cesium oxide and water

Sodium carbonate precipitates out the Mg+2 and Ca+2 ions out as the respective metal carbonates and introduces Na+ ions into the solutions. Division of Toxicology and Human Health Sciences 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. Cookies used to make website functionality more relevant to you. This information is important because this substance may harm you. CESIUM (Data in metric tons of cesium oxide unless otherwise noted) Domestic Production and Use: In 2020, no cesium was mined domestically, and the United States was 100% . Caesium fluoride or caesium aluminium fluoride are used in fluxes formulated for brazing aluminium alloys that contain magnesium. [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. The majority of Alkaline Earth Metals also produce hydroxides when reacted with water. Sodium (and to some extent potassium) form peroxides, \(X_2O_2\), containing the more complicated \(O_2^{2-}\) ion. We can write the changes for the Cs atom as, (1) Cs(s) Cs(g); #H_"sub"# = +79 kJ/mol Federal Guidance for Radiation Protection. 2Cs(s) + 2HO(l) H(g) + 2Cs(aq) + 2OH(aq). Group 1 metals are very reactive, and must be stored out of contact with air to prevent oxidation. Thus, measuring the light pulse with a photomultiplier tube can allow the accumulated radiation dose to be quantified. With the exception of beryllium (Be), the alkaline metal hydrides react with water to produce the metal hydroxide and hydrogen gas. Industrial gauges that detect the flow of liquid through pipes. 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). [109], Caesium salts have been evaluated as antishock reagents following the administration of arsenical drugs. 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. This release does not always lead to exposure. Everyone has small amounts of cesium in their body. Annual Limits on Intake (ALIs) for on-the-job exposure are 100 Ci (1x102 Ci) for 134Cs and 200 Ci (2x102 Ci) for 137Cs. The remaining 90% has a biological half-life between 50 and 150 days. However, this only applies to the lower half of the group, in which the metal ions are large and have a low charge density. [80] Caesium clocks regulate the timing of cell phone networks and the Internet.[81]. All information these cookies collect is aggregated and therefore anonymous. Caesium oxide is used in photocathodes to detect infrared signals in devices such as image intensifiers, vacuum photodiodes, photomultipliers, and TV camera tubes [3] L. R. Koller described the first modern photoemissive surface in 1929-30 as a layer of caesium on a layer of caesium oxide on a layer of silver. 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. [120] Accumulation of caesium-137 in lakes has been a great concern after the Chernobyl disaster. 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. No known taste or odor is associated with cesium compounds. The most common radioactive form of cesium is Cs-137. Its polarity makes it a good solvent and is commonly known as the universal solvent. People who work in industries that process or use natural cesium or cesium compounds can be exposed to higher-than-normal levels of cesium. Sodium is the alkali element that reacts most violently with water. Radioactive decay decreases the concentration of 134Cs and 137Cs. Radiocaesium does not accumulate in the body as readily as other fission products (such as radioiodine and radiostrontium). solid cesium reacts with solid cesium nitrite to form solid cesium oxide and nitrogen gas. If you work in the nuclear power industry, you may also be exposed to higher-than-normal levels of radioactive cesium, but there are many precautionary measures taken at these facilities to minimize this exposure. 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. [68] The primary smaller-scale commercial compounds of caesium are caesium chloride and nitrate. 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. Now imagine bringing a small positive ion close to the peroxide ion. 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 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. 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. Your doctor might need to ask your state health department to investigate. A simple oxide ion can be formed if the oxygen atom on the right "breaks off": Hence, the positive ion polarizes the negative ion. It exhibits polarity and is naturally found in the liquid, solid, and vapor states. The wicked water is now being collected in large tanks that were hastily built near the wrecked reactors. The nonmetal oxides react with water to form oxoacids. 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. Beryllium (Be) is the only alkaline earth metal that does not react with water. [12] Xenon was used in the experimental spacecraft Deep Space 1 launched in 1998. Cesium binds strongly to most soils and does not travel far below the surface of the soil. No known taste or odor is associated with cesium compounds. . [101][102] Nevertheless, field-emission electric propulsion thrusters that accelerate liquid metal ions such as caesium have been built. 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. The second, symbol s, is the SI unit of time. Pure cesium metal is silvery white in color and very soft, but pure cesium is not expected to be found in the environment. [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. