Consider the elements Ne,Na,and Mg. The eleme | vedclass

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(B) The electronic configurations are: $_{10}Ne = 1s^2 2s^2 2p^6$ $_{11}Na = 1s^2 2s^2 2p^6 3s^1$ $_{12}Mg = 1s^2 2s^2 2p^6 3s^2$ $1$. Highest first i

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$Ne$,$Mg$

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(B) The electronic configurations are: $_{10}Ne = 1s^2 2s^2 2p^6$ $_{11}Na = 1s^2 2s^2 2p^6 3s^1$ $_{12}Mg = 1s^2 2s^2 2p^6 3s^2$ $1$. Highest first ionization enthalpy: $Ne$ has the highest first ionization enthalpy because it is a noble gas with a stable,fully-filled valence shell $(2s^2 2p^6)$. $2$. Lowest second ionization enthalpy: The second ionization enthalpy involves removing an electron from a unipositive ion. For $Na^+$,the configuration becomes $1s^2 2s^2 2p^6$ (stable noble gas configuration),making the second ionization enthalpy very high. For $Mg^+$,the configuration is $1s^2 2s^2 2p^6 3s^1$. Removing the second electron from $Mg^+$ leads to the stable $Mg^{2+}$ ion $(1s^2 2s^2 2p^6)$,which is energetically favorable. Thus,$Mg$ has the lowest second ionization enthalpy among the given elements.

Consider the elements $Ne$,$Na$,and $Mg$. The element with the highest first ionization enthalpy and the element with the lowest second ionization enthalpy,respectively,are:

Similar Questions

Given below are two statements:
Statement $(I)$: The first ionisation enthalpy of the elements $Na$, $Mg$, $Cl$ and $Ar$ follows the order $Na > Mg > Cl > Ar$.
Statement $(II)$: Among $Ca$, $Al$, $Fe$ and $B$, the third ionisation enthalpy is very high for $Ca$.

The first ionisation potentials $(eV)$ of $Be$ and $B$ respectively are :-

Which particle may be removed from a stable neutral atom with the least energy change?

The first ionization energy of magnesium is smaller as compared to that of elements $X$ and $Y$,but higher than that of $Z$. The elements $X$,$Y$ and $Z$,respectively,are :

The set representing the correct order of first ionisation potential is

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