Ligands in inorganic complex compounds are the atoms, ions, or molecules that bind to a central metal atom or ion. They donate electron pairs to the metal, forming a coordinate covalent bond.

Here's a breakdown of common ligands:

Types of Ligands:

* Monodentate: These ligands bind to the metal atom through a single donor atom. Examples include:

* Halogens: Cl-, Br-, I-

* Water: H2O

* Ammonia: NH3

* Carbon monoxide: CO

* Cyanide: CN-

* Bidentate: These ligands have two donor atoms that can bind to the metal atom. Examples include:

* Ethylenediamine: en (NH2CH2CH2NH2)

* Oxalate: C2O42-

* Glycinate: H2NCH2COO-

* Polydentate: These ligands have more than two donor atoms that can bind to the metal atom. Examples include:

* Ethylenediaminetetraacetate: EDTA4- (a hexadentate ligand)

* Porphyrins: (present in heme, chlorophyll)

Ligand Nomenclature:

* Ligands are named according to their identity. For example:

* Aqua: H2O

* Ammine: NH3

* Chloro: Cl-

* Cyano: CN-

* Oxalato: C2O42-

* The number of ligands is indicated by prefixes such as:

* Mono: One

* Di: Two

* Tri: Three

* Tetra: Four

* Penta: Five

* Hexa: Six

Examples of Inorganic Complex Compounds:

* Tetraamminecopper(II) sulfate: [Cu(NH3)4]SO4

* Ligands: Ammonia (NH3)

* Potassium hexacyanoferrate(II): K4[Fe(CN)6]

* Ligands: Cyanide (CN-)

* Tetraaquacopper(II) ion: [Cu(H2O)4]2+

* Ligands: Water (H2O)

Important Notes:

* The number and type of ligands can significantly affect the properties of the complex.

* Ligands can be neutral, negatively charged (anionic), or rarely, positively charged (cationic).

* The central metal atom or ion typically has a coordination number, which represents the number of ligands directly bonded to it.

Understanding the ligands in inorganic complex compounds is crucial for comprehending their structure, bonding, and reactivity.