Among the following, the CORRECT combinations are
A. $ \mathrm{IF_3} \rightarrow $ T-shaped ($ sp^3d $)
B. $ \mathrm{IF_5} \rightarrow $ Square pyramidal ($ sp^3d^2 $)
C. $ \mathrm{IF_7} \rightarrow $ Pentagonal bipyramidal ($ sp^3d^3 $)
D. $ \mathrm{ClO_4^-} \rightarrow $ Square planar ($ sp^2d $)
Choose the correct answer from the options given below:

Question

What is the molar mass of sulfur dioxide (SO$_2)$?

Answer 1

To determine the correct combinations of molecular shapes and hybridizations for the given compounds, let's analyze each option individually:

$\mathrm{IF_3}$ - T-shaped ($sp^3d$):
- $\mathrm{IF_3}$ has 3 bonded pairs and 2 lone pairs of electrons on the iodine atom.
- The electron geometry is trigonal bipyramidal, and the molecular geometry is T-shaped.
- The hybridization for iodine in $\mathrm{IF_3}$ is $sp^3d$.
Conclusion: The shape and hybridization combination given is correct.
$\mathrm{IF_5}$ - Square pyramidal ($sp^3d^2$):
- $\mathrm{IF_5}$ has 5 bonded pairs and 1 lone pair of electrons on the iodine atom.
- The electron geometry is octahedral, and the molecular geometry is square pyramidal.
- The hybridization for iodine in $\mathrm{IF_5}$ is $sp^3d^2$.
Conclusion: The shape and hybridization combination given is correct.
$\mathrm{IF_7}$ - Pentagonal bipyramidal ($sp^3d^3$):
- $\mathrm{IF_7}$ has 7 bonded pairs and no lone pairs on the iodine atom.
- The electron and molecular geometry is pentagonal bipyramidal.
- The hybridization for iodine in $\mathrm{IF_7}$ is $sp^3d^3$.
Conclusion: The shape and hybridization combination given is correct.
$\mathrm{ClO_4^-}$ - Square planar ($sp^2d$):
- $\mathrm{ClO_4^-}$ has 4 bonded pairs and no lone pairs on the chlorine atom.
- The electron geometry is tetrahedral, not square planar, for such coordination.
- There is an incorrect assumption of square planar geometry and $sp^2d$ hybridization. The correct geometry is tetrahedral, with $sp^3$ hybridization.
Conclusion: The shape and hybridization combination given is incorrect.

After evaluating each combination, we find that the given option A, B, C and D is incorrect based on the information for $\mathrm{ClO_4^-}$. Therefore, there seems to be a mismatch between the options provided and their correctness in the chemical context. Double-check the specific question or options for accuracy.

Answer 2

To determine the correct combinations of molecular shapes and hybridizations for the given compounds, let's analyze each option individually:

$\mathrm{IF_3}$ - T-shaped ($sp^3d$):
- $\mathrm{IF_3}$ has 3 bonded pairs and 2 lone pairs of electrons on the iodine atom.
- The electron geometry is trigonal bipyramidal, and the molecular geometry is T-shaped.
- The hybridization for iodine in $\mathrm{IF_3}$ is $sp^3d$.
Conclusion: The shape and hybridization combination given is correct.
$\mathrm{IF_5}$ - Square pyramidal ($sp^3d^2$):
- $\mathrm{IF_5}$ has 5 bonded pairs and 1 lone pair of electrons on the iodine atom.
- The electron geometry is octahedral, and the molecular geometry is square pyramidal.
- The hybridization for iodine in $\mathrm{IF_5}$ is $sp^3d^2$.
Conclusion: The shape and hybridization combination given is correct.
$\mathrm{IF_7}$ - Pentagonal bipyramidal ($sp^3d^3$):
- $\mathrm{IF_7}$ has 7 bonded pairs and no lone pairs on the iodine atom.
- The electron and molecular geometry is pentagonal bipyramidal.
- The hybridization for iodine in $\mathrm{IF_7}$ is $sp^3d^3$.
Conclusion: The shape and hybridization combination given is correct.
$\mathrm{ClO_4^-}$ - Square planar ($sp^2d$):
- $\mathrm{ClO_4^-}$ has 4 bonded pairs and no lone pairs on the chlorine atom.
- The electron geometry is tetrahedral, not square planar, for such coordination.
- There is an incorrect assumption of square planar geometry and $sp^2d$ hybridization. The correct geometry is tetrahedral, with $sp^3$ hybridization.
Conclusion: The shape and hybridization combination given is incorrect.

After evaluating each combination, we find that the given option A, B, C and D is incorrect based on the information for $\mathrm{ClO_4^-}$. Therefore, there seems to be a mismatch between the options provided and their correctness in the chemical context. Double-check the specific question or options for accuracy.

Show Hint

The Correct Option is A

Solution and Explanation

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