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By Joan Lewis, Lynette Chiles

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2. Molecular Orbital Theory : According to this theory, the excitation of a molecule means the transference of one electron from an orbital of lower energy to that of higher energy. 19 These e1ectrons may be a, 1t or n (non-bonding) e1ectrons. The higher energy states are commonly known as antibonding orbitals. The antibonding orbitals associated with a and 1t bonds are called a* and 1t* orbitals respectively. However, there are no antibonding orbitals associated with n (non-bonding) electrons because they do not form bonds.

6, 6°-Tetra methyl-4-hydroxy azobenzene) cis-isomer (Non-planar, colourless) trans-isomer (Planar. coloured) In case of Mischler's hydrol the 1t-electrons o~cillate behveen the following hvo resonance ",' -, structures, which are planar. (CHJ)2N , -0,. t _ ~6l CH~_ N(CH J )2 (CHl);N-< rCH-{ )-N(CHl)z The compound has blue colour in acetic 'acid solution: If dilute hydrochloric ac'id is -added it gets protonated. Due to the hydroxyl group at the central carbon atom the molecule becomes non-planar.

1 : Absorption spectra of benzene, aniline, nitrobenzene. and p-nitroaniline. tfect. The hypsochrome group diminishes resonance, often by forcing 1t-orbitals out of coplanarity. Changes in the structure of a dye due to which the intensity of absorption increases are said to be hyperchromic. On the other hand, structural changes which decrease the intensity of absorption are termed as hypochromic. 2 Bathochromic, hypsochromic, hypo~romic and hyperchromic etlects are represented by the absorption spectra (Fig.

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