Ceric ammonium nitrate

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Ammonium cerium(IV) nitrate
Ammonium cerium(IV) nitrate
Names
IUPAC name
Diammonium cerium(IV) nitrate
Other names
Ceric ammonium nitrate (CAN)
Identifiers
16774-21-3
ChemSpider 157072
EC number 240-827-6
Jmol-3D images Image
PubChem 180504
Properties
H8N8CeO18
Molar mass 548.26 g/mol
Appearance orange-red crystals
Melting point 107 to 108 °C (225 to 226 °F; 380 to 381 K)
141 g/100 mL (25 °C)
227 g/100 mL (80 °C)
Structure
Crystal structure Monoclinic
Icosahedral
Related compounds
Related compounds
Ammonium nitrate
Cerium(IV) oxide
Except where noted otherwise, data is given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
Infobox references

Ceric ammonium nitrate (CAN) is the inorganic compound with the formula (NH4)2Ce(NO3)6. This orange-red, water-soluble cerium salt is a specialised oxidizing agent in organic synthesis and a standard oxidant in quantitative analysis.

Preparation, properties, and structure[edit]

The anion [Ce(NO
3
)
6
]2−
is generated by dissolving Ce
2
O
3
in hot concentrated HNO3.

The salt consists of the anion [Ce(NO
3
)
6
]2−
and a pair of NH4+ counter ions. The ammonium ions are not involved in the oxidising reactions of this salt. In the anion each nitrate group is chelated to the cerium atom in a bidentate manner as shown below:

Hexanitratocerate anion

The anion [Ce(NO
3
)
6
]2−
has idealized Oh molecular symmetry. The CeO12 core defines an icosahedron.[1]

Ce4+ is a strong one-electron oxidizing agent. In terms of its redox potential (E° ~ 1.61 V vs. N.H.E.) it is even stronger oxidizing agent than Cl2 (E° ~ 1.36 V). Few shelf-stable reagents are stronger oxidants. In the redox process Ce(IV) is converted to Ce(III), a one-electron change, signaled by the fading of the solution color from orange to a pale yellow (providing that the substrate and product are not strongly colored).

Applications in organic chemistry[edit]

In organic synthesis, CAN is useful as an oxidant for many functional groups (alcohols, phenols, and ethers) as well as C–H bonds, especially those that are benzylic. Alkenes undergo dinitroxylation, although the outcome is solvent-dependent. Quinones are produced from catechols and hydroquinones and even nitroalkanes are oxidized.

CAN provides an alternative to the Nef reaction; for example, for ketomacrolide synthesis where complicating side reactions usually encountered using other reagents. Oxidative halogenation can be promoted by CAN as an in situ oxidant for benzylic bromination, and the iodination of ketones and uracil derivatives.

For the synthesis of heterocycles[edit]

Catalytic amounts of aqueous CAN allow the efficient synthesis of quinoxaline derivatives. Quinoxalines are known for their applications as dyes, organic semiconductors, and DNA cleaving agents. These derivatives are also components in antibiotics such as echinomycin and actinomycin. The CAN-catalyzed three-component reaction between anilines and alkyl vinyl ethers provides an efficient entry into 2-methyl-1,2,3,4-tetrahydroquinolines and the corresponding quinolines obtained by their aromatization.

As a deprotection reagent[edit]

CAN is traditionally used to release organic ligands from metal carbonyls. In the process, the metal is oxidised, CO is evolved, and the organic ligand is released for further manipulation.[2]

CAN is used to convert para-methoxybenzyl and 3,4-dimethoxybenzyl ethers, which are protecting groups for alcohols.[3][4] Two equivalents of CAN are required for each equivalent of para-methoxybenzyl ether. The alcohol is released, and the para-methoxybenzyl ether converts to para-methoxybenzaldehyde. The balanced equation is as follows:

2 (NH4)2Ce(NO3)6 + H3COC6H4CH2OR + H2O → 4 NH4+ + 2 Ce3+ + 12 NO3 + 2 H+ + H3COC6H4CHO + HOR

Other applications[edit]

CAN is also a component of chrome etchant,[5] a material that is used in the production of photomasks and liquid crystal displays.

References[edit]

  1. ^ Thomas A. Beineke; J. Delgaudio (1968). "Crystal structure of ceric ammonium nitrate". Inorg. Chem. 7 (4): 715–721. doi:10.1021/ic50062a020.  edit
  2. ^ L. Brener, J. S. McKennis, and R. Pettit "Cyclobutadiene in Synthesis: endo-Tricyclo[4.4.0.02,5]deca-3,8-diene-7,10-dione" Org. Synth. 1976, 55, 43.doi:10.15227/orgsyn.055.0043
  3. ^ Boons, Geert-Jan.; Hale, Karl J. (2000). Organic Synthesis with Carbohydrates (1st ed.) Sheffield, England: Sheffield Academic Press. pp.33
  4. ^ Kocienski, Phillip J. (1994). Protecting Groups Stuttgart, New York Georg Thieme Verlag. pp 8-9, 52-54
  5. ^ Walker, Perrin; William H. Tarn (1991). CRC Handbook of Metal Etchants. pp. 287–291. ISBN 0-8493-3623-6. 

External links[edit]