Magnesium (Mg) reacts with water vapor to form magnesium hydroxide and hydrogen gas. The hardening species often cannot be boiled off. The most important source of commercial cesium is a mineral known as pollucite, which usually contains about 5-32% cesium oxide (Cs2O). The equation for the formation of the peroxide is like the sodium equation above: \[ 2K + O_2 \rightarrow K_2O_2 \label{5}\]. Furthermore, the consequences of external exposure to gamma radiation and beta particles are not unique to 137Cs and 134Cs, but are very similar for all gamma and beta emitting radionuclides. The reaction continues even when the solution becomes basic. Reactivity increases as you go down the group; the less reactive metals (lithium, sodium and potassium) are stored in oil (because of its density, lithium floats in oil, but because it is less reactive than the other metals in the group, the thin coating of oil that results is sufficient to prevent reaction). solid cesium reacts with solid cesium nitrite to form solid cesium oxide and nitrogen gas. In the two-electrode vacuum tube converter, caesium neutralizes the space charge near the cathode and enhances the current flow. The unit cell axes are shown in black. The hydroxide ions combine with the bicarbonate ions in the water to produce water and a carbonate ion. Examples include phosphoric acid and sulfuric acid. From this reaction it is apparent that OH- is produced, creating a basic or alkaline environment. It is also used in the catalytic conversion of sulfur dioxide into sulfur trioxide in the production of sulfuric acid.[12]. If you are exposed to cesium, many factors determine whether you'll be harmed. Natural cesium is present in the environment in only one stable form, as the isotope 133Cs. for use in medical devices and gauges. However, the relatively low concentrations of stable cesium do not warrant any immediate steps to reduce exposure. [82], Caesium is also important for its photoemissive properties, converting light to electron flow. Many of these chemical reactions behave in trends that can be categorized using the periodic table. Alkali metals react with oxygen to form monoxides, peroxides, or superoxides. In order to soften the water, water treatment plants add an alkaline earth metal hydroxide, such as slake lime [Ca(OH)2]. \(Be_{(s)}+2H_{2}O_{(l)} \longrightarrow\), \(Ne_{(g)}+2H_{2}O_{(l)} \longrightarrow\), \(Cl_{2\;(g)}+2H_{2}O_{(l)} \longrightarrow\), \(Li_2O_{(s)}+2H_{2}O_{(l)} \longrightarrow\), Metal oxides form basic solutions in water. The oxide forms of each element can be summarized as follows: The more complicated ions are unstable in the presence of a small positive ion. To soften permanent water, sodium carbonate (Na2CO3) is added. One interesting consequence of this is that tin (Sn) is often sprayed as a protective layer on iron cans to prevent the can from corroding. You may be exposed by breathing, eating, or drinking the substance, or by skin contact. A number of people in Brazil, who handled radioactive cesium that was scavenged from a medical machine used for radiation therapy, became sick from exposure to the radiation; a few of them died. The analogous platinum compound, red caesium platinide (Cs 2 Pt), contains the platinide ion that behaves as a pseudo chalcogen. This substance is often used to treat water and to remove harmful \(SO_{2(g)}\) from industrial smokestacks. Name the base. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Why is combustion an exothermic reaction? The products of this reaction include oxygen gas and hydrogen fluoride. Compounds of nitrogen (nitrates and nitrites) as well as nitrogen gas (N2) dissolve in water but do not react. We can write the changes for the Cs atom as, (1) Cs(s) Cs(g); #H_"sub"# = +79 kJ/mol Cesium compounds can travel long distances in the air before being brought back to the earth by rainfall and gravitational settling. All information these cookies collect is aggregated and therefore anonymous. Permanent hard water contains bicarbonate ions (HCO3-) as well as other anions such as sulfate ions (SO4-2). . A small portion is also released in the feces. Similarly to the alkali metal oxides, alkaline earth metal monoxides combine with water to form metal hydroxide salts (as illustrated in the equation below). Furthermore, it is biodegradable and may be recycled, which is important in view of its high cost (about $4,000per barrel in 2001). How can I find the activation energy in potential energy diagrams? Except where otherwise noted, data are given for materials in their, https://en.wikipedia.org/w/index.php?title=Caesium_monoxide&oldid=1070844348, This page was last edited on 9 February 2022, at 15:30. Cesium (chemical symbol Cs) is a soft, flexible, silvery-white metal that becomes liquid near room temperature, but easily bonds with chlorides to create a crystalline powder. Being a heavy element, caesium provides good stopping power with better detection. In the same way, the aluminate, carbonate, or hydroxide may be reduced