Chemistry Hybridization: Sigma, Pi Bonds and Sp3

Hybridization in Chemistry

Sigma and Pi Bonds

• Sigma (σ) bonds: formed by head-on overlap of atomic orbitals, resulting in a cylindrical shape
• Pi (π) bonds: formed by lateral overlap of atomic orbitals, resulting in a nodal plane
• Sigma bonds are stronger than pi bonds due to greater orbital overlap
• Multiple bonds (double, triple) contain one sigma bond and one or two pi bonds

Sp3 Hybridization

• Sp3 hybridization occurs when an atom has four electron domains (e.g., methane, CH4)
• The s orbital and three p orbitals mix to form four equivalent hybrid orbitals
• Each sp3 hybrid orbital has 25% s character and 75% p character
• The resulting molecule has a tetrahedral shape

spd, spd2, sp2, and spd3 Hybridization

• spd Hybridization: occurs when an atom has five electron domains (e.g., phosphorus, PF5)
  • The s orbital, three p orbitals, and one d orbital mix to form five hybrid orbitals
  • The resulting molecule has a trigonal bipyramidal shape
• spd2 Hybridization: occurs when an atom has six electron domains (e.g., sulfur, SF6)
  • The s orbital, three p orbitals, and two d orbitals mix to form six hybrid orbitals
  • The resulting molecule has an octahedral shape
• sp2 Hybridization: occurs when an atom has three electron domains (e.g., ethene, C2H4)
  • The s orbital and two p orbitals mix to form three hybrid orbitals
  • The resulting molecule has a trigonal planar shape
• spd3 Hybridization: occurs when an atom has seven electron domains (e.g., iodine, IF7)
  • The s orbital, three p orbitals, and three d orbitals mix to form seven hybrid orbitals
  • The resulting molecule has a pentagonal bipyramidal shape

Sigma and Pi Bonds

• Sigma bonds are formed by head-on overlap of atomic orbitals, resulting in a cylindrical shape
• Pi bonds are formed by lateral overlap of atomic orbitals, resulting in a nodal plane
• Sigma bonds are stronger than pi bonds due to greater orbital overlap
• Multiple bonds (double, triple) contain one sigma bond and one or two pi bonds

Sp3 Hybridization

• Sp3 hybridization occurs when an atom has four electron domains (e.g., methane, CH4)
• The s orbital and three p orbitals mix to form four equivalent hybrid orbitals
• Each sp3 hybrid orbital has 25% s character and 75% p character
• The resulting molecule has a tetrahedral shape

Other Hybridizations

• spd Hybridization: occurs when an atom has five electron domains (e.g., phosphorus, PF5)
• The s orbital, three p orbitals, and one d orbital mix to form five hybrid orbitals
• The resulting molecule has a trigonal bipyramidal shape
• spd2 Hybridization: occurs when an atom has six electron domains (e.g., sulfur, SF6)
• The s orbital, three p orbitals, and two d orbitals mix to form six hybrid orbitals
• The resulting molecule has an octahedral shape
• sp2 Hybridization: occurs when an atom has three electron domains (e.g., ethene, C2H4)
• The s orbital and two p orbitals mix to form three hybrid orbitals
• The resulting molecule has a trigonal planar shape
• spd3 Hybridization: occurs when an atom has seven electron domains (e.g., iodine, IF7)
• The s orbital, three p orbitals, and three d orbitals mix to form seven hybrid orbitals
• The resulting molecule has a pentagonal bipyramidal shape

Learn about the formation of sigma and pi bonds in chemistry, their differences, and the concept of sp3 hybridization. Understand the characteristics of single, double, and triple bonds.