Hybridization

HYBRIDIZATION

  • The process of combining two atomic orbitals to create new hybridized orbitals.

  • Results in hybrid orbitals with different energies and shapes.

  • Primarily involves atomic orbitals of the same energy level.

ORBITALS HYBRID

  • New orbitals formed through hybridization.

  • Explain atomic bonding properties and molecular geometry.

  • Example: Carbon forms four sp3 hybrid orbitals, arranged tetrahedrally around the carbon atom which creates bonds with four different atoms.

FEATURES OF HYBRIDIZATION

  • Occurs between atomic orbitals with equal energies.

  • Number of hybrid orbitals formed equals the number of orbitals that mix.

  • Even filled orbitals can participate.

  • Only occurs during bond formation.

  • Knowing the hybridization allows prediction of molecular shapes.

  • Larger lobe of hybrid orbital is positive, smaller lobe is negative.

TYPES OF HYBRIDIZATION

  • Classified as sp3, sp2, sp, sp3d, sp3d2, or sp3d3 based on orbitals involved in mixing.

SHAPES OF HYBRIDIZED ORBITALS

  1. Linear (sp): 180° angle; results from 2 electron groups.

  2. Trigonal Planar (sp2): 120° angle; results from 3 electron groups.

  3. Tetrahedral (sp3): 109.5° angle; results from 4 electron groups.

  4. Trigonal Bipyramidal (sp3d): 90° and 120° angles; results from 5 groups.

  5. Octahedral (sp3d2): 90° angle; results from 6 groups.

SP HYBRIDIZATION

  • Formed by one s and one p orbital combining to create two sp orbitals.

  • Produces linear molecules at a 180° angle.

  • Example: Beryllium compounds (e.g., BeF2, BeH2).

EXAMPLE: BeF2

  • In BeF2, sp-hybridized orbitals of Be overlap with fluorine's orbitals, creating a linear shape.

SP2 HYBRIDIZATION

  • Combines one s and two p orbitals to form three equivalent sp2 orbitals.

  • Also known as trigonal hybridization, with 120° angles.

  • Example: Boron compounds.

EXAMPLE: BF3

  • In BF3, sp2 hybridized orbitals of B create σ-bonds with fluorine at 120°, resulting in a trigonal planar shape.

SP3 HYBRIDIZATION

  • Combines one s orbital and three p orbitals to form four sp3 hybrid orbitals.

  • Arranged tetrahedrally with angles of 109.5°.

  • Example: Methane (CH4) where sp3 orbitals overlap with hydrogen's 1s orbitals to form a symmetrical tetrahedral molecule.