Question

The electronic configuration of sulphur is
(A). K(2), L(8), M(6)
(B). K(2), L(8), M(8)
(C). K(2), L(6)
(D). K(2), L(8)

Answer 1

- Hint: This type of electronic configuration is based on Bohr Bury Schemes. K, L and M are subshells in which electrons are arranged and the corresponding energy levels are known as 1,2,3 and so on. This model was proposed by Niels Bohr.

Complete step-by-step solution -
In 1913, Niels Bohr proposed the model and the postulates are-
The electron moves in a definite circular path of fixed energy around a central nucleus, just like our solar system in which different planets revolve around the Sun in a definite trajectory. These paths are called orbits, or energy levels. The electron moving in the orbit does not radiate. In other words, it does not lose energy; therefore, these orbits are called stationary orbits or stationary states. The bold concept of stationary state could answer the problem of stability of atm faced by Rutherford’s model.
The shells of definite energy are represented by letters K, L, M, N etc or by positive integers 1, 2, 3, etc. The energies of the shells increase with the number; n=1level is of the lowest energy. Further, the maximum number of electrons that can be accommodated in each shell is given by $2{{\text{n}}^{2}}$ , where n is the number of the level.
Here K can accommodate 2 electrons, L can accommodate 8 electrons and M can accommodate 18 electrons.
Thus, the electronic configuration of sulphur whose atomic number is 16 is given by
K(2), L(8), M(6) and the correct option is (A).

Note: The electron can change its shell or energy level by absorbing or releasing energy. An electron at a lower state of energy ${{\text{E}}_{i}}$ can go to a final higher state of energy ${{\text{E}}_{f}}$ by absorbing a single photon of energy given by-
$\text{E=h}\nu$