Question

The electronic configuration of silicon is ________ and that of sulphur is_______
A.Silicon –$2,8,1$ ; Sulphur- $2,8,6$
B.Silicon - $2,8,4$ ; Sulphur- $2,8,3$
C.Silicon - $2,8,2$ ; Sulphur- $2,8,6$
D.Silicon- $2,8,4$ ; Sulphur- $2,8,6$

Answer 1

Silicon belongs to group $14$ and Sulphur belongs to group $16$ . Both of the elements belong to the p-block of the periodic table. The electronic configuration of both the elements will be the number of electrons in the shell .

Complete step by step answer:
The electronic configuration of any element depends on its atomic number. The atomic number of any element is the number of protons in a neutral atom. The atomic number of Silicon is $14$ and the atomic number of Sulphur is $16$ . The number of protons as well as number of electrons in Silicon and Sulphur 14 and 16 respectively. The number of electrons will determine the electronic configuration.
The filling capacity of $K,L,M$ is $2,8,8$ respectively.
For Silicon, the number of electrons in $K$ is $2$, the number of electrons in $L$ is $8$, the remaining electrons are 4 which goes in $M$ . Its electronic configuration will be $2,8,4$ .
For Sulphur, the number of electrons in $K$ is $2$,the number of electrons in $L$ is $8$, the remaining electrons are $6$ that goes on $2,8$ $M$. Its electronic configuration is $2,8,6$ .
Thus, the correct option is (D).

Note: $2,8$ is the configuration of sodium and will be common to both silicon and sulphur. The number of valence electrons in both will determine their further configuration.