Which statement is not correct about `NO_(2)` ?

Options

A. It is paramagnetic
B. It forms dimer and paramanetism is lost
C. It has one coordinate bond
D. It has nitrogen oxygen triple bond

Explanation

To determine which statement is not correct about \( NO_2 \), we will analyze the properties and structure of the molecule step by step.

### Step 1: Understand the Valence Electrons
- Nitrogen (N) has 5 valence electrons.
- Each Oxygen (O) has 6 valence electrons.
- In \( NO_2 \), there are one nitrogen and two oxygen atoms, giving a total of \( 5 + 2 \times 6 = 17 \) valence electrons.

**Hint:** Count the total number of valence electrons from all atoms involved in the molecule.

### Step 2: Draw the Lewis Structure
- Nitrogen forms a double bond with one oxygen atom and a single bond with the other oxygen atom.
- The single bond oxygen has a lone pair, which can be donated to nitrogen, forming a coordinate bond.
- This results in nitrogen having a formal charge of +1 and one of the oxygen atoms having a formal charge of -1.

**Hint:** Use the octet rule to guide how bonds are formed and how lone pairs are distributed.

### Step 3: Determine the Magnetic Properties
- To check if \( NO_2 \) is paramagnetic, we need to look for unpaired electrons.
- In the Lewis structure, nitrogen has one unpaired electron after forming the bonds, which makes \( NO_2 \) paramagnetic.

**Hint:** Remember that paramagnetic species have unpaired electrons, while diamagnetic species do not.

### Step 4: Analyze the Bonding
- The bonds in \( NO_2 \) consist of one double bond and one coordinate bond.
- The statement claiming that there is a nitrogen-oxygen triple bond is incorrect, as \( NO_2 \) only has one double bond and one coordinate bond.

**Hint:** Verify each bond type and count to ensure accuracy in the bonding description.

### Step 5: Identify the Incorrect Statement
- Based on the analysis:
- \( NO_2 \) is paramagnetic (correct).
- \( NO_2 \) has one coordinate bond (correct).
- The incorrect statement is that \( NO_2 \) has a nitrogen-oxygen triple bond.

**Hint:** Compare the statements given in the question with your findings to identify which one does not align with the established facts.

### Conclusion
The statement that is not correct about \( NO_2 \) is that it has a nitrogen-oxygen triple bond. The correct bonding in \( NO_2 \) consists of one double bond and one coordinate bond.