Give Basic Theory of UV Spectroscopy. #Spectroscopy #Organic Chemistry
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U.V. spectroscopy is based on the electronic excitation of molecules. The absorptions from the ultraviolet regions supply energy which is sufficient to raise an electron form one energy level to a higher one.
According to the molecular orbital approach the absorbed energy of light is used to transfer an electron from a bonding or non-bonding molecular orbital to an anti-bonding molecular orbital.
For example in acetone all single bonds are sigma bond, while double bond is pi bond and lone pairs of electrons with oxygen which don’t take part in bonding are non bonding electrons.
Now, the electron thus transferred may be a sigma (𝛔) bond electron or a pi (𝛑) bond electron or it may be an electron of a lone-pair (n).i.e. a non-bonding pair.
The possible electronic transitions (→) that are involved in ultraviolet and visible region are:
𝛔 → 𝛔*
𝛔 → 𝛑*
𝛑 → 𝛔*
𝛑 → 𝛑*
n → 𝛔*
n → 𝛑*
A 𝛑 → 𝛑* transition occurs with a compound containing double bond and an n → 𝛑* transition occurs with a compound containing heteroatom, e.g. Thus increasing amounts of energy are required to raise n, 𝛑 and 𝛔 electrons from their bonding to the corresponding anti-bonding molecular orbitals. In fact, 𝛔 electrons are held very tightly and hence the energy required for 𝛔 → 𝛔* transition is so much that it requires absorption of wavelengths from the far ultraviolet region.
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U.V. spectroscopy is based on the electronic excitation of molecules. The absorptions from the ultraviolet regions supply energy which is sufficient to raise an electron form one energy level to a higher one.
According to the molecular orbital approach the absorbed energy of light is used to transfer an electron from a bonding or non-bonding molecular orbital to an anti-bonding molecular orbital.
For example in acetone all single bonds are sigma bond, while double bond is pi bond and lone pairs of electrons with oxygen which don’t take part in bonding are non bonding electrons.
Now, the electron thus transferred may be a sigma (𝛔) bond electron or a pi (𝛑) bond electron or it may be an electron of a lone-pair (n).i.e. a non-bonding pair.
The possible electronic transitions (→) that are involved in ultraviolet and visible region are:
𝛔 → 𝛔*
𝛔 → 𝛑*
𝛑 → 𝛔*
𝛑 → 𝛑*
n → 𝛔*
n → 𝛑*
A 𝛑 → 𝛑* transition occurs with a compound containing double bond and an n → 𝛑* transition occurs with a compound containing heteroatom, e.g. Thus increasing amounts of energy are required to raise n, 𝛑 and 𝛔 electrons from their bonding to the corresponding anti-bonding molecular orbitals. In fact, 𝛔 electrons are held very tightly and hence the energy required for 𝛔 → 𝛔* transition is so much that it requires absorption of wavelengths from the far ultraviolet region.
Ask a question at http://bit.ly/2GrIMbs
Answer a question at http://bit.ly/2V26gM5
Other Subjects:
Adult Education @ http://bit.ly/2KFPK0s
Analytical Chemistry @ http://bit.ly/2Gq24Ok
Applied Physics @ http://bit.ly/2Xh4S64
Engineering Drawing @ http://bit.ly/2IHro43
English @ http://bit.ly/2V8FSk4
Environmental Studies @ http://bit.ly/2UGKlLa
General Medicine @ http://bit.ly/2Gtn8Uh
Mathematics @ http://bit.ly/2UEZVqH
Organic Chemistry @ http://bit.ly/2GkXvTY
Physical Chemistry @ http://bit.ly/2v5EQX5
Soft Skills @ http://bit.ly/2Zf6wa3
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