D-orbital elements

[305920501]

Are there any real-world examples of molecules where the elements that can utilize the d-orbital fill the entire 10 possible spaces for electrons (for example with Iodine)? Are these molecules more or less stable than those that only fill an octet?

[Averie Moore 2F]

I'm not sure how to answer the first part of your question but d-orbital elements prefer to be in either a half or filled subshell. They are more stable this way due to their allowance of a symmetrical distribution of electrons.

[Isabelle Huerta 2I]

Sulfur, in its bonding with six fluorine atoms, exceeds the octet rule by utilizing its empty d-orbitals, accommodating a total of 12 electrons around the sulfur atom.
Another example, Phosphorus can have an expanded octet by bonding with five chlorine atoms, utilizing its empty d-orbitals to accommodate a total of 10 electrons around the phosphorus atom. These molecules are relatively stable despite violating the octet rule because the d-orbitals of the central atoms are available for bonding, allowing them to accommodate more than eight electrons.