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In which of the following arrangements the sequence is not strictly according to the property written against it:
- a)CO2< SiO2< SnO2< PbO2: increasing oxidising power
- b)HF < HCl < HBr < HI: increasing acid strength
- c)NH3< PH3< AsH3< SbH3: increasing basic strength
- d)B < C < O < N: increasing first ionization enthalpy
Correct answer is option 'C'. Can you explain this answer?
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In which of the following arrangements the sequence is not strictly ac...
Explanation of Incorrect Sequence in Option C
In the provided options, the sequence in option C is identified as incorrect due to the increasing basic strength of hydrides of Group 15 elements (NH3, PH3, AsH3, SbH3).
Basic Strength of Hydrides
- NH3 (Ammonia): Strong base due to high electronegativity of nitrogen.
- PH3 (Phosphine): Weaker base compared to NH3, as phosphorus is less electronegative and does not effectively donate the lone pair.
- AsH3 (Arsine): Even weaker than PH3 due to the even lower electronegativity of arsenic.
- SbH3 (Stibine): The weakest base among these hydrides, as antimony is the least electronegative and least able to donate its lone pair.
Trends in Basic Strength
- The increasing atomic size and decreasing electronegativity from nitrogen to antimony lead to a decrease in basic strength. Hence, the sequence should be:
NH3 > PH3 > AsH3 > SbH3 (decreasing basic strength)
Conclusion
Therefore, option C is incorrect as it suggests an increasing trend in basic strength when the actual trend is a decreasing one. The other options (A, B, and D) align correctly with their respective trends, making option C the odd one out.
In the provided options, the sequence in option C is identified as incorrect due to the increasing basic strength of hydrides of Group 15 elements (NH3, PH3, AsH3, SbH3).
Basic Strength of Hydrides
- NH3 (Ammonia): Strong base due to high electronegativity of nitrogen.
- PH3 (Phosphine): Weaker base compared to NH3, as phosphorus is less electronegative and does not effectively donate the lone pair.
- AsH3 (Arsine): Even weaker than PH3 due to the even lower electronegativity of arsenic.
- SbH3 (Stibine): The weakest base among these hydrides, as antimony is the least electronegative and least able to donate its lone pair.
Trends in Basic Strength
- The increasing atomic size and decreasing electronegativity from nitrogen to antimony lead to a decrease in basic strength. Hence, the sequence should be:
NH3 > PH3 > AsH3 > SbH3 (decreasing basic strength)
Conclusion
Therefore, option C is incorrect as it suggests an increasing trend in basic strength when the actual trend is a decreasing one. The other options (A, B, and D) align correctly with their respective trends, making option C the odd one out.
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In which of the following arrangements the sequence is not strictly according to the property written against it: a)CO2< SiO2< SnO2< PbO2: increasing oxidising power b)HF < HCl < HBr < HI: increasing acid strength c)NH3< PH3< AsH3< SbH3: increasing basic strength d)B < C < O < N: increasing first ionization enthalpyCorrect answer is option 'C'. Can you explain this answer?
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