Caesium perchlorate

Caesium perchlorate^[1][2]

Names
IUPAC name Caesium perchlorate
Other names Cesium perchlorate
Identifiers
CAS Number	13454-84-7
ChemSpider	109912
EC Number	236-643-0
Jmol interactive 3D	Image
PubChem	3035378
InChI InChI=1S/ClHO4.Cs/c2-1(3,4)5;/h(H,2,3,4,5);/q;+1/p-1 Key: WKDKOOITVYKILI-UHFFFAOYSA-M InChI=1/ClHO4.Cs/c2-1(3,4)5;/h(H,2,3,4,5);/q;+1/p-1 Key: WKDKOOITVYKILI-REWHXWOFAB
SMILES [Cs+].[O-]Cl(=O)(=O)=O
Properties
Chemical formula	CsClO4
Molar mass	232.36 g/mol
Appearance	Colorless crystalls
Density	3.327 g/cm^3
Melting point	250 °C (482 °F; 523 K) (decomposes)
Solubility in water	1.974 g/100 ml (25 °C)
Refractive index (nD)	1.4887
Structure
Crystal structure	orthorhombic (<219 °C) cubic (>219 °C, a = 798 pm)
Space group	Pnma (<219 °C) F43m (>219 °C)
Lattice constant	a = 982 pm, b = 600 pm, c = 779 pm (orthorhombic, <219 °C)
Hazards
Safety data sheet	External MSDS
Flash point	Non-flammable
Related compounds
Other anions	Caesium chloride Caesium chlorate
Other cations	Lithium perchlorate Sodium perchlorate Potassium perchlorate Rubidium perchlorate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Caesium perchlorate, CsClO₄ (also known as cesium perchlorate), is a perchlorate of caesium. It forms white crystals, which are sparingly soluble in cold water and ethanol. It dissolves more easily in hot water.

CsClO₄ is the least soluble of the alkali metal perchlorates (followed by Rb, K, Li, and Na), a property which may be used for separatory purposes and even for gravimetric analysis. ^[3] This low solubility played an important role in the characterization of francium as an alkali metal, as francium perchlorate coprecipitates with caesium perchlorate.^[4]

Table of solubility in water^[1][2]

Temperature (°C)	0	8.5	14	25	40	50	60	70	99
Solubility (g / 100 ml)	0.8	0.91	1.91	1.974	3.694	5.47	7.30	9.79	28.57

When heated, CsClO₄ decomposes to caesium chloride above 250 °C. Like all perchlorates, it is a strong oxidant and may react violently with reducing agents and organic materials, especially at elevated temperatures.

References

1. Perry, Dale L.; Phillips, Sidney L. (1995), Handbook of Inorganic Compounds, CRC Press.
2. Brezina, F.; Mollin, J.; Pastorek, R.; Sindelar, Z. (1986), Chemicke tabulky anorganickych sloucenin, SNTL.
3. Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. p. 1017. ISBN 0-08-022057-6..
4. Hyde, E. K. (1952), "Radiochemical Methods for the Isolation of Element 87 (Francium)", J. Am. Chem. Soc. 74 (16): 4181–84, doi:10.1021/ja01136a066

External links

• Sigma-Aldrich MSDS

Salts and the ester of the Perchlorate ion
HClO4																	He
LiClO4	Be(ClO4)2											B(ClO4)4^−	ROClO3	N(ClO4)3 NH4ClO4	O	FClO4	Ne
NaClO4	Mg(ClO4)2											Al(ClO4)3	Si	P	S	ClO4^− ClOClO3 Cl2O7	Ar
KClO4	Ca(ClO4)2	Sc(ClO4)3	Ti(ClO4)4	VO(ClO4)3	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	Zr	Nb	Mo	Tc	Ru	Rh	Pd(ClO4)2	AgClO4	Cd(ClO4)2	In	Sn	Sb	Te	I	Xe
CsClO4	Ba(ClO4)2		Hf	Ta	W	Re	Os	Ir	Pt	Au	Hg2(ClO4)2, Hg(ClO4)2	Tl(ClO4)3	Pb(ClO4)2	Bi(ClO4)3	Po	At	Rn
Fr	Ra		Rf	Db	Sg	Bh	Hs	Mt	Ds	Rg	Cn	Uut	Fl	Uup	Lv	Uus	Uuo
		↓
		La	Ce(ClO4)x	Pr	Nd	Pm	Sm	Eu	Gd	Tb	Dy	Ho	Er	Tm	Yb	Lu
		Ac	Th	Pa	UO2(ClO4)2	Np	Pu	Am	Cm	Bk	Cf	Es	Fm	Md	No	Lr