Among `N_(2)O,SO_(2),I_(3)^(+)` and `I_(3)^(-)`, the linear species are ………..and……….

Explanation

To determine which of the given compounds are linear, we will analyze each compound's hybridization and molecular geometry.

### Step 1: Analyze N₂O (Nitrous oxide)
- **Structure**: N₂O can be represented as N≡N-O.
- **Hybridization**: The central nitrogen (the one bonded to oxygen) is sp hybridized because it forms a triple bond with one nitrogen and a single bond with oxygen.
- **Geometry**: Since it has two bonding pairs and no lone pairs on the central nitrogen, the molecular geometry is linear.

### Step 2: Analyze SO₂ (Sulfur dioxide)
- **Structure**: SO₂ can be represented as O=S=O.
- **Hybridization**: Sulfur in SO₂ is sp² hybridized because it has two double bonds with oxygen and one lone pair.
- **Geometry**: The presence of a lone pair causes the molecular geometry to be bent, not linear.

### Step 3: Analyze I₃⁺ (Iodine triiodide cation)
- **Structure**: I₃⁺ can be represented as I-I-I with one iodine atom at the center.
- **Hybridization**: The central iodine has two bonding pairs and two lone pairs, giving it a steric number of 4, which corresponds to sp³ hybridization.
- **Geometry**: The molecular shape is bent due to the presence of lone pairs, not linear.

### Step 4: Analyze I₃⁻ (Iodine triiodide anion)
- **Structure**: I₃⁻ can also be represented as I-I-I with one iodine atom at the center.
- **Hybridization**: The central iodine has two bonding pairs and three lone pairs, giving it a steric number of 5, which corresponds to sp³d hybridization.
- **Geometry**: The three lone pairs occupy equatorial positions in a trigonal bipyramidal arrangement, leading to a linear molecular shape.

### Conclusion
From the analysis, the linear species among the given compounds are:
- **N₂O**
- **I₃⁻**

### Final Answer
The linear species are N₂O and I₃⁻.