Magnesium chlorate

Names
IUPAC name

Magnesium dichlorate hexahydrate

Systematic IUPAC name

Magnesium dichlorate

Other names

* Magnesium(II) chlorate

Identifiers

CAS Number

* 10326-21-3
* (dihydrate): 36355-97-2
* (hexahydrate): 7791-19-7

3D model (JSmol)

* Interactive image
* (dihydrate): Interactive image
* (hexahydrate): Interactive image

ChemSpider |

* 64853748
* (dihydrate): 80564724
* (hexahydrate): 128878

EC Number |

* 233-711-1

PubChem CID

* 25155
* (dihydrate): 71437298
* (hexahydrate): 146100

UNII |

* M536P01U3N

UN number | 2723

CompTox Dashboard (EPA)

* (hexahydrate): DTXSID30999110

InChI

* InChI=1S/2ClHO3.Mg/c2*2-1(3)4;/h2*(H,2,3,4);/q;;+2/p-2

Key: NNNSKJSUQWKSAM-UHFFFAOYSA-L

* (dihydrate): InChI=1S/2ClHO3.Mg.2H2O/c2*2-1(3)4;;;/h2*(H,2,3,4);;2*1H2/q;;+2;;/p-2

Key: YTXOASNCVSJHNM-UHFFFAOYSA-L

* (hexahydrate): InChI=1S/2ClHO3.Mg.6H2O/c2*2-1(3)4;;;;;;;/h2*(H,2,3,4);;6*1H2/q;;+2;;;;;;/p-2

Key: XKPLAISKKLSAQQ-UHFFFAOYSA-L

SMILES

* Cl(=O)(=O)[O-].Cl(=O)(=O)[O-].[Mg+2]

* (dihydrate): O.O.[Mg+2].[O-]Cl(=O)=O.[O-]Cl(=O)=O

* (hexahydrate): O.O.O.O.O.O.[O-]Cl(=O)=O.[O-]Cl(=O)=O.[Mg+2]

Properties

Chemical formula

| Mg(ClO3)2
Molar mass | 191.20 g/mol
Appearance  | White crystalline solid
Density | 1.747 g/cm3 (hexahydrate)[1]
Melting point |  35 °C (95 °F; 308 K)[2]
Boiling point |  120 °C (248 °F; 393 K)[2] (decomposition)

Solubility in water

| 114 g/100 ml (0 °C)
123 g/100 ml (10 °C)
135 g/100 ml (20 °C)
155 g/100 ml (30 °C)
178 g/100 ml (50 °C)
242 g/100 ml (60 °C)
268 g/100 ml (100 °C)[2]
Solubility in acetone  | Soluble
Structure[1]

Crystal structure

| Monoclinic

Space group

| P21/c

Lattice constant

a = 6.39 Å, b = 6.51 Å, c = 13.90 Å

α = 90°, β = 100.3°, γ = 90°

Lattice volume (V)

| 590.1 Å3
Hazards
GHS pictograms |
GHS Signal word | Warning

GHS hazard statements

| H302, H332
Lethal dose or concentration (LD, LC):

LD50 (median dose)

| 6348 mg/kg (rat, oral)
Related compounds

Other cations

| Calcium chlorate
Strontium chlorate
Barium chlorate

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Infobox references

Magnesium chlorate refers to inorganic compounds with the chemical formula Mg(ClO3)2(H2O)x. The anhydrous (x = 0), dihydrate (x = 2), and hexahydrate (x = 6) are known. These are thermally labile white solids. The hexahydrate has been identified on the Martian surface.[3]

## Contents

* 1 Production
* 2 Properties
* 3 Uses
* 4 Hazards
* 5 References

## Production

Samples of magnesium chlorate were first claimed in 1920 as the result of treating magnesium oxide with chlorine. A more modern method involves electrolysis of magnesium chloride.[4] The magnesium chlorate can be purified by exploiting its solubility in acetone.[4]

A more simple method of production is the reaction of barium chlorate and magnesium sulfate:

Ba(ClO3)2 \+ MgSO4 → BaSO4↓ + Mg(ClO3)2

The precipitated barium sulfate is filtered to yield a solution of magnesium chlorate, which when evaporated, yields crystals of the hexahydrate.[1]

## Properties

The hexahydrate Mg(ClO3)2·6H2O decomposes to the tetrahydrate at 35 °C. At 65 °C, it dehydrates to the dihydrate, then at 80 °C forms a basic salt. If further heated to 120 °C it decomposes to water, oxygen, chlorine, and magnesium oxide.[2]

As confirmed by X-ray crystallography, the di- and hexahydrates feature octahedral Mg2+ centers. The other ligands are water, exclusively in the hexahydrate. In the dihydrate, chlorate is also coordinated and functions as a bridging ligand.[1]

## Uses

Magnesium(II) chlorate is used as a powerful desiccant and a defoliant for cotton, potato, and rice. It is also found as a lubricant in eye drops as an inactive ingredient.[5]

## Hazards

Magnesium chlorate is an oxidizer and can in principle form explosive mixtures.

## References

1. ↑ 1.0 1.1 1.2 1.3 Kossev, K; Tsvetanova, L.; Dimowa, L.; Nikolova, R.; Shivachev, B. (2013). "Synthesis and Crystal Structure of Magnesium Chlorate Dihydrate and Magnesium Chlorate Hexahydrate". Bulgarian Chemical Communications 45: 543–548.
2. ↑ 2.0 2.1 2.2 2.3 Joseph William Mellor (1922). Supplement to Mellor's Comprehensive Treatise on Inorganic and Theoretical Chemistry: suppl. 3. K, Rb, Cs, Fr. Longmans, Green and Company.
3. ↑ Ojha, Lujendra; Wilhelm, Mary Beth; Murchie, Scott L.; McEwen, Alfred S.; Wray, James J.; Hanley, Jennifer; Massé, Marion; Chojnacki, Matt (2015). "Spectral evidence for hydrated salts in recurring slope lineae on Mars". Nature Geoscience 8 (11): 829–832. doi:10.1038/ngeo2546. Bibcode: 2015NatGe...8..829O.
4. ↑ 4.0 4.1 Herbert Maxim (1948) (in English). The electrolytic production of magnesium chlorate and perchlorate. the Department of Chemical Engineering: University of Southern California.
5. ↑ "MAGNESIUM CHLORATE" (in English). U.S. Department of Health & Human Services. https://drugs.ncats.io/substance/M536P01U3N#general.

* v
* t
* e

Magnesium compounds

* MgB2
* MgBr2
* MgCO3
* MgC2O4
* MgC6H6O7
* MgC14H10O4
* MgCl2
* Mg(ClO4)2
* MgF2
* MgH2
* Mg(HCO3)2
* MgI2
* Mg(NO3)2
* MgO
* MgO2
* Mg(OH)2
* MgPo
* MgS
* MgSO3
* MgSO4
* MgU2O7
* Mg2Al3
* Mg2Si
* Mg2SiO4
* Mg2Si3O8
* Mg3N2
* Mg3(PO4)2
* Mg2(CrO4)2

Template:Chlorates

0.00

(0 votes)

Original source: https://en.wikipedia.org/wiki/Magnesium chlorate. Read more

|

Retrieved from "https://handwiki.org/wiki/index.php?title=Chemistry:Magnesium_chlorate&oldid=4032972"
*[CID]: Compound ID
*[EPA]: U.S. Environmental Protection Agency
*[H302]: Harmful if swallowed
*[H332]: Harmful if inhaled
*[v]: View this template
*[t]: Discuss this template
*[e]: Edit this template