by magnesium. As mentioned earlier, many Group 1 and Group 2 oxides react with water to form metal hydroxides. Cesium is also used in highly accurate atomic clocks. Caesium iodide (CsI), bromide (CsBr) and caesium fluoride (CsF) crystals are employed for scintillators in scintillation counters widely used in mineral exploration and particle physics research to detect gamma and X-ray radiation. Manfred Bick, Horst Prinz, "Cesium and Cesium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry 2005, Wiley-VCH, Weinheim. Registry (ATSDR). Cesium orthomolybdate Cs 2 MoO 4, together with Cs 2 UO 4 mentioned already, is one of the main components of the joint oxide gain, the multicomponent phase that forms in fast neutrons reactors in the space between fuel and cladding [8-10].Cs 2 MoO 4 shows a phase transition at T tr =(841.31.0) K and melts at T fus =(1229.50.2) K [66].Several authors have measured the vapor pressure . The equation for the formation of the simple oxide is analogous to the lithium equation: \[ 4Na + O_2 \rightarrow 2Na_2O \label{3}\] The peroxide equation is: Cs(s) + O 2 (g) CsO 2 (s) Reaction of caesium with water Sodium Oxide. One notable reaction within this group is aluminum's (Al) reaction with water. [12], Caesium-based atomic clocks use the electromagnetic transitions in the hyperfine structure of caesium-133 atoms as a reference point. Everyone has small amounts of cesium in their body. \[MO_{(s)}+H_2O_{(l)} \longrightarrow M(OH)_{2(s)} \label{6}\]. Consider the peroxide ion, \(O_2^{2-}\), which has the following structure: The covalent bond between the two oxygen atoms is relatively weak. Description. If you need to go back and make any changes, you can always do so by going to our Privacy Policy page. Lithium (and to some extent sodium) form simple oxides, \(X_2O\), which contain the common \(O^{2-}\) ion . Cesium compounds do not react violently with air or water and are generally very soluble in water. Only a little iodine dissolves in water to form a yellowish solution and hypoiodous (\(\ce{HOI}\)) acid has very weak bleaching characteristic. Atlanta, GA: U.S. Department of Health Potassium, rubidium and cesium form superoxides, \(XO_2\). Cesium-137 is produced by nuclear fission for use in medical devices and gauges. '' > Complete ionic and Net ionic /a > chemical equation for each of! As in all equations, it is important they be balanced out. The function of a drilling fluid is to lubricate drill bits, to bring rock cuttings to the surface, and to maintain pressure on the formation during drilling of the well. Because of the increased specific volume of cesium, as compared with the lighter alkali metals, there is a lesser tendency for it to form alloy systems with other metals. The majority of Alkaline Earth Metals also produce hydroxides when reacted with water. Oxides of Group 1 elements also react with water to create basic solutions. 4770 Buford Highway It exhibits polarity and is naturally found in the liquid, solid, and vapor states. [5], Elemental magnesium reduces caesium oxide to elemental caesium, forming magnesium oxide as a side-product:[6][7]. Cesium compounds do not react violently with air or water and are generally very soluble in water. What happens to cesium when it enters the environment? Regulations can be enforced by law. It is difficult to determine if a person has been exposed only to external radiation from radioactive cesium. The concentration of natural cesium in air is generally less than 1 nanogram (1 nanogram equals 1/1,000,000,000 of a gram) per cubic meter of air (ng/m3). Reactivity of the simple Oxides: \(X_2O\), status page at https://status.libretexts.org. Sodium (and to some extent potassium) form peroxides, \(X_2O_2\), containing the more complicated \(O_2^{2-}\) ion. This can give an indication of whether a person has been exposed to levels of cesium that are higher than those normally found in food, water, or air. The discovered haematococcus strains were successful in the removal of up to 50 % of radioactive cesium from low-level contaminated water containing 5 Bq/ ml initial concentration. CESIUM (Data in metric tons of cesium oxide unless otherwise noted) Domestic Production and Use: In 2019, no cesium was mined domestically, and the United States was 100% . Based on eye irritation, the NIOSH has established a recommended exposure limit (REL) for cesium hydroxide of 2 mg/m3 as a timeweighted average (TWA) for up to a 10-hour workday and a 40-hour workweek. Depending on the period of the metal, a different type of oxide is formed when the metal is burned . lithium superoxide sodium superoxide potassium superoxide . Cesium Hydroxide Hydrate is a water soluble Cesium source for use in oxygen-sensitive applications, such as metal production. Scientists have the responsibility to treat research animals with care and compassion. Without laboratory animals, scientists would lose a basic method to get information needed to make wise decisions to protect public health. [16], To obtain a pure sample of caesium, 44,000 litres (9,700impgal; 12,000USgal) of mineral water had to be evaporated to yield 240 kilograms (530lb) of concentrated salt solution. 