Among the elements Ca, Mg, P and Cl, the orde | vedclass

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(B) Atomic radius decreases across a period from left to right due to an increase in effective nuclear charge,while it increases down a group due to t

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$Cl < P < Mg < Ca$

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(B) Atomic radius decreases across a period from left to right due to an increase in effective nuclear charge,while it increases down a group due to the addition of new shells.The electronic configurations are:$Mg (Z=12): [Ne] 3s^2$$P (Z=15): [Ne] 3s^2 3p^3$$Cl (Z=17): [Ne] 3s^2 3p^5$$Ca (Z=20): [Ar] 4s^2$$Mg, P,$ and $Cl$ belong to the $3^{rd}$ period. Within the same period,the atomic radius decreases as $Z$ increases: $Mg > P > Cl$.$Ca$ belongs to the $4^{th}$ period,so it has a larger atomic radius than the $3^{rd}$ period elements.Therefore,the increasing order of atomic radii is $Cl < P < Mg < Ca$.

Among the elements $Ca, Mg, P$ and $Cl,$ the order of increasing atomic radii is

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