Attachment of [XeF]+ ions with [AsF6]- ions in their compound

The compound formed when [XeF]+ ions attach to [AsF6]- ions is known as xenon hexafluoroarsenate. To understand how this compound is formed, we need to consider the charges and electron configurations of the ions involved.

The [XeF]+ ion has a single positive charge because xenon (Xe) loses one electron. Xenon is a noble gas with an electron configuration of [Kr]5s24d105p6, so by losing one electron, it attains a stable electron configuration of [Kr]5s24d105p5. This leaves the xenon atom with an empty 5p orbital, making it an electron-deficient cation.

On the other hand, the [AsF6]- ion is a negatively charged polyatomic ion. Arsine (As) belongs to Group 15 of the periodic table and has an electron configuration of [Ar]3d104s24p3. When it reacts with six fluoride (F) atoms, each donating an electron, it forms a stable ion with a filled outer electron shell. This leads to the formation of the hexafluoroarsenate ion, [AsF6]-.

The attachment of the [XeF]+ ion with the [AsF6]- ion occurs through an ionic bond. The electron-deficient [XeF]+ cation accepts a lone pair of electrons from the electron-rich [AsF6]- ion. This allows the xenon atom to complete its valence shell, while the negative charge on the [AsF6]- ion is balanced by the positive charge on the [XeF]+ ion.

Overall, the compound formed is xenon hexafluoroarsenate, written as [XeF][AsF6]. It is worth noting that [XeF]+ ions are highly reactive and tend to form compounds with electron-rich species such as [AsF6]- through ionic bonding.