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The 59 pages that link to Coordination complex, each with the reason it gives.

• Oxidation stateBroader topic: Metal oxidation states are inferred from the complex’s charge and the ligands’ assigned charges.

• Transition metalNarrower topic: Transition-metal ions commonly form these complexes because their orbitals accommodate ligand bonding.

• ChelationNarrower topic: A chelate is a coordination complex distinguished by a ligand making multiple bonds to its metal.

• Crystal field theoryNarrower topic: Crystal field theory describes the metal-centered electronic structure of these compounds.

• HydrateRelated: Some hydrate water molecules bind directly to metal ions as ligands.

• LigandNarrower topic: The ligand is one component of this broader chemical structure.

• CobaltRelated: Cobalt readily forms coordination complexes with distinctive colors and structures.

• Lone pairBroader topic: Ligands commonly bind metal centers by donating lone pairs.

• Coordination numberBroader topic: In complexes, coordination number usually counts donor atoms bonded to the central metal.

• Ligand field theoryNarrower topic: Ligand field theory describes the electronic structure of these metal-centered assemblies.

• MordantNarrower topic: Metal ions in many mordants coordinate with dye molecules and help connect them to fibers.

• Polyatomic ionCompared with: Complex ions also act as charged units, but their metal–ligand bonding distinguishes them from common covalent polyatomic ions.

• Coordinate covalent bondBroader topic: Ligands commonly donate electron pairs to metal centers to form these structures.

• Crystal waterRelated: Water molecules can bind metal ions directly as ligands within a crystal.

• Lewis baseBroader topic: Ligands commonly bind metal centers by donating Lewis-base electron pairs.

• CyanideNarrower topic: Many cyanides are metal complexes in which CN⁻ acts as a ligand.

• PorphyrinNarrower topic: A metal inserted into a porphyrin cavity creates a coordination complex.

• Chemical speciationRelated: Complex formation is a major route by which dissolved elements change chemical form.

• Inorganic chemistryBroader topic: Metal–ligand bonding forms a major class of inorganic compounds with distinctive structures and reactivity.

• Iron(II)Related: Fe²⁺ often occurs bound to ligands rather than as an isolated ion.

• Iron(III)Narrower topic: Iron(III) commonly occurs inside complexes rather than as an isolated ion.

• RhodiumRelated: Molecular rhodium catalysts change reactivity as ligands bind and exchange.

• ScandiumRelated: Scandium(III) forms complexes with water and other ligands despite its relatively simple chemistry.

• d-blockRelated: D-block ions commonly form complexes whose structures depend on their d electrons.

• Magnesium ionNarrower topic: Mg²⁺ binds oxygen-rich ligands in proteins and metabolites, positioning them for chemical reactions.

• 18-electron ruleNarrower topic: The 18-electron count is applied to the metal center within these structures.

• Lead(II) ionRelated: Ligands can bind Pb²⁺ through lone-pair donation, forming complexes in solution.

• Manganese(II)Narrower topic: Mn²⁺ commonly forms complexes whose geometry and reactivity depend on their ligands.

• Metal carbonylNarrower topic: Metal carbonyls are a class of coordination complexes.

• Square planar molecular geometryNarrower topic: Square-planar geometry is a common arrangement of ligands in coordination complexes.

• Aluminium chlorideNarrower topic: AlCl₃ forms donor–acceptor complexes when other molecules supply electron pairs.

• Copper(II) chlorideNarrower topic: Copper(II) forms chloride- and water-coordinated species in solutions and hydrates.

• Valence shellBroader topic: Ligands interact with a metal’s valence orbitals, often beyond simple octet patterns.

• IUPAC nomenclature of inorganic chemistryBroader topic: Its names must identify the central atom, ligands, and sometimes geometry or charge.

• Potassium ferricyanideNarrower topic: Six cyanide ligands surround the iron center in its ferricyanide ion.

• Zinc chlorideRelated: In water, zinc ions bind water molecules and chloride ions in changing coordination environments.

• Copper(II) hydroxideRelated: Copper(II) readily changes coordination environment, affecting the solid’s structure and reactions.

• Ethylenediaminetetraacetic acidNarrower topic: EDTA’s metal-binding products are coordination complexes.

• Chloroauric acidNarrower topic: Tetrachloroaurate is a coordination complex with gold at its center.

• FerricyanideNarrower topic: Ferricyanide is a compact example with one metal center and six ligands.

• Gold(III) chlorideNarrower topic: Gold(III) chloride forms coordination complexes when ligands bind to gold.

• Inorganic compoundBroader topic: Metal-containing inorganic compounds often have distinctive structures formed by ligand coordination.

• Beryllium chlorideNarrower topic: Donor ligands coordinate to beryllium, producing complexes such as tetrahedral chloroberyllate ions.

• Cobalt(II) chlorideNarrower topic: Cobalt ions bind water or chloride ligands in solution and hydrated solids.

• Copper(I) chlorideNarrower topic: Chloride ligands form soluble complexes with copper(I), changing CuCl's behavior in chloride-rich solutions.

• Electron countingBroader topic: Metal complexes are a major setting for systematic electron-counting rules.

• Potassium thiocyanateNarrower topic: Thiocyanate acts as a ligand in colored complexes with iron and other metals.

• Tin(IV) chlorideRelated: Donor ligands can bind tin and form higher-coordinate complexes.

• Zinc hydroxideRelated: In strongly alkaline water, dissolved zinc forms hydroxide-containing coordination species.

• Aluminium triacetateNarrower topic: Water and acetate can coordinate aluminium rather than behaving as entirely separate ions.