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Which one of the following oxides is expected to exhibit paramagnetic behavior and how CO2 and SiO2 is false? =CO2 ,SO2 ,ClO2, SiO2
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Which one of the following oxides is expected to exhibit paramagnetic...
Introduction
In chemistry, paramagnetism is a type of magnetism where the material is weakly attracted to an external magnetic field. In this response, we will determine which oxide exhibits paramagnetic behavior and explain why CO2 and SiO2 do not exhibit such behavior.
Paramagnetism
Paramagnetism occurs when an atom or molecule has one or more unpaired electrons. These unpaired electrons align themselves with an external magnetic field, causing the material to be weakly attracted to the field. The more unpaired electrons a material has, the stronger its paramagnetic behavior will be.
Oxides
Oxides are compounds that contain oxygen and one or more other elements. Some common oxides include CO2, SO2, ClO2, and SiO2.
CO2
CO2 is not expected to exhibit paramagnetic behavior because it has no unpaired electrons. Each carbon atom in CO2 is bonded to two oxygen atoms, forming a double bond. This double bond results in the carbon atom having no unpaired electrons, making CO2 diamagnetic rather than paramagnetic.
SiO2
SiO2 is also not expected to exhibit paramagnetic behavior because it has no unpaired electrons. Silicon in SiO2 forms four covalent bonds with four oxygen atoms, resulting in no unpaired electrons. Therefore, SiO2 is diamagnetic rather than paramagnetic.
SO2
SO2 is expected to exhibit paramagnetic behavior because it has unpaired electrons. The sulfur atom in SO2 has one unpaired electron, making it paramagnetic. The unpaired electron will align with an external magnetic field, causing SO2 to be weakly attracted to the field.
ClO2
ClO2 is also expected to exhibit paramagnetic behavior because it has unpaired electrons. The chlorine atom in ClO2 has one unpaired electron, making it paramagnetic. The unpaired electron will align with an external magnetic field, causing ClO2 to be weakly attracted to the field.
Conclusion
In summary, SO2 and ClO2 are expected to exhibit paramagnetic behavior due to their unpaired electrons, while CO2 and SiO2 are not expected to exhibit such behavior because they have no unpaired electrons.
In chemistry, paramagnetism is a type of magnetism where the material is weakly attracted to an external magnetic field. In this response, we will determine which oxide exhibits paramagnetic behavior and explain why CO2 and SiO2 do not exhibit such behavior.
Paramagnetism
Paramagnetism occurs when an atom or molecule has one or more unpaired electrons. These unpaired electrons align themselves with an external magnetic field, causing the material to be weakly attracted to the field. The more unpaired electrons a material has, the stronger its paramagnetic behavior will be.
Oxides
Oxides are compounds that contain oxygen and one or more other elements. Some common oxides include CO2, SO2, ClO2, and SiO2.
CO2
CO2 is not expected to exhibit paramagnetic behavior because it has no unpaired electrons. Each carbon atom in CO2 is bonded to two oxygen atoms, forming a double bond. This double bond results in the carbon atom having no unpaired electrons, making CO2 diamagnetic rather than paramagnetic.
SiO2
SiO2 is also not expected to exhibit paramagnetic behavior because it has no unpaired electrons. Silicon in SiO2 forms four covalent bonds with four oxygen atoms, resulting in no unpaired electrons. Therefore, SiO2 is diamagnetic rather than paramagnetic.
SO2
SO2 is expected to exhibit paramagnetic behavior because it has unpaired electrons. The sulfur atom in SO2 has one unpaired electron, making it paramagnetic. The unpaired electron will align with an external magnetic field, causing SO2 to be weakly attracted to the field.
ClO2
ClO2 is also expected to exhibit paramagnetic behavior because it has unpaired electrons. The chlorine atom in ClO2 has one unpaired electron, making it paramagnetic. The unpaired electron will align with an external magnetic field, causing ClO2 to be weakly attracted to the field.
Conclusion
In summary, SO2 and ClO2 are expected to exhibit paramagnetic behavior due to their unpaired electrons, while CO2 and SiO2 are not expected to exhibit such behavior because they have no unpaired electrons.
Community Answer
Which one of the following oxides is expected to exhibit paramagnetic...
ClO2 exhibit paramagnetic behaviour because it has odd number of electrons. Cl has 17 and two oxygen atom has 32, so total number of electrons being 49. While others have even number of electrons, CO2 has 38, SO2 has 48 and SiO2 has 46 electrons.
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Which one of the following oxides is expected to exhibit paramagnetic behavior and how CO2 and SiO2 is false? =CO2 ,SO2 ,ClO2, SiO2
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Which one of the following oxides is expected to exhibit paramagnetic behavior and how CO2 and SiO2 is false? =CO2 ,SO2 ,ClO2, SiO2 for NEET 2025 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about Which one of the following oxides is expected to exhibit paramagnetic behavior and how CO2 and SiO2 is false? =CO2 ,SO2 ,ClO2, SiO2 covers all topics & solutions for NEET 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Which one of the following oxides is expected to exhibit paramagnetic behavior and how CO2 and SiO2 is false? =CO2 ,SO2 ,ClO2, SiO2.
Which one of the following oxides is expected to exhibit paramagnetic behavior and how CO2 and SiO2 is false? =CO2 ,SO2 ,ClO2, SiO2 for NEET 2025 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about Which one of the following oxides is expected to exhibit paramagnetic behavior and how CO2 and SiO2 is false? =CO2 ,SO2 ,ClO2, SiO2 covers all topics & solutions for NEET 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Which one of the following oxides is expected to exhibit paramagnetic behavior and how CO2 and SiO2 is false? =CO2 ,SO2 ,ClO2, SiO2.
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