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  Shape of p-orbitals

Shape of p-orbitals:

For p-subshell l = 1, there are three values of m that is, -1, 0, +1.This means that p orbitals can have three possible orientations. These three p-orbitals are equivalent in energy (i.e., degenerate state) though differ in their orientations. Each p-orbital consists of two lobes symmetrical around a specific axis. Depending upon the orientation of the lobes, these are symbolized as 2px, 2py and 2pz accordingly as they are symmetrical about X, Y and Z - axis correspondingly.

The line in the figure symbolizes the cross-section of the 3-dimensional boundary surface of p-orbitals. The boundary surface means the surface that encloses 90% of the dots representing the electrons. The two lobes of each p-orbital are separated by a nodal plane (i.e., a plane having zero electron density). For illustration, for 2px orbital, YZ plane is the nodal plane of x.

942_p orbitals.jpg


  

                                                        Figure: Shapes of 2px, 2py and 2pz orbitals

790_p orbitals2.jpg

                                                             Figure: Nodal plane for 2px orbital

Therefore, p-orbitals have dumb-bell shape and encompass directional character. The probability of finding the electron is equivalent in both the lobes. The p-orbitals of higher energy levels have alike shapes though their size are larger.

 

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