OM theory when metals(Ni,Cu,etc) are involved

[demander]

MO theory when metals(Ni,Cu,etc) are involved

i know the TOM theory when envolving only 2nd period/N,O,F,etc) but when a metal of d-block is envolved how the theory works? for example Ni have configuration [Ar]4s2 3d8
but in oxidation 2+ it loses energy so for the OM theory we need to consider the 3s,3p and 3d electrons right? so 16 electrons as the 4s electrons were lost in oxidation... so if we need to connect Ni with N how much the 16 electrons instead the normal 8 afects the situation, i need to see that this connection is paramagnetic, but i have a lot of doubts with the OM theory in situations like this
have we to consider the orbital 2 of N against the 3 of Niquel? nothing changes with the fact of having the d electrons?

 

[Nino MMP]

In terms of the MO theory, when metals like Ni, Cu, etc are involved, it is important to take into account both the s and d orbitals. Since the d orbitals have higher energy than the s orbitals, they will be filled first when forming bonds. In terms of the connection between Ni and N, it is important to note that Ni has 8 electrons in its outermost shell, while N has 5. Therefore, when forming a bond between the two elements, the Ni must donate 3 electrons to the N atom. This will result in a paramagnetic bond, as the electrons are not paired up in the same orbital.

 

[Blueshift5]

I would like to clarify that OM (Orbital Mixing) theory and MO (Molecular Orbital) theory are both used to describe the bonding and properties of molecules. OM theory is a simplified version of MO theory and is often used for simple molecules involving only 2nd period elements like N, O, F, etc. MO theory, on the other hand, is more comprehensive and can be applied to more complex molecules, including those involving d-block metals like Ni and Cu.

In MO theory, the valence electrons of a metal are treated as delocalized and can participate in bonding with other atoms. In the case of Ni, the 4s and 3d electrons are both involved in bonding and can contribute to the formation of molecular orbitals. When Ni is in its 2+ oxidation state, it has a total of 16 valence electrons (8 from 3d and 8 from 4s). These electrons will contribute to the formation of molecular orbitals with other atoms, such as N.

The presence of d electrons in Ni does have an effect on the bonding with N. The 3d orbitals are lower in energy than the 4s and 4p orbitals of N, so they will contribute more to the bonding. This means that the bonding between Ni and N will be stronger and more covalent in nature. This also explains why the connection between Ni and N is paramagnetic, as the unpaired d electrons in Ni contribute to its overall magnetic moment.

In terms of connecting Ni with N, the 16 valence electrons of Ni will be evenly distributed among the molecular orbitals formed between the two atoms. This includes both the 3d and 4s orbitals of Ni, as well as the 2p orbitals of N. The specific interactions between these orbitals will depend on the specific geometry and bonding between the two atoms.

Overall, MO theory provides a more comprehensive understanding of the bonding and properties of molecules involving d-block metals like Ni and Cu. It takes into account the delocalization of electrons and the interactions between different orbitals, providing a more accurate description of the chemical system.