-
We detected your language preference as English. Would you like to switch to the English version for a better experience?
Switch to English
Stay here
The Vitamin C (Ascorbic acid) Lewis structure is C–C single bond, C–O single bond and 2 C–H single bond; the central C has 4 electron domains (0 lone pairs), giving a tetrahedral electron-domain arrangement and a tetrahedral molecular geometry with a 109.5° bond angle. C is best described as sp3-hybridized, and Vitamin C (Ascorbic acid) is polar because the tetrahedral shape (and/or unequal terminal atoms) prevents cancellation of the bond dipoles.
Figure 1: Lewis Structure of Vitamin C (Ascorbic acid) (C6H8O6)
| Chemical Formula | C6H8O6 |
| CAS Number | 50-81-7 |
| Total Valence Electrons | 68 |
| Lewis Structure | C–C single bond, C–O single bond and 2 C–H single bond |
| Electron-Domain Geometry | tetrahedral |
| Molecular Geometry | tetrahedral |
| Hybridization Model | sp3 (central C) |
| Bond Angle | 109.5° |
| Polarity | Polar molecule |
Carboxylic acids and esters are flavors, fragrances, polymers (PET, polyesters, alkyds) and solvents/intermediates; acetate and phthalate esters are plasticizers, and acids are precursors to salts, amides and anhydrides.
To draw the Vitamin C (Ascorbic acid) Lewis structure we first count the total valence electrons. C6H8O6 contains 6×4 (C) + 8×1 (H) + 6×6 (O); the net charge of 0 gives a total of 68 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).
Total valence electrons = 6×4 (C) + 8×1 (H) + 6×6 (O) = 68 electrons.
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 single bond, C–O single bond and 2 C–H single bond; no lone pairs on C.
Counting bonding and nonbonding electrons around C therefore satisfies the octet/expanded-octet requirement for the drawn structure.
VSEPR theory states that the 4 electron domains around C 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 C 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 C, 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, C uses sp3 hybrid orbitals to form the 4 equivalent electron-domain directions (4 bonding + 0 lone pair).
Formal charge on central C = V − N − ½B = 4 − 0 − ½×8 = 2. The nonzero formal charge is distributed by resonance / charge separation; the drawn structure is the lowest-energy contributor.
Vitamin C (Ascorbic acid) is polar. The tetrahedral 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.
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 Vitamin C (Ascorbic acid) the tetrahedral 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.
| Species | Formula | Central Atom | Electron Domains | Molecular Geometry | Polarity |
|---|---|---|---|---|---|
| Vitamin C (Ascorbic acid) | C6H8O6 | C | 4 | tetrahedral | Polar |
| 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 |
Vitamin C (Ascorbic acid) is polar. Its tetrahedral geometry (and/or unequal terminal atoms) stops the bond dipoles from cancelling.
C–C single bond, C–O single bond and 2 C–H single bond; no lone pairs on C. It uses all 68 valence electrons and the preferred structure carries a formal charge of 2 on the central atom.
The C angle is about 109.5°. Lone-pair repulsion compresses the angle from the ideal tetrahedral value.
The conventional model is sp3. Vitamin C (Ascorbic acid) has 4 electron domains around the central C.
The CAS number is 50-81-7. PubChem (CID 54670067) and NIST identify this with C6H8O6; 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 50-81-7 identifies the substance, not a universal purity specification.
 |
 |
|
 |
 |
 |
EN
Agricultural News
Food News
Industrial News
Cosmetic News
Pharmaceutical News
Science News
1YR
