In the long or modern form of the periodic table, the element in the periodic table have been divided into four blocks, `s-p-d`-and `f`-. Each period begins with the filling of new energy shell. Two series of `f`-block elements are placed at the bottom of the periodic table.
The last element of the `p`-block in the present periodic table is represented by the configuration, where `[X]` represents inert gas is

Options

A. `[X]7s^(2)p^(6)`
B. `[X]5f^(14),6d^(10),7s^(2)7p^(5)`
C. `[X]4f^(14),5d^(10),6s^(2)6p^(6)`
D. `[X]` None of the above

Answer

C

Explanation

Last element of the `p`-block is `Rn` with `Z = 86`, group `18`, period `6`.
Therefore, its valence electronic configuration is `6s^(2) 6p^(6)`.