Complex

A complex is a collection of buildings closely packed togethernormally with a perimeter wall or fence surrounding them.

In psychology , a complex is an important principle in psychoanalysis and other schools.

This article is about complexes in chemistry; see complex number for the mathematical and engineering usage.

In chemistry , a complex is a structure composed of a central metal atom or ion , generally a cation , surrounded by a number of negatively charged ions orneutral molecules possessing lonepairs . A complex may also be called a coordination compound or metal complex.

The ions/molecules surrounding the metal are called ligands . A ligand that is boundto a metal ion is said to be coordinated with the ion. The process of binding to the metal ion with more thanone coordination site per ligand is called chelation . Compounds that bind avidlyto form complexes are thus called chelating agents (for example, EDTA ).

Simple ligands like water or chlorine form only one link with the central atom and are said to be monodentate . Some ligands are capable offorming multiple links to the same metal atom, and are described as bidentate, tridentate etc. EDTA is hexadentate, which accounts for the great stability of many of its complexes.

Typically, the chemistry of complexes is dominated by interactions between s and p orbitals of the ligands and the d (or f) orbitals of the metal ions. Because of this, simple octet bonding theory fails in the case of complexes and to understand the chemistry of these systems, a deeper understanding of chemical bonding rulesis necessary.

One such rule is called electron counting , or the rule of 18. Crystal fieldtheory , introduced by Hans Bethe in 1929 , is a more quantum mechanically based attempt atunderstanding complexes. But crystal field theory treats all interactions in a complex as ionic. Ligand field theory ,introduced in 1935 and built from molecular orbital theory , can handle a broader range of complexes and can explain complexes inwhich the interactions are covalent . The chemical applications of group theory can aid in the understanding of crystal or ligand field theory, byallowing simple, symmetry based solutions to the formal equations.

Naming complexes

The basic procedure for naming a complex:

1. Write the names of the ligands in alphabetical order.
   • Multiply occurring monodentate ligands receive a prefix according to the number of occurrences: di-, tri-,tetra-, penta-, or hexa. Polydentate ligands (e.g., ethylenediamine, oxalate) receive bis-,tris-, tetrakis-, etc.
   • Anions end in o. This replaces the final 'e' when the anion ends with '-ate', e.g. sulfate becomessulfato. It replaces 'ide': cyanide becomes cyano.
   • Neutral ligands are given their usual name, with some exceptions: NH₃ becomes ammine; H₂Obecomes aqua; CO becomes carbonyl.
2. Write the name of the central atom/ion. If the complex is an anion, the central atom's name will end in -ate, andits Latin name will be used if available (except for mercury).
3. If the central atom's oxidation state needs to be specified (when it is one of several possible, or zero), write it as aRoman numeral (or 0) in parentheses.

Examples:

[NiCl₄]^2- → tetrachloronickelate (II) ion

[CuNH₃Cl₅]^3- → amminepentachlorocuprate(II) ion

[Cd(en)₂(CN)₂] → dicyanobisethylenediaminecadmium(II)

Transition metals make good central ions for complexes.

To study the behaviour of complexes in solution, it is possible to record pH spectra which shows the interaction betweencomplexing agent and central ion as a function of the degree of dissociation of their functional groups, see the Cordis OnlineAbstract at http://www.theoprax-research.com/cordisth.htm or the free pH-spectra databaseat http://www.Theoprax-Research.com/pool.html .