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Which one of the following pairs is isostructural (i.e., having the same shape and hybridization)? [2012]
- a)
- b)
- c)
- d)
Correct answer is option 'D'. Can you explain this answer?
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Which one of the following pairs is isostructural (i.e., having the sa...
BF4- hybridisation sp3, tetrahedral structure.
NH4+ hybridisation sp3, tetrahedral structure.
NH4+ hybridisation sp3, tetrahedral structure.
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Which one of the following pairs is isostructural (i.e., having the sa...
To determine which pair of compounds is isostructural, we need to compare their molecular shapes and hybridization.
a) BCl3 and BrCl3-:
BCl3 has a trigonal planar shape with sp2 hybridization. Each B-Cl bond is formed by the overlap of one sp2 hybrid orbital from boron and one 2p orbital from chlorine. BrCl3- has a tetrahedral shape, which means it has sp3 hybridization. Therefore, these two compounds are not isostructural.
b) NH3 and NO3-:
NH3 has a trigonal pyramidal shape with sp3 hybridization. Each N-H bond is formed by the overlap of one sp3 hybrid orbital from nitrogen and one 1s orbital from hydrogen. NO3- has a trigonal planar shape, which means it has sp2 hybridization. Therefore, these two compounds are not isostructural.
c) NF3 and BF3:
NF3 has a pyramidal shape with sp3 hybridization. Each N-F bond is formed by the overlap of one sp3 hybrid orbital from nitrogen and one 2p orbital from fluorine. BF3 also has a trigonal planar shape, which means it has sp2 hybridization. Therefore, these two compounds are not isostructural.
d) BF4- and NH4+:
BF4- has a tetrahedral shape with sp3 hybridization. Each B-F bond is formed by the overlap of one sp3 hybrid orbital from boron and one 2p orbital from fluorine. NH4+ also has a tetrahedral shape and sp3 hybridization. Each N-H bond is formed by the overlap of one sp3 hybrid orbital from nitrogen and one 1s orbital from hydrogen. Therefore, these two compounds are isostructural.
In conclusion, the pair of compounds that is isostructural is (d) BF4- and NH4+.
a) BCl3 and BrCl3-:
BCl3 has a trigonal planar shape with sp2 hybridization. Each B-Cl bond is formed by the overlap of one sp2 hybrid orbital from boron and one 2p orbital from chlorine. BrCl3- has a tetrahedral shape, which means it has sp3 hybridization. Therefore, these two compounds are not isostructural.
b) NH3 and NO3-:
NH3 has a trigonal pyramidal shape with sp3 hybridization. Each N-H bond is formed by the overlap of one sp3 hybrid orbital from nitrogen and one 1s orbital from hydrogen. NO3- has a trigonal planar shape, which means it has sp2 hybridization. Therefore, these two compounds are not isostructural.
c) NF3 and BF3:
NF3 has a pyramidal shape with sp3 hybridization. Each N-F bond is formed by the overlap of one sp3 hybrid orbital from nitrogen and one 2p orbital from fluorine. BF3 also has a trigonal planar shape, which means it has sp2 hybridization. Therefore, these two compounds are not isostructural.
d) BF4- and NH4+:
BF4- has a tetrahedral shape with sp3 hybridization. Each B-F bond is formed by the overlap of one sp3 hybrid orbital from boron and one 2p orbital from fluorine. NH4+ also has a tetrahedral shape and sp3 hybridization. Each N-H bond is formed by the overlap of one sp3 hybrid orbital from nitrogen and one 1s orbital from hydrogen. Therefore, these two compounds are isostructural.
In conclusion, the pair of compounds that is isostructural is (d) BF4- and NH4+.
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Which one of the following pairs is isostructural (i.e., having the same shape and hybridization)? [2012]a)b)c)d)Correct answer is option 'D'. Can you explain this answer?
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