Alkenes in SP² Hybridization

Alkenes in SP² Hybridization Definition 

• Alkenes in SP² Hybridization, the carbon atoms involved in the double bond (C=C) undergo sp² hybridization, which determines their geometry and bonding characteristics.

1. Hybridization Process

1. Formation:

   • One s orbital and two p orbitals on a carbon atom hybridize to form three sp² orbitals.

2. Geometry:

   • The sp² orbitals arrange in a trigonal planar shape with bond angles of ~120°.

3. Sigma (σ) Bonds:

   • Each sp² carbon forms three σ bonds:
     • Two with carbon or hydrogen atoms.
     • One σ bond with the other carbon in the double bond.

2. Pi (π) Bond Formation

1. Unhybridized p Orbital:

   • The remaining p orbital (not involved in hybridization) is perpendicular to the sp² plane.

2. Double Bond Composition:

   • One σ bond (sp²–sp² overlap) and one π bond (side-to-side p orbital overlap).
   • The π bond restricts rotation, making the double bond rigid.

3. Example: Ethene (C₂H₄)

1. Hybridization:

   • Each carbon in ethene (ethylene) is sp² hybridized.

2. Bonding:

   • Each carbon forms:
     • Two σ bonds with hydrogen atoms.
     • One σ bond with the other carbon.
     • One π bond from p orbital overlap.

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