-
We detected your language preference as English. Would you like to switch to the English version for a better experience?
Switch to English
Stay here
The Xenon oxytetrafluoride Lewis structure is Xe–F single bond, Xe–F single bond, Xe–F single bond, Xe–F single bond and Xe–O double bond; the central Xe has 6 electron domains (1 lone pair), giving a octahedral electron-domain arrangement and a square pyramidal molecular geometry with a 90° bond angle. Xe is best described as sp3d2-hybridized, and Xenon oxytetrafluoride is polar because the square pyramidal shape (and/or unequal terminal atoms) prevents cancellation of the bond dipoles.
Figure 1: Lewis Structure of Xenon oxytetrafluoride (F4OXe)
| Chemical Formula | F4OXe |
| CAS Number | 13774-85-1 |
| Total Valence Electrons | 42 |
| Lewis Structure | Xe–F single bond, Xe–F single bond, Xe–F single bond, Xe–F single bond and Xe–O double bond |
| Electron-Domain Geometry | octahedral |
| Molecular Geometry | square pyramidal |
| Hybridization Model | sp3d2 (central Xe) |
| Bond Angle | 90° |
| Polarity | Polar molecule |
Noble-gas compounds such as Xenon oxytetrafluoride 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 oxytetrafluoride Lewis structure we first count the total valence electrons. F4OXe contains 4×7 (F) + 6 (O) + 8 (Xe); the net charge of 0 gives a total of 42 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 = 4×7 (F) + 6 (O) + 8 (Xe) = 42 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, Xe–F single bond, Xe–F single bond and Xe–O double bond; one lone pair 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 1 of these domains are lone pair(s) — and lone pairs repel more strongly than bonding pairs — the observed molecular geometry is square pyramidal; the Xe bond angle is set to 90° 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 1 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 (5 bonding + 1 lone pair).
Formal charge on central Xe = V − N − ½B = 8 − 2 − ½×12 = 0. The preferred Lewis structure carries zero formal charge on the central atom (and on the terminals), so it is the dominant contributor.
Xenon oxytetrafluoride is polar. The square pyramidal 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 oxytetrafluoride the square pyramidal 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 oxytetrafluoride | F4OXe | Xe | 6 | square pyramidal | 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 oxytetrafluoride is polar. Its square pyramidal geometry (and/or unequal terminal atoms) stops the bond dipoles from cancelling.
Xe–F single bond, Xe–F single bond, Xe–F single bond, Xe–F single bond and Xe–O double bond; one lone pair on Xe. It uses all 42 valence electrons and the preferred structure carries zero formal charge on the central atom.
The Xe angle is about 90°. Lone-pair repulsion compresses the angle from the ideal octahedral value.
The conventional model is sp3d2. Xenon oxytetrafluoride has 6 electron domains around the central Xe.
The CAS number is 13774-85-1. PubChem and NIST identify this with F4OXe; 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 13774-85-1 identifies the substance, not a universal purity specification.
 |
|
 |
 |
|
EN
Agricultural News
Food News
Industrial News
Cosmetic News
Pharmaceutical News
Science News
4YRS
