Posted: Sun May 20, 2018 11:39 am
I'm a bit confused about this phrase "empty d-orbital", because earlier in the course I got the sense that orbitals are states that electrons can be in, rather than locations. My understanding is that when an atom has no electrons in a d-orbital state, then the d-orbital does not exist for that atom. So how can there be an empty orbital? What is a better way to understand why atoms, row 3 and below, can accommodate more than eight valence electrons in bonding?