The correct statement is:

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Question

(A) Boron $(B)$ has a valence shell configuration of $2s^2 2p^1$. It has only four orbitals available for bonding $(2s, 2p_x, 2p_y, 2p_z)$. Therefore,

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Boron has a maximum covalency of four.

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(A) Boron $(B)$ has a valence shell configuration of $2s^2 2p^1$. It has only four orbitals available for bonding $(2s, 2p_x, 2p_y, 2p_z)$. Therefore, its maximum covalency is $4$. Beryllium $(Be)$ has a valence shell configuration of $2s^2$. It has only two valence orbitals $(2s, 2p)$. Magnesium $(Mg)$ has a valence shell configuration of $3s^2$. It has $3s, 3p_x, 3p_y, 3p_z$ and $3d$ orbitals available. Thus, it can exhibit a covalency higher than $4$ (e.g.,$6$ in $[Mg(H_2O)_6]^{2+}$). Aluminum $(Al)$ has a valence shell configuration of $3s^2 3p^1$. It has $3s, 3p_x, 3p_y, 3p_z$ and five $3d$ orbitals, totaling $9$ valence orbitals. Thus, the correct statement is that Boron has a maximum covalency of $4$.

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