Question

Whether \[{\text{L}}{{\text{i}}^{\text{ + }}}\] has greatest reducing nature
A. True
B. False

Answer 1

Hint: Reduction means the addition of an electron to an atom or a species. The atom or species donating that electron or the one which is helping in reduction is called a reducing agent and the one which undergoes reduction is getting reduced. Usually metal ions readily give electrons and are good reducing agents.

Complete step by step answer:
Metal atoms are usually said to be electropositive ones because most of them would like to lose their outer electrons and desires to have a stable outer electronic configuration. In a periodic table, metals usually occupy the left side and they are the ones having the least nuclear force of attraction when compared to other atoms in their respective periods.
Lithium having atomic number 3 has the electronic configuration as follows:
\[{\text{Li - 1}}{{\text{s}}^{\text{2}}}{\text{2}}{{\text{s}}^{\text{1}}}\]
Here we can see that Li has one electron in its outermost shell and a fully filled 1s orbital. It would be difficult for the atom to gain an electron and to have a fully filled outer orbit. So, it would readily lose the one electron in its outermost shell and thereby having a completely filled 1s orbital. In this way, it acquires stable electronic configuration.
After losing the one electron in the outermost orbital, Li acquires the +1-oxidation state and becomes \[{\text{L}}{{\text{i}}^{\text{ + }}}\] having the electronic configuration as follows;
\[{\text{L}}{{\text{i}}^{\text{ + }}}\]-\[{\text{1}}{{\text{s}}^{\text{2}}}\]
Now we can see that Li has a stable outer electronic configuration and it will not prefer losing its electrons. As only those atoms or species that donates electrons are said to have a reducing nature are called as reducing agents, \[{\text{L}}{{\text{i}}^{\text{ + }}}\] will no longer donates electrons in a reaction as it has a stable 1s orbital.
Also being at the top of the group of alkali metals in the periodic table, Li is least electropositive because as we go down the group, the number of shells or orbitals increases and the outermost electron will suffer less nuclear force of attraction. So, it will be easier for alkali metals to lose its outermost electrons on going down the group.

For all these reasons we can say that the statement that \[{\text{L}}{{\text{i}}^{\text{ + }}}\] has a high reducing nature is a false statement.

Additional information:
Oxidation and reduction are common in a reaction. Atoms or elements participate in a reaction to acquire stable outer electronic configuration. They do so by gaining or losing their valence shell electrons. This results in oxidation or reduction of the atom.

Note: Lithium exerts the greatest polarizing effect which means the dissolution of the substance in water by absorbing water molecules by weak valency forces, among the other alkali metals o, on negative ions. The degree of hydration will be large when the size of cation is small. It is a fact that \[{\text{L}}{{\text{i}}^{\text{ + }}}\] has great reducing nature in aqueous medium because of the maximum hydration energy of the \[{\text{L}}{{\text{i}}^{\text{ + }}}\] ion.