Visible and Ultraviolet Spectroscopy MANIK

PHARM 3235

Md. Imran Nur Manik

Lecturer

Department of Pharmacy

Northern University Bangladesh

Visible and Ultraviolet Spectroscopy

Prepared By: Md. Imran Nur Manik; B.Pharm; M.Pharm Page 1 [email protected]; Lecturer; Department of Pharmacy; Northern University Bangladesh.

Ultraviolet-Visible Spectroscopy

Introduction:

Spectroscopy:

Spectroscopy is the study of interaction between matter (mass) and radiated energy. Such interaction includes –

1. Absorption of the incident radiant energy. 2. Emission of radiant energy. 3. Scattering or reflection of incident radiant energy. 4. Impedance of radiant energy transmission. 5. Changing the frequency/wavelength of the transmitted radiant energy. 6. Causing interaction between molecules in a non-stationary state and sustaining it.

Absorption spectroscopy/spectrometry:

Absorption spectroscopy may be defined as the analysis of chemical substances by measurement of the amount of radiant energy absorbed by the substance.

UV-Visible spectroscopy:

UV-visible spectroscopy is a type of absorption spectroscopy which uses the UV and visible part of the EM spectrum.

Electromagnetic (EM) spectrum:

Spectrum:

Spectrum is the condition where a characteristic is not limited to a fixed set of values rather it varies infinitely within a continuum.

By that definition, radiation arranged by wavelength is a spectrum; drug activity in terms of action against bacteria is a spectrum.

Electromagnetic spectrum:

It is the arrangement of all types of electromagnetic radiation in order of their increasing or decreasing wavelength (or frequency).

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The above diagram shows the electromagnetic spectrum where radiations are arranged in the decreasing order of wavelength from left to right.

Visible and UV spectrum:

Color

Wavelength

Violet 400-420 Indigo 420-440 Blue 440-490

Green 490-570 Yellow 570-585 Orange 585-620

Red 620-780 The visible spectrum starts at 400 nm and ends at around 700 nm. The electromagnetic radiation adjacent to the violet visible radiation is called ultraviolet radiation. The electromagnetic radiation adjacent to the red visible radiation is called infrared radiation.

The UV spectrum ranges from 10 nm to 380 nm. The UV radiation has been classified as UV A (400-315 nm), UV B (315-280 nm) and UV C (280-10 nm) based on their wavelength.

Relationship between wavelength & color

Wavelength (nm) Spectrum region Colour absorbed Colour transmitted 400-420 Visible Violet Green-yellow 420-500 Visible Blue yellow 500-570 Visible Green Red 570-600 Visible yellow Blue 600-630 Visible orange Green-blue 630-700 Visible Red Green

Electromagnetic radiation:

Electromagnetic radiation is a form of energy that shows wave-like characteristics and –

1. It can travel without any medium 2. At vacuum it moves at speed of light 3. Contains both electric and magnetic field components. These two components oscillate

(moving back and forth) in a phase perpendicular to each other. When an electric field oscillates it causes the oscillation of the corresponding magnetic field which in turn oscillates the next electric field. Thus the EM radiation moves forward without any medium.

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EM radiation is described by wavelength () or frequency (n). The relationship between wavelength and frequency is given in following equation.

nλc Where c is the speed/velocity of the wave. At vacuum c is equal to the speed of light i.e.

11018 103103 cmsms . Pharmacists rarely use frequency value for analytical purposes and wavelength value is of more importance.

Wavelength:

The wavelength of an wave is the linear distance between two consecutive corresponding

points of the same phase.

Since wave repeats a cycle over and over again, the lineardistance between two identical

points of two adjacent cycle is the wavelength. Thus wavelength is the linear distance

between the two corresponding peaks of a wave.

Frequency:

It is the number of cycles occuring per second

One cycle completed

Effect of electromagnetic radiation on a substance:

When a beam of electromagnetic radiation passes through a transparent medium of the substance (the substance under analysis must be in solution for proper analysis), the radiation is absorbed and/or transmitted by the substance. The absorption of the radiation depends on the –

- Chemical nature of the substance - Wavelength of the radiation

The radiation not absorbed is transmitted by the substance and it is called transmitted light which can be measured by an instrument called the spectrophotometer. The record is called the spectrum of that substance.

Transmittance “T”

The amount of light that passes through a particular thickness of solution is known as transmittance T.

Transmittance can be expressed as the ratio of the intensity of the transmitted light I to the intensity of the incident light beam Io

I

IT

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Absorbance “A”

The negative logarithm of the base ten of transmittance is called absorbance.

logTA

I

IlogA

I

IlogA

It is also called optical density.

Absorbance is directly proportional to the concentration of the solution when the thickness of the medium is constant.

Laws governing spectrophotometry

As described before, when a substance is placed in the path of light (EM radiation), a number of events e.g. absorption, transmission, elastic and nonelastic scattering of light may take place.

The absorption of EM radiation/light by molecules is governed by two laws – Lambert’s law and Beer’s law.

LAMBERT'S LAW

Lambert described how intensity changes with distance in an absorbing medium.

Lambert’s Law: When a beam of monochromatic radiation is passed through a solution of an absorbing medium, the decrease in the intensity of radiation with thickness of the solution is directly proportional to the intensity of the incident light.

