Resonance Structures Calculator

Analyze resonance structures, calculate average bond order, and understand electron delocalization.

Molecule Structure

Select Molecule Preset

Central Atom

Number of Equivalent Terminal Atoms

Number of Double Bonds (in one structure)

Total Charge

Number of Resonance Structures

equivalent contributing structures

Average Bond Order

1.67

Equivalent Bonds?

Yes

Double Bond Character

33.3%

Single Bond Character

66.7%

Resonance Stabilization

High (extensive delocalization)

Resonance Hybrid Description

Each N-O bond has 33.3% double bond character

Understanding Resonance

Resonance occurs when a molecule can be represented by two or more valid Lewis structures that differ only in the placement of electrons. The actual molecule is a resonance hybrid - an average of all contributing structures. Resonance leads to electron delocalization, which increases stability. The more equivalent resonance structures a molecule has, the more stable it is. Bond lengths in resonance hybrids are intermediate between single and double bond lengths.

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