cesium oxide and water

The equation for the formation of the peroxide is like the sodium equation above: \[ 2K + O_2 \rightarrow K_2O_2 \label{5}\]. An official website of the United States government. 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.". [72] In 1882, he produced caesium metal by electrolysing caesium cyanide, avoiding the problems with the chloride.[74]. 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. It has a particularly convenient Feshbach spectrum to enable studies of ultracold atoms requiring tunable interactions. The carbonate ion then precipitates out with the metal ion to form MCO3(s). Only a little iodine dissolves in water to form a yellowish solution and hypoiodous (\(\ce{HOI}\)) acid has very weak bleaching characteristic. [5], Elemental magnesium reduces caesium oxide to elemental caesium, forming magnesium oxide as a side-product:[6][7]. Balanced equation for reaction (smallest integer coefficients): + Name of base: Metal oxides can react with water to form bases. The sublimation energy (1) is the smallest of the alkali metals because the Cs atoms are the biggest. How can I find the activation energy in potential energy diagrams? and in x-ray phosphors. [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. Forming complicated oxides from the metals releases more energy and makes the system more energetically stable. Depending on the period of the metal, a different type of oxide is formed when the metal is burned . 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. Crystalline cesium iodide and cesium fluoride are used in scintillation counters, which convert energy from ionizing radiation into pulses of visible light for radiation detection and spectroscopy. Some of the cesium that your body absorbs can remain in your body for weeks or months, but is slowly eliminated from your body through the urine and feces. Laws today protect the welfare of research animals, and scientists must comply with strict animal care guidelines. and Human Services, Public Health Service. [12] Caesium is also used as a source of positive ions in secondary ion mass spectrometry (SIMS). Similarly to the alkali metal oxides, alkaline earth metal monoxides combine with water to form metal hydroxide salts (as illustrated in the equation below). Uses advised against Food, drug, pesticide or biocidal product use. This includes breast milk and pasteurized milk. Cesium sulfates are soluble in water and are thought to be used primarily in water treatment, fuel cells, and to improve optical quality for . [82], Caesium is also important for its photoemissive properties, converting light to electron flow. But corrosion by caesium on spacecraft components has pushed development in the direction of inert gas propellants, such as xenon, which are easier to handle in ground-based tests and do less potential damage to the spacecraft. A becquerel is the amount of radioactive material in which 1 atom transforms every second. Sodium carbonate precipitates out the Mg+2 and Ca+2 ions out as the respective metal carbonates and introduces Na+ ions into the solutions. 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. [91] Doping with caesium compounds enhances the effectiveness of several metal-ion catalysts for chemical synthesis, such as acrylic acid, anthraquinone, ethylene oxide, methanol, phthalic anhydride, styrene, methyl methacrylate monomers, and various olefins. The hydrogen halides react with water to form hydrohalic acids (\(\ce{HX}\)). The larger metals form complicated oxides due to energetic factors. 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. It is also used in the catalytic conversion of sulfur dioxide into sulfur trioxide in the production of sulfuric acid.[12]. The level of cesium in air and water is generally very low. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. In water and moist soils, most cesium compounds are very soluble. JavaScript appears to be disabled on this computer. You might also experience acute radiation syndrome, which includes such effects as nausea, vomiting, diarrhea, bleeding, coma, and even death. [77], Caesium metal is one of the most reactive elements and is highly explosive in the presence of water. The resulting surface is bright and shiny. The pure elements in this family do not tend to react with water. Cesium compounds do not react violently with air or water and are generally very soluble in water. Its reduced derivative . Oxides of Group 1 elements also react with water to create basic solutions. Both the oxide and suboxides are brightly coloured. : 13233 CAS-No 12260-45-6 Synonyms No information available Recommended Use Laboratory chemicals. In larger amounts, Cs-137 is used in: External exposure to large amounts of Cs-137 can cause burns, acute radiation sickness and even death. Permanent hard water contains bicarbonate ions (HCO3-) as well as other anions such as sulfate ions (SO4-2). The half-life of 134Cs is about 2 years and the half-life of 137Cs is about 30 years. [80] Caesium clocks regulate the timing of cell phone networks and the Internet.