Incident

lightTransmitted

light1/6 1/6 1/61/6 1/6 1/6

Intensity decreases

as light pass through

each layer

The solution has been hypothetically divided

into 6 layers of equal thicknes. According to

the Lambert's law, each layer absorbs same

fraction of the passing light even though the

intensity decreases.

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Let,

I be the intensity of incident radiation.

b be the thickness of the solution.

ThenI

db

dI

KIdb

dI

K'=Absorbing co efficient or Proportionality constant

Idb

dIK

Now integrating the equation between the limit I=Iₒ at b=0

And I=I at b=b

We get,

I

I

b

dbK

I

dI

0

b0I

I bK lnI

b.KI

Iln

b.KI

Ilog303.2

b.303.2

K

I

Ilog

EbI

Ilog

Where 2.303

K

=E= Extinction co efficient

We know that absorbance I

Ilog

A

Thus A= Eb

A∞b

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The amount of light absorbed by the medium (solution/ sample) at a given wavelength is proportional to thickness of the absorbing layer i.e. path length of the light

Basically it states that the absorbance is proportional to the path length i.e.

A∞b

Beer’s law

Relates the absorption of light to the properties of the material through which the light is travelling.

Beer’s Law: When a beam of monochromatic radiation is passed through a solution of an absorbing medium, the decrease in the intensity of radiation with thickness of the solution is directly proportional to the intensity of the incident light as well as concentration of the solution.

Let I be the intensity of incident radiation.

x be the thickness of the solution.

C be the concentration of the solution.

C.Idx

dI

C.Idx

dIK

K'=Absorbing co efficient or Proportionality constant

C.dxI

dIK

Now integrating the equation between the limit I=Iₒ at x=0

And I=I at x=l (l=Path length of the sample which is usually 1 cm)

we get

I

I

l

K

.dxCI

dI

0

l0I

I x CKlnI

.C.lKI

Iln

.C.lKI

I2.303log

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C.l2.303

K

I

Ilog

lCE ..I

Ilog

Where 303.2

K

=Extinction co efficient

We know that absorbance I

Ilog

A

Thus A=E.C.l

From the equation it is seen that the absorbance which is also called as optical density (OD) of a solution in a container of fixed path length is directly proportional to the concentration of a solution.

Accordingly The amount of light absorbed by the a medium (solution/ sample) is proportional to the concentration of the absorbing material or solute present.

This law states that absorption of the incident light is proportional to the number of absorbing molecules. So according to this law –

A∞c

Where, c is concentration of the substance in solution and A is absorbance.

Thus the concentration of a coloured solute in a solution may be determined in the lab by measuring the ABSORBANCY OF LIGHT AT A GIVEN WAVELENGTH

Combining Beer’s law and Lambert’s law – Beer-Lambert law/Equation of absorbance:

According to the Lambert’s law –

bA

According to the Beer’s Law –

cA Combining the two laws we have –

A∞bc

abcI

I

abcA

KbcA

0log

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Where,

ty"absorptivi" as termed and constant alityproportion a is It a

molecules absorbing the of ionConcentrat c

solution absorbing or sample of length Path b

light dtransmitte the of Intensity I

light incident of Intensity I

Absorbance A

0

Absorptivity:

Absorptivity is a measure of how easily the absorbing molecules can absorb the electromagnetic radiation. It is specific for a given substance. It is defined as the absorbance by a sample of unit concentration and where the path is of unit length.

It is mathematically quotient of the absorbance (A) divided by the concentration of the solution (gm/L) and the path length (cm).

bc

Aa

When c is expressed in moles/litre in the Beer-Lambert law, the absorptivity is called molar absorptivity or molar extinction coefficient and it is expressed by

bc

A

When, c is expressed as %w/v, the absorptivity is expressed as %11cmA .

Deviations from Beer-Lambert law

The accuracy of the Beer Lambert law is dependant upon some chemical and instrumental factors –

1. This law specifically the part concerning concentration is not maintained in high concentrated solutions. This is because –

a. In highly concentrated solutions, degree of interaction between molecules is higher at higher concentration. Thus the molecules will not absorb radiation in same manner as when they are in dilute solution.

b. The absorptivity of solution doesn’t remain constant as the concentration changes. c. The refractive index of the solution may change in high concentration.

2. If the solution contains particulate matter then scattering of light occurs which interfere with the absorption process.

3. If the sample is fluorescent or phosphorescent then this law is not obeyed. 4. If the light is non-monochromatic (in practice, monochromatic light is difficult to produce)

i.e. not completely monochromatic.

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Absorption of radiant energy

Effect on molecules upon absorption of radiation:

Electromagnetic radiation is energy. When a molecule absorbs radiation it gains energy. The higher the frequency the greater will be the gain in energy. This energy can bring about one or more of the following changes –

1. The absorbed energy may break bonds within molecule. e.g. conversion of ergosterol to calciferol.

2. The absorbed energy may increase vibration or rotation of atoms within the molecule. This principle is used in IR spectroscopy.

3. It may change nuclear or electronic spin. This property is used in NMR spectroscopy. 4. It may cause electrons to rise to higher energy level.

The UV and visible radiation absorption will cause the last effect i.e. transition of electrons within the molecule.

Energy of a molecule

Every molecule has a definite energy state. Energy possessed by a molecule can be classified in several categories. These are

1. Transitional energy (Etrans) 2. Vibrational Energy (Evib) 3. Rotational Energy (Erota) 4. Electronic energy (Eelec)

Transitional energy

Molecule as a whole can move from one place to another and the energy associated with this motion (Velocity) is called transitional energy as well as the movement is called transitional movement.

Vibrational Energy (Evib)

The movement of a part of a molecule or a group of molecules that move within themself is called vibrational movement and the energy associated with this vibration is called vibrational energy.

Rotational Energy (Erota)

Molecule can rotate along its axis and the energy associated with this rotation is called rotational energy.

Electronic Energy (Eelec)

Electrons of each atom moves around the central nuclei and the energy associated with this movement is called electronic energy

Translational < Rotational < Vibrational < Electronic

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For example, a simple molecule, such as H2, may have the following energy levels:

Theory or principle of Electronic spectroscopy or molecular Spectroscopy

When a molecule absorbs electro magnetic radiation like UV or Visible light its electron gets promoted from the ground state to the higher energy state or excited state. (Ground State: The molecules when attained in a state, having lower energy level i.e. normal unexcited condition or state is called ground state. Excited state: Absorbsion of EMR by the molecule results in the shipment of the molecule in the higher energy state called excited state)

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In the ground state the spin of electrons in each molecular orbital is essentially paired. In the higher energy state, the spins of electrons are either paired i.e. excited singlet state or parallel excited triplet state. Normally the absorption of the UV or visible light results in the transition of the singlet ground state to become singlet excited state.

To get the molecule in the higher energy level the energy difference between the two energy level must be equal to the energy of photon absorbed, which can be expressed as

Energy required to get in the excited state, ΔE=E2-E1=hν

Here, E1= Lower energy level

E2=Higher Energy Level

h= Planks Constant

ν=Frequency

Generally the energy of the triplet excited state is lower than the singlet excited state. Thus to be stable the molecule quickly returns from one of its higher energy level to lower one by the emission of radiation.

Therefore an electron that has been raised to the higher energy level by the absorption of radiation, quickly returns to the ground energy level within 10-8 seconds either directly or by the way of second excited state and will give molecular absorption spectrum.

(Molecular absorption spectrum: A set of bands or lines generated, due to the absorption of EMR by the molecules is called MAS. It is actually a graph obtained by plotting the absorption against wavelength)

As the transmission rates are different for different molecule or structure, so the absorption spectra will be different also. Greater the number of molecules capable of absorbing the light of different given wavelength the greater will be the extent of light absorption. MAS is characteristics for a molecule and there is no similarity in MAS of one molecule with other, Thus it is used to in the quantitative analysis of the molecules.

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Generally the absorption spectra is graphically represented by plotting the absorbance (A) on the Y axis and the wavelength on the x axis.; This is the principle or theory of UV or visible molecular absorption spectroscopy.

Electronic transition

When UV and visible radiation excites the molecule the electrons are temporally moved from one orbital (bonding orbital according to MOT) to another orbital (Anti-bonding orbital according to MOT). These electrons may be σ, π or n (non-bonding) electrons. (Time requires 10-8 sec)

Thus possible transitions are –

1. σ → σ* 2. n → σ* 3. π → π* 4. n → π*

(There is no n* orbital as n electrons don’t form bonds).

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σ → σ* transition:

C C C C

1. This type of transition takes place in the saturated centre of the molecules. 2. Here, an electron from a stable σ orbital goes to an unstable or anti-bonding σ orbital

(represented by σ*). 3. High energy is required to excite electrons present in the σ orbital as they are held tightly.

Therefore saturated compounds do not absorb radiation from normal UV-Vis spectrophotometer which generates radiation of 190-780 nm region.

n → σ* transition:

C X C

n

O

N

X

O

n

n

n

N

SS

1. This type of transition occurs in saturated compounds containing heteroatom which has an unshared electron pair.

2. Electron transits from unshared pair to anti-bonding σ orbital. 3. This type of transition may take place in halogen, sulfur, nitrogen and oxygen containing

compounds. 4. This transition requires high energy and therefore doesn’t occur in presence of the EM

radiation produced by normal UV-Vis spectrophotometer.

π → π* transition (K-band):

C O C

O

1. Takes place in unsaturated compounds containing double or triple bonds. 2. Electron transits from stable π orbital to an unstable/anti-bonding π orbital (represented

by π*). 3. It requires less energy as π bonds are sufficiently weaker than σ bonds. Conjugated

double bonds further lowers required energy. For example β-carotene containing 11 conjugated double bonds absorbs energy at 451 nm (visible region).

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n → π* transition (R-band):

C OC On *

1. This type of transition takes place in compounds having heteroatom which contains unshared electron pair.

2. Electron transits from unshared pair to anti-bonding π orbital. 3. Requires lower energy and therefore respond to the radiation produced by normal UV-Vis

spectrophotometer. 4. Carbonyl compounds, cyanides etc. show this type of transition. 5.

