Silicon, Circuits, and the Digital Revolution

Introduction to Electronic Structure

### Review of Atomic Physics

 Schematic of helium atom. What's wrong with it? Each atom has a number of electrons about the nucleus. Energy levels of electrons in an atom are quantized (discrete levels) Electron may be elevated to excited state by addition of energy "Excited" electron can relax to lower level by emitting photon. Example of emission spectrum: hydrogen; (from bluegiant.phys.ksu.edu)

### Pauli Exclusion Principle

How do electrons "stack up" in the atom?
Each electron in an atom must have a unique state;
that is, each electron must have a different set of quantum numbers
(n, l, m, s)
Classroom seating analogy
- no two students in same seat
- each seat may be indexed by row and "column" (in auditorium)
The energy is primarily determined by the prinicipal quantum number
n = 1, 2, 3, ...     - recall the hydrogen spectrum.
Then follows the so-called orbital angular momentum values l,m
Followed by spin s, either spin-up, s=+1/2, or spin-down, s=-1/2.

A particular atomic orbital has fixed values of n, l, and m and can thus contain a maximum of TWO electrons (one of each spin).

### Building Elements

Each additional electron gives the electron "cloud" of the atom a much different behavior -- That is why each element is different.

Only two electrons may go into the lowest energy state,
known as the 1s state, with (n,l,m)=(1,0,0)
Two more may go into the 2s state, with (n,l,m)=(2,0,0)
Six may go into the 2p state,
since there are 3 different angular momentum values:
(2,1,-1), (2,1,0), (2,1,1)

### Periodic Table

Examine an abridged Periodic Table
 hydrogen: 1s1 helium: 1s2 lithium: 1s2, 2s1 beryllium: 1s2, 2s2 boron: 1s2, 2s2, 2p1 carbon: 1s2, 2s2, 2p2 nitrogen: 1s2, 2s2, 2p3 oxygen: 1s2, 2s2, 2p4 flourine: 1s2, 2s2, 2p5 neon: 1s2, 2s2, 2p6 sodium: [Ne] 3s1

### Chemistry

Much of chemistry depends on how "filled" the shells are:
A filled shell is a very stable configuration