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Chlorine pentafluoride is an interhalogen compound with formula ClF 5. This colourless gas is a strong oxidant that was once a candidate oxidizer for rockets. The molecule adopts a square pyramidal structure with C 4v symmetry, [1] as confirmed by its high-resolution 19 F NMR spectrum. [2] It was first synthesized in 1963. [3]
Unlike other hydrohalic acids, such as hydrochloric acid, hydrogen fluoride is only a weak acid in water solution, with acid dissociation constant (pK a) equal to 3.19. [36] HF's weakness as an aqueous acid is paradoxical considering how polar the HF bond is, much more so than the bond in HCl, HBr, or HI. The explanation for the behavior is ...
[1] [2] [3] Introduced by Gilbert N. Lewis in his 1916 article The Atom and the Molecule, a Lewis structure can be drawn for any covalently bonded molecule, as well as coordination compounds. [4] Lewis structures extend the concept of the electron dot diagram by adding lines between atoms to represent shared pairs in a chemical bond.
Chloryl fluoride is the chemical compound with the formula ClO 2 F. It is commonly encountered as side-product in reactions of chlorine fluorides with oxygen sources. [1] It is the acyl fluoride of chloric acid.
Chlorine monofluoride: Chlorine trifluoride: Chlorine pentafluoride: Molar mass: 54.45 g/mol 92.45 g/mol 130.45 g/mol CAS number: Melting point: −155.6 °C −76.3 °C −103 °C Boiling point: −100 °C 11.8 °C −13.1 °C Standard enthalpy of formation Δ f H° gas: −50.29 kJ/mol −158.87 kJ/mol −238.49 kJ/mol
Hypervalent iodine compounds are useful reagents in organic chemistry (e.g. Dess–Martin periodinane) Tetra-, penta- and hexavalent phosphorus, silicon, and sulfur compounds (e.g. PCl 5, PF 5, SF 6, sulfuranes and persulfuranes) Noble gas compounds (ex. xenon tetrafluoride, XeF 4) Halogen polyfluorides (ex. chlorine pentafluoride, ClF 5)
Phosphorus pentafluoride is a relatively inert gas, notable as a mild Lewis acid and a fluoride ion acceptor. It is a fluxional molecule in which the axial (ax) and equatorial (eq) fluorine atoms interchange positions by the Berry pseudorotation mechanism .
All have the sodium chloride (rock salt) structure and are soluble in water and even some alcohols. [1] Because the fluoride anion is highly basic, many alkali metal fluorides form bifluorides with the formula MHF 2. Sodium and potassium bifluorides are significant to the chemical industry. [2]