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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 c

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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).$A: 2p_z$ ($\sigma$-type) and $2p_x$ ($\pi$-type) have different symmetries, so they do not combine.$B: 2s$ ($\sigma$-type) and $2p_x$ ($\pi$-type) have different symmetries, 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.$E: 2p_z$ ($\sigma$-type) and $3d_{x^2-y^2}$ ($\delta$-type) 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]?
$A: 2p_z + 2p_x$
$B: 2s + 2p_x$
$C: 3d_{xy} + 3d_{x^2-y^2}$
$D: 2s + 2p_z$
$E: 2p_z + 3d_{x^2-y^2}$

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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]?$A: 2p_z + 2p_x$$B: 2s + 2p_x$$C: 3d_{xy} + 3d_{x^2-y^2}$$D: 2s + 2p_z$$E: 2p_z + 3d_{x^2-y^2}$