Bonding in coordination complexes

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Copper(I) can exhibit a coordination number of 3 in compounds like [Cu(P(C6H5)3)3]+ due to its ability to form bonds with ligands through empty orbitals. In this case, the copper ion has a +1 charge and an electron configuration of [Ar] 4s0 3d10, allowing it to utilize its 4p orbitals for bonding with the lone pairs from the phosphine ligands. The 4s orbital is typically not involved in bonding for copper(I) in this scenario. To determine the coordination number of a metal with ligands, one can analyze the number of donor atoms from the ligands that coordinate to the metal center. Further resources on coordination chemistry can provide more detailed methodologies for understanding these interactions.
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For metals like copper(I), how does it have a coordination number of 3 in some compounds like [Cu(P(C6H5)3)3]+. I've learned that these coordination bonds are formed by interacting lone pairs from ligands and empty orbitals on the central metal atom. In this case, copper has a 1+ charge and configuration of [Ar] 4s0 3d10 and I'm just slightly confused on how it would form 3 bonds...
Would new bonds just be formed between the lone pair on each phosphorous and the 3 4p orbitals from copper? What happens to the 4s orbital in this case?

If there's a method to determine the coordination number of a metal with ligands, could you please expand on that as well or refer me to any sources?

Thanks!
 
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