INTRODUCING NITRILES   This page explains what nitriles are and looks at their simple physical properties such as solubility and boiling points. What are nitriles? Nitriles contain the -CN group, and used to be known as cyanides. Some simple nitriles The smallest organic nitrile is ethanenitrile, CH3CN, (old name: methyl cyanide or acetonitrile - and sometimes now called ethanonitrile). Hydrogen cyanide, HCN, doesn't usually count as organic, even though it contains a carbon atom. Notice the triple bond between the carbon and nitrogen in the -CN group. The three simplest nitriles are: CH3CN ethanenitrile CH3CH2CN propanenitrile CH3CH2CH2CN butanenitrile When you are counting the length of the carbon chain, don't forget the carbon in the -CN group. If the chain is branched, this carbon usually counts as the number 1 carbon.
	Note:  Compounds like this are formed when aldehydes react with hydrogen cyanide. This is therefore the sort of branched nitrile that you are most likely to come across at this level.
Physical properties Boiling points The small nitriles are liquids at room temperature. nitrile boiling point (°C) CH3CN 82 CH3CH2CN 97 CH3CH2CH2CN 116 - 118
	Note:  The majority of the data sheets I have looked at quote this boiling range for butanenitrile. I don't know why it doesn't seem to have a precise boiling point.
These boiling points are very high for the size of the molecules - similar to what you would expect if they were capable of forming hydrogen bonds. However, they don't form hydrogen bonds - they don't have a hydrogen atom directly attached to an electronegative element. They are just very polar molecules. The nitrogen is very electronegative and the electrons in the triple bond are very easily pulled towards the nitrogen end of the bond. Nitriles therefore have strong permanent dipole-dipole attractions as well as van der Waals dispersion forces between their molecules.
Solubility in water Ethanenitrile is completely soluble in water, and the solubility then falls as chain length increases. nitrile solubility at 20°C CH3CN miscible CH3CH2CN 10 g per 100 cm3 of water CH3CH2CH2CN 3 g per 100 cm3 of water The reason for the solubility is that although nitriles can't hydrogen bond with themselves, they can hydrogen bond with water molecules. One of the slightly positive hydrogen atoms in a water molecule is attracted to the lone pair on the nitrogen atom in a nitrile and a hydrogen bond is formed. There will also, of course, be dispersion forces and dipole-dipole attractions between the nitrile and water molecules. Forming these attractions releases energy. This helps to supply the energy needed to separate water molecule from water molecule and nitrile molecule from nitrile molecule before they can mix together. As chain lengths increase, the hydrocarbon parts of the nitrile molecules start to get in the way. By forcing themselves between water molecules, they break the relatively strong hydrogen bonds between water molecules without replacing them by anything as good. This makes the process energetically less profitable, and so solubility decreases. MECHANISM OF THE ACID catalyzed HYDROLYSIS OF NITRILES Step 1: An acid/base reaction. Since we only have a weak nucleophile so activate the nitrile, protonation makes it more electrophilic. Step 2: The water O functions as the nucleophile attacking the electrophilic C in the CºN, with the electrons moving towards the positive center.  Step 3: An acid/base reaction. Deprotonate the oxygen that came from the water molecule. The remaining task is a tautomerization at N and O centers. Step 4: An acid/base reaction. Protonate the N gives us the -NH2 we need....  Step 5: Use the electrons of an adjacent O to neutralise the positive at the N and form the p bond in the C=O.  Step 6: An acid/base reaction. Deprotonation of the oxonium ion reveals the carbonyl in the amide intermediate....halfway to the acid.....  What about the rest ?