(a) XeF2,
(b) XeF4,
(c) XeF6,
(d) XeOF4,
(e) XeO2F2. In each case Xe is the central atom.
The Correct Answer and Explanation is:
Here’s a detailed analysis of the molecular geometry, hybridization, and bonding of each xenon compound:
(a) XeF₂ – Xenon Difluoride
- Lewis Structure: Xe is bonded to two fluorine atoms, with 3 lone pairs on Xe.
- Electron Domains: 5 (2 bonding + 3 lone pairs)
- Electron Geometry: Trigonal bipyramidal
- Molecular Geometry: Linear
- Hybridization: sp³d
Explanation:
XeF₂ has five electron domains around xenon — two bonding pairs and three lone pairs. The three lone pairs occupy equatorial positions in the trigonal bipyramidal arrangement to minimize repulsion, leaving the two fluorine atoms in axial positions. This gives XeF₂ a linear molecular geometry. Despite xenon being a noble gas, it can expand its octet due to the availability of 5d orbitals.
(b) XeF₄ – Xenon Tetrafluoride
- Lewis Structure: Xe is bonded to four F atoms, with 2 lone pairs on Xe.
- Electron Domains: 6 (4 bonding + 2 lone pairs)
- Electron Geometry: Octahedral
- Molecular Geometry: Square planar
- Hybridization: sp³d²
Explanation:
In XeF₄, the six electron domains (4 bonding and 2 lone pairs) arrange in an octahedral geometry. The lone pairs occupy opposite positions, minimizing repulsion. This arrangement results in a square planar molecular geometry. The molecule is symmetric and nonpolar despite the polar Xe–F bonds.
(c) XeF₆ – Xenon Hexafluoride
- Lewis Structure: Xe bonded to 6 F atoms, with 1 lone pair on Xe.
- Electron Domains: 7 (6 bonding + 1 lone pair)
- Electron Geometry: Pentagonal bipyramidal (distorted)
- Molecular Geometry: Distorted octahedral (monocapped)
- Hybridization: sp³d³
Explanation:
XeF₆ has seven electron domains. Ideally, this leads to a pentagonal bipyramidal electron geometry, but the presence of one lone pair distorts the shape. The molecule adopts a distorted octahedral geometry with one position occupied by a lone pair. It is highly reactive and acts as a fluorinating agent.
(d) XeOF₄ – Xenon Oxytetrafluoride
- Lewis Structure: Xe is bonded to 4 F atoms and 1 O atom (double bond), with 1 lone pair.
- Electron Domains: 6 (5 bonding + 1 lone pair)
- Electron Geometry: Octahedral
- Molecular Geometry: Square pyramidal
- Hybridization: sp³d²
Explanation:
XeOF₄ has six electron domains: one oxygen double bond, four fluorine bonds, and one lone pair. The lone pair causes a distortion from the ideal octahedral shape, resulting in a square pyramidal geometry. The presence of both electronegative fluorine and oxygen makes this molecule polar.
(e) XeO₂F₂ – Xenon Dioxide Difluoride
- Lewis Structure: Xe is bonded to 2 O (double bonds) and 2 F atoms, with 1 lone pair.
- Electron Domains: 5 (4 bonding + 1 lone pair)
- Electron Geometry: Trigonal bipyramidal
- Molecular Geometry: See-saw
- Hybridization: sp³d
Explanation:
With five electron domains and one lone pair, XeO₂F₂ adopts a trigonal bipyramidal electron geometry. The lone pair prefers the equatorial position, leading to a see-saw shape. The molecular geometry is asymmetric and polar due to the differences in electronegativity and arrangement of atoms.
These xenon compounds illustrate the ability of noble gases to form stable compounds by expanding their valence shells, often resulting in complex geometries driven by VSEPR theory
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