The CORRECT order of first ionisation enthalp | vedclass

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Question

(B) The electronic configurations of the elements are:$Mg (Z=12): [Ne] 3s^2$$Al (Z=13): [Ne] 3s^2 3p^1$$P (Z=15): [Ne] 3s^2 3p^3$$S (Z=16): [Ne] 3s^2

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$Al < Mg < S < P$

Vedclass · Answer

(B) The electronic configurations of the elements are:$Mg (Z=12): [Ne] 3s^2$$Al (Z=13): [Ne] 3s^2 3p^1$$P (Z=15): [Ne] 3s^2 3p^3$$S (Z=16): [Ne] 3s^2 3p^4$$1$. $Mg$ has a fully filled $3s$ orbital,making it more stable than $Al$,so $I.E._{Mg} > I.E._{Al}$.$2$. $P$ has a half-filled $3p$ subshell $(3p^3)$,which is highly stable,making its $I.E.$ higher than that of $S$ $(3p^4)$.$3$. Across a period,$I.E.$ generally increases. Combining these factors,the order is $Al < Mg < S < P$.

The $CORRECT$ order of first ionisation enthalpy is:

Similar Questions

The second ionization enthalpy of an element is always higher than its first ionization enthalpy because

Assertion : Element has a tendency to lose the electron$(s)$ to attain the stable configuration.
Reason : Ionization enthalpy is the energy released to remove an electron from an isolated gaseous atom in its ground state.

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