-
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 Thiosulfate ion Lewis structure is S–O single bond, S–O double bond, S–S double bond and S–O single bond; the central S has 4 electron domains (0 lone pairs), giving a tetrahedral electron-domain arrangement and a tetrahedral molecular geometry with a 109.5° bond angle. S is best described as sp3-hybridized, and Thiosulfate ion is polar because the tetrahedral shape (and/or unequal terminal atoms) prevents cancellation of the bond dipoles.
Figure 1: Lewis Structure of Thiosulfate ion (O3S2-2)
| Chemical Formula | O3S2-2 |
| CAS Number | 14383-50-7 |
| Net Charge | -2 |
| Total Valence Electrons | 32 |
| Lewis Structure | S–O single bond, S–O double bond, S–S double bond and S–O single bond |
| Electron-Domain Geometry | tetrahedral |
| Molecular Geometry | tetrahedral |
| Hybridization Model | sp3 (central S) |
| Bond Angle | 109.5° |
| Polarity | Polar molecule |
In aqueous and process chemistry, O3S2-2 exists as the anion Thiosulfate ion ion. It is encountered as a counterion and a controlled source of S in salts, buffers, electrochemistry and analytical protocols, and as a reactant in syntheses that require a defined equivalent of S-containing material.
To draw the Thiosulfate ion Lewis structure we first count the total valence electrons. O3S2-2 contains 3×6 (O) + 2×6 (S) − 2 (net anion); the net charge of -2 gives a total of 32 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 = 3×6 (O) + 2×6 (S) − 2 (net anion) = 32 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–O single bond, S–O double bond, S–S double bond and S–O single bond; no lone pairs 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 4 electron domains around S arrange to minimize mutual repulsion, giving an tetrahedral electron-domain geometry.
Because 0 of these domains are lone pair(s) — and lone pairs repel more strongly than bonding pairs — the observed molecular geometry is tetrahedral; the S bond angle is set to 109.5° 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 0 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 sp3 hybrid orbitals to form the 4 equivalent electron-domain directions (4 bonding + 0 lone pair).
Formal charge on central S = V − N − ½B = 6 − 0 − 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.
Thiosulfate ion is polar. The tetrahedral 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 Thiosulfate ion the tetrahedral 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 |
|---|---|---|---|---|---|
| Thiosulfate ion | O3S2-2 | S | 4 | tetrahedral | 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 |
Thiosulfate ion is polar. Its tetrahedral geometry (and/or unequal terminal atoms) stops the bond dipoles from cancelling.
S–O single bond, S–O double bond, S–S double bond and S–O single bond; no lone pairs on S. It uses all 32 valence electrons and the preferred structure carries zero formal charge on the central atom.
The S angle is about 109.5°. Lone-pair repulsion compresses the angle from the ideal tetrahedral value.
The conventional model is sp3. Thiosulfate ion has 4 electron domains around the central S.
The CAS number is 14383-50-7. PubChem (CID 1084) and NIST identify this with O3S2-2; 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 14383-50-7 identifies the substance, not a universal purity specification.
 |
|
 |
EN
Agricultural News
Food News
Industrial News
Cosmetic News
Pharmaceutical News
Science News
