Molecule which follows octet rule

Options

A. `CIO_(2)`
B. NO
C. `NO_(2)`
D. `N_(2)O_(3)`

Answer

To determine which molecule follows the octet rule, we need to analyze the electron configuration of each molecule and see if each atom in the molecule has 8 electrons in its valence shell. The octet rule states that atoms tend to bond in such a way that they each have 8 electrons in their outermost shell, achieving a stable electron configuration.

### Step-by-Step Solution:

1. **Understanding the Octet Rule**:
The octet rule states that atoms are most stable when they have 8 electrons in their outermost shell. This is typically achieved through bonding with other atoms.

2. **Analyze ClO2- (Chlorite Ion)**:
- Chlorine (Cl) has 7 valence electrons.
- Each oxygen (O) has 6 valence electrons.
- In ClO2-, chlorine shares electrons with two oxygen atoms.
- Drawing the Lewis structure, we find that chlorine has 10 electrons around it (due to bonding and lone pairs), which does not satisfy the octet rule.

3. **Analyze NO (Nitric Oxide)**:
- Nitrogen (N) has 5 valence electrons.
- Oxygen (O) has 6 valence electrons.
- The Lewis structure shows that nitrogen has 7 electrons around it after bonding with oxygen, which does not satisfy the octet rule.

4. **Analyze NO2 (Nitrogen Dioxide)**:
- Nitrogen (N) has 5 valence electrons.
- Each oxygen (O) has 6 valence electrons.
- The structure shows nitrogen has 9 electrons around it, which again does not satisfy the octet rule.

5. **Analyze N2O3 (Dinitrogen Trioxide)**:
- Each nitrogen (N) has 5 valence electrons.
- Each oxygen (O) has 6 valence electrons.
- The Lewis structure shows that each nitrogen and each oxygen has 8 electrons around them after bonding.
- Therefore, all atoms in N2O3 satisfy the octet rule.

6. **Conclusion**:
Among the given molecules, only **N2O3** follows the octet rule as all the atoms have 8 electrons in their valence shell.

### Final Answer:
The molecule that follows the octet rule is **N2O3**.