Question

If we use the magnitude of the IE1 as an indicator of ease of oxidation, Li is the most difficult of the alkali metals to oxidise. On the other hand, if E0redn (standard reduction electrode potential) is used as the criterion, Li is the easiest to oxidise. How can we explain this discrepancy?

Answer 1

The ease of oxidation of lithium (Li) among the alkali metals can be explained by considering ionization energy and standard reduction electrode potential. Lithium has a higher ionization energy compared to other alkali metals, making it difficult to oxidize based on the magnitude of its IE1.

Step-by-step explanation:

The apparent discrepancy in the ease of oxidation of lithium (Li) among the alkali metals can be explained by considering two factors: ionization energy (IE) and standard reduction electrode potential (E0redn).

Lithium has a smaller atomic radius compared to other alkali metals, which makes it difficult to remove its valence electron and hence it has a higher ionization energy. This means that Li is the most difficult to oxidize based on the magnitude of its IE1.

However, when considering standard reduction electrode potential, Li is the easiest to oxidize. This is because Li has the most negative E0redn value, indicating that it has the highest tendency to undergo oxidation.

This discrepancy arises due to the different criteria used to measure ease of oxidation, with IE1 focusing on ionization energy and E0redn focusing on reduction potential.