Effect of solvents on electronic transition

The polarity of the solvent affect the energy required for electronic transition. This is described below. We need to remember that polarity results from unequal distribution of electrons – the greater is the difference the greater is the polarity.

n → π* transition:

More energy required

Shift to Shorter wavelength

Ground state

Excitated state

C OC O

More polar Less polar

n *x

y

n

The diagram above illustrates the polarity of the molecule at excited state and ground state. If the solvent is polar, then dipole-dipole interaction between the solvent molecule and sample molecule will be greatest at ground state. Hence, energy of the grounds state is lowered significantly but that of excited state is raised (or not lowered significantly). The result is that more energy i.e. radiation of shorter wavelength is required to excite the electrons.

π → π* transition:

Ground state

Excitated state

C OC O

Less polar More polar

*

xy

Less energy required

Shift to longer wavelength

Here polarity increases after transition.

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Thus the polar solvent molecule will show greater interaction with the excited state than with ground state. Hence, energy required for excitation is decreased.

n → σ* transition:

Ground state

Excitated state

C OC O

More polar Less polar

n *x

y

n

More energy required

Shift to shorter wavelength

The polarity decreases after transition to excited state. So the polar solvent prefers the ground state. Hence more energy is required for excitation.

σ → σ* transition:

Polarity unchanged

C C C C

In saturated compounds (no atom with lone pair of electrons though) transition doesn’t change polarity much. Thus solvent effect is not seen.

Impurities

Impurities in the solvent affect the result in UV-Vis spectroscopy. The impurity will absorb light hence the absorbance is exaggerated. This is why commercial absolute ethanol should not be used to prepare sample solution as it contains benzene as impurity which strongly absorbs light in the UV region.

Nature of the absorption band

The solvents used in sample preparation will absorb radiation at some specific wavelength. So, radiation of that wavelength becomes unavailable for spectral studies. For example, chloroform will strongly absorb radiation of below 245 nm. Thus this solvent can’t be used in a sample that will be run at a wavelength lower than 245 nm. The table below shows the minimum wavelength at which the solvent can be used to make sample solution. For example, methanol should not be used if the sample is to be run at wavelength lower than 203 nm.

Solvents Minimum wavelength for 1 cm cell, nm

Solvents Minimum wavelength for 1 cm cell, nm

Acetonitrile 190 Ethanol 204

Water 191 Ether 215

Hexane 201 Chloroform 237

Methanol 203 Carbon tetrachloride

257

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Absorbing groups

There are two types of groups present in a molecule which is responsible for characteristic electromagnetic radiation absorption by the molecule. These are described below –

1. Chromophore

A chromophore is a chemical group that absorbs light at a specific frequency and so imparts color to a molecule.

It is defined as any isolated covalently bonded group that shows a characteristic absorption in the ultraviolet or visible region.

When a chromophore is attached to a saturated hydrocarbon, produces a molecule that absorbs a maximum of UV or visible energy at some specific wavelength. Compounds containing a chropmophoric group called a chromogen.

Some chromophores are listed below –

Chromophore Structure Example of molecule max Acetylene (carbon-carbon triple bond) C C Acetylene 173 Amide CONH2 Acetamide <208 Azo N N Azomethane 347 Carbonyl (ketone)

C

O

Acetone 271

Carbonyl (Aldehyde)

C

O

H

Acetaldehyde 293

Ethylene (carbon-carbon double bond) C C

Ethylene 234

Nitrile C N Acetonitrile <160 A compound may contain two or more chromophores and then the relative position of the chromophores will determine the absorption of radiation.

Chemical structure of beta-carotene. The eleven conjugated double bonds that form the chromophore of the molecule are highlighted in red.

2. Auxochrome: An auxochrome is a group of atoms attached to a chromophore which modifies the ability of that chromophore to absorb light. They themselves fail to produce the colour; but when present along with the chromophores in an organic compound intensifies the colour of the chromogen. Auxochrome group contains at least one atom with lone pair of electrons. Examples include the hydroxyl group (-OH), the amino group (-NH2), the aldehyde group (-CHO), ─NHR, ─NR2.

Benzene shows absorption maximum at 255 nm whereas aniline at 280 nm.

=255 nm = 280 nm

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https://en.wikipedia.org/wiki/Beta-carotene

https://en.wikipedia.org/wiki/Chromophore

https://en.wikipedia.org/wiki/Absorption_(light)

https://en.wikipedia.org/wiki/Chromogen

https://en.wikipedia.org/wiki/Hydroxyl_group

https://en.wikipedia.org/wiki/Amino_group

https://en.wikipedia.org/wiki/Aldehyde



M/A: They have lone pair electrons that interferes with the chromophores electron transition system i.e. with the electronic localization. This affects the conjugation system of the compound and causes the

shipment of the max as well as ϵmax to the higher value. Higher the conjugation higher the shipment.

Terminologies describing effects of solvent, chromophores and auxochromes

Absorption and intensity shifts

1. Bathochromic shift or Red shift: It is the displacement/shift of max (absorption maximum) towards longer wavelength. This may occur due to solvent effect, conjugation or auxochrome addition.

Ab

sorb

an

ce

0 X

Y

max

max

Shift

Hexane

Aqueous acid

max

max= 230

=203

It is known as red shift. Following is an example of this effect.

