sp hybrid

(noun)

an orbital formed between one s-orbital and one p-orbital

Related Terms

Examples of sp hybrid in the following topics:

  • sp Hybridization

    • In sp hybridization, the s orbital overlaps with only one p orbital.
    • Atoms that exhibit sp hybridization have sp orbitals that are linearly oriented; two sp orbitals will be at 180 degrees to each other.
    • Any central atom surrounded by just two regions of valence electron density in a molecule will exhibit sp hybridization.
    • Hybridization of an s orbital and a p orbital of the same atom produces two sp hybrid orbitals.
    • The right energy-level diagrams shows sp hybridized orbitals on Be in the linear BeCl2 molecule.

  • Hybridization in Molecules Containing Double and Triple Bonds

    • sp2, sp hybridizations, and pi-bonding can be used to describe the chemical bonding in molecules with double and triple bonds.
    • The hybrids are named for the atomic orbitals involved in the hybridization.
    • In this case, sp hybridization leads to two double bonds.
    • sp hybridization explains the chemical bonding in compounds with triple bonds, such as alkynes; in this model, the 2s orbital mixes with only one of the three p-orbitals, resulting in two sp orbitals and two remaining p-orbitals.
    • The sp hybridized orbitals are used to overlap with the 1s hydrogen orbitals and the other carbon atom.

  • sp2 Hybridization

    • In order to explain the bonding, the 2s orbital and two of the 2p orbitals (called sp2 hybrids) hybridize; one empty p-orbital remains.
    • sp2 Hybridization in Ethene and the Formation of a Double Bond
    • In this case, carbon will sp2 hybridize; in sp2 hybridization, the 2s orbital mixes with only two of the three available 2p orbitals, forming a total of three sp hybrid orbitals with one p-orbital remaining.
    • The carbon atoms are sp2 hybridized.
    • In sp^2 hybridization, the 2s orbital mixes with only two of the three available 2p orbitals, forming a total of three sp^2 orbitals with one p-orbital remaining.

  • Nucleophilic Addition Reactions & Reduction

    • The sp-hybrid carbon atoms of the triple-bond render alkynes more electrophilic than similarly substituted alkenes.
    • Isolated carbon double-bonds are not reduced by sodium in liquid ammonia, confirming the electronegativity difference between sp and sp2 hybridized carbons.

  • Substitution

    • Such addition-elimination processes generally occur at sp2 or sp hybridized carbon atoms, in contrast to SN1 and SN2 reactions.

  • Atomic and Molecular Orbitals

    • These hybrid orbitals have a specific orientation, and the four are naturally oriented in a tetrahedral fashion.
    • A mixing of the 2s-orbital with two of the 2p orbitals gives three sp2 hybrid orbitals, leaving one of the p-orbitals unused.
    • Two sp2 hybridized carbon atoms are then joined together by sigma and pi-bonds (a double bond), as shown in part B.
    • Finally, in the case of carbon atoms with only two bonding partners only two hybrid orbitals are needed for the sigma bonds, and these sp hybrid orbitals are directed 180º from each other.
    • Two p-orbitals remain unused on each sp hybridized atom, and these overlap to give two pi-bonds following the formation of a sigma bond (a triple bond), as shown below.

  • Double and Triple Covalent Bonds

    • Double and triple bonds can be explained by orbital hybridization, or the 'mixing' of atomic orbitals to form new hybrid orbitals.
    • Hybridization describes the bonding situation from a specific atom's point of view.
    • A combination of s and p orbitals results in the formation of hybrid orbitals.
    • Each carbon has two sp hybrid orbitals, and one of them overlaps with its corresponding one from the other carbon atom to form an sp-sp sigma bond.
    • A schematic of the resulting orientation in space of sp3 hybrid orbitals.

  • Basicity of Amines

    • The first of these is the hybridization of the nitrogen.
    • In pyridine the nitrogen is sp2 hybridized, and in nitriles (last entry) an sp hybrid nitrogen is part of the triple bond.

  • Carbonyl Compounds

    • As shown in the diagram below, two Lewis structures, differing in the hybridization of oxygen, may be drawn.
    • An sp2–sp sigma bond should be stronger and shorter than a sp2–sp2 sigma bond, and the shorter bond distance will enhance the pi-bonding.
    • The average values given in the following table indicate that C=C is 13% shorter and 76% stronger than a C–C bond, whereas C=O is 15% shorter and over 100% stronger than a C–O bond, possibly reflecting the sp hybridization of the oxygen.
    • In the sp2-oxygen model these occupy very similar (degenerate) orbitals, but in the sp-oxygen model one pair is in a relatively low energy sp-orbital and the other in a higher energy p-orbital.
    • The n → π* excited state shown in brackets at the center of the diagram may also be described as the resonance hybrid drawn below.

  • Solubility Product

    • $PbCl_2 \rightleftharpoons Pb^{2+} + 2Cl^- \text{ gives }\ K_{sp} = [Pb^{2+}][Cl^-]^2$