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. With the exception of \(\ce{HF}\), the hydrohalic acids are strong acids in water. The resulting surface is bright and shiny. Legal. What recommendations has the federal government made to protect human health? 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. A common characteristic of most Alkali Metals is their ability to displace H2(g) from water. The general reaction of calcium, strontium, and barium with water is represented below, where M represents calcium, strontium, or barium: \[M_{(s)} + 2H_2O_{(l)} \longrightarrow M(OH)_{2(aq)}+H_{2\;(g)} \label{5}\]. [110], Nonradioactive caesium compounds are only mildly toxic, and nonradioactive caesium is not a significant environmental hazard. 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. Hypobromous (\(\ce{HOBr}\)) acid is a weak bleaching agent. The energy input steps (1) and (2) are related to the activation energy of the reaction. 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. It is an important commercial product and an intermediate in the purification of the element from the ores. Cesium oxide is a hygroscopic yellow-orange solid that can be reduced to elemental cesium in a reaction with magnesium metal. The lower the activation energy, the faster the reaction. Above: Extended unit cell of Cs 18 Hg 8 O 6 in a projection approximately along a.Green cubes depict the [Hg 8] 6 anions, oxide anions are drawn as red spheres, cesium cations as blue spheres. [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. 2Na(s) + 2H 2 O(l) 2NaOH(aq) . The unit cell axes are shown in black. How can I draw a simple energy profile for an exothermic reaction in which 100 kJ mol-1 is Why is the respiration reaction exothermic? It is used in photoelectric cells because caesium-based cathodes, such as the intermetallic compound K2CsSb, have a low threshold voltage for emission of electrons. Larger pieces of potassium produce a lilac flame. 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). Historically, the most important use for caesium has been in research and development, primarily in chemical and electrical fields. The sublimation energy (1) is the smallest of the alkali metals because the Cs atoms are the biggest. External exposure to radiation may occur from natural or man-made sources. These included environmental dispersion of radiocesium and uptake in reindeer, caribou, and livestock. The larger metals form complicated oxides due to energetic factors. Other industrial devicesthat measure the thickness of materials such as paper or sheets of metal. You must also consider the other chemicals you're exposed to and your age, sex, diet, family traits, lifestyle, and state of health. Lithium also reacts with the nitrogen in the air to produce lithium nitride and is the only Group 1 element that forms a nitride: \[ 6Li + N_2 \rightarrow 2Li_3N \label{2}\]. Permanent hard water contains bicarbonate ions (HCO3-) as well as other anions such as sulfate ions (SO4-2). At the top of the group, the small ions with a higher charge density tend to polarize the more complicated oxide ions to the point of disintegration. 2Cs (s) + 2HO (l) H (g) + 2Cs (aq) + 2OH (aq) The reaction is so explosive that it often shatters the container. 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. [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. Alkali metals are also known to react violently and explosively with water. Preparation. Larger Group 1 ions have less of an effect on the peroxide ion because of their low charge density. Caesium hydroxide is a very strong base, and will rapidly corrode glass. If the substance is radioactive, you may also be exposed to radiation if you are near it. 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. Naturally-occurring cesium occurs in the environment mostly from the erosion and weathering of rocks and minerals. Health professionals examining people who have health problems similar to those resulting from radiation exposure would need to rely on additional information, such as the testing of blood samples for cell counts and chromosomal damage, in order to establish if such people had been affected by being near a source of radioactivity. 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 It is difficult to determine if a person has been exposed only to external radiation from radioactive cesium. Similarly to the Group 1 oxides, the hydrides of the Group 1 elements react with water to form a basic solution. Temporary hard water contains bicarbonate (HCO3-) which forms CO3-2(aq), CO2(g), and H2O when heated. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. The first accurate caesium clock was built by Louis Essen in 1955 at the National Physical Laboratory in the UK. Once cesium enters your body, your kidneys begin to remove it from the blood; some cesium is quickly released from your body in the urine. Write an equation to show how cesium oxide can react with water to form a base. '' > Complete ionic and Net ionic /a > chemical equation for each of! Depending on the period of the metal, a different type of oxide is formed when the metal is burned . The latest versions are more accurate than 1 part in 1015, about 1 second in 20million years. Will the following reaction create an acidic or basic solution? [82], Caesium is also important for its photoemissive properties, converting light to electron flow. [86], The element is used as an internal standard in spectrophotometry. 