Hybridization

1. Carbon configuration Hybridization Carbon in excited state can form 4 bonds

2. Hybrid orbital= an orbital created by the combination of atomic orbitals in the same atom 1 orbital s + 3 orbitals p= sp3 Form 4 hybrid orbitals with a tetrahedral arrangement

3. Energy changes occurring in hybridization • Hybridization of an s orbital with all three p orbitals (px , py, and pz) results in four sp3 hybrid orbitals. sp3 hybrid orbitals are oriented at bond angle of 109.5 degrees from each other. This 109.5 degree arrangement gives tetrahedral geometry

4. C in alkanes has a sp3 hybridation ethane methane

5. sp3 Hybridization in Methane • Carbon's 2s and all three of its 3p orbitals hybridize to form four sp3 orbitals. These orbitals then bond with four hydrogen atoms through sp3-s orbital overlap, creating methane. The resulting shape is tetrahedral, since that minimizes electron repulsion.

6. sp2 hybridization • Hybridization of an s orbital with two p orbitals (px and py) results in three sp2 hybrid orbitals that are oriented at 120o angle to each other. Sp2 hybridization results in trigonal geometry.

7. 1 orbital s + 2 p = 3sp2 Form 3 hybrid orbitals with a 120° angle With orbital p remained this C can arrange a double bond characteristic of alkenes (ethene)

8. sp2 Hybridization in Ethene • These hybridized orbitals align themselves in the trigonal planar structure. • For each carbon, two of these sp orbitals bond with two 1s hydrogen orbitals through s-sp orbital overlap.

9. The atoms that form the double bond cannot move in space unlike the single one. The double bond is very reactive and it can produce alkanes or alcohol by way of the addition reaction

10. sp Hybridization • In it, the 2s orbital and one of the 2p orbitals hybridize to form two sp orbitals, each consisting of 50% s and 50% p character.  • The front lobes face away from each other and form a straight line leaving a 180° angle between the two orbitals

11. Form 2 hybrid orbitals with a 180° angle 1 orbital s + 1 p = 2sp Two orbitals direct perpendicularly remain available. So the molecule can form a triple bond

12. The triple bond is characteristic of alkynes like ethine Sigma bond= covalent bond formed by overlap of atomic orbitals along the bond axis Pi bond= a bond formed by the overlap of p orbitals on adjacent atoms, perpendicular to any sigma bond

13. sp Hybridization in Ethyne • The first bond consists of sp-sp orbital overlap between the two carbons. Another two bonds consist of s-sp orbital overlap between the sp hybridized orbitals of the carbons and the 1s orbitals of the hydrogens.