Both `CO_(2) and N_(2)O` are linear but dipole moment of `CO_(2) ` is zero but for `N_(2)O` it is non-zero, Why ?

Explanation

To understand why the dipole moment of CO₂ is zero while that of N₂O is non-zero, despite both being linear molecules, we can follow these steps:

### Step 1: Understand the Molecular Structures
- **CO₂ (Carbon Dioxide)**: The molecular structure consists of one carbon atom double bonded to two oxygen atoms. The arrangement is linear due to the sp hybridization of carbon, which allows for a symmetrical distribution of charge.
- **N₂O (Nitrous Oxide)**: The structure consists of two nitrogen atoms and one oxygen atom. The arrangement is also linear, but the electronegativity differences and the presence of lone pairs lead to an asymmetrical distribution of charge.

### Step 2: Draw the Lewis Structures
- For **CO₂**:
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