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The Sulfuric acid Lewis structure is S–O single bond, S–O double bond, S–O double bond and S–O single bond; the central S has 4 electron domains (0 lone pairs), giving a tetrahedral electron-domain arrangement and a tetrahedral molecular geometry with a 109.5° bond angle. S is best described as sp3-hybridized, and Sulfuric acid is nonpolar because the bond dipoles cancel by molecular symmetry.
Figure 1: Lewis Structure of Sulfuric acid (H2O4S)
| Chemical Formula | H2O4S |
| CAS Number | 7664-93-9 |
| Total Valence Electrons | 32 |
| Lewis Structure | S–O single bond, S–O double bond, S–O double bond and S–O single bond |
| Electron-Domain Geometry | tetrahedral |
| Molecular Geometry | tetrahedral |
| Hybridization Model | sp3 (central S) |
| Bond Angle | 109.5° |
| Polarity | Nonpolar molecule |
Sulfuric acid is the highest-volume industrial chemical; it is produced via the contact process (SO3 + H2O → H2SO4). It is the dominant agent for fertilizer phosphate processing (phosphoric acid, MAP/DAP), ore leaching, petroleum refining, and pickling/cleaning of metals.
Its strong acidity and dehydrating power make it essential in titrations, sulfonation of detergents and dyes, and the manufacture of pigments, explosives and batteries (lead–acid electrolyte).
To draw the Sulfuric acid Lewis structure we first count the total valence electrons. H2O4S contains 2×1 (H) + 4×6 (O) + 6 (S); the net charge of 0 gives a total of 32 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).
Total valence electrons = 2×1 (H) + 4×6 (O) + 6 (S) = 32 electrons.
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: S–O single bond, S–O double bond, S–O double bond and S–O single bond; no lone pairs on S.
Counting bonding and nonbonding electrons around S 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 S–terminals bonds are equivalent in the resonance hybrid.
VSEPR theory states that the 4 electron domains around S arrange to minimize mutual repulsion, giving an tetrahedral 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 tetrahedral; the S bond angle is set to 109.5° rather than the ideal value for the electron-domain geometry.
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 S, the lone-pair domains occupy positions that minimize overall repulsion while pushing the bonding domains (and therefore the bonded atoms) closer together.
In the conventional localized-bond model, S uses sp3 hybrid orbitals to form the 4 equivalent electron-domain directions (4 bonding + 0 lone pair).
Formal charge on central S = V − N − ½B = 6 − 0 − ½×12 = 0. The preferred Lewis structure carries zero formal charge on the central atom (and on the terminals), so it is the dominant contributor.
Sulfuric acid is nonpolar. Although individual S–terminal bonds are polar when the atoms differ in electronegativity, the tetrahedral geometry makes their vector sum zero, so there is no net molecular dipole.
The sulfur atom in sulfuric acid is hypervalent (expanded octet); the tetrahedral arrangement of four oxygen ligands is the textbook example of an AX4 electron-domain pattern built on a third-period central atom.
Consistent with VSEPR and structural chemistry of oxoacids.Its nonpolar character governs solvation and intermolecular behavior; specify grade and handling when sourcing.
| Species | Formula | Central Atom | Electron Domains | Molecular Geometry | Polarity |
|---|---|---|---|---|---|
| Sulfuric acid | H2O4S | S | 4 | tetrahedral | 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 |
Sulfuric acid is nonpolar. Its tetrahedral symmetry cancels the bond dipoles exactly.
S–O single bond, S–O double bond, S–O double bond and S–O single bond; no lone pairs on S. It uses all 32 valence electrons and the preferred structure carries zero formal charge on the central atom.
The S angle is about 109.5°. Lone-pair repulsion compresses the angle from the ideal tetrahedral value.
The conventional model is sp3. Sulfuric acid has 4 electron domains around the central S.
The CAS number is 7664-93-9. PubChem (CID 1118) and NIST identify this with H2O4S; use it to locate suppliers and database records.
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 7664-93-9 identifies the substance, not a universal purity specification.
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