1) An orbital is a three dimensional description of the most likely location of an electron around an atom. There are four types of orbitals that you should be familiar with s, p, d and f (sharp, principle, diffuse and fundamental).
So here are a couple of pictures of atoms with their shells populated by electrons to help you remember this atomic theory. So now that we have reminded ourselves about the orbitals and how the electrons fill them, we need to address how these orbitals interact when two or more atoms bond together.

Below is a diagram that shows the probability of finding an electron around the nucleus of a hydrogen atom. For this process, we will discuss other theories: The Valence Bond Theory and The Molecular Orbital Theory.
In the n=1 shell you only find s orbitals, in the n=2 shell, you have s and p orbitals, in the n=3 shell, you have s, p and d orbitals and in the n=4 up shells you find all four types of orbitals. As with any theory, these explanations will only stand as truth until someone (you maybe?) comes up with a better explanation or description.

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