Amongst `NO_(3)^(-), AsO_(3)^(3-), CO_(3)^(2-),ClO_(3)^(-),SO_(3)^(2-) and BO_(3)^(3-)`, the non-planar species are :

Options

A. `CO_(3)^(2-),SO_(3)^(2-),BO_(3)^(3-)`
B. `AsO_(3)^(3-), ClO_(3)^(-),SO_(3)^(2-)`
C. `NO_(3)^(-),CO_(3)^(2-),BO_(3)^(3-)`
D. `SO_(3)^(2-),NO_(3)^(-),BO_(3)^(3-)`

Answer

To determine the non-planar species among the given ions, we will calculate the hybridization and steric number for each species using the formula:

\[ \text{Steric Number} = \frac{1}{2} \left( V + M + C \right) \]

Where:
- \( V \) = number of valence electrons of the central atom
- \( M \) = number of monovalent atoms attached to the central atom
- \( C \) = charge (add for anions, subtract for cations)

Let's analyze each species step by step:

### Step 1: Analyze NO₃⁻ (Nitrate Ion)
- **Valence Electrons (N)**: 5
- **Charge**: -1
- **Steric Number Calculation**:
\[ \text{Steric Number} = \frac{1}{2} (5 + 3 + 1) = \frac{9}{2} = 4.5 \text{ (not applicable, use bond pairs)} \]
- 3 bond pairs, 0 lone pairs → **Hybridization**: sp² → **Shape**: Trigonal planar (Planar)

### Step 2: Analyze AsO₃³⁻ (Arsenate Ion)
- **Valence Electrons (As)**: 5
- **Charge**: -3
- **Steric Number Calculation**:
\[ \text{Steric Number} = \frac{1}{2} (5 + 3 + 3) = \frac{11}{2} = 5.5 \text{ (not applicable, use bond pairs)} \]
- 3 bond pairs, 1 lone pair → **Hybridization**: sp³ → **Shape**: Pyramidal (Non-planar)

### Step 3: Analyze CO₃²⁻ (Carbonate Ion)
- **Valence Electrons (C)**: 4
- **Charge**: -2
- **Steric Number Calculation**:
\[ \text{Steric Number} = \frac{1}{2} (4 + 3 + 2) = \frac{9}{2} = 4.5 \text{ (not applicable, use bond pairs)} \]
- 3 bond pairs, 0 lone pairs → **Hybridization**: sp² → **Shape**: Trigonal planar (Planar)

### Step 4: Analyze ClO₃⁻ (Chlorate Ion)
- **Valence Electrons (Cl)**: 7
- **Charge**: -1
- **Steric Number Calculation**:
\[ \text{Steric Number} = \frac{1}{2} (7 + 3 + 1) = \frac{11}{2} = 5.5 \text{ (not applicable, use bond pairs)} \]
- 3 bond pairs, 1 lone pair → **Hybridization**: sp³ → **Shape**: Pyramidal (Non-planar)

### Step 5: Analyze SO₃²⁻ (Sulfite Ion)
- **Valence Electrons (S)**: 6
- **Charge**: -2
- **Steric Number Calculation**:
\[ \text{Steric Number} = \frac{1}{2} (6 + 3 + 2) = \frac{11}{2} = 5.5 \text{ (not applicable, use bond pairs)} \]
- 3 bond pairs, 1 lone pair → **Hybridization**: sp³ → **Shape**: Pyramidal (Non-planar)

### Step 6: Analyze BO₃³⁻ (Boron Trioxide)
- **Valence Electrons (B)**: 3
- **Charge**: -3
- **Steric Number Calculation**:
\[ \text{Steric Number} = \frac{1}{2} (3 + 3 + 3) = \frac{9}{2} = 4.5 \text{ (not applicable, use bond pairs)} \]
- 3 bond pairs, 0 lone pairs → **Hybridization**: sp² → **Shape**: Trigonal planar (Planar)

### Conclusion
The non-planar species among the given ions are:
- AsO₃³⁻ (Pyramidal)
- ClO₃⁻ (Pyramidal)
- SO₃²⁻ (Pyramidal)

Thus, the non-planar species are **AsO₃³⁻, ClO₃⁻, and SO₃²⁻**.