Chemistry Hybridization: Sigma, Pi Bonds and Sp3
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Questions and Answers

What is the shape of the molecule formed through sp3 hybridization?

  • Tetrahedral (correct)
  • Pentagonal bipyramidal
  • Trigonal bipyramidal
  • Octahedral
  • Which type of bond is formed by lateral overlap of atomic orbitals?

  • Single bond
  • Pi (π) bond (correct)
  • Sigma (σ) bond
  • Double bond
  • What is the shape of the molecule formed through spd2 hybridization?

  • Trigonal planar
  • Octahedral (correct)
  • Trigonal bipyramidal
  • Tetrahedral
  • What character does each sp3 hybrid orbital have?

    <p>25% s and 75% p</p> Signup and view all the answers

    What is the reason for sigma bonds being stronger than pi bonds?

    <p>Greater orbital overlap</p> Signup and view all the answers

    What is the shape of the molecule formed through sp2 hybridization?

    <p>Trigonal planar</p> Signup and view all the answers

    How many electron domains are required for spd hybridization?

    <p>Five</p> Signup and view all the answers

    What is the shape of the molecule formed through spd3 hybridization?

    <p>Pentagonal bipyramidal</p> Signup and view all the answers

    How many hybrid orbitals are formed in sp3 hybridization?

    <p>Four</p> Signup and view all the answers

    What type of bond is formed by head-on overlap of atomic orbitals?

    <p>Sigma (σ) bond</p> Signup and view all the answers

    Study Notes

    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

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    Description

    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.

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