-
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 Nitrosyl fluoride Lewis structure is N–O double bond and N–F single bond; the central N has 3 electron domains (1 lone pair), giving a trigonal planar electron-domain arrangement and a bent molecular geometry with a ≈119° bond angle. N is best described as sp2-hybridized, and Nitrosyl fluoride is polar because the bent shape (and/or unequal terminal atoms) prevents cancellation of the bond dipoles.
Figure 1: Lewis Structure of Nitrosyl fluoride (FNO)
| Chemical Formula | FNO |
| CAS Number | 7789-25-5 |
| Total Valence Electrons | 18 |
| Lewis Structure | N–O double bond and N–F single bond |
| Electron-Domain Geometry | trigonal planar |
| Molecular Geometry | bent |
| Hybridization Model | sp2 (central N) |
| Bond Angle | ≈119° |
| Polarity | Polar molecule |
The N oxide Nitrosyl fluoride is a key industrial intermediate. Nonmetal oxides such as SO3 and P4O10 are acid anhydrides for sulfuric and phosphoric acid manufacture, while metal/semimetal oxides are ceramics, refractories, catalysts and pigment precursors.
To draw the Nitrosyl fluoride Lewis structure we first count the total valence electrons. FNO contains 7 (F) + 5 (N) + 6 (O); the net charge of 0 gives a total of 18 valence electrons to place.
The central atom is N. 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 (F) + 5 (N) + 6 (O) = 18 electrons.
Place N 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: N–O double bond and N–F single bond; one lone pair on N.
Counting bonding and nonbonding electrons around N therefore satisfies the octet/expanded-octet requirement for the drawn structure.
VSEPR theory states that the 3 electron domains around N arrange to minimize mutual repulsion, giving an trigonal planar 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 bent; the N bond angle is set to ≈119° 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 N, 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, N uses sp2 hybrid orbitals to form the 3 equivalent electron-domain directions (2 bonding + 1 lone pair).
Formal charge on central N = V − N − ½B = 5 − 2 − ½×6 = 0. The preferred Lewis structure carries zero formal charge on the central atom (and on the terminals), so it is the dominant contributor.
Nitrosyl fluoride 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 Nitrosyl fluoride 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 |
|---|---|---|---|---|---|
| Nitrosyl fluoride | FNO | N | 3 | bent | Polar |
| Ammonia | H3N | N | 4 | trigonal pyramidal | Polar |
| Ammonium | H4N | N | 4 | tetrahedral | Nonpolar |
| Hydrazine | H4N2 | N | 4 | trigonal pyramidal | Polar |
| Nitrogen | N2 | N | 2 | linear (diatomic) | Nonpolar |
| Nitric oxide | NO | N | 3 | linear (diatomic) | Polar |
Nitrosyl fluoride is polar. Its bent geometry (and/or unequal terminal atoms) stops the bond dipoles from cancelling.
N–O double bond and N–F single bond; one lone pair on N. It uses all 18 valence electrons and the preferred structure carries zero formal charge on the central atom.
The N angle is about ≈119°. Lone-pair repulsion compresses the angle from the ideal trigonal planar value.
The conventional model is sp2. Nitrosyl fluoride has 3 electron domains around the central N.
The CAS number is 7789-25-5. PubChem (CID 123261) and NIST identify this with FNO; 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 7789-25-5 identifies the substance, not a universal purity specification.
 |
|
 |
EN
Agricultural News
Food News
Industrial News
Cosmetic News
Pharmaceutical News
Science News
