1. SPECTROSCOPY
SPECTROSCOPY
It is the study of interaction between matter and electromagnetic radiation.
Absorption Spectroscopy Passes the Radiation Wave
 UV-range=200-380nm
 Visible=380-780nm
 Near-IR=780-2500nm
 IR=2.5-40um
ULTRAVIOLET-VISIBLE SPECTROSCOPY
 UV-range=200-380nm
 Visible=380-780nm
It is used to measure the multiple bonds or atomic conjugation within the molecule. The
UV-Visible region is subdivided as below
 Vacuum UV: 100-200 nm
 Near UV: 200 to 400 nm
 Visible region: 400 to 750 nm
Basics of UV Light Absorption:
UV Light Absorption Ultraviolet/visible spectroscopy involves the absorption of
ultraviolet/visible light by a molecule causing the promotion of an electron from a ground
electronic state to an excited electronic state Absorption of this relatively high-energy
light causes electronic excitation. The easily accessible part of this region (wavelengths
of 200 to 800 nm) shows absorption only if conjugated pi-electron systems are present.
Electromagnetic Spectrum

2. Electronic spectroscopy
Electronic transactions involved Electronic spectroscopy Out of the six transitions outlined, only
the two lowest energy ones (left-most, colored blue) are achieved by the energies available in the
200 to 800 nm spectrum. As a rule, energetically favored electron promotion will be from the
highest occupied molecular orbital (HOMO) to the lowest unoccupied molecular orbital
(LUMO) , and the resulting species is called an excited state.
Electronic transactions involved
σ * (anti-bonding)
π * (anti-bonding)
E ή π * π * σ * σ σ *
π π * ή (non-bonding)
ή π *
σ π * π (bonding)
σ (bonding)
Types of Transitions:
Types of Transitions There are several types of electronic transitions available to a molecule
including:
 σ to σ * (alkanes)
 σ to π * (carbonyl compounds)
 π to π * (alkenes, carbonyl compounds, alkynes, Azo compounds)
 ή to σ * (oxygen, nitrogen, sulfur, and halogen compounds)
 ή to π * (carbonyl compounds)
σ σ * Transitions:
σ σ * Transitions an electron in a bonding σ orbital is excited to the corresponding antI bonding
orbital. The energy required is large. For example, alkanes as methane (which has only C-H
bonds, and can only undergo σ σ * transitions) shows an absorbance maximum at 125 nm.
Absorption maxima due to σ σ * transitions are not seen in typical UV-Visible spectra (200 - 700
nm). σ bonds are very strong and requires higher energy of vacuum UV.
ή σ * Transitions:
ή σ * Transitions Saturated compounds containing atoms with lone pairs (non-bonding electrons)
are capable of ή σ * as transitions. These transitions usually need less energy than σ σ *
transitions. They can be initiated by light whose wavelength is in the range 150 - 250 nm. The
number of organic functional groups with n σ * peaks in the UV region is small. These

3. transitions are involved in saturated compound with one hetero atom with unshared pair of
electron i.e. saturated halides, ethers, aldehide, ketones, amines etc. These transitions are
sensitive to hydrogen bonding e.g. alcohol and ethers which absorbs at wavelength shorter than
185 nm therefore used as a solvent in UV.
π π * Transitions:
π π * Transitions For molecules that possess π bonding as in alkenes, alkynes, aromatics, acyl
compounds or nitriles, energy that is available can promote electrons from a π Bonding
molecular orbital to a π Antibonding molecular orbital ( π * ). This is called a π π * transition.
The absorption peaks for these transitions fall in an experimentally convenient region of the
spectrum (200 - 700 nm). These transitions need an unsaturated group in the molecule to provide
the π electrons.
ή π * Transitions:
ή π * Transitions Even lone pairs that exist on Oxygen atoms and Nitrogen atoms may be
promoted from their non-bonding molecular orbital to a π antibonding molecular orbital within
the molecule. This is called an ή π * transition and requires less energy (longer wavelength)
compared to a ή π * transition within the same chromaphore. These are available in compounds
with unsaturated centers. e.g. Alkenes. They requires lowest energy as compare to others.
Terminology
Chromaphore:
A covalently unsaturated group responsible for electronic absorption. Or any group of atoms that
absorbs light whether or not a color is thereby produced. Eg c=c, c=o, No2 etc A compound
containing chromaphore is called chromogen. There are two types of chromaphore Independent
chromaphore: single chromaphore is sufficient to import color to the compound e.g. Azo group
Dependent chromaphore: When more than one chromaphore is required to produce color. Eg
acetone having 1 kentone group is colorless where as diacetyl having two kentone groups is
yellow
.
Auxochrome::
A saturated group with non bonding electron when attached to chromaphore alters both
wavelengths as well as intensity of absorption. Eg OH, NH2, NHR etc. OR A group which
extends the conjugation of a chromaphore by sharing of nonbonding electrons.

