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Which of the following pairs are isostructural?
- a)SO2-4 and BF-4
- b)NH3 and NH+4
- c)CO32- and CO2
- d)CH4 and BF3
Correct answer is option 'A'. Can you explain this answer?
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Which of the following pairs are isostructural?a)SO2-4 and BF-4b)NH3 a...
SO2-4 and BF-4 have sp3 hybridisation and are tetrahedral in shape.
Most Upvoted Answer
Which of the following pairs are isostructural?a)SO2-4 and BF-4b)NH3 a...
Answer:
Explanation:
To determine which of the given pairs are isostructural, we need to compare their molecular geometries and electron pair arrangements.
a) SO2-4 and BF-4:
- The sulfate ion (SO2-4) has a tetrahedral electron pair arrangement and a trigonal pyramidal molecular geometry.
- The tetrahedral electron pair arrangement means that there are four electron pairs around the central atom (S), including three bonding pairs and one lone pair.
- The trigonal pyramidal molecular geometry arises from the repulsion between the bonding pairs and the lone pair, which causes the bonding pairs to be pushed closer together, creating a slight distortion in the molecular shape.
- The tetrafluoroborate ion (BF-4) also has a tetrahedral electron pair arrangement and a trigonal pyramidal molecular geometry.
- Similar to the sulfate ion, the tetrahedral electron pair arrangement in the tetrafluoroborate ion results from the presence of four electron pairs around the central atom (B), including three bonding pairs and one lone pair.
- The repulsion between the bonding pairs and the lone pair leads to a distortion in the molecular shape, resulting in a trigonal pyramidal geometry.
- Since both SO2-4 and BF-4 have the same electron pair arrangement (tetrahedral) and molecular geometry (trigonal pyramidal), they are isostructural.
b) NH3 and NH4:
- Ammonia (NH3) has a trigonal pyramidal electron pair arrangement and a trigonal pyramidal molecular geometry.
- The trigonal pyramidal electron pair arrangement arises from the presence of three electron pairs around the central atom (N), including three bonding pairs and no lone pairs.
- The molecular geometry is also trigonal pyramidal since there is no repulsion between bonding pairs and lone pairs.
- The ammonium ion (NH4) also has a trigonal pyramidal electron pair arrangement and a trigonal pyramidal molecular geometry.
- The trigonal pyramidal electron pair arrangement results from the presence of three electron pairs around the central atom (N), including three bonding pairs and no lone pairs.
- Again, there is no repulsion between bonding pairs and lone pairs, leading to a trigonal pyramidal molecular geometry.
- Since both NH3 and NH4 have the same electron pair arrangement (trigonal pyramidal) and molecular geometry (trigonal pyramidal), they are isostructural.
c) CO32- and CO2:
- The carbonate ion (CO32-) has a trigonal planar electron pair arrangement and a trigonal planar molecular geometry.
- The trigonal planar electron pair arrangement arises from the presence of three electron pairs around the central atom (C), including three bonding pairs and no lone pairs.
- The molecular geometry is also trigonal planar since there is no repulsion between bonding pairs and lone pairs.
- Carbon dioxide (CO2) has a linear electron pair arrangement and a linear molecular geometry.
- The linear electron pair arrangement results from the presence of two electron pairs around the central atom (C), including two bonding pairs and no lone pairs.
- The molecular geometry is also linear since there is no repulsion between bonding pairs and lone pairs.
- Since CO32- and CO2 have different electron
Explanation:
To determine which of the given pairs are isostructural, we need to compare their molecular geometries and electron pair arrangements.
a) SO2-4 and BF-4:
- The sulfate ion (SO2-4) has a tetrahedral electron pair arrangement and a trigonal pyramidal molecular geometry.
- The tetrahedral electron pair arrangement means that there are four electron pairs around the central atom (S), including three bonding pairs and one lone pair.
- The trigonal pyramidal molecular geometry arises from the repulsion between the bonding pairs and the lone pair, which causes the bonding pairs to be pushed closer together, creating a slight distortion in the molecular shape.
- The tetrafluoroborate ion (BF-4) also has a tetrahedral electron pair arrangement and a trigonal pyramidal molecular geometry.
- Similar to the sulfate ion, the tetrahedral electron pair arrangement in the tetrafluoroborate ion results from the presence of four electron pairs around the central atom (B), including three bonding pairs and one lone pair.
- The repulsion between the bonding pairs and the lone pair leads to a distortion in the molecular shape, resulting in a trigonal pyramidal geometry.
- Since both SO2-4 and BF-4 have the same electron pair arrangement (tetrahedral) and molecular geometry (trigonal pyramidal), they are isostructural.
b) NH3 and NH4:
- Ammonia (NH3) has a trigonal pyramidal electron pair arrangement and a trigonal pyramidal molecular geometry.
- The trigonal pyramidal electron pair arrangement arises from the presence of three electron pairs around the central atom (N), including three bonding pairs and no lone pairs.
- The molecular geometry is also trigonal pyramidal since there is no repulsion between bonding pairs and lone pairs.
- The ammonium ion (NH4) also has a trigonal pyramidal electron pair arrangement and a trigonal pyramidal molecular geometry.
- The trigonal pyramidal electron pair arrangement results from the presence of three electron pairs around the central atom (N), including three bonding pairs and no lone pairs.
- Again, there is no repulsion between bonding pairs and lone pairs, leading to a trigonal pyramidal molecular geometry.
- Since both NH3 and NH4 have the same electron pair arrangement (trigonal pyramidal) and molecular geometry (trigonal pyramidal), they are isostructural.
c) CO32- and CO2:
- The carbonate ion (CO32-) has a trigonal planar electron pair arrangement and a trigonal planar molecular geometry.
- The trigonal planar electron pair arrangement arises from the presence of three electron pairs around the central atom (C), including three bonding pairs and no lone pairs.
- The molecular geometry is also trigonal planar since there is no repulsion between bonding pairs and lone pairs.
- Carbon dioxide (CO2) has a linear electron pair arrangement and a linear molecular geometry.
- The linear electron pair arrangement results from the presence of two electron pairs around the central atom (C), including two bonding pairs and no lone pairs.
- The molecular geometry is also linear since there is no repulsion between bonding pairs and lone pairs.
- Since CO32- and CO2 have different electron
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Which of the following pairs are isostructural?a)SO2-4 and BF-4b)NH3 and NH+4c)CO32- and CO2d)CH4 and BF3Correct answer is option 'A'. Can you explain this answer?
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