Shape of orbitals

         (1) Shape of 's' orbital

         (i) For the 's' orbital l=0 & m=0 so 's' orbital have one unidirectional orientation only that is the probability of finding the electrons is same in all the directions.

         (ii) The size and energy of the 's' orbital with the increasing 'n' will be given by 1s < 2s < 3s < 4s.

(iii) s-orbitals also called as radial node or modal surface. However there is no radial node for 1s orbital since it is beginning from the nucleus.

(2) Shape of 'p' orbitals

         (i) For the 'p' orbital l=1, & m=+1,0,-1 means that there are three 'p' orbitals, which can be symbolised as p_x, p_y, p_z

        (ii) The shape of 'p' orbital is a dumb bell in which the two lobes on the opposite side are separated by the nodal plane.

         (iii) p-orbital has the directional properties.

 (3) Shape of 'd' orbital

         (i) For 'd' orbital l =2 then values of 'm' can be given as -2, -1, 0, +1, +2.   This shows that 'd' orbitals has five orbitals which are given by 

         (ii) Each 'd' orbital is identical in size, shape and energy.

         (iii) The shape of the d orbital is a double dumb bell.

         (iv) It also has directional properties.

(4) Shape of 'f' orbital

         (i) For 'f' orbital the l=3 then the values of  'm' can be given as -3, -2,  -1,0,+1,+2,+3. It shows that 'f' orbitals have seven orientation which can be   given as 

         (ii) The 'f' orbital is quite complicated in shape.

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