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Chlorine trifluoride is an interhalogen compound with the formula ClF 3.It is a colorless, poisonous, corrosive, and extremely reactive gas that condenses to a pale-greenish yellow liquid, the form in which it is most often sold (pressurized at room temperature).
ClF ClF 3 ClF 5; Systematic name: Chlorine monofluoride: Chlorine trifluoride: Chlorine pentafluoride: Molar mass: 54.45 g/mol 92.45 g/mol 130.45 g/mol CAS number
Structure of chlorine trifluoride, an example of a compound with T-shaped coordination geometry.. In chemistry, T-shaped molecular geometry describes the structures of some molecules where a central atom has three ligands.
When comparing a polar and nonpolar molecule with similar molar masses, the polar molecule in general has a higher boiling point, because the dipole–dipole interaction between polar molecules results in stronger intermolecular attractions. One common form of polar interaction is the hydrogen bond, which is also
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]
Trifluoromethyl group covalently bonded to an R group. The trifluoromethyl group is a functional group that has the formula-CF 3.The naming of is group is derived from the methyl group (which has the formula -CH 3), by replacing each hydrogen atom by a fluorine atom.
This electronic structure has an electric dipole, hence the name polar bond. In reality, the atoms carry partial charges; the more electronegative atom of the two involved in the bond will usually carry a partial negative charge. One exception to this is carbon monoxide. In this case, the carbon atom carries the partial negative charge although ...
Rocket fuel chemist John Drury Clark reported in his book Ignition! that chloryl fluoride "is indecently reactive, and the hardest to keep of all the CI-O-F compounds, since it apparently dissolves the protective metal fluoride coatings that make the storage of ClF 3 comparatively simple."