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  2. Chloryl - Wikipedia

    en.wikipedia.org/wiki/Chloryl

    The ClO + 2 cation is isoelectronic with SO 2, [3] and has a bent structure with a bond angle close to 120°. The Cl–O bond is of bond order 1.5, with its Lewis structure consisting of a double bond and a dative bond which does not utilize d-orbitals. [4] The red color of ClO + 2 is caused by electron transitions into an antibonding orbital.

  3. Lewis structure - Wikipedia

    en.wikipedia.org/wiki/Lewis_structure

    Lewis structure of a water molecule. Lewis structures – also called Lewis dot formulas, Lewis dot structures, electron dot structures, or Lewis electron dot structures (LEDs) – are diagrams that show the bonding between atoms of a molecule, as well as the lone pairs of electrons that may exist in the molecule.

  4. Dichlorine monoxide - Wikipedia

    en.wikipedia.org/wiki/Dichlorine_monoxide

    The structure of dichlorine monoxide is similar to that of water and hypochlorous acid, with the molecule adopting a bent molecular geometry (due to the lone pairs on the oxygen atom) and resulting in C 2V molecular symmetry. The bond angle is slightly larger than normal, likely due to steric repulsion between the bulky chlorine atoms.

  5. Chlorine oxide - Wikipedia

    en.wikipedia.org/wiki/Chlorine_oxide

    dichlorine hexoxide or chloryl perchlorate, Cl 2 O 6 or [ClO 2] + [ClO 4] −, chlorine (V,VII) oxide; dichlorine heptoxide, Cl 2 O 7, chlorine (VII) oxide; dichlorine octoxide, chlorine (VII) oxide peroxide or dimer of chlorine tetroxide radical, Cl 2 O 8 or (OClO 3) 2; Several ions are also chlorine oxides: chloryl, ClO + 2; perchloryl, ClO ...

  6. Hypochlorite - Wikipedia

    en.wikipedia.org/wiki/Hypochlorite

    2 ClO − → 2 Cl − + O 2 3 ClO − → 2 Cl − + ClO − 3. This reaction is exothermic and in the case of concentrated hypochlorites, such as LiOCl and Ca(OCl) 2, can lead to dangerous thermal runaway and is potentially explosive. [5] The alkali metal hypochlorites decrease in stability down the group.

  7. Dichlorine hexoxide - Wikipedia

    en.wikipedia.org/wiki/Dichlorine_hexoxide

    It reacts with gold to produce the chloryl salt [ClO 2] + [Au(ClO 4) 4] −: [7] 2Au + 6Cl 2 O 6 → 2 [ClO 2] + [Au(ClO 4) 4] − + Cl 2. Several other transition metal perchlorate complexes are prepared using dichlorine hexoxide. Nevertheless, it can also react as a source of the ClO 3 radical: [citation needed] 2 AsF 5 + Cl 2 O 6 → 2 ClO 3 ...

  8. Chlorate - Wikipedia

    en.wikipedia.org/wiki/Chlorate

    Other oxyanions of chlorine can be named "chlorate" followed by a Roman numeral in parentheses denoting the oxidation state of chlorine: e.g., the ClO − 4 ion commonly called perchlorate can also be called chlorate(VII). As predicted by valence shell electron pair repulsion theory, chlorate anions have trigonal pyramidal structures.

  9. Radical (chemistry) - Wikipedia

    en.wikipedia.org/wiki/Radical_(chemistry)

    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.