Copper(II) oxide Lewis Structure

Copper(II) oxide Lewis Structure: CuO Lewis Structure, linear (diatomic) Geometry, sp3d Hybridization & Polarity

Copper(II) oxide Key Facts

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

Figure 1: Lewis Structure of Copper(II) oxide (CuO)

Chemical Formula	CuO
CAS Number	1317-38-0
Total Valence Electrons	6
Lewis Structure	linear diatomic molecule with one single bond
Electron-Domain Geometry	linear
Molecular Geometry	linear (diatomic)
Hybridization Model	sp3d
Bond Angle	180°
Polarity	Polar molecule

PubChem (CID 164827) and NIST list Copper(II) oxide as CuO with CAS 1317-38-0; molecular weight ≈ 79.55 g/mol. View CAS 1317-38-0 dictionary details on Guidechem →

Applications of Copper(II) oxide (CAS 1317-38-0)

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) 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 1317-38-0 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) oxide Lewis structure we first count the total valence electrons. CuO contains 6 (O); the net charge of 0 gives a total of 6 valence electrons to place.

The central atom is O. 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 = 6 (O) = 6 electrons.

Step 2 - Lewis Structure & Electron Distribution

Place O 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 single bond; 3 lone pair(s) on O.

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

O–X

O: 3 lone pairs, 1 bonding domain

1 bonding domains + 3 lone pairs = 5 electron domains

Expanded Octet: d-Orbital Participation Central O belongs to period 3 or below, so it can accommodate more than eight electrons: low-lying d orbitals become available and the linear (diatomic) arrangement with 5 domains reflects this expanded valence shell. The octet rule alone does not apply to such hypervalent species.

Step 3 - VSEPR Theory & Geometry

VSEPR theory states that the 5 electron domains around O arrange to minimize mutual repulsion, giving an linear electron-domain geometry.

Because 3 of these domains are lone pair(s) — and lone pairs repel more strongly than bonding pairs — the observed molecular geometry is linear (diatomic); the O 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 3 lone pair(s) on O, 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, O uses sp3d hybrid orbitals to form the 5 equivalent electron-domain directions (1 bonding + 3 lone pair).

Formal-charge check

Formal charge on central O = V − N − ½B = 6 − 6 − ½×2 = -1. The nonzero formal charge is distributed by resonance / charge separation; the drawn structure is the lowest-energy contributor.

Modeling Note Modeling Note: sp3d / sp3d hybridization is a convenient localized-bond teaching model. Modern quantum-chemical descriptions of hypervalent Copper(II) oxide use molecular orbitals and do not require populated d orbitals as the primary bonding picture.

Is Copper(II) oxide Polar or Nonpolar?

Copper(II) 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 Copper(II) 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
Copper(II) oxide	CuO	O	5	linear (diatomic)	Polar
Water	H₂O	O	4	bent	Polar
Hydrogen peroxide	H₂O₂	O	4	bent	Polar
Ozone	O₃	O	3	bent	Polar
Hydronium	H₃O	O	4	trigonal pyramidal	Polar
Hypochlorite	ClO	O	4	linear (diatomic)	Polar

Practice question Starting from the 6 valence electrons of CuO, draw the Lewis structure and confirm the central O atom is sp3d-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 Copper(II) oxide (CAS 1317-38-0)? Browse Supplier on Guidechem →

FAQs

Is CuO polar or nonpolar?

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

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

linear diatomic molecule with one single bond; 3 lone pair(s) on O. It uses all 6 valence electrons and the preferred structure carries a formal charge of -1 on the central atom.

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

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

What is the hybridization of O in Copper(II) oxide?

The conventional model is sp3d. Copper(II) oxide has 5 electron domains around the central O.

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

The CAS number is 1317-38-0. PubChem (CID 164827) and NIST identify this with CuO; use it to locate suppliers and database records.

References

PubChem CID 164827, Copper(II) oxide. Molecular formula, CAS number, molecular weight and chemical identity.
NIST Chemistry WebBook, SRD 69, Copper(II) 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 Copper(II) oxide (CAS 1317-38-0).

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 1317-38-0 identifies the substance, not a universal purity specification.

Make Guideview Preferred Source on Google

Copper(II) oxide Lewis Structure