To which group and period does the element belong if the electronic configuration of an element in its -2 oxidation state is 1s2 2s2 2p6 3s2 3p6 ?

Question

To which group and period does the element belong if the electronic configuration of an element in its -2 oxidation state is 1s2 2s2 2p6 3s2 3p6 ? (A) period 3 . group 16 (B) period 3 . group 17 (C) period 4 . group 16 (D) period 4 . group 17

Tardigrade Admin · Accepted Answer

Electronic configuration =1 s2, 2 s2, 2 p6, 3 s2, 3 p6 =16 electrons Sulphur (Z=16) refer to group 16 and period 3 . Sulphur show- 2 oxidation state.

Q. To which group and period does the element belong if the electronic configuration of an element in its $- 2$ oxidation state is $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6}$ ?

period 3 . group 16

period 3 . group 17

period 4 . group 16

period 4 . group 17

Electronic configuration $= 1 s^{2}, 2 s^{2}, 2 p^{6}, 3 s^{2}, 3 p^{6}$

$= 16$ electrons

Sulphur $(Z = 16)$ refer to group 16 and period $3.$

Sulphur show- 2 oxidation state.

Q. To which group and period does the element belong if the electronic configuration of an element in its −2 oxidation state is 1s22s22p63s23p6 ?