In which of the following molecular shapes mu | vedclass

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(B) The involvement of $d$-orbitals in hybridization depends on the geometry of the molecule:$(a)$ Pentagonal planar geometry involves $sp^3d^3$ hybri

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Trigonal planar

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(B) The involvement of $d$-orbitals in hybridization depends on the geometry of the molecule:$(a)$ Pentagonal planar geometry involves $sp^3d^3$ hybridization,which utilizes the $d_{z^2}$ orbital.$(b)$ Trigonal planar geometry involves $sp^2$ hybridization,which uses only $s$ and two $p$ orbitals $(p_x, p_y)$. Thus,the $d_{z^2}$ orbital is not involved.$(c)$ Linear geometry can involve $sp$ $(s+p_z)$,$sp^3d$ $(s+p_x+p_y+p_z+d_{z^2})$,or $sp^3d^2$ hybridization depending on the central atom's coordination.$(d)$ Square planar geometry typically involves $dsp^2$ or $sp^3d^2$ hybridization,where the $d_{x^2-y^2}$ or $d_{z^2}$ orbitals are involved.Therefore,the $d_{z^2}$ orbital is not required for the $sp^2$ hybridization of a trigonal planar molecule.

In which of the following molecular shapes must the $d_{z^2}$ orbital not be involved in bonding?

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