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2. Hypsochromic shift or Blue shift: it is the displacement of max towards the shorter wavelength. This is usually due to solvent effect.

Abs

orba

nce

0 X

Y

max

max

Shift

Hexane

Aqueous acid

max

max= 230

=203

3. Hyperchromic effect: It is the effect of increased intensity of radiation absorption by the molecule.

Ab

sorb

an

ce

Pyridine 2-methyl pyridine

λmax = 257 nm λmax = 260 nm ε = 2750 ε = 3560

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.

4. Hypochromic effect: It is the effect of decreased intensity of radiation absorption by the molecule.

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

Abs

orba

nce

Naphthalene 2-methyl naphthalene

ε = 19000 ε = 10250

CH3

N N CH3

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Vacuum ultraviolet region

Oxygen of atmosphere absorbs UV light of below 200 nm. So it is difficult to analyze a sample by running it at wavelength below 200 nm. If we want to measure absorption of UV radiation below 200 nm we must remove all the air from the instrument.

Thus vacuum is used. So the UV radiation below 200 nm is known as vacuum ultraviolet region.

This region is relatively uninformative as it excites the σ electrons. Above this region, π electrons are excited. The double and triple bonds are comparatively more informative in the analysis of a

compound. Explanation of electronic transitions in polyenes

Compound max (nm) H2C CH2 175

217

256

290

334

364

As we can see that, ethylene with only one double bond show most absorption at 175nm, whereas 1,3-butadiene show most absorption at 217 nm. Generally the longer the conjugated system the longer is the wavelength of maximum absorption. For example, β-carotene contains 11 double bonds and show maximum absorption at 451 nm (visible range).

When two atomic orbitals are combined, two molecular orbitals are produced. One is of high energy. This is the unstable molecular orbital called the anti-bonding orbital. Another is of lower energy and this is the stable orbital. Electrons are present in the stable orbital.

Two atomic p orbitals

High energy: Antibonding orbital. Electron not present in this

molecular orbital i.e it is the Lowest unoccupied molecular

orbital (LUMO).

Low energy: Bonding orbital. Electrons are present in this

molecular orbital. It is the Highest occupied molecular

orbital (HOMO)

Substraction of the wave functions of the atomic orbitals

Addition of the wave functions of the atomic orbitals

Figure: Molecular orbitals in ethylene

En

erg

y

Eenrgy required for

excitation in ethylene.

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Below is the molecular orbitals of 1,3-butadiene. There are two double bonds in this molecule. Each double bond forms two molecular orbital – one bonding orbital and one anti-bonding orbital.

The two bonding orbitals of the two double bonds combine to form two molecular orbitals. Among them one is higher in energy than ethylene molecule and another is lower. The higher energy molecular orbital is the HOMO.

Similarly, the two anti-bonding orbitals of two double bonds will produce two new molecular orbitals. One of them will be lower in energy than the excited ethylene molecule and another will be higher in energy than excited ethylene molecule (excited is the keyword – in HOMO determination we took the molecular orbital that was higher in energy than the ground state ethylene molecule, not excited ethylene molecule). Among the two the molecular orbital with lower energy than the excited ethylene molecule is the LUMO. One should remember that anti-bonding molecular orbitals are normally unoccupied and becomes occupied when electrons are excited.

As we can see that the energy difference between LUMO and HOMO of 1,3-butadiene will lower than that of ethylene. (Ethylene has only one anti-bonding orbital which is the LUMO for ethylene, 1,3-butadiene has two anti-bonding orbitals where the one which has lower energy than LUMO of ethylene is the LUMO of 1,3-butadiene).

This is the HOMO

This is the LUMO

Anti-bonding

molecular orbitals

Bonding

molecular orbitals

Eenrgy for

excitation

En

erg

y

Figure: Molecular orbitals of 1,3-butadiene

Each of these two MO is equivalent

to the LUMO of

ethylene

Each of these two MO is equivalent

to the HOMO of

ethylene

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As the double bonds/conjugation increases, so the energy difference between LUMO and HOMO decreases (e.g. in ethylene the difference is 176 kcal/mol and in 1,3-butadiene the difference is 131 kcal/mol). Thus increase of double bonds decrease energy required for absorption.

Antibonding

orbitals

Bonding

orbitals

H2C CH2

Ethylene Butadiene Hexatriene Octetraene

En

erg

y

Figure: Energy gap for excitation in polyenes

Instrumentation

Spectrometer

Spectrometer is an instrument that is used to measure a physical property over a specific region of the spectrum of that property.

The physical property is usually the intensity of light but other properties can also be used. For example in mass spectrometer, relative abundance of particles is measured over mass-to-charge ratio.

Simply spectrometer is any instrument used to measure spectrum.

Spectrophotometer

A spectrophotometer is an instrument used to measure the intensity of light over a specific region of the electromagnetic spectrum.

In another words, a spectrophotometer is a spectrometer with a photomultiplier that is used to detect light and determine its intensity as a function of wavelength.

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Colorimeter

A colorimeter is a spectrophotometer which is designed to detect only the absorption at the visible region i.e. it will measure the intensity of light at the visible region of the electromagnetic spectrum.

