Chemistry:Curium(III) nitrate
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Names | |
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Other names
Curium trinitrate, Curium nitrate
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Identifiers | |
3D model (JSmol)
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EC Number |
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PubChem CID
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Properties | |
Cm(NO3)3 | |
Molar mass | 433.09 g/mol |
Melting point | 400 °C (752 °F; 673 K) |
Hazards | |
GHS Signal word | Warning |
Related compounds | |
Related compounds
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Terbium(III) nitrate, Lutetium(III) nitrate, Cerium(III) nitrate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
Infobox references | |
Curium(III) nitrate is an inorganic compound, a salt of curium and nitric acid with the chemical formula Cm(NO3)3.[1][2][3]
Synthesis
Reaction of curium and nitric acid:[4]
- Cm + 4 HNO
3 → Cm(NO
3)
3 + NO + 2 H
2O
Physical properties
Curium(III) nitrate is a solid that exists as a hydrate or anhydrate, depending on the synthesis. The hydrates melt at 90 and 180 °C in crystallization water. The anhydrate decomposes to curium(IV) oxide at temperatures above 400 °C.[5]
Applications
Curium(III) nitrate can be used to make curium(IV) oxide.
References
- ↑ Волков, А.И.; Жарский, И.М. (2005) (in ru). Большой химический справочник. Современная школа. p. 132. ISBN 985-6751-04-7.
- ↑ Skerencak, A.; Panak, Petra J.; Hauser, W.; Neck, Volker; Klenze, R.; Lindqvist-Reis, P.; Fanghänel, Thomas (January 2009). "TRLFS study on the complexation of Cm(III) with nitrate in the temperature range from 5 to 200 °C". Radiochimica Acta 97 (8). doi:10.1524/ract.2009.1631. https://www.degruyter.com/document/doi/10.1524/ract.2009.1631/pdf. Retrieved 19 August 2021.
- ↑ Modolo, Giuseppe; Kluxen, Paul; Geist, Andreas (January 2010). "Demonstration of the LUCA process for the separation of americium(III) from curium(III), californium(III), and lanthanides(III) in acidic solution using a synergistic mixture of bis(chlorophenyl)dithiophosphinic acid and tris(2-ethylhexyl)phosphate". Radiochimica Acta 98 (4). doi:10.1524/ract.2010.1708. http://juser.fz-juelich.de/record/9815/files/%5BRadiochimica%20Acta%5D%20Demonstration%20of%20the%20LUCA%20process%20for%20the%20separation%20of%20americium%28III%29%20from%20curium%28III%29%20californium%28III%29%20and%20lanthanides%28III%29%20in%20acidic%20solution%20using%20a%20synergistic%20mixture%20of%20bis%28chloro.pdf.
- ↑ Edelmann, Frank T.; Herrmann, Wolfgang A. (14 May 2014) (in en). Synthetic Methods of Organometallic and Inorganic Chemistry, Volume 6, 1997: Volume 6: Lanthanides and Actinides. Georg Thieme Verlag. p. 23. ISBN 978-3-13-179221-1. https://books.google.com/books?id=6IuZAwAAQBAJ&dq=Ytterbium+(III)+nitrate&pg=PA226. Retrieved 19 August 2021.
- ↑ Morss, L. R.; Edelstein, Norman M.; Fuger, Jean (21 October 2010) (in en). The Chemistry of the Actinide and Transactinide Elements (Set Vol.1-6): Volumes 1-6. Springer Science & Business Media. p. 1422. ISBN 978-94-007-0211-0. https://books.google.com/books?id=9vPuV3A0UGUC&pg=PA1422. Retrieved 23 August 2021.
Salts and covalent derivatives of the nitrate ion
HNO3 | He | ||||||||||||||||
LiNO3 | Be(NO3)2 | B(NO3)−4 | C | NO−3, NH4NO3 |
O | FNO3 | Ne | ||||||||||
NaNO3 | Mg(NO3)2 | Al(NO3)3 | Si | P | S | ClONO2 | Ar | ||||||||||
KNO3 | Ca(NO3)2 | Sc(NO3)3 | Ti(NO3)4 | VO(NO3)3 | Cr(NO3)3 | Mn(NO3)2 | Fe(NO3)3, Fe(NO3)2 |
Co(NO3)2, Co(NO3)3 |
Ni(NO3)2 | Cu(NO3)2 | Zn(NO3)2 | Ga(NO3)3 | Ge | As | Se | Br | Kr |
RbNO3 | Sr(NO3)2 | Y(NO3)3 | Zr(NO3)4 | Nb | Mo | Tc | Ru | Rh | Pd(NO3)2 | AgNO3 | Cd(NO3)2 | In | Sn | Sb(NO3)3 | Te | I | Xe(NO3)2 |
CsNO3 | Ba(NO3)2 | Hf | Ta | W | Re | Os | Ir | Pt | Au | Hg2(NO3)2, Hg(NO3)2 |
Tl(NO3)3, TlNO3 |
Pb(NO3)2 | Bi(NO3)3 BiO(NO3) |
Po | At | Rn | |
FrNO3 | Ra(NO3)2 | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |
↓ | |||||||||||||||||
La(NO3)3 | Ce(NO3)3, Ce(NO3)4 |
Pr | Nd(NO3)3 | Pm | Sm | Eu(NO3)3 | Gd(NO3)3 | Tb(NO3)3 | Dy | Ho | Er | Tm | Yb | Lu | |||
Ac(NO3)3 | Th(NO3)4 | Pa | UO2(NO3)2 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr |
Original source: https://en.wikipedia.org/wiki/Curium(III) nitrate.
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