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The 114 pages that link to Chemical bond, each with the reason it gives.

• Oxidation stateNarrower topic: Oxidation-state assignment idealizes bonds as completely ionic, even when they are covalent.

• HydrolysisNarrower topic: Hydrolysis is defined by breaking a bond through reaction with water.

• Molecular geometryNarrower topic: Bond connectivity sets which atoms are positioned relative to one another.

• StereochemistryNarrower topic: Bonding determines which molecular arrangements are possible and how atoms connect.

• ElectronegativityNarrower topic: Electronegativity describes electron attraction specifically within a bond.

• WaterNarrower topic: The O–H bonds within each molecule are distinct from attractions between water molecules.

• Valence electronNarrower topic: Valence electrons are the electrons shared or transferred in many chemical bonds.

• Oxidizing agentNarrower topic: Bond changes often accompany the electron transfer caused by an oxidizing agent.

• IUPAC nomenclatureNarrower topic: Bonding patterns underlie the structural information conveyed by many chemical names.

• Chemical reactionNarrower topic: Reactions transform substances by breaking, forming, or reorganizing these interactions.

• Transition stateNarrower topic: Partial bond formation and breaking define the structure of many transition states.

• Lewis acidNarrower topic: Lewis acidity describes one way a chemical bond forms through shared electron-pair donation.

• Structural formulaNarrower topic: Lines in structural formulas commonly represent bonds between atoms.

• Electron shellNarrower topic: Outer-shell electrons participate in the interactions that form bonds.

• AdhesionNarrower topic: Some interfaces adhere through covalent, ionic, or other chemical bonds across the boundary.

• Linus PaulingNarrower topic: Pauling’s theories of molecular structure centered on explaining how bonds form and behave.

• Molecular vibrationNarrower topic: Bond stiffness supplies the restoring forces underlying many molecular vibrations.

• Hydrogen fluorideNarrower topic: The polar H–F bond underlies HF’s molecular properties and reactions.

• Electron affinityNarrower topic: Electron gain energetics contribute to the ionic and covalent bonding patterns of elements.

• Bond orderNarrower topic: Bond order quantifies bonding interactions within this broader idea.

• Octet ruleNarrower topic: The octet rule is a simple heuristic for anticipating some bonding arrangements.

• Bond dissociation energyNarrower topic: Dissociation energy quantifies the energetic cost of breaking one specified bond.

• AllotropyNarrower topic: Elements can form allotropes by changing how their atoms bond.

• Dissociation (chemistry)Narrower topic: Dissociation separates particles that were associated through chemical bonds or ionic interactions.

• MoleculeNarrower topic: Molecular atoms are joined by these interactions.

• Bond angleNarrower topic: A bond angle is defined by two chemical bonds meeting at a shared atom.

• Chemical reactivityNarrower topic: Reactivity involves changing the bonds that hold reactants and products together.

• CohesionNarrower topic: Cohesion is a bulk intermolecular effect, distinct from the bonds within molecules.

• Molecular polarityNarrower topic: Molecular polarity depends on how electrons are distributed across chemical bonds.

• OxideNarrower topic: Different bond types account for the varied structures and properties of oxides.

• Noble gas compoundNarrower topic: Noble gas compounds are distinctive examples of chemical bonding by normally unreactive elements.

• Molecular structureNarrower topic: Bonds define which atoms are connected and constrain their relative positions.

• Thermal degradationNarrower topic: Thermal degradation changes compounds by breaking or rearranging these interactions.

• Torsional strainNarrower topic: Torsional strain concerns the relative alignment of bonds around a shared connection.

• Noncovalent interactionNarrower topic: The broader category includes covalent and ionic bonds, which are distinguished from noncovalent interactions.

• Bond lengthNarrower topic: Bond length describes the spatial separation within this interaction.

• PhotodissociationNarrower topic: Photodissociation specifically removes a molecule's atoms from a bonded arrangement.

• Xenon hexafluoroplatinateNarrower topic: The disputed formulation raises questions about how xenon and platinum fluoride are bound.

• Gilbert N. LewisNarrower topic: His electron-pair theory became a major framework for explaining covalent bonding.

• Diatomic moleculeNarrower topic: Diatomic molecules are held together by bonds between their two atoms.

• Allotropes of carbonNarrower topic: Different carbon allotropes arise from different patterns of bonding between carbon atoms.

• PhysisorptionNarrower topic: The absence of a newly formed chemical bond distinguishes physisorption from chemisorption.

• Ball-and-stick modelNarrower topic: Each rod stands for a bond linking two atoms.

• Cyclic compoundNarrower topic: The bonds linking a sequence of atoms into a closed path define a ring.

• Organic reactionNarrower topic: Bond changes are the defining molecular events in organic reactions.

• Structural isomerNarrower topic: Changing which atoms are bonded defines structural isomerism.

• Valence shellNarrower topic: Bond formation is the main way valence-shell electrons link atoms.

• Helium compoundsNarrower topic: Helium species form through bonding mechanisms unlike ordinary valence-bond compounds.

• IUPAC nomenclature of inorganic chemistryNarrower topic: Bonding determines which structural features names may need to specify.

• NonmetalNarrower topic: Nonmetal properties emerge partly from the bonds their atoms form.