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The Xenon tetrachloride Lewis structure is Xe–Cl single bond, Xe–Cl single bond, Xe–Cl single bond and Xe–Cl single bond; the central Xe has 6 electron domains (2 lone pairs), giving a octahedral electron-domain arrangement and a square planar molecular geometry with a 90° bond angle. Xe is best described as sp3d2-hybridized, and Xenon tetrachloride is nonpolar because the bond dipoles cancel by molecular symmetry.
Figure 1: Lewis Structure of Xenon tetrachloride (Cl4Xe)
| Chemical Formula | Cl4Xe |
| CAS Number | 13780-40-0 |
| Total Valence Electrons | 36 |
| Lewis Structure | Xe–Cl single bond, Xe–Cl single bond, Xe–Cl single bond and Xe–Cl single bond |
| Electron-Domain Geometry | octahedral |
| Molecular Geometry | square planar |
| Hybridization Model | sp3d2 (central Xe) |
| Bond Angle | 90° |
| Polarity | Nonpolar molecule |
Noble-gas compounds such as Xenon tetrachloride 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 tetrachloride Lewis structure we first count the total valence electrons. Cl4Xe contains 4×7 (Cl) + 8 (Xe); the net charge of 0 gives a total of 36 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 (Cl) + 8 (Xe) = 36 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–Cl single bond, Xe–Cl single bond, Xe–Cl single bond and Xe–Cl single bond; 2 lone pairs 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 square planar; 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 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 (4 bonding + 2 lone pair).
Formal charge on central Xe = V − N − ½B = 8 − 4 − ½×8 = 0. The preferred Lewis structure carries zero formal charge on the central atom (and on the terminals), so it is the dominant contributor.
Xenon tetrachloride is nonpolar. Although individual Xe–terminal bonds are polar when the atoms differ in electronegativity, the square planar geometry makes their vector sum zero, so there is no net molecular dipole.
A common misconception is that polar bonds guarantee a polar molecule. Xenon tetrachloride shows the opposite: identical bond dipoles arranged with square planar 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.
| Species | Formula | Central Atom | Electron Domains | Molecular Geometry | Polarity |
|---|---|---|---|---|---|
| Xenon tetrachloride | Cl4Xe | Xe | 6 | square planar | Nonpolar |
| 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 tetrachloride is nonpolar. Its square planar symmetry cancels the bond dipoles exactly.
Xe–Cl single bond, Xe–Cl single bond, Xe–Cl single bond and Xe–Cl single bond; 2 lone pairs on Xe. It uses all 36 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 tetrachloride has 6 electron domains around the central Xe.
The CAS number is 13780-40-0. PubChem and NIST identify this with Cl4Xe; 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 13780-40-0 identifies the substance, not a universal purity specification.
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