cesium oxide and water cesium oxide and water

[88] Other uses of the metal include high-energy lasers, vapour glow lamps, and vapour rectifiers. Cesium-137 is produced by nuclear fission for use in medical devices and gauges. . The reaction continues even when the solution becomes basic. 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 information is important because exposure to this substance may harm you and because these sites may be sources of exposure. Similarly to the Group 1 oxides, the hydrides of the Group 1 elements react with water to form a basic solution. The becquerel is a new international unit known as the SI unit, and the curie is an older, traditional unit; both are currently used. The level of cesium in air and water is generally very low. Small pieces of potassium heated in air melt and convert instantly into a mixture of potassium peroxide and potassium superoxide without a visible flame. 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. \[\ce{Cl2(g) + 2H2O(l) HCl(aq) + HOCl(aq)}\]. The other type of hard water is permanent hard water. The equation for the reaction can be written as follow: Caesium => Cs Caesium nitrite => CsNO cesium oxide => CsO nitrogen gas => N Caesium + Caesium nitrite > Caesium oxide + Nitrogen gas Cs + CsNO > CsO + N The most common radioactive form of cesium is Cs-137. 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 . Thus, measuring the light pulse with a photomultiplier tube can allow the accumulated radiation dose to be quantified. Thank you for taking the time to confirm your preferences. [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. Unlike the components of many other heavy liquids, caesium formate is relatively environment-friendly. [79] Caesium clocks have improved over the past half-century and are regarded as "the most accurate realization of a unit that mankind has yet achieved. If you do not allow these cookies we will not know when you have visited our site, and will not be able to monitor its performance. [84][85] Nevertheless, germanium, rubidium, selenium, silicon, tellurium, and several other elements can be substituted for caesium in photosensitive materials.[12]. Caesium monoxide, (Cs2O), often simply Caesium oxide, is the simplest and most common oxide of the caesium. Cesium Oxide is a highly insoluble thermally stable Cesium source suitable for glass, optic and ceramic applications. Larger Group 1 ions have less of an effect on the peroxide ion because of their low charge density. Federal Guidance for Radiation Protection. Compounds of nitrogen (nitrates and nitrites) as well as nitrogen gas (N2) dissolve in water but do not react. 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. How can I find the activation energy in potential energy diagrams? Fissioning that occurs without any outside cause is called "spontaneous fission." \[\ce{I2(g) + 2H2O(l) HI(aq) + HOI(aq)}\]. In the same way, the aluminate, carbonate, or hydroxide may be reduced by magnesium. [106] Caesium compounds may have been used as fuel additives to reduce the radar signature of exhaust plumes in the Lockheed A-12 CIA reconnaissance aircraft. Magnesium (Mg) reacts with water vapor to form magnesium hydroxide and hydrogen gas. 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. Find another reaction Thermodynamic properties of substances The solubility of the substances Periodic table of elements Picture of reaction: oding to search: Cs2O + H2O = 2 CsOH Consequently, cesium is not readily available for uptake by vegetation through roots. The mining and milling of certain ores can also release cesium to the air, water, and soil. [117][118][119] Plants vary widely in the absorption of caesium, sometimes displaying great resistance to it. Exceptionally pure and gas-free caesium can be produced by 390C (734F) thermal decomposition of caesium azide CsN3, which can be produced from aqueous caesium sulfate and barium azide. They have also been used to treat epilepsy. Upper Saddle River, New Jersey 2007. 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. From this reaction it is apparent that OH- is produced, creating a basic or alkaline environment. Cookies used to make website functionality more relevant to you. The radiological impacts in Europe from 137Cs and 134Cs released from the Chernobyl accident, however, were great. The alkaline earth metals were precipitated either as sulfates or oxalates, leaving the alkali metal in the solution. It reacts with oxygen in the air to give white lithium oxide: \[ 4Li + O_2 \rightarrow 2Li_2O \label{1}\]. Cesium compounds can travel long distances in the air before being brought back to the earth by rainfall and gravitational settling. \[ X_2O + H_2O \rightarrow 2X^+_{(aq)} + OH^-_{(aq)} \label{9}\], \[ X_2O + 2HCl \rightarrow 2XCl + H_2O \label{10}\], \[ 2XO_2 + 2H_2O \rightarrow 2XOH + H_2O_2 + O_2 \label{14}\], \[ 2XO_2 + 2HCl \rightarrow 2XCl + H_2O_2 + O_2 \label{15}\]. A shorter version, the ToxFAQs, These cookies allow us to count visits and traffic sources so we can measure and improve the performance of our site. In such cases, follow the advice of public health officials who will publish guidelines for reducing exposure to radioactive