**Branch :**First Year-Engineering Syllabus

**Subject :**Chemistry

## Hybridization

**Hybridization: **

Hybridization is a ubiquitous concept in molecular chemistry. A pictorial description runs like this. As four hydrogen approach a carbon atom, one of the 2s electrons of C gets "promoted" to a vacant 2p giving four unpaired electrons. These four orbitals rearrange into a regular tetrahedral arrangement and combine with the four 1s orbitals of the four hydrogens to give a tetrahedral CH_{4}. Remember orbitals are mathematical functions. In quantum chemistry (the subarea of chemistry which studies the bonding in molecules using quantum mechanical principles), the bonding MOs are calculated for the most stable configuration of a molecule and from these levels (when the results agree with spectroscopic and other thermal data), inferences regarding hybridization are conclusively drawn. In LiF we have already seen sp hybrids.

In H_{2}O we mentioned hybrids formed by combining one s and three p orbitals on O. These are referred to as sp^{3} hybrids. These occur in all saturated carbon compounds. The tetrahedral bonding in a saturated carbon atom is a result of this hybridization. The four combinations for the four sp^{3} hybrids are given below.

The angle between any two sp^{3} hybrids can be found by the same argument. Take two sp^{3} hybrids. Two unit vectors along the hybrids h_{1} and h_{2} are and . The dot product is -1/ 3 and cos ^{-1} (-1/ 3) = 109^{o} 28' which is the tetrahedral angle.

It should be noted that all hybrid combinations are not completely regular. E.g. in CH_{3}Br, the hybrid in the direction of Br is likely to be more directed (due to the electronegativity of Br) towards Br than the others towards hydrogens.

The next case of hybridization is sp2, which predominantly occurs in carbon compounds containing double bonds.The best example is ethene CH2 = CH2. Each carbon atom is "connected" to three "centers", one adjacent carbon and two hydrogens.

To get 3 equivalent orbitals in 3 directions in a plane, one s (2s) and two 2p (2p_{x} and 2p_{z}) orbitals in the xz plane are used. The three sp^{2} orbitals on the first carbon are:

Figure 1 Hybrid Orbitals.

Orbital h_{1} is directed towards the second carbon to its right. Orbitals h_{2} and h_{3} are directed towards negative z. To get the angle between the orbitals, treat the p orbitals as vectors. The s orbitals are spherically symmetrical and independent of direction. They are like scalars and do not contribute to directionality. If z axis is and x axis is , then the unit vectors corresponding to h_{2} and h_{3} are -1/ 2 and -1/ 2 -( ) . The dot product or cos ( , the angle between the two vectors) is ( 1/4-3/4).

Since cos = -1/ 2, = 120^{o}, which is the angle between the two sp^{2} hybrids. The same angle is found between any pair among the three hybrids. Among the four electrons in C, three can be placed, with one electron in each orbital to bind with an adjacent C or two hydrogens. All these three hybrid orbitals are in the molecular plane of C_{2}H_{4}. The fourth electron is in the p_{y} orbital which is in a plane perpendicular to the molecular plane. This electron binds with its counterpart on the other carbon atom to give a bond, which is the double bond in C_{2}H_{4}.