When molten sulfur reacts with chlorine gas, a vile-smelling orange liquid forms that has an empirical formula of SCl. The structure of this compound has a formal charge of zero on all elements in the compound. Draw the Lewis structure for the vile-smelling orange liquid.

The formal charge (FC) is the charge that is more close to the actual charge in the real molecules and ions. It can be calculated based on the number of valence electrons (V), the shared electrons (S) and the electrons in the lone pairs (L) by the equation:

FC = V - (L + S/2)

Sulfur is in group 16 of the periodic table, so it has 6 valence electrons, and chlorine is from group 17 of the periodic table, and so it has 7 valence electrons. Chlorine can share only one electron, so it is stable. Sulfur can expand its octet (because it's from the third period) and can have more than 8 electrons when stable.

The possible formulas, from the empiric one, are:

SCl, S₂Cl₂, and S₃Cl₃.

To have FC = 0, chlorine must done only one bond, because S = 2, and L = 6, so:

FC = 7 - (6 + 2/2) = 0

So, it can not be the central atom of a structure. In the SCl, it will hav only a simple bond, so for sulfur, S = 2, and L = 4 (only the lone pairs are counted)

FC = 6 - (4+ 2/2) = +1

For S₂Cl₂, the two sulfurs must be bonded to a simple bond, and each one to one chlorine, thus, for both od them S = 4, and L = 4. so

FC = 6 - (4 + 4/2) = 0

So, it is the correct structure. The lewis structure represents the bonds by lines and the lone pairs of electrons by dots, and it is shown below.

shrutiagrawal1798 shrutiagrawal1798 · Answer 2 · 2021-12-28T14:24:53+01:00

The vile smelling compound with zero formal charge formed has been [tex]\rm S_2Cl_2[/tex].

The formal charge has been the charge over the elements in the compound, that has been equivalent to the real molecular charge. The formal charge (FC) can be given as:

[tex]FC=V-(L+\dfrac{S}{2} )[/tex]

Where,

L has been the lone pairs

V has been the valence electrons

S has been the shared electrons

The empirical formula for the compound has been SCl. The formal charge on Cl bonded with S in [tex]\rm S_2Cl_2[/tex] has been:

[tex]FC=\rm 7-(6+\dfrac{2}{2} )\\\\FC=0[/tex]

Thus, the vile smelling compound formed has been [tex]\rm S_2Cl_2[/tex].

The Lewis structure of the compound has been given in the image attached.

For more information about Lewis structure, refer to the link:

https://brainly.com/question/4144781