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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.

• 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.

• 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.

• 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.

• 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.

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

• 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.

• 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.

• 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.

• 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.

• 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.

• Bent molecular geometryRelated: Valence electrons determine how many bonds and lone pairs surround the central atom.

• NonmetalRelated: The number and behavior of valence electrons help determine nonmetal reactivity and bonding.

• PnictogenRelated: Pnictogens generally have five valence electrons, shaping their bonding patterns.

• Post-transition metalRelated: The outer s and p electrons govern much of these elements’ chemistry.

• CaesiumRelated: Caesium’s lone valence electron drives its characteristic +1 chemistry.

• Main-group elementRelated: Main-group chemistry is largely governed by the number of valence electrons.

• Triple bondRelated: The three shared pairs are made from valence electrons.

• Boron groupRelated: Each group 13 element has three valence electrons.

• Period 3 elementRelated: The number of outer-shell electrons increases across Period 3 and shapes its chemistry.

• Period 5 elementRelated: Valence-electron patterns connect the row’s position to its chemical behavior.

• Arrow pushingRelated: Curved arrows track valence electrons as they change bonding or remain as lone pairs.

• Period 2 elementRelated: The number of outer-shell electrons generally increases from lithium to neon.

• Atomic and molecular structureRelated: Valence electrons largely determine which molecular structures atoms can form.

• Orbital hybridisationRelated: Hybridisation models the orbitals associated with an atom’s bonding electrons.