[81]. Granites contain an average cesium concentration of about 1 part of cesium in a million parts of granite (ppm) and sedimentary rocks contain about 4 ppm. The second, symbol s, is the SI unit of time. The reaction produces a white solid mixture of sodium oxide and sodium peroxide. For the most part, Group 14 elements do not react with water. It is also well-documented that mushrooms from contaminated forests accumulate radiocaesium (caesium-137) in the fungal sporocarps. is also available. Chloride into water 2. zinc acetate and cesium /a > 1 strontium react with liquid water = 2Cs + ! General Chemistry: Principles & Modern Applications. Regulations and recommendations can be expressed in not-to-exceed levels in air, water, soil, or food that are usually based on levels that affect animals; they are then adjusted to help protect people. Agency for Toxic Substance and Disease Registration. (2) Cs(g) Cs(g); #I_1# = +375.7 kJ/mol Cerium(III) oxide, also known as cerium oxide, cerium trioxide, cerium sesquioxide, cerous oxide or dicerium trioxide, is an oxide of the rare-earth metal cerium. 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. Scientists have the responsibility to treat research animals with care and compassion. Radioactive isotopes are constantly decaying or changing into different isotopes by giving off radiation. Historically, the most important use for caesium has been in research and development, primarily in chemical and electrical fields. In the reaction with water, hydrogen gas is released. Both rubidium and cesium metals ignite in air and produce superoxides, \(RbO_2\) and \(CsO_2\) . Since 1967, the International System of Measurements has based the primary unit of time, the second, on the properties of caesium. Your doctor might need to ask your state health department to investigate. From: Epitaxial Growth of Complex Metal Oxides, 2015 Related terms: Nanoparticle ZnO Al2O3 Metal Oxide Conductivity Oxide Nanostructured Material Oxygen Vacancy View all Topics Download as PDF Set alert 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. 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. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. The two types of hard water include temporary hard water and permanent hard water. Caesium monoxide, (Cs2O), often simply Caesium oxide, is the simplest and most common oxide of the caesium. Cesium-137 is used in small amounts for calibration of radiationdetection equipment, such as Geiger-Mueller counters. It is a pale yellow-white powder with the chemical formula CeO 2. Using larger amounts of sodium or burning it in oxygen gives a strong orange flame. What happens to cesium when it enters the environment? 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). The Environmental Protection Agency (EPA) identifies the most serious hazardous waste sites in the nation. ( III ) oxide reacts with Lithium to form solid calcium hydroxide phosphoric. Sometimes cesium is used as a getter for residual gas impurities in vacuum tubes and as a coating in tungsten filaments or cathodes of the tubes. Cesium reacts with cold water to form hydrogen gas and a solution of cesium ions and hydroxide ions. The first accurate caesium clock was built by Louis Essen in 1955 at the National Physical Laboratory in the UK. [12], Caesium-133 can be laser cooled and used to probe fundamental and technological problems in quantum physics. 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. For some chemicals, animal testing may be necessary. profile for cesium, Agency for Toxic Substances and Disease Registry, U.S. Department of Health & Human Services. You can be exposed to stable or radioactive cesium by breathing air, drinking water, or eating food containing cesium. Ballard, James W., Infrared sensitivity of cesium oxide. \(Be_{(s)}+2H_{2}O_{(l)} \longrightarrow\), \(Ne_{(g)}+2H_{2}O_{(l)} \longrightarrow\), \(Cl_{2\;(g)}+2H_{2}O_{(l)} \longrightarrow\), \(Li_2O_{(s)}+2H_{2}O_{(l)} \longrightarrow\), Metal oxides form basic solutions in water. Now imagine bringing a small positive ion close to the peroxide ion. [4] It is a good electron emitter; however, its high vapor pressure limits its usefulness. In the case of a radioactive chemical, it is also important to gather information concerning the radiation dose and dose rate to the body. Animals given very large doses of cesium compounds have shown changes in behavior, such as increased activity or decreased activity, but it is highly unlikely that you would breathe, eat, or drink amounts of stable cesium large enough to cause similar effects. On average, a person swallows about 10 g of stable cesium per day in food and water, and breathes about 0.025 g per day. Manfred Bick, Horst Prinz, "Cesium and Cesium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry 2005, Wiley-VCH, Weinheim. Read the section on the reactions of Cesium with water, and of Cesium Hydroxide with biological materials. This Public Health Statement is the summary chapter from the Toxicological Profile for cesium. Small pieces of potassium heated in air melt and convert instantly into a mixture of potassium peroxide and potassium superoxide without a visible flame. SAFETY DATA SHEET Revision Date 21-Feb-2020 Revision Number 2 1. The fuel was ionized by contact with a charged tungsten electrode. Cookies used to enable you to share pages and content that you find interesting on CDC.gov through third party social networking and other websites. This is most effective if the positive ion is small and highly charged (if it has a high charge density, or a lot of charge packed into a small volume). [4] However, the relatively low concentrations of stable cesium do not warrant any immediate steps to reduce exposure. Similarly to the Group 1 oxides, the hydrides of the Group 1 elements react with water to form a basic