Shapes of Atomic Orbital’s

Shapes of Atomic Orbital’s

An orbital is the region of shape around the nucleus within which the probability of finding an electron of a given energy is maximum (90-95%). The shape or contour diagram of this region of electron cloud gives the shape of the orbital. It is fundamentally determined by the Azimuthal quantum number (l), while the orientation of orbital depends on the magnetic quantum number (m). Let us now see the shapes of different orbital in the various subshells.

s-orbital’s(l=o) 

These orbital are spherical and symmetrical about the nucleus. The probability of finding the electron is zero near the nucleus keep on increasing as the distance from nucleus increase, becomes maximum and thereafter decreases.

The size of the orbital depends upon the value of principal quantum number (n). Greater the value of n, large is the zero of the orbital. Therefore, 2s orbital is large the 1s orbital but both of them are non-direction and spherically symmetrical is shape.

Closer inspection of 2s orbital suggests that there is vacant space between two successive s-orbital know as radial node or nodal surface. So, 2s orbital suggest is characterized with one radial node. However, there is no radial node for 1s orbital since it is starting from the nucleus.

p-orbital(l=1)

The probability of finding the p-electron is maximum in two lobes on the opposite side of the nucleus. This gives rise to a dumb- bell shape for the p-shape the p-orbital. For p-orbital l = 1. Hence, m = -1, o, +1.  Thus, p-orbital have three different orientations. These are designated as p_x , p_y, and p_z depending upon whether the density of electron is maximum along the x, y, and z- axis, respectively. They are symmetrical but have direction characters. The two lobes of p-orbital are separated by a nodal plane, where the probability of finding electron is zero.

The three p-orbital belonging to a particular energy shell have have equal energies and are called degenerate orbital.-

d-orbital’s(l = 2) :-

For d –orbital’s, l = 2, Hence m = -2, -1, 0, +1, +2 5 different values of m suggests that there are 5d-orbital’s--  d_xy d_yz d_zx p_z²  and d_x²_-y² . They have relatively complex geometry. Out of the five orbitals, the three (d_xy d_yz d_zx) project in between the axis and the other two and the other two p_z² and d_x²_-y² lie along the axis.

f-orbital’s :--

Foe f-orbitals, l = 3, Hence m = -3, -2, -1, 0, +1,+2, +3. Thus there are 7 f-orbital. They have relatively complex geometry.