2004. One curie is the amount of radioactive material in which 37 billion atoms transform every second; this is approximately equivalent to the radioactivity of 1 gram of radium. is also available. Caesium vapour is used in many common magnetometers. 2Cs (s) + 2HO (l) H (g) + 2Cs (aq) + 2OH (aq) The reaction is so explosive that it often shatters the container. Federal Guidance for Radiation Protection. As you go down the Group, the valence electron is further from the nucleus and is screened by more layers of inner electrons. Caesium hydroxide is a very strong base, and will rapidly corrode glass. . Huheey, James E., Ellen A. Keiter, and Richard L. Keiter. General Chemistry: Principles & Modern Applications. As a daughter product of fission bomb testing from the 1950s through the mid-1980s, caesium-137 was released into the atmosphere, where it was absorbed readily into solution. Please click here to see any active alerts. The general reaction for alkali metal hydrides and water is given below: \[MH_{(s)} + H_2O_{(l)} \longrightarrow M^+_{(aq)}+OH^-_{(aq)}+H_{2(g)} \label{4}\]. Caesium (cesium in USA) metal reacts rapidly with water to form a colourless basic solution of caesium hydroxide (CsOH) and hydrogen gas (H2). The hydroxides of calcium, strontium, and barium are only slightly soluble in water; however, enough hydroxide ions are produced to make a basic environment. and in x-ray phosphors. Cesium is like potassium; it enters cells and helps to maintain a balance of electrical charges between the inside and the outside of cells so that cells can perform tasks that depend on those electrical charges. It is an orange solid. Very few applications existed for caesium until the 1920s, when it came into use in radio vacuum tubes, where it had two functions; as a getter, it removed excess oxygen after manufacture, and as a coating on the heated cathode, it increased the electrical conductivity. Internal exposure to Cs-137through ingestion or inhalationallows the radioactive material to be distributed in the soft tissues, especially muscle tissue,which increases cancer risk. Caesium-134, and to a lesser extent caesium-135, have also been used in hydrology to measure the caesium output by the nuclear power industry. Caesium has also been used in thermoluminescent radiation dosimetry (TLD): When exposed to radiation, it acquires crystal defects that, when heated, revert with emission of light proportionate to the received dose. In some examples, the cesium tungsten oxide nanoparticles and zwitterionic stabilizer may be present in the previously mentioned water-based dispersion, which is incorporated (as a pigment. [108] Caesium metal has also been considered as the working fluid in high-temperature Rankine cycle turboelectric generators. Known year-to-year variation within that period allows correlation with soil and sediment layers. The latest versions are more accurate than 1 part in 1015, about 1 second in 20million years. [101][102] Nevertheless, field-emission electric propulsion thrusters that accelerate liquid metal ions such as caesium have been built. Molecular weight: 946.3 Melting point: 4.3 C (decomposes) Cesium sulfates are soluble in water and are thought to be used primarily in water treatment, fuel cells, and to improve optical quality for . Plants and vegetation growing in or nearby contaminated soil may take up small amounts of Cs-137 from the soil. Cesium sulfates are soluble in water and are thought to be used primarily in water treatment, fuel cells, and to improve optical quality for . The nonmetal oxides react with water to form oxoacids. Consequently, cesium is not readily available for uptake by vegetation through roots. The superoxide (\(O_2^-\)) ions are even more easily pulled apart; these are only stable in the presence of the large ions toward the bottom of the group. These factors include the dose (how much), the duration (how long), and how you come in contact with it. Pure cesium metal is silvery white in color and very soft, but pure cesium is not expected to be found in the environment. It forms yellow-orange hexagonal crystals. The hydrogen halides react with water to form hydrohalic acids (\(\ce{HX}\)). For the most part, Group 14 elements do not react with water. Now imagine bringing a small positive ion close to the peroxide ion. From this mixture, the lithium was precipitated by ammonium carbonate. [12] Aqueous solutions of caesium formate (HCOOCs+)made by reacting caesium hydroxide with formic acidwere developed in the mid-1990s for use as oil well drilling and completion fluids. [103], Caesium nitrate is used as an oxidizer and pyrotechnic colorant to burn silicon in infrared flares,[104] such as the LUU-19 flare,[105] because it emits much of its light in the near infrared spectrum. Balanced equation for reaction (smallest integer coefficients): + Name of base: