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The Chlorine difluoride anion Lewis structure is Cl–F single bond and Cl–F single bond; the central Cl has 4 electron domains (2 lone pairs), giving a tetrahedral electron-domain arrangement and a bent molecular geometry with a ≈104.5° bond angle. Cl is best described as sp3-hybridized, and Chlorine difluoride anion is polar because the bent shape (and/or unequal terminal atoms) prevents cancellation of the bond dipoles.
Figure 1: Lewis Structure of Chlorine difluoride anion (ClF2)
| Chemical Formula | ClF2 |
| CAS Number | 13191-03-2 |
| Net Charge | -1 |
| Total Valence Electrons | 22 |
| Lewis Structure | Cl–F single bond and Cl–F single bond |
| Electron-Domain Geometry | tetrahedral |
| Molecular Geometry | bent |
| Hybridization Model | sp3 (central Cl) |
| Bond Angle | ≈104.5° |
| Polarity | Polar molecule |
In aqueous and process chemistry, ClF2 exists as the anion Chlorine difluoride anion ion. It is encountered as a counterion and a controlled source of Cl in salts, buffers, electrochemistry and analytical protocols, and as a reactant in syntheses that require a defined equivalent of Cl-containing material.
To draw the Chlorine difluoride anion Lewis structure we first count the total valence electrons. ClF2 contains 7 (Cl) + 2×7 (F) − 1 (net anion); the net charge of -1 gives a total of 22 valence electrons to place.
The central atom is Cl. 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 = 7 (Cl) + 2×7 (F) − 1 (net anion) = 22 electrons.
Place Cl 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: Cl–F single bond and Cl–F single bond; 2 lone pairs on Cl.
Counting bonding and nonbonding electrons around Cl therefore satisfies the octet/expanded-octet requirement for the drawn structure.
VSEPR theory states that the 4 electron domains around Cl arrange to minimize mutual repulsion, giving an tetrahedral 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 bent; the Cl bond angle is set to ≈104.5° 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 2 lone pair(s) on Cl, 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, Cl uses sp3 hybrid orbitals to form the 4 equivalent electron-domain directions (2 bonding + 2 lone pair).
Formal charge on central Cl = V − N − ½B = 7 − 4 − ½×4 = 1. The nonzero formal charge is distributed by resonance / charge separation; the drawn structure is the lowest-energy contributor.
Chlorine difluoride anion is polar. The bent 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 Chlorine difluoride anion the bent 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 |
|---|---|---|---|---|---|
| Chlorine difluoride anion | ClF2 | Cl | 4 | bent | Polar |
| Hydrogen chloride | HCl | Cl | 4 | linear (diatomic) | Polar |
| Chlorine | Cl2 | Cl | 4 | linear (diatomic) | Nonpolar |
| Chlorine trifluoride | ClF3 | Cl | 5 | T-shaped | Polar |
| Chlorine pentafluoride | ClF5 | Cl | 6 | square pyramidal | Polar |
| Chlorate | ClO3 | Cl | 4 | trigonal pyramidal | Polar |
Chlorine difluoride anion is polar. Its bent geometry (and/or unequal terminal atoms) stops the bond dipoles from cancelling.
Cl–F single bond and Cl–F single bond; 2 lone pairs on Cl. It uses all 22 valence electrons and the preferred structure carries a formal charge of 1 on the central atom.
The Cl angle is about ≈104.5°. Lone-pair repulsion compresses the angle from the ideal tetrahedral value.
The conventional model is sp3. Chlorine difluoride anion has 4 electron domains around the central Cl.
The CAS number is 13191-03-2. PubChem and NIST identify this with ClF2; 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 13191-03-2 identifies the substance, not a universal purity specification.
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