Selenium dioxide
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| Names | |
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| Other names
Selenium(IV) oxide
Selenous anhydride | |
| Identifiers | |
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3D model (JSmol)
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PubChem CID
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| UN number | 3283 |
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| Properties[2] | |
| Page Module:Chem2/styles.css has no content.SeO2 | |
| Molar mass | 110.969 g·mol−1 |
| Appearance | White tetragonal needles or powder |
| Odor | rotten horseradish |
| Density | 3.95 g/cm3, solid |
| Melting point | 360 °C (680 °F; 633 K) (sealed tube) |
| Boiling point | 315 °C (599 °F; 588 K) (sublimation point) |
| 263.4 g/100mL (Template:Cvt, forms selenous acid) | |
| Solubility in ethanol | soluble |
| Solubility in acetone | slightly soluble |
| Solubility in methanol | soluble |
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| Band gap | 3.29 eV[1] |
| −27.2×10−6 cm3/mol | |
| 2.62±0.05 D | |
| Structure[1] | |
| Tetragonal | |
| P42/mbc | |
| 4/mmm | |
a = 8.37 Å, b = 8.37 Å, c = 5.08 Å α = 90°, β = 90°, γ = 90°
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Lattice volume (V)
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356.23 Å3 |
Formula units (Z)
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8 |
| Thermochemistry[2] | |
Std enthalpy of
formation (ΔfH⦵298) |
−225.4 kJ/mol |
| Hazards | |
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| Flash point | Non-flammable |
Threshold limit value (TLV)
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0.2 mg/m3 (TWA) |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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LCLo (lowest published)
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| NIOSH (US health exposure limits):[a] | |
PEL (Permissible)
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0.2 mg/m3 |
REL (Recommended)
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0.2 mg/m3 |
IDLH (Immediate danger)
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1 mg/m3 (as Se) |
| Related compounds | |
Other cations
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Related selenium oxides
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Selenium trioxide |
Related compounds
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Template:Chembox Footer/trackingTemplate:Short description
Selenium dioxide is the chemical compound with the formula Page Module:Chem2/styles.css has no content.SeO2. This colorless solid is one of the most frequently encountered compounds of selenium. It is used in making specialized glasses as well as a reagent in organic chemistry.[7]
Properties
Solid Page Module:Chem2/styles.css has no content.SeO2 is a one-dimensional polymer, the chain consisting of alternating selenium and oxygen atoms. Each Se atom is pyramidal and bears a terminal oxide group. The bridging Page Module:Chem2/styles.css has no content.Se−O bond lengths are Template:Cvt and the terminal Page Module:Chem2/styles.css has no content.Se−O distance is Template:Cvt.[8] The relative stereochemistry at Se alternates along the polymer chain (syndiotactic).
In the gas phase selenium dioxide is present as dimers and other oligomeric species, at higher temperatures it is monomeric.[9][page needed] The monomeric form adopts a bent structure very similar to that of sulfur dioxide with a bond length of Template:Cvt.[9][page needed] The dimeric form has been isolated in a low temperature argon matrix and vibrational spectra indicate that it has a centrosymmetric chair form.[8] Dissolution of Page Module:Chem2/styles.css has no content.SeO2 in selenium oxydichloride give the trimer Page Module:Chem2/styles.css has no content.[Se(O)O]3.[9][page needed]
The solid sublimes readily. At very low concentrations the vapour has a revolting odour, resembling decayed horseradishes. At higher concentrations the vapour has an odour resembling horseradish sauce and can burn the nose and throat on inhalation. Whereas Page Module:Chem2/styles.css has no content.SO2 tends to be molecular and Page Module:Chem2/styles.css has no content.SeO2 is a one-dimensional chain, Page Module:Chem2/styles.css has no content.TeO2 is a cross-linked polymer.[8]
Page Module:Chem2/styles.css has no content.SeO2 is considered an acidic oxide: it dissolves in water to form selenous acid.[9] Often the terms selenous acid and selenium dioxide are used interchangeably. It reacts with base to form selenite salts containing the Page Module:Chem2/styles.css has no content.SeO2−3 anion. For example, reaction with sodium hydroxide produces sodium selenite:
- Page Module:Chem2/styles.css has no content.SeO2 + 2 NaOH → Na2SeO3 + H2O
Preparation
Selenium dioxide is prepared by oxidation of selenium by burning in air or by reaction with nitric acid or hydrogen peroxide, but perhaps the most convenient preparation is by the dehydration of selenous acid:[citation needed]
- Page Module:Chem2/styles.css has no content.2 H2O2 + Se → SeO2 + 2 H2O
- Page Module:Chem2/styles.css has no content.3 Se + 4 HNO3 + H2O → 3 H2SeO3 + 4 NO
- Page Module:Chem2/styles.css has no content.H2SeO3 ⇌ SeO2 + H2O
Occurrence
The natural form of selenium dioxide, downeyite, is a very rare mineral. It is only found at a small number of coal-seam fires, where it forms around vents created from escaping gasses.[10]
Uses
Organic synthesis
SeO2 is an important reagent in organic synthesis. Oxidation of paraldehyde (acetaldehyde trimer) with SeO2 gives glyoxal[11] and the oxidation of cyclohexanone gives 1,2-cyclohexanedione.[12] The selenium starting material is reduced to selenium, and precipitates as a red amorphous solid which can easily be filtered off.[12] This type of reaction is called a Riley oxidation. It is also renowned as a reagent for allylic oxidation, a reaction that entails the following conversion:[13]
This can be described more generally as:
- Page Module:Chem2/styles.css has no content.R2C=CR′−CHR″2 + [O] → R2C=CR′−C(OH)R″2
where R, R', R" may be alkyl or aryl substituents.
