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  Shape of s-orbitals

Shape of s-orbitals:

For s-orbitals, if l = 0, the value of m is 0 that is, there is only one possible orientation. It means that the probability of finding an electron is similar in all directions at a specified distance from the nucleus. It must, thus, be spherical in shape. Therefore all s-orbitals are non- directional and spherically symmetrical around the nucleus.

The size of an s-orbital depends upon the value of principal quantum number n. Greater the value of ‘n’ is, larger is the size of the orbital.

1200_s orbitals.jpg


                                                            Figure: Shapes of 1s and 2s-orbitals

A significant feature of the 2s-orbital is that there is a spherical shell in this orbital where the probability of finding the electron is zero. This is termed as a node or nodal surface. In 2s orbital there is only one spherical node. The number of nodes or nodal surfaces in s-orbital of any energy level is equivalent to (n-1); here n is the principal quantum number.

 

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