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Understanding Hybridization of Atomic Orbitals

May 6, 2025

Hybridization of Atomic Orbitals

What is Hybridization?

  • Hybridization: Combining atomic orbitals to form hybrid orbitals.
  • Example:
    • spĀ³ hybrid orbital is a combination of 1 s orbital and 3 p orbitals (sĀ¹pĀ³).
    • spĀ²: Combination of 1 s orbital and 2 p orbitals.
    • sp: Combination of 1 s orbital and 1 p orbital.
    • dĀ²spĀ³: Combination of 2 d orbitals, 1 s orbital, and 3 p orbitals.

Atomic Orbitals

  • s Orbital: Looks like a sphere; represents probability of finding an electron.
  • p Orbitals: Three types based on orientation:
    • pįµŖ: Along x-axis.
    • pįµ§: Along y-axis.
    • pš“: Along z-axis.

Hybridization in Carbon

  • Electron Configuration: 1sĀ² 2sĀ² 2pĀ².
  • Valence Electrons: 4 valence electrons.

spĀ³ Hybrid Orbital

  • Uses 4 orbitals (1 s and 3 p).
  • Character:
    • 25% s character (1 out of 4 is s).
    • 75% p character (3 out of 4 are p).
  • Energy Level: Closer to 2p due to higher p character.
  • Degenerate Orbitals: All have the same energy.

spĀ² Hybrid Orbital

  • Uses 3 orbitals (1 s and 2 p); 1 p remains unhybridized.
  • Character:
    • 33% s character (1 out of 3 is s).
    • 67% p character (2 out of 3 are p).
  • Energy Level: Closer to 2p than 2s, less p character than spĀ³.

sp Hybrid Orbital

  • Uses 2 orbitals (1 s and 1 p); 2 p orbitals remain unhybridized.
  • Character:
    • 50% s character.
    • 50% p character.
  • Energy Level: In between s and p orbitals.

Orbital Hybridization

  • Number of Hybrid Orbitals: Equals the number of atomic orbitals mixed.
  • Sigma Bonds:
    • Formed from hybrid orbitals.
    • Present in every single bond.
  • Pi Bonds:
    • Formed from unhybridized p orbitals.
    • Present in double and triple bonds.

Bond Strength and Length

  • Triple Bonds: Stronger and shorter than single bonds.
  • Sigma vs Pi Bonds:
    • Sigma bonds are stronger than pi bonds.
    • Easier to break a pi bond than a sigma bond.

Counting Sigma and Pi Bonds

  • Sigma Bonds: Every bond contains one sigma bond.
  • Pi Bonds: Every double bond has one pi bond.
  • Example: A structure with 7 bonds and 2 double bonds has 7 sigma bonds and 2 pi bonds.

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