Chemistry:Strontium oxalate
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| Names | |
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| IUPAC name
Strontium oxalate
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| Identifiers | |
3D model (JSmol)
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PubChem CID
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| Properties | |
| SrC 2O 4 | |
| Molar mass | 175.64 g·mol−1 |
| Appearance | White powder |
| Density | 2.08 g/cm3 |
| Melting point | Decomposes above 150 °C (302 °F; 423 K) (monohydrate)[1] |
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| Solubility in Acetic acid |
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| Hazards[3] | |
| Safety data sheet | Ambeed Inc. Strontium Oxalate SDS |
| GHS pictograms | 
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| GHS Signal word | Warning |
| HH302Script error: No such module "Preview warning".Category:GHS errors, HH312Script error: No such module "Preview warning".Category:GHS errors | |
| PP280Script error: No such module "Preview warning".Category:GHS errors | |
| NFPA 704 (fire diamond) | |
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Other anions
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Strontium oxalate is a compound with the chemical formula SrC
2O
4. Strontium oxalate can exist either in a hydrated form (SrC
2O
4 · nH
2O) or as the acidic salt of strontium oxalate (SrC
2O
4 · mH
2C
2O
4 · nH
2O).[5][verification needed]
Use in pyrotechnics
With the addition of heat, strontium oxalate will decompose based on the following reaction:[1]
- SrC
2O
4 → SrO + CO
2 + CO
Strontium oxalate is a useful red color emitter for use in pyrotechnics. It decomposes into strontium oxide, a good scarlet red emitter with two strong peaks at 595 and 597 nm. The oxide reacts with moisture in the atmosphere to form the hydroxide, so its three strong peaks of 682 nm, 671 nm, and 606 nm are also relevant.[6]
Decomposition produces carbon monoxide (CO), which can reduce magnesium oxide (a broad spectrum emitter which can wash out colors) to magnesium gas, resulting in a more transparent flame. This makes it a better emitter than other common strontium compounds in the presence of magnesium:
MgO(s) + CO → Mg(g) + CO
2
When magnesium is not present, there is no benefit from the production of CO gas and strontium carbonate is usually preferable.[1]
Chlorine donors or chlorinated oxidizers result in a shift towards formation of strontium chloride which produces a slightly different, deeper red spectrum, having its three strongest peaks at 674 nm, 661 nm, and 636 nm.[6]
References
- ↑ 1.0 1.1 1.2 1.3 Shimizu, Takeo (2013). "2. Chemical Components of Fireworks Compositions". in Kosanke, B.L. (pdf). Pyrotechnic Chemistry (1.1 ed.). Whitewater, CO, USA: Journal of Pyrotechnics, Inc.. p. 2-10. ISBN 978-1-889526-31-7. http://www.jpyro.co.uk/wp-content/uploads/bk2022h.pdf?page=38.
- ↑ O'Neil, M.J., ed (2013). The Merck index: an encyclopedia of chemicals, drugs, and biologicals (15. ed.). Cambridge: The Royal Society of Chemistry. ISBN 9781849736701.
- ↑ 3.0 3.1 Sigma-Aldrich Co., Strontium oxalate.
- ↑ "Strontium oxalate SDS". Thermo Fisher Scientific. 30 March 2024. https://www.fishersci.com/store/msds?partNumber=AA3957336&productDescription=STRONTIUM+OXALATE+500G&vendorId=VN00024248&countryCode=US&language=en.
- ↑ Knaepen, E.; Mullens, J.; Yperman, J.; Van Poucke, L.C. (July 1996). "Preparation and thermal decomposition of various forms of strontium oxalate". Thermochimica Acta 284 (1): 213–227. doi:10.1016/0040-6031(96)02863-8. Bibcode: 1996TcAc..284..213K.
- ↑ 6.0 6.1 "Color Values and Spectra of the Principal Emitters in Colored Flames". Journal of Pyrotechnics. Pyrotechnic Literature Series No. 11 Selected Pyrotechnic Publications of K. L. and B. J. Kosanke (2003 and 2004) (7): 58, 63. http://www.jpyro.co.uk/wp-content/uploads/K07_052_wetq.pdf?page=12.
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