Search results
Results from the WOW.Com Content Network
Few compounds of californium have been made and studied. [1] The only californium ion that is stable in aqueous solutions is the californium(III) cation. [2] The other two oxidation states are IV (strong oxidizing agents) and II (strong reducing agents). [3]
Californium is a silvery-white actinide metal [12] with a melting point of 900 ± 30 °C (1,650 ± 50 °F) and an estimated boiling point of 1,743 K (1,470 °C; 2,680 °F). [13] The pure metal is malleable and is easily cut with a knife. Californium metal starts to vaporize above 300 °C (570 °F) when exposed to a vacuum. [14]
This page was last edited on 23 October 2017, at 22:37 (UTC).; Text is available under the Creative Commons Attribution-ShareAlike 4.0 License; additional terms may apply.
Californium(III) oxide forms a yellow-green solid with a melting point of 1750 °C and exists in three modifications. [2] The body-centered cubic modification forms a crystal lattice with a = 1083.9 ± 0.4 pm. The transition temperature between body-centered cubic and monoclinic structures is about 1400 °C. [3] [4] It is insoluble in water. [5]
The Serbian Wikipedia (Serbian: Википедија на српском језику, Vikipedija na srpskom jeziku) is the Serbian-language version of the free online encyclopedia Wikipedia. Created on 16 February 2003, it reached its 100,000th article on 20 November 2009 before getting to another milestone with the 200,000th article on 6 July ...
Californium(IV) oxide is a black-brown solid that has a cubic fluorite crystal structure with a lattice parameter, the distance between unit cells in the crystal, of 531.0 ± 0.2 pm. Crystals of californium(III) oxide normally have a body-centered cubic symmetry. They convert to a monoclinic form upon heating to about 1400 °C and melt at 1750 °C.
Californium oxychloride (Cf OCl) is a radioactive salt first discovered in measurable quantities in 1960. It is composed of a single californium cation and oxychloride consisting of one chloride and one oxide anion. It was the first californium compound ever isolated. [1]
This occurs because of the much greater lattice energy afforded by the more highly charged Ca 2+ cation compared to the hypothetical Ca + cation. [10] Calcium, strontium, barium, and radium are always considered to be alkaline earth metals; the lighter beryllium and magnesium, also in group 2 of the periodic table, are often included as well.