Question 17 (1 point} Bohr developed his model by applying Newton's second law of motion {F = ma) to an electron. The net force is described as Coulomb's law for the interaction between an electron of charge I: -q that is a distance r from a proton of charge +q. that force would be F = %. The acceleration of the electron is in circular orbit. so the acceleration of the electron's orbit 2 around the more massive proton is given by a : If. This gives the equation k 2 % : % which should look familiar. Bohr also had to look at angular momentum of the orbiting electron, which is beyond physics 30, but this is where Planck's constant comes in. Using the above classical physics and quantum ideas Bohr came up with the following equation to solve for orbital radii of the electron in a hydrogen atom. hgng T : n. 411:2 kmqg Determine the orbital radius, in m. of an electron in the orbital. n = [1.0000x10"0) around a hydrogen atom. Note: Your answer is assumed to be reduced to the highest power possible. Your