The incorrect statement among the following i | vedclass

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(B) The correct answer is $(B)$.$1$. The first ionisation potential $(IE_1)$ of $Al$ $([Ne] 3s^2 3p^1)$ is less than $Mg$ $([Ne] 3s^2)$ because $Mg$ h

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The second ionisation potential of $Mg$ is greater than the second ionisation potential of $Na$

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(B) The correct answer is $(B)$.$1$. The first ionisation potential $(IE_1)$ of $Al$ $([Ne] 3s^2 3p^1)$ is less than $Mg$ $([Ne] 3s^2)$ because $Mg$ has a stable fully-filled $s$-orbital.$2$. The second ionisation potential $(IE_2)$ of $Na$ $([Ne] 3s^1 \rightarrow [Ne])$ is much higher than that of $Mg$ $([Ne] 3s^2 \rightarrow [Ne] 3s^1)$ because the second electron in $Na$ is removed from a stable noble gas core $([Ne])$.$3$. $IE_1$ of $Na$ is less than $Mg$ due to higher effective nuclear charge and stable configuration of $Mg$.$4$. The third ionisation potential $(IE_3)$ of $Mg$ is higher than $Al$ because the third electron in $Mg$ is removed from a stable noble gas core $([Ne])$,whereas in $Al$ it is removed from the $3s^2$ subshell.

The incorrect statement among the following is:

Similar Questions

Which of the following elements has the highest ionisation energy?

The first ionization enthalpy of the following elements are in the order:

The electronic configuration which is associated with the highest first ionisation enthalpy is:

Given below are two statements:
Statement $I$: The first ionization energy of $Pb$ is greater than that of $Sn$.
Statement $II$: The first ionization energy of $Ge$ is greater than that of $Si$.
In the light of the above statements,choose the correct answer from the options given below:

If the $IP$ of $Na$ is $5.48 \, eV$,the ionisation potential of $K$ will be ............ $eV$.

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