4. Bathochromic group: The group which deepens the colour of chromaphore is called
bathochromic group. Eg. Primary, secondary and tertiary amino groups. Bathochromic shift:
(Red shift) shift of lambda max to longer side or less energy is called bathochromic shift or read
shift. This is due to substitution or solvent effect.
Hypsochromic shift: (Blue shift) shift of lambda max to shorter side and higher energy is called
hypsochromic or blue shift. Eg solvent effect. Hyperchromic effect: an increase in absorption
intensity Hypochromic effect: A decrease in absorption intensity.

5. SOME SPECTRUMS OF ORGANIC ANALYTES

6. Instrumentation: :
Instrumentation: A beam of light from a visible and/or UV light source (colored red) is separated
into its component wavelengths by a prism or diffraction grating. Each monochromatic (single
wavelength) beam in turn is split into two equal intensity beams by a half-mirrored device. One
beam, the sample beam (colored magenta), passes through a small transparent container (cuvette)
containing a solution of the compound being studied in a transparent solvent. The other beam,
the reference (colored blue), passes through an identical cuvette containing only the solvent. The
intensities of these light beams are then measured by electronic detectors and compared. The
intensity of the reference beam, which should have suffered little or no light absorption, is
defined as I0. The intensity of the sample beam is defined as I . Over a short period of time, the
spectrometer automatically scans all the component wavelengths.

7. Solvent effect::
Solvent effect: Different compounds may have very different absorption maxima and
absorbances. Intensely absorbing compounds must be examined in dilute solution, so that
significant light energy is received by the detector, and this requires the use of completely
transparent (non-absorbing) solvents. The most commonly used solvents are water, ethanol,
hexane and cyclohexane. Solvents having double or triple bonds, or heavy atoms (e.g. S, Br & I)
are generally avoided.
Choice of Solvent:
 First criteria for good solvent are that it does not absorb uv-radiation in the same region.
As the substance whose o-absorptivity is not meaning that it does not absorb radiation.
 Eample: The solvent do not contain conjugated system H2O, ETHANOL (95%),
HEXANE,.
 Second criteria for absorption if it on fine structure on absorption band. Non-polar
solvent (not contain) do not make H-bond with the solute (organic solvent) and spectrum
of solvent is approximate to gases state (steam is puriest form), in which fine structure
often observe. In molar solvent the H-bonding forms a solute-solvent complex and fine
structure may disappear.
 It should contain polar system and conjugated form.
UV-Visible spectrum:
UV-Visible spectrum A spectrum is a plot of the intensity of energy detected versus the
wavelength (or mass or momentum or frequency, etc.) of the energy.

8. GUIDELINE TO OBSERVE UV-SPECTRUM
 In case of single band of wavelength, < 220nm usually indicate ή- σ * (amine NH3),
alcohol, ether and thiols
Exception: ή- π * (cyano group).it can identify because of its weak transition
absorbtivity 100 (ether, alcohols and amines).which is further identify by IR.
 A single band of low absorbtivity,10-100,at 250-360nm,indicate ή- π * transition
,indicate(CN,C=O,COOH,COR,N=N,C=N,NO2).
 Two bands of medium intensity, absorbtivity 1000-10.000 both with Lambda (λ) above
200nm indicates aromatic system.(polynuclear aromatic substance a 3rd band appear
near 200nm.where it cannot be observe.
 Bands of high intensity, absorbtivity, 10,000-20,000 appear above210nm.Generally
represent alpha-beta unsaturated ketones, dienes, and polyene.
 Simple ketones,acids,esters,amides and other compounds containing both π system and
unsaturated electron pairs shows two absortion.At shorter wavelenghth below 250nm.
 Compounds that are highly colored, exhibit their spectra in visible region, unlikely to
contain long chain conjugated system or polycyclic aromatic system chromaphore.
 If an organic compound does not absorb uv-visible radiation, it means that the
compounds do not contain conjugated double bonds.
 If an organic compound absorbs uv-vis radiation, it means that the compound contains a
carbonyl group or conjugated double bonds.for example, conjugated dienes, carbonyl
compounds and aromatic compounds all absorb in the uv-vis region.
APPLICATIONS
Qualitative and quantitative analysis.
SOURCE; deuterium lamp, hydrogen lamp.
VISIBLE –SPECTROSCOPY
Tungstun tamp,
IR-SPECTROSCOPY
RANGE=2.5u-40um
SOURCE=Zarconium-oxide,
Rare earth oxide
, nearst and global.
IR- radiation is weak; it does supply sufficient energy for bonds in the molecules to
vibrate by stretching or bending. The atoms of the molecules can be considered as linked
by springs that are set in motion by the application of energy. As the molecules is

