A) \[Rb<K<Na<Li\]
B) \[Li<Na<K<Rb\]
C) \[Na<K<Rb<Li\]
D) \[Rb<Na<K<Li\]
Correct Answer: C
Solution :
The alkali metals are strong reducing agents, lithium the most and sodium the least powerful. The standard electrode potential \[({{E}^{o}})\] which measures the reducing power represents the overall change \[M(s)\xrightarrow{{}}M(g)\] Sublimation enthalpy \[M(g)\xrightarrow{{}}{{M}^{+}}(g)+{{e}^{-}}\] ionization enthalpy \[{{M}^{+}}(g)+{{H}_{2}}O\xrightarrow{{}}{{M}^{+}}(aq)\] hydration enthalpy With the small size of its ion, lithium has the highest hydration enthalpy which accounts for its high negative \[E{}^\circ \] value and its high reducing power.| Metal | Li | Na | K | Rb |
| \[{{E}^{\text{o}-}}/V\]for | ||||
| \[({{M}^{+}}/M)\] | \[-3.04\] | \[-2.714\] | \[-2.925\] | \[-2.930\] |
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