Xenon is a noble gas with a full outer electron shell, making it relatively unreactive. It does not readily form compounds with other elements, such as fluorine, because the energy required to remove electrons from xenon to form bonds is extremely high, making the formation of xenon fluorides energetically unfavorable.
The formula for xenon pentafluoride is XeF5.
Xenon pentafluoride (XeF5) has a total of 8 valence electrons. Xenon (Xe) contributes 8 valence electrons, while each fluorine (F) atom contributes 7 valence electrons. The 5 fluorine atoms in XeF5 contribute a total of 35 valence electrons.
XeF5+
It will be weakly polar as a neutral compound, due to the presence of 1 unshared pair of electrons around the central xenon atom. (Additionally, the relatively large number of electrons in this compound will yield temporary dipoles in the form of dispersion forces.) If it's an ion, then I would need to know its charge. If its charge is +2 (meaning it has lost 2 electrons,) then that ion would be non-polar.
Because there will be one electron left once Xe forms 3 bonds with F, and has 2 lone pair of electrons in the case of XeF3. in the case of XeF5, there will be 5 bond pairs, and 1 lone pair. still 1 electron will be left, which is not possible.
The formula for xenon pentafluoride is XeF5.
Xenon pentafluoride (XeF5) has a total of 8 valence electrons. Xenon (Xe) contributes 8 valence electrons, while each fluorine (F) atom contributes 7 valence electrons. The 5 fluorine atoms in XeF5 contribute a total of 35 valence electrons.
XeF5+
It will be weakly polar as a neutral compound, due to the presence of 1 unshared pair of electrons around the central xenon atom. (Additionally, the relatively large number of electrons in this compound will yield temporary dipoles in the form of dispersion forces.) If it's an ion, then I would need to know its charge. If its charge is +2 (meaning it has lost 2 electrons,) then that ion would be non-polar.