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

Transcript text: Listen Choose the best Lewis structure for $\mathrm{OCl}_{2}$. $\ddot{C l}-\ddot{O}=C l:$ $\therefore \mathrm{Cl}=\mathrm{O}=\mathrm{Cl}:$ $: \ddot{C} l-\ddot{O}-\ddot{C}:$ $: C \mathrm{Cl}=\ddot{O}-\ddot{C} \mid:$

Solution

Solution Steps

Step 1: Determine the Total Number of Valence Electrons

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:

\[ 6 + 2 \times 7 = 20 \]

Step 2: Draw the Skeleton Structure

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

Step 3: Distribute Electrons to Satisfy the Octet Rule

Place a pair of electrons (a single bond) between each pair of bonded atoms: $\mathrm{Cl} - \mathrm{O} - \mathrm{Cl}$.
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.

Step 4: Verify the Structure

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).