This is basically correct. Look up "pi-backbonding" for a good explanation. Bonus fact: Electron backdonation into antibonding orbitals turns out to be really important in catalysis where bond breaking is important.ReidMerrill said:I suspect it has something to do with these ligands having lone pair electrons AND open π* orbitals.
How correct is this and if it is wrong then what is the explanation?
Coordination chemistry is a branch of chemistry that deals with the study of coordination compounds, which are molecules or ions that contain a central metal atom or ion bonded to one or more surrounding ligands.
Ligands are molecules or ions that bond to a central metal atom or ion in a coordination compound. They can be either neutral molecules or anions, and they donate a pair of electrons to form a coordinate covalent bond with the metal atom.
Ligands play a crucial role in determining the physical, chemical, and biological properties of coordination compounds. They can influence the geometry, color, and magnetic properties of the compound, as well as its reactivity and stability.
There are several types of ligands in coordination chemistry, including monodentate (bonding through a single atom), bidentate (bonding through two atoms), polydentate (bonding through multiple atoms), and chelating (bonding through multiple atoms in a ring structure).
Ligands are typically named based on their chemical formula, with the ligand name placed before the metal atom or ion in the compound's name. For example, in the compound [Cu(NH3)4]Cl2, the ligand is ammonia and is named tetraamminecopper(II) chloride.