1. Ligands and electron counting in organometallic chemistry
Textbook: Chapters 1.4 – 1.6, 3.3

2. Ligands in organometallic chemistry
Neutral 2e donors: PR3 (phosphines), CO (carbonyl), R2C=CR2 (alkenes), RC≡CR (alkynes, can also donate 4e), N≡CR (nitriles)
Anionic 2e donors: X- (halide), CH3- (methyl), CR3- (alkyl), Ph- (phenyl), H- (hydride) The following can also donate 4e if needed, but initially count them as 2e donors (unless they are acting as bridging ligands): OR- (alkoxide), SR- (thiolate), NR2- (inorganic amide), PR2- (phosphide)
Anionic 4e donors: C3H5- (allyl), O2- (oxide), S2- (sulfide), NR2- (imide), CR22- (alkylidene) and from the previous list: OR- (alkoxide), SR- (thiolate), NR2- (inorganic amide), PR2- (phosphide)
Anionic 6e donors: Cp- (cyclopentadienyl), O2- (oxide)
Z ligands: do not bring e to the metal: BR3, AlR3

3. hx kx mx Nomenclature h5-Cp h3-Cp h3-allyl h1-allyl h1-dppe / k1-dppe
- bridging ligand

4. Ordering: from ACS publications
In formulas with Cp (cyclopentadienyl) ligands, the Cp usually comes first, followed by the metal center: Cp2TiCl2
Other anionic multi-electron donating ligands are also often listed in front of the metal.
In formulas with hydride ligands, the hydride is sometimes listed first.
Rule # 1, however, takes precedence over this rule: HRh(CO)(PPh3)2 and Cp2TiH2
Bridging ligands are usually placed next to the metals in question, then followed by the other ligands
Note that rules 1 & 2 take precedence: Co2(m-CO)2(CO)6, Rh2(m-Cl)2(CO)4, Cp2Fe2(m-CO)2(CO)2

5. Coordination geometriesCN
Geometry
Example 2
3, trigonal
3, T shape
4, tetrahedron
4, square planar
[NC–Ag–CN]–
Pt(PPh3)3
[Rh(PPh3)3]+
Ti(CH2Ph)4

6. Coordination geometriesCN
Geometry
Example
5, trigonal bipyramid
5, square pyramid
6, octahedron
6, pseudo-octahedron
[Co(CNPh)5]2+
W(CO)6
FeCp2

7. Coordination geometriesCN
Geometry
Example
6, antiprism
7, capped octahedron
7, pentagonal biprism
WMe6
[ReH(PR3)3(MeCN)3]+
[IrH5(PPh3)2]

8. Electron counting and the 18 electron rule
Determine the oxidation state of the transition metal center(s) and the metal centers resulting d-electron count. To do this one must:
a) note any overall charge on the metal complex
b) know the charges of the ligands bound to the metal center (ionic ligand method)
c) know the number of electrons being donated to the metal center from each ligand (ionic ligand method)
Add up the electron counts for the metal center and ligands.
Complexes with 18e counts are referred to as saturated, because there are no empty low-lying orbitals to which another incoming ligand can coordinate. Complexes with counts lower than 18e are called unsaturated and can electronically bind additional ligands.

9. A simple example

10. Method 1) There is no overall charge on the complex.
2) There is one anionic ligand (CH3-, methyl group).
3) Since there is no overall charge on the complex (it is neutral), and since there is one anionic ligand present, the Re metal atom must have a +1 charge to compensate for the one negatively charged ligand. The +1 charge on the metal is also its oxidation state. So the Re is in the +1 oxidation state.

11. More examples 1. 2.

12. Metal-metal bonded example

13. Method for metal-metal complexes
The simple rule for M-M bonding is that if you have two metal atoms next to one another and each has an odd electron-count, you pair the odd electrons to make a M-M bond.
This example also has m-Cl ligands. Bridging ligands with at least 2 lone pairs almost always donate 2e- to each metal center.
Oxidation state determination: There is a total of two anionic ligands for two metal centers (overall complex is neutral). Thus each metal center needs to have a +1 oxidation state to balance the anionic ligands.

14. Exceptions to the 18 electron rule

15. Different metals: general properties
From left to right, the electronegativity increases substantially:
Early TM are electropositive:
often found in the highest permissible oxidation state
d2 are very easily oxidized: very p basic
Late TM are relatively electronegative:
Often found in low oxidation states
Back donation is not so marked: ligands are subject to nucleophilic attack
Electronegativity

16. Types of metal-ligand interactions
Sigma (s) donor ligands Pi (p) donor ligands
Pi (p) acceptor ligands
Examples of donor and acceptor ligands
Sigma donor
Pi donor*
Pi acceptor*
CR3- H-
RO-, R2N-
F-, Cl-
RCOO-
CO, olefin
CN-
PR3
These ligands also act as s donors.