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Properties of substance:

xenon difluoride

Group of substances:

inorganic

Physical appearance:

colorless tetragonal crystals

Empirical formula (Hill's system for organic substances):

F2Xe

Structural formula as text:

XeF2

Molar/atomic mass: 169.3

Melting point (°C):

129.03

Boiling point (°C):

155

Decomposition temperature (°C):

600

Solubility (g/100 g of solvent):

acetonitrile: 21.5 (0°C) [Ref.]
acetonitrile: 41 (21°C) [Ref.]
ammonia liquid : insoluble [Ref.]
bromine pentafluoride: 189.6 (20°C) [Ref.]
bromine trifluoride: soluble [Ref.]
chlorine pentafluoride: insoluble [Ref.]
dimethylsulfoxide: soluble [Ref.]
hydrogen fluoride : 108 (-2°C) [Ref.]
hydrogen fluoride : 167.3 (30°C) [Ref.]
iodine pentafluoride: 153.8 [Ref.]
molybdenum hexafluoride : sparingly soluble [Ref.]
nitrogen(III) fluoride oxide - hydrogen fluoride: 1085 (16.8°C) [Ref.]
pyridine: soluble [Ref.]
sulfur dioxide: soluble [Ref.]
tungsten(VI) fluoride: sparingly soluble [Ref.]
water: 2.5 (0°C) [Ref.]

Interatomic distances and bond angles:

Interatomic distances (in pm): 198 (Xe-F)

Density:

4.32 (25°C, g/cm3)

Reactions of synthesis:

  1. [Ref.1]
    Xe + F2 → XeF2
  2. [Ref.1]
    2CF3OF + Xe → XeF2 + CF3OOCF3

Reactions:

  1. Yeild 4%. [Ref.1]
    NaBrO3 + XeF2 + H2O → NaBrO4 + Xe + 2HF
  2. [Ref.1]
    2KrF2 + AuF5 → Kr2F3[AuF6]

Vapour pressure (Torr):

3.8 (25°C)
318 (100°C)

Electrode potential:

XeF2 + 2H+ + 2e- → Xe + 2HF, E = 2.64 V (water, 25°C)

Standard molar enthalpy (heat) of formation ΔfH0 (298.15 K, kJ/mol):

-176 (s)

Molar enthalpy (heat) of fusion ΔfusH (kJ/mol):

16.8

ΔHsublimation (kJ/mol):

50.6

Standard molar entropy S0 (298.15 K, J/(mol·K)):

259.403 (g)

Molar heat capacity at constant pressure Cp (298.15 K, J/(mol·K)):

54.108 (g)

Standard molar enthalpy (heat) of formation ΔfH (298 K, kJ/mol)

-107.03 (g) [Ref.]
-162.76 (s) [Ref.]

Standard molar Gibbs energy of formation ΔfG (298 K, kJ/mol)

-73.39 (g) [Ref.]
-86.11 (s) [Ref.]

Critical temperature (°C):

358

Critical pressure (MPa):

9.3

Critical density (g/cm3):

1.14

References:

  1. CRC Handbook of Chemistry and Physics. - 95ed. - CRC Press, 2014. - pp. 4-98
  2. Holleman A.F., Wiberg E., Wiberg N. Lehrbuch der Anorganischen Chemie. - Berlin: Walter de Gruyter, 1995. - pp. 422-424
  3. Progress in inorganic chemistry. - Vol. 29. - John Wiley & Sons, 1982. - pp. 192-198
  4. Reedijk J., Poeppelmeier K. Comprehensive Inorganic Chemistry II. - Vol. 1. - Elsevier, 2013. - pp. 814-817
  5. Карапетьянц М.Х., Дракин С.И. Общая и неорганическая химия. - М.: Химия, 1981. - pp. 490 [Russian]
  6. Лидин Р.А., Аликберова Л.Ю., Логинова Г.П. Неорганическая химия в вопросах. - М.: Химия, 1991. - pp. 224-225 [Russian]
  7. Некрасов Б.В. Основы общей химии. - Т.1. - М.: Химия, 1973. - pp. 243-244 [Russian]
  8. Рабинович В.А., Хавин З.Я. Краткий химический справочник. - Л.: Химия, 1977. - pp. 75 [Russian]
  9. Спицын В.И., Мартыненко Л.И. Неорганическая химия. - Ч.1. - М.: ИМУ, 1991. - pp. 227-228 [Russian]
  10. Успехи химии. - 1965. - Т.34, №6. - pp. 970-974 [Russian]
  11. Успехи химии. - 1974. - Т.43, №12. - pp. 2148-2154, 2167 [Russian]
  12. Успехи химии. - 2001. - Т.70, №3. - pp. 262-298 [Russian]
  13. Химическая энциклопедия. - Т. 2. - М.: Советская энциклопедия, 1990. - pp. 549 [Russian]

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    © Collected Ruslan Anatolievich Kiper, burewestnik@mail.ru