Question

Name the element which has twice as many electrons in its second shell as in its first shell. Write its electronic configuration also.

Answer 1

The electronic configuration of elements has defined the shell and electrons. With the help of this, the above question can be answered.
The electronic configuration is defined as the distribution of electrons into the orbitals of an atom.

Complete step by step answer:
Carbon has a unique element number and the carbon atomic number is 6.
K shell: 2 electrons
L shell: 4 electrons
Valency can be determined by the K, L, M, N... configuration of the atom. The 2s and 2p are part of the L shell. In K shell 2 electrons can be stored in L shell 8 electrons can be stored.
In that way, the configuration of carbon is 2,4 as 2 in K and 4 in L. Carbon is an element which can do covalent bonding as it will want to achieve the same configuration of the nearest inert gas, in this case, the configuration of the nearest inert gas are He and Ne. To achieve the stable inert gas configuration carbon whether it has to lose or gain four electrons.
In this carbon can’t hold 10 electrons with 6 protons and losing would be difficult due to carbon making covalent bonds instead of ionic bonding.
The electronic configuration of carbon is $1{s^2}2{s^2}2{p^2}$ (2, 4).
The element which has twice as many electrons in its second shell as in the first shell is carbon.
The correct answer is carbon.

Note:
The carbon electronic configuration is written as 2, 4.
In the outermost shell there is a presence of 4 electrons. Carbon undergoes the octet rule and forms 4 covalent bonds with other atoms to get a stable electronic configuration. Carbon is tetravalent (It means the valency of carbon is 4).