Question

: What is the oxidation state of Xe in \[Xe\left[ {Pt{F_6}} \right]\] ?
A. +1
B. +2
C. +4
D. +6

Answer 1

Hint: Xenon is an inert gas. Its electronic configuration is \[[Kr]4{d^{10}}5{s^2}5{p^6}\] . All orbitals that are filled have paired electrons. Xenon can combine with an even number of F atoms to form $Xe{F_2}$ , $Xe{F_4}$ and $Xe{F_6}$ . This is because the promotion of 1, 2, or 3 electrons from the 5p filled orbitals to 5d vacant orbitals will give rise to 2,4,6 half-filled orbitals.

Complete step by step answer:
-The periodic table is a great source of information about the elements and their relation to each other. Changes of different periodic properties. Also, this helps to predict the properties of the elements even if they are not discovered. Inert gases are from group 18. Which is on the extreme right side of the periodic table.
-The periodic table is a great source of information about the elements and their relation to each other. Changes of different periodic properties. Also, this helps to predict the properties of the elements even if they are not discovered. Inert gases are from group 18. Which is on the extreme right side of the periodic table.
-In the given compound. The oxidation number of the xenon of this compound can be calculated by summation of all the charges of the ligands and subtract that value from the total charge of the compound.
In this complex \[Xe\left[ {Pt{F_6}} \right]\] , the fluorine shows -1 charge, platinum shows +4 charges. Therefore, let the charge of the xenon is x, then the value of x is
 \[
  x + 4 + \left( { - 1 \times 6} \right) = 0 \\
  x + 4 - 6 = 0 \\
  x - 2 = 0 \\
  x = + 2 \\
 \]
So, the oxidation state is +2.

So, the correct answer is B.

Note:
In 1961, Neil Barnett was experimenting with fluorine and platinum and produced a dark red solid compound. He did a lot of research to find out its chemical composition. He found out that the product formed was \[Pt{F_6}\] (platinum hexafluoride), which can oxidize oxygen and produced red solid identified as \[{O_2}^ + Pt{F_6}^ - \] .
The unusual thing about this compound was that it had positively charged oxygen, whereas oxygen generally has a negative charge. Therefore, he believed that \[Pt{F_6}\] is a stronger oxidizing agent than oxygen. And thereby he concluded that oxygen and xenon have similar ionization energies.