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Nilanjan Bhowmick AIR 3, CSIR NET (Earth Science)
- IIT JAM
- Chemistry (CY)
How heat of hydration differ in periodic table . please explain with this question
how heat of hydration differ in periodic table . please explain with this question
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Priyanshu kumar Best Answer
Hydration energy depends upon size of cation and charge of cation so higher the charge of cation and lower the size of cation have higher hydration energy. So, here Al 3+ will have highest hydration due to smaller size and charge.
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got roni...??
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yes sir thank s
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always welcome dear😊
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Suman Kumar![best-answer]()
The attractions are stronger the smaller the ion. For example, hydration enthalpies fall as you go down a group in the Periodic Table. The small lithium ion has by far the highest hydration enthalpy in Group1, and the small fluoride ion has by far the highest hydration enthalpy in Group 7. In both groups, hydration enthalpy falls as the ions get bigger.
The attractions are stronger the more highly charged the ion. For example, the hydration enthalpies of Group 2 ions (like Mg2+) are much higher than those of Group 1 ions (like Na+).
More the attraction more will be the heat of hydration. So Al³+ is correct option
thanks sir