Correct increasing order of first ionisation | vedclass

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Question

(A) As we move across the period,nuclear charge increases and atomic size decreases,hence ionisation enthalpy generally increases.For $Al$ $([Ne] 3s^2

Vedclass · Accepted Answer

$Na  Al < Si$

Vedclass · Answer

(A) As we move across the period,nuclear charge increases and atomic size decreases,hence ionisation enthalpy generally increases.For $Al$ $([Ne] 3s^2 3p^1)$,the electron is removed from a partially filled $3p$ orbital,whereas for $Mg$ $([Ne] 3s^2)$,the electron is removed from a stable,fully filled $3s$ orbital.Removal of an electron from a stable,fully filled orbital requires more energy than removal from a partially filled orbital.Therefore,the ionisation enthalpy of $Mg$ is greater than that of $Al$.The correct order of first ionisation enthalpies is: $Na  Al < Si$.

Correct increasing order of first ionisation potential is

Similar Questions

The order of the magnitude of first ionisation potentials of $Be$,$B$,$N$ and $O$ is

Identify the element having the highest ionization enthalpy.

Would you expect the first ionization enthalpies for two isotopes of the same element to be the same or different? Justify your answer.

The first ionization enthalpy $(\Delta_{i} H)$ values of the third period elements,$Na, Mg$ and $Si$ are respectively $496, 737$ and $786 \, kJ \, mol^{-1}$. Predict whether the first $\Delta_{i} H$ value for $Al$ will be more close to $575$ or $760 \, kJ \, mol^{-1}$? Justify your answer.

The correct order of first ionization potential $(IP)$ is:

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