`CO_(3)^(2-)` anion has which of the following characterstics

Options

A. Bonds of unequal length
B. `sp^(3)` hybridization of C atom
C. Resonance stabilization
D. Different bond angles

Answer

To analyze the characteristics of the carbonate anion \( \text{CO}_3^{2-} \), we can follow these steps:

### Step 1: Understand the Structure of Carbonate Ion
The carbonate ion consists of one carbon atom bonded to three oxygen atoms. The overall charge of the ion is -2.

### Step 2: Draw the Lewis Structure
To draw the Lewis structure of \( \text{CO}_3^{2-} \):
- Carbon (C) is the central atom.
- Oxygen (O) atoms are surrounding the carbon atom.
- There are two negative charges distributed among the oxygen atoms.

The Lewis structure can be represented as:
- One double bond between carbon and one oxygen atom, and two single bonds between carbon and the other two oxygen atoms, each carrying a negative charge.

### Step 3: Identify Resonance Structures
The carbonate ion exhibits resonance. This means that the double bond can shift between the three oxygen atoms. The resonance structures can be depicted as:
1. \( \text{O}=\text{C}(\text{O}^-) \text{O}^- \)
2. \( \text{O}^-\text{C}(\text{O}=\text{O}^-) \)
3. \( \text{O}^-\text{O}^-\text{C}=\text{O} \)

### Step 4: Analyze Bond Lengths
Due to resonance, all C-O bonds in the carbonate ion are of equal length. This is a key characteristic of resonance structures, where the actual bond order is an average of the contributing structures.

### Step 5: Determine Hybridization of Carbon
To find the hybridization of the carbon atom in \( \text{CO}_3^{2-} \):
- Carbon has 4 valence electrons.
- There are three oxygen atoms bonded to carbon (considering the charge).
- Using the formula for hybridization:
\[ \text{Hybridization} = \frac{1}{2} \left( V + M + C \right) \]
where \( V \) is the number of valence electrons, \( M \) is the number of monovalent atoms (0 in this case), and \( C \) is the charge (+2 for anions).
- Thus, \( \text{Hybridization} = \frac{1}{2} (4 + 0 + 2) = 3 \), which indicates \( \text{sp}^2 \) hybridization.

### Step 6: Analyze Bond Angles
The geometry of the carbonate ion is trigonal planar due to \( \text{sp}^2 \) hybridization, leading to bond angles of approximately 120 degrees.

### Conclusion
From the analysis:
- The carbonate ion does not have bonds of unequal length (all are equal).
- The carbon atom is \( \text{sp}^2 \) hybridized, not \( \text{sp}^3 \).
- It exhibits resonance stabilization.
- The bond angles are equal (120 degrees), not different.

Thus, the only characteristic that the carbonate ion \( \text{CO}_3^{2-} \) possesses is **resonance stabilization**.