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Due to strong and extensive hydrogen bonding, it boils near room temperature, a much higher temperature than other hydrogen halides. Hydrogen fluoride is an extremely dangerous gas, forming corrosive and penetrating hydrofluoric acid upon contact with moisture. The gas can also cause blindness by rapid destruction of the corneas.
Solid fluorine carriers", compounds that can release fluorine upon heating, notably cobalt trifluoride, [116] may be used instead, or hydrogen fluoride. After the reaction, the molecular size is not changed significantly, as the elements have very similar van der Waals radii. [114]
In hydrogen fluoride (HF), the hydrogen 1s orbital can mix with fluorine 2p z orbital to form a sigma bond because experimentally the energy of 1s of hydrogen is comparable with 2p of fluorine. The HF electron configuration 1σ 2 2σ 2 3σ 2 1π 4 reflects that the other electrons remain in three lone pairs and that the bond order is 1.
Hydrofluoric acid is a solution of hydrogen fluoride (HF) in water.Solutions of HF are colorless, acidic and highly corrosive.A common concentration is 49% (48-52%) but there are also stronger solutions (e.g. 70%) and pure HF has a boiling point near room temperature.
Elemental fluorine and virtually all fluorine compounds are produced from hydrogen fluoride or its aqueous solution, hydrofluoric acid. Hydrogen fluoride is produced in kilns by the endothermic reaction of fluorite (CaF 2) with sulfuric acid: [169] CaF 2 + H 2 SO 4 → 2 HF(g) + CaSO 4. The gaseous HF can then be absorbed in water or liquefied ...
Hypofluorous acid, chemical formula H O F, is the only known oxyacid of fluorine and the only known oxoacid in which the main atom gains electrons from oxygen to create a negative oxidation state. The oxidation state of the oxygen in this acid (and in the hypofluorite ion OF − and in its salts called hypofluorites) is 0, while its valence is 2.
Organofluorine compounds are pervasive. Many drugs, many polymers, refrigerants, and many inorganic compounds are made from fluoride-containing reagents. Often fluorides are converted to hydrogen fluoride, which is a major reagent and precursor to reagents. Hydrofluoric acid and its anhydrous form, hydrogen fluoride, are particularly important. [4]
This is significantly stronger than the bonds of carbon with other halogens (an average bond energy of e.g. C-Cl bond is around 320 kJ/mol [1]) and is one of the reasons why fluoroorganic compounds have high thermal and chemical stability. The carbon–fluorine bond is relatively short (around 1.4 Å [1]). The Van der Waals radius of the ...