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Which one of the following oxides is exp...

Which one of the following oxides is expected to exhibit paramagnetic behaviour?

A

`CO_(2)`

B

`SO_(2)`

C

`ClO_(2)`

D

`SiO_(2)`

Text Solution

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The correct Answer is:
To determine which oxide exhibits paramagnetic behavior, we need to analyze the valence electrons of each compound and check for the presence of unpaired electrons. Paramagnetic substances have unpaired electrons, while diamagnetic substances have all paired electrons. ### Step-by-Step Solution: 1. **Identify the Oxides**: The options given are: - A) CO2 (Carbon Dioxide) - B) SO2 (Sulfur Dioxide) - C) ClO2 (Chlorine Dioxide) - D) SiO2 (Silicon Dioxide) 2. **Count the Valence Electrons**: - **For CO2**: - Carbon (C) has 4 valence electrons. - Oxygen (O) has 6 valence electrons, and there are 2 oxygen atoms. - Total = 4 + (6 × 2) = 4 + 12 = 16 electrons (even). - **For SO2**: - Sulfur (S) has 6 valence electrons. - Oxygen (O) has 6 valence electrons, and there are 2 oxygen atoms. - Total = 6 + (6 × 2) = 6 + 12 = 18 electrons (even). - **For ClO2**: - Chlorine (Cl) has 7 valence electrons. - Oxygen (O) has 6 valence electrons, and there are 2 oxygen atoms. - Total = 7 + (6 × 2) = 7 + 12 = 19 electrons (odd). - **For SiO2**: - Silicon (Si) has 4 valence electrons. - Oxygen (O) has 6 valence electrons, and there are 2 oxygen atoms. - Total = 4 + (6 × 2) = 4 + 12 = 16 electrons (even). 3. **Determine Magnetic Behavior**: - **CO2**: 16 electrons (even) → Diamagnetic. - **SO2**: 18 electrons (even) → Diamagnetic. - **ClO2**: 19 electrons (odd) → Contains unpaired electrons → Paramagnetic. - **SiO2**: 16 electrons (even) → Diamagnetic. 4. **Conclusion**: The oxide that exhibits paramagnetic behavior is **C) ClO2**.
To determine which oxide exhibits paramagnetic behavior, we need to analyze the valence electrons of each compound and check for the presence of unpaired electrons. Paramagnetic substances have unpaired electrons, while diamagnetic substances have all paired electrons. ### Step-by-Step Solution: 1. **Identify the Oxides**: The options given are: - A) CO2 (Carbon Dioxide) - B) SO2 (Sulfur Dioxide) - C) ClO2 (Chlorine Dioxide) ...
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Knowledge Check

  • Which one of the following oxides is neutral ?

    A
    SrO
    B
    `AI_(2)O_(3)`
    C
    `CO_(2)`
    D
    CO

  • Which of the following complex species is not expected to exhibit optical isomerism ?

    A
    `[Co(en) (NH_(3))_(2) Cl_(2)]^(+)`
    B
    `[Co(en)_(3)]^(3+)`
    C
    `[Co(en)_(2) Cl_(2)]^(+)`
    D
    `[Co(NH_(3))_(3)Cl_(3)]`

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