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The Selenium tetrachloride Lewis structure is Se–Cl single bond, Se–Cl single bond, Se–Cl single bond and Se–Cl single bond; the central Se has 5 electron domains (1 lone pair), giving a trigonal bipyramidal electron-domain arrangement and a seesaw molecular geometry with a ≈90° / 120° bond angle. Se is best described as sp3d-hybridized, and Selenium tetrachloride is polar because the seesaw shape (and/or unequal terminal atoms) prevents cancellation of the bond dipoles.
Figure 1: Lewis Structure of Selenium tetrachloride (Cl4Se)
| Chemical Formula | Cl4Se |
| CAS Number | 10026-03-6 |
| Total Valence Electrons | 34 |
| Lewis Structure | Se–Cl single bond, Se–Cl single bond, Se–Cl single bond and Se–Cl single bond |
| Electron-Domain Geometry | trigonal bipyramidal |
| Molecular Geometry | seesaw |
| Hybridization Model | sp3d (central Se) |
| Bond Angle | ≈90° / 120° |
| Polarity | Polar molecule |
This organic compound is used as a solvent, intermediate or specialty reagent in fine-chemical, pharmaceutical and materials synthesis; specify grade and impurity profile when sourcing.
To draw the Selenium tetrachloride Lewis structure we first count the total valence electrons. Cl4Se contains 4×7 (Cl) + 6 (Se); the net charge of 0 gives a total of 34 valence electrons to place.
The central atom is Se. 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) + 6 (Se) = 34 electrons.
Place Se 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: Se–Cl single bond, Se–Cl single bond, Se–Cl single bond and Se–Cl single bond; one lone pair on Se.
Counting bonding and nonbonding electrons around Se therefore satisfies the octet/expanded-octet requirement for the drawn structure.
VSEPR theory states that the 5 electron domains around Se arrange to minimize mutual repulsion, giving an trigonal bipyramidal 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 seesaw; the Se bond angle is set to ≈90° / 120° 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 Se, 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, Se uses sp3d hybrid orbitals to form the 5 equivalent electron-domain directions (4 bonding + 1 lone pair).
Formal charge on central Se = V − N − ½B = 6 − 2 − 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.
Selenium tetrachloride is polar. The seesaw 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 Selenium tetrachloride the seesaw 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 |
|---|---|---|---|---|---|
| Selenium tetrachloride | Cl4Se | Se | 5 | seesaw | Polar |
| Selenium dioxide | O2Se | Se | 3 | bent | Polar |
| Hydrogen selenide | H2Se | Se | 4 | bent | Polar |
Selenium tetrachloride is polar. Its seesaw geometry (and/or unequal terminal atoms) stops the bond dipoles from cancelling.
Se–Cl single bond, Se–Cl single bond, Se–Cl single bond and Se–Cl single bond; one lone pair on Se. It uses all 34 valence electrons and the preferred structure carries zero formal charge on the central atom.
The Se angle is about ≈90° / 120°. Lone-pair repulsion compresses the angle from the ideal trigonal bipyramidal value.
The conventional model is sp3d. Selenium tetrachloride has 5 electron domains around the central Se.
The CAS number is 10026-03-6. PubChem (CID 66205) and NIST identify this with Cl4Se; 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 10026-03-6 identifies the substance, not a universal purity specification.
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