# How does the anti-bonding eg orbital (eg*) affect the bonding of ligands?

In the molecular orbital for octahedral metal-ligand complexes, there is an eg orbital and an eg* orbital. When the d orbitals on the metal split, it will fill up some of the eg* orbitals I believe. However, my question is that won't these orbitals cancel out with the eg orbitals and make fewer bonds? For example, $$\ce{Ni^{2+}}$$is a $$\ce{d^8}$$ metal and will split in the presence of ligands and will partially fill the eg* orbitals. The $$\ce{Ni^{2+}}$$ metal can then form complexes like $$\ce{[Ni(H_2O)_6]^{2+}}$$ with 6 ligands attached. My question is how would the filling of the eg* orbitals affect the bonding and chemical properties of the compound? Here is the diagram I am referencing to:

• It might be more clear if you indicate that the t and e levels represent 3 and 2 orbitals, respectively, even though there is only one line. Thus a d8 metal has the e* level only half-filled. – Andrew Mar 21 at 12:20
• Sure, I will change it. Thanks. – M.L Mar 21 at 18:02
• Short answer: slightly reduced bond order. As for effect on chemical properties, what is your reference point for comparison? – Andrew May 6 at 11:27