no2 - lewis structure and vsepr model illustrate how a simple diatomic oxide displays resonance, a bent geometry, and electron‑pair repulsion that can be predicted using VSEPR theory, making it a cornerstone example for students learning about molecular shape and bonding Easy to understand, harder to ignore..
Introduction
The nitric oxide radical (NO₂) is frequently encountered in atmospheric chemistry, combustion processes, and industrial synthesis. Its Lewis structure reveals an odd electron, while the VSEPR model explains the observed bent shape with a bond angle of approximately 134°. Understanding both the electron‑dot representation and the spatial arrangement of electron pairs provides insight into the molecule’s reactivity, polarity, and spectroscopic properties. This article walks through the step‑by‑step construction of the NO₂ Lewis diagram, interprets the resulting geometry with VSEPR, and answers common questions that arise when applying these concepts.
Steps
- Count valence electrons – Nitrogen contributes 5 electrons, each oxygen contributes 6, and the extra electron for the radical adds 1, giving a total of 5 + (2 × 6) + 1 = 18 electrons.
- Place the central atom – Position nitrogen as the central atom and single‑bond it to each oxygen.
- Distribute remaining electrons – Fill the outer octets of the oxygens first, then place any leftover electrons on the central atom.
- **Form multiple
