- Describe the role of hybridization in the formation of double and triple bonds.
- A new hybrid orbital forms when atomic orbitals are mixed; this process is called hybridization.
- The bonding in ethene (which contains a C=C) occurs due to sp2 hybridization in each of the carbon atoms.
- Molecules with triple bonds, such as acetylene, have two pi bonds and one sigma bond.
- double bonda covalent bond in which two electron pairs (instead of the usual one) are shared between two atoms; most common between carbon atoms and carbon, oxygen, or nitrogen atoms
- pi bondcovalent chemical interactions where two lobes of one involved atomic (p) orbital overlap two lobes of the other involved atomic (p) orbital
- triple bonda covalent bond in which three electron pairs (instead of the usual one) are shared between two atoms; most common between carbon atoms and carbon or nitrogen atoms; symbolized in formulae as ≡
- hybridisationmixing atomic orbitals to form new hybrid orbitals suitable for the qualitative description of atomic bonding properties
In chemistry, hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals suitable for describing bonding properties. Hybridized orbitals are very useful in explaining of the shape of molecular orbitals for molecules, and are an integral part of valence bond theory.
The hybrids are named for the atomic orbitals involved in the hybridization. In methane (CH4) for example, a set of sp3 orbitals forms by mixing one s- and three p-orbitals on the carbon atom. The orbitals are directed toward the four hydrogen atoms, which are located at the vertices of a regular tetrahedron.
Ethene (C2H4) has a double bond between the carbons. For this molecule, carbon will sp2 hybridize. In sp2 hybridization, the 2s orbital mixes with only two of the three available 2p orbitals, forming a total of 3 sp2 orbitals with one p-orbital remaining. In ethylene (ethene), the two carbon atoms form a sigma bond by overlapping two sp2 orbitals; each carbon atom forms two covalent bonds with hydrogen by s–sp2 overlapping all with 120° angles. The pi bond between the carbon atoms forms by a 2p-2p overlap. The hydrogen-carbon bonds are all of equal strength and length, which agrees with experimental data.
Multiple bonds can also occur between dissimilar atoms. When the two O-atoms are brought up to opposite sides of the carbon atom in carbon dioxide, one of the p orbitals on each oxygen forms a pi bond with one of the carbon p-orbitals. 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 chemical bonding in acetylene (ethyne) (C2H2) consists of sp-sp overlap between the two carbon atoms forming a sigma bond, as well as two additional pi bonds formed by p-p overlap. Each carbon also bonds to hydrogen in a sigma s-sp overlap at 180° angles.
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