Sncl2 is reducing but pbcl2 is neither reducing not oxidising.. why?

Question

Answer

Explanation:

Reduction potential:

- SnCl2 undergoes reduction because it has a higher reduction potential compared to PbCl2.
- The reduction potential of SnCl2 is more negative than that of PbCl2, making SnCl2 more likely to be reduced.

Electronic configuration:

- In the case of SnCl2, tin (Sn) is in its +2 oxidation state and can be reduced to Sn.
- On the other hand, lead (Pb) in PbCl2 is already in its +2 oxidation state and cannot be further reduced.

Chemical behavior:

- SnCl2 can act as a reducing agent because it can easily donate electrons to another species, allowing it to undergo reduction.
- PbCl2, on the other hand, does not have the ability to donate electrons easily and therefore does not undergo reduction or oxidation reactions.

Conclusion:

- In summary, SnCl2 is reducing because of its higher reduction potential, its electronic configuration that allows it to be reduced, and its chemical behavior as a reducing agent. PbCl2, on the other hand, is neither reducing nor oxidizing due to its inherent properties.

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