{"id":1252,"date":"2018-11-28T16:55:00","date_gmt":"2018-11-28T16:55:00","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-potsdam-organicchemistry2\/?post_type=chapter&p=1252"},"modified":"2019-01-08T15:23:47","modified_gmt":"2019-01-08T15:23:47","slug":"20-1-introduction-to-polar-pi-bonds","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-potsdam-organicchemistry2\/chapter\/20-1-introduction-to-polar-pi-bonds\/","title":{"raw":"20.1. Introduction to polar pi Bonds","rendered":"20.1. Introduction to polar pi Bonds"},"content":{"raw":"
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Nucleophilic additions to aldehydes and ketones: the general picture<\/span><\/h2>\r\n<\/div>\r\n<\/header>
Before we consider in detail the reactivity of aldehydes and ketones, we need to look back and remind ourselves of what the bonding picture looks like in a carbonyl.\u00a0 Carbonyl carbons are sp2<\/sup> hybridized, with the three sp2<\/sup> orbitals forming soverlaps with orbitals on the oxygen and on the two carbon or hydrogen atoms.\u00a0 These three bonds adopt trigonal planar geometry.\u00a0 The remaining unhybridized 2p orbital on the central carbonyl carbon is perpendicular to this plane, and forms a \u2018side-by-side\u2019 pbond with a 2p orbital on the oxygen.\"image006.png\"The carbon-oxygen double bond is polar: oxygen is more electronegative than carbon, so electron density is higher on the oxygen side of the bond and lower on the carbon side.\u00a0 Recall that bond polarity can be depicted with a dipole arrow, or by showing the oxygen as holding a partial negative charge and the carbonyl carbon a partial positive charge.\"image008.png\"A third way to illustrate the carbon-oxygen dipole is to consider the two main resonance contributors of a carbonyl group: the major form, which is what you typically see drawn in Lewis structures, and a minor but very important contributor in which both electrons in the pbond are localized on the oxygen, giving it a full negative charge.\u00a0 The latter depiction shows the carbon with an empty 2p orbital and a full positive charge.The result of carbonyl bond polarization, however it is depicted, is straightforward to predict. The carbon, because it is electron-poor, is an electrophile: it is a great target for attack by an electron-rich nucleophilic group. Because the oxygen end of the carbonyl double bond bears a partial negative charge, anything that can help to stabilize this charge by accepting some of the electron density will increase the bond\u2019s polarity and make the carbon more electrophilic. Very often a general acid group serves this purpose, donating a proton to the carbonyl oxygen.\"image010.png\"The same effect can also be achieved if a Lewis acid, such as a magnesium ion, is located near the carbonyl oxygen.Unlike the situation in a nucleophilic substitution reaction, when a nucleophile attacks an aldehyde or ketone carbon there is no leaving group \u2013 the incoming nucleophile simply \u2018pushes\u2019 the electrons in the pi bond up to the oxygen.\"image012.png\"Alternatively, if you start with the minor resonance contributor, you can picture this as an attack by a nucleophile on a carbocation.\r\n\r\n\"image014.png\"\r\n\r\nAfter the carbonyl is attacked by the nucleophile, the negatively charged oxygen has the capacity to act as a nucleophile.\u00a0 However, most commonly the oxygen acts instead as a base, abstracting a proton from a nearby acid group in the solvent or enzyme active site.\r\n\r\n\"image016.png\"\r\n\r\nThis very common type of reaction is called a nucleophilic addition<\/strong>. In many biologically relevant examples of nucleophilic addition to carbonyls, the nucleophile is an alcohol oxygen or an amine nitrogen, or occasionally a thiol sulfur. In one very important reaction type known as an aldol reaction (which we will learn about in section 13.3<\/a>) the nucleophile attacking the carbonyl is a resonance-stabilized carbanion.\u00a0 In this chapter, we will concentrate on reactions where the nucleophile is an oxygen or nitrogen.\r\n\r\n. . . on to the next section <\/a>. . .\r\n
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Contributors<\/h3>\r\n