Linked from

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.

• Covalent bondCompared with: Unlike covalent bonding, the usual model emphasizes transferred electrons and charged ions.

• Ionic compoundNarrower topic: It names the attraction that binds the ions in an ionic compound.

• Chemical bondBroader topic: Electron transfer can create the charged partners whose attraction binds ionic solids.

• Valence electronBroader topic: Electron transfer between valence shells creates the ions that attract.

• Sodium chlorideNarrower topic: This attraction holds sodium and chloride ions together in the solid.

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

• Intermolecular forceCompared with: Its extended ionic lattice differs from forces between discrete molecules.

• 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.

• Van der Waals forceCompared with: Unlike van der Waals forces, ionic bonding involves full charges rather than fluctuating or permanent dipoles.

• 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.

• Pi bondCompared with: Unlike ionic bonding, a pi bond involves shared electron density between atoms.

• Metallic bondingCompared with: Unlike metallic bonding, ionic bonding centers on distinct cations and anions.

• Disulfide bondCompared with: Ionic interactions can stabilize proteins but do not join cysteine sulfur atoms covalently.

• Lattice energyNarrower topic: Lattice energy measures the collective stabilization from ionic attractions in a solid.

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

• Potassium chlorideNarrower topic: Electrostatic attraction between K⁺ and Cl⁻ holds the KCl crystal together.

• SaltNarrower topic: Attraction between sodium and chloride ions holds salt’s crystal lattice together.

• 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.

• Magnesium oxideNarrower topic: The attraction between Mg²⁺ and O²⁻ holds the crystal together.

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

• Carbon–carbon bondCompared with: Unlike this shared-electron bond, ionic bonding joins charged species electrostatically.

• Coordinate covalent bondCompared with: Unlike an ionic bond, a coordinate covalent bond involves a shared electron pair.

• 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.

• Hard and soft acids and basesCompared with: HSAB preferences also apply to ionic interactions, not only coordinate bonds.

• 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.

• Potassium iodideNarrower topic: The attraction between K⁺ and I⁻ forms the solid compound.

• 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.

• Calcium oxalateNarrower topic: The attraction between calcium and oxalate ions holds the solid together.

• Noncovalent interactionCompared with: Its classification as a bond contrasts with electrostatic attractions that do not create an ionic solid.

• Calcium chlorideNarrower topic: The crystal’s structure arises from attraction between calcium cations and chloride anions.

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

• Aluminium oxideNarrower topic: The ionic model helps explain Al₂O₃'s high melting point and electrical behavior.

• 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.

• Calcium fluorideNarrower topic: Electrostatic attraction between Ca²⁺ and F⁻ holds the solid together.

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

• Diatomic moleculeCompared with: Some two-atom species, such as sodium chloride molecules in the gas phase, are strongly ionic.