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Tungsten(VI) fluoride, also known as tungsten hexafluoride, is an inorganic compound with the formula W F 6. It is a toxic, corrosive, colorless gas, with a density of about 13 kg/m 3 (22 lb/cu yd) (roughly 11 times heavier than air). [2] [3] It is the densest known gas under standard ambient temperature and pressure (298 K, 1 atm). [4]
Tungsten tetrafluoride is an inorganic compound with the formula WF 4. This little studied solid has been invoked, together with tungsten pentafluoride , as an intermediate in the chemical vapor deposition of tungsten films using tungsten hexafluoride .
Tungsten fluoride may refer to: Tungsten tetrafluoride (tungsten(IV) fluoride) Tungsten pentafluoride (tungsten(V) fluoride) Tungsten hexafluoride (tungsten(VI) fluoride)
Covalent and ionic bonding form a continuum, with ionic character increasing with increasing difference in the electronegativity of the participating atoms. Covalent bonding corresponds to sharing of a pair of electrons between two atoms of essentially equal electronegativity (for example, C–C and C–H bonds in aliphatic hydrocarbons).
Tungsten(V) fluoride is an inorganic compound with the formula WF 5. It is a hygroscopic yellow solid. It is a hygroscopic yellow solid. Like most pentafluorides, it adopts a tetrameric structure, consisting of [WF 5 ] 4 molecules.
The reaction of tungsten(VI) oxytetrachloride and hydrogen fluoride will also produce WOF 4. [3] WOCl 4 + 4HF → WOF 4 + 4HCl. WOF 4 can also prepared by the reaction of lead(II) fluoride and tungsten trioxide at 700 °C. [3] 2PbF 2 + WO 3 → WOF 4 + 2PbO. Tungsten(VI) oxytetrafluoride hydrolyzes into tungstic acid. [1] [9] WOF 4 + 2 H 2 O ...
In 1941 Van Arkel recognised three extreme materials and associated bonding types. Using 36 main group elements, such as metals, metalloids and non-metals, he placed ionic, metallic and covalent bonds on the corners of an equilateral triangle, as well as suggested intermediate species.
The 3-center 4-electron (3c–4e) bond is a model used to explain bonding in certain hypervalent molecules such as tetratomic and hexatomic interhalogen compounds, sulfur tetrafluoride, the xenon fluorides, and the bifluoride ion.