Chlorate is an anion-containing chemical compound; chlorates are also chloric acid salts. Almost any combustible element (sugar, sawdust, charcoal, organic solvents, metals, etc.) will quickly ignite chlorate salt combinations. Chlorates were originally often used in pyrotechnics; however, their use has been declined due to their instability. The majority of pyrotechnic applications that previously employed chlorates have transitioned to perchlorates, which are more stable. In this article, we will explore a little more about chlorate and its chemical formula in detail.

Chlorate Chemical Formula

The formula for chlorate anion is \({\rm{ClO}}_3^ – \).

In this anion, the chlorine atom is in the \(+5\) oxidation state. When we use a Roman number in parenthesis with chlorates, such as chlorate(V), we are referring to a specific chlorine oxyanion.

Chlorates should be stored away from organics and easily oxidizable materials because they are strong oxidizers.

Structure and Bonding of Chlorate

Chlorate has a chemical formula \({\rm{ClO}}_3^ – \).

As all of the \({\rm{Cl – O}}\) bonds have the same bond length (\(1.49\,\mathop {\rm{A}}\limits^{\rm{o}} \) in potassium chlorate), we cannot adequately represent it by a single Lewis structure. Furthermore, the chlorine atom is hypervalent. Instead, it is frequently regarded as a hybrid structure of multiple resonance structures.

Chlorate anions have trigonal pyramidal structures, as predicted by valence shell electron pair repulsion theory. Chlorates have a molar mass of \(83.45\;{\rm{g}}/{\rm{mol}}\).

Preparation of Chlorate

The various preparation methods of chlorate are explained below

Laboratory Preparation of Chlorate

Metal chlorates are made by adding chlorine to hot  and concentrated metal hydroxides such as \({\rm{KOH}}\):

\(3{\rm{C}}{{\rm{l}}_2} + 6{\rm{KOH}} \to 5{\rm{KCl}} + {\rm{KCl}}{{\rm{O}}_3} + 3{{\rm{H}}_2}{\rm{O}}\)

Chlorine undergoes disproportionation (reduction as well as oxidation) in this reaction. Chlorine has oxidation number zero and produces chloride \({\rm{C}}{{\rm{l}}^ – }\) (oxidation number \(-1\)) and chlorate(V) \({\rm{ClO}}_3^ – \) (oxidation number \(+5\)). When cold aqueous metal hydroxides react with chlorine, they produce chloride and hypochlorite (oxidation number \(+1\)).

Industrial Preparation of Chlorate

Sodium chlorate is synthesised on a large scale using an aqueous sodium chloride solution (brine). If the electrolysis equipment allows for the mixing of chlorine and sodium hydroxide, the disproportionation reaction occurs. The electrical power used for electrolysis heats the reactants to \(50 – {70^ \circ }{\rm{C}}\).

Occurrence of Chlorate

According to a recent study, natural chlorate deposits can be found all over the world, with relatively high concentrations found in arid and hyper-arid regions.

The chlorate content of rainfall samples was also measured, with the amount of chlorate being comparable to that of perchlorate. It is thought that chlorate and perchlorate share a common natural formation mechanism and may be involved in the chlorine biogeochemistry cycle. The presence of natural chlorate could also explain why a wide range of microorganisms is capable of reducing chlorate to chloride.

Furthermore, the evolution of chlorate reduction may be an ancient phenomenon because all perchlorate reducing bacteria described so far use chlorate as a terminal electron acceptor. It should be stated unequivocally that no chlorate-dominant minerals are known at this time. This means that the chlorate anion exists only as a substitution in known mineral species or, eventually, in pore-filling solutions.

Chlorates Oxyanions

If the word “chlorate” is followed by a Roman numeral in brackets, it means the oxyanion contains chlorine in the indicated oxidation state, namely:

By this definition, “chlorate” refers to any chlorine oxyanion. The term “chlorate” is commonly used to refer to chlorine oxyanion in the \(+5\) oxidation state.

Compounds of Chlorates

Examples of chlorates include sodium chlorate, potassium chlorate and magnesium chlorate.

