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The first step in examining elements and their structure is to understand Hydrogen.  Bohr and Schrödinger both had models of Hydrogen that aid in understanding this structure.  Wavefunction solutions can deduce the probability density in both the radial and angular directions.  This ultimately leads to the "dumbbell" models of electron clouds seen in introductory chemistry classes.

        The energy levels of hydrogen are a function of the quantum number n.  View this applet which shows Bohr and Schrödinger model of the energy levels.  

        1.  What are the Lyman, Balmer, Paschen, and Brackett series?   

        2.  What is the difference between the Bohr and Schrödinger model of energy levels?  What is the condition to exclude an energy transition in the Schrödinger model?

Hydrogen Radial and Angular Probability

     Wavefunction solutions to the Schrödinger equation have radial and angular probability densities.  These applets solve those and give a good visual representation of these probabilities.  To view them you must click on "Radial" or "Angular" from the toolbar on the right of the page.

Radial

        1. What is "n", "l", and "m"?

        2.  What happens when you increase "n" with "l" and "m" equal to zero?  What happens to the R_nl(r) vs r plot?

        3.  Now set n to a value like 4 and increase l.  What happens?

        4.  What is the effect of changing "m"?  Switch "m" from 1 to -1 and explain what happens.  

Angular

        1.  Same set of questions for the angular plot.