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Directions: The following question is based on the paragraph given below.
The noble gases have closed-shell electronic configuration and are monatomic gases under normal conditions. The low boiling points of the lighter noble gases are due to weak dispersion forces between the atoms and the absence of other interatomic interactions.
The direct reaction of xenon with fluorine leads to a series of compounds with oxidation numbers +2, +4 and +6. XeF4 reacts violently with water to give XeO3. The compound can also be prepared using XeF6 as the starting compound. The compounds of xenon exhibit rich stereochemistry and their geometries can be deduced considering the total number of electron pairs in the valence shell.
The chemical nature of the compounds XeF4 and XeF6 is expected to be
- a)oxidising
- b)reducing
- c)unreactive
- d)strong basic
Correct answer is option 'A'. Can you explain this answer?
Most Upvoted Answer
Directions: The following question is based on the paragraph given be...
The chemical nature of the compounds XeF4 and XeF6 is expected to be oxidising.
Explanation:
I. Introduction
- The noble gases are a group of elements that have closed-shell electronic configurations, meaning they have a stable electron arrangement.
- Under normal conditions, noble gases exist as monatomic gases, which means they exist as single atoms rather than molecules.
II. Low Boiling Points of Noble Gases
- The lighter noble gases, such as helium, neon, and argon, have very low boiling points.
- This is because the weak dispersion forces between the atoms are the only interatomic interactions present.
- Dispersion forces are the attractive forces between temporary dipoles that occur due to the movement of electrons in atoms.
- These weak forces result in low boiling points for the noble gases.
III. Xenon Compounds
- Xenon, being a noble gas, also forms compounds under certain conditions.
- The direct reaction of xenon with fluorine leads to a series of compounds with oxidation numbers of 2, 4, and 6.
- XeF4, for example, has xenon in the +4 oxidation state.
IV. Reactivity with Water
- XeF4 reacts violently with water to give XeO3.
- This reaction suggests that XeF4 is an oxidizing agent.
- Oxidizing agents are substances that accept electrons from other substances, causing them to undergo oxidation.
V. Preparation of XeO3
- XeO3 can also be prepared using XeF6 as the starting compound.
- This further supports the idea that XeF4 is an oxidizing agent.
- XeF6 has xenon in the +6 oxidation state.
VI. Rich Stereochemistry
- The compounds of xenon exhibit rich stereochemistry, meaning they have a variety of different geometric arrangements.
- The geometries of these compounds can be deduced by considering the total number of electron pairs in the valence shell of xenon.
- This is due to the ability of xenon to form multiple bonds and accommodate different arrangements of electron pairs.
VII. Conclusion
- Based on the information provided, the chemical nature of the compounds XeF4 and XeF6 is expected to be oxidizing.
- This is supported by their ability to react with water and their involvement in oxidation-reduction reactions.
Explanation:
I. Introduction
- The noble gases are a group of elements that have closed-shell electronic configurations, meaning they have a stable electron arrangement.
- Under normal conditions, noble gases exist as monatomic gases, which means they exist as single atoms rather than molecules.
II. Low Boiling Points of Noble Gases
- The lighter noble gases, such as helium, neon, and argon, have very low boiling points.
- This is because the weak dispersion forces between the atoms are the only interatomic interactions present.
- Dispersion forces are the attractive forces between temporary dipoles that occur due to the movement of electrons in atoms.
- These weak forces result in low boiling points for the noble gases.
III. Xenon Compounds
- Xenon, being a noble gas, also forms compounds under certain conditions.
- The direct reaction of xenon with fluorine leads to a series of compounds with oxidation numbers of 2, 4, and 6.
- XeF4, for example, has xenon in the +4 oxidation state.
IV. Reactivity with Water
- XeF4 reacts violently with water to give XeO3.
- This reaction suggests that XeF4 is an oxidizing agent.
- Oxidizing agents are substances that accept electrons from other substances, causing them to undergo oxidation.
V. Preparation of XeO3
- XeO3 can also be prepared using XeF6 as the starting compound.
- This further supports the idea that XeF4 is an oxidizing agent.
- XeF6 has xenon in the +6 oxidation state.
VI. Rich Stereochemistry
- The compounds of xenon exhibit rich stereochemistry, meaning they have a variety of different geometric arrangements.
- The geometries of these compounds can be deduced by considering the total number of electron pairs in the valence shell of xenon.
- This is due to the ability of xenon to form multiple bonds and accommodate different arrangements of electron pairs.
VII. Conclusion
- Based on the information provided, the chemical nature of the compounds XeF4 and XeF6 is expected to be oxidizing.
- This is supported by their ability to react with water and their involvement in oxidation-reduction reactions.
