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The paramagnetic species is...

The paramagnetic species is

A

`KO_2`

B

`SiO_2`

C

`TiO_2`

D

`BaO_2`

Text Solution

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The correct Answer is:
To determine which of the given species is paramagnetic, we need to analyze each option based on the presence of unpaired electrons. A substance is considered paramagnetic if it has one or more unpaired electrons in its electron configuration. ### Step-by-Step Solution: 1. **Analyze KO2 (Potassium Superoxide)**: - KO2 contains the superoxide ion (O2^-). - The superoxide ion has one unpaired electron. - Since KO2 has an unpaired electron, it is **paramagnetic**. 2. **Analyze SiO2 (Silicon Dioxide)**: - SiO2 is a covalent compound where silicon forms double bonds with oxygen. - In SiO2, all electrons are paired. - Therefore, SiO2 is **diamagnetic**. 3. **Analyze TiO2 (Titanium Dioxide)**: - TiO2 contains titanium, which is a transition metal. - Titanium in TiO2 has a d-electron configuration that results in all electrons being paired. - Hence, TiO2 is also **diamagnetic**. 4. **Analyze BaO2 (Barium Peroxide)**: - BaO2 contains the peroxide ion (O2^2-). - The peroxide ion has all electrons paired. - Therefore, BaO2 is **diamagnetic**. ### Conclusion: Among the options analyzed, only KO2 is paramagnetic due to the presence of an unpaired electron in the superoxide ion. **Final Answer**: The paramagnetic species is **KO2**.
To determine which of the given species is paramagnetic, we need to analyze each option based on the presence of unpaired electrons. A substance is considered paramagnetic if it has one or more unpaired electrons in its electron configuration. ### Step-by-Step Solution: 1. **Analyze KO2 (Potassium Superoxide)**: - KO2 contains the superoxide ion (O2^-). - The superoxide ion has one unpaired electron. - Since KO2 has an unpaired electron, it is **paramagnetic**. ...
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