Early Quantum Mechanics The Atom

on to the atom. The atom contains electrons and we may influence the energy of those electrons using electromagnetic radiation. Therefore, our discussion of the nature of electrons and light will be significant in the discussion of the atom. Coulomb s Law will also be invoked in the upcoming discussion. 

So finally, our short history leads us to Niels Bohr and early quantum theory. Bohr s analysis of the problem has errors and limited applicability. However, it is the start of a new field, explains the data available at the time and provides an indication of the new direction physical thought had taken. Therefore, we ll treat it in detail here. 

This is known as the Balmer Formula — why is n set equal to integers from 3 to infinity We ll see shortly This equation was later generalized by Rydberg to what we now call the Rydberg Equation 

The constant, 109,680 cm-1 in Eq. 3.2, is often given the symbol Rh and is known as the Rydberg constant for hydrogen. This is what Bohr had to work with in his theoretical development, but as you can see, it is an extremely significant empirical result. Now, we go back to the orbital model with which we began this discussion. What do we know from classical physics 

The centripetal force is Coulombic, after all we are looking at an electron and a collection of protons 

---