Chemistry:Silver chlorate
From HandWiki
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| Names | |
|---|---|
| IUPAC name
Silver(I) chlorate
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| Systematic IUPAC name
Silver(I) chlorate(V) | |
| Other names
Argentous chlorate[1]
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| EC Number |
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PubChem CID
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| UNII | |
| UN number | 1479 |
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| Properties[5] | |
| AgClO3 | |
| Molar mass | 191.32 g·mol−1 |
| Appearance | white crystals |
| Density |
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| Melting point | 230 °C (446 °F; 503 K)[2] |
| Boiling point | 270 °C (518 °F; 543 K)[2] (decomposes) |
| 17.6 g/100 g | |
| Solubility in alcohols | soluble |
| Band gap | |
| Structure (cubic)[3] | |
| Cubic [198] | |
| P213 | |
| 23 | |
a = 6.63 Å, b = 6.63 Å, c = 6.63 Å α = 90°, β = 90°, γ = 90°
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Lattice volume (V)
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291.06 Å3 |
Formula units (Z)
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4 |
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| Structure (tetragonal)[4] | |
| Tetragonal [87] | |
| I4/m | |
| 4/m | |
a = 8.67 Å, b = 8.67 Å, c = 8.17 Å α = 90°, β = 90°, γ = 90°
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Lattice volume (V)
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614.13 Å3 |
Formula units (Z)
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8 |
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| Thermochemistry[5] | |
Std molar
entropy (S |
142.0 J.mol-1.K-1 |
Std enthalpy of
formation (ΔfH⦵298) |
−30.3 kJ⋅mol−1 |
Gibbs free energy (ΔfG˚)
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64.5 kJ⋅mol−1 |
| Hazards | |
| GHS pictograms |  
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| GHS Signal word | Danger |
| H272, H315, H319, H335 | |
| P210, P220, P221, P261, P264, P271, P280, P302+352, P304+340+312Script error: No such module "Preview warning".Category:GHS errors, P305+351+338, P332+313, P337+313, P362, P370+378, P403+233, P405, P501 | |
| NFPA 704 (fire diamond) | |
Threshold limit value (TLV)
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0.01 mg/m3[1] (TWA) |
| NIOSH (US health exposure limits):[1] | |
PEL (Permissible)
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0.01 mg/m3 |
REL (Recommended)
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0.01 mg/m3 (TWA) |
| Related compounds | |
Other anions
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Other cations
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Related compounds
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is   ?)
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| Infobox references | |
Silver chlorate is an inorganic compound with molecular formula AgClO
3. It exists in two forms: white tetragonal prisms, and cubic crystals.[2][7] Like all chlorates, it is water-soluble and an oxidizing agent. It is light-sensitive, so it must be stored in tightly closed dark-coloured containers.[8]
Production
Silver chlorate is produced by the reaction of silver nitrate with sodium chlorate to produce both silver chlorate and sodium nitrate:[8]
- AgNO
3 + NaClO
3 → AgClO
3 + NaNO
3
Alternatively, it may be produced by the bubbling of chlorine gas through a suspension of silver oxide (Ag
2O), or by dissolving Ag
2O or metallic silver in chloric acid.[2]
Structure
AgClO
3 normally exists as tetragonal crystals which undergo a transition to a cubic phase at 139 °C (282 °F).[7]
Safety
Aside from the potential dangers associated with strong oxidizers, silver chlorate may cause argyria, eye irritation, skin irritation, and temporary respiratory issues.[9]
It also has the potential to detonate when heated very rapidly, or from mechanical shock.[1] If exposed to ammonia it may form the explosive complex triamminesilver chlorate (AgClO
3 · 3NH
3).[2]
References
- ↑ 1.0 1.1 1.2 1.3 1.4 Sigma-Aldrich Co., Silver chlorate. Retrieved on 28 July 2025.
- ↑ 2.0 2.1 2.2 2.3 2.4 2.5 Fedoroff, Basil T.; Sheffield, Oliver E.; Clift, George D.; Reese, Earl F. (1 January 1962). "C - Chlorates - Silver Chlorate". Encyclopedia of Explosives and Related Items: Vol 2 (B (Explosif) through Chloric acid). Picatinny Arsenal, NJ: Army Armament Research Development and Engineering Center: Warheads, Energetics, and Combat Support Armaments Research Center. p. C197. AD0422747, PATR 2700. https://apps.dtic.mil/sti/pdfs/AD0422747.pdf#page=608. Retrieved 28 July 2025.
- ↑ 3.0 3.1 "Materials Data on AgClO3 (cubic)". Lawrence Berkeley National Laboratory (LBNL), Berkeley, CA: LBNL Materials Project. 2020-05-02. doi:10.17188/1303485. https://next-gen.materialsproject.org/materials/mp-775761.
- ↑ 4.0 4.1 "Materials Data on AgClO3 (tetragonal)". Lawrence Berkeley National Laboratory (LBNL), Berkeley, CA: LBNL Materials Project. 2020-07-18. doi:10.17188/1202095. https://next-gen.materialsproject.org/materials/mp-27941.
- ↑ 5.0 5.1 Template:RubberBible97th
- ↑ "SDS - Silver chlorate". Elkton, MD: Colonial Metals. 3 July 2017. p. 5. https://www.colonialmetals.com/wp-content/uploads/2016/12/9023-Silver-Chlorate.pdf.
- ↑ 7.0 7.1 Deshpande, Vilas; Suryanarayana, S V; Frantz, C (December 1982). "Tetragonal to cubic phase transition in silver chlorate" (pdf). Bulletin of Materials Science 4 (5): 563–568. doi:10.1007/BF02824963. https://www.ias.ac.in/article/fulltext/boms/004/05/0563-0568.
- ↑ 8.0 8.1 Glemser, O.; Sauer, H. (1965). "19. Copper, Silver, Gold". in Brauer, Georg. Handbook of Preparative Inorganic Chemistry v2 (2nd ed.). New York, USA: Academic Press. p. 1037. ISBN 0-323-16129-4. https://archive.org/details/Handbook_of_Preparative_Inorganic_Chemistry_1_2_Brauer/page/n1083/mode/1up. Retrieved 28 July 2025.
- ↑ "SDS: Silver Chlorate". Sigma-Aldrich. p. 8. https://www.sigmaaldrich.com/US/en/sds/aldrich/227900?userType=anonymous. "May cause argyria (a slate-gray or bluish discoloration of the skin and deep tissues due to the deposit of insoluble albuminate of silver)., To the best of our knowledge, the chemical, physical, and toxicological properties have not been thoroughly investigated."
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