Complete the Lewis structures for \( \text{COCl}_2 \) and \( \text{SOCl}_2 \) using the skeletal structure shown below, being sure to follow the procedure for minimizing the sum of the absolute values for the formal charges, where the octet rule need not be followed. Based on the complete structures, which statement below is true?\[\begin{array}{cc}\begin{array}{c}\begin{array}{c}\begin{align*}\left[ \begin{array}{c} \\ \\\end{array} \right] \\\text{Cl} - \text{N} \equiv \text{Cl} \\\end{align*}\end{array}\end{array} \begin{array}{c} \left[ \begin{array}{c} \text{ }\\ \text{O} \\ \text{ } \end{array} \right]^+ \\ \\\end{array}&\begin{array}{c}\begin{array}{c}\left[ \begin{array}{c} \\ \\\end{array} \right] \\\text{Cl} - \text{Br} - \text{Cl} \\\end{array} \left[ \begin{array}{c} \text{ }\\ \text{O} \\ \text{ } \end{array}\right]^+ \end{array}\end{array}\]**Hint:** Consider the potential for multiple bonds on the molecules and be sure to account for all valence electrons.**Options:**1. The \( \text{NOCl}_2^+ \) exhibits formal charges but no resonance hybrids, while the \( \text{BrOCl}_2^+ \) exhibits both formal charges and resonance hybrids.2. The \( \text{NOCl}_2^+ \) exhibits both formal charges and resonance hybrids, while the \( \text{BrOCl}_2^+ \) exhibits resonance hybrids but no formal charges.3. The \( \text{BrOCl}_2^+ \) exhibits formal charges but no resonance hybrids, while the \( \text{NOCl}_2

Lewis’s structure: Lewis’s bonding theory is based on the octet rule. The Lewis structure is a simplified representation of the valance shell electrons (bond pair and lone pair) of a molecule.In the Lewis structure, the valance electrons are represented by the dot. The lone pair of electrons is represented by a pair of dots and the bonding electron pair can be represented by the pair of dots between the atoms or by a bond line. The Lewis structure of the given two ions is as follows:Formal charge: The formal charge (FC) is the charge assigned to an atom in a molecule, assuming that electrons in all chemical bonds are shared equally between the atoms of the molecule. When we calculate the formal charge, we ignore the partial charges generated by the difference in electronegativity of the atoms. The formal charge in the above ions is as follows: The nitrogen atom of NOCl2+ has a +1 formal charge and the bromine atom of BrOCl2+ has also a +1 formal charge.Resonance structure: If the Lewis structure of a molecule or ion cannot explain by a single structure then more than one Lewis structure is written, these Lewis structures are different by the position of the lone pair of electrons and the pi bond. These structures are called resonance structures.The position of the atoms does not change in all the resonance structures. The movement of pi electrons in resonance structures is shown by the curved arrow. NOCl2+ does not show resonance but BrOCl2+ shows the resonance as follows:The correct option is as follows: The NOCl2+ exihibits formal charge but no resonance hybrid, while the BrOCl2+ exihibits both formal charge and resonance hybrid.