Fig: Colorimeter

Parts of the UV-Visible spectrophotometer:

Basic Parts

1. A Stable and cheap radiant energy source. 2. A monochromator, to break the polychromatic radiation into component wavelength (or)

bands of wavelengths. 3. Transport vessels (cuvettes), to hold the sample. 4. A Photosensitive detector and an associated readout system.

Fig: Basic Parts of spectrophotometer

The UV-visible spectrometer is a spectrophotometer designed to work in the UV and visible range of the electromagnetic spectrum.

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It consists of following parts –

1. Radiation source: A source for UV and visible light is perquisite. A UV-visible spectrophotometer works at around 190-800 nm range. Usually two sources are used –

a. Hydrogen or deuterium discharge lamp: It emits electromagnetic radiation of 185-365 nm wavelengths.

b. Tungsten lamp (6V or 12V): It emits electromagnetic radiation of 350-800 nm. Since, none of them produces the complete range of the target spectrum. They are used simultaneously.

Requirements for radiation source

1. The radiation should be continuous 2. Its spectrum should include all the wavelengths required for the analysis. 3. The power of the beam should be such that, the solution can transmit some or all of the radiation energy at all wavelengths. 4. The power of the beam must remain constant throughout the measurement.

Various UV radiation sources are as follows

a. Deuterium lamp b. Hydrogen lamp c. Tungsten lamp d. Xenon discharge lamp e. Mercury arc lamp

RADIANT ENERGY SOURCES

Materials which can be excited to high energy states by a high voltage electric discharge (or) by electrical heating serve as excellent radiant energy sources. Sources of Ultraviolet radiation: Most commonly used sources of UV radiation are the hydrogen lamp and the deuterium lamp. Xenon lamp may also be used for UV radiation, but the radiation produced is not as stable as the hydrogen lamp. Sources of Visible radiation: “Tungsten filament” lamp is the most commonly used source for visible radiation. It is inexpensive and emails continuous radiation in the range between 350 and 2500nm. “Carbon arc” which provides more intense visible radiation is used in a small number of commercially available instruments. Sources of IR radiation: “Nernst Glower” and “Global” are the most satisfactory sources of IR radiation. Global is more stable than the nearest flower.

For Visible region

Tungsten filament lamp • Use for region 350nm to 2000nm. • These measure most effectively in the visible

region from 320 - 1100 nm • Instruments that only use Tungsten halogen

lamps as the light source will only measure in the visible region.

For ultra violet region

Hydrogen discharge lamp Fig. Tungsten filament lamp • Consist of two electrode contain in Hydrogen filled silica envelop. • Gives continuous spectrum in region 185-380nm. above 380nm emission is not continuous

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Fig. Hydrogen discharge lamp

Deuterium lamps:

• Deuterium arc lamps measure in the UV region 190 -

370 nm

• As Deuterium lamps operate at high temperatures,

normal glass housings cannot be used for the casing.

Instead, a fused quartz, UV glass, or magnesium fluoride

envelope is used.

• When run continuously typical lamp life for a Deuterium

lamp is approximately 1000 hours, however this can be

extended by up to a factor of three using PTR technology.

• Deuterium lamps are always used with a Tungsten halogen lamp to allow measurements to be performed

in both the UV and visible regions.

2. Monochromator: The monochromator disperses the polychromatic light by means of a prism or grating (in grating there is a flat surface having alternating reflective and non-reflective portions). The desired monochromatic light is obtained by changing the angular position of prism or grating and this monochromatic light is allowed to pass to sample.

Monochromatic Light: The light having a single wavelength and frequency i.e. the light that vibrates at a single wavelength.

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Polychromatic Light: The light having several colours i.e. light having electromagnetic radiation of several wavelengths.

The light must be monochromatic as extinction coefficient is variable with wavelength.

2. WAVELENGTH SELECTORS

Wavelength selectors are of two types.

1. Filters: “Gelatin” filters are made of a layer of gelatin, colored with organic dyes and sealed between glass

plates.

2. Monochromators: A monochromator resolves polychromatic radiation into its individual wavelengths and

isolates these wavelengths into very narrow bands. The essential components of a monochromator are.

a. Entrance slip-admits polychromatic light from the source

b. Collimating device – Collimates the polychromatic light onto the dispersion device.

c. Wavelength resolving device like a PRISM (or) a GRATING

d. A focusing lens (or) a mirror

e. An exit slip – allows the monochromatic beam to escape.

The kinds of the resolving element are of primary importance

PRISMS: A prism disperses polychromatic light from the source into its constituent wavelengths by virtue of its

ability to reflect different wavelengths to a different extent;

The degree of dispersion by the prism depends on upon

a. The optical angle of the Prism (usually 600)

b. The material of which it is made

Two types of Prisms are usually employed in commercial instruments. Namely, 600cornu quartz prism and

300 Littrow Prism.

GRATINGS: Gratings are often used in the monochromators of spectrophotometers operating ultraviolet, visible

and infrared regions.

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3. Sample compartment: The sample is kept in a small tube of square cross section called “cuvette” i.e. the tube has four sides.

There are two opposite sides through which the light is supposed to pass (i.e. these two sides form the optical window). The other two sides are usually unclear (in some cases, all four sides may be clear) and used for handling. The cuvette (at least the optical window of the cuvette) is made of glass, plastic or fused quartz. The glass and plastic cuvettes are used to measure at visible spectrum while quartz cuvettes are used to measure at ultraviolet spectrum. The length of the optical window is usually 1cm.