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Directions: The following question is based on the paragraph given be...
The oxidation state of Xe in XeF4 is +4 and in XeF6 is +6. These oxidation states of Xe are displayed only with elements with high electronegativity, like oxygen and fluorine. Since, Xe will have a tendency to get reduced, the nature of fluorides of xenon is expected to be oxidising.
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Directions: The following question is based on the paragraph given below.The noble gases have closed-shell electronic configuration and are monatomic gases under normal conditions. The low boiling points of the lighter noble gases are due to weak dispersion forces between the atoms and the absence of other interatomic interactions.The direct reaction of xenon with fluorine leads to a series of compounds with oxidation numbers +2, +4 and +6. XeF4 reacts violently with water to give XeO3. The compound can also be prepared using XeF6 as the starting compound. The compounds of xenon exhibit rich stereochemistry and their geometries can be deduced considering the total number of electron pairs in the valence shell.The chemical nature of the compounds XeF4 and XeF6 is expected to bea)oxidisingb)reducingc)unreactived)strong basicCorrect answer is option 'A'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about Directions: The following question is based on the paragraph given below.The noble gases have closed-shell electronic configuration and are monatomic gases under normal conditions. The low boiling points of the lighter noble gases are due to weak dispersion forces between the atoms and the absence of other interatomic interactions.The direct reaction of xenon with fluorine leads to a series of compounds with oxidation numbers +2, +4 and +6. XeF4 reacts violently with water to give XeO3. The compound can also be prepared using XeF6 as the starting compound. The compounds of xenon exhibit rich stereochemistry and their geometries can be deduced considering the total number of electron pairs in the valence shell.The chemical nature of the compounds XeF4 and XeF6 is expected to bea)oxidisingb)reducingc)unreactived)strong basicCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Directions: The following question is based on the paragraph given below.The noble gases have closed-shell electronic configuration and are monatomic gases under normal conditions. The low boiling points of the lighter noble gases are due to weak dispersion forces between the atoms and the absence of other interatomic interactions.The direct reaction of xenon with fluorine leads to a series of compounds with oxidation numbers +2, +4 and +6. XeF4 reacts violently with water to give XeO3. The compound can also be prepared using XeF6 as the starting compound. The compounds of xenon exhibit rich stereochemistry and their geometries can be deduced considering the total number of electron pairs in the valence shell.The chemical nature of the compounds XeF4 and XeF6 is expected to bea)oxidisingb)reducingc)unreactived)strong basicCorrect answer is option 'A'. Can you explain this answer?.
Directions: The following question is based on the paragraph given below.The noble gases have closed-shell electronic configuration and are monatomic gases under normal conditions. The low boiling points of the lighter noble gases are due to weak dispersion forces between the atoms and the absence of other interatomic interactions.The direct reaction of xenon with fluorine leads to a series of compounds with oxidation numbers +2, +4 and +6. XeF4 reacts violently with water to give XeO3. The compound can also be prepared using XeF6 as the starting compound. The compounds of xenon exhibit rich stereochemistry and their geometries can be deduced considering the total number of electron pairs in the valence shell.The chemical nature of the compounds XeF4 and XeF6 is expected to bea)oxidisingb)reducingc)unreactived)strong basicCorrect answer is option 'A'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about Directions: The following question is based on the paragraph given below.The noble gases have closed-shell electronic configuration and are monatomic gases under normal conditions. The low boiling points of the lighter noble gases are due to weak dispersion forces between the atoms and the absence of other interatomic interactions.The direct reaction of xenon with fluorine leads to a series of compounds with oxidation numbers +2, +4 and +6. XeF4 reacts violently with water to give XeO3. The compound can also be prepared using XeF6 as the starting compound. The compounds of xenon exhibit rich stereochemistry and their geometries can be deduced considering the total number of electron pairs in the valence shell.The chemical nature of the compounds XeF4 and XeF6 is expected to bea)oxidisingb)reducingc)unreactived)strong basicCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Directions: The following question is based on the paragraph given below.The noble gases have closed-shell electronic configuration and are monatomic gases under normal conditions. The low boiling points of the lighter noble gases are due to weak dispersion forces between the atoms and the absence of other interatomic interactions.The direct reaction of xenon with fluorine leads to a series of compounds with oxidation numbers +2, +4 and +6. XeF4 reacts violently with water to give XeO3. The compound can also be prepared using XeF6 as the starting compound. The compounds of xenon exhibit rich stereochemistry and their geometries can be deduced considering the total number of electron pairs in the valence shell.The chemical nature of the compounds XeF4 and XeF6 is expected to bea)oxidisingb)reducingc)unreactived)strong basicCorrect answer is option 'A'. Can you explain this answer?.
