Xenon difluoride Lewis Structure

Xenon difluoride Lewis Structure: F₂Xe Lewis Structure, linear Geometry, sp3d Hybridization & Polarity

Xenon difluoride Key Facts

The Xenon difluoride Lewis structure is Xe–F single bond and Xe–F single bond; the central Xe has 5 electron domains (3 lone pairs), giving a trigonal bipyramidal electron-domain arrangement and a linear molecular geometry with a 180° bond angle. Xe is best described as sp3d-hybridized, and Xenon difluoride is nonpolar because the bond dipoles cancel by molecular symmetry.

Figure 1: Lewis Structure of Xenon difluoride (F₂Xe)

Chemical Formula	F₂Xe
CAS Number	13709-36-9
Total Valence Electrons	22
Lewis Structure	Xe–F single bond and Xe–F single bond
Electron-Domain Geometry	trigonal bipyramidal
Molecular Geometry	linear
Hybridization Model	sp3d (central Xe)
Bond Angle	180°
Polarity	Nonpolar molecule

PubChem (CID 83674) and NIST list Xenon difluoride as F ₂Xe with CAS 13709-36-9; molecular weight ≈ 169.29 g/mol. View CAS 13709-36-9 dictionary details on Guidechem →

Applications of Xenon difluoride (CAS 13709-36-9)

Noble-gas compounds such as Xenon difluoride 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.

Selective Fluorinator XeF₂ in particular is used to introduce fluorine and to etch oxides in semiconductor processing.

Strong Oxidizer Higher xenon fluorides oxidize refractory metals and support specialized fluorination.

Handling Moisture- and organics-sensitive; processed in passivated, anhydrous equipment.

Procurement Note "Xenon difluoride" is supplied in multiple commercial grades and package sizes. Specify purity, grade, moisture/impurity limits, package (cylinder, drum or bulk) and intended process, and use CAS 13709-36-9 as the primary identifier when screening suppliers; always confirm regional availability and safety documentation (SDS).

Step 1 - Valence Electrons & Central Atom

To draw the Xenon difluoride Lewis structure we first count the total valence electrons. F₂Xe contains 2×7 (F) + 8 (Xe); the net charge of 0 gives a total of 22 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).

Valence-electron count

Total valence electrons = 2×7 (F) + 8 (Xe) = 22 electrons.

Step 2 - Lewis Structure & Electron Distribution

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 and Xe–F single bond; 3 lone pairs on Xe.

Counting bonding and nonbonding electrons around Xe therefore satisfies the octet/expanded-octet requirement for the drawn structure.

Xe–F Xe–F

Xe: 3 lone pairs, 2 bonding domains

2 bonding domains + 3 lone pairs = 5 electron domains

Expanded Octet: d-Orbital Participation Central Xe belongs to period 3 or below, so it can accommodate more than eight electrons: low-lying d orbitals become available and the linear arrangement with 5 domains reflects this expanded valence shell. The octet rule alone does not apply to such hypervalent species.

Step 3 - VSEPR Theory & Geometry

VSEPR theory states that the 5 electron domains around Xe arrange to minimize mutual repulsion, giving an trigonal bipyramidal electron-domain geometry.

Because 3 of these domains are lone pair(s) — and lone pairs repel more strongly than bonding pairs — the observed molecular geometry is linear; the Xe bond angle is set to 180° rather than the ideal value for the electron-domain geometry.

Repulsion hierarchy

A useful VSEPR approximation is: lone pair–lone pair repulsion > lone pair–bonding pair repulsion > bonding pair–bonding pair repulsion. With 3 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.

Hybridization & Formal Charge

In the conventional localized-bond model, Xe uses sp3d hybrid orbitals to form the 5 equivalent electron-domain directions (2 bonding + 3 lone pair).

Formal-charge check

Formal charge on central Xe = V − N − ½B = 8 − 6 − ½×4 = 0. The preferred Lewis structure carries zero formal charge on the central atom (and on the terminals), so it is the dominant contributor.

Modeling Note Modeling Note: sp3d / sp3d hybridization is a convenient localized-bond teaching model. Modern quantum-chemical descriptions of hypervalent Xenon difluoride use molecular orbitals and do not require populated d orbitals as the primary bonding picture.

Is Xenon difluoride Polar or Nonpolar?

Xenon difluoride is nonpolar. Although individual Xe–terminal bonds are polar when the atoms differ in electronegativity, the linear geometry makes their vector sum zero, so there is no net molecular dipole.

Expert Quote — Structural Chemistry Perspective

A common misconception is that polar bonds guarantee a polar molecule. Xenon difluoride shows the opposite: identical bond dipoles arranged with linear symmetry cancel exactly, yielding a nonpolar species.

Interpretation consistent with standard VSEPR / molecular-geometry references.

Its nonpolar character governs solvation and intermolecular behavior; specify grade and handling when sourcing.

Structural Comparison Table

Species	Formula	Central Atom	Electron Domains	Molecular Geometry	Polarity
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

Practice question Starting from the 22 valence electrons of F₂Xe, draw the Lewis structure and confirm the central Xe atom is sp3d-hybridized with linear geometry. What happens to the bond angle if one terminal atom is replaced by a more electronegative substituent?

Looking for industrial bulk or specified-grade supplies of Xenon difluoride (CAS 13709-36-9)? Browse Supplier on Guidechem →

FAQs

Is F₂Xe polar or nonpolar?

Xenon difluoride is nonpolar. Its linear symmetry cancels the bond dipoles exactly.

What is the Lewis structure of Xenon difluoride?

Xe–F single bond and Xe–F single bond; 3 lone pairs on Xe. It uses all 22 valence electrons and the preferred structure carries zero formal charge on the central atom.

What is the bond angle in Xenon difluoride?

The Xe angle is about 180°. Lone-pair repulsion compresses the angle from the ideal trigonal bipyramidal value.

What is the hybridization of Xe in Xenon difluoride?

The conventional model is sp3d. Xenon difluoride has 5 electron domains around the central Xe.

What is the CAS number of Xenon difluoride?

The CAS number is 13709-36-9. PubChem (CID 83674) and NIST identify this with F₂Xe; use it to locate suppliers and database records.

References

PubChem CID 83674, Xenon difluoride. Molecular formula, CAS number, molecular weight and chemical identity.
NIST Chemistry WebBook, SRD 69, Xenon difluoride. Formula, CAS Registry Number and thermochemical / spectroscopic data.
IUPAC Gold Book. Definitions for "lone pair", "VSEPR", "hybridization" and "formal charge".
Atkins, P. & de Paula, J., Physical Chemistry. VSEPR, molecular geometry and dipole moments.
Guidechem supplier & dictionary records. Commercial sourcing and CAS-linked property pages for Xenon difluoride (CAS 13709-36-9).

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 13709-36-9 identifies the substance, not a universal purity specification.

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Xenon difluoride Lewis Structure