solution. [12], Most of the mined caesium (as salts) is directly converted into caesium formate (HCOOCs+) for applications such as oil drilling. It takes less energy to get the atoms into the vapour phase. Cs + O 2 CsO 2 . Reactivity of the simple Oxides: \(X_2O\), status page at https://status.libretexts.org. Upper Saddle River, New Jersey 2007. Name the base. Cesium oxide is a hygroscopic yellow-orange solid that can be reduced to elemental cesium in a reaction with magnesium metal. Completion fluids assist the emplacement of control hardware after drilling but prior to production by maintaining the pressure. The resulting solution is basic because of the dissolved hydroxide. It forms yellow-orange hexagonal crystals. The analogous platinum compound, red caesium platinide (Cs 2 Pt), contains the platinide ion that behaves as a pseudo chalcogen. This information is important because this substance may harm you. As in all equations, it is important they be balanced out. [12] The caesium standard is the primary standard for standards-compliant time and frequency measurements. Identification Product Name Caesium hydroxide hydrate Cat No. When a substance is released from a large area, such as an industrial plant, or from a container, such as a drum or bottle, it enters the environment. Legal. Alkali metals react with oxygen to form monoxides, peroxides, or superoxides. 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. In such cases, follow the advice of public health officials who will publish guidelines for reducing exposure to radioactive material when necessary. This technique can form pyramids and regularly shaped etch pits for uses such as Microelectromechanical systems. External exposure to radiation may occur from natural or man-made sources. The exception to this general assumption is beryllium, whose oxide (BeO) does not react with water. If you were to breathe, eat, drink, touch, or come close to large amounts of radioactive cesium, cells in your body could become damaged from the radiation that might penetrate your entire body, much like x-rays, even if you did not touch the radioactive cesium. A .gov website belongs to an official government organization in the United States. The most important source of commercial cesium is a mineral known as pollucite, which usually contains about 5-32% cesium oxide (Cs 2 O). Do not include states. Laboratories use special techniques to measure the amount of cesium in body fluids such as blood and urine, as well as in feces or other human samples. Consequently, cesium is not readily available for uptake by vegetation through roots. Petrucci, et al. We take your privacy seriously. Temporary hard water contains bicarbonate (HCO3-) which forms CO3-2(aq), CO2(g), and H2O when heated. Compounds of nitrogen (nitrates and nitrites) as well as nitrogen gas (N2) dissolve in water but do not react. Because of its abundance on earth, it is important to note that it is involved in many chemical reactions. Registry (ATSDR). Radiocaesium does not accumulate in the body as readily as other fission products (such as radioiodine and radiostrontium). 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 . [17], The isotopes 134 and 137 are present in the biosphere in small amounts from human activities, differing by location. The reaction is so explosive that it often shatters the container. [12], Caesium-based atomic clocks use the electromagnetic transitions in the hyperfine structure of caesium-133 atoms as a reference point. With the exception of beryllium (Be), the alkaline metal hydrides react with water to produce the metal hydroxide and hydrogen gas. If your doctor finds that you have been exposed to significant amounts of cesium, ask whether your children might also be exposed. and in x-ray phosphors. Caesium oxide (IUPAC name) or cesium oxide describes inorganic compounds composed of caesium and oxygen. profile for cesium. The unit cell axes are shown in black. Friestad, Gregory K.; Branchaud, Bruce P.; Navarrini, Walter and Sansotera, Maurizio (2007) "Cesium Fluoride" in, General Conference on Weights and Measures, International Union of Pure and Applied Chemistry, "NIST Radionuclide Half-Life Measurements", "History of the recommended atomic-weight values from 1882 to 1997: a comparison of differences from current values to the estimated uncertainties of earlier values", "C&EN: It's Elemental: The Periodic Table Cesium", "Density of melts of alkali metals and their Na-K-Cs and Na-K-Rb ternary systems", "A Basic Rule of Chemistry Can Be Broken, Calculations Show", "Caesium in high oxidation states and as a p-block element", "Forcing Cesium into Higher Oxidation States Using Useful hard x-ray Induced Chemistry under High Pressure", "Effects of relativistic motion of electrons on the chemistry of gold and platinum", "Single-atom electron energy loss spectroscopy of light elements", "The Crystal Structure of Cesium Monoxide", "Nucleosynthesis in Asymptotic Giant Branch Stars: Relevance for Galactic Enrichment and Solar System Formation", IEER Report: Transmutation Nuclear Alchemy Gamble, Chernobyl's Legacy: Health, Environmental and Socia-Economic Impacts and Recommendations to the Governments of Belarus, Russian Federation and Ukraine, "Transmutation of Cesium-137 Using Proton Accelerator", "Distribution of the elements in some major units of the Earth's crust", 10.1130/0016-7606(1961)72[175:DOTEIS]2.0.CO;2, "Cesium as a Raw Material: Occurrence and Uses", "The Tanco