Fig. cuvette

4. Detector: The detector converts the radiant energy into electrical energy. Most detectors depend on the photoelectric effect. The current is then proportional to the light intensity and therefore a measure of it. Important requirements for a detector include

i. High sensitivity to allow the detection of low levels of radiant energy ii. Short response time iii. Long term stability iv. An electric signal which easily amplified for typical readout apparatus.

In spectrophotometer the detector is a photomultiplier tube. It consists of following parts – a. One cathode (electron emitter): It emits electrons when the photon of radiation strikes it.

b. Several electrodes called dynodes: After the cathode there are a number of electrodes called the dynodes. The dynode next to cathode is more positive than cathode and produces several electrons for each electron striking it. The dynode next to the 1st dynode is even more positive and it also produces more electrons. By the time electrons are collected at anode, for each photon about 106-107 electrons are generated. c. One anode: It receives the electrons generated on the way. The resulting current is then measured.

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Anode

Dynode I

Dynode II

Dynode III

Dynode IV

Cathode

Light

Fig. Photomultiplier tube

5. Recorder: From the measurement of current obtained from transmitted light, it plots a graph of absorbance versus wavelength.

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The chart recorder

Chart recorders usually plot absorbance against wavelength. This particular substance has what are known as absorbance peaks at 255 and 395 nm. How these arise and how they are interpreted are discussed on another page.

Fig. The output of chart recorder.

Working principle

Firstly, the machine is started. The machine will run and take a reading of the intensity of the radiation source. This is the incident light intensity.

Entrance slit

Exit slit

Detector

Cuvette

Red

VioletPrism

MonochromatorLight source

I0

IReadout

device

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The sample is placed inside the instrument in cuvette. Light is generated by the radiation source and then passed through the monochromator. The monochromatic light is passed through the sample and then the intensity of the transmitted light is measured in the detector. From the intensity of the incident light and intensity of the transmitted light the computer will calculate and show the absorbance.

Then the blank/reference (sample solution minus the sample molecules) is placed in the instrument.

The intensity of the transmitted light is measured again. From these two values the relative intensities light before passing the sample molecules and after passing the sample molecules can be determined.

So basically there are two measurements involved.

In some single beam spectrophotometer a “zeroing” method is used where the absorbance by the reference is set as baseline value and then the absorption by the sample is measured relative to it.

Double beam spectrophotometer:

In single beam spectrophotometer there is a necessity to make two separate measurements. This has been eliminated with the double beam spectrophotometer.

In this instrument the blank (the reference cell) and the sample solution (sample cell) is placed simultaneously in the spectrophotometer. The light generated by the radiation source is passed through the monochromator and the monochromatic light is split into two beams (this is done by a rotating disc).

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One beam passes through the reference cell and other passes through the sample cell. Then the transmitted light (whether from reference cell or sample cell) is sent to the detector. The detector will measure the intensities of the transmitted light. A computer will analyze the intensities and subtract the intensity of transmitted light from sample cell from the intensity of the transmitted light from reference cell.

Thus the absorption by the rest of the part of solution is cancelled.

a) Single-beam spectrophotometer b) Double-beam spectrophotometer

a) Single beam spectrophotometer

A single-beam instrument uses only single beam of radiation through a single cell. The reference cell is used to set the absorbance scale at zero for the wavelength to be studied. It is then replaced by sample cell to determine the absorbance of the sample at that wavelength.

Fig: Single-beam spectrophotometer

b) Double-beam spectrophotometer

A double beam instrument divides the radiation into two beams of equal intensity which are passed through two separate cells. One of the two cells contains the sample solution, while other, called the reference cell, contains either the pure solvent or a blank solution. Since the absorption by the sample is automatically corrected for absorption occurring in the solvent, the readout from the instrument is the difference between amounts of the radiations absorbed in the two cells.

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Fig: Double-beam spectrophotometer

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Applications of UV spectroscopy

1. Structure elucidation of organic compounds: UV spectroscopy is useful in the structure elucidation of organic molecules,( the presence or absence of unsaturation, the presence of hetero atoms). From the location of peaks and combination of peaks, it can be concluded that whether the compound is saturated or unsaturated, hetero atoms are present or not etc.

2. Identification of an unknown compound- An unknown compound can be identified with the help of UV spectroscopy. The spectrum of unknown compound is compared with the spectrum of a reference compound and if both the spectrums coincide then it confirms the identification of the unknown substance.

3. Quantitative analysis: UV absorption spectroscopy can be used for the quantitative determination of compounds that absorb UV radiation. This determination is based on Beer’s law. A = abc

4. Detection of Impurities: Additional peaks can be observed due to impurities in the sample and it can be compared with that of standard raw material. Benzene appears as a common impurity in cyclohexane. Its presence can be easily detected by its absorption at 255 nm.

5. Qualitative analysis: In UV absorption spectroscopy identification is done by comparing the absorption spectrum with the spectra of known compounds. UV absorption spectroscopy is generally used for characterizing aromatic compounds and aromatic olefins.

6. Chemical kinetics: Kinetics of reaction can also be studied using UV spectroscopy. The UV radiation is passed through the reaction cell and the absorbance changes can be observed.

7. Molecular weight determination: Molecular weights of compounds can be measured spectrophotometrically by preparing the suitable derivatives of these compounds.

8. As HPLC detector: A UV/Vis spectrophotometer may be used as a detector for HPLC.

9. Detection of extent of conjugation- The extent of conjugation in the polyenes can be detected with the help of UV spectroscopy.

10. Determination of configurations of geometrical isomers- It is observed that cis-alkenes absorb at different wavelength than the trans-alkenes. The cis-isomer suffers distortion and absorbs at lower wavelength as compared to trans-isomer.

Theoretical determination of max of compounds:

In 1941, Robert Burns Woodward first put forward a set of rules to predict the λmax of a given compound in UV-Vis spectroscopy. These rules were applicable to open chain and 6-membered ring dienes.

Later the rules were modified by Fischer Scott and Louis Fieser. This is known as the Woodward-Fieser rules (This rule works well when the conjugated system is only 4 double bonds long. When more than four double bonds are present, one must use the Fieser-Kuhn rules instead).

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Various types of double bonds in conjugation are:

1. Homoannular dienes: It is a cyclic diene having conjugated doubles bonds in the same ring. e.g. Toluene, Naphthalene.

2. Acyclic dienes: Diene containedvin an open chain syatem. Where the basic unit is butadiene.

3. Heteroannular dienes: It is a cyclic diene in which double bonds in conjugation are present in different ring.

4. Endocyclic conjugated double bond: It is the double bond present in the ring.

5. Exocyclic conjugated double bond: It is a double bond is a double bond, part of the conjugated system and formed by any carbon atom of any ring but present outside of the ring.

According to the rules each type of diene or triene system have a fixed value at which absorption takes place. This constitutes the basic value or parent value. The contributions made by various alkyl substances or ring residue, double bonded extending conjugation and polar group such as –Cl, -Br, -OR are added to the basic value to obtain λmax for a particular compound. Ring residue is a C-C bond, not a part of the conjugated system; but attached to any one of the carbon atoms of the conjugated poyene system.

The parent values and contribution of different substituents or groups are given below (Conjugated trienes and dienes/solvent ethanol/pi-pi* transition)

1. Parent Values: Cyclic conjugated dien or butadiene 217nm

Acyclic triene 245 nm Heteroannular conjugated diene 215 nm Homoannular conjugated diene 253 nm

2. Increment for each substituent: Alkyl substituent or ring residue 5 nm

Exocyclic double bond 5 nm Double bond extending conjugation 30 nm

3. Auxochromes –OR +6 nm –SR +30 nm

–BR, -Cl +5 nm -NR2 +60 nm

-OCOCH3 0

Modified rules for open chain dienes:

According to the modified rules, calculation can be made as follows –

onscontributiOtheroncontributitsSubstituenvalueParentmax

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Such values are listed below –

Class Structure Wavelength value (nm)

Parent/base/core

C C

C

H

H C

H

H

H

H

217

A double bond extension of the conjugation C C

Thus, following structure has the λmax of 24430214

C C

C

H

H C

H

C

H

H C

H

HH

30

Alkyl group substituent ─R 5

Auxochromic (attached to the chromophore) OX

─OH, ─OR 6

Auxochrome – Acyloxy

Auxochrome – Ester C

O

R O C

O

R

0

Axochrome – Amine

N

R

R

60

Auxochrome – Halogen (X) Cl, Br 5

Sulfide SR 30

Phenyl

60

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Example explaining the modified rules for open chain dienes:

H3C C

C C

C C

C C

HC

H

H

H

H NH2

Cl H

OH

C

CH3

NH2

Here,

Parent value 217

Double bond extension of the conjugation 30

One Cl group 5

One NR2 group 60

two alkyl group (shown in sky blue and orange)

52

One OH group 6

total =328 nm

Modified rule for benzoyl derivatives:

Class Structure Wavelength value (nm)

Parent/base/core

C

OX

1. When X = Alkyl group or ring residue, 246.

2. When X = H, 250. 3. When X = OH or OR,

230.

Alkyl or ring residue on ortho or meta position.

3

Alkyl or ring residue on para position. 10

OH, OR at ortho or meta position. 7

OH, OR at para position. 25

NH2 at ortho or meta position. 13

NH2 at para position. 58

NHAc at ortho or meta position. 20

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NHAc at para position. 45

Cl at ortho or meta position. 0

Cl at para position 10

Br at ortho or meta position. 2

Br at para position. 15

Explanation of the modified rules for benzoyl derivatives:

O

H3CO

H2N

OCH3

OH

Here,

Parent value 246 (Since X = R)

Ring residue at ortho position 3

Ring residue at meta position 3

Ring residue at para position 10

NH2 group at ortho position 13

OR group at meta position 7

Total = 282 nm

[(A more elaborate description of the rules that can be used to determine the λmax of compounds can be found on www.pharmaxchange.info) – for conjugated diene systems, transoid and cisoid concept is important).

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http://www.pharmaxchange.info/



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Visible and Ultraviolet Spectroscopy MANIK

Health & Medicine

Transcript of Visible and Ultraviolet Spectroscopy MANIK