4. The magnetic and electric fields create each other again and
again
An EM wave travels in all directions. The figure only shows
a wave traveling in one direction
The electric and magnetic fields vibrate at right angles to
the direction the wave travels so it is a transverse wave
5. What is the speed of EM waves?
All EM waves travel
300,000 km/sec in space
(speed of light-nature’s
limit!)
EM waves usually travel
slowest in solids and
fastest in gases
Material Speed
(km/s)
Vacuum 300,000
Air <300,000
Water 226,000
Glass 200,000
Diamond 124,000
6. Properties of EM Waves
1. Waves
Wavelength= distance from crest to crest
Frequency= number of wavelengths that pass a given point in 1 s (Hertz or
cycles/sec or sec-1)
As frequency increases, wavelength becomes smaller
The velocity of
light, C, is given
by the equation:
7. Photons/Particles
The energy E of photon depends upon the frequency of the radiation
E = hn
E = hC/l
Energy is inversely proportional to wavelength
Where, h = Planck’s constant (6.626 x 10-34 J s)
n = frequency of the radiation (common units = cm-1)
Properties of EM Waves
8. The Electromagnetic Spectrum
Human eyes are only
able to process
information from the
visible part of the
spectrum
Toward longer
wavelengths, the
spectrum includes
infrared light,
microwaves, and radio
Toward shorter
wavelengths, the
spectrum includes
ultraviolet light, X-rays,
and gamma rays
All of these are forms of
electromagnetic
radiation
9. Visible light is a small portion of this spectrum. This is
the only part of this energy range that our eyes can
detect. What we see is a rainbow of colors
Red Orange Yellow Green Blue Indigo Violet
10. Radiation Interactions with Matter
Emission – release of electromagnetic waves
Absorption – receiving of electromagnetic waves
Scattering – deflection of electromagnetic waves in all
directions
Reflection – deflection of electromagnetic waves into the
backwards direction
Energy Transfer
• Conduction –molecule to molecule within a substance
• Convection (and advection) –mass movement of a fluid
• Radiation –absorption of electromagnetic waves
11. The absorption process
How does matter absorb radiation?
When polychromatic light (white light/whole spectrum) is
passed though an object it absorbs certain of the
wavelengths, leaving the unabsorbed wavelengths to be
transmitted.
These residual transmitted wavelengths will be seen as a
color. This color is complementary to the absorbed colors.
12. The colors we see in objects are the colors that are
reflected, all other colors are absorbed.
Red T-shirt Red- Red is reflected
All wavelengths
are absorbed-
Black (Black also,
isn’t really a color)
When all colors are being reflected we see white light
(white isn’t really a color)
13. Absorption is a process in which chemical species (atom,
ion or molecule) in a transparent medium selectively
attenuate certain frequencies of EMR
Absorption spectrum is a plot of the amount of light
absorbed by a sample as a function of wavelength.
At room temperature most substance are in their lowest
energy or ground state (G.S.)
When an atom, molecule or ion absorbs EMR and is
promoted to higher energy states or excited states
The E.S. is a (T.S.) and the species soon looses the energy
it gained and returns to its (G.S.) by relaxation process
either as heat of collision or sometimes emits radiation of
specific wavelength
14. When molecule absorbs light
What happens to absorbed energy ?
S2, S1 = Singlet States
15. More Complex Electronic Processes
Fluorescence:
absorption of radiation to an
excited state, followed by
emission of radiation to a
lower state of the same
multiplicity
Phosphorescence:
absorption of radiation to an
excited state, followed by
emission of radiation to a
lower state of different
multiplicity
0 sec 1 sec
Example of Phosphorescence
16. Singlet state:
spins are paired, no net
angular momentum (and
no net magnetic field)
Triplet state:
spins are unpaired, net
angular momentum (and
net magnetic field)
