INTRODUCTION TO THE ARYL HALIDES (HALOGENOARENES)
This page looks at the structure and physical properties of three simple aryl halides - chlorobenzene, bromobenzene and iodobenzene. An aryl halide has a halogen atom attached directly to a benzene ring.
The structure of chlorobenzene
We'll look in some detail at the structure of chlorobenzene. Bromobenzene and iodobenzene are just the same.
The simplest way to draw the structure of chlorobenzene is:
. . . but to understand chlorobenzene properly, you need to dig a bit deeper than this.
Warning! You need to understand about the bonding in benzene in order to make sense of this next bit.
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There is an interaction between the delocalised electrons in the benzene ring and one of the lone pairs on the chlorine atom. This overlaps with the delocalised ring electron system . . .
. . . giving a structure rather like this:
This delocalisation is by no means complete, but it does have a significant effect on the properties of both the carbon-chlorine bond and the polarity of the molecule.
The delocalisation introduces some extra bonding between the carbon and the chlorine, making the bond stronger. This has a major effect on the reactions of compounds like chlorobenzene.
There is also some movement of electrons away from the chlorine towards the ring. Chlorine is quite electronegative and usually draws electrons in the carbon-chlorine bond towards itself. In this case, this is offset to some extent by the movement of electrons back towards the ring in the delocalisation. The molecule is less polar than you would otherwise have expected.
Chlorobenzene, bromobenzene and iodobenzene are all oily liquids. The boiling points increase as the halogen atom gets bigger.
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The main attractions between the molecules will be van der Waals dispersion forces. These increase as the number of electrons in the molecule increases. This is the reason that the boiling points increase as the halogen atom gets bigger.
There will also be permanent dipole-dipole attractions involved in the chlorobenzene and bromobenzene, but very little in the iodobenzene. Iodine has much the same electronegativity as carbon.
These dipole-dipole attractions must be very unimportant relative to the dispersion forces because the most polar molecule (the chlorobenzene) has the lowest boiling point of the three.
Solubility in water
The aryl halides are insoluble in water. They are denser than water and form a separate lower layer.
The molecules are quite large compared with a water molecule. In order for chlorobenzene to dissolve it would have to break lots of existing hydrogen bonds between water molecules. You also have to break the quite strong van der Waals dispersion forces between chlorobenzene molecules. Both of these cost energy.
The only new forces between the chlorobenzene and the water would be van der Waals dispersion forces. These aren't as strong as hydrogen bonds (or the original dispersion forces in the chlorobenzene), and so you wouldn't get much energy released when they form.
It simply isn't energetically profitable for chlorobenzene (and the others) to dissolve in water.