GQ/x480-GeH.jpg' alt='Nfpa 72 2010 Handbook' title='Nfpa 72 2010 Handbook' />Caesium Wikipedia. Caesium,  5. 5Cs. General properties. Pronunciation. SEE zee m. Alternative namecesium US, informalAppearancepale gold. Standard atomic weightAr, standard7. Caesium in the periodic table. Atomic numberZ5. Group, periodgroup 1 alkali metals, period 6. Blocks block. Element category alkali metal. I/510XvDc9uxL.jpg' alt='Nfpa 72 2010 Handbook' title='Nfpa 72 2010 Handbook' />Electron configurationXe 6s. Electrons per shell. Physical properties. Phaseat STPsolid. Melting point. 30. K 2. 8. 5 C, 8. FBoiling point. Dress Up Rush No Time Limit there. K 6. 71 C, 1. FDensitynear r. Critical point. 19. K, 9. 4 MPa2Heat of fusion. Jmol. Heat of vaporization. Jmol. Molar heat capacity. Absolute alcohol, alcohol, cologne spirit, drinking alcohol, ethane monoxide, ethylic alcohol, EtOH, ethyl alcohol, ethyl hydrate, ethyl hydroxide, ethylol, grain. Content Description Get uptodate on industrial machinery safety and compliance with the electronic 2015 NFPA 79 Handbook. Save 15 on the Standard and Handbook Set NFPA 72 National Fire Alarm and Signaling Code helps you save lives with fire detection, signaling, and emergency communications systems that function as intended. ASTM develops technical standards for industry worldwide. Nfpa 72 2010 Handbook' title='Nfpa 72 2010 Handbook' />JmolKVapour pressure. P Pa1. 10. 10. 01 k. T K4. 18. 46. 95. Atomic properties. N,NDIETHYLANILINE C10H15N CID 7061 structure, chemical names, physical and chemical properties, classification, patents, literature, biological activities. Publishes fire and building safety standards including the National Electrical Code. Title II Regulations Supplementary Information. DEPARTMENT OF JUSTICE. CFR Part 35 CRT Docket No. AG Order No. 3180 2010. Yangnla mcadelede 4 altn t 1 Yangn, doal afetler dnda, genelde insan hatasndan dolay meydana gelir. Yangn nlemek. 2Imidazolidinethione is a degradation product of ethylenebisdithiocarbamate fungicides. It has been found to be carcinogenic and to cause THYROID hyperplasia. Content Description For safety around flammable and combustible liquids, using the latest NFPA 30 is the first priority. Enforceable under OSHA and many state and. Oxidation states1, 1 a strongly basic oxideElectronegativity. Pauling scale 0. Ionization energies. Jmol. 2nd 2. 23. Jmol. Jmol. Atomic radiusempirical 2. Covalent radius. 24. Van der Waals radius. Miscellanea. Crystal structurebody centred cubic bcc. Thermal expansion. K at 2. 5 CThermal conductivity. WmKElectrical resistivity. CMagnetic orderingparamagnetic4Youngs modulus. GPa. Bulk modulus. GPa. Mohs hardness. Brinell hardness. MPa. CAS Number. 74. History. Namingfrom Latin caesius, sky blue, for its spectral colours. Discovery. Robert Bunsen and Gustav Kirchhoff1. First isolation. Carl Setterberg1. Main isotopes of caesium. Wikidata. Caesium or cesiumnote 1 is a chemical element with symbol Cs and atomic number 5. It is a soft, silvery gold alkali metal with a melting point of 2. C 8. 3. 3 F, which makes it one of only five elemental metals that are liquid at or near room temperature. Caesium has physical and chemical properties similar to those of rubidium and potassium. The most reactive of all metals, it is pyrophoric and reacts with water even at 1. C 1. 77 F. It is the least electronegative element, with a value of 0. Pauling scale. It has only one stable isotope, caesium 1. Caesium is mined mostly from pollucite, while the radioisotopes, especially caesium 1. The German chemist Robert Bunsen and physicist Gustav Kirchhoff discovered caesium in 1. The first small scale applications for caesium were as a getter in vacuum tubes and in photoelectric cells. In 1. 96. 7, acting on Einsteins proof that the speed of light is the most constant dimension in the universe, the International System of Units used two specific wave counts from an emission spectrum of caesium 1. Since then, caesium has been widely used in highly accurate atomic clocks. Since the 1. 99. 