Write an electronic configuration of elements with an electron sextet, e.g O, S etc.

Hint: According to the octet rule having six electrons in the outermost valence shell instead of the eight valence electrons ensure maximum stability.

Complete step by step solution:
Electronic configuration is the distribution of electrons of an atom or molecule into the respective orbitals of the elements there are total four orbitals with unique shape and valence they are: s orbital, p orbital, d orbital and f orbital.
Three set of rules are followed while writing an electronic configuration of an element according to its atomic number the rules are: Aufbau, Pauli’s exclusion and hund's rule to specify which electron goes to which orbital, spin number and rules such as exceptional stability of fully filled and half filled orbital. The elements with an electron sextet are oxygen, sulphur, selenium and selenium. The atomic number to the elements is 8, 16, 34 and 52 respectively. Hence the electron configuration for the elements is:
O=$1{s^2}2{s^2}2{p^4}$
S=$1{s^2}2{s^2}2{p^6}3{s^2}3{p^4}$
Se=$1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}4{s^2}3{d^{10}}4{p^4}$
Te=$1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}4{s^2}3{d^{10}}4{p^6}5{s^2}4{d^{10}}5{p^4}$
Generally electrons are filled in the orbitals in the fashion as 1s,2s,2p,3s,3p,4s,3d,4p,5s,4d,5p,6s,4f,5d,6p. It is important to know that s orbital can accommodate only 2 electrons , p orbital can accommodate electrons and d orbital can accommodate 10 electrons at max. Whereas an orbital can accommodate 14 electrons.

Note:
There are rules such as after filling the d orbital with 5 electrons even if the orbitals before d orbital are empty as it makes the element exceptionally stable. S orbital starts with one but the first p orbital is 2p and first d orbital is 3d.