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The 207 pages that link to Oxidation state, each with the reason it gives.

• Electron configurationRelated: Ion formation changes electron occupancy and often changes the resulting configuration.

• OxygenRelated: Oxygen’s usual oxidation state is −2, with notable exceptions such as peroxides.

• OxidationRelated: An increase in oxidation state tracks electron loss, even when no free electrons appear.

• ElectronegativityRelated: Electronegativity determines which atom receives the bonding electrons in oxidation-state assignments.

• Valence electronRelated: Valence-electron accounting helps track electron transfers in reactions.

• Coordination complexRelated: It helps determine the central metal’s electron count and likely charge.

• Oxidizing agentRelated: Its decrease tracks the oxidizing agent’s acceptance of electrons.

• Transition metalRelated: Transition metals often access multiple oxidation states through changes in d-electron count.

• Rare-earth elementRelated: Most rare earths favor the +3 state, while some also show stable alternatives.

• SulfateRelated: Sulfur’s +6 and oxygen’s −2 assignments account for sulfate’s −2 charge.

• Periodic trendsRelated: Valence patterns help anticipate common oxidation states and their changes among related elements.

• Coordination chemistryRelated: Oxidation-state bookkeeping helps determine metal identity and complex charge.

• Redox potentialRelated: Changes in oxidation state track which atoms lose or gain electrons.

• Lattice energyRelated: Ionic charges derived from oxidation states help predict lattice-energy trends.

• NitrateRelated: Nitrogen has oxidation state +5 in nitrate, helping explain its redox chemistry.

• ActinideRelated: Early actinides can access several oxidation states because 5f, 6d, and 7s electrons are close in energy.

• Electrode potentialRelated: Changes in oxidation state identify the redox transformations associated with an electrode.

• Iron oxideRelated: The +2 and +3 states account for the principal stoichiometric iron oxides.

• MagnetiteRelated: Magnetite contains iron in both +2 and +3 oxidation states.

• Chemical nomenclatureRelated: Roman numerals in names distinguish metals that form ions with different oxidation states.

• Potassium ionRelated: Potassium has oxidation state +1 in K⁺ and most of its compounds.

• ReductionRelated: Reduction is identified by a decrease in an atom’s oxidation state.

• SilverRelated: Silver’s usual +1 state predicts the formulas of many of its compounds.

• CathodeRelated: Reduction at the cathode lowers the oxidation state of the reacting species.

• Mössbauer spectroscopyRelated: Isomer shifts and quadrupole patterns help distinguish iron oxidation states.

• TinRelated: Tin commonly forms compounds in the +2 and +4 oxidation states.

• AnionRelated: Oxidation states track electron accounting but need not equal an ion’s actual charge.

• FluorideRelated: The gloss’s −1 oxidation state distinguishes fluoride-containing compounds.

• Half-reactionRelated: Changes in oxidation state identify which species lose or gain electrons.

• OxideRelated: It provides a consistent way to describe oxygen’s charge and balance oxide formulas.

• OxoacidRelated: The central element’s oxidation state helps distinguish related oxoacids.

• Perchloric acidRelated: Chlorine has oxidation state +7 in perchloric acid, its highest common state.

• Potassium permanganateRelated: Assigning oxidation states identifies manganese as +7 in permanganate and tracks its reduction.

• CationRelated: Electron loss that forms cations often corresponds to an increase in oxidation state.

• ChromateRelated: Oxygen’s usual −2 assignment gives chromium a +6 oxidation state in chromate.

• PeroxidesRelated: Peroxide oxygen has oxidation state −1, unlike oxygen in most compounds.

• SulfideRelated: Sulfur’s oxidation state distinguishes sulfide from more oxidized sulfur species.

• YttriumRelated: Yttrium overwhelmingly forms compounds in the +3 oxidation state.

• Alkaline earth metalRelated: The common +2 oxidation state reflects the loss of two outer electrons.

• BromideRelated: Bromine has oxidation state −1 in bromide, unlike its positive states in some compounds.

• SeleniumRelated: Selenium adopts several oxidation states, especially −2, +4, and +6.

• IodideRelated: Iodine has oxidation state −1 in iodide.

• Xenon hexafluoroplatinateRelated: Its assignment helps describe electron transfer and the uncertain ionic formulation.

• Chemical speciationRelated: Different oxidation states often correspond to forms with sharply different reactivity and mobility.

• ChlorateRelated: Chlorine has oxidation state +5 in ClO₃⁻.

• Inorganic chemistryRelated: Oxidation states track electron changes in inorganic compounds and reactions.

• Potassium chlorateRelated: Chlorine’s oxidation state helps explain its reduction during chlorate decomposition.

• Reducing agentRelated: An increase in the agent’s oxidation state tracks its electron loss.

• ScandiumRelated: Scandium overwhelmingly adopts the +3 oxidation state in its compounds.

• Silver nitrateRelated: Silver is in the +1 oxidation state in AgNO₃ and can be reduced to Ag(0).