9. subjected to the individual wavelength in the 5000-667cm-1 range, it absorbs only those
possessing exactly the energy required to cause a particular viberation.Energy
absorptions are recorded as bands(peaks) on chart paper.
Since different bonds and functional groups at different wavelength, an infrared
spectrum is used to determine the structure of organic molecules. For example, carbon-
carbon triple-bond is stronger than a carbon-carbon double bond and requires a shorter
wavelength (greater energy) to stretch).The same consideration apply to carbon-oxygen
and carbon-nitrogen bonds.
An infrared spectrum studied in two section
 Functional group region
 Fingerprint region
Functional group region
The area from 5000cm-1-1300cm-1 is called the functional group region. The bands
in this region are particularly useful in determining the type of functional groups
percentage in the molecule.
Finger print region

10. The area from 1300cm-1 to 667cm-1 is called the fingerprint region. A peak by
peak match of unknown spectrum with the spectrum of the suspected compound in this
region can be used, much like a fingerprint to confirm its identity.
EXAMPLES
METHANOL

11. BUTANONE
ISOBUTYLAMINE

12. INSTRUMENTATION
The instrument that determines the absorption IR spectrum of a compound is called IR
spectrophotometer.
TYPES: there are two types.
 Dispersive –IR spectrometer

13.  Fourier transform Ir spectrometer
Both of these instrument travel spectra of compound in the common range of
4000-400cm-1.
The spectra of both instruments are nearly identical, while FTIR-spectra provide
IR-spectra more rapidly than the dispersive instrument.
DIR-spectrometer : the instrument produce a beam of IR radiation from a hot
wire (IR source).The beam of by means of mirror divided into two parallel beam
of equal intensity radiation,
 Beam sample analysis
 Reference
 Both beams can pass through monochromatic, which disperse
each into continuous spectrum of frequencies or IR-light by beam
chopper. Which is a rotating chamber that passes the two beams
alternately through a diffracting gratting serve as prism which
varies of frequency or range?
 The thermo-couple detector senses the ratio between the sample
and the reference that what beam has bean absorbed by the
sample and which uneffective.
 After the singnal from the detector is amplifies the recorder cause
the resulting specterum of sample on chart.
 The IR-chart is recorded as a frequency of the IR-radiation
charges by the rotation of the diffraction gratting.
 Disperive spectrum is recorded in frequency domain, It is
common to plot frequency is live transmission.This is recorded as
percentage transmitter from detector from record the ratio of
intensity of two beam therefore.
%T=is/ir x100
Is=sample beam intensity
Ir=intensity of reference
SAMPLE PREPARATION
To obtain the IR-spectrum compound is dissolved in a solvent or diluents .This solution is then
will replace in sample beam by pure solvent beam in a identical beam.
The instrument automatically subtracts the spectrum of solvent from that of sample. The
instrument also cancel the effect of IR spectrum NO2, CO2.If pure liquid is analyzed the sample
is varyingly in a sample beam and nothing is inserted in a reference beam.
When the spectrum of liquid is obtain. The effects of atmospheric gas automatically cancel, since
they are present in both beams.
FTIR-SPECTROSCOPY
The most common IR-spectrometer are design to consist of optical pathway, produce a pattern
called interferofram,(broader instrument optical pathway)There is optical pathway to analyses

