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The 70 pages that link to Valence electron, each with the reason it gives.

• Oxidation stateRelated: Oxidation-state bookkeeping tracks the formal reassignment of bonding valence electrons.

• Periodic tableBroader topic: Valence electrons help explain the shared reactions of a group.

• Covalent bondBroader topic: These are the electrons atoms share in covalent bonds.

• Electron configurationBroader topic: Outer-shell occupancy is the configuration feature most directly tied to bonding.

• Chemical bondBroader topic: These electrons are the main participants in ordinary chemical bonds.

• ElectronegativityBroader topic: These are the electrons whose unequal sharing electronegativity describes.

• Lewis structureNarrower topic: Lewis structures track these electrons to account for bonds and lone pairs.

• Functional groupRelated: Valence electrons determine the bonding patterns that make each group distinctive.

• Doping (semiconductors)Related: Differences in valence electrons explain why a dopant can donate or accept charge.

• Formal chargeRelated: The atom’s neutral valence-electron count is the starting value in the formal-charge calculation.

• IonRelated: These outer electrons are commonly transferred when atoms form ions.

• ResonanceRelated: Contributors rearrange valence electrons while keeping the total electron count fixed.

• Alkali metalBroader topic: Each alkali metal has one outer-shell electron, which it readily loses.

• Ionization energyRelated: The first ionization energy usually removes an outer-shell electron.

• Noble gasRelated: A filled set of valence electrons underlies the group’s characteristic low reactivity.

• Periodic trendsRelated: Valence-electron counts repeat by group and help explain recurring chemical behavior.

• Aufbau principleRelated: Predicted configurations identify the electrons most relevant to an element's chemistry.

• Metallic bondingBroader topic: Valence electrons become delocalized in the standard account of metallic bonding.

• Hückel's ruleNarrower topic: Applying the rule begins by identifying which valence electrons enter the π system.

• Electron affinityRelated: Valence-shell structure largely determines the configuration formed after electron gain.

• Free radicalRelated: Radical reactivity depends on how the unpaired valence electron interacts with other species.

• Lone pairNarrower topic: Lone pairs consist of valence electrons that remain associated with one atom.

• Bond orderRelated: Their allocation across bonds and orbitals underlies bond-order descriptions.

• HalogenRelated: Halogen atoms have seven valence electrons and tend to gain one more.

• Octet ruleBroader topic: Octet counting concerns the electrons available in an atom’s outer shell.

• Potassium ionRelated: Potassium’s one valence electron is the electron removed in ion formation.

• Periodic lawBroader topic: Valence electrons account for many recurring similarities among elements in a group.

• MoleculeRelated: The sharing or redistribution of these electrons determines molecular bonding.

• Sigma bondRelated: Shared valence electrons occupy the bonding orbital that defines a sigma bond.

• Carbon–carbon bondRelated: Carbon’s four valence electrons support multiple carbon–carbon bonding patterns.

• Coordinate covalent bondRelated: The donated pair consists of valence electrons from the donor atom.

• AnionBroader topic: Anions commonly gain electrons into their outer electron shell.

• Lewis baseNarrower topic: Lewis-base behavior depends on the availability of valence electrons for donation.

• VSEPR theoryRelated: Counting valence electrons is the starting point for assigning bonds and lone pairs.

• Hybrid orbitalRelated: Hybridization models the orbitals used by an atom's valence electrons.

• BismuthRelated: Bismuth’s five outer electrons help explain its common compounds and oxidation states.

• Alkaline earth metalRelated: Group 2 atoms have two outer-shell electrons available for bonding.

• Calcium ionRelated: Calcium’s two outer electrons are the ones it typically loses.

• Inert-pair effectNarrower topic: The effect concerns the differing chemical availability of valence s and p electrons.

• Gilbert N. LewisRelated: Lewis used outer-shell electrons to explain how atoms form chemical bonds.

• ChalcogenRelated: Chalcogens generally have six valence electrons, shaping their bonding and oxidation states.

• Metal (chemistry)Broader topic: Metal atoms’ relatively available valence electrons enable metallic bonding and positive ions.

• Resonance structureNarrower topic: Only valence-electron placement changes between resonance structures.

• sp² hybridizationRelated: Hybrid-orbital descriptions organize the bonding behavior of valence electrons.

• Hypervalent moleculeRelated: Counting these electrons around a central atom identifies a hypervalent Lewis structure.

• Single bondNarrower topic: The shared pair in a single bond comes from the atoms' valence electrons.

• Electron-deficient compoundNarrower topic: The available valence electrons determine whether conventional bonds can account for the framework.

• Actinide conceptRelated: Actinide chemistry reflects the unusual accessibility of 5f, 6d, and 7s electrons.

• Double bondRelated: The shared pairs in a double bond come from the atoms' valence electrons.

• Phosphorus oxidation stateRelated: Oxidation-state calculations count assigned valence electrons against phosphorus’s elemental reference.