{"id":1377,"date":"2018-03-21T15:03:13","date_gmt":"2018-03-21T15:03:13","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-orgbiochemistry\/chapter\/reactions-of-alcohols\/"},"modified":"2018-10-30T18:48:29","modified_gmt":"2018-10-30T18:48:29","slug":"reactions-of-alcohols","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/chapter\/reactions-of-alcohols\/","title":{"raw":"14.5 Reactions of Alcohols","rendered":"14.5 Reactions of Alcohols"},"content":{"raw":"
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Learning Objectives<\/h3>\r\n
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  1. Give three major types of reactions of alcohols.<\/li>\r\n \t
  2. Describe the result of the oxidation of a primary alcohol.<\/li>\r\n \t
  3. Describe the result of the oxidation of a secondary alcohol.<\/li>\r\n<\/ol>\r\n<\/div>\r\nChemical reactions in alcohols occur mainly at the functional group, but some involve hydrogen atoms attached to the OH-bearing carbon atom or to an adjacent carbon atom. Of the three major kinds of alcohol reactions, which are summarized in <\/span>Figure 14.4 \"Reactions of Alcohols\"<\/a>, two\u2014dehydration and oxidation\u2014are considered here. The third reaction type\u2014esterification\u2014is covered in <\/span>Chapter 15 \"Organic Acids and Bases and Some of Their Derivatives\"<\/a>, <\/span>Section 15.8 \"Preparation of Esters\"<\/a>.<\/span>\r\n\r\n<\/div>\r\n
    \r\n\r\n[caption id=\"\" align=\"alignnone\" width=\"2538\"]\"image\" Figure 14.4 Reactions of Alcohols.\u00a0 Oxidation and dehydration of alcohols are considered here. <\/em>[\/caption]\r\n\r\n<\/div>\r\n
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    Dehydration<\/h2>\r\n

    As noted in Figure 14.4 \"Reactions of Alcohols\"<\/a>, an alcohol undergoes dehydration in the presence of a catalyst to form an alkene and water. The reaction removes the OH group from the alcohol carbon atom and a hydrogen atom from an adjacent carbon atom in the same molecule.\u00a0 Note that this is the reverse of the hydration reaction of alkenes.<\/p>\r\n\r\n

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    Under the proper conditions, it is possible for the dehydration to occur between two<\/em> alcohol molecules. The entire OH group of one molecule and only the hydrogen atom of the OH group of the second molecule are removed. The two ethyl groups attached to an oxygen atom form an ether molecule.<\/p>\r\n\r\n

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    Note<\/h3>\r\n

    Both dehydration and hydration reactions occur continuously in cellular metabolism, with enzymes serving as catalysts and at a temperature of about 37\u00b0C. (For more information about hydration reactions, see Chapter 13 \"Unsaturated and Aromatic Hydrocarbons\"<\/a>, Section 13.4 \"Chemical Properties of Alkenes\"<\/a>.) The following reaction occurs in the Embden\u2013Meyerhof pathway. (For more information about metabolic reactions, see Chapter 20 \"Energy Metabolism\"<\/a>.)<\/p>\r\n\r\n

    \"image\"<\/div>\r\n

    Although the participating compounds are complex, the reaction is the same: elimination of water from the starting material. The idea is that if you know the chemistry of a particular functional group, you know the chemistry of hundreds of different compounds.<\/p>\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n

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    Oxidation<\/h2>\r\n

    Primary and secondary alcohols are readily oxidized. We saw earlier how methanol and ethanol are oxidized by liver enzymes to form aldehydes. Because a variety of oxidizing agents can bring about oxidation, we can indicate an oxidizing agent without specifying a particular one by writing an equation with the symbol [O] above the arrow. You may picture H2<\/sub>O as a by-product. \u00a0\u00a0 For example, we write the oxidation of ethanol\u2014a primary alcohol\u2014to form acetaldehyde\u2014an aldehyde\u2014as follows:<\/p>\r\n\r\n

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    We shall see (in Section 14.9 \"Aldehydes and Ketones: Structure and Names\"<\/a>) that aldehydes are even more easily oxidized than alcohols and yield carboxylic acids.<\/p>\r\n

    Secondary alcohols are oxidized to ketones<\/em>. The oxidation of isopropyl alcohol by potassium dichromate (K2<\/sub>Cr2<\/sub>O7<\/sub>) gives acetone, the simplest ketone:<\/p>\r\n\r\n

    \"image\"<\/div>\r\n

    Unlike aldehydes, ketones are relatively resistant to further oxidation (Section 14.9 \"Aldehydes and Ketones: Structure and Names\"<\/a>), so no special precautions are required to isolate them as they form.<\/p>\r\n

