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The bond energy of difluorine is much lower than that of either Cl 2 or Br 2 and similar to the easily cleaved peroxide bond; this, along with high electronegativity, accounts for fluorine's easy dissociation, high reactivity, and strong bonds to non-fluorine atoms.

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Unreactive substances like powdered steel, glass fragments, and asbestos fibers react quickly with cold fluorine gas; wood and water spontaneously combust under a fluorine jet. Spheres indicate F 2 molecules that may assume any angle.

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Other molecules are constrained to planes. Main article: Phases of fluorine Animation showing the crystal structure of beta-fluorine.

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Molecules on the faces of the unit cell have rotations constrained to a plane. At room temperature, fluorine is a gas of diatomic molecules[4] pale yellow when pure sometimes described as yellow-green. Other radioisotopes have half-lives less than 70 seconds; most decay in less than half a second.]

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