Benzophenone is a naturally occurring organic compound with the formula (C6H5)2CO, generally abbreviated Ph2CO. Benzophenone has been found in some fungi, fruits and plants, including grapes.[4] It is a white solid with a low melting point and rose-like odor[5] that is soluble in organic solvents. Benzophenone is the simplest diaromatic ketone. It is a widely used building block in organic chemistry, being the parent diarylketone.
Benzophenone can be used as a photo initiatorinultraviolet (UV)-curing applications[6] such as inks, imaging, and clear coatings in the printing industry. Benzophenone prevents UV light from damaging scents and colors in products such as perfumes and soaps.
Benzophenone can also be added to plastic packaging as a UV blocker to prevent photo-degradation of the packaging polymers or its contents. Its use allows manufacturers to package the product in clear glass or plastic (such as a PETE water bottle).[7] Without it, opaque or dark packaging would be required.
In biological applications, benzophenones have been used extensively as photophysical probes to identify and map peptide–protein interactions.[8]
Benzophenone is used as an additive in flavorings or perfumes for "sweet-woody-geranium-like notes."[9]
Addition of a solution of benzophenone in THF to a vial containing THF, sodium metal, and a stir bar, yielding the deep blue benzophenone anion radical. Playback speed 4x original recording. Notice that the stirbar is not Teflon-coated, which would be attacked by the ketyl.A solvent pot containing dibutyl ether solution of sodium benzophenone ketyl, which gives it its purple color.
Alkali metals reduce benzophenone to the deeply blue colored radical anion, diphenylketyl:[15]
M + Ph2CO → M+Ph2CO•−
Generally sodium is used as the alkali metal. Sodium-benzophenone ketyl is used in the purification of organic solvents, particularly ethers, because it reacts with water and oxygen to give non-volatile products.[16][17] Adsorbents such as alumina, silica gel, and especially molecular sieves are superior and far safer.[18] The sodium-benzophenone method is common since it gives a visual indication that water, oxygen, and peroxides are absent from the solvent. Large scale purification may be more economical using devices which utilize adsorbents such as the aforementioned alumina or molecular sieves.[19] The ketyl is soluble in the organic solvent being dried, which leads to faster purification. In comparison, sodium is insoluble, and its heterogeneous reaction is much slower. When excess alkali metal is present a second reduction may occur, resulting in a color transformation from deep blue to purple:[15]
M + M+Ph2CO•− → (M+)2(Ph2CO)2−
Commercially significant derivatives and analogues[edit]
There are over 300 natural benzophenones, with great structural diversity and biological activities. They are being investigated as potential sources of new drugs. [20]Substituted benzophenones such as oxybenzone and dioxybenzone are used in many sunscreens. The use of benzophenone-derivatives which structurally resemble a strong photosensitizer has been criticized (see sunscreen controversy).
It is considered "essentially nontoxic."[10] Benzophenone is however banned as a food additive by the US Food and Drug Administration, despite the FDA's continuing stance that this chemical does not pose a risk to public health under the conditions of its intended use.[22][23] Benzophenone derivatives are known to be pharmacologically active. From a molecular chemistry point of view interaction of benzophenone with B-DNA has been demonstrated experimentally.[24] The interaction with DNA and the successive photo-induced energy transfer is at the base of the benzophenone activity as a DNA photosensitizer and may explain part of its therapeutic potentialities.
In 2014, benzophenones were named Contact Allergen of the Year by the American Contact Dermatitis Society.[25]
^Dornan, L.; Muldoon, M. (2015). "A highly efficient palladium(II)/polyoxometalate catalyst system for aerobic oxidation of alcohols". Catalysis Science & Technology. 5 (3): 1428–1432. doi:10.1039/c4cy01632g.
^Lee, C. C. (1953). "The Mechanism of the Ketonic Pyrolysis of Calcium Carboxylates". The Journal of Organic Chemistry. 18 (9): 1079–1086. doi:10.1021/jo50015a003.
^ abConnelly, Neil; Geiger, William (March 28, 1996). "Chemical Redox Agents for Organometallic Chemistry". Chemical Reviews. 96 (2): 877–910. doi:10.1021/cr940053x. PMID11848774.
^Armarego, W. L. F.; Chai, C. (2003). Purification of laboratory chemicals. Oxford: Butterworth-Heinemann. ISBN978-0-7506-7571-0.
^Williams, D. B. G.; Lawton, M. (2010). "Drying of Organic Solvents: Quantitative Evaluation of the Efficiency of Several Desiccants". The Journal of Organic Chemistry. 75 (24): 8351–4. doi:10.1021/jo101589h. PMID20945830. S2CID17801540.
