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A general linear imide functional group

In organic chemistry, an imide is a functional group consisting of two acyl groups bound to nitrogen.[1] The compounds are structurally related to acid anhydrides, although imides are more resistant toward hydrolysis. In terms of commercial applications, imides are best known as components of high-strength polymers, called polyimides.


Most imides are cyclic compounds derived from dicarboxylic acids, and their names reflect the parent acid[2]. Examples are succinimide, derived from succinic acid, and phthalimide, derived from phthalic acid. For imides derived from amines (as opposed to ammonia), the N-substituent is indicated by a prefix. For example, N-ethylsuccinimide is derived from succinic acid and ethylamine. Isoimides are isomeric with normal imides and have the formula RC(O)OC(NR′)R″. They are often intermediates that convert to the more symmetrical imides. Organic compounds called carbodiimides have the formula RN=C=NR. They are unrelated to imides.

Imides from dicarboxylic acids[edit]

The PubChem links gives access to more information on the compounds, including other names, ids, toxicity and safety.

n Common name Systematic name Structure PubChem parent dicarboxylic acid structure
2 Succinimide Pyrrolidine-2,5-dione Succinimide.svg 11439 Succinic acid Succinic acid.png
2, unsaturated, cis carbon-carbon double bonds Maleimide Pyrrole-2,5-dione Maleimide.png 10935 Maleic acid Maleic-acid-2D-skeletal-A.png
3 Glutarimide Piperidine-2,6-dione Glutarimide.svg 70726 Glutaric acid Glutaric acid.png
6 Phthalimide Isoindole-1,3-dione Phthalimide.svg 6809 Phthalic acid Phthalic-acid-2D-skeletal.png


Being highly polar, imides exhibit good solubility in polar media. The N–H center for imides derived from ammonia is acidic and can participate in hydrogen bonding. Unlike the structurally related acid anhydrides, they resist hydrolysis and some can even be recrystallized from boiling water.

Occurrence and applications[edit]

Many high strength or electrically conductive polymers contain imide subunits, i.e., the polyimides. One example is Kapton where the repeat unit consists of two imide groups derived from aromatic tetracarboxylic acids.[3] Another example of polyimides is the polyglutarimide typically made from polymethylmethacrylate (PMMA) and ammonia or a primary amine by aminolysis and cyclization of the PMMA at high temperature and pressure, typically in an extruder. This technique is called reactive extrusion. A commercial polyglutarimide product based on the methylamine derivative of PMMA, called Kamax, was produced by the Rohm and Haas company. The toughness of these materials reflects the rigidity of the imide functional group.

Interest in the bioactivity of imide-containing compounds was sparked by the early discovery of the high bioactivity of the Cycloheximide as an inhibitor of protein biosynthesis in certain organisms. Thalidomide, famous for its adverse effects, is one result of this research. A number of fungicides and herbicides contain the imide functionality. Examples include Captan, which is considered carcinogenic under some conditions, and Procymidone.[4]

Illustrative imides, from left: N-ethylmaleimide, a biochemical reagent; phthalimide, an industrial chemical intermediate; Captan, a controversial pesticide; thalidomide, a drug that once caused many birth defects; a subunit of Kapton, a high strength polymer used to make space suits.

In the 21st century new interest arose in thalidomide's immunomodulatory effects, leading to the class of immunomodulators known as immunomodulatory imide drugs (IMiDs).


Most common imides are prepared by heating dicarboxylic acids or their anhydrides and ammonia or primary amines. The result is a condensation reaction:[5]

(RCO)2O + R′NH2 → (RCO)2NR′ + H2O

These reactions proceed via the intermediacy of amides. The intramolecular reaction of a carboxylic acid with an amide is far faster than the intermolecular reaction, which is rarely observed.

They may also be produced via the oxidation of amides, particularly when starting from lactams.[6]

R(CO)NHCH2R' + 2 [O] → R(CO)N(CO)R' + H2O

Certain imides can also be prepared in the isoimide-to-imide Mumm rearrangement.


For imides derived from ammonia, the N–H center is weakly acidic. Thus, alkali metal salts of imides can be prepared by conventional bases such as potassium hydroxide. The conjugate base of phthalimide is potassium phthalimide. These anion can be alkylated to give N-alkylimides, which in turn can be degraded to release the primary amine. Strong nucleophiles, such as potassium hydroxide or hydrazine are used in the release step.

Treatment of imides with halogens and base gives the N-halo derivatives. Examples that are useful in organic synthesis are N-chlorosuccinimide and N-bromosuccinimide, which respectively serve as sources of "Cl+" and "Br+" in organic synthesis.

Imides in coordination chemistry[edit]

The ligand in coordination chemistry known as imide has the formula NR. Imido ligands form multiple bond to the metal. In some the M-N-C angle is 180º but often the angle is decidedly bent. The parent imide (NH2-) is an intermediate in nitrogen fixation by synthetic catalysts.[7]

Structure of a representative imido complex (py = pyridine, CMe3 = tert-butyl)[8]


  1. ^
  2. ^ Martynov, A. V. (2005-12-06). "New Approach to the Synthesis of trans-Aconitic Acid Imides". ChemInform. 36 (49): no–no. doi:10.1002/chin.200549068. ISSN 1522-2667.
  3. ^ Walter W. Wright and Michael Hallden-Abberton "Polyimides" in Ullmann's Encyclopedia of Industrial Chemistry, 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a21_253
  4. ^ Peter Ackermann, Paul Margot, Franz Müller "Fungicides, Agricultural" in Ullmann's Encyclopedia of Industrial Chemistry, 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a12_085
  5. ^ Vincent Rodeschini, Nigel S. Simpkins, and Fengzhi Zhangi (2009). "Illustrative imide formation from amine and anhydride". Organic Syntheses.; Collective Volume, 11, p. 1028
  6. ^ Sperry, Jonathan (27 September 2011). "The Oxidation of Amides to Imides: A Powerful Synthetic Transformation". Synthesis. 2011 (22): 3569–3580. doi:10.1055/s-0030-1260237.
  7. ^ Nugent, W. A.; Mayer, J. M., "Metal-Ligand Multiple Bonds," J. Wiley: New York, 1988.
  8. ^ Hazari, N.; Mountford, P., "Reactions and Applications of Titanium Imido Complexes", Acc. Chem. Res. 2005, 38, 839-849. doi:10.1021/ar030244z

External links[edit]