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The Sulfur tetrachloride Lewis structure is S–Cl single bond, S–Cl single bond, S–Cl single bond and S–Cl single bond; the central S 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. S is best described as sp3d-hybridized, and Sulfur tetrachloride is polar because the seesaw shape (and/or unequal terminal atoms) prevents cancellation of the bond dipoles.
Figure 1: Lewis Structure of Sulfur tetrachloride (Cl4S)
| Chemical Formula | Cl4S |
| CAS Number | 13451-08-6 |
| Total Valence Electrons | 34 |
| Lewis Structure | S–Cl single bond, S–Cl single bond, S–Cl single bond and S–Cl single bond |
| Electron-Domain Geometry | trigonal bipyramidal |
| Molecular Geometry | seesaw |
| Hybridization Model | sp3d (central S) |
| 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 Sulfur tetrachloride Lewis structure we first count the total valence electrons. Cl4S contains 4×7 (Cl) + 6 (S); the net charge of 0 gives a total of 34 valence electrons to place.
The central atom is S. 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 (S) = 34 electrons.
Place S 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: S–Cl single bond, S–Cl single bond, S–Cl single bond and S–Cl single bond; one lone pair on S.
Counting bonding and nonbonding electrons around S therefore satisfies the octet/expanded-octet requirement for the drawn structure.
VSEPR theory states that the 5 electron domains around S 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 S 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 S, 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, S uses sp3d hybrid orbitals to form the 5 equivalent electron-domain directions (4 bonding + 1 lone pair).
Formal charge on central S = 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.
Sulfur 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 Sulfur 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 |
|---|---|---|---|---|---|
| Sulfur tetrachloride | Cl4S | S | 5 | seesaw | Polar |
| Sulfur dioxide | SO2 | S | 3 | bent | Polar |
| Sulfur trioxide | O3S | S | 3 | trigonal planar | Nonpolar |
| Sulfur hexafluoride | F6S | S | 6 | octahedral | Nonpolar |
| Sulfur tetrafluoride | F4S | S | 5 | seesaw | Polar |
| Sulfate | O4S | S | 4 | tetrahedral | Nonpolar |
Sulfur tetrachloride is polar. Its seesaw geometry (and/or unequal terminal atoms) stops the bond dipoles from cancelling.
S–Cl single bond, S–Cl single bond, S–Cl single bond and S–Cl single bond; one lone pair on S. It uses all 34 valence electrons and the preferred structure carries zero formal charge on the central atom.
The S angle is about ≈90° / 120°. Lone-pair repulsion compresses the angle from the ideal trigonal bipyramidal value.
The conventional model is sp3d. Sulfur tetrachloride has 5 electron domains around the central S.
The CAS number is 13451-08-6. PubChem (CID 13932016) and NIST identify this with Cl4S; 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 13451-08-6 identifies the substance, not a universal purity specification.
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