![]() ![]() Hybridization of the 2s and all three 2p AOs forms four sp 3 hybrid orbitals, oriented 109.5° with respect to each other (move the slider around to see the before/after of hybridization). The sp 3 hybrid orbitals are higher in energy than the sp 2 hybrid orbitals, as illustrated in Figure 4.įigure 4. The angle between any two bonds is 109.5 degrees.Īn sp 3 hybrid orbital has 75% “ p” character and 25% “ s” character, a 3:1 ratio, hence the superscript “3” in its name. These hybrid orbitals form four bonds that point toward each corner of a tetrahedron. Four sp 3 hybridized orbitals point from the tetrahedron’s center toward the four corners. Three views of a tetrahedron are shown at left. A tetrahedron has four equilateral triangular sides and four apexes (corners). The four sp 3 hybridized orbitals are oriented at 109.5° with respect to each other, each pointing toward a different corner of a tetrahedron-a tetrahedral geometry.Ī tetrahedron is a three-dimensional object that has four equilateral triangular faces and four apexes (corners). Hybridization of the 2s and two of the 2p AOs forms three sp 2 hybrid orbitals, oriented 120° with respect to each other in the same plane one of the 2p AOs remain unhybridized (move the slider around to see the before/after of hybridization).Ĭombining one valence s AO and all three valence p AOs produces four degenerate sp 3 hybridized orbitals, as shown in Figure 4 for the case of 2 s and 2p AOs. Energetically, sp 2 hybrid orbitals lie closer to the p AO than the s AO, as illustrated in Figure 2 (the sp 2 hybrid orbitals are higher in energy than the sp hybrid orbitals).įigure 2. ![]() The sp 2 hybrid orbitals have twice as much “ p” character as “ s” character this is indicated by the superscript “2” in sp 2. After hybridization, there is one unhybridized 2 p AO left on the atom. Each hybrid orbital is pointed toward a different corner of an equilateral triangle. The three sp 2 hybrid orbitals are oriented at 120° with respect to each other and are in the same plane-a trigonal planar (or triangular planar) geometry. However, in a covalent molecule, the one large lobe of each sp hybrid orbital gives greater overlap with another orbital from another atom, yielding σ bonds that lower the molecule’s energy.Ĭombining one valence s AO and two valence p AOs produces three degenerate sp 2 hybrid orbitals, as shown in Figure 2 for the case of 2 s and 2p AOs. For example, a beryllium atom is lower in energy with its two valence electrons in the 2 s AO than if the electrons were in the two sp hybrid orbitals. The hybridized orbitals are not energetically favorable for an isolated atom. (Move the slider to see the before/after of hybridization). Hybridization of the 2s and one of the 2p AOs forms two sp hybrid orbitals, oriented 180° with respect to each other the two other 2p AOs remain unhybridized. From the local 3D geometry of each atom, we can obtain the overall 3D geometry of the molecule.įigure 1.The type of hybrid orbitals for each atom can be determined from the Lewis structure (or resonance structures) of a molecule.The type of hybrid orbitals for each bonded atom in a molecule correlates with the local 3D geometry of that atom.The number of hybrid orbitals equals the number of valence AOs that were combined to produce the hybrid orbitals. ![]() Most π bonds are formed from overlap of unhybridized AOs.
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