Which of the following overlaps is incorrect (assuming the Z-axis is internuclear axis)?

(A) $2p_y+2p_y⟶\pi$Bond formation

(B)  $2p_x+2p_x⟶\sigma -$Bond formation

(C) $3d_{xy}+3d_{xy}⟶\pi -$Bond formation

(D) $2s+2p_y⟶\pi -$Bond formation

(E) $3d_{xy}+3d_{xy}⟶\delta -$Bond formation

(F) $2p_z+2p_z⟶\sigma -$Bond formation

Solution:

$\mathrm{\pi }$ bonds are covalent chemical bonds where two lobes of an orbital in an atom orbital two lobes of an orbital on another atom & this over lop occurs bterally 4 perpendicularly to internuclear axis
Delta bonds are formed by sideways overlap of 4 lobes of $\mathrm{d}-$orbitals perpendicular to internuclear axis.
B) In (B), $2p_x$ orbitals are perpendicular to z-axis 4 should more $\mathrm{\pi }$ bond.
C) In (C), $3d_{xy}$ are perpendicular to z axis 4. should more delta bond
D) In (D) $2\mathrm{s}$, ($\mathrm{s}-$ orbital) only make sigma bonds.

Hence, the option D is correct.