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The shape of XeO2F2 molecule is
- a)trigonal bipyramidal
- b)square planar
- c)tetrahedral
- d)see-saw
Correct answer is option 'D'. Can you explain this answer?
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The shape of XeO2F2 molecule isa)trigonal bipyramidalb)square planarc...
XeO2F2 has trigonal bipyramidal geometry, but due to presence of lone pairs of electrons on equatorial position, its actual shape is see-saw.
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The shape of XeO2F2 molecule isa)trigonal bipyramidalb)square planarc...
Understanding the Molecular Geometry of XeO2F2
The molecular shape of xenon oxydifluoride (XeO2F2) can be analyzed using the VSEPR (Valence Shell Electron Pair Repulsion) theory, which helps predict the geometry of molecules based on the repulsion between electron pairs.
Electron Pair Geometry
- XeO2F2 has a total of 4 bonding pairs (2 O and 2 F) and 1 lone pair on the central xenon atom.
- This results in a total of 5 electron pairs around the xenon atom.
Prediction of Shape
- According to VSEPR theory, when there are 5 electron pairs, the electron pair geometry is trigonal bipyramidal.
- However, the presence of a lone pair affects the arrangement of the bonded atoms.
Actual Molecular Shape
- The lone pair occupies one of the equatorial positions in the trigonal bipyramidal arrangement.
- This forces the bonded atoms (2 O and 2 F) to adopt a see-saw shape due to the repulsion from the lone pair.
Conclusion
- Therefore, the correct molecular shape of XeO2F2 is see-saw, confirming that option 'D' is correct.
This understanding of molecular geometry is crucial in the study of chemical bonding and reactivity, especially for competitive exams like NEET.
The molecular shape of xenon oxydifluoride (XeO2F2) can be analyzed using the VSEPR (Valence Shell Electron Pair Repulsion) theory, which helps predict the geometry of molecules based on the repulsion between electron pairs.
Electron Pair Geometry
- XeO2F2 has a total of 4 bonding pairs (2 O and 2 F) and 1 lone pair on the central xenon atom.
- This results in a total of 5 electron pairs around the xenon atom.
Prediction of Shape
- According to VSEPR theory, when there are 5 electron pairs, the electron pair geometry is trigonal bipyramidal.
- However, the presence of a lone pair affects the arrangement of the bonded atoms.
Actual Molecular Shape
- The lone pair occupies one of the equatorial positions in the trigonal bipyramidal arrangement.
- This forces the bonded atoms (2 O and 2 F) to adopt a see-saw shape due to the repulsion from the lone pair.
Conclusion
- Therefore, the correct molecular shape of XeO2F2 is see-saw, confirming that option 'D' is correct.
This understanding of molecular geometry is crucial in the study of chemical bonding and reactivity, especially for competitive exams like NEET.
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The shape of XeO2F2 molecule isa)trigonal bipyramidalb)square planarc)tetrahedrald)see-sawCorrect answer is option 'D'. Can you explain this answer?
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