The detailed study of the structure of the atom belongs primarily to physics, but is of extreme interest to chemists since atomic (and molecular) structure determines the physical and chemical properties of the atoms or molecules. The errors in early theories of atomic structure led to the development of Quantum Mechanics, a theory that more properly describes the wave nature of electrons, and hence the electronic structure of atoms and molecules. The focus here will be on concepts rather than the mathematics.
The important concepts you will be familiar with when you have completed these pages include:
- failures of old theories, why Quantum Mechanics is necessary
- what is a wavefunction
- how do the "quantum numbers" relate to the wavefunction
- what are nodes
- what is the "phase" of an orbital
- what are orbitals: their size, shape, number and types of nodes.
A guide to the site is listed below, and the buttons at the bottom of each page will provide sequential access.
| The Orbitals | ||||||||
| 1s | ||||||||
| 2s | 2py | 2pz | 2px | |||||
| 3s | 3py | 3pz | 3px | 3dxy | 3dyz | 3dz2 | 3dxz | 3dx2-y2 |
| 4s | 4py | 4pz | 4px | 4dxy | 4dyz | 4dz2 | 4dxz | 4dx2-y2 |
| 4fy(3x2-y2) | 4fxyz | 4fyz2 | 4fz3 | 4fxz2 | 4fz(x2-y2) | 4fx(x2-3y2) | ||
| Compare the Orbitals |
| The 1s 2s 3s 4s The 3s 3p 3d The 4s 4p 4d 4f |
| Effect of Increasing Nuclear Charge on the Orbitals |
| Compare the 1s Orbital for H, He+, Li+2 |
| The energy of the hydrogen orbitals The mathematics of the hydrogen orbitals |