To understand the Bohr model of the hydrogen atom. In 1913 Niels Bohr formulated a method of calculating the different energy levels of the hydrogen atom. He did this by combining both classical and quantum ideas. In this problem, we go through the steps needed to understand the Bohr model of the atom.

Consider an electron with charge -e and mass m orbiting in a circle around a hydrogen nucleus(a single proton) with charge +e . In the classical model, the electron orbits around the nucleus, being held in orbit by the electromagnetic interaction between itself and the protons in the nucleus, much like planets orbit around the sun, being held in orbit by their gravitational interaction. When the electron is in a circular orbit, it must meet the condition for circular motion: The magnitude of the net force toward the center, Fc, is equal to mv2 / r. Given these two pieces of information, deduce the velocity v of the electron as it orbits around the nucleus.