In comparison to boron,beryllium has

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(D) The atomic number of beryllium $(Be)$ is $4$ and boron $(B)$ is $5$. Since $B$ has a higher atomic number than $Be$,it has a greater nuclear charg

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lesser nuclear charge and greater first ionisation enthalpy

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(D) The atomic number of beryllium $(Be)$ is $4$ and boron $(B)$ is $5$. Since $B$ has a higher atomic number than $Be$,it has a greater nuclear charge. The electronic configuration of $Be$ is $1s^2 2s^2$ (fully filled $s$-orbital),while $B$ is $1s^2 2s^2 2p^1$. Due to the stable fully filled $2s$-orbital in $Be$,it requires more energy to remove an electron compared to $B$. Therefore,$Be$ has a lesser nuclear charge and a greater first ionisation enthalpy compared to $B$.

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