A d-orbital, defined by the quantum number , is a region of space around the nucleus where an electron is most likely to be found. The letter ”d” is of spectroscopic origin, standing for ‘diffuse’.
One-electron d-orbital wavefunctions can be expressed using the total wavefunction of a hydrogenic atom:
where
, the radial wavefunction, is the radial component of .
, the spherical harmonics, is the angular component of .
are the associated Laguerre polynomials.
are the associated Legendre polynomials.
is the normalisation constant of the radial wavefunction.
is the normalisation constant of the spherical harmonics.
is the principal quantum number, where
is the orbital angular momentum quantum number (also known as azimuthal quantum number), where and .
is the magnetic quantum number, where .
The principal quantum number, , is also called a shell. Since when , there are five d-orbitals that are characterised by the set of quantum numbers of , , , and in each shell for . Four of the five d-orbitals have cloverleaf shapes, while the fifth has a lobular structure along the -axis with a doughnut-shaped region around the equatorial plane. Each of the five d-orbitals has two angular nodes. Consider the set . Substituting these values into the explicit formula for yields:
where .
Converting from spherical coordinates to Cartesian coordinates, where , gives
Eq478 is known as the wavefunction for the orbital. When or , . Therefore, the wavefunction is zero at in spherical coordinates. This implies that the angular nodes occur at two conical surfaces with their apices at the origin, extending at along the -axis.
For the sets and , we have and , respectively. These two wavefunctions include the factor , which may complicate calculations when they undergo symmetry operations. Therefore, we take linear combinations of these wavefunctions to form simpler wavefunctions. The first linear combination is , which normalises to , or equivalently in Cartesian coordinates:
where and .
when or . This implies that has two nodal planes: and .
Question
If and are already normalised, why do we need to normalise a linear combination of them? How do we normalise a linear combination of and ?
Answer
When forming a linear combination of normalised wavefunctions, the result is not necessarily normalised. Consider a general linear combination , where and are coefficients. The normalisation condition for requires that , where represents the volume element in spherical coordinates. Expanding and noting that and are orthonormal, we have . If , which is the case for the two linear combinations of and , will not be normalised.
To normalise , we have or
Since and ,
Using (see this article for proof) and setting and gives .
The second normalised linear combination is , or equivalently,
where and .
when or . This implies that has two nodal planes: and .
For the remaining sets and , we apply the same logic to give and , where . when or , which implies two diagonal nodal planes. when or , which implies two nodes described by the planes and .