Carbon suboxide Lewis Structure

Carbon suboxide Lewis Structure: C₃O₂ Lewis Structure, linear Geometry, sp Hybridization & Polarity

Carbon suboxide Key Facts

The Carbon suboxide Lewis structure is C–C double bond and C–C double bond; the central C has 2 electron domains (0 lone pairs), giving a linear electron-domain arrangement and a linear molecular geometry with a 180° bond angle. C is best described as sp-hybridized, and Carbon suboxide is nonpolar because the bond dipoles cancel by molecular symmetry.

Figure 1: Lewis Structure of Carbon suboxide (C₃O₂)

Chemical Formula	C₃O₂
CAS Number	504-64-3
Total Valence Electrons	24
Lewis Structure	C–C double bond and C–C double bond
Electron-Domain Geometry	linear
Molecular Geometry	linear
Hybridization Model	sp (central C)
Bond Angle	180°
Polarity	Nonpolar molecule

PubChem (CID 136332) and NIST list Carbon suboxide as C ₃O ₂ with CAS 504-64-3; molecular weight ≈ 68.03 g/mol. View CAS 504-64-3 dictionary details on Guidechem →

Applications of Carbon suboxide (CAS 504-64-3)

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 "Carbon suboxide" 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 504-64-3 as the primary identifier when screening suppliers; always confirm regional availability and safety documentation (SDS).

Step 1 - Valence Electrons & Central Atom

To draw the Carbon suboxide Lewis structure we first count the total valence electrons. C₃O₂ contains 3×4 (C) + 2×6 (O); the net charge of 0 gives a total of 24 valence electrons to place.

The central atom is C. 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 = 3×4 (C) + 2×6 (O) = 24 electrons.

Step 2 - Lewis Structure & Electron Distribution

Place C 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: C–C double bond and C–C double bond; no lone pairs on C.

Counting bonding and nonbonding electrons around C 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 C–terminals bonds are equivalent in the resonance hybrid.

C=C C=C

C: 0 lone pairs, 2 bonding domains

2 bonding domains + 0 lone pairs = 2 electron domains

Octet Rule: Why C Has Eight Electrons C forms 2 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 2 electron domains around C arrange to minimize mutual repulsion, giving an linear 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 linear; the C 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 0 lone pair(s) on C, 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, C uses sp hybrid orbitals to form the 2 equivalent electron-domain directions (2 bonding + 0 lone pair).

Formal-charge check

Formal charge on central C = V − N − ½B = 4 − 0 − ½×8 = 0. The preferred Lewis structure carries zero formal charge on the central atom (and on the terminals), so it is the dominant contributor.

Modeling Note Modeling Note: sp is a compact model for the 2 electron-domain directions around C; full quantum-chemical treatments use molecular orbitals.

Is Carbon suboxide Polar or Nonpolar?

Carbon suboxide is nonpolar. Although individual C–terminal bonds are polar when the atoms differ in electronegativity, the linear 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. Carbon suboxide shows the opposite: identical bond dipoles arranged with linear 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
Carbon suboxide	C₃O₂	C	2	linear	Nonpolar
Carbon dioxide	CO₂	C	2	linear	Nonpolar
Carbon monoxide	CO	C	2	linear (diatomic)	Polar
Carbon disulfide	CS₂	C	2	linear	Nonpolar
Methane	CH₄	C	4	tetrahedral	Nonpolar
Ethane	C₂H₆	C	4	tetrahedral	Nonpolar

Practice question Starting from the 24 valence electrons of C₃O₂, draw the Lewis structure and confirm the central C atom is sp-hybridized with linear 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 Carbon suboxide (CAS 504-64-3)? Browse Supplier on Guidechem →

FAQs

Is C₃O₂ polar or nonpolar?

Carbon suboxide is nonpolar. Its linear symmetry cancels the bond dipoles exactly.

What is the Lewis structure of Carbon suboxide?

C–C double bond and C–C double bond; no lone pairs on C. It uses all 24 valence electrons and the preferred structure carries zero formal charge on the central atom.

What is the bond angle in Carbon suboxide?

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

What is the hybridization of C in Carbon suboxide?

The conventional model is sp. Carbon suboxide has 2 electron domains around the central C.

What is the CAS number of Carbon suboxide?

The CAS number is 504-64-3. PubChem (CID 136332) and NIST identify this with C₃O₂; use it to locate suppliers and database records.

References

PubChem CID 136332, Carbon suboxide. Molecular formula, CAS number, molecular weight and chemical identity.
NIST Chemistry WebBook, SRD 69, Carbon suboxide. 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 Carbon suboxide (CAS 504-64-3).

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 504-64-3 identifies the substance, not a universal purity specification.

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Carbon suboxide Lewis Structure

Carbon suboxide Lewis Structure