Editing Acyl group (section)

==Reactivity trends==
There are five main types of acyl derivatives. [[Acid halide]]s are the most reactive towards nucleophiles, followed by [[anhydride]]s, [[ester]]s, and [[amide]]s. [[Carboxylate]] ions are essentially unreactive towards nucleophilic substitution, since they possess no leaving group. The reactivity of these five classes of compounds covers a broad range; the relative reaction rates of acid chlorides and amides differ by a factor of 10<sup>13</sup>.<ref name=carey>{{cite book|last=Carey|first=Francis A.|title=Organic Chemistry|year=2006|publisher=McGraw-Hill|location=New York|isbn=0072828374|pages=[https://archive.org/details/organicchemistry6th00care/page/866 866–868]|edition=6th|url=https://archive.org/details/organicchemistry6th00care/page/866}}</ref>

:[[File:Reactivity of Carboxylic Acid Derivatives Towards Nucleophiles.png|Acid chlorides are most reactive towards nucleophiles, followed by anhydrides, esters, amides, and carboxylate anions.|590px]]

A major factor in determining the reactivity of acyl derivatives is leaving group ability, which is related to acidity. Weak bases are better leaving groups than strong bases; a species with a strong [[conjugate acid]] (e.g. [[hydrochloric acid]]) will be a better leaving group than a species with a weak conjugate acid (e.g. [[acetic acid]]). Thus, [[chloride]] ion is a better leaving group than [[acetate ion]]. The reactivity of acyl compounds towards nucleophiles decreases as the basicity of the leaving group increases, as the table shows.<ref name=wade3>Wade 2010, pp. 998–999.</ref>

{| class="wikitable"
|-
! Compound Name
! Structure
! Leaving Group
! width="120" | p''K<sub>a</sub>'' of Conjugate Acid
|-
| [[Acetyl chloride]]
| [[File:Acetyl-chloride_skeletal.svg|center|60px]]
| [[File:Chloride.png|center|34px]]
| −7
|-
| [[Acetic anhydride]]
| [[File:Acetic anhydride2DACS.svg|center|96px]]
| [[File:Acetate anion.png|center|69px]]
| 4.76
|-
| [[Ethyl acetate]]
| [[File:Ethyl-acetate-2D-skeletal.svg|center|96px]]
| [[File:Ethoxide.png|center|69px]]
| 15.9
|-
| [[Acetamide]]
| [[File:Acetamide-2D-skeletal.png|center|77px]]
| [[File:Amide anion.png|center|48px]]
| 38
|-
| [[Acetate]] anion 
| [[File:Acetate anion.png|center|69px]]
| N/a
| N/a
|-
|}

[[File:Resonance Forms of an Amide.png|thumb|264px|The two major resonance forms of an amide.]] Another factor that plays a role in determining the reactivity of acyl compounds is [[resonance (chemistry)|resonance]]. Amides exhibit two main resonance forms. Both are major contributors to the overall structure, so much so that the amide bond between the carbonyl carbon and the amide nitrogen has significant [[double bond]] character. The [[activation energy|energy barrier]] for rotation about an amide bond is 75–85 kJ/mol (18–20 kcal/mol), much larger than values observed for normal single bonds. For example, the C–C bond in ethane has an energy barrier of only 12 kJ/mol (3 kcal/mol).<ref name=carey /> Once a nucleophile attacks and a tetrahedral intermediate is formed, the energetically favorable resonance effect is lost. This helps explain why amides are one of the least reactive acyl derivatives.<ref name=wade3 />

Esters exhibit less resonance stabilization than amides, so the formation of a tetrahedral intermediate and subsequent loss of resonance is not as energetically unfavorable. Anhydrides experience even weaker resonance stabilization, since the resonance is split between two carbonyl groups, and are more reactive than esters and amides. In acid halides, there is very little resonance, so the energetic penalty for forming a tetrahedral intermediate is small. This helps explain why acid halides are the most reactive acyl derivatives.<ref name=wade3 />