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The peroxide ion Lewis structure is Si–O single bond, Si–O single bond, Si–O single bond and Si–O single bond; the central Si has 4 electron domains (0 lone pairs), giving a tetrahedral electron-domain arrangement and a tetrahedral molecular geometry with a 109.5° bond angle. Si is best described as sp3-hybridized, and peroxide ion is nonpolar because the bond dipoles cancel by molecular symmetry.
Figure 1: Lewis Structure of peroxide ion (O4SiZr)
| Chemical Formula | O4SiZr |
| CAS Number | 14940-68-2 |
| Total Valence Electrons | 28 |
| Lewis Structure | Si–O single bond, Si–O single bond, Si–O single bond and Si–O single bond |
| Electron-Domain Geometry | tetrahedral |
| Molecular Geometry | tetrahedral |
| Hybridization Model | sp3 (central Si) |
| Bond Angle | 109.5° |
| Polarity | Nonpolar molecule |
The Si oxide peroxide ion is a key industrial intermediate. Nonmetal oxides such as SO3 and P4O10 are acid anhydrides for sulfuric and phosphoric acid manufacture, while metal/semimetal oxides are ceramics, refractories, catalysts and pigment precursors.
To draw the peroxide ion Lewis structure we first count the total valence electrons. O4SiZr contains 4×6 (O) + 4 (Si); the net charge of 0 gives a total of 28 valence electrons to place.
The central atom is Si. 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 = 4×6 (O) + 4 (Si) = 28 electrons.
Place Si 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: Si–O single bond, Si–O single bond, Si–O single bond and Si–O single bond; no lone pairs on Si.
Counting bonding and nonbonding electrons around Si therefore satisfies the octet/expanded-octet requirement for the drawn structure.
VSEPR theory states that the 4 electron domains around Si 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 Si 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 Si, 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, Si uses sp3 hybrid orbitals to form the 4 equivalent electron-domain directions (4 bonding + 0 lone pair).
Formal charge on central Si = 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.
peroxide ion is nonpolar. Although individual Si–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.
A common misconception is that polar bonds guarantee a polar molecule. peroxide ion shows the opposite: identical bond dipoles arranged with tetrahedral 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.
| Species | Formula | Central Atom | Electron Domains | Molecular Geometry | Polarity |
|---|---|---|---|---|---|
| peroxide ion | O4SiZr | Si | 4 | tetrahedral | Nonpolar |
| Silicon tetrafluoride | F4Si | Si | 4 | tetrahedral | Nonpolar |
| Silane | H4Si | Si | 4 | tetrahedral | Nonpolar |
peroxide ion is nonpolar. Its tetrahedral symmetry cancels the bond dipoles exactly.
Si–O single bond, Si–O single bond, Si–O single bond and Si–O single bond; no lone pairs on Si. It uses all 28 valence electrons and the preferred structure carries zero formal charge on the central atom.
The Si angle is about 109.5°. Lone-pair repulsion compresses the angle from the ideal tetrahedral value.
The conventional model is sp3. peroxide ion has 4 electron domains around the central Si.
The CAS number is 14940-68-2. PubChem (CID 61775) and NIST identify this with O4SiZr; 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 14940-68-2 identifies the substance, not a universal purity specification.
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