Class I:
In class I complexes, the Δo splitting is small and often applies to 3d metals and σ ligands at lower end of the spectrochemical series. In this case the t2g orbital is nonbonding in nature and may be occupied by 0−6 electrons (Figure 2). The eg* orbital is weakly antibonding and may be occupied by 0−4 electrons. As a consequence, 12−22 valence electron count may be obtained for this class of compounds. Owing to small Δtetr splitting energy, the tetrahedral transition metal complexes also belongs to this class.

Class II:
In class II complexes, the Δo splitting is relatively large and is applicable to 4d and 5d transition metals having high oxidation state and for σ ligands in the intermediate and upper range of the spectrochemical series. In this case, the t2g orbital is essentially nonbonding in nature and can be filled by 0−6 electrons (Figure 3). The eg* orbital is strongly antibonding and is not occupied at all. Consequently, the valence shell electron count of these type of complexes would thus be 18 electrons or less.

Class III:
In class III complexes, the Δo splitting is the largest and is applicable to good σ donor and π acceptor ligands like CO, PF3, olefins and arenes located at the upper end of the spectrochemical series. The t2gorbital becomes bonding owing to interactions with ligand orbitals and should be occupied by 6 electrons. The eg* orbital is strongly antibonding and therefore remains unoccupied.

Problems:

State the oxidation state of the metal and the total valence electron count of the following species.

1. V(C2O4)33−

Ans: +3 and 14 2. Mn(acac)3 Ans: +3 and 16 3. W(CN)83− Ans: +5 and 17 4. CpMn(CO)3 Ans: 0 and 18 5. Fe2(CO)9 Ans: 0 and 18 Self Assessment test

State the oxidation state of the metal and the total valence electron count of the following species.

1. TiF62-

Ans: +4 and 12 2. Ni(en)32+ Ans: +2 and 20 3. Cu(NH3)62+ Ans: +2 and 21 4. W(CN)84- Ans: +4 and 18 5. CH3Co(CO)4 Ans: 0 and 18

 

 

 

Summary:

The transition metal complexes may be classified into the following three types. (i). The ones that do not obey the 18 valence electron rule are of class I type (ii). the ones that do not exceed the 18 valence electron rule are of class II and (iii). the ones that strictly follow the 18 valence electron rule. Depending upon the interaction of the metal orbitals with the ligand orbitals and also upon the nature of the ligand position in spectrochemical series, the transition metal organometallic compounds can form into any of the three categories.

The 18-electron rule is used primarily for predicting and rationalizing formulae for stable metal complexes, especially organometallic compounds. The rule is based on the fact that the valence shells of transition metals consist of nine valence orbitals (one s orbital, three p orbitals and five d orbitals), which collectively can accommodate 18 electrons as either bonding or nonbonding electron pairs. This means that, the combination of these nine atomic orbitals with ligand orbitals creates nine molecular orbitals that are either metal-ligand bonding or non-bonding. When a metal complex has 18 valence electrons, it has achieved the same electron configuration as the noble gas in the period. The rule and its exceptions are similar to the application of the octet rule to main group elements.

This rule applies primarily to organometallic compounds, and the 18 electrons come from the 9 available orbitals in d orbital elements (1 s orbital, 3 p orbitals, and 5 d orbitals). The rule is not helpful for complexes of metals that are not transition metals, and interesting or useful transition metal complexes will violate the rule because of the consequences deviating from the rule bears on reactivity. If the molecular transition metal complex has an 18 electron count, it is called saturated. This means that additional ligands cannot bind to the transition metal because there are no empty low-energy orbitals for incoming ligands to coordinate. If the molecule has less than 18 electrons, then it is called unsaturatedand can bind additional ligands.

 

 

 

Electron counting:

Two methods are commonly employed for electron counting:

1. Neutral atom method: Metal is taken as in zero oxidation state for counting purpose

2. Oxidation state method: We first arrive at the oxidation state of the metal by considering the number of anionic ligands present and overall charge of the complex

To count electrons in a transition metal compound:

1. Determine the oxidation state of the transition metal and the resulting d-electron count.

• Identify if there are any overall charges on the molecular complex.

• Identify the charge of each ligand.

1. Determine the number of electrons from each ligand that are donated to the metal center.

2. Add up the electron counts for the metal and for each ligand.

Reactivity:

The 18 electron rule allows one to predict the reactivity of a certain compound. The associative mechanism means that there is an addition of a ligand while a dissociative mechanism means that there is a loss of a ligand. When the electron count is less than 18, a molecule will most likely undergo an associative reaction. For example: (C2H4)PdCl2

• 16 electron count

• Would it more likely lose a C2H4 or gain a CO? Losing a C2H4 results in a 14 electron complex while gaining a CO gives an 18 electron complex. From the 18 electron rule, we will expect that the compound will more likely undergo an associative addition of CO.

 

 

Example :

:

 

 

 

 

1. There is no overall charge on the molecule and there is one anionic ligand (CH3-)

• The Re metal must have a positive charge that balances out the anionic ligand charge to equal the 0 overall molecular charge. Since there is a -1 charge contribution from the methyl ligand, the Re metal has a +1 charge.

• Because the Re metal is in the +1 oxidation state, it is a d6 electron count. It would have been its regular d7 electron count if it had a neutral (0) oxidation state.

1. The CH3- ligand contributes 2 electrons. Each CO ligand contributes 2 electrons. Each PR3 ligand contributes 2 electrons. The H2C=CH2 ligand contributes 2 electrons.

2. Adding up the electrons:

• Re(1): 6 electrons

• CH3-: 2 electrons

• 2 x CO: 2 x 2 electrons = 4 electrons

• 2 x PR3: 2 x 2 electrons = 4 electrons

• H2C=CH2: 2 electrons

• Total: 18 electrons

In this example, the molecular compound has an 18 electron count, which means that all of its orbitals are filled and the compound is stable

Example :

: [M(CO)7]+

The 18 electron rule can also be used to help identify an unknown transition metal in a compound. Take for example [M(CO)7]+. To find what the unknown transition metal M is, simply work backwards:

1. 18 electrons

2. Each (CO) ligand contributes 2 electrons

• 7 x 2 electrons = 14 electrons

1. 18 - 14 = 4 electrons

2. d4

3. M(I) oxidation state

4. The unknown metal M must be V, Vanadium

Example:

: [Co(CO)5]z

Similarly to Example 2, the 18 electron rule can also be applied to determine the overall expected charge of an molecule. Take for example [Co(CO)5]z. To find the unknown charge z:

1. 18 electrons

2. Each CO ligand contributes 2 electrons

3. 5 x 2 electrons = 10 electrons

4. Co is typically d9

5. 9 + 10 = 19 electrons

6. To satisfy the 18 electron rule, the [Co(CO)5]z compound must have a charge of z = +1

7.