Phases of fluorine

Fluorine forms diatomic molecules (F
2) that are gaseous at room temperature with a density about 1.3 times that of air.[1][note 1] Though sometimes described as yellow-green, pure fluorine gas is actually a very pale yellow. The color can only be observed in concentrated fluorine gas when looking down the axis of long tubes, as it appears transparent when observed from the side in normal tubes or if allowed to escape into the atmosphere.[3] The element has a "pungent" characteristic odor that is noticeable in concentrations as low as 20 ppb.[4]

Fluorine condenses to a bright yellow liquid at −188 °C (−307 °F),[5] which is near the condensation temperatures of oxygen and nitrogen.

The solid states of fluorine rely on Van der Waals forces to hold molecules together, which, because of the small size of the fluorine molecules, are relatively weak. Consequently, the solid states of fluorine are more similar to that of oxygen[6][7] or the noble gases than to those of the heavier halogens.

Fluorine solidifies at −220 °C (−363 °F)[5] into a cubic structure, called beta-fluorine. This phase is transparent and soft, with significant disorder of the molecules; its density is 1.70 g/cm3.

At −228 °C (−378 °F) fluorine undergoes a solid–solid phase transition into a monoclinic structure called alpha-fluorine. This phase is opaque and hard, with close-packed layers of molecules, and is denser at 1.97 g/cm3.[9] The solid state phase change requires more energy than the melting point transition and can be violent, shattering samples and blowing out sample holder windows.[10][11]

  1. ^ Jaccaud et al. 2005, p. 2.
  2. ^ Shelquist, Richard (2010). "An introduction to air density and density altitude calculations". Shelquist Engineering. Retrieved 29 April 2011.
  3. ^ Burdon, Emson & Edwards 1987, p. 471.
  4. ^ Lide 2004, p. 4.12.
  5. ^ a b Dean 1999, p. 523.
  6. ^ Jordan, Streib & Lipscomb 1964, p. 760.
  7. ^ Jordan et al. 1964.
  8. ^ Jordan, Streib & Lipscomb 1964, Fig. 1
  9. ^ Meyer, Barrett & Greer 1969.
  10. ^ Young 1975, p. 10
  11. ^ Barrett, Meyer & Wasserman 1967.


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