Which of the following linear combinations of | vedclass

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(D) For the formation of molecular orbitals,the atomic orbitals must have the same symmetry with respect to the internuclear axis ($z$-axis in this ca

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$D$ Only

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(D) For the formation of molecular orbitals,the atomic orbitals must have the same symmetry with respect to the internuclear axis ($z$-axis in this case).$A$: $2p_z$ and $2p_x$ have different symmetries ($p_z$ is $\sigma$-type,$p_x$ is $\pi$-type),so they do not combine.$B$: $2s$ and $2p_x$ have different symmetries ($s$ is $\sigma$-type,$p_x$ is $\pi$-type),so they do not combine.$C$: $3d_{xy}$ and $3d_{x^2-y^2}$ have different symmetries,so they do not combine.$D$: $2s$ and $2p_z$ both have cylindrical symmetry about the $z$-axis ($\sigma$-type),so they can combine to form a $\sigma$ molecular orbital.$E$: $2p_z$ and $3d_{x^2-y^2}$ have different symmetries,so they do not combine.Therefore,only the combination in $D$ leads to the formation of a molecular orbital.

Which of the following linear combinations of atomic orbitals will lead to the formation of molecular orbitals in homonuclear diatomic molecules [internuclear axis in $z$-direction]?

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