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CBC Method- Covalent Bond Classification
This mode of classification is also referred to as the L-X Notation. It was developed by M. H. Green in the mid 1990s as a solution for the need to describe organometallic complexes in a way that isn’t as prone to limitations, like those that arise from the very definition of oxidation state. Instead this method looks at the nature of the ligands as opposed to the transition metal center of the complex. By focusing on the ligands, it can acknowledge the fact that many situations regardless of the ligand, that the 18 electron rule is being obeyed.[1] According to this method there are three basic types of interactions that allow for binding between the metal center and the ligands to occur. These three interactions can then be labeled, and therefore distinguished, as X, L and Z. These are differentiated by differences in how they bond with the metal center.

Types of Ligands
X-type ligands are those that donate one electron to the metal and accept one electron from the metal when using the neutral ligand method of electron counting, or donate two electrons to the metal when using the donor pair method of electron counting. Regardless of whether it is considered neutral or anionic, these ligands yield normal covalent bonds.[3] A few examples of this type of ligand are H, halogens (Cl, Br, F, etc.), OH-, CN, CH3, and NO (bent).

L-type ligands are neutral ligands that donate two electrons to the metal center regardless of the electron counting method being used. These electrons can come from lone pairs, pi or sigma donors.[4] The bonds formed between these ligands and the metal are dative covalent bonds, which are also known as coordinate bonds. Examples of this type of ligand include CO, PR3, NH3, H2O, carbenes (=CRR'), and alkenes.

Z-type ligands are those that accept two electrons from the metal center as opposed to the donation occurring with the other two types of ligands. However, these ligands also form dative covalent bonds like the L-type.[3] This type of ligand is not usually used, because in certain situations it can be written in terms of L and X.  For example if a Z ligand is accompanied by an L type, it can be written as X2. Examples of these ligands are Lewis acids, such as BR3.[1]

Uses of the Notation
When given a metal complex and the trends for the ligand types, the complex can be written in a more simplified manner with the form [MLlXxZz]Q±. The subscripts represent the numbers of each ligand type present in that complex, M is the metal center and Q is the overall charge on the complex. Some examples of this overall notation are as follows:

[Mn(CO)6]+ --> [ML6]+

[Ir(CO)(PPh3)2(Cl)(NO)]2+ --> [ML3X2]2+

[Fe(CO)2(CN)4]2- --> [ML2X2]2-

Also from this general form, the values for electron count, oxidation state, coordination number, number of d-electrons, valence number and the ligand bond number[3] can be calculated.

Electron Count = N + x + 2l – Q

Where N is the group number of the metal.

Oxidation State (OS) = x + Q

Coordination Number (CN) = x + l

Number of d-electrons (dn) = N- OS                                      = N- (x + Q)

Valence Number (VN)= x + 2z

Ligand Bond Number (LBN) = l + x + z

Other Uses
This template of writing a metal complex also allows for better comparison of molecules with different charges. This can happen when the assignment is reduced to its “equivalent neutral class”. The equivalent neutral class is the classification of the complex if the charge was localized on the ligand as opposed to the metal center.[2] In other words, the equivalent neutral class is the representation of the complex as though there was no charge.