14. IR interferogram .The interferogram is a complex signal but it’s waves like pattern contain all
frequency that make up the IR-spectrum.
Interferogram is plot of intensity vs. time, called time domain spectrum.
FTIR-SPECTRUM
In chemical analysis, frequency domain spectrum is preferred over time domain spectrum is a
plot of intensity vs. frequency vs. time.
OPEARTION OR WORKING OF FTIR
Computer interferogram FTIR instrument operate in a single mode to obtain spectrum .first
interferogram of the background being recorded by example (co2).This background
interferogram subjected to Fourier transformer which yield a spectrum of background., then
sample i9s placed into the beam spectrum is obtain resulting from Fourier transform of
interferogram .The spectra contain absorption of sample and background and now where
automatical subtract spectrum of background from the sample which identical to dispersive
spectrum.
PREPARATION OF SAMPLE
To determine the IR-spectrum of compound sample is placed in holder or cell as must be
constructed from ionic substance (NACL), KBr.
Glass or plastic absorb Irradiation, so it should be not.
KBr plates are expensive then NACL, and useful in the range of 4000-400cm-1.
NACL is useful in the range 4000-659cm-1 and band with frequency less than this value will not
be observe ,since only a few band appear bellow 650cm-1.NACL.
LIQUID
A drop of liquid is placed between a pair of polished and NACL and KBR plot refer to as salt
plates, where plots are squeeze gently a this liquid film are formed between them. Spectrum of
obtain is know next spectrum since solvent.
Salt plates are water soluble, so analyzing compound must be free from water; the pair of plate is
inserted, into a holder, which fixed into a spectrometer.
SOLIDS
There are three common methods to grounded sample mix with powder KBr melts and seal the
compound into a matrix results in FTIR plot or disc should be transport, which can be inserted
into holder in IR-spectrometer.
ADVANTAGE: In case of wood plates for disc the spectrum have no interfering band, since
KBr transport down to 4000cm-1.
DISADVATNTAGE: KBr through absorb water which may interfere with the spectrum.
SECOND METHOD
NUJOL MULL METHOD

15. This method is involve straining the compound with mineral oil,nojol to create a suspension off
finely ground sample in mineral oil dispersed in mineral oil. The thick suspension MULL place
between the salt plates then it analyses in the spectrometer.
Disadvantage: Mineral oil obscure band over shallow band that may be present in the analyzing
compound.
THIRD METHOD
DISSLOUTION IN ORGANIC SOLVENT
It may be used with solid which dissolve in organic solvent, must commonly CCL4.In case of
mineral oil some region of spectrum are it also bind with solvent. It is also observed in organic
solvent (especially at 785cm-1).
Although it is possible to cancel out the solvent from the spectrum of sample by computer.
C. NUCLEAR MAGNETIC RESONANCE (NMR) SPECTROSCOPY
 Nuclear magnetic resonance spectroscopy involves absorption of electromagnetic
radiation in the radio frequency region. Absorption of radio waves in the presence of
magnetic field is accompanied by a special type of nuclear transition, and for this reason
we call this type of spectroscopy nuclear magnetic resonance (NMR) spectroscopy.
 The nuclei of certain atoms behave as if they are spinning chages.Any spinning charge
creates a magnetic field and behaves as if it were a tiny bar magnet, Of the three most
common in organic compound, only the hydrogen nucleus proton behaves in this manner.
 When a proton in an organic molecule is placed in a strong magnetic field, it can align
with the field or against it.
 In the more stable low-energy state, it is aligned with the magnetic field. (Up field).that
appears toward left on chart paper...
 If energy is supplied in the form of radio waves of exactly the right frequency, radiation
will be absorbed and the nucleus will flip and align against the applied magnetic field in
the less stable higher energy state(downfield) .that appear right on chart paper.

16. 4. The chemical shift and shielding (POSITION OF SIGNALS)
 Chemical Shift (Position of Signals) The utility of NMR is that all protons do not show
resonance at same frequency because, it is surrounded by particular no. of valence
electrons which vary from atom to atom so, they exist in slightly different electronic
environment from one another.
 Position of signals in spectrum help us to know nature of protons i.e. aromatic, aliphatic,
acetylinic, vinylic, adjacent to electron releasing or withdrawing group.
 . When the sample absorb the energy ,however reorientation of the nucleus spin induces a
RF signal in the plane of the detector coil, and the instrument respond by recording this
as a resonance signal or peak. As the field is increases linearly, the pen travel across the
recording chart, AQ pen travel left to right.
 A magnetic field is increases. Highly shield protons appear right of this chart, (UP
FIELD). And deshielded appear to the left. (DOWN FIELD) This is continuous
spectrum instrument because in which magnetic field in the continuous fashion up field
and downfield.

17. Spin-Spin Splitting in NMR Spectrum
Peaks are often split into multiple peaks due to magnetic interactions between nonequivalent
protons on adjacent carbons; the process is called Spin-spin Splitting/Coupling.
I. Spin-spin splitting: It occurs only between nonequivalent protons on the same carbon or
adjacent carbons.
II. Peak: The units into which an NMR signal is split; doublet, triplet, quartet, multiplet, etc.
III. Signal splitting: Splitting of an NMR signal into a set of peaks by the influence of
neighboring nonequivalent hydrogens.
IV. Signal coupling: An interaction in which the nuclear spins of adjacent atoms influence
each other and lead to the splitting of NMR signals.
Equivalent Protons
 These equivalent protons do not split each other.

18.  Protons bonded to the same carbon will split each other only if they are not equivalent.
Equivalent protons have the same chemical shift.
 Equivalent protons have same chemical shift without splitting occurs.
Non-equivalent Protons

19.  If Ha and Hb are not equivalent, the splitting is observed.
 Nonequivalent protons on adjacent carbons have magnetic fields that may align with or
oppose the external field.
 This magnetic coupling causes the proton to absorb slightly downfield when the external
field is reinforced and slightly up field when the external field is opposed.
 All possibilities exist, so signal is split.
 Non equivalent protons have different chemical shift with splitting occurs
 Bonds. 43Splitting is not generally observed between protons separated by more than
three bonds.
Non equivalent protons have different chemical shift with splitting occur.
Splitting is not observed between protons separated by more than three σ – bonds .

20. 5. INSTRUMENTATION
CONTINOUSE-WAVE SPECTROMETER.
1. It is the basic elements of a classical 60-MHz NMR spectrometer. The sample is
dissolved in a solvent containing no interfering protons (usually CCl4, CDCl3), and a
small amount of TMS is added to serve as an internal reference.
2. The sample cell is in small is a small cylindrical glass tube that suspended in the gap
between the faces of the pole pieces of the magnet, The sample is spin around its axis to
ensure that all parts of the solution experience a relatively uniform magnetic field.
3. Also in the magnet gap is a coil attached to 60-MHz radiofrequency generator .This coil
supplies the electromagnetic energy used to change the spin orientation of the proton
.perpendicular to the RF oscillator coil is detector coil, When no absorption of energy is
take place ,the detector coil pick up non of the energy given off by the RF oscillatory coil
,
4. When the sample absorb the energy ,however reorientation of the nucleus spin induces a
RF signal in the plane of the detector coil, and the instrument respond by recording this
as a resonance signal or peak. As the field is increases linearly, the pen travel across the
recording chart,AQ pen travel left to right .
5. A magnetic field is increases. Highly shield protons appear right of this chart,(UP
FIELD). And deshielded appear to the left.(DOWN FIELD) This is continuous
spectrum instrument because in which magnetic field in the continuous fashion up field
and downfield.
6. The peak is calculated from frequency difference from TMS, It’s called frequency
domain spectrum. When peak is generating it ring with Cw spectrum...
7. CW-type of NMR spectrometer is use that excite the the nuclei of the isotope under
observation one type at a time. And H1 nuclei type of proton (phenyl, vinyl, methyl,) is
excited individually and is resonance peak is observed and recorded independently. They
excite one time individually, all other are not observed until all of the type have come
into resonance.
PULSE FOURIER TRANSFORM (FT) INSTRUMENT
 FT-transform NMR instrument is modern type of instrument that excite the
magnetic nuclei simultaneously,
 E.g. isotope of the hydrogen nuclei resonance at the same time.
 The magnetic field uses a short (1-10micro-sec) 90MHz).This high power
burst is called pulse.

