Concept Of Hybridization Involving S, P And D Orbitals

Hybridisation (or hybridization) is the mathematical process of merging two or more atomic orbitals from the same atom to create a completely new orbital that is distinct from its constituents.

The energy levels of the original atomic orbitals are similar, but not identical (for example, a 2s orbital might hybridise with a 2p orbital). Different orbitals, such as the s, p, and d orbitals, are involved in hybridization.

The resulting hybrid orbitals have the same energy level as each other and are directed to establish bonds with other atoms.

Given the model’s shortcomings and the relative effectiveness of other models such as valence shell electron pair repulsion theory, there are reasons against teaching hybridised orbitals to general chemistry students as a way of understanding molecular bonding (VSEPR).

Definition of Hybridization

Hybridization is the process of combining atomic orbitals to create a new atomic orbital. The new orbital can hold the same number of electrons as the previous orbitals.The new, hybridised orbital characteristics and energy are a ‘average’ of the original unhybridized orbitals.

The best explanation for why all C – H bonds in molecules like methane are identical has been proposed: hybridization.

Example

Carbon atoms have the electron configuration 1s² 2s² 2p² in their normal state.

The four outermost electrons, found in the 2s and 2p sublevels, can establish chemical interactions with other atoms.

The 2s orbital may carry up to two electrons, and there are three 2p orbitals, each of which can hold up to two electrons, for a total of six electrons in the 2p orbitals.

These electron orbitals appear like this when seen individually. (Each is centred on the 

sp vs sp² vs sp³ Hybridization: What’s the Difference

Orbitals are hypothetical structures that could contain electrons. Scientists have hypothesised several geometries for these orbitals based on various discoveries. Atomic orbitals, molecular orbitals, and hybrid orbitals are the three primary types of orbitals. Hybridization of an atom’s atomic orbitals results in orbitals that are suited for chemical bonding. Hybridization is the process of combining various atomic orbitals to generate hybrid orbitals in chemistry. There are several types of hybridizations that result in different types of hybrid orbitals, such as sp, sp2, and sp3. Hybridization of s and p atomic orbitals in various ratios produces these orbitals. The main distinction between sp, sp², and sp3 hybridization is that sp hybridization produces hybrid orbitals with 50% s orbital characteristics,

sp² hybridization produces hybrid orbitals with 33% s orbital characteristics, and sp³ hybridization produces hybrid orbitals with 25% s orbital characteristics.

Hybrid Orbital

sp Hybridization

The hybridization of a s atomic orbital with a p atomic orbital is known as sp hybridization. Three p orbitals make up an electron shell. As a result, after the hybridization of a s orbital with one of these p orbitals, the atom still has two unhybridized p orbitals. All s and p orbitals are treated as atomic orbitals (s+p) in this case. The s and p orbitals have a 1:1 ratio. As a result, the s orbital fraction is 1/2, and the p orbital fraction is 1/2.

Total atomic orbitals x (1/2) x % = S (or p) characteristic percentage

= 50%

The hybrid orbitals that result have 50 percent s features and 50 percent p characteristics. The spatial arrangement of sp orbitals is linear since only two hybrid orbitals are created. The two hybrid orbitals are pointing in different directions. As a result, the angle formed by these orbitals is 180^o.

sp² Hybridization

One s atomic orbital is mixed with two p atomic orbitals in sp² hybridization. Sp² hybrid orbitals are the freshly generated hybrid orbitals. The hybrid orbitals that result have roughly 33.33 percent s characters and 66.66 percent p characters. This is because the hybridization involves three atomic orbitals in total, with the percentages of s and p properties varying as follows.

All s and p orbitals are treated as atomic orbitals (s+p+p) in this case. The s and p orbitals have a 1:2 ratio. As a result, the s orbital percentage is 1/3 and the p orbital fraction is 2/3.

Total atomic orbitals x (1/ 3) x 100 % S characteristic percentage

= 33.33 %

Total atomic orbitals x (2/ 3) x 100 %P characteristic proportion

= 66.66 %

The sp² hybrid orbitals have a trigonal planar spatial layout. As a result, the angle between these orbitals is 120^o. Because only two of the three p orbitals are engaged in this hybridization, the atoms that undergo it have one unhybridized p orbital.

 sp³ Hybridization

One’s atomic orbital is mixed with three p atomic orbitals in sp3 hybridization. Because all three p orbitals are involved in hybridization, the atoms do not have unhybridized p orbitals. The orbitals that result are referred to as sp3 hybrid orbitals. We can determine the s and p properties of these orbitals in the same way that we can for sp² orbitals.

All s and p orbitals are treated as atomic orbitals in sp³ hybridization (s+p+p+p). The s and p orbitals have a 1:3 ratio.  As a result, the s orbital fraction is ¼,and the p orbital fraction is ¾. 

Conclusion

Hybrid orbitals are the result of a model that combines atomic orbitals on a single atom in ways that result in a new set of orbitals with geometries suitable for forming bonds in the VSEPR model’s expected directions. The VSEPR model predicts geometries that are strikingly similar to those found in actual molecules.