Questions: Choose the best Lewis structure for OCl2. Cl-O=Cl: Therefore Cl=O=Cl: : Cl-O-Cl: : CCl=O-Cl :

Solution Steps

To find the best Lewis structure for $\mathrm{OCl}_2$, we first need to determine the total number of valence electrons. Oxygen ($\mathrm{O}$) has 6 valence electrons, and each chlorine ($\mathrm{Cl}$) has 7 valence electrons. Therefore, the total number of valence electrons is:

$$6 + 2 \times 7 = 20$$

The central atom is usually the least electronegative, which is oxygen in this case. Therefore, the skeleton structure is $\mathrm{Cl} - \mathrm{O} - \mathrm{Cl}$.

1. Place a pair of electrons (a single bond) between each pair of bonded atoms: $\mathrm{Cl} - \mathrm{O} - \mathrm{Cl}$.
2. Distribute the remaining electrons to satisfy the octet rule for each atom, starting with the outer atoms (chlorines) and then the central atom (oxygen).

• Each $\mathrm{Cl}$ needs 6 more electrons to complete its octet: $2 \times 6 = 12$ electrons.
• The remaining 6 electrons are placed on the oxygen atom to complete its octet.

Ensure that each atom has a complete octet and that the total number of electrons used is 20. The structure should look like this:

$$: \ddot{C}l - \ddot{O} - \ddot{C}l:$$

Each chlorine has 8 electrons (2 from the bond and 6 as lone pairs), and oxygen has 8 electrons (4 from the bonds and 4 as lone pairs).

Final Answer