The first ionization enthalpies of Mg and Al | vedclass

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Question

(D) Magnesium $(Mg)$ has the atomic number $12$ and electronic configuration $[Ne] 3s^2$. Since the $3s$ orbital is fully filled,it is more stable and

Vedclass · Accepted Answer

$IE_1(Mg) = 737.7 \ kJ \cdot mol^{-1}, IE_1(Al) = 577.5 \ kJ \cdot mol^{-1}$

Vedclass · Answer

(D) Magnesium $(Mg)$ has the atomic number $12$ and electronic configuration $[Ne] 3s^2$. Since the $3s$ orbital is fully filled,it is more stable and requires more energy to remove an electron.Aluminium $(Al)$ has the atomic number $13$ and electronic configuration $[Ne] 3s^2 3p^1$. The electron is removed from the $3p$ orbital,which is easier to remove than an electron from a fully filled $3s$ orbital.Therefore,the first ionization enthalpy of $Mg$ $(737.7 \ kJ \cdot mol^{-1})$ is higher than that of $Al$ $(577.5 \ kJ \cdot mol^{-1})$.

The first ionization enthalpies of $Mg$ and $Al$ can be expected to be

Similar Questions

Which of the following orders regarding ionization energy is correct?

The correct order of $IE_2$ (second ionization enthalpy) is:

Observe the following statements.
Statement $(A)$: In general,the ionisation potential value decreases on moving down in the group.
Statement $(B)$: The $1$st ionisation potential of sodium is greater than that of potassium.
Correct answer is:

The first $I.E.$ of $Na, Mg, Al$ and $Si$ are in the order:

Among the following,which has the highest first ionization energy?

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