material when necessary. Toxicological Predict the products of the following reactions: status page at https://status.libretexts.org, Hydrogen fluoride (HF) and molecular oxygen (O, Birk, James P. "Predicting Inorganic Reactions.". Cs + O 2 CsO 2 . Caesium fluoride enjoys a niche use in organic chemistry as a base[24] and as an anhydrous source of fluoride ion. This substance is often used to treat water and to remove harmful \(SO_{2(g)}\) from industrial smokestacks. The nonmetal oxides react with water to form oxoacids. It was reported that 134Cs (radioactive) has been found in at least 3 of the 1,636 current or former NPL sites and 137Cs (radioactive) has been detected in at least 23 of the 1,636 current or former NPL sites. [12] Caesium is also used as a source of positive ions in secondary ion mass spectrometry (SIMS). Federal organizations that develop recommendations for toxic substances include the Agency for Toxic Substances and Disease Registry (ATSDR), the National Institute for Occupational Safety and Health (NIOSH), and the FDA. These included environmental dispersion of radiocesium and uptake in reindeer, caribou, and livestock. It is one in a series of Public Health Statements about hazardous substances and their health effects. The balanced equation for reaction of solid cesium with liquid water = 2Cs + 2H2O 2CsOH + H2. Cesium is a naturally-occurring element found in rocks, soil, and dust at low concentrations. The two types of hard water include temporary hard water and permanent hard water. This Public Health Statement is the summary chapter from the Toxicological Profile for cesium. [71], From the caesium chloride, the two scientists estimated the atomic weight of the new element at 123.35 (compared to the currently accepted one of 132.9). In this event, the Group 1 metal is oxidized to its metal ion and water is reduced to form hydrogen gas and hydroxide ions. The hydroxides of calcium, strontium, and barium are only slightly soluble in water; however, enough hydroxide ions are produced to make a basic environment. Reactions of Main Group Elements with Water is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. You can be exposed to stable or radioactive cesium by breathing air, drinking water, or eating food containing cesium. \[MO_{(s)}+H_2O_{(l)} \longrightarrow M(OH)_{2(s)} \label{6}\]. The Centers for Disease Control and Prevention (CDC) cannot attest to the accuracy of a non-federal website. Caesium vapour thermionic generators are low-power devices that convert heat energy to electrical energy. You may be exposed by breathing, eating, or drinking the substance, or by skin contact. and in x-ray phosphors. The general reaction of an alkali metal (M) with H2O (l) is given in the following equation: \[\ce{ 2M(s) + 2H2O(l) \longrightarrow 2M^{+}(aq) + 2OH^{-}(aq) + H2 (g)} \]. 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. Lower left: connection pattern of the coordination polyhedra of cesium cations around . If you are exposed to cesium, many factors determine whether you'll be harmed. Plants and animals contain cesium at concentrations of about 1-300 ng/g. The larger metals form complicated oxides due to energetic factors. Consider the peroxide ion, \(O_2^{2-}\), which has the following structure: The covalent bond between the two oxygen atoms is relatively weak. If the substance is radioactive, you may also be exposed to radiation if you are near it. In addition, if babies were to be exposed to enough radiation while in their mothers womb during the time when their nervous system is rapidly developing, they could experience changes in their brains that could result in changes in behavior or decreased mental abilities. cesium tungsten oxideReverso Context-: cesium doped tungsten oxide Context Documents Collaborative Dictionary Expressio Reverso Corporate The most important factor is whether or not there has been recent fallout from a nuclear explosion such as a weapons test or an accident that has occurred at a nuclear power plant. Legal. Why are do we called Group 1 and 2 metals "alkali" and "alkaline"? Oxide compounds are not conductive to electricity. Balanced equation for reaction (smallest integer coefficients): + Name of base: Metal oxides can react with water to form bases. This includes breast milk and pasteurized milk. These cookies may also be used for advertising purposes by these third parties. The process yielded 9.2 grams (0.32oz) of rubidium chloride and 7.3 grams (0.26oz) of caesium chloride from the initial 44,000litres of mineral water. Cesium binds strongly to most soils and does not travel far below the surface of the soil. { 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, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\). Once again, these are strongly exothermic reactions and the heat produced inevitably decomposes the hydrogen peroxide to water and more oxygen. Identification Product Name Caesium hydroxide hydrate Cat No. [72] In 1882, he produced caesium metal by electrolysing caesium cyanide, avoiding the problems with the chloride.