No! I will not relive the horrors of that chemistry class again... you can't make me. I am happily an aerospace engineer now where I don't need this chemistry nonsense, or quantum mechanics.

All the spaces there are all the possible locations for the electrons.

Close, but not quite - the spaces are the most likely locations for the electrons at any moment in time. There is always a small chance they've fucked off over the street for a nanosecond when you take your measurement.

Except they only look like that if there is an external reference system imposing some structure on the atom! Otherwise all orbitals are basically spherical because they can all just be in a superposition of all possible orbitals and we couldn't tell a difference...

And then suddenly you have two atoms meeting and need to explain why 1+1=0 for their molecular orbits -.-

I don't think so. Orbitals give you the spaces of highest probability! Electrons could be outside as well. And since it is based on probability it is definitely a useful model.

Electronic orbitals are regions within the atom in which electrons have the highest probability of being found.

https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Supplemental_Modules_(Physical_and_Theoretical_Chemistry)/Quantum_Mechanics/09._The_Hydrogen_Atom/Atomic_Theory/Electrons_in_Atoms/Electronic_Orbitals

Then you get to "orbital hybridization" and everything quickly goes downhill.