For example: Yttrium: 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d1 5s2 The outermost orbital is the s-orbital but d-orbital is unfilled. How does overlap of orbital take place in YCl3 as d-orbital is beneath s-orbital Is it because there is no covalent bonding taking place. How can we interpret ionic bonding or metallic bonding in terms of orbitals?


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