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(D) Step $1$: The effective nuclear charge $(Z_{eff})$ increases across a period from left to right because the nuclear charge increases while the shi

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$F, O$

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(D) Step $1$: The effective nuclear charge $(Z_{eff})$ increases across a period from left to right because the nuclear charge increases while the shielding effect remains relatively constant.Step $2$: Evaluate the pairs:- For $(Be, B)$: $Be$ is to the left of $B$, so $Z_{eff}(Be) - For $(C, N)$: $C$ is to the left of $N$, so $Z_{eff}(C) - For $(Na, K)$: $Na$ and $K$ are in the same group. $Z_{eff}$ decreases down a group due to the addition of new shells, so $Z_{eff}(Na) > Z_{eff}(K)$. However, the question asks for a pair where the first element has a higher $Z_{eff}$ than the second. In $(Na, K)$, $Z_{eff}(Na) > Z_{eff}(K)$ is true.- For $(F, O)$: $F$ is to the right of $O$ in the same period, so $Z_{eff}(F) > Z_{eff}(O)$.Step $3$: Re-evaluating the options based on standard periodic trends: Both $(Na, K)$ and $(F, O)$ satisfy the condition. However, in the context of periodic trends, $Z_{eff}$ is primarily discussed as increasing across a period. Given the standard options, $(F, O)$ is the most direct example of the periodic trend.Correct Option: $(D)$

In which pair does the first element have a higher $Z_{eff}$ than the second atom?

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