Disulfur Lewis Structure

Disulfur Lewis Structure: S₂ Lewis Structure, linear (diatomic) Geometry, sp2 Hybridization & Polarity

Disulfur Key Facts

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

Figure 1: Lewis Structure of Disulfur (S₂)

Chemical Formula	S₂
CAS Number	23550-45-0
Total Valence Electrons	12
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	Nonpolar molecule

PubChem (CID 5460602) and NIST list Disulfur as S ₂ with CAS 23550-45-0; molecular weight ≈ 64.13 g/mol. View CAS 23550-45-0 dictionary details on Guidechem →

Applications of Disulfur (CAS 23550-45-0)

Disulfur is encountered as a reagent, intermediate or specialty chemical in inorganic, organometallic and materials synthesis. Confirm grade, purity and supplier documentation (SDS) before specifying for a process.

Reagent / Intermediate Used in synthesis and formulation where the substance's reactivity is required.

Specialty Chemical Specified by grade for the intended process or research use.

Sourcing Verify purity, package and regional availability via the CAS identifier.

Procurement Note "Disulfur" 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 23550-45-0 as the primary identifier when screening suppliers; always confirm regional availability and safety documentation (SDS).

Step 1 - Valence Electrons & Central Atom

To draw the Disulfur Lewis structure we first count the total valence electrons. S₂ contains 2×6 (S); the net charge of 0 gives a total of 12 valence electrons to place.

The central atom is S. 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 = 2×6 (S) = 12 electrons.

Step 2 - Lewis Structure & Electron Distribution

Place S 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 S therefore satisfies the octet/expanded-octet requirement for the drawn structure.

S–X

S: 2 lone pairs, 1 bonding domain

1 bonding domains + 2 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 S arrange to minimize mutual repulsion, giving an linear electron-domain geometry.

Because 2 of these domains are lone pair(s) — and lone pairs repel more strongly than bonding pairs — the observed molecular geometry is linear (diatomic); the S 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 2 lone pair(s) on S, 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, S uses sp2 hybrid orbitals to form the 3 equivalent electron-domain directions (1 bonding + 2 lone pair).

Formal-charge check

Formal charge on central S = V − N − ½B = 6 − 4 − ½×4 = 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: sp2 is a compact model for the 3 electron-domain directions around S; full quantum-chemical treatments use molecular orbitals.

Is Disulfur Polar or Nonpolar?

Disulfur is nonpolar. Although individual S–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. Disulfur 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
Disulfur	S₂	S	3	linear (diatomic)	Nonpolar
Sulfur dioxide	SO₂	S	3	bent	Polar
Sulfur trioxide	O₃S	S	3	trigonal planar	Nonpolar
Sulfur hexafluoride	F₆S	S	6	octahedral	Nonpolar
Sulfur tetrafluoride	F₄S	S	5	seesaw	Polar
Sulfate	O₄S	S	4	tetrahedral	Nonpolar

Practice question Starting from the 12 valence electrons of S₂, draw the Lewis structure and confirm the central S 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 Disulfur (CAS 23550-45-0)? Browse Supplier on Guidechem →

FAQs

Is S₂ polar or nonpolar?

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

What is the Lewis structure of Disulfur?

linear diatomic molecule with one double bond and a lone pair on each atom. It uses all 12 valence electrons and the preferred structure carries zero formal charge on the central atom.

What is the bond angle in Disulfur?

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

What is the hybridization of S in Disulfur?

The conventional model is sp2. Disulfur has 3 electron domains around the central S.

What is the CAS number of Disulfur?

The CAS number is 23550-45-0. PubChem (CID 5460602) and NIST identify this with S₂; use it to locate suppliers and database records.

References

PubChem CID 5460602, Disulfur. Molecular formula, CAS number, molecular weight and chemical identity.
NIST Chemistry WebBook, SRD 69, Disulfur. 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 Disulfur (CAS 23550-45-0).

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 23550-45-0 identifies the substance, not a universal purity specification.

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Disulfur Lewis Structure

Disulfur Lewis Structure