Search
- 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/1.3.05%3A_Valence_Bond_TheoryValence bond theory describes bonding as a consequence of the overlap of two separate atomic orbitals on different atoms that creates a region with one pair of electrons shared between the two atoms. ...Valence bond theory describes bonding as a consequence of the overlap of two separate atomic orbitals on different atoms that creates a region with one pair of electrons shared between the two atoms. When the orbitals overlap along an axis containing the nuclei, they form a σ bond. When they overlap in a fashion that creates a node along this axis, they form a π bond.
- https://chem.libretexts.org/Courses/Oregon_Institute_of_Technology/OIT%3A_CHE_333_-_Organic_Chemistry_III_(Lund)/New_Page/2%3A_Introduction_to_Organic_Structure_and_Bonding_II/2.1%3A_Valence_Bond_TheoryValence bond theory is most often used to describe bonding in organic molecules. In this model, bonds are considered to form from the overlap of two atomic orbitals on different atoms, each orbital c...Valence bond theory is most often used to describe bonding in organic molecules. In this model, bonds are considered to form from the overlap of two atomic orbitals on different atoms, each orbital containing a single electron. In looking at simple inorganic molecules such as molecular hydrogen (H2) or hydrogen fluoride (HF), our present understanding of s and p atomic orbitals will suffice. In order to explain the bonding in organic molecules, however, we will need to introduce hybrid orbitals
- https://chem.libretexts.org/Courses/CSU_San_Bernardino/CHEM_2100%3A_General_Chemistry_I_(Mink)/08%3A_Advanced_Theories_of_Covalent_Bonding/8.02%3A_Valence_Bond_TheoryValence bond theory describes bonding as a consequence of the overlap of two separate atomic orbitals on different atoms that creates a region with one pair of electrons shared between the two atoms. ...Valence bond theory describes bonding as a consequence of the overlap of two separate atomic orbitals on different atoms that creates a region with one pair of electrons shared between the two atoms. When the orbitals overlap along an axis containing the nuclei, they form a σ bond. When they overlap in a fashion that creates a node along this axis, they form a π bond.
- https://chem.libretexts.org/Bookshelves/Organic_Chemistry/Intermediate_Physical_Organic_(Morsch)/01%3A_Models_of_Chemical_Bonding/1.04%3A_Molecular_orbital_theory-_conjugation_and_aromaticityValence bond theory does a remarkably good job at explaining the bonding geometry of many of the functional groups in organic compounds. There are some areas, however, where the valence bond theory f...Valence bond theory does a remarkably good job at explaining the bonding geometry of many of the functional groups in organic compounds. There are some areas, however, where the valence bond theory falls short. It fails to adequately account, for example, for some interesting properties of compounds that contain alternating double and single bonds. In order to understand these properties, we need to think about chemical bonding in a new way, using the ideas of molecular orbital (MO) theory.
- https://chem.libretexts.org/Courses/Williams_School/Chemistry_IIA/01%3A_Molecular_Geometry_and_Bonding_Theories/1.07%3A_Molecular_OrbitalsA molecular orbital is an allowed spatial distribution of electrons in a molecule that is associated with a particular orbital energy. Unlike an atomic orbital, which is centered on a single atom, a m...A molecular orbital is an allowed spatial distribution of electrons in a molecule that is associated with a particular orbital energy. Unlike an atomic orbital, which is centered on a single atom, a molecular orbital extends over all the atoms in a molecule or ion. Hence the molecular orbital theory of bonding is a delocalized approach. Molecular orbitals are constructed using linear combinations of atomic orbitals (LCAOs), which describe overlapping atomic orbitals.
