Chlorite

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Chlorite

This discusses some chlorine compounds. Chlorite is also a type of mineral; see chlorite group
Chlorite group

The chlorites are a group of Silicate minerals minerals. Chlorites can be described by the following four Solid solution based on their chemistry via substitution of the following four elements in the silicate lattice; Mg, Fe, Ni, and Mn....
.

The chlorite ion

Ion

An ion is an atom or molecule which has lost or gained one or more electrons, giving it a positive or negative electrical charge. According to the Bohr_model this will be from or in the outer shield 'n'....
is ClO₂^-. A chlorite (compound) is a compound that contains this group, with chlorine

Chlorine

Chlorine...
in oxidation state

Oxidation state

In chemistry, the oxidation state is an indicator of the degree of oxidation of an atom in a chemical compound. The formal oxidation state is the hypothetical Electrical charge that an atom would have if all bonds to atoms of different elements were 100% Ionic bond....
+3. Chlorites are also known as salt

Salt

A salt, in chemistry, is defined as the product formed from the neutralisation reaction of acids and base . Salts are ionic compounds composed of cations and anions so that the product is electrically electric charge ....
s of chlorous acid

Chlorous acid

Chlorous acid is a chemical compound with the formula HClO2. It is a weak acid. Chlorine possesses oxidation state +3 in this acid. The pure substance is unstable, disproportionating to hypochlorous acid and chloric acid ....
.

rine can assume oxidation states of -1, +1, +3, +5, or +7 within the corresponding anions Cl^-, ClO^-, ClO₂^-, ClO₃^-, or ClO₄^-, known commonly and respectively as chloride, hypochlorite, chlorite, chlorate, and perchlorate.

free acid, chlorous acid, HClO₂, is only stable at low concentrations.

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Oxidation states

Chlorine can assume oxidation states of -1, +1, +3, +5, or +7 within the corresponding anions Cl^-, ClO^-, ClO₂^-, ClO₃^-, or ClO₄^-, known commonly and respectively as chloride, hypochlorite, chlorite, chlorate, and perchlorate.

oxidation state	-1	+1	+3	+5	+7
anion named	chloride Chloride The chloride ion is formed when the chemical element chlorine picks up one electron to form an anion Cl−....	hypochlorite Hypochlorite The hypochlorite ion is ChlorineOxygen-. A hypochlorite compound is a chemical compound containing this group, with chlorine in oxidation state +1....	chlorite	chlorate Chlorate The chlorate anion has the formula ClO3-. In this case, the chlorine atom is in the +5 oxidation state. "Chlorate" can also refer to chemical compounds containing this anion; Chlorate#Compounds are the salt s of chloric acid....	perchlorate Perchlorate Perchlorates are the salt derived from perchloric acid . They occur both naturally and through manufacturing. They have been used as a medicine for more than 50 years to treat thyroid gland disorders....
formula	Cl^-	ClO^-	ClO₂^-	ClO₃^-	ClO₄^-
structure

Some chlorite compounds

sodium chlorite
Sodium chlorite

Sodium chlorite is a chemical compound used in the manufacture of paper....
, NaClO₂
magnesium chlorite, Mg(ClO₂)₂

Manufacture

The free acid, chlorous acid, HClO₂, is only stable at low concentrations. Since it cannot be concentrated, it is not a commercial product. However, the corresponding sodium salt, sodium chlorite

Sodium chlorite

Sodium chlorite is a chemical compound used in the manufacture of paper....
, NaClO₂ is stable and inexpensive enough to be commercially available. The corresponding salts of heavy metals (Ag⁺, Hg⁺, Tl⁺, Pb²⁺, and also Cu²⁺ and NH₄⁺) decompose explosively with heat or shock.

Sodium chlorite is derived indirectly from sodium chlorate

Sodium chlorate

Sodium chlorate is a chemical compound with the chemical formula . When pure, it is a white crystalline powder that is readily soluble in water....
, NaClO₃. First, the explosively unstable gas chlorine dioxide

Chlorine dioxide

Chlorine dioxide is a chemical compound with the formula ClO2. This reddish-yellow gas crystallizes as orange crystals at -59 ?C. As one of several oxides of chlorine, it is a potent and useful oxidizing agent used in water treatment and in bleaching....
, ClO₂ is produced by reducing sodium chlorate in a strong acid solution with a suitable reducing agent (for example, sodium chloride, sulfur dioxide, or hydrochloric acid).

H₂SO₄(aq) + NaClO₃(s) ? NaHSO₄(aq) + HClO₃(aq)
HClO₃(aq) ? 2ClO₂(g) + HClO₄(aq) + H₂O(l)

(Other routes for the preparation of chlorine dioxide

Chlorine dioxide

Hydrogen peroxide

Hydrogen peroxide is a very pale blue liquid which appears colorless in a dilute solution, slightly more viscous than water. It is a weak acid....
, H₂O₂ yielding sodium chlorite

Sodium chlorite

Sodium chlorite is a chemical compound used in the manufacture of paper....
(NaClO₂). (Sodium, Na⁺, spectator ions are not shown in the following equations).

2ClO₂(g) + 2OH^- ? ClO₂^-(aq) + ClO₃^-(aq) + H₂O(l)
ClO₃^-(aq) + H₂O₂(l) ? ClO₂^-(aq) + H₂O(l) + O₂(g)

Usage

The main application of sodium chlorite

Sodium chlorite

Sodium chlorite is a chemical compound used in the manufacture of paper....
is the generation of chlorine dioxide for bleaching and stripping of textiles, pulp, and paper. It is also used for disinfection in a few municipal water treatment plants after conversion to chlorine dioxide

Chlorine dioxide

Chlorine dioxide is a chemical compound with the formula ClO2. This reddish-yellow gas crystallizes as orange crystals at -59 ?C. As one of several oxides of chlorine, it is a potent and useful oxidizing agent used in water treatment and in bleaching....
. An advantage in this application, as compared to the more commonly used chlorine, is that trihalomethanes are not produced from organic contaminants. Sodium chlorite

Sodium chlorite

Sodium chlorite is a chemical compound used in the manufacture of paper....
, NaClO₂ also finds application as a component of contact lens cleaning solution under the trade name purite.

Sodium chlorite, like many oxidizers, should be protected from inadvertent contamination by organic materials to avoid the formation of an explosive mixture.