Explore: Ions Complexes

complexes are called chelate complexes; the formation of such complexes is called chelation, complexation, and coordination. The central atom or ion,

of complex: compounds formed by the interaction of a metal ion with a ligand and supramolecular complexes, such as host–guest complexes and complexes of

hydrogen ions and hydroxide ions are strongly solvated, with hydrogen bonds between oxygen and hydrogen atoms. Indeed, the bihydroxide ion H 3O− 2 has

chemistry, metal aquo complexes are coordination compounds containing metal ions with only water as a ligand. These complexes are the predominant species

is important in nature. With metal ions, thiolates behave as ligands to form transition metal thiolate complexes. The term mercaptan is derived from

Using kinetically inert metal ions, complexes containing monodentate amino acids have been characterized. These complexes exist in either the N or the

trivalent ions are hard acceptors and form more stable complexes with oxygen-donor ligands than with nitrogen-donor ligands. The larger ions are 9-coordinate

both the ion exchanger and ion. This can be dependent on the size, charge, or structure of the ions. Common examples of ions that can bind to ion exchangers

widely used to bind to iron (Fe2+/Fe3+) and calcium ions (Ca2+), forming water-soluble complexes even at neutral pH. It is thus used to dissolve Fe- and

Greek ion and -phore 'ion carrier') is a chemical species that reversibly binds ions. Many ionophores are lipid-soluble entities that transport ions across