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Mass Spectrometry

  • Schedule : 7 minutes
  • Who is this for: Graduates, Lab technicians

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Duration: Self Paced
Schedule: 7 minutes
Level: Intermediate

Course Overview

Know about Magnetic Sector Instrument
Working Principle
Samples
High-Resolution Spectrum

 

Transcript
 

Mass spectrometry allows chemists to weigh atoms and molecules, not directly on a balance, but by measuring how ions formed from them are accelerated and deflected by electric and sometimes magnetic fields. 

There are many types of mass spectrometer,

but they all work on this basic principle. This instrument is called a magnetic sector

instrument. The sample is introduced here and the positive

ions are formed here by bombardment of the sample with a beam of electrons.

The ions are then accelerated by an electric field and then deflected in a curve by a further

electric field. They then bend through a magnetic field and

are further deflected by another electric field here.

The ions then enter a detector here. By varying the electric and magnetic fields,

ions of different mass can be made to enter the detector.

These pumps keep the interior of the instrument under a high vacuum.

This is to allow the ions which are moving at speeds of many kilometres per second a

free path without collisions with air molecules.

As the ions are formed from molecules of the sample, they may fall apart or fragment.

The ion of largest mass is often the parent

or molecular ion, an ionised molecule that has not fragmented.

Other peaks of smaller mass may represent charged fragments of this ion.

The masses of these fragments may give clues as to the structure of the original molecule.

Liquid samples are placed in the tiny sample tube, as shown.

Here, we're running the mass spectrum of limonene, an alkene which can be obtained from the peel

of citrus fruits. Only a little is required.

Mass spectrometry can detect down to as few as 10 to the minus 12 moles.

Volatile samples can be run neat; less volatile ones are dissolved in a solvent

such as dichloromethane, which then evaporates.

The sample tube is placed in this probe, which

is then inserted into the instrument via an airlock so that the vacuum in the instrument is maintained.

Volatile samples will vaporise at the low

pressure inside the instrument but the probe can be heated to vaporise less volatile ones.

The electrons stream out from a heated cathode towards an anode which is held at a potential

of around +70 volts relative to the cathode.

This is the ionisation chamber where the positive ions are formed.

These are formed when high energy electrons strike the sample molecules.

You can think of this as the electron beam

knocking out an electron from the sample molecule.

The sample fits here and ions pass out through this slit.

The heater itself is here. The electrons are accelerating in this direction

and the ions stream in this direction through the slit.

The positive ion beam passes between two charged curved plates which deflect it in a curve

so it enters the area here where an electromagnet produces a vertical magnetic field.

This further deflects the beam in an arc of a circle. On emerging from the magnetic field

the beam is deflected again by another set of charged plates which direct it into the detector.

The amount of deflection by the magnetic field

depends on the mass of the ion. Strictly, it's mass to charge ratio, but the

vast majority of ions have only a single charge. The deflection also depends on the strength

of the field. Heavier ions will not be deflected sufficiently

in the magnetic field to reach the detector. Lighter ions will be deflected too much.

During a run, the magnetic field is gradually increased so that ions of successively greater

mass enter the detector. The mass spectrum of limonine looks like this.

Each vertical line, called a peak, represents a different ion and its mass, in relative

atomic mass units, is shown on the horizontal axis.

The height of a peak represents the abundance that ion.

The peak at 136 units represents the parent ion, the whole molecule that has lost an electron.

The peak at mass 121 units (136-15) is the parent ion from which one of the CH3 groups,

relative molecular mass 15, has broken off in the ionisation chamber.

The peak at mass 107 (121-14) could be formed by further loss of a CH2 group.

Other peaks are caused by more complex breakdowns and rearrangements.

Simple mass spectra show the masses of ions to the nearest whole number which is fine

for many purposes. However, this instrument can display masses to three decimal places

of an atomic mass unit. This is called a high resolution spectrum.

It enables us to distinguish between different molecular formulae which have the same relative

molecular mass to the nearest whole number.

Here, we see that the relative molecular mass

of limonine is 136.125. This means that we can distinguish C10H16 from say C9H12O which would

have a relative molecular mass of 136.194 to three decimal places.

Many mass spectrometers are of desktop size. This one takes in samples from a gas chromatography

instrument. As each component comes off the gas chromatography

column it is fed directly into the mass spectrometer.

The combined technique is called gas chromatography mass spectrometry or GCMS. This is the column from the gas chromatograph.

This particular mass spectrometer does not use magnetic deflection of the ions, it uses

a complex electric field. However, the principle of forming ions from

the sample and separating them according to mass underlies all types of mass spectrometer.

This is the gas chromatogram of an impure extract of orange zest. The large peak is

limonine and the others represent impurities.

Clicking on the peak shows the mass spectrum of limonine.