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° value and its high reducing power.| Metal \[{{E}^{\text{O-}}}/V\]for | Li | Na | K | Rb |
| \[({{M}^{+}}/M)\] | -3.04 | -2.714 | -2.925 | -2.930 |
You need to login to perform this action.
You will be redirected in
3 sec
