A) \[~X>Y>Z\]
B) \[~Z>Y>X\]
C) \[~X=Y=Z\]
D) \[~Z>X>Y\]
Correct Answer: A
Solution :
All alkali metal salts are soluble in water. The degree of hydration depends upon the size of the cation. Smaller the size of a cation, greaten is its charge density and hence, greater is its tendency to withdraw electrons molecules which are thus polarised. \[\text{L}{{\text{i}}^{\text{+}}}\]ion being smallest in size among alkali metal ions is the most extensively hydrated while\[C{{s}^{+}}\]ion the largest alkali metal ion is the least hydrated. The size of hydrated alkali ions is as \[L{{i}^{+}}>N{{a}^{+}}>{{K}^{+}}>R{{b}^{+}}>C{{s}^{+}}\] (Relative ionic radii in water) (Relative degree of hydration)
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