dit-pr bonding is shown in (a) P2 O3, P2 O5, PO4 ^3- (b) CO, NO, CO2, NO2 (c) NH3, PH3, BiH3 (d)

step 1 Among the given option here, among the given options here, D -P -P -P -P -P bonding is shown in

Dit-pr bonding is shown in (a) P2 O3, P2 O5, PO4 ^3- (b) CO,...

dit-pr bonding is shown in (a) $\mathrm{P}_{2} \mathrm{O}_{3}, \mathrm{P}_{2} \mathrm{O}_{5}, \mathrm{PO}_{4}{ }^{3}-$ (b) $\mathrm{CO}, \mathrm{NO}, \mathrm{CO}_{2}, \mathrm{NO}_{2}$ (c) $\mathrm{NH}_{3}, \mathrm{PH}_{3}, \mathrm{BiH}_{3}$ (d) $\mathrm{NO}_{3}^{-}, \mathrm{NO}_{2}-\mathrm{N}^{3-}, \mathrm{CN}^{-}$

dit-pr bonding is shown in
(a) $\mathrm{P}_{2} \mathrm{O}_{3}, \mathrm{P}_{2} \mathrm{O}_{5}, \mathrm{PO}_{4}{ }^{3}-$
(b) $\mathrm{CO}, \mathrm{NO}, \mathrm{CO}_{2}, \mathrm{NO}_{2}$
(c) $\mathrm{NH}_{3}, \mathrm{PH}_{3}, \mathrm{BiH}_{3}$
(d) $\mathrm{NO}_{3}^{-}, \mathrm{NO}_{2}-\mathrm{N}^{3-}, \mathrm{CN}^{-}$

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Key Concepts

Dative (Coordinate) Bonding

Dative bonding involves the formation of a covalent bond when one atom donates both electrons to the bond, typically bonding to an electron?deficient center. This concept is key in understanding many bonding situations in coordination chemistry and in molecules where electron pairs are not equally shared.

Pi Backbonding

Pi backbonding is a secondary bonding interaction where electron density is transferred from filled orbitals of one species into empty or partially filled pi* orbitals of an adjacent atom. This interaction supplements the primary sigma bond and can significantly influence the electronic structure and properties of the molecule.

Molecular Orbital Theory

Molecular orbital theory explains chemical bonding by describing how atomic orbitals combine to form molecular orbitals that are delocalized over a molecule. This theory is essential for understanding the formation of both sigma and pi bonds, including cases where one bonding component has a dative character, as it allows for analysis of bonding interactions and electron delocalization.

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