Selenium dioxide can also be used to synthesize 1,2,3-selenadiazoles from acylated hydrazone derivatives.[14]
As a colorant
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Selenium dioxide imparts a red colour to glass. It is used in small quantities to counteract the colour due to iron impurities and so to create (apparently) colourless glass. In larger quantities, it gives a deep ruby red colour.
Selenium dioxide is the active ingredient in some cold-bluing solutions.
It was also used as a toner in photographic developing.
Safety
Selenium is an essential element, but ingestion of more than 5 mg/d leads to nonspecific symptoms.[15]
Notes
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- ^ PEL, REL, and IDLH values are based on sodium selenide, which is an order of magnitude more toxic than other selenium compounds.[5]
References
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- ^ a b Page Module:Citation/CS1/styles.css has no content."Materials Explorer - Selenium dioxide". next-gen.materialsproject.org. The Materials Project. Retrieved 27 April 2026.
- ^ a b Template:RubberBible97th
- ^ Page Module:Citation/CS1/styles.css has no content."Selenium dioxide safety and hazards". pubchem.ncbi.nlm.nih.gov. Retrieved 2022-12-02.
- ^ a b Page Module:Citation/CS1/styles.css has no content."SDS - Selenium dioxide". www.fishersci.com. ThermoFisher Scientific. 19 December 2025. p. 3. Retrieved 27 April 2026.
- ^ a b Page Module:Citation/CS1/styles.css has no content."Selenium compounds (as Se)". Immediately Dangerous to Life or Health Concentrations. National Institute for Occupational Safety and Health.
- ^ Sigma-Aldrich Co., Selenium dioxide.
- ^ Page Module:Citation/CS1/styles.css has no content.Hoekstra, William J.; Fairlamb, Ian J. S.; Giroux, Simon; Chen, Yuzhong (2017). "Selenium(IV) Oxide". Encyclopedia of Reagents for Organic Synthesis. pp. 1–12. doi:10.1002/047084289X.rs008.pub3. ISBN 978-0-470-84289-8.
- ^ a b c Page Module:Citation/CS1/styles.css has no content.Devillanova, Franceso A. (2007). Handbook of Chalcogen Chemistry: New Perspectives in Sulfur, Selenium and Tellurium. Royal Society of Chemistry. ISBN 9780854043668.
- ^ a b c d Page Module:Citation/CS1/styles.css has no content.Holleman, Arnold Frederik; Wiberg, Egon (2001), Wiberg, Nils (ed.), Inorganic Chemistry, translated by Eagleson, Mary; Brewer, William, San Diego/Berlin: Academic Press/De Gruyter, ISBN 0-12-352651-5
- ^ Page Module:Citation/CS1/styles.css has no content.Finkelman, Robert B.; Mrose, Mary E. (1977). "Downeyite, the first verified natural occurrence of SeO2" (PDF). American Mineralogist. 62: 316–320.
- ^ Page Module:Citation/CS1/styles.css has no content.Ronzio, A. R.; Waugh, T. D. (1944). "Glyoxal Bisulfite". Organic Syntheses. 24: 61. doi:10.15227/orgsyn.024.0061; Page Module:Citation/CS1/styles.css has no content.Collected Volumes, vol. 3, 1955, p. 438.
- ^ a b Page Module:Citation/CS1/styles.css has no content.Hach, C. C.; Banks, C. V.; Diehl, H. (1952). "1,2-Cyclohexanedione Dioxime". Organic Syntheses. 32: 35. doi:10.15227/orgsyn.032.0035; Page Module:Citation/CS1/styles.css has no content.Collected Volumes, vol. 4, 1963, p. 229.
- ^ Page Module:Citation/CS1/styles.css has no content.Coxon, J. M.; Dansted, E.; Hartshorn, M. P. (1977). "Allylic Oxidation with Hydrogen Peroxide–Selenium Dioxide: trans-Pinocarveol". Organic Syntheses. 56: 25. doi:10.15227/orgsyn.056.0025; Page Module:Citation/CS1/styles.css has no content.Collected Volumes, vol. 6, 1988, p. 946.
- ^ Page Module:Citation/CS1/styles.css has no content.Lalezari, Iraj; Shafiee, Abbas; Yalpani, Mohamed (1969). "A novel synthesis of selenium heterocycles: substituted 1,2,3-selenadiazoles". Tetrahedron Letters. 10 (58): 5105–5106. doi:10.1016/S0040-4039(01)88895-X.
- ^ Script error: No such module "Template wrapper".
External links
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