INTRODUCING PHENYLAMINE

This page looks at the structure and physical properties of phenylamine - also known as aniline or aminobenzene. Phenylamine has an -NH₂ group attached directly to a benzene ring.

The structure of phenylamine

Phenylamine is a primary amine - a compound in which one of the hydrogen atoms in an ammonia molecule has been replaced by a hydrocarbon group.

However, in comparison with simple primary amines like methylamine, the properties of phenylamine are slightly different. This is because the lone pair on the nitrogen atom interacts with the delocalised electrons in the benzene ring.

The simplest way to draw the structure of phenylamine is:

There is an interaction between the delocalised electrons in the benzene ring and the lone pair on the nitrogen atom. The lone pair overlaps with the delocalised ring electron system . . .

. . . giving a structure rather like this:

The donation of the nitrogen's lone pair into the ring system increases the electron density around the ring. That makes the ring much more reactive than it is in benzene itself.

It also reduces the availability of the lone pair on the nitrogen to take part in other reactions. In particular, it makes phenylamine much more weakly basic than primary amines where the -NH₂ group isn't attached to a benzene ring. That will be explored elsewhere in this section. (See the phenylamine menu - link at the bottom of this page.)

Physical properties

Pure phenylamine is a colourless liquid, but it darkens rapidly on exposure to light and air. It is normally a brown oily liquid.

Melting and boiling points

It is useful to compare phenylamine's melting and boiling points with those of methylbenzene (toluene). Both molecules contain a similar number of electrons and are a very similar shape. That means that the intermolecular attractions due to van der Waals dispersion forces are going to be very similar.

The reason for the higher values for phenylamine is in part due to permanent dipole-dipole attractions due to the electronegativity of the nitrogen - but is mainly due to hydrogen bonding.

Hydrogen bonds can form between a lone pair on a nitrogen on one molecule and the hydrogen on the -NH₂ group of one of its neighbours.

Solubility in water

Phenylamine is slightly soluble in water - about 3.6 g (depending on where you get the data from!) of phenylamine will dissolve in 100 g of water at 20°C. Mixtures containing more phenylamine than this separate into two layers, with the phenylamine forming the bottom one.

Phenylamine is somewhat soluble in water because of its ability to form hydrogen bonds with the water.

However, the benzene rings in the phenylamine break more hydrogen bonds between water molecules than are reformed between water and the -NH₂ groups. The water molecules also disrupt fairly strong van der Waals attractions between the phenylamine molecules.

Both of these effects mean that dissolving phenylamine in water isn't very energetically profitable, and so stop the phenylamine from being very soluble.

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