Explanation of Assertion (A):
In aqueous solutions, acts as a reducing agent and is oxidised to . This is because has a stable electronic configuration. Conversely, acts as an oxidising agent and is reduced to , which has a stable half-filled electronic configuration.
Explanation of Reason (R):
The half-filled electronic configuration provides extra stability due to symmetrical distribution of electrons and exchange energy. This explains why and are more stable compared to their respective other oxidation states.
Conclusion:
Both Assertion (A) and Reason (R) are true. The reason given (R) correctly explains why is reducing and is oxidising, as it is related to the stability of the resulting electronic configurations.
Given below are two statements:
Statement (I): The first ionization energy of Pb is greater than that of Sn.
Statement (II): The first ionization energy of Ge is greater than that of Si.
In light of the above statements, choose the correct answer from the options given below:
If and
and , then the value of equals to: