6p orbitals

The shape of the three 6p orbitals. From left to right: 6p_y, 6p_z, and 6p_x. For each, the yellow zones are where the wave functions have positive values and the white zones denote negative values.

The three 6p orbitals. Use the previous and next icons to see other views

The three 6p orbitals including orbital nodes. Use the previous and next icons to see other views

Nodes of the three 6p orbitals. Use the previous and next icons to see other views

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For any atom, there are three 6p orbitals. These orbitals have the same shape but are aligned differently in space. The three 6p orbitals normally used are labelled 6p_x, 6p_y, and 6p_z since the functions are "aligned" along the x, y, and z axes respectively.

Each 6p orbital has ten lobes. There is a planar node normal to the axis of the orbital (so the 6p_x orbital has a yz nodal plane, for instance). Apart from the planar node there are also four spherical nodes that partition off the small inner lobes. The 7p) orbital is more complex still since it has five spherical nodes.

The origin of the planar node becomes clear when inspecting the wave equations which, for instance, includes an x term in the case of the 6p_x orbital. When x = 0, then there is a node, and this by definition is the yz plane.

The origin of the spherical nodes becomes clearer when inspecting the wave equations, which include a (840 - 840ρ + 252ρ² - 28ρ³ + ρ⁴) term. When (840 - 840ρ + 252ρ² - 28ρ³ + ρ⁴) = 0, then there are nodes.