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Silver chlorite

Names
IUPAC name Silver chlorite
Other names Silver(I) chlorite
Identifiers
CAS Number	7783-91-7
3D model (JSmol)	Interactive image
ChemSpider	8031311
PubChem CID	9855611
InChI InChI=1S/Ag.ClHO2/c;2-1-3/h;(H,2,3)/q+1;/p-1
SMILES Cl=O.
Properties
Chemical formula	AgClO2
Molar mass	175.32 g/mol
Appearance	Slightly yellow solid
Melting point	156 °C (313 °F; 429 K) (decomposes)
Solubility in water	0.45 g/100ml
Refractive index (nD)	2.1
Structure
Crystal structure	Orthorhombic
Space group	Pcca
Lattice constant	a = 6.075 Å, b = 6.689 Å, c = 6.123 Å
Thermochemistry
Heat capacity (C)	20.81 cal/deg
Std molar entropy (S298)	32.16 cal/deg
Std enthalpy of formation (ΔfH298)	0.0 kcal/mol
Hazards
GHS labelling:
Pictograms
Related compounds
Other anions	Silver chlorate Silver perchlorate Silver hypochlorite
Other cations	Sodium chlorite
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). Infobox references

Silver chlorite is a chemical compound with the formula AgClO₂. This slightly yellow solid is shock sensitive and has an orthorhombic crystal structure.

Preparation

Silver chlorite is prepared by the reaction of silver nitrate and sodium chlorite:

AgNO₃ + NaClO₂ → AgClO₂ + NaNO₃

Reactions and properties

If normally heated, it explodes violently at 105 °C:

AgClO₂ → AgCl + O₂

If heated very carefully, it decomposes at 156 °C to form silver chloride. It can also decompose to silver chlorate is chlorous acid is present.

Silver chlorite reacts explosively with various substances such as sulfur and hydrochloric acid, forming silver chloride. It also gets reduced by sulfur dioxide, and reacts with sulfuric acid to form chlorine dioxide. This compound explodes in contact with iodomethane and iodoethane.

Silver chlorite complexes

Silver chlorite can react with anhydrous ammonia to form triammonia-silver chlorite:

AgClO₂ + 3NH₃ → 3NH₃·AgClO₂

References

1. ^ A. G. Massey; N. R. Thompson; B. F. G. Johnson (2016). The Chemistry of Copper, Silver and Gold (Ebook). Pergamon International Library of Science, Technology, Engineering and Social Studies: Elsevier Science. p. 108. ISBN 9781483181691.
2. ^ F. Solymosi (1968). "The Thermal Stability and Some Physical Properties of Silver Chlorite, Chlorate and Perchlorate*". Zeitschrift für Physikalische Chemie. 57 (1). Oldenbourg Wissenschaftsverlag: 1–18. doi:10.1524/zpch.1968.57.1_2.001. S2CID 102195060.
3. M. Okuda; M. Ishihara; M. Yamanaka; S. Ohba; Y. Saito (1990). "Structures of lead chlorite, magnesium chlorite hexahydrate and silver chlorite". Acta Crystallogr. 46 (10): 1755–1759. Bibcode:1990AcCrC..46.1755O. doi:10.1107/S010827019000066X.
4. ^ Wendell V. Smith; Kenneth S. Pitzer; Wendell M. Latimer (1937). "Silver Chlorite: Its Heat Capacity from 15 to 300K., Free Energy and Heat of Solution and Entropy. The Entropy of Chlorite Ion". J. Am. Chem. Soc. 59 (12): 2640–2642. doi:10.1021/ja01291a046.
5. J. Cooper; R. E. Marsh (1961). "On the structure of AgClO₂". Acta Crystallogr. 14 (2): 202–203. Bibcode:1961AcCry..14..202C. doi:10.1107/S0365110X61000693.
6. ^ Joseph William Mellor (1922). Supplement to Mellor's Comprehensive Treatise on Inorganic and Theoretical Chemistry: suppl. 3. K, Rb, Cs, Fr. University of Illinois at Urbana-Champaign: Longmans, Green and Company. p. 284.
7. Urben, Peter, ed. (2013). Bretherick's Handbook of Reactive Chemical Hazards. Elsevier Science. p. 4. ISBN 9780080523408.

• Silver compounds
• Chlorites