In the following, which species does not contain \[s{{p}^{3~}}\] hybridization?
A. \[N{{H}_{3}}\] ​
B. \[C{{H}_{4}}\]​
C. \[{{H}_{2}}O\]
D. \[C{{O}_{2}}\]

Hint: In chemistry, hybridization is the idea of combining two atomic orbitals to create a brand-new category of hybridised orbitals. Typically, this mixing creates hybrid orbitals with completely distinct energies, morphologies, etc. In hybridization, the same-energy level atomic orbitals are primarily involved. However, assuming they contain equal energy, both fully filled and partially filled orbitals can participate in this process.

Complete step-by-step answer:When two atomic orbitals join to generate a hybrid orbital in a molecule, the energy of the individual atoms' orbitals is redistributed to give orbitals of equivalent energy. We refer to this process as hybridization. The atomic orbitals with equivalent energies are mixed together during the hybridization process, which primarily involves the fusion of two s orbitals, two p orbitals, or the mixing of a s orbital with a p orbital or a d orbital. Hybrid orbitals are the new orbitals that are created in this way. More importantly, hybrid orbitals are very helpful in describing the characteristics of atomic bonds and molecular geometry.
A. The 2s and 2p orbitals in the ammonia molecule combine to form four \[s{{p}^{3~}}\] hybrid orbitals, one of which is filled by a single electron pair.
B. A single 2s orbital and three 2p orbitals of the carbon combine to generate four \[s{{p}^{3~}}\] orbitals, which together form the bonds in a methane molecule.
C. Water contains 8 valence electrons (2(1) + 6). Tetrahedral electron pair arrangements around the O atom in water call for \[s{{p}^{3~}}\] hybridization. The two lone pairs on oxygen are held in two of the four \[s{{p}^{3~}}\] hybrid orbitals, while the other two are utilised to create bonds with the two hydrogen atoms.
D. The main hybridization type of carbon dioxide is sp. Carbon forms 2 double bonds with two oxygen atoms. IT has a linear structure.

Option ‘D ’ is correct

Note: Atomic orbitals with comparable energies hybridise.
The number of atomic orbitals mixing equals the number of hybrid orbitals that are created.
Not every orbital with half of its volume filled must participate in hybridization. Orbitals that are fully filled and have somewhat varying energies can also take part.
Only when a bond is formed does hybridization take place, not when a gaseous atom is left alone.
If the molecule's hybridization is known, the shape of the molecule can be predicted.
In a hybrid orbital, the larger lobe is always positive while the smaller lobe on the other side is always negative.