Ionisation energy in group I elements varies | vedclass

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(A) The ionisation energy of elements in a group decreases as we move down the group due to an increase in atomic size and the shielding effect.As the

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$Li > Na > K > Cs$

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(A) The ionisation energy of elements in a group decreases as we move down the group due to an increase in atomic size and the shielding effect.As the atomic size increases,the outermost electron is further from the nucleus,resulting in a weaker electrostatic attraction between the nucleus and the valence electron.For group $I$ (alkali metals),the order of ionisation energy is $Li > Na > K > Rb > Cs$.Therefore,the correct decreasing order is $Li > Na > K > Cs$.

$I.P.$ \text{ Trend}	Reason
$A$. $N > O$	Half-filled configuration
$B$. $Zr < Hf$	Lanthanide contraction
$C$. $Na > K$	$Z_{eff}$
$D$. $Al < Ga$	Transition contraction

Ionisation energy in group $I$ elements varies in the decreasing order as:

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$I.P.$ \text{ Trend} Reason

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