    Note that in oxidation of both primary (RCH2<\/sub>OH) and secondary (R2<\/sub>CHOH) alcohols, two hydrogen atoms are removed from the alcohol molecule, one from the OH group and other from the carbon atom that bears the OH group.<\/p>\r\n\r\n

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    Note<\/h3>\r\n

    These reactions can also be carried out in the laboratory with chemical oxidizing agents. One such oxidizing agent is potassium dichromate. The balanced equation (showing only the species involved in the reaction) in this case is as follows:<\/p>\r\n\r\n

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    The complexity of this equation explains why we use [O] above the arrow to indicate that an unspecified oxidizing agent either removes 2 H atoms from or adds an O atom to the organic molecule rather than writing the details of how the oxidizing agent works.<\/div>\r\n<\/div>\r\n<\/div>\r\n

    Alcohol oxidation is important in living organisms. Enzyme-controlled oxidation reactions provide the energy cells need to do useful work. One step in the metabolism of carbohydrates involves the oxidation of the secondary alcohol group in isocitric acid to a ketone group:<\/p>\r\n\r\n

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    Note that the overall type of reaction is the same as that in the conversion of isopropyl alcohol to acetone. (For more information on metabolic reactions, see Chapter 20 \"Energy Metabolism\"<\/a>.)<\/p>\r\n

    Tertiary alcohols (R3<\/sub>COH) are resistant to oxidation because the carbon atom that carries the OH group does not have a hydrogen atom attached but is instead bonded to other carbon atoms. The oxidation reactions we have described involve the formation of a carbon-to-oxygen double bond. Thus, the carbon atom bearing the OH group must be able to release one of its attached atoms to form the double bond. The carbon-to-hydrogen bonding is easily broken under oxidative conditions, but carbon-to-carbon bonds are not. Therefore tertiary alcohols are not easily oxidized.<\/p>\r\n\r\n

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    Example 4<\/h3>\r\n

    Write an equation for the oxidation of each alcohol. Use [O] above the arrow to indicate an oxidizing agent. If no reaction occurs, write \u201cno reaction\u201d after the arrow.<\/p>\r\n\r\n

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    1. CH3<\/sub>CH2<\/sub>CH2<\/sub>CH2<\/sub>CH2<\/sub>OH<\/li>\r\n \t
    2. \r\n
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      Solution<\/p>\r\n

      The first step is to recognize the class of each alcohol as primary, secondary, or tertiary.<\/p>\r\n\r\n

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      1. \r\n

        This alcohol has the OH group on a carbon atom that is attached to only one<\/em> other carbon atom, so it is a primary alcohol. Oxidation forms first an aldehyde.\u00a0 The additional step where the aldehyde oxidizes to a carboxylic acid will be discussed in a later section.<\/p>\r\n\r\n

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      2. \r\n

        This alcohol has the OH group on a carbon atom that is attached to three other carbon atoms, so it is a tertiary alcohol. No reaction occurs.<\/p>\r\n\r\n

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      3. \r\n

        This alcohol has the OH group on a carbon atom that is attached to two other carbon atoms, so it is a secondary alcohol; oxidation gives a ketone.<\/p>\r\n\r\n

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        Skill-Building Exercise<\/h3>\r\n

        Write an equation for the oxidation of each alcohol. Use [O] above the arrow to indicate an oxidizing agent. If no reaction occurs, write \u201cno reaction\u201d after the arrow.<\/p>\r\n\r\n

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        1. \r\n
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        2. \r\n
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        3. \r\n
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          \"image\"<\/div>\r\n<\/div><\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\n
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          Concept Review Exercises<\/h3>\r\n<\/div>\r\n
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          1. \r\n
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            In a reaction, compound W with the molecular formula C4<\/sub>H10<\/sub>O is converted to compound X with the formula C4<\/sub>H8<\/sub>O. Is W oxidized, reduced, dehydrated, or none of these? Explain.<\/p>\r\n\r\n<\/div><\/li>\r\n \t

          2. \r\n
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            In a reaction, 2 mol of compound Y with the molecular formula C4<\/sub>H10<\/sub>O is converted to 1 mol of compound Z with the formula C8<\/sub>H18<\/sub>O. Is Y oxidized, reduced, or neither? Explain.<\/p>\r\n\r\n<\/div><\/li>\r\n<\/ol>\r\n[reveal-answer q=\"168363\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"168363\"]\r\n

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            1. oxidized; H is removed<\/li>\r\n \t
            2. neither; water is removed[\/hidden-answer]\r\n
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              Key Takeaways<\/h3>\r\n