A large difference between the fourth and fif | vedclass

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(C) Ionization energy is the energy required to remove an electron from a gaseous atom or ion. When the fourth electron is removed,the atom achieves a

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$4$ valence electrons in an atom

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(C) Ionization energy is the energy required to remove an electron from a gaseous atom or ion. When the fourth electron is removed,the atom achieves a stable electronic configuration (such as a noble gas configuration). Removing the fifth electron would require breaking this stable configuration,which demands a significantly higher amount of energy. Therefore,a large jump between the $4^{th}$ and $5^{th}$ ionization energies indicates that the atom has $4$ valence electrons.

List-$I$ (Electronic configuration of neutral atom where $n=2$)	List-$II$ ($1^{st}$ Ionization Energy in $\text{kJ mol}^{-1}$)
$A. ns^2$	$I. 2080$
$B. ns^2np^1$	$II. 899$
$C. ns^2np^3$	$III. 800$
$D. ns^2np^6$	$IV. 1402$

$A$ large difference between the fourth and fifth ionization energies indicates the presence of

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The ionisation potentials of $Li$ and $K$ are $5.4 \ eV$ and $4.3 \ eV$ respectively. The ionisation potential of $Na$ will be ................ $eV$.

Match List-$I$ with List-$II$:
List-$I$ (Electronic configuration of neutral atom where $n=2$) List-$II$ ($1^{st}$ Ionization Energy in $\text{kJ mol}^{-1}$)
$A. ns^2$ $I. 2080$
$B. ns^2np^1$ $II. 899$
$C. ns^2np^3$ $III. 800$
$D. ns^2np^6$ $IV. 1402$

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