Chemistry:Strontium perchlorate
| Names | |
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| Other names
Strontium(II) perchlorate; Strontium diperchlorate
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| EC Number |
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PubChem CID
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| Properties | |
| Sr(ClO 4) 2 | |
| Molar mass | 286.51 g·mol−1 |
| Appearance | White crystals |
| Density | 2.973 g/cm3[1] |
| Melting point | 477 °C (891 °F; 750 K)[1] (decomposes vigorously) |
| 309.7 g/100 g | |
| Solubility in ethyl acetate | 136.9 g/100 g |
| Solubility in methanol | 221.0 g/100 g |
| Solubility in ethanol | 180.7 g/100 g |
| Solubility in 1-propanol | 140.4 g/100 g |
| Solubility in 1-butanol | 113.5 g/100 g |
| Solubility in isobutanol | 77.9 g/100 g |
| Structure[2] | |
| orthorhombic | |
| Pbca | |
a = 14.18206 Å, b = 9.78934 Å, c = 9.37624 Å α = 10.009°, β = 90°, γ = 90°
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Lattice volume (V)
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1301.73 Å3 |
| 8 | |
| Hazards | |
| GHS pictograms |  
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| GHS Signal word | Danger |
| H272, H315, H319, H335 | |
| P210, P221, P280, P305+351+338, P403+233, P501 | |
| NFPA 704 (fire diamond) | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Strontium perchlorate is a deliquescent white crystalline compound with the formula Sr(ClO
4)
2.[1]
It is a strong oxidizer which gives red flames. It can be used in pyrotechnics; however, usually the more common strontium nitrate is used. Strontium perchlorate has been used in gelled flame compositions where its hygroscopic nature isn't an issue, in a polymerized candle composition that excluded water, and in an experimental high-atmosphere flash powder.[1]
Strontium perchlorate has been characterized in multiple hydrated forms; a trihydrate (Sr(ClO
4)
2 · 3H2O), tetrahydrate (Sr(ClO
4)
2 · 4H2O) and nonahydrate (Sr(ClO
4)
2 · 9H2O).[2]
Synthesis
Hydrated forms may be prepared by dissolving pure strontium nitrate in an excess of perchloric acid, neutralizing the excess acid with strontium carbonate, centrifuging off solids, and chilling to precipitate crystals.
The anhydrous form may be prepared by drying the hydrate at 250 °C (482 °F), which gives a yield of 50%, or by the addition of anhydrous perchloric acid to a solution of strontium ion in anhydrous trifluoroacetic acid followed by filtration of the precipitated solid and removal of excess acid under vacuum.[1]
References
- ↑ 1.0 1.1 1.2 1.3 1.4 Kaye, Seymour M. (1 January 1978). "P - Perchlorates". Encyclopedia of Explosives and Related Items. Volume 8. Dover, NJ: Army Armament Research And Development Center - Large Caliber Weapon Systems Lab. p. P168-9. ADA057762, PATR 2700. https://apps.dtic.mil/sti/pdfs/ADA057762.pdf.
- ↑ 2.0 2.1 Hyoung, Jooeun; Lee, Hyeon Woo; Kim, So Jin; Shin, Hong Rim; Hong, Seung-Tae (2019). "Crystal structure of strontium perchlorate anhydrate, Sr(ClO4)2, from laboratory powder X-ray diffraction data". Acta Crystallographica Section E 75 (4): 447–450. doi:10.1107/S2056989019003335. PMID 31161054.
- ↑ 3.0 3.1 "Strontium perchlorate (SDS)". Strem Catalog. 20 July 2021. https://www.strem.com/product/93-3817.
Compounds containing perchlorate group
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| HClO4 | He | ||||||||||||||||||
| LiClO4 | Be(ClO4)2 | B(ClO4)−4 B(ClO4)3 |
ROClO3 | N(ClO4)3 NH4ClO4 NOClO4 |
O | FClO4 | Ne | ||||||||||||
| NaClO4 | Mg(ClO4)2 | Al(ClO4)3 | Si | P | S | ClO−4 ClOClO3 Cl2O7 |
Ar | ||||||||||||
| KClO4 | Ca(ClO4)2 | Sc(ClO4)3 | Ti(ClO4)4 | VO(ClO4)3 VO2(ClO4) |
Cr(ClO4)3 | Mn(ClO4)2 | Fe(ClO4)3 | Co(ClO4)2, Co(ClO4)3 |
Ni(ClO4)2 | Cu(ClO4)2 | Zn(ClO4)2 | Ga(ClO4)3 | Ge | As | Se | Br | Kr | ||
| RbClO4 | Sr(ClO4)2 | Y(ClO4)3 | Zr(ClO4)4 | Nb(ClO5)4 | Mo | Tc | Ru | Rh(ClO4)3 | Pd(ClO4)2 | AgClO4 | Cd(ClO4)2 | In(ClO4)3 | Sn(ClO4)4 | Sb | TeO(ClO4)2 | I | Xe | ||
| CsClO4 | Ba(ClO4)2 | Hf(ClO4)4 | Ta(ClO5)5 | W | Re | Os | Ir | Pt | Au | Hg2(ClO4)2, Hg(ClO4)2 |
Tl(ClO4)3 | Pb(ClO4)2 | Bi(ClO4)3 | Po | At | Rn | |||
| FrClO4 | Ra | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |||
| ↓ | |||||||||||||||||||
| La | Ce(ClO4)x | Pr | Nd | Pm | Sm(ClO4)3 | Eu(ClO4)3 | Gd(ClO4)3 | Tb(ClO4)3 | Dy(ClO4)3 | Ho(ClO4)3 | Er(ClO4)3 | Tm(ClO4)3 | Yb(ClO4)3 | Lu(ClO4)3 | |||||
| Ac | Th(ClO4)4 | Pa | UO2(ClO4)2 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr | |||||
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