This page guides you through the mechanism for the nucleophilic addition / elimination reaction between acyl chlorides (acid chlorides) and amines.

Ethanoyl chloride is taken as a typical acyl chloride. Similarly, ethylamine is taken as a typical amine. Changing either the acyl choride or the amine won't affect the mechanism in any way.

Remember that the reaction produces N-ethylethanamide and ethylammonium chloride.

N-ethylethanamide is an N-substituted amide. Ethanamide (a simple amide) has the formula CH₃CONH₂. In an N-substituted amide, one of the hydrogens on the nitrogen has been substituted by a hydrocarbon group – which may be either an alkyl group (as here), or a benzene ring.

In the case we are discussing, an ethyl group has replaced one of the hydrogens on the nitrogen – hence N-ethylethanamide.

The other product is ethylammonium chloride. Ammonium chloride is NH₄Cl. In ethylammonium chloride, one of the hydrogens on the nitrogen has been substituted by an ethyl group.

Nucleophiles are either fully negative ions, or else have a strongly δ- charge somewhere on a molecule.

Nitrogen is more electronegative than both hydrogen and carbon and so drags the bonding electrons towards itself. That produces a significant amount of negative charge on the nitrogen atom. The nitrogen also has an active lone pair of electrons. It is this which attacks the ethanoyl chloride.

The carbon atom in the -COCl group has both an oxygen atom and a chlorine atom attached to it. Both of these are very electronegative. They both pull electrons towards themselves, leaving the carbon atom quite positively charged. It is that carbon atom which is attacked by the lone pair on the nitrogen atom in an ethylamine molecule.

The ethanoyl chloride molecule is also planar (flat) around that carbon atom, and that leaves plenty of room for a nucleophile to attack either from above or below the plane of the molecule.

The reaction happens in two main stages – an addition stage, followed by an elimination stage.

In the addition stage, an ethylamine molecule becomes attached to the carbon in the ethanoyl chloride.

As the lone pair on the nitrogen approaches the fairly positive carbon in the ethanoyl chloride, it moves to form a bond with it. In the process, the two electrons in one of the carbon-oxygen bonds are repelled entirely onto the oxygen, leaving it negatively charged.

Notice that the nitrogen atom has gained a positive charge. The underlying reason for this is that when the lone pair forms a bond with the carbon, electrons are moving away from the nitrogen. What matters, though, is that you remember to show the positive charge in an exam. Think of it like this:

If you leave out the positive charge, two things are wrong with the equation:

• The charges don't balance. You start with two overall neutral molecules and, if you forgot the positive charge, you would end up with a negative ion. There has got to be a positive charge somewhere to balance the negative one.
• The nitrogen looks wrong! Nitrogen normally forms three bonds, but here it is forming four. Nitrogen can only form four bonds if it carries a positive charge. (A positively charged nitrogen atom has the same electronic structure as carbon – which normally forms four bonds.)

Finally, one of the hydrogens attached to the nitrogen is removed as a hydrogen ion. The electrons in the hydrogen-nitrogen bond move back onto the nitrogen, cancelling the positive charge.

The hydrogen ion might be removed in one of two ways. The first way is entirely consistent with what happens in the reactions between water or ethanol and acyl chlorides. The hydrogen is removed by the chloride ion.

The hydrogen chloride produced would at once react with any excess ethylamine present to form ethylammonium chloride.

The other (more likely) possibility is that the hydrogen ion gets removed directly by an ethylamine molecule. This forms an ethylammonium ion. The ethylammonium ion together with the chloride ion formed in the previous stage makes up the ethylammonium chloride produced in the reaction.