Assertion :Lithium is the weakest reducing agent among alkali metals.
Reason: In alkali metals ionization energy decreases down the group.
Read the above assertion and reason and choose the correct option regarding it.
Assertion :Lithium is the weakest reducing agent among alkali metals.
Reason: In alkali metals ionization energy decreases down the group.
The correct option is C Assertion is incorrect but reason is correct
Alkali metals are very good reducing agents because of their great tendency to lose electrons. The reducing character increases from Na to Cs. However, Li is stronger reducing agent than Na due to greater hydration energy.
Explanation: An element, which acts as a reducing agent, must have low ionization energy. Alkali metals act as strong reducing agents as their ionization energy values are low. Since, ionization decreases on moving down from Li to Cs, the reducing property increases in same order. Thus, Li is the weakest reducing agent while Cs is the strongest reducing agent amongst alkali metals in a free gaseous state.The tendency of an element to lose an electron in solution is measured by its standard oxidation potential value (Eo) . Since alkali metals have high Eo values, these are strong reducing agents. However, it is observed that Li is the strongest reducing agent amongst alkali metals in solution as Eo value of Li is maximum. At first sight, lithium having a high value of ionization energy amongst alkali metals acts as the strongest reducing agent in solution. This can be explained if we understand the fact that ionization energy is the property of an isolated atom in a gaseous state while oxidation potential is concerned when the metal atom goes into the solution.
So Assertion is incorrect but Reason is correct,
Alkali metals are very good reducing agents because of their great tendency to lose electrons. The reducing character increases from Na to Cs. However, Li is stronger reducing agent than Na due to greater hydration energy.
Explanation: An element, which acts as a reducing agent, must have low ionization energy. Alkali metals act as strong reducing agents as their ionization energy values are low. Since, ionization decreases on moving down from Li to Cs, the reducing property increases in same order. Thus, Li is the weakest reducing agent while Cs is the strongest reducing agent amongst alkali metals in a free gaseous state.The tendency of an element to lose an electron in solution is measured by its standard oxidation potential value (Eo) . Since alkali metals have high Eo values, these are strong reducing agents. However, it is observed that Li is the strongest reducing agent amongst alkali metals in solution as Eo value of Li is maximum. At first sight, lithium having a high value of ionization energy amongst alkali metals acts as the strongest reducing agent in solution. This can be explained if we understand the fact that ionization energy is the property of an isolated atom in a gaseous state while oxidation potential is concerned when the metal atom goes into the solution.
So Assertion is incorrect but Reason is correct,
