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The Difluoroborane Lewis structure is B–F single bond, B–F single bond and B–H single bond; the central B has 3 electron domains (0 lone pairs), giving a trigonal planar electron-domain arrangement and a trigonal planar molecular geometry with a 120° bond angle. B is best described as sp2-hybridized, and Difluoroborane is polar because the trigonal planar shape (and/or unequal terminal atoms) prevents cancellation of the bond dipoles.
Figure 1: Lewis Structure of Difluoroborane (BF2H)
| Chemical Formula | BF2H |
| CAS Number | 13535-16-5 |
| Total Valence Electrons | 18 |
| Lewis Structure | B–F single bond, B–F single bond and B–H single bond |
| Electron-Domain Geometry | trigonal planar |
| Molecular Geometry | trigonal planar |
| Hybridization Model | sp2 (central B) |
| Bond Angle | 120° |
| Polarity | Polar molecule |
As a hydride of B, Difluoroborane is typically a strong reducing agent, a potential fuel component, or a precursor in inorganic and organometallic synthesis. Many pnictogen/sulfur hydrides are toxic, foul-smelling and pyrophoric or flammable, and are handled with appropriate ventilation and inert-atmosphere technique.
To draw the Difluoroborane Lewis structure we first count the total valence electrons. BF2H contains 3 (B) + 2×7 (F) + 1 (H); the net charge of 0 gives a total of 18 valence electrons to place.
The central atom is B. 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 (B) + 2×7 (F) + 1 (H) = 18 electrons.
Place B 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: B–F single bond, B–F single bond and B–H single bond; no lone pairs on B.
Counting bonding and nonbonding electrons around B therefore satisfies the octet/expanded-octet requirement for the drawn structure.
VSEPR theory states that the 3 electron domains around B arrange to minimize mutual repulsion, giving an trigonal planar 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 trigonal planar; the B bond angle is set to 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 0 lone pair(s) on B, 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, B uses sp2 hybrid orbitals to form the 3 equivalent electron-domain directions (3 bonding + 0 lone pair).
Formal charge on central B = V − N − ½B = 3 − 0 − ½×6 = 1. The nonzero formal charge is distributed by resonance / charge separation; the drawn structure is the lowest-energy contributor.
Difluoroborane is polar. The trigonal planar 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 Difluoroborane the trigonal planar 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 |
|---|---|---|---|---|---|
| Difluoroborane | BF2H | B | 3 | trigonal planar | Polar |
| Boron trifluoride | BF3 | B | 3 | trigonal planar | Nonpolar |
| Boron trichloride | BCl3 | B | 3 | trigonal planar | Nonpolar |
| Diborane | B2H6 | B | 3 | trigonal planar | Polar |
Difluoroborane is polar. Its trigonal planar geometry (and/or unequal terminal atoms) stops the bond dipoles from cancelling.
B–F single bond, B–F single bond and B–H single bond; no lone pairs on B. It uses all 18 valence electrons and the preferred structure carries a formal charge of 1 on the central atom.
The B angle is about 120°. Lone-pair repulsion compresses the angle from the ideal trigonal planar value.
The conventional model is sp2. Difluoroborane has 3 electron domains around the central B.
The CAS number is 13535-16-5. PubChem (CID 139565) and NIST identify this with BF2H; 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 13535-16-5 identifies the substance, not a universal purity specification.
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