Which of the following do not exhibit resonance.

Options

A. `CO_(3)^(-2)`
B. `ClO_(3)^(-)`
C. `SiO_(2)`
D. `SO_(3)^(-2)`

Explanation

To determine which of the given compounds do not exhibit resonance, we will analyze each option step by step.

### Step 1: Analyze Carbonate (CO₃²⁻)
1. **Structure**: The carbonate ion has one carbon atom bonded to three oxygen atoms. It has one double bond and two single bonds, with the two single-bonded oxygen atoms each carrying a negative charge.
2. **Resonance**: The double bond can shift between the three oxygen atoms, allowing for multiple resonance structures. Therefore, carbonate does exhibit resonance.

**Hint**: Look for the presence of double bonds and charges that can shift between atoms to identify resonance.

### Step 2: Analyze Chlorate (ClO₃⁻)
1. **Structure**: The chlorate ion consists of one chlorine atom bonded to three oxygen atoms, with one double bond and two single bonds. One of the single-bonded oxygen atoms carries a negative charge.
2. **Resonance**: Similar to carbonate, the double bond can shift among the oxygen atoms, resulting in multiple resonance structures. Thus, chlorate also exhibits resonance.

**Hint**: Check if the structure allows for the movement of electrons between atoms, indicating resonance.

### Step 3: Analyze Silicon Dioxide (SiO₂)
1. **Structure**: Silicon dioxide is not a discrete molecule like CO₂; instead, it exists as a network solid with a repeating structure. Each silicon atom is bonded to four oxygen atoms in a tetrahedral arrangement.
2. **Resonance**: Since SiO₂ does not have a stable double bond structure and cannot form pi bonds due to the large size of silicon, it does not exhibit resonance.

**Hint**: Consider the molecular structure and bonding capabilities of the central atom to determine if resonance is possible.

### Step 4: Analyze Sulfide (SO₃²⁻)
1. **Structure**: The sulfide ion has one sulfur atom bonded to three oxygen atoms, with one double bond and two single bonds. Each of the single-bonded oxygen atoms carries a negative charge.
2. **Resonance**: The double bond can shift among the oxygen atoms, creating multiple resonance structures. Therefore, sulfide does exhibit resonance.

**Hint**: Look for the possibility of forming multiple valid Lewis structures to identify resonance.

### Conclusion
After analyzing all the given options, we conclude that the only compound that does not exhibit resonance is Silicon Dioxide (SiO₂).

**Final Answer**: SiO₂ (Silicon Dioxide) does not exhibit resonance.