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Structure. The shape of the molecule is a distorted tetrahedron with the O-Se-O angle being 126.2°, the O-Se-F angle being 108.0° and F-Se-F being 94.1°. [3]
Seleninyl fluoride can be produced by the reaction of selenium oxychloride and potassium fluoride. [3]2 KF + SeOCl 2 → 2 KCl + SeOF 2. It can also be produced by the reaction of selenium tetrafluoride with water or selenium dioxide.
Lewis structure of a water molecule. Lewis structures – also called Lewis dot formulas, Lewis dot structures, electron dot structures, or Lewis electron dot structures (LEDs) – are diagrams that show the bonding between atoms of a molecule, as well as the lone pairs of electrons that may exist in the molecule.
Selenium tetrafluoride (Se F 4) is an inorganic compound.It is a colourless liquid that reacts readily with water. It can be used as a fluorinating reagent in organic syntheses (fluorination of alcohols, carboxylic acids or carbonyl compounds) and has advantages over sulfur tetrafluoride in that milder conditions can be employed and it is a liquid rather than a gas.
Although selenium hexafluoride is quite inert and slow to hydrolyze, it is toxic even at low concentrations, [9] especially by longer exposure. In the U.S., OSHA and ACGIH standards for selenium hexafluoride exposure is an upper limit of 0.05 ppm in air averaged over an eight-hour work shift.
Selenium dioxide. Selenium compounds are compounds containing the element selenium (Se). Among these compounds, selenium has various oxidation states, the most common ones being −2, +4, and +6.
The monomeric form adopts a bent structure very similar to that of sulfur dioxide with a bond length of 161 pm. [6] The dimeric form has been isolated in a low temperature argon matrix and vibrational spectra indicate that it has a centrosymmetric chair form. [5] Dissolution of SeO 2 in selenium oxydichloride give the trimer [Se(O)O] 3. [6]
The number of electron pairs in the valence shell of a central atom is determined after drawing the Lewis structure of the molecule, and expanding it to show all bonding groups and lone pairs of electrons. [1]: 410–417 In VSEPR theory, a double bond or triple bond is treated as a single bonding group. [1]