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Number of double bond present in the Lewis structure of $ PF_6^ - $ is :

Last updated date: 25th Jul 2024
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Hint: For hexafluorophosphate, [ $ P{F_6} $ ]-, there are six bonded groups and so no lone pairs. This anion is useful in synthesis as it also aids the crystallisation of bulky cations by having a suitable size match for the cation. The ion's negative charge is distributed through all seven atoms.

Complete answer:
The valence shell electron pair repulsion (VSEPR) theory is a mathematical model for predicting 3-D molecular geometry based on the number of valence shell electron bond pairs between atoms in a molecule or ion. As long as the central atom is not a metal, it can predict the form of almost all compounds with a central atom.
In this compound the central atom is phosphorus. We know that initially the valence electron on the central atom is $ 5 $ . The $ 6 $ Fluoride atom contributes one electron each. Hence, we add one negative charge to P. So the total valence electron is $ 12 $ .
Dividing $ 12 $ by $ 2 $ , we get $ 6 $ . Hence, the geometry formed in $ 6 $ electron pairs is Octahedral geometry. Therefore, The VSEPR model for $ {\left[ {P{F_6}} \right]^ - } $ is Octahedral.
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In this figure, we can conclude that there are no double bonds in the compound. Hence, the No. of double bonds present in the Lewis structure of $ PF_6^ - $ is $ 0 $ .

Hexafluorophosphate is most commonly used as the lithium salt, lithium hexafluorophosphate. This salt is a natural electrolyte in industrial secondary batteries, such as lithium-ion cells, when combined with dimethyl carbonate.