Krypton difluoride structureĪ liner KrF 2 has a similar structure to that of XeF 2 with the Kr-F bond distance of 189 pm. A mixture of KrF 2 and XeF 2 fluorinated many trivalent lanthanide compounds like LnF 4, LnF 7 − 3, and LnOF 2, where Ln = Ce, Pr, Nd, Tb, and Dy. KrF 2 uses a fluorinating agent that fluorinates xenon or noble metals like silver and gold. The chemical compound KrF 2 is less stable than XeF 2 and dissociated into Kr and F 2 at room temperature. It is also formed by the action of OF 2 on Kr in presence of sunlight. ![]() The rare gas compound, KrF 2 may be prepared by passing an electric discharge through a mixture of krypton and fluorine molecules at low pressure in a U-tube immersed with liquid oxygen. ![]() The only known unstable halide compound is krypton difluoride (KrF 2). The clathrates or cage compounds are formed mainly with water and para-quinol by trapping krypton molecules in the hydrogen bonding network. But it formed a few unstable chemical compounds with fluorine along with clathrates or cage compounds. The chemistry of krypton or other noble gases like helium, neon, and argon is different from other elements of the periodic table due to their filled valence shell configuration and high ionization energy.
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