Question

Draw the electron dot structure of $S_8$ molecule.

Answer 1

Hint: To answer this question, you must recall the Lewis dot structures for various elements and how to draw them. Lewis structures of chemical species (elements or compounds) are the graphic representations of the distribution of electrons around the constituent atoms. The electron pairs are represented using dots. The shared electron pairs depict the number of bonds formed between the atoms.

Complete step by step solution:
Sulphur has atomic number 16 and has six valence electrons. So, we can write its electronic configuration as: $S:\left[Ne\right]3s^{2}3p^4$
It needs two more electrons to attain a stable noble gas like configuration. So in the $S_8$ molecule, each Sulphur atom will form covalent bonds with two other Sulphur atoms giving the molecule a crown shape. The electron dot structure of $S_8$ molecule can be drawn as follows:

Note:
Lewis structures are commonly used for predicting the number and the types of bonds that are formed by an atom. One must follow some steps when drawing the Lewis structure for species which are:
First, we need to calculate the total number of valence electrons present in the molecules by adding the separate individual valencies of the constituent atoms.
In case of any anions present, extra electrons are added as dots in the structure and in case of cations, electrons are subtracted.
The least electronegative atom in the molecule must be placed as the central atom with all other atoms placed around it with a single bond.
Lone pairs must be assigned first to the most electronegative atoms.
Now draw multiple bonds if needed in order to complete the octet of each atom in the molecule.