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Among the following pairs, those in which both the species have the similar shape:
(I) N3-, XeF2
(II) [ClF2]+, [ICl2]+
(III) [ICl4]+, [PtCl4]2-
(IV) XeO3, SO3
(II) [ClF2]+, [ICl2]+
(III) [ICl4]+, [PtCl4]2-
(IV) XeO3, SO3
- a)I and II only
- b)I and III only
- c)I, II and III only
- d)II, III and IV only
Correct answer is option 'A'. Can you explain this answer?
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Most Upvoted Answer
Among the following pairs, those in which both the species have the si...
(I) XeF2 is linear with two F atoms in the axial position and three lone pairs in the equatorial position. N3-(Azide ion) is also linear.
(II) Both the central atoms are halogens, so they will have similar shape.
(III) [ICl4]+ will be see-saw in shape as predicted by VSEPR but [PtCl4]2- is square planar.
(IV) XeO3 has a lone pair and will have pyramidal shape. SO3 has trigonal planar shape.
So, option A is correct.
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Community Answer
Among the following pairs, those in which both the species have the si...
Similar Shapes:
When we talk about the shape of a molecule, we refer to its geometry or arrangement of atoms in three-dimensional space. Two molecules are said to have similar shapes if they have the same geometry or symmetry.
Pairwise Comparison:
(I) N3-, XeF2:
- N3- has a linear geometry with a triple bond between the nitrogen atoms.
- XeF2 has a linear geometry with two lone pairs of electrons on the xenon atom.
- These two molecules have different shapes and hence are not similar.
(II) [ClF2], [ICl2]:
- [ClF2] has a trigonal bipyramidal geometry with one lone pair of electrons on the chlorine atom.
- [ICl2] has a bent or V-shaped geometry with two lone pairs of electrons on the iodine atom.
- These two molecules have different shapes and hence are not similar.
(III) [ICl4], [PtCl4]2-:
- [ICl4] has a square planar geometry with four chlorine atoms and one lone pair of electrons on the iodine atom.
- [PtCl4]2- also has a square planar geometry with four chlorine atoms and two negative charges on the platinum atom.
- These two molecules have the same shape and hence are similar.
(IV) XeO3, SO3:
- XeO3 has a trigonal pyramidal geometry with three oxygen atoms and one lone pair of electrons on the xenon atom.
- SO3 has a trigonal planar geometry with three oxygen atoms and no lone pairs of electrons.
- These two molecules have different shapes and hence are not similar.
Conclusion:
From the pairwise comparison, we can conclude that only option (A) I and II have different shapes, and hence they are the only pairs where both the species do not have similar shapes.
When we talk about the shape of a molecule, we refer to its geometry or arrangement of atoms in three-dimensional space. Two molecules are said to have similar shapes if they have the same geometry or symmetry.
Pairwise Comparison:
(I) N3-, XeF2:
- N3- has a linear geometry with a triple bond between the nitrogen atoms.
- XeF2 has a linear geometry with two lone pairs of electrons on the xenon atom.
- These two molecules have different shapes and hence are not similar.
(II) [ClF2], [ICl2]:
- [ClF2] has a trigonal bipyramidal geometry with one lone pair of electrons on the chlorine atom.
- [ICl2] has a bent or V-shaped geometry with two lone pairs of electrons on the iodine atom.
- These two molecules have different shapes and hence are not similar.
(III) [ICl4], [PtCl4]2-:
- [ICl4] has a square planar geometry with four chlorine atoms and one lone pair of electrons on the iodine atom.
- [PtCl4]2- also has a square planar geometry with four chlorine atoms and two negative charges on the platinum atom.
- These two molecules have the same shape and hence are similar.
(IV) XeO3, SO3:
- XeO3 has a trigonal pyramidal geometry with three oxygen atoms and one lone pair of electrons on the xenon atom.
- SO3 has a trigonal planar geometry with three oxygen atoms and no lone pairs of electrons.
- These two molecules have different shapes and hence are not similar.
Conclusion:
From the pairwise comparison, we can conclude that only option (A) I and II have different shapes, and hence they are the only pairs where both the species do not have similar shapes.
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Among the following pairs, those in which both the species have the similar shape:(I) N3-, XeF2(II) [ClF2]+, [ICl2]+(III) [ICl4]+, [PtCl4]2-(IV) XeO3, SO3a)I and II onlyb)I and III onlyc)I, II and III onlyd)II, III and IV onlyCorrect answer is option 'A'. Can you explain this answer?
Question Description
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