Section B 2 UV-visible (electronic) spectroscopy Flashcards
• Typical chromophores include :
conjugated polyunsaturated systems : -C=C-C=C- etc : carotene
polyaromatic systems : chlorophyll
systems containing C=O, C=S, C-P species etc
molecules containing transition metal ions (Fe3+, Co2+ etc) :
e.g. haemoglobin
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Important things to determine :
- Number and position(s) of the peaks: quoted in tables as λmax values : (but also as 1/λ in cm-1 units)
- Relative peak intensities - this helps work out what kind of electronic transitions are involved.
- Absolute peak intensities - you can do this by measuring the Absorbance values for several concentrations
of a samples and using the Beer-Lambert law to determine the characteristic ε for the electronic transition - All this information can be used to help identify the molecule and the electronic transitions involved. It gives
useful structural information - including the extent of polyunsaturated; aromatic systems, the presence of O,
N, S, P etc, or if a transition metal ion is present, its coordination geometry, oxidation state etc - Can also be used for quantitative or quantitative analysis - important in forensics, biomedicine etc : is a
given compound present ? How much of it is present ?
• The energy jump is related to the frequency and wavelength of light absorbed by Planck’s
relation : ΔE = h ν = hc / λ%
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• The UV-vis absorptions are due to electronic transitions between these orbital energy levels
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• Transitions between σ , π, π, σ, n levels give rise
to characteristic UV-vis spectra in organic
molecules
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ππ* transitions usually lie in the UV range (200-300
nm) for “simple” organic molecules
πσ* transitions usually lie at too high energy (ΔE = hν =
hc/λ) to be observable in laboratory UV-vis spectra
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ethylene (C2H4)
λmax = 163 nm
π - π* transition
• The π and π* orbitals interact along the =C-C=C- chain ….
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• The π - π* transition shifts to longer wavelength as the chain length increases (red shift)
usually by ~30 nm per additional C=C bond unit (start from ethylene : λmax = 163 nm)
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e.g., β-carotene : C40H56 : 11 conjugated -C-C=C- bonds : strong absorption in blue-green range (480 - 510 nm) :
gives rise to yellow-red colour component : present in carrots, butter, egg yolks, green leaves and vegetables :
precursor to vitamin A in liver (C20H30O : present in animal fats, egg yolk, fish oils) : necessary for growth and weight
gain ; resistance to infection; night vision
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carotene -
absorb blue-green (400-500 nm)
benzene
π - π* for benzene : λmax = 203 nm
Substituents : -CH3, -Cl, -NO2, -OH, -CO2H etc change this value between 203 - 295 nm
Polycyclic aromatic systems : anthracene, phenanthene etc : move λmax to longer
wavelength (π - π* at lower energy)
This peak is the π-π* transition for
C6H6 :
“spikes” on this peak are due to
vibrational transitions occurring along with
the electronic transition
Chlorophyll -
is a polyunsaturated/aromatic ring system containing -C=C- and -C=N- bonds. Used to
capture sunlight and initiate photosynthesis process. The electronic absorptions at 400-450 (blueviolet)
nm and 600-700 nm (red) result in the green-yellow colour reflected from plant leaves
λmax = 428 nm
(blue-violet)
λmax = 660 nm
(red)
Quantitative Spectroscopy - the Beer-Lambert Law
Absorbance A = (log10 Io/It) = ε . c. L
concentration c: moles per litre (moles dm-3)
ε is the molar absorptivity (extinction coefficient) : units L mol-1 cm-1
• If ε is known for a compound, we can use the Beer-Lambert law relation to determine concentrations.
• For unknown compounds, we can determine ε by graphing measured absorbance vs known concentration.
• The value of ε determined for a compound can then be used to determine the type of transition involved -
e.g., σ-π, π-π* transition etc : this helps us work out the electronic structure and bonding
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- If there is no observable UV-vis spectrum, there are : (a) no multiple bonds ; aromatics ; O, N, S
containing groups; transition metal ions. We are likely dealing with fully saturated hydrocarbons.
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