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Valence Bond Theory

bond polarity - measure of electron sharing

  • overall dipole = sum of bond dipoles
    • dipoles have magnitude/direction
    • consider shape to find overall polarity
  • nonpolar molecule - overall dipole moment of 0
    • bond dipoles cancel each other out
  • polar molecule - nonzero overall dipole moment
    • when molecule not the same all around

valence-bond theory - explains covalent bonding

  • orbitals overlap to form covalent bonds
  • optimum distance between bonded nuclei
  • bond length - distance where attractive forces (between electrons/nuclei) are balanced by repulsive forces (between electrons/electrons, nuclei/nuclei)

hybrid orbitals - new orbitals formed by a mix of other orbitals

  • hybridization - process of mixing/changing atomic orbitals
  • energy released by bond formation > energy needed to promote electrons to higher levels
  • sp hybrid orbital - 1 electron from s subshell promoted to p subshell
    • able to form 2 bonds
    • forms linear arrangement
  • sp2 hybrid orbital - 1 electron from s subshell promoted to p subshell
    • 1 electron in s subshell, 2 electrons in p subshell
    • forms trigonal planar arrangement
  • sp3 hybrid orbital - 1 electron from s subhsell promoted to fill p subshell
    • forms tetrahedral arrangement
  • hybridization w/ d orbitals - possible w/ atoms in 3 rd period and beyond
    • sp3d hybrid orbital - trigonal bipyramidal arrangement
    • sp3d2hybrid orbital - octahedron arrangement
Subject: 
Chemistry
Subject X2: 
Chemistry

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