atomic number.6.3 Jonization Enthalplesalkaline earth metals have low ionizationthalpies due to fairly large size of the atoms.ce the atomic size increases down theup, their ionization enthalpy decreasesble 10.2). The first ionisation enthalpies ofalkaline earth metals are higher than thosehe corresponding Group 1 metals. This isto their small size as compared to theesponding alkali metals. It is interestingote that the second ionisation enthalpiesy why inwritten largw size it should be smal

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Q. The first ionisation enthalpies of the alkaline earth metals are higher than that of alkali metals but second ionisation enthalpies are smaller, why?

Question 2

Why does $H^{+}$ ion always get associated with other atom or molecules?

(a) Ionisation enthalpy of hydrogen resembles that of alkali metals.

(b) Its reactivity is similar to halogens

(d) Loss of an electron from hydrogen atom results in a nucleus of very small size as compare to other or ions. Due to small size it cannot exist free.

Q. Alkaline earth metals always form divalent cations even though their second ionisation enthalpies are almost double than their first ionisation enthalpies

Q. Assertion :The crystalline salts of alkaline earth metals contain more water of crystallization than the corresponding alkali metal salts. Reason: The size of alkaline earth metal ions is lower than the size of alkali metal ions. The lower the size of the cation, the higher is the hydration energy. So the salts of alkaline earth metals have more water molecules of crystallization than those of alkali metals.

The first ionization energies of alkaline earth metals are higher than those of the alkali metals. This is because ...

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