CHFO, also named formyl fluoride, is a small polar covalent molecule widely studied in structural chemistry and organic synthesis. Its molecular structure follows fundamental covalent bonding rules, including the octet rule and valence electron conservation. The accurate Lewis structure of CHFO is the basis for analyzing its molecular geometry, hybridization state, charge distribution and chemical reactivity. Unlike complex organic molecules, CHFO has a simple atomic composition with one carbon, one hydrogen, one fluorine and one oxygen atom, forming a stable carbonyl-containing structure.

1. Valence Electron Calculation

The construction of the CHFO Lewis structure starts with total valence electron counting. Each atom contributes fixed valence electrons: carbon provides 4 valence electrons, hydrogen provides 1 valence electron, fluorine provides 7 valence electrons, and oxygen provides 6 valence electrons. The total number of valence electrons in one CHFO molecule is 18. Hydrogen only forms one single bond without lone pairs, while fluorine and oxygen retain non-bonding lone pairs to satisfy electron saturation.

2. Construction of CHFO Lewis Structure

Carbon acts as the central atom of CHFO due to its higher bonding capacity and lower electronegativity compared with oxygen and fluorine. The central carbon forms three covalent bonds: one single bond with hydrogen, one single bond with fluorine, and one double bond with oxygen. In this structure, all atoms satisfy the octet rule except hydrogen, which meets the duet rule. Fluorine carries three lone electron pairs, and oxygen carries two lone electron pairs, with no residual valence electrons in the molecule.

3. Formal Charge Distribution

Formal charge evaluation verifies the rationality of the CHFO Lewis structure. The formal charge of hydrogen, central carbon, oxygen and fluorine is all zero. A structure with zero formal charges on all atoms is the most stable and dominant configuration of CHFO. No resonance structures exist for CHFO, as any bond rearrangement will generate non-zero formal charges and break the octet balance of atoms.

4. Molecular Geometry and Hybridization

Based on VSEPR theory, the central carbon atom of CHFO has three bonding electron groups and no lone electron pairs, corresponding to sp2 hybridization. The electron pair geometry and molecular geometry are both trigonal planar with a planar molecular framework. The C? point group symmetry is confirmed by its planar structure. The unequal electronegativity of oxygen and fluorine creates a permanent dipole moment, making CHFO a polar molecule with distinct chemical reactivity in acyl transfer reactions.