How can electrons still occupy orbitals in metals if they are delocalised?
Because they're not even localized in say a hydrogen orbital. Check out atomic orbitals on Wikipedia where you can read this: "The electrons do not orbit the nucleus in the sense of a planet orbiting the sun, but instead exist as standing waves". They exist as waves, and waves are delocalised. Even ordinary waves. Take a look at the Wikipedia Wind wave article where you can see this gif:
GNUFDL image by Kraaiennest, see Wikipedia
You might think of an ocean wave as something that's a metre-high hump on top of the sea. But look at the red test particles in the animation above. They go round and round, and this motion still occurs deep under the water. It diminishes with depth, but nevertheless the wave takes "many paths" and isn't localized to the metre-high hump. The wave nature of matter means electrons aren't totally unlike this. Don't think of them as little billiard-ball things. Don't think of an electron as some little ball that has a field, instead think the electron's field is what it is. And this field doesn't have an edge. So an electron in an ordinary orbital is not localized anyway. So when it's say a 3s electron in a metal, it's even less localized, but the change isn't so drastic.
I was reading about why most metals are gray/silvery in colour and it said something about d orbital electrons transitioning to s orbitals and the visible spectrum not having sufficient energy to raise them.
IMHO it's worth having a google on electrons shiny. Metals are shiny because of the free electrons.
But take Scandium for example, it forms a $Sc^{+3}$ ion, so it has no d electrons and these are now delocalised. How can these delocalised electrons still occupy the orbital?
Noting Gert's answer re Scandium Chloride, it's because they're in "molecular" orbitals. See this article by Jim Clark which IMHO explains it fairly well: "The electrons can move freely within these molecular orbitals, and so each electron becomes detached from its parent atom. The electrons are said to be delocalised. The metal is held together by the strong forces of attraction between the positive nuclei and the delocalised electrons." IMHO it would be better if the electrons were shown as red circles fading to pink around the metal ion rather than red dots, but nevermind. I am reminded of a barn dance myself, where you swap partners.