More Complex Electronic Processes
Spins paired
No net magnetic field
Spins unpaired
net magnetic field
10-5 to 10-8 s
10-4 to 10 s
17. E(ex)-E(g) = hn of the photon absorbed.
UV / VIS - Electronic transition (along with vibrational/rotational)
IR - Vibrational and rotational (No electronic transition)
Microwave - Rotational transitions alone
PMR/ NMR – Change in Nuclear Spin under magnetic
field
Etotal = Eelectronic + Evibrational + Erotational
Total Energy of the System
18. Common Spectroscopic Methods Based on Electromagnetic Radiation
Type of Spectroscopy Usual Wavelength
Range
Type of Quantum Transition
Gamma-ray emission 0.005-1.4 Å Nuclear
X-ray absorption, emission,
fluorescence, and diffraction
0.1-100 Å Inner electron
Vacuum ultraviolet
absorption
10-180 nm Bonding electrons
Ultraviolet visible
absorption, emission,
fluorescence
180 -780 nm Bonding electrons
Infrared absorption and
Raman scattering
0.78-300 mm Rotation/vibration of molecules
Microwave absorption 0.75-3.75 mm Rotation of molecules
Electron spin resonance 3 cm Spin of electrons in a magnetic field
Nuclear magnetic
resonance
0.6-10 m Spin of nuclei in a magnetic field
20. Beers Lamberts law
When a light passes through absorbing medium at right
angle to the plane of surface or the medium or the solution,
the rate of decrease in the intensity of the transmitted light
decreases exponentially as the thickness of the medium
increases arithmetically
Lambert’s law :
“When a beam of light is allowed to pass through a
transparent medium, the rate of decrease of intensity with the
thickness of medium is directly proportional to the intensity of
light”
21. Beers Lamberts law
Mathematically,
- dI / dt α I
-dI / dt = KI . . . . . . . . .(1)
Where,
I = intensity of incident light
t = thickness of the medium
K= proportionality constant
By integration of equation (1), and putting I=I0 when t=0,
I0/ It = kt or It= I0 e-kt
22. Beers Lamberts law
Where,
I0 = intensity of incident light
It = intensity of transmitted light
k = constant which depends upon wavelength and
absorbing medium used
By changing the above equation from natural log, we get,
It = I0 e-Kt . . . . . . . . . .(2)
Where,
K = k/ 2.303
So, It = I0 e-0.4343 kt
It = I010-Kt . . . . . . . . . .(3)
23. Beers Lamberts law
Beer’s law :
“Intensity of incident light decreases exponentially as the
concentration of absorbing medium increases arithmetically.”
The above sentence is very similar to Lambert’s law.
So, It = I0 e-k' c
It = I0 10-0.4343 k' c
It = I0 10 K' c . . . . . . . . . .(4)
Where, k' and K'= proportionality constants
c = concentration
24. Beers Lamberts law
Beer’s law :
By combining equation (3) and (4), we get,
It = I0 10 -act
I0 / It = 10 act
Where, K and K' = a or ε
c = concentration
t or b = thickness of the medium
log I0 / It = εbc . . . . . . . . . .(5)
Where, ε = absorptivity, a constant dependent
upon the λ of the incident radiation and
nature of absorbing material
25. Beers Lamberts law
Beer’s law :
The value of ε will depend upon the method of expression of
concentration.
The ratio I0 / It is termed as transmittance T, and
The ratio log I0 / It is termed as absorbance A
Formerly, absorbance was termed as optical density D or
extinction coefficient E, and
The ratio I0 / It is termed as opacity.
Thus,
A = log I0 / It . . . . . . . . . .(6)
26. Beers Lamberts law
Beer’s law :
From equation (5) and (6),
A = εbc . . . . . . . . . .(7)
Thus,
“absorbance is the product of absorptivity, optical path length
and the concentration of the solution”
According to equation (7),
A = log I0 / It
27. Beers Lamberts law
Beer’s law :
Transmittance T is a ratio of intensity of transmitted light to
that of the incident light.
