Leuco dye

Transformation between leuco and colored form of crystal violet lactone, halochromism.
Transformation between leuco and colored form induced by ultraviolet radiation, photochromism.

A leuco dye (from the Greek leukos: white ) is a dye which can switch between two chemical forms; one of which is colorless. Reversible transformations can be caused by heat, light or pH; resulting in examples of thermochromism, photochromism and halochromism respectively. Irreversible transformation typically involve reduction or oxidation.[1] The colorless form is sometimes referred to as the leuco form.

Leuco dyes form the basis of thermal printer papers and certain pH indicators.

Examples

The most common example is in applying sulfur dyes and vat dyes; with indigo being a classic case. This is characteristically purple but is also completely insoluble in water, meaning that it cannot be applied to clothes directly. It is instead reduced to indigo white (sometimes Leucoindigo), which is water-soluble but colorless. When a submerged fabric is removed from a dyebath of white indigo the dye quickly combines with oxygen in the air and reverts to the insoluble, intensely colored indigo. The reduction step is typically achieved with sodium dithionite, hydroxyacetone and hydrogen, or by electrochemical methods.[2][3]

The spiro form of an oxazine is a colorless leuco dye; the conjugated system of the oxazine and another aromatic part of the molecule is separated by an sp3-hybridized "spiro" carbon. After protonating a part of the molecule, irradiation with UV light (see Photochromism), or introducing other kind of such change, the bond between the spiro carbon and the oxazine interrupts, the ring opens, the spiro carbon achieves sp2 hybridization and becomes planar, the aromatic group rotates, aligns its π-orbitals with the rest of the molecule, and a conjugated system forms, with ability to absorb photons of visible light, and therefore appear colorful.[1]

Another example of a leuco dye is the crystal violet lactone, which in its lactone form is colorless or slightly yellowish, but in low pH, when it is protonated, it becomes intensely violet.[1] Other examples are phenolphthalein and thymolphthalein, colorless in acidic to neutral pH, but becoming pink and blue in alkaline environment. Other example are many redox indicators, which undergo reversible color change between colored and colorless form at a specific electrode potential.

See also

References

  1. 1 2 3 Chemistry and Applications of Leuco Dyes. Ramaiah Muthyala. 302 pag. Springer; 1997 edition. ISBN 978-0306454592
  2. ↑ Božič, Mojca; Kokol, Vanja (2008). "Ecological alternatives to the reduction and oxidation processes in dyeing with vat and sulphur dyes". Dyes and Pigments. 76 (2): 299–309. doi:10.1016/j.dyepig.2006.05.041.
  3. ↑ Roessler, Albert; Jin, Xiunan (December 2003). "State of the art technologies and new electrochemical methods for the reduction of vat dyes". Dyes and Pigments. 59 (3): 223–235. doi:10.1016/S0143-7208(03)00108-6.


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