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explain different type of hybridizations and it's geometrical shapes?

sp3 hybridization

Type of hybrid Diagram Atomic orbitals used Number of hybrid orbitals formed Number of atoms bonded to the C Geometry
sp3 Diagram of sp3 hybrid orbitals. [62orb06a.JPG] s, p, p, p 4 4 tetrahedral

sp3 hybridization results from the combination of the s orbital and all three p orbitals in the second energy level of carbon. It results in four hybrid orbitals and occurs when a carbon atom is bonded to four other atoms. The geometric arrangement of those four hybrid orbitals is called tetrahedral.

sp2 hybridization

Type of hybrid Diagram Atomic orbitals used Number of hybrid orbitals formed Number of atoms bonded to the C Geometry
sp2 Diagram of sp2 hybrid orbitals. [62orb06b.JPG] s, p, p 3 3 flat triangular

Another kind of hybridization uses the s orbital and two of the p orbitals from the second energy level of carbon to form three hybrid orbitals. This kind of hybridization is called sp2 hybridization. It has three hybrid orbitals and there is also an unchanged p orbital that is not shown here. The geometric arrangement of these three sp2 hybrid orbitals is in a flat plane with 120 degree angles between them. The leftover p orbital lies at a 90 degree angle to the hybrid orbitals. If it had been included in this diagram, its two lobes would be pointing directly at and away from you. This kind of hybridization occurs when a carbon atom is bonded to three other atoms. If it is a very simple molecule with just the carbon atom and the other three atoms, it would be a flat triangular molecule. If this is part of a larger molecule, this part would have a flat triangular shape.

sp hybridization

Type of hybrid Diagram Atomic orbitals used Number of hybrid orbitals formed Number of atoms bonded to the C Geometry
sp Diagram of sp hybrid orbitals. [62orb06c.JPG] s, p 2 2 linear

There is still a third type of hybridization, it is sp hybridization. In it the s orbital and one of the p orbitals from carbon's second energy level are combined together to make two hybrid orbitals. Those hybrid orbitals form a straight line. There is a 180 degree angle between one orbital and the other orbital. They are exactly opposite one another from the center of the carbon atom. Because this type of sp hybridization only uses one of the p orbitals, there are still two p orbitals left which the carbon can use. Those p orbitals are at right angles to one another and to the line formed by the hybrid orbitals. If they were shown in this diagram, one would go straight up and down and the other would go straight toward and away from you. This kind of hybridization occurs when a carbon atom is bonded to two other atoms.



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