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. A .gov website belongs to an official government organization in the United States. Special radiation detectors can be used to detect if a person has absorbed radioactive cesium. The most common radioactive form of cesium is Cs-137. [69], Alternatively, caesium metal may be obtained from the purified compounds derived from the ore. Caesium chloride and the other caesium halides can be reduced at 700 to 800C (1,292 to 1,472F) with calcium or barium, and caesium metal distilled from the result. Upper Saddle River, New Jersey 2007. Potassium, rubidium and cesium form superoxides, \(XO_2\). 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. Caesium was not recognized as a high-performance industrial metal until the 1950s. The equation for the formation of the peroxide is like the sodium equation above: \[ 2K + O_2 \rightarrow K_2O_2 \label{5}\]. Chloride into water 2. zinc acetate and cesium /a > 1 strontium react with liquid water = 2Cs + ! Hypochlorous (\(\ce{HOCl}\)) acid is a strong bleaching agent and is not very stable in solution and readily decomcomposes, especially when exposed to sunlight, yielding oxygen. Common cations in the water include Mg+2 and Ca+2. How can I calculate the activation energy of a reaction? However, the number of sites evaluated for cesium is not known. Official websites use .gov Studies utilizing metal oxides adsorbents such as titanium oxide are well documented [32], [33], . Cesium binds strongly to soil and concrete, but does not travel very far below the surface. Secure .gov websites use HTTPS Legal. [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). The federal government develops regulations and recommendations to protect public health. Because of its abundance on earth, it is important to note that it is involved in many chemical reactions. [12], Magnetohydrodynamic (MHD) power-generating systems were researched, but failed to gain widespread acceptance. The reaction produces a white solid mixture of sodium oxide and sodium peroxide. Medical radiation therapy devices for treating cancer. Cesium forms a number of mercury amalgams. The equation for the formation of the simple oxide is analogous to the lithium equation: \[ 4Na + O_2 \rightarrow 2Na_2O \label{3}\], \[ 2Na + O_2 \rightarrow Na_2O_2 \label{4}\]. So Cs reacts extremely fast and you get an explosion. Details of the supplier of the safety data sheet It forms yellow-orange hexagonal crystals. Some cesium salts are used in making mineral waters. Both stable and radioactive cesium are the same element and behave in a similar manner chemically and in the body. As more sites are evaluated, the sites at which cesium is found may increase. [117][118][119] Plants vary widely in the absorption of caesium, sometimes displaying great resistance to it. It reacts with oxygen in the air to give white lithium oxide: \[ 4Li + O_2 \rightarrow 2Li_2O \label{1}\]. It combines quickly with oxygen in the air and reacts violently with water. [17], The isotopes 134 and 137 are present in the biosphere in small amounts from human activities, differing by location. Quantities of radioactive cesium, as well as other radioactive elements, are measured in units of mass (grams) or radioactivity (curies or becquerels). From this mixture, the lithium was precipitated by ammonium carbonate. Short exposure to extremely large amounts of radiation might cause nausea, vomiting, diarrhea, bleeding, coma, and even death. This section discusses potential health effects from exposures during the period from conception to maturity at 18 years of age in humans. Consider the peroxide ion, \(O_2^{2-}\), which has the following structure: The covalent bond between the two oxygen atoms is relatively weak. It is also well-documented that mushrooms from contaminated forests accumulate radiocaesium (caesium-137) in the fungal sporocarps. Cells like muscle cells and nerve cells require changing electrical charges in order to function properly and allow you to think and move. Animal testing may also be used to identify health effects such as cancer or birth defects. Cesium sulfates are soluble in water and are thought to be used primarily in water treatment, fuel cells, and to improve optical quality for . As you go down the Group, the valence electron is further from the nucleus and is screened by more layers of inner electrons. . Many of these chemical reactions behave in trends that can be categorized using the periodic table. For the most part, Group 14 elements do not react with water. cesium tungsten oxideReverso Context-: cesium doped tungsten oxide Context Documents Collaborative Dictionary Expressio Reverso Corporate 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. How can I find the activation energy in potential energy diagrams? Regulations can be enforced by law. The high water solubility is a disadvantage which makes it incompatible with large pool irradiators for food and medical supplies. These species react with water in different ways: \[\ce{M2O(s) + 2H2O(l) \longrightarrow 2M^{+}(aq) + 2OH^{-} (aq)} \label{1}\], \[\ce{M2O2(s) + 2H2O(l) \longrightarrow 2M^{+}(aq) + 2OH^{-} (aq) + H2O2(aq)} \label{2}\], \[\ce{2MO2 (s) + 2H2O(l) \longrightarrow 2M^{+}(aq) + 2OH^{-} (aq) + H2O2 (aq) + O2(g)} \label{3}\]. For the most current information, check with the federal agency or organization that provides it. The pure elements in this family do not tend to react with water. Water is composed of two hydrogen atoms and an oxygen atom. Plants and animals contain cesium at concentrations of about 1-300 ng/g. The hydrogen halides react with water to form hydrohalic acids (\(\ce{HX}\)). Name the base. 