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## Homework Statement

In the classical Bohr model of the hydrogen atom, the nucleus has one positive electronic charge Q_n = e = +1.602E-19 Coulombs and the single electron (mass = 9.1E-31 kg and Q_e = -e = -1.602E-19 C, one negative electronic charge) orbits the nucleus in a circular orbit. In the Bohr model, stable orbits result only when the angular momentum is an integral multiple of h/(2\pi) (remember,

**L**=

**r**x

**p**, but for circular orbits

**r**is perpendicular to

**p**, so here L = mvr = n(h/2\pi) and h = Planck's constant = 6.626E-34 J-s.

a) Calculate the speed with which the electron must orbit the proton for the ground state (n = 1) in the Bohr model of the hydrogen atom.

b) What is the radius of this ground state orbit? You probably know from Chemistry that the atomic size is about an Angstrom (10E-10 m). Is your answer close to this?

## Homework Equations

[tex]L = mvr = \frac{nh}{2\pi}[/tex]

Not sure if this one is needed, but:

[tex]F = \frac{1}{4\pi\epsilon_0} \frac{|q_1q_2|}{r^2}[/tex]

## The Attempt at a Solution

From the first equation,

[tex]v = \frac{nh}{2\pi mr}[/tex]

I know what n, h, and m are, but I don't have r (well, I know it's .529E-10, but I can't use it). For this reason, I'm trying to use the second equation to find r from the charge values for the proton and electron, but I don't know F, the force on each charge. Any ideas?

Thanks!