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Chemistry LibreTexts

Hybridization II

  • Page ID
    25293
  • For polyatomic molecules we would like to be able to explain:

    • The number of bonds formed
    • Their geometries

    sp Hybrid Orbitals

    Consider the Lewis structure of gaseous molecules of BeF2:

    • The VSEPR model predicts this structure will be linear
    • What would valence bond theory predict about the structure?

    The fluorine atom electron configuration:

    • 1s22s22p5

    • There is an unpaired electron in a 2p orbital
    • This unpaired 2p electron can be paired with an unpaired electron in the Be atom to form a covalent bond

    The Be atom electron configuration:

    • 1s22s2

    • In the ground state, there are no unpaired electrons (the Be atom is incapable of forming a covalent bond with a fluorine atom
    • However, the Be atom could obtain an unpaired electron by promoting an electron from the 2s orbital to the 2p orbital:

    This would actually result in two unpaired electrons, one in a 2s orbital and another in a 2p orbital

    • The Be atom can now form two covalent bonds with fluorine atoms
    • We would not expect these bonds to be identical (one is with a 2s electron orbital, the other is with a 2p electron orbital)

    However, the structure of BeF2 is linear and the bond lengths are identical

    • We can combine wavefunctions for the 2s and 2p electrons to produce a "hybrid" orbital for both electrons
    • This hybrid orbital is an "sp" hybrid orbital

    • The orbital diagram for this hybridization would be represented as:

    Note:

    • The Be 2sp orbitals are identical and oriented 180° from one another (i.e. bond lengths will be identical and the molecule linear)
    • The promotion of a Be 2s electron to a 2p orbital to allow sp hybrid orbital formation requires energy.
      • The elongated sp hybrid orbitals have one large lobe which can overlap (bond) with another atom more effectively
      • This produces a stronger bond (higher bond energy) which offsets the energy required to promote the 2s electron

    sp2 and sp3 Hybrid Orbitals

    Whenever orbitals are mixed (hybridized):

    • The number of hybrid orbitals produced is equal to the sum of the orbitals being hybridized
    • Each hybrid orbital is identical except that they are oriented in different directions

    BF3

    Boron electron configuration:

    • The three sp2 hybrid orbitals have a trigonal planar arrangement to minimize electron repulsion

    Note

    sp2 refers to a hybrid orbital being constructed from one s orbital and two p orbitals. Although it looks like an electron configuration notation, the superscript '2' DOES NOT refer to the number of electrons in an orbital.

    • An s orbital can also mix with all 3 p orbitals in the same subshell

    CH4

    • Thus, using valence bond theory, we would describe the bonds in methane as follows: each of the carbon sp3 hybrid orbitals can overlap with the 1s orbitals of a hydrogen atom to form a bonding pair of electrons
    Note

    sp3 refers to a hybrid orbital being constructed from one s orbital and three p orbitals. Although it looks like an electron configuration notation, the superscript '3' DOES NOT refer to the number of electrons in an orbital.

    Note

    The two steps often observed when constructing hybrid orbitals is to

    1. promote a valence electron from the ground state configuration to a higher energy orbital, and then
    2. hybridize the appropriate valence electron orbitals to achieve the desired valence electron geometry (i.e. the correct number of hybrid orbitals for the appropriate valence electron geometry)

    H2O

    Oxygen

    Hybridization Involving d Orbitals

    Atoms in the third period and higher can utilize d orbitals to form hybrid orbitals

    PF5

    Similarly hybridizing one s, three p and two d orbitals yields six identical hybrid sp3d2 orbitals. These would be oriented in an octahedral geometry.

    • Hybrid orbitals allows us to use valence bond theory to describe covalent bonds (sharing of electrons in overlapping orbitals of two atoms)
    • When we know the molecular geometry, we can use the concept of hybridization to describe the electronic orbitals used by the central atom in bonding

    Steps in predicting the hybrid orbitals used by an atom in bonding:

    1. Draw the Lewis structure

    2. Determine the electron pair geometry using the VSEPR model

    3. Specify the hybrid orbitals needed to accommodate the electron pairs in the geometric arrangement

    NH3

    1. Lewis structure

    2. VSEPR indicates tetrahedral geometry with one non-bonding pair of electrons (structure itself will be trigonal pyramidal)

    3. Tetrahedral arrangement indicates four equivalent electron orbitals

    Valence Electron Pair Geometry

    Number of Orbitals

    Hybrid Orbitals

    Linear

    2

    sp

    Trigonal Planar

    3

    sp2

    Tetrahedral

    4

    sp3

    Trigonal Bipyramidal

    5

    sp3d

    Octahedral

    6

    sp3d2