The chemistry of elements and compounds is guided by the electrons of atoms. Orbitals, are defined as the matter waves for an allowed energy state of an electron in an atom or molecule. Each orbital corresponds to waves for different energy states. There are four types of orbitals important in chemistry: s, p, d and f.
Studying orbital shapes relies on the Heisenberg uncertainty principle, which states that the position of electrons can not be exactly determined. The probability of the location of electrons in orbitals is used to construct electron density diagrams to illustrate the shapes of those orbitals. Regions where the dot density is thicker are the locations where the electron is most likely to be at any given moment.
This program generates the shapes of orbitals for all orbitals in the range 1s - 4d.
INSTRUCTIONS
1. To view an orbital, simply click on one of the orbital boxes.
The electron density picture will appear, plotted on the appropriate
axes. Note that the image is a two-dimensional cross-section of
the orbital's electron density, and the axes used sometimes differ
