It's not quite accurate to talk about electrons orbiting the nucleus like planets around a star. The quantum mechanical model of the atom describes electrons as existing in probability clouds called orbitals. These orbitals represent regions where there's a high chance of finding an electron.

Here's why the idea of changing the direction of an electron's "orbit" is tricky:

* No defined path: Electrons don't have a set path within an atom. They exist in a fuzzy, probabilistic cloud.

* Quantum jumps: Electrons can only transition between energy levels (orbitals) by absorbing or emitting a specific amount of energy (a photon). This transition is not a smooth change in direction but rather a "quantum jump."

* Spin: Electrons have an intrinsic property called spin, which is like a tiny magnetic field. This spin is quantized, meaning it can only have two values: spin up or spin down. These values are associated with different magnetic moments and can be influenced by external magnetic fields.

What you *can* do:

* External magnetic fields: A strong magnetic field can influence the spin of an electron, potentially causing it to align with the field. This is the basis of magnetic resonance imaging (MRI).

* Electric fields: Electric fields can also influence the motion of electrons, but this is typically studied in the context of electric currents.

In summary: You can't change the direction of an electron's motion in the sense of making it move in a specific circular path. However, you can influence its energy levels, spin, and movement through external magnetic and electric fields.