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The 67 pages that link to Molecular orbital theory, each with the reason it gives.

• Covalent bondCompared with: It explains shared bonding electrons as molecular orbitals rather than localized pairs.

• Electron configurationNarrower topic: Molecular configurations extend orbital occupancy beyond isolated atoms.

• Molecular geometryRelated: Its delocalized orbitals explain bonding and shapes that localized bond pictures cannot fully capture.

• Chemical bondRelated: It explains bonding through molecular-wide electron states rather than localized pairs.

• Atomic orbitalCompared with: It contrasts with localized bonding pictures by combining atomic states into delocalized molecular states.

• Lewis structureCompared with: It models delocalized electrons beyond the localized pairs drawn in Lewis structures.

• ResonanceCompared with: It explains delocalized electrons directly rather than representing them with Lewis contributors.

• Crystal field theoryNarrower topic: Its delocalized orbitals provide a broader framework for interpreting metal–ligand bonding.

• Valence bond theoryCompared with: It contrasts with valence bond theory’s localized bonds by treating molecular orbitals as delocalized.

• Aufbau principleCompared with: Molecules fill molecular orbitals rather than the atom-centered orbitals targeted by this principle.

• Metallic bondingRelated: Its delocalized-orbital picture connects metallic bonding with quantum descriptions of molecules.

• Hückel's ruleNarrower topic: Hückel's rule follows from the energy levels of cyclic molecular orbitals.

• Bond orderNarrower topic: Its bonding-minus-antibonding electron count gives the standard molecular definition of bond order.

• Octet ruleCompared with: It explains bonding and stability without requiring each atom to satisfy a localized octet.

• Ligand field theoryRelated: Ligand field theory uses molecular-orbital ideas to account for covalent metal–ligand bonding.

• Physical chemistryRelated: It accounts for molecular bonding and electronic properties using quantum principles.

• MoleculeRelated: It explains bonding through electron states extending over the molecule.

• Frontier molecular orbital theoryNarrower topic: Frontier-orbital theory selects particular molecular orbitals from this broader framework.

• Bond angleRelated: Its orbital picture offers a deeper account of bonding directions and molecular geometry.

• HyperconjugationNarrower topic: It describes hyperconjugation as mixing and delocalization among molecular orbitals.

• VSEPR theoryCompared with: It provides a more detailed electronic account than VSEPR’s shape rules.

• Hybrid orbitalCompared with: It explains bonding without requiring localized hybrid orbitals as fundamental entities.

• Tight-binding modelNarrower topic: Tight binding carries orbital-combination reasoning from molecules into periodic lattices.

• Singlet oxygenNarrower topic: It explains oxygen’s electronic configurations and why its ground state has unpaired electrons.

• Bent's ruleCompared with: It explains bonding without requiring Bent's localized hybrid-orbital assignments.

• BoranesNarrower topic: It describes the delocalized orbitals that ordinary localized bond pictures miss.

• Robert Burns WoodwardRelated: Woodward drew on orbital reasoning to explain reaction behavior and formulate predictive selection rules.

• Xenon difluorideNarrower topic: It gives a fuller account of the delocalized bonding in XeF₂ than a simple Lewis structure.

• DiboraneNarrower topic: It accounts for bonding across each boron–hydrogen–boron bridge.

• OxyanionRelated: It gives a more complete account of delocalized bonding in oxyanions.

• Physical organic chemistryNarrower topic: Orbital interactions explain why molecular geometry and substituents change reaction pathways.

• Resonance structureCompared with: It describes delocalized electrons directly rather than combining Lewis drawings.

• sp² hybridizationCompared with: It accounts for delocalized bonding without requiring localized hybrid bonds.

• Trigonal planar molecular geometryCompared with: It explains bonding without treating localized sp² orbitals as the fundamental description.

• Walter HeitlerCompared with: It contrasts with the localized electron-pair picture associated with Heitler and London.

• Xenon tetrafluorideRelated: It provides a bonding account that avoids treating xenon’s d orbitals as essential to XeF₄.

• CyclobutadieneNarrower topic: The orbitals explain cyclobutadiene’s degenerate nonbonding levels and destabilized planar configuration.

• Cyclopentadienyl anionNarrower topic: Its orbital energy levels explain why six electrons stabilize the cyclic conjugated ring.

• Hypervalent moleculeNarrower topic: It accounts for delocalized bonding that localized Lewis structures represent imperfectly.

• Linear combination of atomic orbitalsNarrower topic: LCAO is a common construction method within this broader theory.

• Molecular electronicsNarrower topic: It supplies the electronic structure used to predict molecular transport.

• 18-electron ruleNarrower topic: It explains bonding and stability beyond the rule’s simple electron total.

• Electron-deficient compoundRelated: Delocalized orbitals provide a direct account of bonding across three or more atoms.

• Metal carbonylNarrower topic: It accounts for the donor and acceptor orbitals behind metal–CO bonding.

• Double bondNarrower topic: It explains double bonds as occupied bonding orbitals rather than localized electron pairs.

• Robert S. MullikenBroader topic: Mulliken developed this framework to explain molecular structure and bonding.

• AntiaromaticityNarrower topic: The degenerate frontier orbitals of 4n rings explain their unusual instability.

• Boron trifluorideRelated: Its account of BF₃ bonding clarifies why simple empty-orbital explanations are incomplete.

• Krypton difluorideRelated: It explains KrF₂’s three-center, four-electron bonding across the linear F–Kr–F unit.

• Linear molecular geometryNarrower topic: It explains bonding and electronic structure beyond localized bond-angle models.