[74]. Bromine liquid dissolves slowly in water to form a yellowish-brown solution. Both rubidium and cesium metals ignite in air and produce superoxides, \(RbO_2\) and \(CsO_2\) . The wicked water is now being collected in large tanks that were hastily built near the wrecked reactors. Because of the bright blue lines in the emission spectrum, they derived the name from the Latin word caesius, meaning sky-blue. Man-made sources of radioactive materials are found in consumer products, industrial equipment, atom bomb fallout, and to a smaller extent from hospital waste, medical devices, and nuclear reactors. After conversion to the nitrates and extraction with ethanol, a sodium-free mixture was obtained. Even though it has only a +1 charge, the lithium ion at the top of the group is very small small; therefore it has a high enough charge density that any peroxide ion near it breaks down into an oxide and an oxygen atom. 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. Petrucci, et al. To soften permanent water, sodium carbonate (Na2CO3) is added. Animal testing may also be used to identify health effects such as cancer or birth defects. Potassium, rubidium and cesium form superoxides, \(XO_2\). for use in medical devices and gauges. If you have questions or concerns, please contact your community or state health or environmental quality department or: For more information, contact: 2Cs (s) + 2HO (l) H (g) + 2Cs (aq) + 2OH (aq) The reaction is so explosive that it often shatters the container. In the case of a radioactive chemical, it is also important to gather information concerning the radiation dose and dose rate to the body. It takes less energy to get the atoms into the vapour phase. The high water solubility is a disadvantage which makes it incompatible with large pool irradiators for food and medical supplies. 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. Cookies used to track the effectiveness of CDC public health campaigns through clickthrough data. [77] Caesium formate brine can be blended with potassium and sodium formates to decrease the density of the fluids to that of water (1.0g/cm3, or 8.3pounds per gallon). 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. Lithium (and to some extent sodium) form simple oxides, \(X_2O\), which contain the common \(O^{2-}\) ion . When solid cesium oxide is added to water, you get this equation: Cs2O (s) + H2O (l) --> 2 CsOH (aq) Wiki User 2009-10-25 23:14:05 This answer is: Study guides Chemistry 19 cards To name a. ATSDR can also tell you the location of occupational and environmental health clinics. Some cesium salts are used in making mineral waters. Cesium-137 is used in small amounts for calibration of radiationdetection equipment, such as Geiger-Mueller counters. This page examines the reactions of the Group 1 elements (lithium, sodium, potassium, rubidium and cesium) with oxygen, and the simple reactions of the various oxides formed. [83] The range of photoemissive devices using caesium include optical character recognition devices, photomultiplier tubes, and video camera tubes. To protect the public from the harmful effects of toxic chemicals and to find ways to treat people who have been harmed, scientists use many tests. With the exception of \(\ce{HF}\), the hydrohalic acids are strong acids in water. The most important source of commercial cesium is a mineral known as pollucite, which usually contains about 5-32% cesium oxide (Cs 2 O). So Cs reacts extremely fast and you get an explosion. from Wikipedia. Permanent hard water contains bicarbonate ions (HCO3-) as well as other anions such as sulfate ions (SO4-2). A becquerel is the amount of radioactive material in which 1 atom transforms every second. The most basic oxide, as expected, is cesium oxide, amphoteric oxides have values near zero (water was chosen to calibrate the scale at a value of 0.0). [12] Xenon was used in the experimental spacecraft Deep Space 1 launched in 1998. For the most current information, check with the federal agency or organization that provides it. 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. 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. Common cations in the water include Mg+2 and Ca+2. Secure .gov websites use HTTPS A .gov website belongs to an official government organization in the United States. As in all equations, it is important they be balanced out. It is an anisotropic etchant of silicon, exposing octahedral planes. You must also consider the other chemicals you're exposed to and your age, sex, diet, family traits, lifestyle, and state of health. the anhydride of perchloric acid. The effects of exposure to any hazardous substance depend on the dose, the duration, how you are exposed, personal traits and habits, and whether other chemicals are present. The amount of cesium in drinking water is ordinarily about 1 microgram (1 microgram equals 1/1,000,000 of a gram) per liter of water (g/L). Cesium forms a number of mercury amalgams. Because biochemical processes can confuse and substitute caesium with potassium, excess caesium can lead to hypokalemia, arrhythmia, and acute cardiac arrest, but such amounts would not ordinarily be encountered in natural sources. 