Nitric oxide Lewis Structure

Nitric oxide Lewis Structure: NO Lewis Structure, linear (diatomic) Geometry, sp2 Hybridization & Polarity

Nitric oxide Key Facts

The Nitric oxide Lewis structure is a linear diatomic with a polar bond between its two atoms; because the two atoms differ in electronegativity, Nitric oxide is polar.

Figure 1: Lewis Structure of Nitric oxide (NO)

Chemical Formula	NO
CAS Number	10102-43-9
Total Valence Electrons	11
Lewis Structure	linear diatomic molecule with one double bond and a lone pair on each atom
Electron-Domain Geometry	linear
Molecular Geometry	linear (diatomic)
Hybridization Model	sp2
Bond Angle	180°
Polarity	Polar molecule

PubChem (CID 145068) and NIST list Nitric oxide as NO with CAS 10102-43-9; molecular weight ≈ 30.006 g/mol. View CAS 10102-43-9 dictionary details on Guidechem →

Applications of Nitric oxide (CAS 10102-43-9)

The N oxide Nitric oxide 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.

Acid Anhydride / Intermediate Gateway to the corresponding oxoacid and its salts (fertilizers, detergents).

Materials & Catalysis Oxide ceramics, refractories, catalysts and pigment feedstocks.

Process Gas / Reagent Oxidizing or reactive reagent in inorganic and environmental processing.

Procurement Note "Nitric oxide" is supplied in multiple commercial grades and package sizes. Specify purity, grade, moisture/impurity limits, package (cylinder, drum or bulk) and intended process, and use CAS 10102-43-9 as the primary identifier when screening suppliers; always confirm regional availability and safety documentation (SDS).

Step 1 - Valence Electrons & Central Atom

To draw the Nitric oxide Lewis structure we first count the total valence electrons. NO contains 5 (N) + 6 (O); the net charge of 0 gives a total of 11 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).

Valence-electron count

Total valence electrons = 5 (N) + 6 (O) = 11 electrons.

Step 2 - Lewis Structure & Electron Distribution

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: linear diatomic molecule with one double bond and a lone pair on each atom.

Counting bonding and nonbonding electrons around N therefore satisfies the octet/expanded-octet requirement for the drawn structure.

N–O

N: 1 lone pair, 1 bonding domain

1 bonding domains + 1 lone pairs = 3 electron domains

Octet & Diradical Note In a simple Lewis drawing each atom of this homonuclear diatomic carries lone pairs; species such as O₂ are more accurately described by molecular-orbital theory (paramagnetism arises from unpaired electrons in π* orbitals).

Step 3 - VSEPR Theory & Geometry

VSEPR theory states that the 3 electron domains around N arrange to minimize mutual repulsion, giving an linear 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 linear (diatomic); the N bond angle is set to 180° rather than the ideal value for the electron-domain geometry.

Repulsion hierarchy

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.

Hybridization & Formal Charge

In the conventional localized-bond model, N uses sp2 hybrid orbitals to form the 3 equivalent electron-domain directions (1 bonding + 1 lone pair).

Formal-charge check

Formal charge on central N = V − N − ½B = 5 − 2 − ½×4 = 1. The nonzero formal charge is distributed by resonance / charge separation; the drawn structure is the lowest-energy contributor.

Modeling Note Modeling Note: sp2 is a compact model for the 3 electron-domain directions around N; full quantum-chemical treatments use molecular orbitals.

Is Nitric oxide Polar or Nonpolar?

Nitric oxide is polar. The linear (diatomic) 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.

Expert Quote — Structural Chemistry Perspective

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 Nitric oxide the linear (diatomic) 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.

Structural Comparison Table

Species	Formula	Central Atom	Electron Domains	Molecular Geometry	Polarity
Nitric oxide	NO	N	3	linear (diatomic)	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
Nitrogen dioxide	NO₂	N	3	bent	Polar

Practice question Starting from the 11 valence electrons of NO, draw the Lewis structure and confirm the central N atom is sp2-hybridized with linear (diatomic) geometry. What happens to the bond angle if one terminal atom is replaced by a more electronegative substituent?

Looking for industrial bulk or specified-grade supplies of Nitric oxide (CAS 10102-43-9)? Browse Supplier on Guidechem →

FAQs

Is NO polar or nonpolar?

Nitric oxide is polar. Its linear (diatomic) geometry (and/or unequal terminal atoms) stops the bond dipoles from cancelling.

What is the Lewis structure of Nitric oxide?

linear diatomic molecule with one double bond and a lone pair on each atom. It uses all 11 valence electrons and the preferred structure carries a formal charge of 1 on the central atom.

What is the bond angle in Nitric oxide?

The N angle is about 180°. Lone-pair repulsion compresses the angle from the ideal linear value.

What is the hybridization of N in Nitric oxide?

The conventional model is sp2. Nitric oxide has 3 electron domains around the central N.

What is the CAS number of Nitric oxide?

The CAS number is 10102-43-9. PubChem (CID 145068) and NIST identify this with NO; use it to locate suppliers and database records.

References

PubChem CID 145068, Nitric oxide. Molecular formula, CAS number, molecular weight and chemical identity.
NIST Chemistry WebBook, SRD 69, Nitric oxide. Formula, CAS Registry Number and thermochemical / spectroscopic data.
IUPAC Gold Book. Definitions for "lone pair", "VSEPR", "hybridization" and "formal charge".
Atkins, P. & de Paula, J., Physical Chemistry. VSEPR, molecular geometry and dipole moments.
Guidechem supplier & dictionary records. Commercial sourcing and CAS-linked property pages for Nitric oxide (CAS 10102-43-9).

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 10102-43-9 identifies the substance, not a universal purity specification.

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Nitric oxide Lewis Structure