Monosodium xenate
One sodium cation and one xenate anion
One sodium cation and one xenate anion
Ball-and-stick model of the component ions
Ball-and-stick model of the component ions
Properties
NaHXeO4
Molar mass 219.29 g/mol
Properties
Appearance White solid
Soluble, decomposes in water[1]
Solubility insoluble chloroform, methanol, ethanol, and carbon tetrachloride[1]
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 extremely unstable, vigorous oxidizer
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 4: Very short exposure could cause death or major residual injury. E.g. VX gasFlammability 0: Will not burn. E.g. waterInstability 4: Readily capable of detonation or explosive decomposition at normal temperatures and pressures. E.g. nitroglycerinSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
4
0
4
OX
Flash point Non-Flammable
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Monosodium xenate is the sodium salt of xenic acid with formula NaHXeO4. It is a powerful oxidizer, owing to being a highly reactive compound of xenon.[2]

Synthesis

Monosodium xenate can be made by mixing solutions of xenon trioxide and sodium hydroxide, followed by freezing to liquid nitrogen temperatures, and dehydrating in a vacuum.[1]

Properties

Monosodium xenate usually exists in the sesquihydrate form, with 1.5 waters of hydration per unit molecule. It is stable up to 160 °C heated in a pure state. However it can explode when subjected to mechanical shock, or lower temperatures when mixed with XeO3.[1] Sodium xenate is slightly toxic with a medium lethal dose between 15 and 30 mg/kg of body weight in mice. Xenate leaves the body very quickly. In mice, the level in blood drops by half in twenty seconds due to it being decomposed and exhaled. In the peritoneum the half-life extends to six minutes.[3]

The dialkali xenates XeO42- have not been discovered, as xenate disproportionates in more alkaline conditions, hence it being rare to the find the dialkaline salt Na2XeO4.[1]


References

  1. ^ a b c d e Spittler, T. M.; Jaselskis, Bruno (August 1965). "Preparation and Properties of Monoalkali Xenates". Journal of the American Chemical Society. 87 (15): 3357–3360. doi:10.1021/ja01093a013.
  2. ^ Peterson, Jeffrey L.; Claassen, Howard H.; Appelman, Evan H. (March 1970). "Vibrational spectra and structures of xenate(VI) and perxenate(VIII) ions in aqueous solution". Inorganic Chemistry. 9 (3): 619–621. doi:10.1021/ic50085a037.
  3. ^ Finkel, A. J.; Miller, C. E.; Katz, J. J. (April 1968). "Metabolic and Toxicological Effects of Water-Soluble Xenon Compounds Are Studied" (PDF). Atomic Energy Commission USA.
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