
Curium(III) oxide

Curium(III) oxide is a compound composed of curium and oxygen with the chemical formula . It is a crystalline solid with a unit cell that contains two curium atoms and three oxygen atoms. The simplest synthesis equation involves the reaction of curium(III) metal with O2−: 2 Cm3+ + 3 O2− ---> Cm2O3. Curium trioxide can exist as five polymorphic forms. Two of the forms exist at extremely high temperatures, making it difficult for experimental studies to be done on the formation of their structures. The three other possible forms which curium sesquioxide can take are the body-centered cubic form, the monoclinic form, and the hexagonal form. Curium(III) oxide is either white or light tan in color and, while insoluble in water, is soluble in inorganic and mineral acids. Its synthesis was first recognized in 1955.
Synthesis.
Curium sesquioxide can be prepared in a variety of ways. (Note: Keep in mind that the ways listed below do not contain all of the possible ways in which it can be produced.)
Ignition with O2: Curium(III) oxalate is precipitated through a capillary tube. The precipitate is ignited by gaseous oxygen at 400 °C, and the resulting product is thermally decomposed via 600 °C and 10−4 mm of pressure.
Aerosolized Curium Sesquioxide: The aerosolization process of Cm2O3 can be done through multiple experimental processes. Typically, Cm2O3 is aerosolized for experimental procedures which set out to discover the effects of curium metal within a biological system.
"Route 1:" The traditional aerosolization reaction utilizes curium metal as the starting material. While curium metal has been discovered to naturally exist as a mixture of 87.4% 244Cm, 8.4% 243Cm, 3.9% other curium isotopes, and ~0.3% of the daughter nuclide, plutonium, in most aerosolized syntheses of curium(III) oxide, curium metal is purified through solvent extraction of curium nitrate and "bis"(2-ethylhexyl) phosphoric acid in toluene to remove the plutonium. NH3OH is then added to the purified curium nitrate, and the resulting precipitate is collected and rinsed with deionized water. The precipitate (Cm2O3) is resuspended in solvent and aerosolized with some sort of high output aerosol generator (ex: Lovelace nebulizer).
"Route 2:" In other aerosolizations, instead of the addition of NH3OH to the purified curium nitrate, ammonium hydroxide is utilized to adjust the pH value of the solution to 9. The increased basicity of the solution creates a curium hydroxide precipitate. This precipitate is then collected through filtration and resuspended in deionized water, and a nebulizer is then used to aerosolize the product.
Reduction by Hydrogen Gas: A solution of curium trichloride is evaporated to dryness with pure nitric acid to produce curium nitrate. The curium nitrate is then ignited in air, producing curium oxide, believed to be an intermediate structure between CmO2 and the formation of Cm2O3. The intermediate is scraped into capillary tubes attached to a vacuum system and reduced with gaseous hydrogen - the result of the combustion of UH3.
Obtaining Curium-244: For many of the reactions described above, curium metal is provided by an outside retailer. In order to obtain curium metal, 239Pu metal can be sent through the pile irradiation process described by the radioactive decay processes below (note that neutrons are indicated by the letter "n" and beta-minus particles by "β−"):
239Pu + n ---> 240Pu + n ---> 241Pu + n ---> 242Pu + n ---> 243Pu+ β− ---> 243Am + n ---> 244Am + β− ---> 244Cu.
However, 244curium is one of the more unstable curium isotopes, so any structural data obtained for compounds containing 244Cm may deviate from the expected as a result of structural damage. It has been experimentally determined that, within one day, 244CmO2's lattice parameter increases by a factor of 0.2%. This has been hypothesized to be a result of the weakening interatomic interactions between curium(IV) and the neighboring oxide groups as a result of alpha-decay. This affects the thermal conductivity of curium oxides, causing it to exponentially decrease over time as the effects of alpha-decay strengthen. Abnormal phase transitions have also been reported and have been theorized to be a result of induced self-irradiation, either by 244Cm or the presence of leftover 244Am from incomplete radioactive decay.
Structure.
The body-centered cubic and monoclinic forms are the most common polymorphic forms of curium trioxide, produced by the chemical reactions detailed above. Their crystalline structures are very similar. One of the polymorphs of curium trioxide - the body-centered cubic form - spontaneously transforms to the hexagonal form after several weeks. This transformation is undergone upon spontaneous 244Cm alpha decay, which produces radiation damage effects within the cubic crystal lattice to distort it to that of hexagonal. Although not experimentally proven, there is speculation that monoclinic curium trioxide may be an intermediate form in between the transformation of the cubic form to that of the hexagonal. The body-centered cubic form of curium trioxide exists below temperatures of 800 °C, the monoclinic form between 800 °C and 1615 °C, and the hexagonal form above 1615 °C.
Crystallography.
The lattice parameters for three of the polymorphic structures of curium sesquioxide are given below.
Hexagonal:
Monoclinic:
Cubic:
Data.
Ever since the discovery (and isolation) of 248Cm, the most stable curium isotope, experimental work on the thermodynamic properties of curium sesquioxide (and other curium compounds) has become more prevalent. However, 248Cm can only be obtained in mg samples, so data collection for 248Cm-containing compounds takes longer than that for compounds which predominantly contain other curium isotopes. The data table below reflects a large variety of data collected specifically for curium sesquioxide, some of which is purely theoretical, but most of which have been obtained from 248Cm-compounds.
Toxicology.
Curium metal is a radionuclide and emits alpa particles upon radioactive decay. Although it has a half life of 34 ms, many curium oxides, including curium sesquioxide, have half lives nearing thousands of years. Curium, in the form of curium sesquioxide, can be inhaled into the body, causing many biological defects. The LD50 of curium is 3 micro-Ci through ingestion and inhalation and 1 micro-Ci through absorption through the skin. In one experiment, rats were introduced to aerosolized particulates of curium(III) oxide. Although the experiment proved that inhaled 244Cm2O3 is half as carcinogenic as compared to inhaled 239PuO2, the rats still suffered from many biological deformities, such as skin lesions, malignant tumors, and lung neoplasms. A small amount of the rat population was able to clear particulate curium sesquioxide from the lungs, suggesting that curium sesquioxide is partially soluble in lung fluid.
Applications.
Curium(III) oxide is heavily used in industrial grade-reactions and reagents. As recently as 2009, actinide oxides, such as curium sesquioxide, are being considered for storage uses (in the form of heavily durable ceramic glassware) for the transportation of the light-and-air sensitive fission and transmutation target substances.
Other reactions.
Curium sesquioxide will spontaneously react with gaseous oxygen at high temperatures. At lower temperatures, a spontaneous reaction will occur over a period of time. Curium trioxide reacted with water has been hypothesized to afford a hydration reaction, but little experimentation has been done to prove the hypothesis. Curium sesquioxide has been shown to not react with nitrogen gas, spontaneously or non-spontaneously.