Copper(II) nitrate Lewis Structure

Copper(II) nitrate Lewis Structure: CuN₂O₆ Lewis Structure, trigonal planar Geometry, sp2 Hybridization & Polarity

Copper(II) nitrate Key Facts

The Copper(II) nitrate Lewis structure is N–O double bond, N–O single bond and N–O single bond; the central N has 3 electron domains (0 lone pairs), giving a trigonal planar electron-domain arrangement and a trigonal planar molecular geometry with a 120° bond angle. N is best described as sp2-hybridized, and Copper(II) nitrate is nonpolar because the bond dipoles cancel by molecular symmetry.

Figure 1: Lewis Structure of Copper(II) nitrate (CuN₂O₆)

Chemical Formula	CuN₂O₆
CAS Number	3251-23-8
Total Valence Electrons	46
Lewis Structure	N–O double bond, N–O single bond and N–O single bond
Electron-Domain Geometry	trigonal planar
Molecular Geometry	trigonal planar
Hybridization Model	sp2 (central N)
Bond Angle	120°
Polarity	Nonpolar molecule

PubChem (CID 18616) and NIST list Copper(II) nitrate as CuN ₂O ₆ with CAS 3251-23-8; molecular weight ≈ 187.56 g/mol. View CAS 3251-23-8 dictionary details on Guidechem →

Applications of Copper(II) nitrate (CAS 3251-23-8)

This organic compound is used as a solvent, intermediate or specialty reagent in fine-chemical, pharmaceutical and materials synthesis; specify grade and impurity profile when sourcing.

Solvent / Reagent Medium for reactions, extraction or formulation.

Intermediate Building block for downstream derivatives.

Specialty Use Targeted role in pharma/fragrance/materials.

Procurement Note "Copper(II) nitrate" 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 3251-23-8 as the primary identifier when screening suppliers; always confirm regional availability and safety documentation (SDS).

Step 1 - Valence Electrons & Central Atom

To draw the Copper(II) nitrate Lewis structure we first count the total valence electrons. CuN₂O₆ contains 2×5 (N) + 6×6 (O); the net charge of 0 gives a total of 46 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 = 2×5 (N) + 6×6 (O) = 46 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: N–O double bond, N–O single bond and N–O single bond; no lone pairs on N.

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

This species is best represented by resonance structures; the π bonding is delocalized over the equivalent terminal atom(s), so all N–terminals bonds are equivalent in the resonance hybrid.

N=O N–O N–O

N: 0 lone pairs, 3 bonding domains

3 bonding domains + 0 lone pairs = 3 electron domains

Octet Rule: Why N Has Eight Electrons N forms 3 bond(s) and retains 0 nonbonding electron(s), reaching an octet. No expanded octet is required for this second-row (or octet-satisfying) central atom.

Step 3 - VSEPR Theory & Geometry

VSEPR theory states that the 3 electron domains around N arrange to minimize mutual repulsion, giving an trigonal planar electron-domain geometry.

Because 0 of these domains are lone pair(s) — and lone pairs repel more strongly than bonding pairs — the observed molecular geometry is trigonal planar; the N bond angle is set to 120° 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 0 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 (3 bonding + 0 lone pair).

Formal-charge check

Formal charge on central N = V − N − ½B = 5 − 0 − ½×8 = 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 Copper(II) nitrate Polar or Nonpolar?

Copper(II) nitrate is nonpolar. Although individual N–terminal bonds are polar when the atoms differ in electronegativity, the trigonal planar geometry makes their vector sum zero, so there is no net molecular dipole.

Expert Quote — Structural Chemistry Perspective

A common misconception is that polar bonds guarantee a polar molecule. Copper(II) nitrate shows the opposite: identical bond dipoles arranged with trigonal planar symmetry cancel exactly, yielding a nonpolar species.

Interpretation consistent with standard VSEPR / molecular-geometry references.

Its nonpolar character governs solvation and intermolecular behavior; specify grade and handling when sourcing.

Structural Comparison Table

Species	Formula	Central Atom	Electron Domains	Molecular Geometry	Polarity
Copper(II) nitrate	CuN₂O₆	N	3	trigonal planar	Nonpolar
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
Nitric oxide	NO	N	3	linear (diatomic)	Polar

Practice question Starting from the 46 valence electrons of CuN₂O₆, draw the Lewis structure and confirm the central N atom is sp2-hybridized with trigonal planar 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 Copper(II) nitrate (CAS 3251-23-8)? Browse Supplier on Guidechem →

FAQs

Is CuN₂O₆ polar or nonpolar?

Copper(II) nitrate is nonpolar. Its trigonal planar symmetry cancels the bond dipoles exactly.

What is the Lewis structure of Copper(II) nitrate?

N–O double bond, N–O single bond and N–O single bond; no lone pairs on N. It uses all 46 valence electrons and the preferred structure carries a formal charge of 1 on the central atom.

What is the bond angle in Copper(II) nitrate?

The N angle is about 120°. Lone-pair repulsion compresses the angle from the ideal trigonal planar value.

What is the hybridization of N in Copper(II) nitrate?

The conventional model is sp2. Copper(II) nitrate has 3 electron domains around the central N.

What is the CAS number of Copper(II) nitrate?

The CAS number is 3251-23-8. PubChem (CID 18616) and NIST identify this with CuN₂O₆; use it to locate suppliers and database records.

References

PubChem CID 18616, Copper(II) nitrate. Molecular formula, CAS number, molecular weight and chemical identity.
NIST Chemistry WebBook, SRD 69, Copper(II) nitrate. 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 Copper(II) nitrate (CAS 3251-23-8).

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 3251-23-8 identifies the substance, not a universal purity specification.

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Copper(II) nitrate Lewis Structure