Out of `NO,NO^(o+)` and `CN^(o+)` the paramagnetic species is `NO^(o+)` .

Explanation

To determine whether the statement is correct, we need to analyze the magnetic properties of the species NO, NO⁺, and CN⁺. A species is considered paramagnetic if it has unpaired electrons in its molecular orbital configuration.

### Step 1: Determine the electron configuration of NO
- **Nitric Oxide (NO)** has a total of 11 electrons (7 from nitrogen and 8 from oxygen).
- The molecular orbital configuration for NO is:
- σ(1s)² σ*(1s)² σ(2s)² σ*(2s)² σ(2p_z)² π(2p_x)¹ π(2p_y)¹
- In this configuration, we can see that there are 2 unpaired electrons in the π(2p_x) and π(2p_y) orbitals.

### Step 2: Determine the electron configuration of NO⁺
- **NO⁺** has one less electron than NO, giving it a total of 10 electrons.
- The molecular orbital configuration for NO⁺ is:
- σ(1s)² σ*(1s)² σ(2s)² σ*(2s)² σ(2p_z)² π(2p_x)¹
- In this configuration, there is 1 unpaired electron in the π(2p_x) orbital.

### Step 3: Determine the electron configuration of CN⁺
- **Cyanide (CN⁺)** has a total of 10 electrons (6 from carbon and 4 from nitrogen).
- The molecular orbital configuration for CN⁺ is:
- σ(1s)² σ*(1s)² σ(2s)² σ*(2s)² σ(2p_z)²
- In this configuration, all electrons are paired, meaning there are no unpaired electrons.

### Step 4: Analyze the paramagnetic properties
- **NO** has 2 unpaired electrons, making it paramagnetic.
- **NO⁺** has 1 unpaired electron, making it paramagnetic as well.
- **CN⁺** has no unpaired electrons, making it diamagnetic.

### Conclusion
The statement that "the paramagnetic species is NO⁺" is correct. Therefore, the correct answer is that both NO and NO⁺ are paramagnetic, while CN⁺ is not.