You are at: University of Sheffield » Chemistry » Mark Winter » Orbitron (atomic orbitals and molecular orbitals)
WebElements Chemdex Chemputer
Introduction Wave function Electron density Dots! Radial distribution Equations

Atomic orbitals: 3d

The shape of the five 3d orbitals. From left to right: (top row) 3dx2-y2 and 3dz2 (bottom row) 3dxy, 3dxz, and 3dyz. For each, the yellow zones are where the wave functions have negative values and the blue zones denote positive values.

For each atom, there are five 3d orbitals. These are labelled 3dxy, 3dxz, 3dyz, 3dx2-y2 and 3dz2. Four of these functions have the same shape but are aligned differently in space. The fifth function (3dz2) has a different shape.

Each 3dxy, 3dxz, 3dyz, and 3dx2-y2 orbital has four lobes. There are two planar node normal to the axis of the orbital (so the 3dxy orbital has yz and xz nodal planes, for instance). The 3dz2 orbital is different and has two conical nodes.

The origin of the planar nodes becomes clear if we examine the wave equations which, for instance, includes an xy term in the case of the 3dxy orbital. Clearly when either x = 0 or y = 0, then we must have a node, and this by definition is the case for the yz and a xz planes.

The higher d-orbitals (4d, 5d, and 6d) are more complex since they have some spherical nodes.

Orbitron logo
Copyright Feedback The images Acknowledgments Problems? References

The Orbitron is a gallery of orbitals on the WWW

The OrbitronTM, a gallery of orbitals on the WWW, URL:
Copyright 2002-2015 Prof Mark Winter [The University of Sheffield]. All rights reserved.
Document served: Wednesday 21st October, 2020