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  2. Valence bond theory - Wikipedia

    en.wikipedia.org/wiki/Valence_bond_theory

    For example, in the case of the F 2 molecule, the F−F bond is formed by the overlap of p z orbitals of the two F atoms, each containing an unpaired electron. Since the nature of the overlapping orbitals are different in H 2 and F 2 molecules, the bond strength and bond lengths differ between H 2 and F 2 molecules.

  3. Modern valence bond theory - Wikipedia

    en.wikipedia.org/wiki/Modern_valence_bond_theory

    In the specific case of H 2, λ ≈ 0.75, and μ ≈ 0.25. The orbitals that were used as the basis (a and b) do not necessarily have to be localized on the atoms involved in bonding. Orbitals that are partially delocalized onto the other atom involved in bonding can also be used, as in the Coulson-Fischer theory .

  4. VSEPR theory - Wikipedia

    en.wikipedia.org/wiki/VSEPR_theory

    Another example is O(SiH 3) 2 with an Si–O–Si angle of 144.1°, which compares to the angles in Cl 2 O (110.9°), (CH 3) 2 O (111.7°), and N(CH 3) 3 (110.9°). [24] Gillespie and Robinson rationalize the Si–O–Si bond angle based on the observed ability of a ligand's lone pair to most greatly repel other electron pairs when the ligand ...

  5. Molecular orbital theory - Wikipedia

    en.wikipedia.org/wiki/Molecular_orbital_theory

    The MOT explains the paramagnetic nature of O 2, which valence bond theory cannot explain. ... This page was last edited on 22 October 2024, at 12:43 (UTC).

  6. Branches of physics - Wikipedia

    en.wikipedia.org/wiki/Branches_of_physics

    The theory is based on two postulates: (1) that the mathematical forms of the laws of physics are invariant in all inertial systems; and (2) that the speed of light in vacuum is constant and independent of the source or observer. Reconciling the two postulates requires a unification of space and time into the frame-dependent concept of spacetime.

  7. Crystal field theory - Wikipedia

    en.wikipedia.org/wiki/Crystal_field_theory

    The lower energy orbitals will be d z 2 and d x 2-y 2, and the higher energy orbitals will be d xy, d xz and d yz - opposite to the octahedral case. Furthermore, since the ligand electrons in tetrahedral symmetry are not oriented directly towards the d-orbitals, the energy splitting will be lower than in the octahedral case.

  8. Mathematical formulation of the Standard Model - Wikipedia

    en.wikipedia.org/wiki/Mathematical_formulation...

    This article describes the mathematics of the Standard Model of particle physics, a gauge quantum field theory containing the internal symmetries of the unitary product group SU(3) × SU(2) × U(1). The theory is commonly viewed as describing the fundamental set of particles – the leptons , quarks , gauge bosons and the Higgs boson .

  9. Bell's theorem - Wikipedia

    en.wikipedia.org/wiki/Bell's_theorem

    Bell's theorem is a term encompassing a number of closely related results in physics, all of which determine that quantum mechanics is incompatible with local hidden-variable theories, given some basic assumptions about the nature of measurement.