UV - VISIBLE SPECTROSCOPY

13-11-2019 Google, Wikipedia
By
Akram khan

What is Spectroscopy ?
 It is the branch of science that deals with the study of interaction of
matter with light or Electromagnetic radiation.
 Optical spectroscopy is based on the interaction of light with matter.
The following figure illustrates what is happening when light is
shining onto an object:
2/3713-11-2019 Google, Wikipedia

Electromagnetic Radiation
 Electromagnetic radiation consist of discrete packets of energy which
are called as photons.
 A photon consists of an oscillating electric field (E) & an oscillating
magnetic field (M) which are perpendicular to each other.

Frequency (ν):
 It is defined as the number of times electrical field radiation oscillates
in one second.
 The unit for frequency is Hertz (Hz).
1 Hz = 1 cycle per second
Wavelength (λ):
 It is the distance between two nearest parts of the wave in the same
phase i.e. distance between two nearest crest or troughs.
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 The relationship between wavelength & frequency can be written
as:
c = ν λ
 As photon is subjected to energy
so
E = h ν
= h c / λ

Interaction of EMR with matter
1) Electronic Energy Levels:
 At room temperature the molecules are in the lowest energy levels
E0 .
∆E = h ν = En - E0 where (n = 1, 2, 3, … etc)
2( Vibrational Energy Levels:
3( Rotational Energy Levels:
 The spacing between energy levels are relatively small i.e. 0.01 to 10
kcal/mole.
 The spacing between energy levels are even smaller than vibrational
energy levels.
∆Erotational < ∆Evibrational < ∆Eelectronic
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A=absorbance
ε =molar absorbtivity with units of L /mol.cm
b=path length of the sample (cuvette)
c =Concentration of the compound in solution, expressed in mol /L
A = ε b c
Beer Lamberts Law:

 The UV radiation region extends from 10 nm to 400 nm and the
visible radiation region extends from 400 nm to 800 nm.
Near UV Region: 200 nm to 400 nm
Far UV Region: below 200 nm
 Far UV spectroscopy is studied under vacuum condition.

The possible electronic transitions can graphically shown as:

• σ → σ* transition
• π → π* transition
• n → σ* transition
• n → π* transition
• σ → π* transition
• π → σ* transition
1
2
3
4
5
6
The possible electronic transitions are

• σ → σ* transition1
• σ electron from orbital is excited to corresponding anti-
bonding orbital σ*.
• The energy required is large for transition.
• e.g. Methane (CH4) has C-H bond only and can
undergo σ → σ* transition and shows absorbance
maxima at 125 nm.

• π → π* transition2
• π electron in a bonding orbital is excited to
corresponding anti-bonding orbital π*.
• Compounds containing multiple bonds like
alkenes, alkynes, carbonyl, nitriles, aromatic
compounds, etc undergo π → π* transitions.
• e.g. Alkenes generally absorb in the region
170 to 205 nm.

• n → σ* transition3
• Saturated compounds containing atoms with
lone pair of electrons like O, N, S and
halogens are capable of n → σ* transition.
• These transitions usually requires less energy
than σ → σ* transitions.
• The number of organic functional groups
with n → σ* peaks in UV region is small (150
– 250 nm). 15/3713-11-2019 Google, Wikipedia

• n → π* transition4
• An electron from non-bonding orbital is
promoted to anti-bonding π* orbital.
• Compounds containing double bond
involving hetero atoms (C=O, C≡N, N=O)
undergo such transitions.
• n → π* transitions require minimum energy
and show absorption at longer wavelength
around 300 nm. 16/3713-11-2019 Google, Wikipedia

5
6
• σ → π* transition
• π → σ* transition
&
• These electronic transitions are forbidden
transitions & are only theoretically possible.
• Thus, n → π* & π → π* electronic transitions
above 200 nm which is accessible to UV-
visible spectrophotometer.
• The UV spectrum is of only a few broad of
absorption. 17/3713-11-2019 Google, Wikipedia

