Final answer:
The 4 lobe shape of a d orbital represents regions where there is a high probability of finding an electron, and each lobe corresponds to a specific orientation in three-dimensional space. However, the lobes themselves don't signify where an electron will be found with absolute certainty at 90° angles.
Explanation:
A d orbital is one of the five orbitals that can describe the probability density of finding an electron in an atom. The lobes of a d orbital represent regions of space with a high probability of finding the electron. In the case of a d orbital, there are four lobes, each with a specific orientation in three-dimensional space.
These lobes can be found along the x, y, and z axes and are often labeled as dz², dx²-y², dxy, and dxz/dyz orbitals. While the lobes suggest the areas where an electron is likely to be found, the specific position or angle where an electron will be located cannot be precisely determined due to the probabilistic nature of electrons according to quantum mechanics.