If first ionization enthalpy (Delta_i H) valu | vedclass

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(A) Ionization enthalpy generally increases across a period due to an increase in effective nuclear charge. However,there are exceptions due to stable

Vedclass · Accepted Answer

$575$

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(A) Ionization enthalpy generally increases across a period due to an increase in effective nuclear charge. However,there are exceptions due to stable electronic configurations. The electronic configuration of $Mg$ $([Ne] 3s^2)$ is more stable than that of $Al$ $([Ne] 3s^2 3p^1)$ because $Mg$ has a completely filled $s$-orbital. Consequently,the first ionization enthalpy of $Al$ is lower than that of $Mg$. The values are: $Na (496) Therefore,the value for $Al$ is $575 \ kJ \ mol^{-1}$.

If first ionization enthalpy $(\Delta_i H)$ values of $Na$,$Mg$ and $Si$ are respectively $496$,$737$ and $786 \ kJ \ mol^{-1}$,the first ionization enthalpy value of $Al$ (in $kJ \ mol^{-1}$) will be

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