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. Many of these chemical reactions behave in trends that can be categorized using the periodic table. This can occur with other alkali metals, but caesium is so potent that this explosive reaction can be triggered even by cold water. The equation for the formation of the simple oxide is analogous to the lithium equation: \[ 4Na + O_2 \rightarrow 2Na_2O \label{3}\], \[ 2Na + O_2 \rightarrow Na_2O_2 \label{4}\]. 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. We can write the changes for the Cs atom as (1) Cs (s) Cs (g); H sub = +79 kJ/mol (2) Cs (g) Cs (g); I 1 = +375.7 kJ/mol [86], The element is used as an internal standard in spectrophotometry. You would probably experience similar effects if you were exposed to any other substance with similar radioactivity. The hydrogen halides react with water to form hydrohalic acids (\(\ce{HX}\)). Some regulations and recommendations for cesium include the following: There are few guidelines for compounds of stable cesium. How can I draw activation energy in a diagram? Heptacesium oxide Formula: Cs7O. Similarly to the alkali metal oxides, alkaline earth metal monoxides combine with water to form metal hydroxide salts (as illustrated in the equation below). Regulations can be enforced by law. These cookies perform functions like remembering presentation options or choices and, in some cases, delivery of web content that based on self-identified area of interests. The species Cs2O forms yellow-orange hexagonal crystals. Do not include states. An estimated 16,461 workers (4,276 of these are female) are potentially exposed to natural cesium and cesium compounds in the United States. [12], The high density of the caesium formate brine (up to 2.3g/cm3, or 19.2pounds per gallon),[77] coupled with the relatively benign nature of most caesium compounds, reduces the requirement for toxic high-density suspended solids in the drilling fluida significant technological, engineering and environmental advantage. Lithium also reacts with the nitrogen in the air to produce lithium nitride and is the only Group 1 element that forms a nitride: \[ 6Li + N_2 \rightarrow 2Li_3N \label{2}\]. It is also well-documented that mushrooms from contaminated forests accumulate radiocaesium (caesium-137) in the fungal sporocarps. SAFETY DATA SHEET Revision Date 21-Feb-2020 Revision Number 2 1. This solid dissolves in the water producing a metal ion (M+2) and hydroxide ions (OH-). [4] Recommendations provide valuable guidelines to protect public health but cannot be enforced by law. This page titled Reactions of Group I Elements with Oxygen is shared under a CC BY-NC 4.0 license and was authored, remixed, and/or curated by Jim Clark. It is known to have a higher selectivity to etch highly p-doped silicon than the more commonly used potassium . You might also experience acute radiation syndrome, which includes such effects as nausea, vomiting, diarrhea, bleeding, coma, and even death. No known taste or odor is associated with cesium compounds. [89] This technology is used primarily in the isolation of viral particles, subcellular organelles and fractions, and nucleic acids from biological samples. "[76] These clocks measure frequency with an error of 2 to 3parts in 1014, which corresponds to an accuracy of 2nanoseconds per day, or one second in 1.4millionyears. The interaction of water with cesium on the strontium titanate surface SrTiO 3 (100), was studied, mainly by means of work function measurements and thermal desorption spectroscopy. To 1.20~molmll have been solid cesium with liquid water balanced equation for sediments ( Comans et al., 1989 ) Large positive affinities. 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. Cesium sulfates are soluble in water and are thought to be used primarily in water treatment, fuel cells, and to improve optical quality for . Agency for Toxic Substances and Disease In order to soften the water, water treatment plants add an alkaline earth metal hydroxide, such as slake lime [Ca(OH)2]. Both the oxide and suboxides are brightly coloured. Cesium reacts with cold water to form hydrogen gas and a solution of cesium ions and hydroxide ions. [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. [12], Caesium-based atomic clocks use the electromagnetic transitions in the hyperfine structure of caesium-133 atoms as a reference point. Its advantages include a half-life of roughly 30 years, its availability from the nuclear fuel cycle, and having 137Ba as a stable end product. The products of this reaction include oxygen gas and hydrogen fluoride. You will be subject to the destination website's privacy policy when you follow the link. The hardening species often cannot be boiled off. Because Cs-137 bonds with chlorides to make a crystalline powder, it reacts in the environment like table salt (sodium chloride): Small quantities of Cs-137 can be found in the environment from nuclear weapons and from nuclear reactor accidents. lithium superoxide sodium superoxide potassium superoxide . A simple oxide ion can be formed if the oxygen atom on the right "breaks off": Hence, the positive ion polarizes the negative ion. JavaScript appears to be disabled on this computer. . The reaction is so explosive that it often shatters the container. 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.