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Orbital Hybridization: Understanding Chemical Bonding

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Orbital hybridization is a fundamental concept in chemistry that explains how atomic orbitals merge to form hybrid orbitals, leading to the formation of σ- and π-bonds. It refines valence bond theory, accounting for the geometry and energy of bonds. Sp3, sp2, and sp hybridizations correspond to single, double, and triple bonds, shaping the molecular geometry into tetrahedral, trigonal planar, and linear forms, respectively.

Fundamentals of Orbital Hybridization in Chemical Bonding

Orbital hybridization is a key concept in chemical bonding that describes the merging of atomic orbitals to form new, equivalent hybrid orbitals conducive to bond formation. This theory refines the valence bond theory by explaining the geometry and energy equivalence of bonds in molecules. Valence bond theory identifies σ-bonds, which result from the head-on overlap of orbitals, and π-bonds, which form through the side-on overlap of orbitals. Hybridization accounts for molecular bonding patterns by combining s, p, and sometimes d orbitals to create hybrid orbitals such as sp3, sp2, and sp, corresponding to the formation of single, double, and triple bonds, respectively.
Molecular models of methane CH4 with tetrahedron of hydrogen atoms, ethene C2H4 with double bond and acetylene C2H2 with triple bond on neutral background.

The Role of sp3 Hybridization in Single Bonds

Sp3 hybridization occurs when one s-orbital and three p-orbitals from the same atom mix to yield four sp3 hybrid orbitals of equal energy. This process is essential for atoms like carbon in methane (CH4), enabling the formation of four equivalent bonds. In its ground state, carbon has two electrons in the 2s orbital and two in the 2p orbitals. Sp3 hybridization promotes one of the 2s electrons to the 2p level, resulting in four unpaired electrons that are then redistributed into the four sp3 orbitals. The tetrahedral arrangement of these orbitals, with bond angles of 109.5°, facilitates the formation of σ-bonds with hydrogen atoms.

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00

Hybrid orbitals like ______, ______, and ______ correspond to single, double, and triple bonds in molecules.

sp3

sp2

sp

01

Definition of sp3 hybridization

Mixing of one s-orbital and three p-orbitals to form four equivalent sp3 hybrid orbitals.

02

Electron configuration of carbon before sp3 hybridization

Ground state carbon has 2 electrons in 2s orbital and 2 in 2p orbitals.

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