Department of Energy Argonne National Laboratory Office of Science NEWTON's Homepage NEWTON's Homepage
NEWTON, Ask A Scientist!
NEWTON Home Page NEWTON Teachers Visit Our Archives Ask A Question How To Ask A Question Question of the Week Our Expert Scientists Volunteer at NEWTON! Frequently Asked Questions Referencing NEWTON About NEWTON About Ask A Scientist Education At Argonne Electron Shells and Bohr Model
Name: Dale H.
Status: educator
Age: 40s
Location: N/A
Country: N/A
Date: 10/8/2003


Question:
One of my 10th grade science students asked a questions regard the Bohr model of the atom which I could not answer. She asked "How did Bohr know that the first electron shell held only 2 electrons? then, how did he know the second held only 8?"


Replies:
Bohr's initial contribution was the explanation of the electronic spectrum of the hydrogen atom, which contains only a single electron. The extension of idea to atoms containing more than a single electron depended upon a rapid succession of both experimental and theoretical results. For example, Franck and Hertz (between 1914 and 1920) measured the energy of electrons scattered from various targets. They found two things:

1. The scattered electrons usually had much less energy than the incident electrons, but that change in energy occurred in steps.

2. Sometimes more electrons were produced (current) than were incident upon the target.

We now know that those observations corresponded to the incident electrons exciting electrons in the target to higher energy levels, and to the ionization of the target electrons, respectively.

Concurrently, in the area of atomic theory Schroedinger (and others) were developing what we now refer to as quantum mechanics. First, for atoms containing a single electron, and later extended to multi-electron atoms. The result of the theory of multi-electron atoms was that stable electronic states corresponded to appearance of certain integers (we now refer to them as quantum numbers). The results of the theory for atoms required the following constraints on the values of those quantum numbers: There were 3 quantum numbers (n, l, s). Pauli showed that no two electrons in an atom could have the same set of (n, l, s). The details of this history is too large to present in detail here, but you will find it explained very well in the classic text"General Chemistry" by Linus Pauling Chapter 5.

Vince Calder


Bohr was about 1912 with all this, I think. At that time, he would have known how many electrons are in a shell by spectroscopic measurements. New energy levels would show up, new emission lines, for the elements as one went from hydrogen on up. This would first be put into ad-hoc rules (by the spectroscopists) but then given a mathematical basic by quantum mechanics maybe 15 years later.

I suggest you read or recommend the student read The Ascent of Man, by Jacob Bronowski. There are some good history chapters in it, of these early days. There was a PBS TV series by him (the book came from the TV), it may still be in libraries. There are many such books, but I have always liked this one. It is fine for 10th grade.

Steven Ross



Click here to return to the Chemistry Archives

NEWTON is an electronic community for Science, Math, and Computer Science K-12 Educators, sponsored and operated by Argonne National Laboratory's Educational Programs, Andrew Skipor, Ph.D., Head of Educational Programs.

For assistance with NEWTON contact a System Operator (help@newton.dep.anl.gov), or at Argonne's Educational Programs

NEWTON AND ASK A SCIENTIST
Educational Programs
Building 360
9700 S. Cass Ave.
Argonne, Illinois
60439-4845, USA
Update: June 2012
Weclome To Newton

Argonne National Laboratory