This is a very common question that occurs in everybodies mind. The answer to which is explained by the presence of a substance called Chromophore in the dyes. By definition dyes are basically aromatic compounds. Their structures have aryl rings that has delocalised electron systems. These structures are said to be responsible for the absorption of electromagnetic radiation that has varying wavelengths, based upon the energy of the electron clouds.
It is actually because of this reason that chromophores do not make dyes coloured. Rather it makes the dyes proficient in their ability to absorb radiation. Chromophores acts by making energy changes in the delocalised electron cloud of the dye. This alteration invariably results in the compound absorbing radiation within the visible range of colours and not outside it. Human eyes detects this absorption, and responds to the colours.
Another possibility is that if the electrons are removed from the electron cloud, it may result in loss of colour. Removing electrons may cause the rest of the electrons to revert to the local orbits. A very good example is the Schiff's reagent. As sulphurous acid reacts with pararosanilin, what happens is that a sulphonic group attaches itself to the compound's central carbon atom. This hampers the conjugated double bond system of the quinoid ring, and causes the electrons to become localised. As a consequence the ring ceases to be a chromophore. As a result, the dye becomes colourless.
To conclude chromophores are the atomic configurations which has delocalised electrons. Generally they are represented as carbon, nitrogen, oxygen and sulphur. They can have alternate single and double bonds.
It is actually because of this reason that chromophores do not make dyes coloured. Rather it makes the dyes proficient in their ability to absorb radiation. Chromophores acts by making energy changes in the delocalised electron cloud of the dye. This alteration invariably results in the compound absorbing radiation within the visible range of colours and not outside it. Human eyes detects this absorption, and responds to the colours.
Another possibility is that if the electrons are removed from the electron cloud, it may result in loss of colour. Removing electrons may cause the rest of the electrons to revert to the local orbits. A very good example is the Schiff's reagent. As sulphurous acid reacts with pararosanilin, what happens is that a sulphonic group attaches itself to the compound's central carbon atom. This hampers the conjugated double bond system of the quinoid ring, and causes the electrons to become localised. As a consequence the ring ceases to be a chromophore. As a result, the dye becomes colourless.
To conclude chromophores are the atomic configurations which has delocalised electrons. Generally they are represented as carbon, nitrogen, oxygen and sulphur. They can have alternate single and double bonds.
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