T = I0 / It
The more general equation can be written as follows:
A = log I0 / It
A = log 1/ T
A = – log T
A = abc
A = εbc
31. 1. Sources
A Light Source should have following properties
Continuous : Emit radiation of all wavelengths within
the spectral region for which they are to be used
Stable
Brightness (high intensity)
Narrow Line Width
Background
Lifetime
Visible and Near IR = 390-700nm UV = 400 –10nm
32. Types of Lamps Used as Sources
1. Tungsten lamp
Excellent source
Operates at 3000 oK
Produces l from 320 to 2500 nm
2. Deuterium Arc lamp
Common lamp
electric discharge causes D2 to dissociate and emit UV
radiation (160 nm – 325 nm)
Used for UV spectroscopic studies
1. Sources
33. Types of Lamps Used as Sources
3. Lasers
High power
Narrow line width
Very good for studying reactions
Coherence : Frequency and waveform are identical and
their phase difference is constant
can fine-tune the desired wavelength (but choice of
wavelength is limited)
Too much expensive
Other good sources are: Xe (250 – 1000 nm),
Hg (280 – 1400 nm)
1. Sources
35. They are used for spectral scanning (varying the wavelength of radiation
over a considerable range )
They can be used for UV/Vis region
All monochromators are similar in mechanical construction
All monochromators employ slits, mirrors, lenses, gratings or prisms
2. Wavelength Selectors (Monochromators)
37. i. Absorption Filters
Simplest kind of filter
This type of filters is colored glass filters
Absorbs a broad portion of the spectrum (complementary color) and transmits
other portions (its color)
Used in the visible region
It permits certain bands of wavelength (bandwidth of ~ 50 nm) to pass through
a. Optical / Interference Filters
38. a. Optical / Interference Filters
ii. Interference Filters
39. Disadvantages
They are not very good wavelength selectors and can’t be used in instruments
utilized in research
This is because they allow the passage of a broad bandwidth which gives a
chance for deviations from Beer’s law
They absorb a significant fraction of the desired radiation
a. Optical / Interference Filters
40. b. Diffraction Gratings
The reflection grating is ruled with a series of
closely spaced, parallel grooves with repeated
distance d
The grating is covered with Al to make it
reflective
When polychromatic light is reflected from the
grating, each groove behaves as a new point
source of radiation.
41. b. Diffraction Gratings
Polychromatic radiation from the entrance
slit is collimated (made into beam of
parallel rays) by a concave mirrors
These rays fall on a reflection grating,
whereupon different wavelengths are
reflected at different angles
The orientation of the reflection grating
directs only one narrow band wavelength,
to the exit slit of the monochromator
Rotation of the grating allows different
wavelengths, to pass through the exit slit
42. b. Diffraction Gratings
When adjacent light rays are in phase,
they reinforce one another
(constructive interference)
When adjacent light rays are not in
phase, they partially or completely
canceled one another (destructive
interference)
43. b. Diffraction Gratings
r
Bragg’s Law (Sir W.H. Bragg and his son Sir W.L. Bragg) : “When the x-ray is incident
onto a crystal surface, its angle of incidence, θ, will reflect back with a same angle of
scattering, θ. And, when the path difference, d is equal to a whole number, n, of wavelength,
a constructive interference will occur”.
nλ=2d (sin θi + sin θr)
Where,
• λ is the wavelength of the x-ray,
• d is the spacing of the crystal layers (path difference),
• θi is the incident angle and θr is angle of reflection
• n is an integer
Since incident angle i = Constant;
Therefore, l r
Reflection Grating
i
d
44. b. Prism Monochromators
Dispersion by prism depends on refraction
of light which is wavelength dependent
Violet color with higher energy (shorter
wavelength) are diffracted or bent most
While red light with lower energy (longer
wavelength are diffracted or bent least
As a result, the poly-chromatic white light
is dispersed into its individual colors
45. Advantages and disadvantages of decreasing monochromator slit width
Exit slit determines the width of radiation (bandwidth) emitted from the
Monochromator
A wider slit width gives higher sensitivity because higher radiation intensity
passes to the sample but on the other hand, narrow slit width gives better
resolution for the spectrum
In general, the choice of slit width to use in an experiment must be made by
compromising these factors. Still, we can overcome the problem of low
sensitivity of the small slit by increasing the sensitivity of the detector
46. Glass – visible
Quartz -UV ,visible both
3. Sample Containers (Cuvettes)
Long
pathlength
Short pathlength (b)
1 cm pathlength
cuvette
1 cm 1 cm
Opaque
Face
Transparent
Face
Square Cylindrical Rectangular
47. Convert radiant energy (photons) into an electrical signal
Ideal Detector :-
High sensitivity - A detector should be sensitive
Fast response time- Fast response over a considerable range of wavelengths
High signal/noise
Constant response for λmax
linear response - Electrical signal produced by the detector must be directly
proportional to the transmitted intensity
4. Detectors
49. Phototube emits electrons from a photosensitive, negatively charged cathode