Chromophore
The part of a molecule responsible for imparting
color, are called as chromophores.
OR
The functional groups containing multiple bonds
capable of absorbing radiations above 200 nm
due to n → π* & π → π* transitions.
e.g. NO2, N=O, C=O, C=N, C≡N, C=C, C=S, etc

λmax = 279 nm
EXAMPLES:
λmax = 291 nm
λmax = 227 nmλmax = 178 nm

Auxochrome
The functional groups attached to a
chromophore which modifies the ability of the
chromophore to absorb light , altering the
wavelength or intensity of absorption.
OR
The functional group with non-bonding electrons
that does not absorb radiation in near UV region
but when attached to a chromophore alters the
wavelength & intensity of absorption.

λmax = 255nm
λmax = 270nm
λmax = 280nm
λmax = 287nm
λmax = 254nm
EXAMPLES:

• Bathochromic Shift (Red Shift)1
• When absorption maxima (λmax) of a
compound shifts to longer wavelength, it is
known as bathochromic shift or red shift.
• The effect is due to presence of an auxochrome
or by the change of solvent.
• e.g. An auxochrome group like –OH, -OCH3
causes absorption of compound at longer
wavelength.

• In alkaline medium, p-nitrophenol shows red
shift. Because negatively charged oxygen
delocalizes more effectively than the unshared
pair of electron.
λmax = 255nm λmax = 265nm

• Hypsochromic Shift (Blue Shift)2
• When absorption maxima (λmax) of a
compound shifts to shorter wavelength, it is
known as hypsochromic shift or blue shift.
• The effect is due to presence of an group
causes removal of conjugation or by the
change of solvent.

• Aniline shows blue shift in acidic medium, it
loses conjugation.

• Hyperchromic Effect3
• When absorption intensity (ε) of a compound is
increased, it is known as hyperchromic shift.
• If auxochrome introduces to the compound,
the intensity of absorption increases.

• Hypochromic Effect4
• When absorption intensity (ε) of a compound is
decreased, it is known as hypochromic shift.

Shifts and effects

Instrumentation
Components of UV-Visible spectrophotometer
 Source
 Filters & Monochromator
 Sample compartment
 Detector
 Recorder

1. LIGHT SOURCES
• Deuterium lamp
• Hydrogen lamp
• Tungsten lamp
• Xenon discharge lamp
• Mercury arc lamp
• Mercury vapour lamp
• Carbonone lamp
UV Sources
Visible Source

2. Wavelength Selectors
Two types of wavelength selectors:
A) Filters
a) Interference Filters
b) Absorption Filters
B) Monochromators
a) Prism type
b) Grating type
Refractive type
Reflective type
Diffraction type
Transmission Type

3. SAMPLE COMPARTMENT
• Optical Glass - 335 - 2500 nm
• Special Optical Glass – 320 - 2500 nm
• Quartz (Infrared) – 220 - 3800 nm
• Quartz (Far-UV) – 170 - 2700 nm
4. Detectors
• Barrier layer cells
• Photo emissive cell detector
• Photomultiplier

Applications
• Detection of Impurites.
• Structure elucidation of organic compounds.
• used for the quantitative and qualitative determination of
compounds that absorb UV radiation.
• This technique is used to detect the presence or absence of
functional group in the group.
• Kinetics of reaction can also be studied using uv spectroscopy.
• Molecular weights of compounds can be measured
spectrophotometrically by preparing the suitable derivatives of
these compounds.
• Uv spectrophotometer may be used as a detector for HPLC.

Advantages
• High accuracy
• Easy to handling
• Provide robust operation
• Utilized in qualitative and quantitative analysis
• Derivative graph can be obtained
• Cost effective instrument
Disadvantages
• Only those molecules are analyzed which have chromophores.
• Only liquid samples are possible to analyzed.
• Result of the absorption can be effective by pH ,temperature and
impurities.
• It takes time to get ready to use it.
• Cuvette handling can affect the reading of the sample.

UV - VISIBLE SPECTROSCOPY

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UV - VISIBLE SPECTROSCOPY