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- https://chem.libretexts.org/Courses/Bellarmine_University/BU%3A_Chem_103_(Christianson)/Phase_3%3A_Atoms_and_Molecules_-_the_Underlying_Reality/10%3A_Molecular_Structure_and_Geometry/10.5%3A_Valence_Bond_TheoryA more sophisticated treatment of bonding is needed for systems such as these. In this section, we present a quantum mechanical description of bonding, in which bonding electrons are viewed as being l...A more sophisticated treatment of bonding is needed for systems such as these. In this section, we present a quantum mechanical description of bonding, in which bonding electrons are viewed as being localized between the nuclei of the bonded atoms. The overlap of bonding orbitals is substantially increased through a process called hybridization, which results in the formation of stronger bonds.
- https://chem.libretexts.org/Courses/Nassau_Community_College/General_Chemistry_1/05%3A_Advanced_Theories_of_Covalent_Bonding/5.03%3A_Hybrid_Atomic_OrbitalsWe can use hybrid orbitals, which are mathematical combinations of some or all of the valence atomic orbitals, to describe the electron density around covalently bonded atoms. These hybrid orbitals ei...We can use hybrid orbitals, which are mathematical combinations of some or all of the valence atomic orbitals, to describe the electron density around covalently bonded atoms. These hybrid orbitals either form sigma (σ) bonds directed toward other atoms of the molecule or contain lone pairs of electrons. We can determine the type of hybridization around a central atom from the geometry of the regions of electron density about it.
- https://chem.libretexts.org/Courses/University_of_Kentucky/UK%3A_General_Chemistry/08%3A_Advanced_Theories_of_Covalent_Bonding/8.2%3A_Hybrid_Atomic_OrbitalsWe can use hybrid orbitals, which are mathematical combinations of some or all of the valence atomic orbitals, to describe the electron density around covalently bonded atoms. These hybrid orbitals ei...We can use hybrid orbitals, which are mathematical combinations of some or all of the valence atomic orbitals, to describe the electron density around covalently bonded atoms. These hybrid orbitals either form sigma (σ) bonds directed toward other atoms of the molecule or contain lone pairs of electrons. We can determine the type of hybridization around a central atom from the geometry of the regions of electron density about it.
- https://chem.libretexts.org/Courses/Earlham_College/CHEM_361%3A_Inorganic_Chemistry_(Watson)/01%3A_Intro_Review_and_Effective_Nuclear_Charge/1.03%3A_Simple_Bonding_Theory/1.3.06%3A_Hybrid_Atomic_OrbitalsWe can use hybrid orbitals, which are mathematical combinations of some or all of the valence atomic orbitals, to describe the electron density around covalently bonded atoms. These hybrid orbitals ei...We can use hybrid orbitals, which are mathematical combinations of some or all of the valence atomic orbitals, to describe the electron density around covalently bonded atoms. These hybrid orbitals either form sigma (σ) bonds directed toward other atoms of the molecule or contain lone pairs of electrons. We can determine the type of hybridization around a central atom from the geometry of the regions of electron density about it.
