Chapter 15: Problem 11

Give reasons for the following: (a) \(\mathrm{SF}_{6}\) is inert but \(\mathrm{SF}_{4}\) is hydrolysed. (b) \(\mathrm{O}_{2}\) can act both as a reducing as well as an oxidising agent.

Short Answer

Expert verified

\(\mathrm{SF}_{6}\) is inert because it forms six sigma bonds with fluorine and has no lone pairs of electrons on its sulfur atom, while \(\mathrm{SF}_{4}\) can be hydrolysed because it has one lone pair of electrons on its sulfur atom that makes it reactive. \(\mathrm{O}_{2}\) can act as both a reducing and an oxidizing agent due to its ability to accept and donate electrons.

Step by step solution

Understanding molecular geometry of SF6 and SF4

For \(\mathrm{SF}_{6}\), sulfur hexafluoride, the central sulfur atom undergoes sp3d2 hybridization. It forms six sigma bonds with six fluorine atoms, resulting in an octahedral structure. As such, there are no lone pairs of electrons on the S atom, making it inert. However, in \(\mathrm{SF}_{4}\), sulfur tetrafluoride, the sulfur atom undergoes sp3d hybridization. It forms four sigma bonds with four fluorine atoms and has one lone pair of electrons in its valence shell, which makes it susceptible to hydrolysis.

Chemical Reaction of SF4 with water

\(\mathrm{SF}_{4}\) undergoes hydrolysis with water due to the presence of its lone pair of electrons creating a polarity that attracts the molecule of water which eventually breaks down the \(\mathrm{SF}_{4}\) molecule. The chemical reaction is given by \(\mathrm{SF}_{4} + 2H_2O → SO_2 + 4HF\)

Understanding the redox behavior of O2

Oxygen (O2) can act as both a reducing and an oxidizing agent due to its ability to accept and donate electrons. Oxygen can be reduced, meaning it gains electrons, by acting as an oxidizing agent. In the presence of heat, O2 is reduced into 2O- ions. Conversely, Oxygen can be oxidized (loses electrons) by acting as a reducing agent. Its conversion into O2- ions is an example of it being oxidized.

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Give reasons for the following: (a) \(\mathrm{SF}_{6}\) is inert but \(\mathrm{SF}_{4}\) is hydrolysed. (b) \(\mathrm{O}_{2}\) can act both as a reducing as well as an oxidising agent.

Short Answer

Step by step solution

Understanding molecular geometry of SF6 and SF4

Chemical Reaction of SF4 with water

Understanding the redox behavior of O2

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