In electron impact (EI) mass spectrometry the molecule is bombarded with highly energetic electrons that knock a weakly bound electron out of the molecule. If you think this is strange, think of throwing bricks at a brick wall: the bricks can’t stick to the wall but can knock loose bricks off the top of the wall. Losing a single electron leaves behind an unpaired electron and a positive charge. The electron that is lost will be one of relatively high energy (the bricks come from the top of the wall), and typically one not involved in bonding, for example an electron from a lone pair.

Thus, ammonia gives NH3 + • and a ketone gives R2C O+ •. These unstable species are known as radical cations, and being charged they are accelerated by an electric fi eld and focused onto the detector, which detects the mass of the ion by how far its path has been deflected by the electric field. It only takes about 20 μs for the radical cations to reach the detector, but sometimes they fragment before they get there, in which case other ions will also be detected. These fragments will always have a lower mass than the ‘parent’ molecular ion, so in a typical mass spectrum we are most interested in the heaviest ion we can see. A typical EI mass spectrum looks like this:

This compound was identifi ed as a pheromone deposited by worker bees when feeding as a marker to deter their colleagues from visiting the same, now depleted, nectar source. Only minute quantities are available for analysis of course, but that doesn’t matter: mass spectrometry is successful even on a microgram scale. The spectrum you see here indicates that the molecule has a mass of 114 because that is the highest mass observed in the spectrum: the molecule is in fact the volatile ketone heptan-2-one.

مواضيع ذات صلة

Chemical reactions

Rotation and rigidity

The carbonyl group

We can hybridize any atoms

Hybridization of atomic orbitals

Molecular orbitals of molecules with more than two atoms

Other factors affecting degree of orbital interaction

Bonds between different atoms

Forming bonds using 2s and 2p atomic orbitals: σ and π orbitals

Bond order

Why hydrogen is diatomic but helium is not

Breaking bonds