Solutions for Directions: The following question is based on the paragraph given below.The noble gases have closed-shell electronic configuration and are monatomic gases under normal conditions. The low boiling points of the lighter noble gases are due to weak dispersion forces between the atoms and the absence of other interatomic interactions.The direct reaction of xenon with fluorine leads to a series of compounds with oxidation numbers +2, +4 and +6. XeF4 reacts violently with water to give XeO3. The compound can also be prepared using XeF6 as the starting compound. The compounds of xenon exhibit rich stereochemistry and their geometries can be deduced considering the total number of electron pairs in the valence shell.The chemical nature of the compounds XeF4 and XeF6 is expected to bea)oxidisingb)reducingc)unreactived)strong basicCorrect answer is option 'A'. Can you explain this answer? in English & in Hindi are available as part of our courses for JEE.
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Here you can find the meaning of Directions: The following question is based on the paragraph given below.The noble gases have closed-shell electronic configuration and are monatomic gases under normal conditions. The low boiling points of the lighter noble gases are due to weak dispersion forces between the atoms and the absence of other interatomic interactions.The direct reaction of xenon with fluorine leads to a series of compounds with oxidation numbers +2, +4 and +6. XeF4 reacts violently with water to give XeO3. The compound can also be prepared using XeF6 as the starting compound. The compounds of xenon exhibit rich stereochemistry and their geometries can be deduced considering the total number of electron pairs in the valence shell.The chemical nature of the compounds XeF4 and XeF6 is expected to bea)oxidisingb)reducingc)unreactived)strong basicCorrect answer is option 'A'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of
Directions: The following question is based on the paragraph given below.The noble gases have closed-shell electronic configuration and are monatomic gases under normal conditions. The low boiling points of the lighter noble gases are due to weak dispersion forces between the atoms and the absence of other interatomic interactions.The direct reaction of xenon with fluorine leads to a series of compounds with oxidation numbers +2, +4 and +6. XeF4 reacts violently with water to give XeO3. The compound can also be prepared using XeF6 as the starting compound. The compounds of xenon exhibit rich stereochemistry and their geometries can be deduced considering the total number of electron pairs in the valence shell.The chemical nature of the compounds XeF4 and XeF6 is expected to bea)oxidisingb)reducingc)unreactived)strong basicCorrect answer is option 'A'. Can you explain this answer?, a detailed solution for Directions: The following question is based on the paragraph given below.The noble gases have closed-shell electronic configuration and are monatomic gases under normal conditions. The low boiling points of the lighter noble gases are due to weak dispersion forces between the atoms and the absence of other interatomic interactions.The direct reaction of xenon with fluorine leads to a series of compounds with oxidation numbers +2, +4 and +6. XeF4 reacts violently with water to give XeO3. The compound can also be prepared using XeF6 as the starting compound. The compounds of xenon exhibit rich stereochemistry and their geometries can be deduced considering the total number of electron pairs in the valence shell.The chemical nature of the compounds XeF4 and XeF6 is expected to bea)oxidisingb)reducingc)unreactived)strong basicCorrect answer is option 'A'. Can you explain this answer? has been provided alongside types of Directions: The following question is based on the paragraph given below.The noble gases have closed-shell electronic configuration and are monatomic gases under normal conditions. The low boiling points of the lighter noble gases are due to weak dispersion forces between the atoms and the absence of other interatomic interactions.The direct reaction of xenon with fluorine leads to a series of compounds with oxidation numbers +2, +4 and +6. XeF4 reacts violently with water to give XeO3. The compound can also be prepared using XeF6 as the starting compound. The compounds of xenon exhibit rich stereochemistry and their geometries can be deduced considering the total number of electron pairs in the valence shell.The chemical nature of the compounds XeF4 and XeF6 is expected to bea)oxidisingb)reducingc)unreactived)strong basicCorrect answer is option 'A'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice Directions: The following question is based on the paragraph given below.The noble gases have closed-shell electronic configuration and are monatomic gases under normal conditions. The low boiling points of the lighter noble gases are due to weak dispersion forces between the atoms and the absence of other interatomic interactions.The direct reaction of xenon with fluorine leads to a series of compounds with oxidation numbers +2, +4 and +6. XeF4 reacts violently with water to give XeO3. The compound can also be prepared using XeF6 as the starting compound. The compounds of xenon exhibit rich stereochemistry and their geometries can be deduced considering the total number of electron pairs in the valence shell.The chemical nature of the compounds XeF4 and XeF6 is expected to bea)oxidisingb)reducingc)unreactived)strong basicCorrect answer is option 'A'. Can you explain this answer? tests, examples and also practice JEE tests.
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