0s, the largest application of the element has been as caesium formate for drilling fluids, but it has a range of applications in the production of electricity, in electronics, and in chemistry. The radioactive isotope caesium 1. Although the element is only mildly toxic, the metals tendency to react violently when in contact with water means that Caesium is considered a hazardous material, and the radioisotopes present a significant health and ecological hazard in the environment. CharacteristicseditPhysical propertiesedit. High purity caesium 1. Caesium is the softest element it has a hardness of 0. Mohs. It is a very ductile, pale metal, which darkens in the presence of trace amounts of oxygen. When in the presence of mineral oil where it is best kept during transport, it loses its metallic lustre and takes on a duller, grey appearance. It has a melting point of 2. C 8. 3. 1 F, making it one of the few elemental metals that are liquid near room temperature. Mercury is the only elemental metal with a known melting point lower than caesium. In addition, the metal has a rather low boiling point, 6. C 1,1. 86 F, the lowest of all metals other than mercury. Its compounds burn with a blue1. Caesium forms alloys with the other alkali metals, gold, and mercury amalgams. At temperatures below 6. C 1,2. 02 F, it does not alloy with cobalt, iron, molybdenum, nickel, platinum, tantalum, or tungsten. It forms well defined intermetallic compounds with antimony, gallium, indium, and thorium, which are photosensitive. It mixes with all the other alkali metals except lithium the alloy with a molar distribution of 4. C 1. 08 F. 1. A few amalgams have been studied Cs. Hg. 2 is black with a purple metallic lustre, while Cs. Hg is golden coloured, also with a metallic lustre. Chemical propertiesedit. Addition of a small amount of caesium to cold water is explosive. Caesium metal is highly reactive and very pyrophoric. It ignites spontaneously in air, and reacts explosively with water even at low temperatures, more so than the other alkali metals first group of the periodic table. It reacts with solid water at temperatures as low as 1. C 1. 77 F. 1. Because of this high reactivity, caesium metal is classified as a hazardous material. It is stored and shipped in dry, saturated hydrocarbons such as mineral oil. It can be handled only under inert gas, such as argon. However, a caesium water explosion is often less powerful than a sodium water explosion with a similar amount of sodium. This is because caesium explodes instantly upon contact with water, leaving little time for hydrogen to accumulate. Caesium can be stored in vacuum sealed borosilicate glassampoules. In quantities of more than about 1. The chemistry of caesium is similar to that of other alkali metals, in particular rubidium, the element above caesium in the periodic table. As expected for an alkali metal, the only common oxidation state is 1. Some small differences arise from the fact that it has a higher atomic mass and is more electropositive than other nonradioactive alkali metals. Caesium is the most electropositive chemical element. The caesium ion is also larger and less hard than those of the lighter alkali metals. Compoundsedit. Ball and stick model of the cubic coordination of Cs and Cl in Cs. Cl. Most caesium compounds contain the element as the cation. Cs, which binds ionically to a wide variety of anions. One noteworthy exception is the caeside anion Cs, and others are the several suboxides see section on oxides below. Salts of Cs are usually colourless unless the anion itself is coloured. Many of the simple salts are hygroscopic, but less so than the corresponding salts of lighter alkali metals. The phosphate,2. Double salts are often less soluble, and the low solubility of caesium aluminium sulfate is exploited in refining Cs from ores. The double salt with antimony such as Cs. Sb. Cl. 4, bismuth, cadmium, copper, iron, and lead are also poorly soluble. Caesium hydroxide Cs. OH is hygroscopic and strongly basic. It rapidly etches the surface of semiconductors such as silicon. Cs. OH has been previously regarded by chemists as the strongest base, reflecting the relatively weak attraction between the large Cs ion and OH 1. Arrhenius base, but a number of compounds that do not dissolve in water, such as n butyllithium and sodium amide,2. A stoichiometric mixture of caesium and gold will react to form yellow caesium auride CsAu upon heating. The auride anion here behaves as a pseudohalogen. The compound reacts violently with water, yielding caesium hydroxide, metallic gold, and hydrogen gas in liquid ammonia it can be reacted with a caesium specific ion exchange resin to produce tetramethylammonium auride. The analogous platinum compound, red caesium platinide Cs. Pt, contains the platinide ion that behaves as a pseudochalcogen.