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The Xenon trifluoride Lewis structure is Xe–F single bond, Xe–F single bond and Xe–F single bond; the central Xe has 6 electron domains (2 lone pairs), giving a octahedral electron-domain arrangement and a see text molecular geometry with a — bond angle. Xe is best described as sp3d2-hybridized, and Xenon trifluoride is polar because the see text shape (and/or unequal terminal atoms) prevents cancellation of the bond dipoles.
Figure 1: Lewis Structure of Xenon trifluoride (F3Xe)
| Chemical Formula | F3Xe |
| CAS Number | 13709-45-0 |
| Total Valence Electrons | 29 |
| Lewis Structure | Xe–F single bond, Xe–F single bond and Xe–F single bond |
| Electron-Domain Geometry | octahedral |
| Molecular Geometry | see text |
| Hybridization Model | sp3d2 (central Xe) |
| Bond Angle | — |
| Polarity | Polar molecule |
Noble-gas compounds such as Xenon trifluoride are among the strongest known fluorinating and oxidizing agents. XeF2 is valued as a selective fluorinator and as a photoresist/oxide etchant in microelectronics, while the higher fluorides are used in fluorination and as powerful oxidizers. They react vigorously with water and organics and are handled only in passivated, rigorously dry systems.
To draw the Xenon trifluoride Lewis structure we first count the total valence electrons. F3Xe contains 3×7 (F) + 8 (Xe); the net charge of 0 gives a total of 29 valence electrons to place.
The central atom is Xe. It is the least electronegative atom capable of forming multiple bonds and is surrounded by the more electronegative terminal atom(s); hydrogen, when present, always occupies a terminal position. Electronegativity considerations place the electron density toward the terminal atom(s).
Total valence electrons = 3×7 (F) + 8 (Xe) = 29 electrons.
Place Xe at the center and connect each surrounding atom with a single bond, complete octets on the terminal atoms, and place any remaining electrons on the central atom. The resulting electron distribution is: Xe–F single bond, Xe–F single bond and Xe–F single bond; 2 lone pairs on Xe and one unpaired electron on Xe.
Counting bonding and nonbonding electrons around Xe therefore satisfies the octet/expanded-octet requirement for the drawn structure.
VSEPR theory states that the 6 electron domains around Xe arrange to minimize mutual repulsion, giving an octahedral electron-domain geometry.
Because 2 of these domains are lone pair(s) — and lone pairs repel more strongly than bonding pairs — the observed molecular geometry is see text; the Xe bond angle is set to — rather than the ideal value for the electron-domain geometry.
A useful VSEPR approximation is: lone pair–lone pair repulsion > lone pair–bonding pair repulsion > bonding pair–bonding pair repulsion. With 2 lone pair(s) on Xe, the lone-pair domains occupy positions that minimize overall repulsion while pushing the bonding domains (and therefore the bonded atoms) closer together.
In the conventional localized-bond model, Xe uses sp3d2 hybrid orbitals to form the 6 equivalent electron-domain directions (3 bonding + 2 lone pair).
Formal charge on central Xe = V − N − ½B = 8 − 4 − ½×6 = 1. The nonzero formal charge is distributed by resonance / charge separation; the drawn structure is the lowest-energy contributor.
Xenon trifluoride is polar. The see text shape prevents cancellation of the bond dipoles. The bond dipoles do not cancel, leaving a net molecular dipole, which strongly influences solvation behavior and intermolecular interactions.
The decisive structural fact is not simply that the individual bonds are polar; it is whether molecular symmetry allows their vector sum to vanish. In Xenon trifluoride the see text arrangement prevents cancellation, so a permanent dipole remains.
Interpretation consistent with standard VSEPR / molecular-geometry references.This polarity profile underpins its behavior as a solvent, reactant or process intermediate; when sourcing, specify grade and container compatibility.
| Species | Formula | Central Atom | Electron Domains | Molecular Geometry | Polarity |
|---|---|---|---|---|---|
| Xenon trifluoride | F3Xe | Xe | 6 | see text | Polar |
| Xenon difluoride | F2Xe | Xe | 5 | linear | Nonpolar |
| Xenon tetrafluoride | F4Xe | Xe | 6 | square planar | Nonpolar |
| Xenon hexafluoride | F6Xe | Xe | 7 | distorted octahedral (seven domains) | Polar |
Xenon trifluoride is polar. Its see text geometry (and/or unequal terminal atoms) stops the bond dipoles from cancelling.
Xe–F single bond, Xe–F single bond and Xe–F single bond; 2 lone pairs on Xe and one unpaired electron on Xe. It uses all 29 valence electrons and the preferred structure carries a formal charge of 1 on the central atom.
The Xe angle is about —. Lone-pair repulsion compresses the angle from the ideal octahedral value.
The conventional model is sp3d2. Xenon trifluoride has 6 electron domains around the central Xe.
The CAS number is 13709-45-0. PubChem and NIST identify this with F3Xe; use it to locate suppliers and database records.
Technical scope: Lewis structures, VSEPR and hybridization are model-based descriptions for chemical communication and structure prediction; actual molecular electronic structure is more accurately represented by molecular-orbital and quantum-chemical methods. Commercial grades vary substantially by supplier and intended use; CAS 13709-45-0 identifies the substance, not a universal purity specification.
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