In the correct Lewis dot structure of `CO_(2)`, the total number of lone pairs are :

Options

A. `:overset(..)(O)::C::overset(..)(O):`
B. `:underset(..)overset(..)(O):overset(..)(C)::overset(..)(O):`
C. `:overset(..)(O)::C:underset(..)overset(..)(O):`
D. `:underset(..)overset(..)(O):C:underset(..)overset(..)(O):`

Answer

To determine the total number of lone pairs in the Lewis dot structure of carbon dioxide (CO₂), we can follow these steps:

### Step 1: Determine the valence electrons
- Carbon (C) has 4 valence electrons.
- Each oxygen (O) has 6 valence electrons. Since there are two oxygen atoms, we have 2 × 6 = 12 valence electrons from oxygen.

**Total valence electrons = 4 (from C) + 12 (from O) = 16 valence electrons.**

**Hint:** Remember to count the valence electrons for each atom based on its group number in the periodic table.

### Step 2: Draw the skeletal structure
- Place the carbon atom in the center and the two oxygen atoms on either side. This gives us a skeletal structure of O-C-O.

**Hint:** The central atom is usually the least electronegative element, which in this case is carbon.

### Step 3: Form bonds between the atoms
- Connect the carbon atom to each oxygen atom with a single bond initially. This uses 4 of the 16 valence electrons (2 electrons per bond).
- Now we have 16 - 4 = 12 valence electrons remaining.

**Hint:** Each bond consists of 2 electrons.

### Step 4: Distribute remaining electrons to complete octets
- Place the remaining 12 electrons around the oxygen atoms to satisfy the octet rule. Each oxygen needs 8 electrons in total.
- Start by placing 6 electrons (3 lone pairs) around each oxygen atom. This uses up all 12 remaining electrons.

**Hint:** Each oxygen atom can hold a maximum of 8 electrons, including those in bonds.

### Step 5: Check the structure
- After placing the lone pairs, we notice that each oxygen has 6 electrons (3 lone pairs) and is connected to carbon with a single bond (2 electrons). This gives each oxygen a total of 8 electrons.
- However, to minimize formal charges, we can convert one lone pair from each oxygen into a double bond with carbon. This results in a double bond between carbon and each oxygen, leading to the final structure of O=C=O.

**Hint:** Double bonds can help satisfy the octet rule while minimizing formal charges.

### Step 6: Count the lone pairs
- In the final structure (O=C=O), each oxygen atom has 2 lone pairs (4 electrons total).
- Therefore, the total number of lone pairs in CO₂ is 2 (from one oxygen) + 2 (from the other oxygen) = 4 lone pairs.

**Final Answer:** The total number of lone pairs in the Lewis dot structure of CO₂ is **4**.

### Summary of Steps:
1. Count valence electrons.
2. Draw the skeletal structure.
3. Form initial bonds.
4. Distribute remaining electrons.
5. Adjust bonds to minimize formal charges.
6. Count the lone pairs.