- https://chem.libretexts.org/Courses/Thompson_Rivers_University/CHEM_1500%3A_Chemical_Bonding_and_Organic_Chemistry/05%3A_Chemical_Bonding_II-_Molecular_Geometry_and_Hybridization_of_Atomic_Orbitals/5.02%3A_Valence_Bond_TheoryValence bond theory describes bonding as a consequence of the overlap of two separate atomic orbitals on different atoms that creates a region with one pair of electrons shared between the two atoms. ...Valence bond theory describes bonding as a consequence of the overlap of two separate atomic orbitals on different atoms that creates a region with one pair of electrons shared between the two atoms. When the orbitals overlap along an axis containing the nuclei, they form a σ bond. When they overlap in a fashion that creates a node along this axis, they form a π bond.
- https://chem.libretexts.org/Courses/Williams_School/Chemistry_I/06%3A_Chemical_Bonding_and_Molecular_Geometry/6.08%3A_Valence_Bond_TheoryValence bond theory describes bonding as a consequence of the overlap of two separate atomic orbitals on different atoms that creates a region with one pair of electrons shared between the two atoms. ...Valence bond theory describes bonding as a consequence of the overlap of two separate atomic orbitals on different atoms that creates a region with one pair of electrons shared between the two atoms. When the orbitals overlap along an axis containing the nuclei, they form a σ bond. When they overlap in a fashion that creates a node along this axis, they form a π bond.
- https://chem.libretexts.org/Courses/Oregon_Institute_of_Technology/OIT%3A_CHE_332_--_Organic_Chemistry_II_(Lund)/1%3A_Fall_term_review_sections/2%3A_Introduction_to_Organic_Structure_and_Bonding_II/2.2%3A_Molecular_orbital_theory-_conjugation_and_aromaticityValence bond theory does a remarkably good job at explaining the bonding geometry of many of the functional groups in organic compounds. There are some areas, however, where the valence bond theory f...Valence bond theory does a remarkably good job at explaining the bonding geometry of many of the functional groups in organic compounds. There are some areas, however, where the valence bond theory falls short. It fails to adequately account, for example, for some interesting properties of compounds that contain alternating double and single bonds. In order to understand these properties, we need to think about chemical bonding in a new way, using the ideas of molecular orbital (MO) theory.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/Chemistry_2e_(OpenStax)/08%3A_Advanced_Theories_of_Covalent_Bonding/8.01%3A_Valence_Bond_TheoryValence bond theory describes bonding as a consequence of the overlap of two separate atomic orbitals on different atoms that creates a region with one pair of electrons shared between the two atoms. ...Valence bond theory describes bonding as a consequence of the overlap of two separate atomic orbitals on different atoms that creates a region with one pair of electrons shared between the two atoms. When the orbitals overlap along an axis containing the nuclei, they form a σ bond. When they overlap in a fashion that creates a node along this axis, they form a π bond.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/ChemPRIME_(Moore_et_al.)/07%3A_Further_Aspects_of_Covalent_Bonding/7.08%3A_Sigma_and_Pi_BondsEach of the two electrons in the pi bond (π bond) exists both above and below the plane of the four H atoms and the two C atoms. In actual fact the difference between the two models of the double bond...Each of the two electrons in the pi bond (π bond) exists both above and below the plane of the four H atoms and the two C atoms. In actual fact the difference between the two models of the double bond (the first model described here and the second found in the section on Orbital Descriptions of Multiple Bonds) is more apparent than real.
- https://chem.libretexts.org/Courses/Centre_College/CHE_332%3A_Inorganic_Chemistry/04%3A_Molecular_Orbitals/4.02%3A_Molecular_Orbital_Theory_of_Diatomic_Molecules/4.2.01%3A_Orbital_OverlapIn the molecular orbital diagram the energy difference between the bonding MO and the atomic orbitals is about the same as the energy difference between the anti-bonding MO and the atomic orbitals. Th...In the molecular orbital diagram the energy difference between the bonding MO and the atomic orbitals is about the same as the energy difference between the anti-bonding MO and the atomic orbitals. The bonding and the antibonding interactions only do not cancel out if the left 1s orbital has the same phanse as the left lobe of the 2p x orbital and the right 1s orbital has the same phase as the right lobe of the 2p x orbital.