when struck by visible or UV radiation
The electrons flow through vacuum to an anode to produce current which is
proportional to radiation intensity
4. Detectors
a. Phototube
hn
e-
-Ve
Photosensitive cathode
amplifier
anode
50. Single channel, but very high sensitivity
Electrons emitted from the photosensitive cathode alloy (Cs3Sb, K2CsSb,
Na2KSb) strike a second surface called dynode which is positive with respect to
the original cathode
Electrons are thus accelerated and can knock out more than one electrons from
the dynode
4. Detectors
b. Photomultiplier Tube
photochathode
anode
high voltage
voltage divider network
dynodes
light
electrons
e-
51. For 9 stages giving 64 electrons for 1
photon, the amplification is 49 or 2.6 x 105)
The output is fed to an amplifier which
generates a signal
To minimise noise it is necessary to operate
at the lowest possible voltage
4. Detectors
b. Photomultiplier Tube
52. An integrated-circuit chip that contains an array of capacitors that store charge
when light creates e-hole pairs
The charge accumulates and is read in a fixed time interval
CCDs are used in similar applications to other detectors, although the CCD is
much more sensitive for measurement of low light levels
4. Detectors
c. Charge-Coupled Devices (CCD)
53. Single Beam Spectrophotometer : Light beam follows a single path from the
source, to the monochromator, to the sample cell and finally to the detector
Types of Spectrophotometers
Double Beam Spectrophotometer
• P = Intensity of transmitted Light
• P0 = Intensity of Incident Light
54. Single beam spectrophotometer is inconvenient because :
The sample and blank must be placed alternately in the light path
For measurements at multiple wavelengths, the blank must be run at each
wavelength
Advantages of double beam instruments are :
The absorption in the sample is automatically corrected for the absorption
occurring in the blank, since the readout of the instrument is log the difference
between the sample beam and the blank beam
Automatic correction for changes of the source intensity and changes in the
detector response with time or wavelength because the two beams are compared
and measured at the same time
Automatic scanning and continuous recording of spectrum (absorbance versus
wavelength)
Advantages of double beam instruments over single beam instruments
55. Deviations from Beer’s
law appear when :
The absorbing species
undergoes association,
dissociation, hydrogen
bonding, complex formation,
hydrolysis, ionization,
polymerization or reaction
with the solvent to give
products that absorb differently
from the analyte
Deviation From Beer’s Law
1. Chemical Deviations
56. The extent of such deviations can be predicted from the molar absorptivities of
the absorbing species and the equilibrium constants for the equilibria involved
Typical equilibria that give rise to this effect include monomer dimer equilibria,
metal complexation equilibria where more than one complex is present,
acid/base equilibria, and solvent-analyte association equilibria
A common example of this behavior is found with acid/base indicators.
Deviations arising from chemical factors can only be observed when
concentrations are changed
Deviation From Beer’s Law
1. Chemical Deviations
57. Since HA is weak acid it exists in equilibrium with its conjugated base A-
Deviations arising from chemical deviations observed only when concentrations
are changed eg. Phenolphthalein:
Deviation From Beer’s Law
1. Chemical Deviations
l = 600 nm
58. Beer’s law strictly applies only when measurements are made with
monochromatic source of radiation
If the band selected corresponds to a region in which the absorptivity of the
analyte is essentially constant, deviation from Beer’s law will be minimum
To avoid deviation, it is advisable to select a wavelength band near the
wavelength of maximum absorption where the analyte absorptivity changes little
with wavelength
The deviations due to stray light are most significant at high absorbance values
Deviation From Beer’s Law
2. Instrumental Deviations
59. Stray light always causes the apparent absorbance to be lower than the true
absorbance
Because stray radiation levels can be as high as 0.5% in modern instruments,
absorbance levels above 2.0 are rarely measured
Another deviation is caused by mismatched cells (unequal pathlengths and
optical characteristics)
This error can be avoided either by using matched cells or by using a linear
regression procedure to calculate both the slope and intercept of the calibration
curve
Deviation From Beer’s Law
2. Instrumental Deviations
60. Wide applicability to both organic and inorganic systems
High sensitivity of 10-6-10-4 M
Moderate to high selectivity
Good accuracy the relative error encountered in concentration lie in the range
from 1% - 3%
Ease and convenience of data acquisition
The important characteristics of Spectrophotometric methods
61. UV-Vis absorption spectrophotometry is
employed primarily for quantitative
analysis
UV-Vis - Used for identification and
estimation of inorganic, organic and
biomedical species
UV/Vis - More widely used in chemical
and clinical laboratories throughout the
world than any other single method
Important Applications of Spectrometric Methods