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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]
The fluorine–fluorine bond of the difluorine molecule is relatively weak when compared to the bonds of heavier dihalogen molecules. The bond energy is significantly weaker than those of Cl 2 or Br 2 molecules and similar to the easily cleaved oxygen–oxygen bonds of peroxides or nitrogen–nitrogen bonds of hydrazines. [8]
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
[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.
Chlorine trifluoride (ClF 3) is a colourless gas that condenses to a green liquid, and freezes to a white solid. It is made by reacting chlorine with an excess of fluorine at 250 °C in a nickel tube. It reacts more violently than fluorine, often explosively. The molecule is planar and T-shaped. It is used in the manufacture of uranium ...
Structure of xenon oxytetrafluoride, an example of a molecule with the square pyramidal coordination geometry. Square pyramidal geometry describes the shape of certain chemical compounds with the formula ML 5 where L is a ligand. If the ligand atoms were connected, the resulting shape would be that of a pyramid with a square base.
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 known as the H-bond.
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 .