Metal oxides can react with water to form bases. This solution can be evaporated to produce caesium chloride or transformed into caesium alum or caesium carbonate. [69], The price of 99.8% pure caesium (metal basis) in 2009 was about $10 per gram ($280/oz), but the compounds are significantly cheaper. { Compounds : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Hard_Water : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Reactions_in_Aqueous_Solutions : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Reactions_of_Main_Group_Elements_with_Carbonates : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Reactions_of_Main_Group_Elements_with_Halogens : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Reactions_of_Main_Group_Elements_with_Hydrogen : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Reactions_of_Main_Group_Elements_with_Nitrogen : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Reactions_of_Main_Group_Elements_with_Oxygen : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Reactions_of_Main_Group_Elements_with_Water : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "The_s-Block_Elements_in_Biology" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { Elements_Organized_by_Block : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Elements_Organized_by_Group : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Elements_Organized_by_Period : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Main_Group_Reactions : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Periodic_Trends_of_Elemental_Properties : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, Reactions of Main Group Elements with Water, [ "article:topic", "Water", "Halogens", "Hard water", "alkali metals", "showtoc:no", "Noble Gases", "Group 1", "Hydrides", "Oxides", "Carbon Family", "Oxygen Family", "Main Group Elements", "Boron Family", "Alkali Metal Hydrides", "Nitrogen Family", "license:ccbyncsa", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FInorganic_Chemistry%2FSupplemental_Modules_and_Websites_(Inorganic_Chemistry)%2FDescriptive_Chemistry%2FMain_Group_Reactions%2FReactions_of_Main_Group_Elements_with_Water, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\). Cerium(IV) oxide, also known as ceric oxide, ceric dioxide, ceria, cerium oxide or cerium dioxide, is an oxide of the rare-earth metal cerium. We take your privacy seriously. It has a particularly convenient Feshbach spectrum to enable studies of ultracold atoms requiring tunable interactions. L. R. Koller described the first modern photoemissive surface in 192930 as a layer of caesium on a layer of caesium oxide on a layer of silver. ATSDR can also tell you the location of occupational and environmental health clinics. [71] They tried to generate elemental caesium by electrolysis of molten caesium chloride, but instead of a metal, they obtained a blue homogeneous substance which "neither under the naked eye nor under the microscope showed the slightest trace of metallic substance"; as a result, they assigned it as a subchloride (Cs2Cl). Small pieces of potassium heated in air melt and convert instantly into a mixture of potassium peroxide and potassium superoxide without a visible flame. It takes less energy to get the atoms into the vapour phase. In fact, boron (B) does not react at with water. [89] This technology is used primarily in the isolation of viral particles, subcellular organelles and fractions, and nucleic acids from biological samples. [113][114], The median lethal dose (LD50) for caesium chloride in mice is 2.3g per kilogram, which is comparable to the LD50 values of potassium chloride and sodium chloride. \[\ce{Cl2(g) + 2H2O(l) HCl(aq) + HOCl(aq)}\]. In water and moist soils, most cesium compounds are very soluble. Lithium is unique in the group because it also reacts with the nitrogen in the air to form lithium nitride. The halogen gases vary in their reactions with water due to their different electronegativities. [12] Caesium is also used as a source of positive ions in secondary ion mass spectrometry (SIMS). The fuel was ionized by contact with a charged tungsten electrode. CDC is not responsible for Section 508 compliance (accessibility) on other federal or private website. Ballard, James W., Infrared sensitivity of cesium oxide. [80] Caesium clocks regulate the timing of cell phone networks and the Internet.[81]. 