What is the difference between cyclohexane and benzene

The aromatic state

Comparison of benzene and cyclohexatriene

You know alkanes and cycloalkanes from chemistry class EF. Cyclohexane is a well-known representative of the cycloalkanes: six carbon atoms have joined together to form a ring, and each carbon atom has two hydrogen atoms. If we remove two H atoms from two neighboring C atoms, we get the cyclohexene. This connection is also known from the EF level. Mostly the chemistry teacher uses them to demonstrate that alkenes decolorize bromine water. Or as an introductory experiment in electrophilic addition in stage Q1.

If we remove two more H atoms, we get a six-membered ring with two C = C double bonds, the cyclohexadiene. This connection is no longer so common in schools.

Now you might think: Okay, if we remove two more H atoms, then we get the compound cyclohexatriene with three C = C double bonds. Wait a minute, isn't that the same thing as benzene?

In fact, no chemist has ever succeeded in producing cyclohexatriene!

Now you definitely say: What's that supposed to mean? Cyclohexatriene is the same as benzene!

Unfortunately, this statement is not entirely true.

Chemical properties

Let us now compare the chemical properties of benzene and the cyclohexatriene, which no one has yet been able to produce.

Cyclohexene, a cycloalkene made up of six carbon atoms and one C = C double bond, decolorizes bromine water, so it goes through an electrophilic addition with Br2 a. The electrophilic addition is typical of the C = C double bond. Cyclohexadiene, i.e. the cycloalkene with six carbon atoms and two C = C double bonds, also undergoes electrophilic addition.

One would think that cyclohexatriene with a third double bond reacts even better with bromine than cyclohexene or cyclohexadiene.

If you add bromine water to benzene, nothing at all happens at first. No trace of discoloration, absolutely no tendency towards electrophilic addition!

If benzene had "correct" C = C double bonds, it would have to react immediately with bromine water. The compelling conclusion: The C = C double bonds in the benzene molecule are not real C = C double bonds at all. On the benzene side, we had already noticed a peculiarity: the six bonds in the benzene molecule are all of the same length. Obviously there are neither “correct” C-C single bonds nor “correct” C = C double bonds in the benzene molecule.

Enthalpy of hydrogenation

When cyclohexene is allowed to react with hydrogen, cyclohexane, the addition product, is formed. This exothermic reaction releases 119.7 kJ / mol of energy, the enthalpy of hydrogenation. If you carry out the same reaction with cyclohexadiene, you get 232.0 kJ / mol of hydrogenation enthalpy, which is about twice the value of cyclohexene.

It is now reasonable to assume that the hydrogenation of cyclohexatriene would result in three times as much as 120 kJ / mol, i.e. approximately 340 to 360 kJ / mol.

However, when benzene is hydrogenated, only a hydrogenation enthalpy of 208.5 kJ / mol is obtained.[2] That is considerably less than one would have expected for the cyclohexatriene, approx. 151 kJ / mol less even.

Here is one of the usual graphical representations found in almost every good school book; I drew the picture myself, of course:

Obviously, benzene is "energetically more favorable" than cyclohexatriene and therefore more stable. This then explains why benzene is not as reactive as cyclohexatriene.

The energy difference of -151 kJ / mol, which is shown in red in the graph, even has its own name: resonance energy or mesomeric energy.

Let's summarize our findings that we have made so far:

The benzene molecule is formally structured like a cyclohexatriene molecule. However, all bonds in the benzene molecule are of the same length, there are neither C-C single nor C = C double bonds. Benzene also does not undergo electrophilic addition, and it is much lower in energy and therefore more stable than a hypothetical cyclohexatriene molecule, as the hydrogenation experiments show.

Most important finding: All C-C bonds in the benzene molecule are equivalent, there are neither single nor double bonds, and they are very stable.

KEKULÉ's oscillation hypothesis:

Chemists like KEKULÉ were already thinking about the molecular structure of benzene in the 19th century and asked themselves what is special about the benzene molecule. KEKULÉ carried out a lot of chemical experiments with benzene, which led him to the conclusion that all C-C bonds in the benzene molecule are equivalent. KEKULÉ finally put forward a groundbreaking hypothesis that tried to explain this equivalence of ties

Oscillation hypothesis: The C = C double bonds in the benzene molecule "flip" several thousand times per second. For a short time each C-C bond is a single bond, then a double bond again.

We make this bold hypothesis clear by means of an illustration:

According to the oscillation hypothesis of 1872, this is exactly how the benzene structure was imagined. Accordingly, the double bonds "fold" several hundred or even 1000 times per second. A fascinating explanation that most people immediately understood.

Unfortunately this hypothesis is wrong. The double bonds do not fold over, but - as we know today - every C-C bond in the benzene molecule is actually half a single bond and half a double bond. You can find out more on the encyclopedia page on mesomerism, which was updated at the end of 2019.

Of course, mesomerism cannot be explained with the spherical cloud model commonly used in schools. It's time we got used to a more powerful atomic model.

You do not have to master the entire orbital model, it is enough if you know the different hybridization states of the C atom.

  • If you are not yet familiar with the orbital model, please go to the index page for the orbital model.
  • If you want to find out more about hybridization in general, you can go to the hybridization page.
  • If you want to find out more about the C atom in the orbital model, you can go straight to the page "The C atom in the orbital model". Alternatively, you can download and work through the worksheet "Models of the C atom", on which everything is explained in a way that is suitable for students (I hope at least).
For experts:

The aromatic state of the benzene molecule

All six carbon atoms in benzene are sp2-hybridized, and the six pz-Orbitals are aligned parallel so that they can (slightly) overlap. This creates a common ring-shaped molecular orbital in which the six pi electrons can move freely, both above and below the plane of the ring.

But I have done all this better on my fifth page about the orbital model, "The Benzene Molecule", which you should definitely take a look at now.

Not only benzene belongs to the aromatics, also all compounds that are derived directly from benzene, for example phenol, nitrobenzene or aniline. But many other organic compounds that are not at all similar to benzene are aromatic. The chemist Erich Hückel (1896-1980) determined in 1930 exactly when a compound belongs to the aromatic group. See the next page "The Hückel Rule".