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[ClO 4] −. [6] It is a red fuming liquid under standard conditions. Chloryl compounds are best prepared by the reaction of FClO 2 with a strong Lewis acid. For example: [5] FClO 2 + AsF 5 → [ClO 2][AsF 6] Other synthesis routes are also possible, including: [5] 5 ClO 2 + 3 AsF 5 → 2 [ClO 2][AsF 6] + AsF 3 O + 4 Cl 2 Cl 2 O 6 + 2 SbF 5 → ...
Chlorine monoxide is a chemical radical with the chemical formula ClO •. It plays an important role in the process of ozone depletion. In the stratosphere, chlorine atoms react with ozone molecules to form chlorine monoxide and oxygen. Cl • + O 3 → ClO • + O 2. This reaction causes the depletion of the ozone layer. [1]
Dichlorine monoxide is highly soluble in water, [6] where it exists in an equilibrium with HOCl. The rate of hydrolysis is slow enough to allow the extraction of Cl 2 O with organic solvents such as CCl 4, [3] but the equilibrium constant ultimately favours the formation of hypochlorous acid. [7]
In the same year that Brønsted and Lowry published their theory, G. N. Lewis created an alternative theory of acid–base reactions. The Lewis theory is based on electronic structure. A Lewis base is a compound that can give an electron pair to a Lewis acid, a compound that can accept an electron pair.
A simple Lewis model also does not account for the phenomenon of aromaticity. For instance, Lewis structures do not offer an explanation for why cyclic C 6 H 6 (benzene) experiences special stabilization beyond normal delocalization effects, while C 4 H 4 (cyclobutadiene) actually experiences a special destabilization.
ClO − 3 + 3 H 2 O + 6 e ... As perchlorate is a weak Lewis base (i.e., ... stating that it had taken "proactive steps" with state and local governments to address ...
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The hydroxyl radical, Lewis structure shown, contains one unpaired electron. Lewis dot structure of a Hydroxide ion compared to a hydroxyl radical. In chemistry, a radical, also known as a free radical, is an atom, molecule, or ion that has at least one unpaired valence electron.