21.  When this discontinue the nuclei start to relax.
 Then these nuclei emitted electromagnetic radiation, it is called free induced
decay (FID). It is time domain frequency instrument.
SPECTRAL ANALYSIS
ALKANE

22. ALKENE

23. C13 NMR SPECTRUM
SPECTROMETRY

24. Use of spectroscopy as quantities tool.
MASS SPECTROSCOPY
The mass spectrum of a compound helps to establish the structure of a new compound
in several different ways:
1) It can give the exact molecular mass. by ionizing it and analyzing its mass using a
magnetic field.
2) It can give a molecular formula or it can reveal the presence of certain structural
units in a molecule.
TERMINOLGIES
M= Molecular ion, the ion that spectrometer analyze. This is the molecule comprised
of lowest +, - atomic mass isotopes.
M/Z=Mass to charge ratio of an analyte ion .if we are asked to find the m/Z ratio for
butane, what would we do?
BUTANE
M/Z (4x12)+(10x1)=58 lowest mass isotopes of carbon.
Sometime a molecule distegrated during the process forming a fragment ion.
Since we desined (M) as the molecules with lowest mass atomic isotopes, we can
identify fragment easily.
By studying many mass spectra we learn that this ratio can be used to determine the
carbon count of analyte.
Exampe: if the relative abundance of the m+1 peak is 5.3% compared to M peak,
how many carbons are in the molecule?
RA=5.3%/1.1=4.8 (5 carbon are in the analyte
molecule),
M+2 RULE

25. NITRGEN RULE
When m/z is M is even number in formula.
When m/z Is M is odd number in formula.
HYDROGEN RULE
For a molecule with “C” and “N” the max number of monovalent atom (hydrogen +
halogen) in the formula.
2C+N+2
DBE= double bond equivalent=C-H/2+N/2+1
INTERPRETATION OF MASS SPECTRUM
SULFUR CHLORINE BROMINE
ISOTOPES 32S, 34S 35C, 37C 79Br, 81Br
RELATIVE
ABUNDANCE
95%,4.2% 75.8%,24.2% 50.7%,49.3%
M/M+2 40:04.4 100,:31.9 100:9>2

26. 79Br=50.695
81Br=49.31%
ELEMENTS AND THEIR ISOTOPES WITH THEIR RELATIVE ABUDANCE
ELEMENT M M+1 M+2 M+4

27. C
12C
(98.89%)
13C
(1.11%)
N
14N
(99.64%)
15N
(0.01%)
O
16O
(99.76%)
17O
(0.04%) 18O (0.20%)
S 32S (95.0%)
32S
(0.76%) 34S (4.22%)
36S
(0.0S%)
F
19F
(100.0%)
CL 35(75.77%)
37CL
(23.23%)
BR
79Br
(50.69%)
81BR
(49.31%)
MS INSTRUMENTATION
Each kind of ion has a particular ratio of mass to charge, i.e. m/e ratio(value). For
most ions, the charge is one and thus, m/e ratio is simply the molecular mass of the
ion.
SAMPLE VAPORIZATION
The basic aspect of organic mass spectrometry consist of bombarding the vapour of
an organic compound with a beam of energetic electron accelerated from a filament
to an energy of 70 eV to form positively charged ions (molecular ions).The heating
coil is is steam the sample and vaporize it.
IONIZATION
The molecules are ionised and broken up into many fragments, some of which are
positive ions. In this technique, molecules are bombarded with a beam of energetic
electrons.
There is electrode are place, that are positive, negative and double negative charged.
Same charge repel to each other where different charge attract to each other. In this
way regulate the movement of ions.
Mass spectroscopy deals with the examination of the characteristics fragments (ions)
arising from the breakdown of organic molecules.
The deflection of ions, however, depends on its mass, charge and velocity. 8The
various positive ions, thus formed, can be accelerated and deflected by magnetic or
electric fields. This fragmentation may result in the formation of an even- electron
ion and radical.

28. DEFLACTION
The deflection is less for a heavy particle as compared to that of a light one. -The
more the ion is charged, the more it gets deflected.
Though organic mass spectrometry is routinely used along with IR, NMR and UV for
structure determination, its basic theory is different from the others.
DETECTION OF IONS
When an ion hits the metal box, its charge is neutralized by an electron jumping from
the metal on to the ionhe beam of ions passing through the machine is detected
electrically. Only ion stream B makes it right through the machine to the ion detector.
The other ions collide with the walls where they will pick up electrons and be
neutralized. They get removed from the mass spectrometer by the vacuum pump.
APMLIFIER
A flow of electrons in the wire is detected as an electric current which can be
amplified and recorded. The more ions arriving, the greater the current.
SPECTRUM
A mass spectrum is the plot of relative abundance of ions against their mass/charge
ratio. 
MS- INSTRUMENTATION