Question

Under certain conditions, the stable form of sulfur consists of rings of eight sulfur atoms. Draw the Lewis diagram for such a ring.

Short answer

The Lewis diagram for ${\mathrm{S}}_8$ring is,

Step-by-step solution

Introduction.

Certain elements in period 3 tend to form not diatomic molecules under standard conditions.
Sulfur is one example. While its "analogue", oxygen has a most common molecular formula ${\mathrm{O}}_2$, such structure of this larger atom can be seen mostly in vapor state. However, the ${\mathrm{S}}_8$sulfur rings follow the norms of Group VI.A anyway: two bonds and two lone pairs.

Images

The image below depicts the Lewis structure of an ${\mathrm{S}}_8$ring.