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The 110 pages that link to Ionic bonding, each with the reason it gives.

• Oxidation stateRelated: The fully ionic model treats every bond as if its electrons belonged to one atom.

• CalciumRelated: Calcium’s compounds often form when calcium ions attract negatively charged ions.

• CeramicRelated: Ionic bonding gives many ceramics high melting points and resistance to deformation.

• IonRelated: Ions form ionic bonds when opposite charges attract in a compound.

• ChlorideRelated: Chloride commonly bonds ionically with positively charged atoms.

• Alkali metalRelated: Alkali metals commonly become positive ions that bind to anions in salts.

• SulfateRelated: It holds sulfate anions together with positively charged ions in sulfate salts.

• HydroxideRelated: This attraction holds hydroxide in salts such as sodium hydroxide.

• HalogenRelated: Metal atoms can transfer electrons to halogens, producing ionic salts.

• Octet ruleRelated: Electron transfer can give each ion a noble-gas-like outer shell.

• Potassium ionRelated: Potassium ions form ionic compounds by attracting negatively charged ions.

• Sodium ionRelated: Na⁺ forms ionic solids through attraction to anions such as chloride.

• AcetateRelated: In acetate salts, this attraction connects acetate anions with counterions such as sodium.

• AnionRelated: Anions form ionic bonds by attracting positively charged ions.

• FluorideRelated: Fluoride salts form when F⁻ pairs with positively charged ions.

• Salt (chemistry)Related: This attraction holds a salt’s ions together in a solid lattice.

• CarboxylateRelated: A carboxylate salt pairs the anion with positively charged counterions.

• SulfideRelated: Many solid sulfides consist of sulfide anions paired with metal cations.

• Alkaline earth metalRelated: Group 2 metals form ionic compounds by attracting negatively charged ions.

• BariumRelated: Barium commonly loses two electrons and forms ionic compounds with anions.

• BromideRelated: This attraction holds bromide ions together with positively charged ions in salts.

• Calcium ionRelated: Ca²⁺ forms ionic compounds by attracting negatively charged ions.

• IodideRelated: Ionic attraction holds iodide in salts with positively charged ions.

• Iron(II)Related: Iron(II) commonly forms ionic compounds with anions such as oxide and sulfate.

• Oxide ionRelated: Its attraction to cations holds many oxide solids together.

• Chemical compoundRelated: Ionic bonding builds compounds such as sodium chloride from charged particles.

• Metal oxideRelated: Many metal oxides are ionic lattices of metal cations and oxide anions.

• Barium oxideRelated: BaO’s lattice consists principally of Ba²⁺ and O²⁻ ions.

• Fluoride ionRelated: Fluoride forms ionic bonds with many metal cations.

• Iron(III) chlorideRelated: The formula reflects charge balance, although solid FeCl₃ has substantial covalent character.

• Lead(II) ionRelated: Pb²⁺ forms ionic compounds by attracting negatively charged ions.

• Beryllium oxideRelated: BeO's bonding has substantial ionic character, alongside strong covalent character.

• Copper(I) oxideRelated: Ionic interactions help hold the copper and oxide ions together.

• NonmetalRelated: Nonmetals often gain electrons from metals, forming anions that bind ionic compounds.

• Lead(II) sulfideRelated: The Pb²⁺ and S²⁻ charges provide a useful first description of PbS bonding.

• Main-group elementRelated: Alkali and alkaline-earth metals often form cations that bond ionically with nonmetals.

• Sodium bromideRelated: Attraction between Na+ and Br− holds the crystal together.

• Halide mineralRelated: It binds halide anions to the cations in these minerals.

• Manganese(II) oxideRelated: The ionic model describes the attraction between Mn²⁺ and O²⁻ in MnO.

• Mercury(II) oxideRelated: The ionic model describes HgO as containing mercury and oxide ions.

• Silver sulfideRelated: The Ag⁺ and S²⁻ oxidation states provide a useful model for the compound's composition.

• Cobalt(II) oxideRelated: Ionic attraction holds the Co²⁺ and O²⁻ ions together in the crystal.

• Potassium hydrideRelated: This attraction holds potassium cations and hydride anions together in the solid.

• Silver nitrideRelated: A simple ionic model is often invoked to rationalize the nominal Ag₃N formula.

• Bonding in solidsRelated: It holds many salts together in extended lattices of positive and negative ions.

• Lithium nitrideRelated: Electrostatic attraction between Li⁺ and N³⁻ accounts for the compound's formal ionic character.

• Sodium formateRelated: It holds sodium and formate ions together in the solid.