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Is the CNO- ion polar?

Jun 4,2026

Yes, the CNO? (fulminate ion) is polar. The fulminate ion (CNO?) is a reactive triatomic polyatomic anion, widely studied in general chemistry due to its diverse resonance structures and unstable bonding characteristics. As an isomer of the stable cyanate ion (NCO?), CNO? has different atomic numbers, unique electron distributions, and higher chemical reactivity.

cno lewis structure

1. Calculation of Total Valence Electrons

The first step in constructing the Lewis structure of CNO? is to calculate the total number of valence electrons. Carbon belongs to Group 14 and has 4 valence electrons; nitrogen belongs to Group 15 and has 5 valence electrons; oxygen belongs to Group 16 and has 6 valence electrons. As a negatively charged anion, CNO? gains an additional valence electron.

The total number of valence electrons in CNO? is calculated to be 4 + 5 + 6 + 1 = 16. This number is the same as that in NCO?, allowing for various double and triple bond combinations and several effective resonance structures with different energy levels.

2. Drawing the Lewis Structure of CNO?

2.1 Atomic Skeleton Confirmation

Unlike the N-C-O sequence of cyanate ions, fulminate ions follow a fixed C-N-O atomic chain. Carbon is at the terminal position, nitrogen is the central atom, and oxygen occupies the other terminal position. This C-N-O skeleton remains unchanged in all resonance structures, which is a fundamental rule for the delocalization of effective electrons.

2.2 Bonding and Lone Pair Electron Arrangement

The central nitrogen atom connects carbon and oxygen through different combinations of single, triple, or double bonds. All atoms strictly follow the octet rule, achieved by adjusting the number of bonding electrons and lone pairs. The outer electrons of the terminal carbon and oxygen atoms are filled with lone pairs, while the central nitrogen atom retains eight surrounding electrons through covalent bonds. No atom is in an extended octet or electron-deficient state.

3. Resonance Structures of the CNO? Ion

The CNO? ion has three effective resonance structures, with significantly different stability, including one relatively stable form and two high-energy unstable forms. Unlike the equivalent resonances of ozone and formate ions, the resonance structures of CNO? are not identical, and their contributions to the actual hybridization structure also differ.

The most stable resonance structure contains a carbon-nitrogen triple bond and a nitrogen-oxygen single bond. In this structure, the formal charge is relatively minimized. The second and third resonance structures have double bonds on both sides, or a triple bond on the nitrogen-oxygen side. These structures lead to severe charge separation and an unreasonable charge distribution, resulting in higher molecular energies.

4. Molecular Geometry and Polarity

According to the Valence Shell Electron Pair Repulsion (VSEPR) theory, the central nitrogen atom has two bonding domains and no lone pairs of electrons. Therefore, the CNO? ion exhibits a linear molecular geometry with bond angles of 180°. Although the CNO? ion has a linear geometry, the atoms at its two ends are different (C and O), resulting in an uneven electron distribution and a net dipole moment. Therefore, it is polar.

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