Which of the following species is diamagnetic? 02- O 02* Oz O 02

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### Question: Understanding Diamagnetic Species

**Which of the following species is diamagnetic?**

- ( ) O₂²⁻
- ( ) O₂⁺
- ( ) O₂⁻
- ( ) O₂

### Explanation:

Diamagnetism is a form of magnetism that occurs when an electron pair in an orbital is paired and thus, the magnetic moments cancel each other out, resulting in no net magnetic moment. Diamagnetic substances are repelled by a magnetic field. 

To determine which species among O₂²⁻, O₂⁺, O₂⁻, and O₂ is diamagnetic, we need to consider their electronic configurations and the resultant magnetic properties:

1. **O₂²⁻ (Peroxide ion)**: This ion has 18 electrons. In accordance with molecular orbital theory, it will have all paired electrons in its molecular orbitals.
2. **O₂⁺ (Superoxide ion)**: This ion has 15 electrons. There will be an unpaired electron in its molecular orbital configuration, making it paramagnetic.
3. **O₂⁻ (Diatomic oxygen anion)**: This ion has 17 electrons. It also has an unpaired electron, making it paramagnetic.
4. **O₂ (Diatomic oxygen)**: This molecule has 16 electrons. Its molecular orbital configuration also includes unpaired electrons, rendering it paramagnetic.

Thus, the correct answer is **O₂²⁻**, as it is the species with all electrons paired, making it diamagnetic.

### Educational Note:

In chemistry, understanding whether a molecule or ion is diamagnetic or paramagnetic is crucial for predicting its behavior in magnetic fields and has implications for various applications and scientific principles.

Remember to always consider the electron configuration and pairing of electrons in molecular orbitals when determining if a species is diamagnetic or paramagnetic.
Transcribed Image Text:### Question: Understanding Diamagnetic Species **Which of the following species is diamagnetic?** - ( ) O₂²⁻ - ( ) O₂⁺ - ( ) O₂⁻ - ( ) O₂ ### Explanation: Diamagnetism is a form of magnetism that occurs when an electron pair in an orbital is paired and thus, the magnetic moments cancel each other out, resulting in no net magnetic moment. Diamagnetic substances are repelled by a magnetic field. To determine which species among O₂²⁻, O₂⁺, O₂⁻, and O₂ is diamagnetic, we need to consider their electronic configurations and the resultant magnetic properties: 1. **O₂²⁻ (Peroxide ion)**: This ion has 18 electrons. In accordance with molecular orbital theory, it will have all paired electrons in its molecular orbitals. 2. **O₂⁺ (Superoxide ion)**: This ion has 15 electrons. There will be an unpaired electron in its molecular orbital configuration, making it paramagnetic. 3. **O₂⁻ (Diatomic oxygen anion)**: This ion has 17 electrons. It also has an unpaired electron, making it paramagnetic. 4. **O₂ (Diatomic oxygen)**: This molecule has 16 electrons. Its molecular orbital configuration also includes unpaired electrons, rendering it paramagnetic. Thus, the correct answer is **O₂²⁻**, as it is the species with all electrons paired, making it diamagnetic. ### Educational Note: In chemistry, understanding whether a molecule or ion is diamagnetic or paramagnetic is crucial for predicting its behavior in magnetic fields and has implications for various applications and scientific principles. Remember to always consider the electron configuration and pairing of electrons in molecular orbitals when determining if a species is diamagnetic or paramagnetic.
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