2Na(s) + 2H 2 O(l) 2NaOH(aq) . Sometimes these not-to-exceed levels differ among federal organizations because of different exposure times (an 8-hour workday or a 24-hour day), the use of different animal studies, or other factors. The amount of radioactive cesium in food and milk is highly dependent upon several factors. The larger metals form complicated oxides due to energetic factors. Chemical element, symbol Cs and atomic number 55, It differs from this value in caesides, which contain the Cs. Radioactive cesium is released to the environment during the normal operation of nuclear power plants, explosion of nuclear weapons, and accidents involving nuclear power plants or nuclear powered satellites or submarines. [86], The element is used as an internal standard in spectrophotometry. One way to see if a chemical will hurt people is to learn how the chemical is absorbed, used, and released by the body. It is defined by taking the fixed numerical value of the caesium frequency Cs, the unperturbed ground-state hyperfine transition frequency of the caesium-133 atom, to be 9192631770 when expressed in the unit Hz, which is equal to s1. Cesium oxide is a hygroscopic yellow-orange solid that can be reduced to elemental cesium in a reaction with magnesium metal. [12], Caesium-133 can be laser cooled and used to probe fundamental and technological problems in quantum physics. Read the section on the reactions of Cesium with water, and of Cesium Hydroxide with biological materials. External exposure to radiation may occur from natural or man-made sources. Email: Contact CDC-INFO. Similarly to the Group 1 oxides, the hydrides of the Group 1 elements react with water to form a basic solution. Aluminum does not appear to react with water because an outer layer of aluminum oxide (Al2O3) solid forms and protects the rest of the metal. It is one in a series of Public Health Statements about hazardous substances and their health effects. from Wikipedia. The reaction produces a white solid mixture of sodium oxide and sodium peroxide. This technique can form pyramids and regularly shaped etch pits for uses such as Microelectromechanical systems. [110], Nonradioactive caesium compounds are only mildly toxic, and nonradioactive caesium is not a significant environmental hazard. The sublimation energy (1) is the smallest of the alkali metals because the Cs atoms are the biggest. [12], Roasting pollucite with calcium carbonate and calcium chloride yields insoluble calcium silicates and soluble caesium chloride. Nonradioactive (stable) cesium can be neither created nor destroyed under typical environmental conditions, but can react with other compounds found in the environment and change into different cesium compounds. Hydroxide, the OH - anion composed of an oxygen atom bonded to a hydrogen atom, is commonly present in nature and is one of the most widely studied molecules in physical chemistry. Group 1 metals are very reactive, and must be stored out of contact with air to prevent oxidation. Exposure to such a large amount could come from the mishandling of a strongindustrial source of Cs-137, a nuclear detonation or a major nuclear accident. This reaction can be generalized to all alkali metal hydrides. Each atom of 134Cs changes into either xenon 134 (134Xe) or barium 134 (134Ba), neither of which is radioactive, while each atom of 137Cs decays to barium 137 (137Ba), which is also not radioactive. A shorter version, the ToxFAQs, Steel cans are made of tinplate (tin-coated steel) or of tin-free steel. To supply the developing market, Cabot Corporation built a production plant in 1997 at the Tanco mine near Bernic Lake in Manitoba, with a capacity of 12,000 barrels (1,900m3) per year of caesium formate solution. Do not include states. The second, symbol s, is the SI unit of time. This is due to its small size and high ionization energy in relation to the other elements in the group. [75] Applications for nonradioactive caesium included photoelectric cells, photomultiplier tubes, optical components of infrared spectrophotometers, catalysts for several organic reactions, crystals for scintillation counters, and in magnetohydrodynamic power generators. In the presence of sufficient oxygen, the compound which produces the most stable compound is dominant (Table 1). [121][122] Experiments with dogs showed that a single dose of 3.8 millicuries (140MBq, 4.1g of caesium-137) per kilogram is lethal within three weeks;[123] smaller amounts may cause infertility and cancer. Cesium (chemical symbol Cs) is a soft, flexible, silvery-white metal that becomes liquid near room temperature, but easily bonds with chlorides to create a crystalline powder. Is there a medical test to determine whether i have been exposed to cesium? You can review and change the way we collect information below. [12], Most of the mined caesium (as salts) is directly converted into caesium formate (HCOOCs+) for applications such as oil drilling. As 134Cs and 137Cs decay, beta particles and gamma radiation are given off. Water is composed of two hydrogen atoms and an oxygen atom. Using larger amounts of sodium or burning it in oxygen gives a strong orange flame. Recommendations and regulations are also periodically updated as more information becomes available. The largest present-day use of nonradioactive caesium is in caesium formate drilling fluids for the extractive oil industry. Some cesium salts are used in making mineral waters. The catalytic role of cesium with respect to the dissociation of water on surface was investigated, by applying two different adsorption processes at room temperature (RT): (1) The adsorption of water on the cesium .