Question:
The shapes of \(XeF_2\), \(XeF_4\), and \(XeO_3\) respectively are
The shapes of \(XeF_2\), \(XeF_4\), and \(XeO_3\) respectively are
Show Hint
Using VSEPR theory:
\[
AX_2E_3 \rightarrow \text{Linear}
\]
\[
AX_4E_2 \rightarrow \text{Square planar}
\]
\[
AX_3E \rightarrow \text{Pyramidal}
\]
where \(E\) represents lone pairs.
Updated On: Jun 24, 2026
- Linear, Tetrahedral, Pyramidal
- Angular, Square Planar, Pyramidal
- Linear, Tetrahedral, Planar
- Linear, Square planar, Pyramidal
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The Correct Option is D
Solution and Explanation
Step 1: Determine the shape of \(XeF_2\).
In \[ XeF_2, \] xenon has \[ 5 \] electron pairs around it: \[ 2\ \text{bond pairs} + 3\ \text{lone pairs} \] According to VSEPR theory, the electron pair geometry is trigonal bipyramidal.
The three lone pairs occupy equatorial positions, leaving the two fluorine atoms opposite to each other.
Hence, the molecular shape is Linear
Step 2: Determine the shape of \(XeF_4\).
In \[ XeF_4, \] xenon has \[ 6 \] electron pairs: \[ 4\ \text{bond pairs} + 2\ \text{lone pairs} \] The electron pair geometry is octahedral.
The two lone pairs occupy opposite positions to minimize repulsion.
Therefore, the molecular shape becomes Square planar
Step 3: Determine the shape of \(XeO_3\).
In \[ XeO_3, \] xenon has \[ 4 \] electron domains: \[ 3\ \text{bond pairs} + 1\ \text{lone pair} \] The electron pair geometry is tetrahedral.
Due to one lone pair, the molecular shape becomes Trigonal pyramidal which is commonly written as Pyramidal
Step 4: Final conclusion.
Thus, the shapes are: \[ XeF_2 \rightarrow \text{Linear} \] \[ XeF_4 \rightarrow \text{Square planar} \] \[ XeO_3 \rightarrow \text{Pyramidal} \] Therefore, the correct answer is \[ \boxed{\text{Linear, Square planar, Pyramidal}} \]
In \[ XeF_2, \] xenon has \[ 5 \] electron pairs around it: \[ 2\ \text{bond pairs} + 3\ \text{lone pairs} \] According to VSEPR theory, the electron pair geometry is trigonal bipyramidal.
The three lone pairs occupy equatorial positions, leaving the two fluorine atoms opposite to each other.
Hence, the molecular shape is Linear
Step 2: Determine the shape of \(XeF_4\).
In \[ XeF_4, \] xenon has \[ 6 \] electron pairs: \[ 4\ \text{bond pairs} + 2\ \text{lone pairs} \] The electron pair geometry is octahedral.
The two lone pairs occupy opposite positions to minimize repulsion.
Therefore, the molecular shape becomes Square planar
Step 3: Determine the shape of \(XeO_3\).
In \[ XeO_3, \] xenon has \[ 4 \] electron domains: \[ 3\ \text{bond pairs} + 1\ \text{lone pair} \] The electron pair geometry is tetrahedral.
Due to one lone pair, the molecular shape becomes Trigonal pyramidal which is commonly written as Pyramidal
Step 4: Final conclusion.
Thus, the shapes are: \[ XeF_2 \rightarrow \text{Linear} \] \[ XeF_4 \rightarrow \text{Square planar} \] \[ XeO_3 \rightarrow \text{Pyramidal} \] Therefore, the correct answer is \[ \boxed{\text{Linear, Square planar, Pyramidal}} \]
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