-
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 Trichlorostannate ion Lewis structure is Sn–Cl single bond, Sn–Cl single bond and Sn–Cl single bond; the central Sn has 4 electron domains (1 lone pair), giving a tetrahedral electron-domain arrangement and a trigonal pyramidal molecular geometry with a ≈107° bond angle. Sn is best described as sp3-hybridized, and Trichlorostannate ion is polar because the trigonal pyramidal shape (and/or unequal terminal atoms) prevents cancellation of the bond dipoles.
Figure 1: Lewis Structure of Trichlorostannate ion (Cl3Sn)
| Chemical Formula | Cl3Sn |
| CAS Number | 15529-74-5 |
| Net Charge | -1 |
| Total Valence Electrons | 26 |
| Lewis Structure | Sn–Cl single bond, Sn–Cl single bond and Sn–Cl single bond |
| Electron-Domain Geometry | tetrahedral |
| Molecular Geometry | trigonal pyramidal |
| Hybridization Model | sp3 (central Sn) |
| Bond Angle | ≈107° |
| Polarity | Polar molecule |
In aqueous and process chemistry, Cl3Sn exists as the anion Trichlorostannate ion ion. It is encountered as a counterion and a controlled source of Sn in salts, buffers, electrochemistry and analytical protocols, and as a reactant in syntheses that require a defined equivalent of Sn-containing material.
To draw the Trichlorostannate ion Lewis structure we first count the total valence electrons. Cl3Sn contains 3×7 (Cl) + 4 (Sn) − 1 (net anion); the net charge of -1 gives a total of 26 valence electrons to place.
The central atom is Sn. 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 = 3×7 (Cl) + 4 (Sn) − 1 (net anion) = 26 electrons.
Place Sn 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: Sn–Cl single bond, Sn–Cl single bond and Sn–Cl single bond; one lone pair on Sn.
Counting bonding and nonbonding electrons around Sn therefore satisfies the octet/expanded-octet requirement for the drawn structure.
VSEPR theory states that the 4 electron domains around Sn arrange to minimize mutual repulsion, giving an tetrahedral 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 trigonal pyramidal; the Sn bond angle is set to ≈107° 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 Sn, 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, Sn uses sp3 hybrid orbitals to form the 4 equivalent electron-domain directions (3 bonding + 1 lone pair).
Formal charge on central Sn = V − N − ½B = 4 − 2 − ½×6 = -1. The nonzero formal charge is distributed by resonance / charge separation; the drawn structure is the lowest-energy contributor.
Trichlorostannate ion is polar. The trigonal pyramidal 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 Trichlorostannate ion the trigonal pyramidal 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 |
|---|---|---|---|---|---|
| Trichlorostannate ion | Cl3Sn | Sn | 4 | trigonal pyramidal | Polar |
| Carbon dioxide | CO2 | C | 2 | linear | Nonpolar |
| Carbon monoxide | CO | C | 2 | linear (diatomic) | Polar |
| Carbon disulfide | CS2 | C | 2 | linear | Nonpolar |
Trichlorostannate ion is polar. Its trigonal pyramidal geometry (and/or unequal terminal atoms) stops the bond dipoles from cancelling.
Sn–Cl single bond, Sn–Cl single bond and Sn–Cl single bond; one lone pair on Sn. It uses all 26 valence electrons and the preferred structure carries a formal charge of -1 on the central atom.
The Sn angle is about ≈107°. Lone-pair repulsion compresses the angle from the ideal tetrahedral value.
The conventional model is sp3. Trichlorostannate ion has 4 electron domains around the central Sn.
The CAS number is 15529-74-5. PubChem and NIST identify this with Cl3Sn; 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 15529-74-5 identifies the substance, not a universal purity specification.
 |
|
EN
Agricultural News
Food News
Industrial News
Cosmetic News
Pharmaceutical News
Science News
