Contact FutureLearn for Support
Skip main navigation
We use cookies to give you a better experience, if that’s ok you can close this message and carry on browsing. For more info read our cookies policy.
We use cookies to give you a better experience. Carry on browsing if you're happy with this, or read our cookies policy for more information.
Blue and Yellow 3-D hexagons

3-dimensional structures of fragrance molecules

Let's look at a more complicated example, (‐)‐citronellol, which has a fresh, floral and clean rose smell and is used in perfumes and insect repellents. From the skeletal structure we can see that (‐)‐citronellol contains both alkene and primary alcohol functional groups. All the carbon atoms have a tetrahedral shape apart from the two carbon atoms in the carbon‐carbon double bond, which, like an aldehyde, are trigonal planar, or flat.


It is also interesting to look at the methyl group bonded to the tetrahedral carbon at position 3 of the carbon chain. You will see it is pointing towards us. The carbon atom at position 3 is distinctive because it is the only carbon bonded to four different groups – we call this an asymmetric or chiral centre.

Interestingly, there are two possible ways of arranging the four different groups at a chiral centre.

In (‐)‐citronellol, we have seen that the methyl group at position 3 points towards us, and the hydrogen points away from us. If these groups are arranged differently, and the –CH3 is pointing away from us, the molecules are non‐identical structures with different shapes – indeed, when the methyl group is pointing away from us, we call it (+)-citronellol.

The use of (+) and (‐) indicates that they rotate a special form of light, called plane‐polarized light, in different directions. Often R or S, in brackets, is also included at the start of a name to indicate how the groups are arranged around a chiral centre – assignment of R or S is taught in our first year degree course.


If you spin around (R)‐(+)‐citronellol and compare this to (S)‐(‐)‐citronellol you will see that they are non‐identical mirror images – the mirror images cannot be arranged in space so that all of the atoms in both structures overlap – we say they are non‐superimposable and we call them enantiomers.


This can be tricky to visualise, so, to help, let's think of our hands. Hands are chiral – a left hand is a mirror image of a right hand. Left and right hands are not superimposable – when placed side by side the fingers and thumbs point in opposite directions. This is just the same for (S)‐(‐)‐citronellol and (R)‐(+)‐citronellol, where the methyl groups point in opposite directions.


As enantiomers have different shapes they can have different biological properties – for example, the two different enantiomers of citronellol have different smells. So, is very important to draw the structure of an enantiomer correctly.

If you would like some further information on enantiomers you may find this YouTube clip of use.

Why is R/S preferable to (+)/(-)?

Imagine I drew a single enantiomer of citronellol and asked you to assign which enantiomer it is. Unless you memorised whether it was (+) or (-) how could you work it out? The difficulty is (without using a polarimeter to measure the angle of rotation of plane polarised light) you cannot. What you need is a naming system that allows you to workout what enantiomer it is just by looking at the structure, and also, be able to draw the correct structure of the enantiomer simply from its name. This is what the R and S system (sometimes called CIP nomenclature) allows. This system ranks the four atoms or groups bonded to a chiral carbon atom - from this, you can assign the enantiomer as R or S. The R and S system is not related to the (+) or (-) sign of the optical rotation. For example, let’s look at two amino acids, serine and tyrosine. Whereas (S)-serine has a positive optical rotation, (S)-tyrosine has a negative value.

Don't worry if you don't feel completely comfortable with all the terminology in this step, which is a challenging one. You can check out our pictorial glossary to help familiarise yourself with the concepts and for new examples that might make everything a bit clearer

Share this article:

This article is from the free online course:

Exploring Everyday Chemistry

University of York