Select the CORRECT statement if the internucl | vedclass

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(A) If the internuclear axis is the $y-$ axis:$1$. Orbitals overlapping along the $y-$ axis form $\sigma$ bonds (e.g.,$p_y - p_y$,$s - p_y$,$d_{y^2} -

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$d_{xy}$ and $d_{xy}$ orbitals of two atoms form a $\pi -$ bond.

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(A) If the internuclear axis is the $y-$ axis:$1$. Orbitals overlapping along the $y-$ axis form $\sigma$ bonds (e.g.,$p_y - p_y$,$s - p_y$,$d_{y^2} - d_{y^2}$). $2$. Orbitals overlapping perpendicular to the $y-$ axis form $\pi$ bonds.$3$. For option $A$: $d_{xy}$ orbitals have lobes in the $xy$ plane. When two $d_{xy}$ orbitals approach along the $y-$ axis,they overlap sideways to form a $\pi$ bond.$4$. For option $B$: $p_z$ orbitals are perpendicular to the $y-$ axis,so they form $\pi$ bonds,not $\sigma$ bonds.$5$. For option $C$: $d_{x^2 - y^2}$ orbitals have lobes along the $x$ and $y$ axes. Overlap along the $y-$ axis results in a $\sigma$ bond due to the $y$ component.$6$. For option $D$: $p_y$ (along $y$) and $d_{zx}$ (in $zx$ plane) have no effective overlap symmetry for a $\pi$ bond.

Select the $CORRECT$ statement if the internuclear axis is the $y-$ axis.

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