- https://chem.libretexts.org/Courses/University_of_Florida/CHM2047%3A_One-Semester_General_Chemistry_(Kleiman)/06%3A_Understanding_Molecules_with_QM/6.10%3A_Valence_Bond_TheoryA more sophisticated treatment of bonding is needed for systems such as these. In this section, we present a quantum mechanical description of bonding, in which bonding electrons are viewed as being l...A more sophisticated treatment of bonding is needed for systems such as these. In this section, we present a quantum mechanical description of bonding, in which bonding electrons are viewed as being localized between the nuclei of the bonded atoms. The overlap of bonding orbitals is substantially increased through a process called hybridization, which results in the formation of stronger bonds.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/Map%3A_Chemistry_-_The_Central_Science_(Brown_et_al.)/09%3A_Molecular_Geometry_and_Bonding_Theories/9.04%3A_Covalent_Bonding_and_Orbital_OverlapA more sophisticated treatment of bonding is needed for systems such as these. In this section, we present a quantum mechanical description of bonding, in which bonding electrons are viewed as being l...A more sophisticated treatment of bonding is needed for systems such as these. In this section, we present a quantum mechanical description of bonding, in which bonding electrons are viewed as being localized between the nuclei of the bonded atoms. The overlap of bonding orbitals is substantially increased through a process called hybridization, which results in the formation of stronger bonds.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/Chemistry_2e_(OpenStax)/08%3A_Advanced_Theories_of_Covalent_Bonding/8.02%3A_Hybrid_Atomic_OrbitalsWe can use hybrid orbitals, which are mathematical combinations of some or all of the valence atomic orbitals, to describe the electron density around covalently bonded atoms. These hybrid orbitals ei...We can use hybrid orbitals, which are mathematical combinations of some or all of the valence atomic orbitals, to describe the electron density around covalently bonded atoms. These hybrid orbitals either form sigma (σ) bonds directed toward other atoms of the molecule or contain lone pairs of electrons. We can determine the type of hybridization around a central atom from the geometry of the regions of electron density about it.
- https://chem.libretexts.org/Courses/Prince_Georges_Community_College/CHEM_2000%3A_Chemistry_for_Engineers_(Sinex)/Unit_2%3A__Molecular_Structure/Chapter_5%3A_Molecular_Geometry/Chapter_5.2%3A_Localized_Bonding_and_Hybrid_OrbitalsThe only difference is that the C atom uses the four singly occupied sp 3 hybrid orbitals to form electron-pair bonds with only three H atoms, and an electron is added to the fourth hybrid orbital to ...The only difference is that the C atom uses the four singly occupied sp 3 hybrid orbitals to form electron-pair bonds with only three H atoms, and an electron is added to the fourth hybrid orbital to give a charge of 1–. The electron-pair geometry is tetrahedral, but the molecular geometry is pyramidal, as in NH 3 .
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/09%3A_Covalent_Bonding/9.22%3A_Hybrid_Orbitals_-_spThis page explores hybridization in chemistry, centering on carbon's bonding in methane (CH4. Despite its electron configuration indicating it should form only two bonds, carbon actually for...This page explores hybridization in chemistry, centering on carbon's bonding in methane (CH4. Despite its electron configuration indicating it should form only two bonds, carbon actually forms four through sp3 hybridization, which mixes one s and three p orbitals. This process results in four equivalent hybrid orbitals, accounting for methane's tetrahedral geometry and bond angles.
- https://chem.libretexts.org/Courses/Williams_School/Chemistry_IIA/01%3A_Molecular_Geometry_and_Bonding_Theories/1.05%3A_Hybrid_OrbitalsThe localized valence bonding theory uses a process called hybridization, in which atomic orbitals that are similar in energy but not equivalent are combined mathematically to produce sets of equivale...The localized valence bonding theory uses a process called hybridization, in which atomic orbitals that are similar in energy but not equivalent are combined mathematically to produce sets of equivalent orbitals that are properly oriented to form bonds. These new combinations are called hybrid atomic orbitals because they are produced by combining (hybridizing) two or more atomic orbitals from the same atom.
- https://chem.libretexts.org/Courses/Lafayette_College/CHEM_212_213%3A_Inorganic_Chemistry_(Nataro)/02%3A_Molecules/2.04%3A_Hybrid_OrbitalsBy the promotion of one of its 2s electrons to an unoccupied 2p orbital, however, followed by the hybridization of the three singly occupied orbitals (the 2s and two 2p orbitals), boron acquires a set...By the promotion of one of its 2s electrons to an unoccupied 2p orbital, however, followed by the hybridization of the three singly occupied orbitals (the 2s and two 2p orbitals), boron acquires a set of three equivalent hybrid orbitals with one electron each, as shown here:
