In order to explain the observed fine structure of spectral lines, Sommerfeld introduced two main modifications in Bohr's theory.

*Sommerfeld
atom model*

In order to explain the
observed fine structure of spectral lines, Sommerfeld introduced two main
modifications in Bohr's theory.

(i) According to Sommerfeld, the path of an
electron around the nucleus, in general, is an ellipse with the nucleus at one
of its foci.

(ii) The velocity of the electron moving in an
elliptical orbit varies at different parts of the orbit. This causes the
relativistic variation in the mass of the moving electron.

Now, when elliptical orbits are permitted, one
has to deal with two variable quantities.

(i) The varying distance of the electron from the
nucleus (r).

(ii) The varying angular position of the electron
with respect to the nucleus i.e the azimuthal angle φ (Fig).

To deal with these two variables, two quantum
numbers are introduced

(i) The principal quantum number n of Bohr's
theory, which determines
the energy of the
electrons, and

(ii) a new quantum number called orbital (or
azimuthal) quantum number (l) which has been
introduced to characterize the angular momentum in an orbit i.e., it
determines the orbital angular momentum of the electron. Its values vary from
zero to (n-1) in steps of unity.

This orbital quantum number (*l*) is useful in finding the possible
elliptical orbits. The possible elliptical orbits are such that

b/a = l+1/n

where *a*
and *b* are semi-major and semi-minor
axes respectively of the ellipse.

According to Sommerfeld's model, for any
principal quantum number *n*, there are
*n* possible orbits of varying
eccentricities called sub-orbits or sub-shells. Out of *n* subshells, one is circular and the remaining (i.e., *n*-1) are elliptical in shape.

These possible sub-orbits possess slightly
different energies because of the relativistic variation of the electron mass.

Consider the first energy level (*n*=1). When *n* = 1, *l* = 0 i.e., in
this energy level, there is only one orbit or sub-shell for the electron. Also,
when *a = b*, the two axes of the
ellipse are equal. As a result of this, the orbit corresponding to *n*=1 is circular. This subshell is
designated as *s* sub-shell. Since,
this sub-shell belongs to *n*=1, it is
designated as 1s (Fig a).

Similarly, for the second energy level *n*=2, there are two permissible
sub-shells for the electrons. For *n*=2,
*l* can take two values, 0 and 1.

When *n*
= 2, *l* = 0.

b/a= 0+1/2 =1/2

or

b=a/2

This subshell corresponding to *l* = 0 is elliptical in shape and is
designated as 2s.

when *n*
= 2, *l* = 1.

b/a= 1+1/2 =2/2 =1

or

b=a

This sub-shell corresponding to *l* = 1 is circular in shape and is
designated as 2*p* (Fig b).

For n = 3, *l*
has three values 0, 1 and 2, i.e. there are three permissible sub-shells for
the electrons.

when n
= 3, *l* = 0.

b/a= (0+1)/3 =1/3 =1 or b=a/3

when n =
3, *l* = 1.

b/a= (1+1)/3 =2/3 =1 or b=2a/3

and when n = 3, *l* = 2.

b/a= (2+1)/3 =3/3 =1 or b=a

The sub-shells corresponding to *l* = 0, 1 and 2 are designated as 3s, 3*p* and 3*d* respectively. The circular shell is designated as 3*d* and the other two are elliptical in
shape (Fig c).

It is common practice to assign letters to *l*-values as given below:

Orbital quantum number l : 0 1 2 3 4

electron state : s p d f g

Hence, electrons in the *l* = 0, 1, 2, 3 … states are said to be in the *s, p, d, f* … states.

*Fine structure of spectral line*

Based on Sommerfeld atom model, the total
energy of an electron in the elliptical orbit can be shown as,

En = (-me^{4}Z^{2} ) / (8ε_{0}^{2}h^{2}n^{2})

This expression is the same as that obtained by
Bohr. Thus the introduction of elliptical orbits gives no new energy levels and
hence no new transition. In this way, the attempt of Sommerfeld to explain the
fine structure of spectral lines failed. But soon, on the basis of variation of
mass of electron with velocity, Sommerfeld could find the solution for the
problem of the fine structure of the spectral lines.

According to Sommerfeld, the velocity of the
electron is maximum when the electron is nearest to the nucleus and minimum
when it is farthest from the nucleus, since the orbit of the electron is elliptical.
This implies that the effective mass of the electron will be different at
different parts of its orbit. Taking into account the relativistic variation of the mass
of the electron, Sommerfeld modified his theory and showed that the path of
electron is not a simple ellipse but a precessing ellipse called a rosette
(Fig).

Based on this idea, Sommerfeld successfully
explained the fine structure of spectral lines of hydrogen atom.

*Drawbacks*

(i)
Though
Sommerfeld's modification gave a theoretical background of the fine structure
of spectral lines of hydrogen, it could not predict the correct number of
observed fine structure of these lines.

(ii)
It could
not explain the distribution and arrangement of electrons in atoms.

(iii)
Sommerfeld's
model was unable to explain the spectra of alkali metals such as sodium,
potassium etc.

(iv)
It could
not explain Zeeman and Stark effect.

(v)
This
model does not give any explanation for the intensities of the spectral lines.

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11th 12th std standard Class Physics sciense Higher secondary school College Notes : Sommerfeld atom model and its Drawbacks |

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