Sodium Chlorate

Sodium chlorate has a chemical formula \({\rm{NaCl}}{{\rm{O}}_3}\) and is an inorganic compound. It is a white crystalline powder that dissolves easily in water. It has a high hygroscopicity. It decomposes at temperatures above \({300^ \circ }{\rm{C}}\), releasing oxygen and leaving sodium chloride behind. Several hundred million tonnes of sodium chlorate are produced each year, primarily for use in bleaching pulp to produce high-brightness paper.

Uses of Sodium Chlorate

1. The main commercial application for sodium chlorate is the production of chlorine dioxide \(\left( {{\rm{Cl}}{{\rm{O}}_2}} \right)\).
2. All perchlorate compounds are manufactured industrially by oxidation of sodium chlorate solutions in electrolysis.
3. It is used in chemical oxygen generators, such as those in commercial aircraft.
4. It’s a non-selective herbicide. It is considered phytotoxic to all parts of green plants. It can also cause death through root absorption.
5. Sodium chlorate can be combined with sucrose sugar to create a highly explosive fuel that burns in airtight spaces, similar to gunpowder.

Potassium Chlorate

Potassium chlorate is a compound with a molecular formula \({\rm{KCl}}{{\rm{O}}_3}\) that contains potassium, chlorine, and oxygen. It is a white crystalline substance in its purest form. It is the second most common chlorate in industrial use, after sodium chlorate. It is a strong oxidising agent and its main application is in safety matches.

Uses of Pottasium Chlorate

1. To prepare oxygen,
2. As a disinfectant,
3. In explosives and fireworks, and
4. In cultivation, forcing the longan tree’s blossoming stage, causing it to produce fruit in warmer climates.

Magnesium Chlorate

Magnesium chlorate is an inorganic compound composed of a magnesium cation and two chlorate anions, with the chemical formula \({\rm{Mg}}{\left( {{\rm{Cl}}{{\rm{O}}_3}} \right)_2}\). It is a white crystalline solid and has a molar mass of \(191.20\;{\rm{g}}/{\rm{mol}}\).

Uses of Magnesium Chlorate

Magnesium(II) chlorate is a highly effective desiccant and a defoliant for cotton, potato, and rice crops. It is also used as an inactive ingredient in eye drops as a lubricant.

Summary

The formula for chlorate anion is \({\rm{ClO}}_3^ – \). Since Chlorates are strong oxidizers, they should be kept away from organics and easily oxidisable materials. They have pyramidal trigonal structures. We also studied some examples and uses of chlorates like- sodium chlorate, potassium chlorate and magnesium chlorate.

FAQs on Chlorate Formula

Q.1. What is the formula of potassium chlorate?
Ans: The molecular formula of potassium chlorate is \({\rm{KCl}}{{\rm{O}}_3}\).

Q.2. What is the formula of ammonium chlorate?
Ans: The molecular formula of ammonium chlorate \({\rm{N}}{{\rm{H}}_4}{\rm{Cl}}{{\rm{O}}_3}\).

Q.3. What is the formula for chlorate?
Ans: The formula for chlorate anion is \({\rm{ClO}}_3^ – \).

Q.4. How can chlorates be prepared?
Ans: In the laboratory, metal chlorates are made by adding chlorine to hot-concentrated metal hydroxides such as \({\rm{KOH}}\):
\(3{\rm{C}}{{\rm{l}}_2} + 6{\rm{KOH}} \to 5{\rm{KCl}} + {\rm{KCl}}{{\rm{O}}_3} + 3{{\rm{H}}_2}{\rm{O}}\)
Chlorine undergoes disproportionation, reduction, and oxidation in this reaction. Chlorine has oxidation number zero and produces chloride \({\rm{C}}{{\rm{l}}^ – }\) (oxidation number \(-1\)) and chlorate(V) \({\rm{ClO}}_3^ – \) (oxidation number \(+5\)). When cold aqueous metal hydroxides react with chlorine, they produce chloride and hypochlorite (oxidation number \(+1\)).

Q.5. What is the charge on chlorate ions?
Ans: The overall charge of chlorate ion is \(-1\).

Q.6. What is chlorate used for?
Ans: Chlorate is a pesticide as well as an explosive. The use of hypochlorite and chlorine dioxide as disinfectants is by far the most common source in drinking water.

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