath the second C atom counting left to right.

      (f)

      This structure shows two double bounded C atoms with C l attached to the upper left, C H subscript 3 attached to the lower right, and H atoms attached to the upper right and lower left in the structure.

      (g)

    12.

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

    1. (c)

      This structure shows a hydrocarbon chain composed of C H subscript 3 C H C H subscript 3 with a C H subscript 2 C H subscript 3 group attached beneath the second C atom counting left to right.

      (d)

      (e)

      This structure shows a hydrocarbon chain composed of C H subscript 3 C H subscript 2 C H subscript 2 C H B r C H subscript 2 C H subscript 3 with a C H subscript 2 C H double bond C H subscript 2 group attached beneath the second C atom counting left to right.

      (f)

    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.

    1. What is the IUPAC name for the compound?
    2. 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:

    1. cis-3-hexene
    2. cis-1-chloro-2-bromoethene
    3. 2-pentyne
    4. 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. 1 mol of 1-butyne reacts with 2 mol of iodine.
    2. 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.

    1. 2-butene reacts with chlorine.
    2. 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.

    1. What is the empirical formula of the compound of silver and carbon?
    2. 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:

    1. ethyl alcohol (in beverages)
    2. methyl alcohol (used as a solvent, for example, in shellac)
    3. ethylene glycol (antifreeze)
    4. isopropyl alcohol (used in rubbing alcohol)
    5. 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)

    This shows a C H subscript 3 group bonded to a C H group. The C atom in the C H group is bonded to an O H group. The C H group is bonded to a C atom. The C atom is bonded below to a C l atom and above to a C H subscript 2 group. The C atom in the C H subscript 2 group is also bonded to a C H subscript 3 group. The C atom is also bonded to a C H subscript 2 group to the right. This C H subscript 2 group is bonded to another C H subscript 2 group. Below this second C H subscript 2 group a C H subscript 3 group is bonded.

    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:

    1. dipropyl ether
    2. 2,2-dimethyl-3-hexanol
    3. 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.

    1. Using Lewis structures, write the chemical equation representing the reaction.
    2. 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.

    1. propanol is converted to dipropyl ether
    2. 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.

    1. 2-butene is treated with water in dilute acid
    2. ethanol is dehydrated to yield ethene
    40.

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

    Structure a shows a C H subscript 3 group bonded up and to the right to a C H group which is bonded down and to the left to a C H subscript 3 group. Above the C H group is bonded an O H group. The C in the C H group is red. Structure b shows a C H subscript 3 group bonded up and to the right to a C H subscript 2 group which is bonded down and to the right to a C H subscript 3 group. The C in the C H subscript 2 group is red. Structure c shows a C H subscript 3 group bonded up and to the right to a red C atom. This C atom forms a double bond with an O atom above it. The C atom also forms a bond with a C H subscript 3 group down and to the right.

    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)

    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 which bonds up and to the right to a C H subscript 2 group. The C H subscript 2 group forms a bond down and to the left to a C atom. This C atom appears in red and forms a double bond with an O atom and a single bond with an H atom.

    (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)

    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 which is bonded down and to the right to a C H group. The C in this C H group appears in red. The C in the C H group is bonded directly below it to a C H subscript 3 group. The C H group is bonded up and to the right to an O H group.

    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.

    1. (f) formaldehyde
    47.

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

    1. 2-propanol
    2. acetone
    3. dimethyl ether
    4. acetic acid
    5. 3-methyl-1-hexene
    48.

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

    1. Draw the Lewis structure and determine the oxidation number and hybridization for each carbon atom in the molecule.
    2. 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:

    1. ethanol reacts with propionic acid
    2. 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. 1-butanol reacts with acetic acid
    2. 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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