Pegmatite at Bernic Lake, Manitoba: X. Pollucite", "Lithium, cesium, and rubidiumThe rare alkali metals", "Cesium formate fluid succeeds in North Sea HPHT field trials", "Chemische Analyse durch Spectralbeobachtungen", "Ueber die Darstellung von Rubidium- und Csiumverbindungen und ber die Gewinnung der Metalle selbst", "Cesium Supplier & Technical Information", "The material flow of radioactive cesium-137 in the U.S. 2000", "IsoRay's Cesium-131 Medical Isotope Used In Milestone Procedure Treating Eye Cancers At Tufts-New England Medical Center", "Level and density measurement using non-contact nuclear gauges", "Isotope Tracers Project Resources on Isotopes Cesium", "A Synopsis of Ion Propulsion Development Projects in the United States: SERT I to Deep Space I", "Infrared illumination compositions and articles containing the same", "Accumulation of potassium, rubidium and caesium (, "IAEA director warns of 'dirty bomb' risk", View the reaction of Caesium (most reactive metal in the periodic table) with Fluorine (most reactive non-metal), https://en.wikipedia.org/w/index.php?title=Caesium&oldid=1137590149, Chemical elements with body-centered cubic structure, Short description is different from Wikidata, Creative Commons Attribution-ShareAlike License 3.0, This page was last edited on 5 February 2023, at 13:01. Larger Group 1 ions have less of an effect on the peroxide ion because of their low charge density. 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. Oxides of Group 1 elements also react with water to create basic solutions. Lithium also reacts with the nitrogen in the air to produce lithium nitride and is the only Group 1 element that forms a nitride: \[ 6Li + N_2 \rightarrow 2Li_3N \label{2}\]. This can occur with other alkali metals, but caesium is so potent that this explosive reaction can be triggered even by cold water. 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. Caesium hydroxide is a very strong base, and will rapidly corrode glass. These factors include the dose (how much), the duration (how long), and how you come in contact with it. "[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. [92] Caesium salts sometimes replace potassium or sodium salts in organic synthesis, such as cyclization, esterification, and polymerization. Cesium compounds can travel long distances in the air before being brought back to the earth by rainfall and gravitational settling. Beryllium (Be) is the only alkaline earth metal that does not react with water. An estimated 16,461 workers (4,276 of these are female) are potentially exposed to natural cesium and cesium compounds in the United States. Reaction of caesium with air Caesium (cesium in USA) is very soft and easily cut. This solid dissolves in the water producing a metal ion (M+2) and hydroxide ions (OH-). The International System of Units (SI) defines the second as the duration of 9,192,631,770 cycles at the microwave frequency of the spectral line corresponding to the transition between two hyperfine energy levels of the ground state of caesium-133. [12], It is highly pyrophoric: the autoignition temperature of caesium is 116C (177F), and it ignites explosively in air to form caesium hydroxide and various oxides. Studies utilizing metal oxides adsorbents such as titanium oxide are well documented [32], [33], . Bromine liquid dissolves slowly in water to form a yellowish-brown solution. In the two-electrode vacuum tube converter, caesium neutralizes the space charge near the cathode and enhances the current flow. (3) Cs(g) Cs(aq); #H_"hydr"# = -276 kJ/mol. Phone: 1-800-CDC-INFO 888-232-6348 (TTY) 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). Cesium oxide react with water Cs 2 O + H 2 O 2CsOH [ Check the balance ] Cesium oxide react with water to produce cesium hydroxide. The bicarbonate ions react with alkaline earth cations and precipitate out of solution, causing boiler scale and problems in water heaters and plumbing. In the presence of sufficient oxygen, the compound which produces the most stable compound is dominant (Table 1). Oxide compounds are not conductive to electricity. Though not commercially feasible, the ore can be directly reduced with potassium, sodium, or calcium in vacuum to produce caesium metal directly. Federal agencies that develop regulations for toxic substances include the Environmental Protection Agency (EPA), the Occupational Safety and Health Administration (OSHA), the Food and Drug Administration (FDA), and the U.S. Nuclear Regulatory Commission (USNRC). 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. If you need to go back and make any changes, you can always do so by going to our Privacy Policy page. A shorter version, the ToxFAQs, Thank you for taking the time to confirm your preferences. [12], The high density of the caesium ion makes solutions of caesium chloride, caesium sulfate, and caesium trifluoroacetate (Cs(O2CCF3)) useful in molecular biology for density gradient ultracentrifugation. Why are do we called Group 1 and 2 metals "alkali" and "alkaline"? { 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, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\). Toxicological The half-life is the time it takes for half of that cesium isotope to give off its radiation and change into a different element. The equation for the formation of the simple oxide is analogous to the lithium equation: \[ 4Na + O_2 \rightarrow 2Na_2O \label{3}\], \[ 2Na + O_2 \rightarrow Na_2O_2 \label{4}\].