Platinum tetrafluoride

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Platinum tetrafluoride
Names
IUPAC name
Platinum(IV) fluoride
Other names
Platinum tetrafluoride
Platinous fluoride
Identifiers
3D model (
JSmol
)
  • InChI=1S/4FH.Pt/h4*1H;/q;;;;+4/p-4
    Key: VFKKSKGQZDULMV-UHFFFAOYSA-J
  • F[Pt](F)(F)F
Properties
F4Pt
Molar mass 271.078[1]
Appearance red-orange solid[1]
Density 7.08 g/cm3 (calc.)[2]
Melting point 600 °C (1,112 °F; 873 K)[1]
+455.0·10−6 cm3/mol
Structure
Orthorhombic, oF40
Fdd2, No. 43[2]
a = 0.9284 nm, b = 0.959 nm, c = 0.5712 nm
Related compounds
Other anions
 Platinum(IV) bromide
Platinum(IV) chloride
Related compounds
Platinum(VI) fluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Platinum tetrafluoride is the

octahedral coordination geometry.[2]

Preparation

The compound was first reported by

fluorination of platinum metal in the presence of hydrogen fluoride.[3] A modern synthesis involves thermal decomposition of platinum hexafluoride.[4]

Properties

Platinum tetrafluoride vapour at 298.15 K consists of individual molecules. The enthalpy of sublimation is 210 kJmol−1.[5] Original analysis of powdered PtF4 suggested a tetrahedral molecular geometry, but later analysis by several methods identified it as octahedral, with four of the six fluorines on each platinum bridging to adjacent platinum centres.[6]

Reactions

A solution of platinum tetrafluoride in water is coloured reddish brown, but it rapidly decomposes, releasing heat and forming an orange coloured

platinum dioxide hydrate precipitate and fluoroplatinic acid.[7]
When heated to a red hot temperature, platinum tetrafluoride decomposes to platinum metal and fluorine gas. When heated in contact with glass, silicon tetrafluoride gas is produced along with the metal.[7]

Platinum tetrafluoride can form adducts with selenium tetrafluoride and bromine trifluoride.[7] Volatile crystalline adducts are also formed in combination with BF3, PF3, BCl3, and PCl3.[7]

Related compounds

The fluoroplatinates are salts containing the PtF62− ion. Fluoroplatinic acid H2PtF6 forms yellow crystals that absorb water from the air. Ammonium, sodium, magnesium, calcium, strontium, and rare earth including lanthanum fluoropalatinate salts are soluble in water.[7] Potassium, rubidium, caesium, and barium salts are insoluble in water.[7]

References

  1. ^
    ISBN 1-4398-5511-0
    .
  2. ^
    doi:10.1002/chin.199245006.[full citation needed
    ]
  3. ^ Moissan, H. "Platinum tetrafluoride". Comptes Rendus Hebdomadaires des Séances de l'Académie des Sciences. 109: 807–9.
  4. doi:10.1016/S0022-1139(00)81471-2
    .
  5. doi:10.1016/0021-9614(88)90125-5
    .
  6. ISBN 9780080578767
    .
  7. ^ a b c d e f Derek Harry Lohmann (October 1961). The fluorides of platinum and related compounds (Thesis). University of British Columbia.
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