What is the shape of orbitals ? Here, we will discuss how to find the shape of s, p and d orbitals.
What is the shape of orbitals ?
An orbital is the region around the nucleus where the probability of finding the electron is maximum.
We get the value of psi, orbital wave equation by solving the Schrodinger wave equation. But psi has no physical significance. Instead, | psi ^2 | has the significance. It gives the electron probability density of the electron.
In case of 1s, the probability of finding the electron is maximum near the nucleus.
In case of 2s electrons, the probability is maximum near the nucleus, then decreases to 0 and again increases. And there after again decreases. The region where the probability of finding the the electron is 0 is called node.
In s orbital, probability of finding the electron is same in all the directions around the nucleus. Therefore, s orbitals are spherical in shape.
What is the shape of p orbitals
P orbital has 2 lobes on the opposite sides of the nucleus. This gives rise to a dumb-bell shaped orbital. The probability of finding the electron is maximum in the 2 lobes but 0 at the node.
P orbitals have 3 different orientations. They are designated as Px, Py and Pz orbitals. Here the electron density will be maximum along the x axis, y axis and z axis respectively. For p orbital, l =1 Therefore, m = -1, 0, +1 which means p orbitals have 3 orientations.
The 3 orbitals Px, Py, and Pz are the degenerate orbitals having energies. 2p has no node, 3p has 1 node and 4p has 2 nodes.
Number of nodes = n -l – 1
What is the shape of d orbitals
For d orbitals, l = 2. Therefore, m = -2, -1, 0 +1, +2 which shows there are 5 d orbitals.
The shape of d orbitals is double dumb-bell or clover shaped. But dz^2 is doughnut shaped orbital.
Check out the structure of NH3 here
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