The single bond covalent radius (SBCR) of P i | vedclass

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(A) Across a period in the periodic table,the atomic radius decreases from left to right due to an increase in effective nuclear charge $(Z_{eff})$.Ph

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Smaller than $P$

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(A) Across a period in the periodic table,the atomic radius decreases from left to right due to an increase in effective nuclear charge $(Z_{eff})$.Phosphorus $(P)$ is in Group $15$ and Chlorine $(Cl)$ is in Group $17$ of the same period (Period $3$).Since $Cl$ is to the right of $P$,the effective nuclear charge of $Cl$ is higher than that of $P$.Therefore,the covalent radius of $Cl$ $(0.099 \ nm)$ is smaller than the covalent radius of $P$ $(0.11 \ nm)$.

The single bond covalent radius $(SBCR)$ of $P$ is $0.11 \ nm$. The single bond covalent radius of $Cl$ is:

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