Atomic orbitals: 6g equations
The symbols used in the following are:
 r = radius expressed in atomic units (1 Bohr radius = 52.9 pm)
 π = 3.14159 approximately
 e = 2.71828 approximately
 Z = effective nuclear charge for that orbital in that atom.
 ρ = 2Zr/n where n is the principal quantum number (5 for the 6g orbitals)
 k = various constants
Table of equations for the 6g orbitals.
Function 
Equation 
Radial wave function, R_{6g} 
= (1/900√70) × (8  ρ)ρ^{4} × Z^{3/2} × e^{ρ/2} 
Angular wave functions: 

Y_{6gz4} 
= k × (35z^{4}  30z^{2}r^{2} + 3r^{4})/r^{4} × (1/4π)^{1/2} 
Y_{6gz3x} 
= k × xz(4z^{2}  3x^{2}  3y^{2})/r^{4} × (1/4π)^{1/2} 
Y_{6gz3y} 
= k × yz(4z^{2}  3x^{2}  3y^{2})/r^{4} × (1/4π)^{1/2} 
Y_{6gz2xy} 
= k × xy(6z^{2}  x^{2}  y^{2})/r^{4} × (1/4π)^{1/2} 
Y_{6gz2(x2  y2)} 
= k × (x^{2}y^{2})(6z^{2}  x^{2}  y^{2})/r^{4} × (1/4π)^{1/2} 
Y_{6gzx3} 
= k × xz(x^{2}  3y^{2})/r^{4} × (1/4π)^{1/2} 
Y_{6gzy3} 
= k × yz(3x^{2}  y^{2})/r^{4} × (1/4π)^{1/2} 
Y_{6gxy(x2y2)} 
= k × xy(x^{2}  y^{2})/r^{4} × (1/4π)^{1/2} 
Y_{6gx4 + y4} 
= k × (x^{4} + y^{4}  6x^{2}y^{2})/r^{4} × (1/4π)^{1/2} 
Wave functions: 

ψ_{6gz4} 
= R_{6g} × Y_{6gz4} 
ψ_{6gz3x} 
= R_{6g} × Y_{6gz3x} 
ψ_{6gz3y} 
= R_{6g} × Y_{6gz3y} 
ψ_{6gz2xy} 
= R_{6g} × Y_{6gz2xy} 
ψ_{6gz2(x2  y2)} 
= R_{6g} × Y_{6gz2(x2  y2)} 
ψ_{6gzx3} 
= R_{6g} × Y_{6gzx3} 
ψ_{6gzy3} 
= R_{6g} × Y_{6gzy3} 
Electron density 
= ψ_{6g}^{2} 
Radial distribution function 
= r^{2}R_{6g}^{2} 
The radial equations for all the 6g orbitals are the same. The real angular functions differ for each and these are listed above.
For sorbitals the radial distribution function is given by 4πr^{2}ψ^{2}, but for nonspherical orbitals (where the orbital angular momentum quantum number l > 0) the expression is as above. See D.F. Shriver and P.W. Atkins, Inorganic Chemistry, 3rd edition, Oxford, 1999, page 15.
