Diatomic carbon Lewis Structure

Diatomic carbon Lewis Structure: C₂ Lewis Structure, linear (diatomic) Geometry, sp Hybridization & Polarity

Diatomic carbon Key Facts

The Diatomic carbon Lewis structure is a linear diatomic with a nonpolar bond between its two atoms; because the two atoms are identical, Diatomic carbon is nonpolar.

Figure 1: Lewis Structure of Diatomic carbon (C₂)

Chemical Formula	C₂
CAS Number	12070-15-4
Total Valence Electrons	8
Lewis Structure	linear diatomic molecule with one triple bond
Electron-Domain Geometry	linear
Molecular Geometry	linear (diatomic)
Hybridization Model	sp
Bond Angle	180°
Polarity	Nonpolar molecule

PubChem (CID 139247) and NIST list Diatomic carbon as C ₂ with CAS 12070-15-4; molecular weight ≈ 24.02 g/mol. View CAS 12070-15-4 dictionary details on Guidechem →

Applications of Diatomic carbon (CAS 12070-15-4)

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 "Diatomic carbon" 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 12070-15-4 as the primary identifier when screening suppliers; always confirm regional availability and safety documentation (SDS).

Step 1 - Valence Electrons & Central Atom

To draw the Diatomic carbon Lewis structure we first count the total valence electrons. C₂ contains 2×4 (C); the net charge of 0 gives a total of 8 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 = 2×4 (C) = 8 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: linear diatomic molecule with one triple bond; 1 lone pair(s) on C.

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

C–X

C: 1 lone pair, 1 bonding domain

1 bonding domains + 1 lone pairs = 2 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 2 electron domains around C 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 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 1 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 (1 bonding + 1 lone pair).

Formal-charge check

Formal charge on central C = V − N − ½B = 4 − 2 − ½×6 = -1. The nonzero formal charge is distributed by resonance / charge separation; the drawn structure is the lowest-energy 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 Diatomic carbon Polar or Nonpolar?

Diatomic carbon is nonpolar. Although individual C–terminal bonds are polar when the atoms differ in electronegativity, the linear (diatomic) 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. Diatomic carbon shows the opposite: identical bond dipoles arranged with linear (diatomic) 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
Diatomic carbon	C₂	C	2	linear (diatomic)	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 8 valence electrons of C₂, draw the Lewis structure and confirm the central C atom is sp-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 Diatomic carbon (CAS 12070-15-4)? Browse Supplier on Guidechem →

FAQs

Is C₂ polar or nonpolar?

Diatomic carbon is nonpolar. Its linear (diatomic) symmetry cancels the bond dipoles exactly.

What is the Lewis structure of Diatomic carbon?

linear diatomic molecule with one triple bond; 1 lone pair(s) on C. It uses all 8 valence electrons and the preferred structure carries a formal charge of -1 on the central atom.

What is the bond angle in Diatomic carbon?

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

What is the hybridization of C in Diatomic carbon?

The conventional model is sp. Diatomic carbon has 2 electron domains around the central C.

What is the CAS number of Diatomic carbon?

The CAS number is 12070-15-4. PubChem (CID 139247) and NIST identify this with C₂; use it to locate suppliers and database records.

References

PubChem CID 139247, Diatomic carbon. Molecular formula, CAS number, molecular weight and chemical identity.
NIST Chemistry WebBook, SRD 69, Diatomic carbon. 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 Diatomic carbon (CAS 12070-15-4).

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 12070-15-4 identifies the substance, not a universal purity specification.

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Diatomic carbon Lewis Structure

Diatomic carbon Lewis Structure