Hydroxyl radical: Difference between revisions

Latest revision as of 04:10, 31 March 2024

The hydroxyl radical, OH, is responsible for the oxidation of most of the compounds that are released into, or formed in, the atmosphere.

It is ubiquitous in the atmosphere, although its mean concentration is about 10⁶cm^-3 and the mixing ratio seldom exceeds 1 ppt (1 part in 10¹²). In the lower atmosphere it is formed by the reaction of excited oxygen atoms O(¹D) with water or by the reaction of hydroperoxyl radicals with nitric oxide. In the stratosphere it is involved in ozone-destroying catalytic cycles. The capacity of the atmosphere to clean itself via the occurrence of oxidation reactions (oxidizing capacity) is usually related to the level of OH present.
Levy, H. 1972. Photochemistry of the lower troposphere. Planet. Space Sci.. 20. 919–935.

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+{{Term
+|Display title=hydroxyl radical
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+|Meaning=The hydroxyl radical, OH, is responsible for the [[oxidation]] of most of the compounds  that are released into, or formed in, the [[atmosphere]].
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+|Explanation=It is ubiquitous in the atmosphere, although its mean concentration is about 10<sup>6</sup>cm<sup>-3</sup> and the  [[mixing ratio]] seldom exceeds 1 ppt (1 part in 10<sup>12</sup>). In the [[lower atmosphere]] it is formed by the  reaction of excited [[oxygen]] atoms O(<sup>1</sup>D) with water or by the reaction of [[hydroperoxyl radicals]]  with [[nitric oxide]]. In the [[stratosphere]] it is involved in ozone-destroying [[catalytic cycles]]. The  capacity of the atmosphere to clean itself via the occurrence of oxidation reactions (oxidizing  capacity) is usually related to the level of OH present.<br/> Levy, H. 1972. Photochemistry of the lower troposphere. Planet. Space Sci.. 20. 919&ndash;935.
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-== hydroxyl radical ==
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-<div class="definition"><div class="short_definition">The hydroxyl radical, OH, is responsible for the [[oxidation]] of most of the compounds  that are released into, or formed in, the [[atmosphere]].</div><br/> <div class="paragraph">It is ubiquitous in the atmosphere, although its mean concentration is about 10<sup>6</sup>cm<sup>&minus;3</sup> and the  [[mixing ratio]] seldom exceeds 1 ppt (1 part in 10<sup>12</sup>). In the [[lower atmosphere]] it is formed by the  reaction of excited [[oxygen]] atoms O(<sup>1</sup>D) with water or by the reaction of [[hydroperoxyl radicals]]  with [[nitric oxide]]. In the [[stratosphere]] it is involved in ozone-destroying [[catalytic cycles]]. The  capacity of the atmosphere to clean itself via the occurrence of oxidation reactions (oxidizing  capacity) is usually related to the level of OH present.</div><br/> </div><div class="reference">Levy, H. 1972. Photochemistry of the lower troposphere. Planet. Space Sci.. 20. 919&ndash;935. </div><br/>
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