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. Burning caesium in excess oxygen will produce caesium superoxide. Why are do we called Group 1 and 2 metals "alkali" and "alkaline"? Rubidium and cesium are typically stored in sealed glass tubes to eliminate contact with air. Linking to a non-federal website does not constitute an endorsement by CDC or any of its employees of the sponsors or the information and products presented on the website. [78] Alkali formates are safe to handle and do not damage the producing formation or downhole metals as corrosive alternative, high-density brines (such as zinc bromide ZnBr2 solutions) sometimes do; they also require less cleanup and reduce disposal costs. and Human Services, Public Health Service. \[\ce{Cl2(g) + 2H2O(l) HCl(aq) + HOCl(aq)}\]. These sites make up the National Priorities List (NPL) and are the sites targeted for long-term federal cleanup activities. Agency for Toxic Substance and Disease Registration. 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). Why are different oxides formed as you go down the Group? How does the activation energy affect reaction rate? The halogen gases vary in their reactions with water due to their different electronegativities. 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. The ionization energy (2) is the smallest of the alkali metals. Caesium fluoride enjoys a niche use in organic chemistry as a base[24] and as an anhydrous source of fluoride ion. Atlanta, GA: U.S. Department of Health This public health statement tells you about cesium and the effects of exposure. 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. The reactions are the same in oxygen and in air, but oxygen will generate a more violent reaction. It reacts with water to form hydrogen peroxide and caesium . Cesium is a naturally-occurring element found in rocks, soil, and dust at low concentrations. [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. Both superoxides are described as either orange or yellow, but rubidium superoxide can also be dark brown. Because of their effect on heart rhythms, however, they are less likely to be used than potassium or rubidium salts. However, the relatively low concentrations of stable cesium do not warrant any immediate steps to reduce exposure. Toxicological 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 Examples include phosphoric acid and sulfuric acid. 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. [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. It is an orange solid. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. 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. : 13233 CAS-No 12260-45-6 Synonyms No information available Recommended Use Laboratory chemicals. Reactivity of the simple Oxides: \(X_2O\), status page at https://status.libretexts.org. [12] The caesium standard is the primary standard for standards-compliant time and frequency measurements. Stable (not radioactive) cesium (133Cs) has been identified in at least 8 of the 1,636 hazardous waste sites that have been proposed for inclusion on the EPA National Priorities List (NPL) (HazDat 2003). 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. [92] Caesium salts sometimes replace potassium or sodium salts in organic synthesis, such as cyclization, esterification, and polymerization. After reduction of the hexachloroplatinate with hydrogen, caesium and rubidium were separated by the difference in solubility of their carbonates in alcohol. 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. The alkaline earth metals were precipitated either as sulfates or oxalates, leaving the alkali metal in the solution. You might also experience acute radiation syndrome, which includes such effects as nausea, vomiting, diarrhea, bleeding, coma, and even death. [12], Caesium-based atomic clocks use the electromagnetic transitions in the hyperfine structure of caesium-133 atoms as a reference point. [12], Caesium-133 can be laser cooled and used to probe fundamental and technological problems in quantum physics. Radioactive forms of cesium are produced by the fission of uranium in fuel elements (fuel rods) during the normal operation of nuclear power plants, or when nuclear weapons are exploded. sodium + water sodium hydroxide + hydrogen. Cesium compounds can travel long distances in the air before being brought back to the earth by rainfall and gravitational settling. [72] In 1882, he produced caesium metal by electrolysing caesium cyanide, avoiding the problems with the chloride.[74]. Once again, these are strongly exothermic reactions and the heat produced inevitably decomposes the hydrogen peroxide to water and more oxygen. 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. About 10% of absorbed radiocaesium washes out of the body relatively quickly in sweat and urine. 2XO2 + 2H2O 2XOH + H2O2 + O2 { 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, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\). 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