化学专业英语 翻译了7

• • 无机物的制备 例题Lithium and sodium are produced from their molten chlorides by electrolysis.The electrolysis of NaCl is carried out about 6000C. The melting point of NaCl is 8010C,too high a temperature to carry out this electrolysis economically.Adding CaCl2 to the mixture reduces the melting point. • 例题Potassium metal is produced by the reduction of molten KCl by liquid sodium • .KCl+Na→NaCl+K • Reaction is reversible at low temperatures.At 8500C,however,the equilibrium is displaced far to the right as K escapes from the molten mixture • Because sodium is so reactive ,its most important use is as a reducing agent in obtaining metals such as titanium,zirconium and hafnium. 例题In the chemical industry,NaCl is a source of many chemicals,including sodium metal,chlorine gas,hydrochloric acid,and sodium hydroxide. [hai'drɔksaid] • 例题Potassium chloride is obtained from naturally occurring brines(concentrated solutions of salts).It is most extensively used in plant fertilizers because potassium is a major essential element for plant growth.[brain] 盐水 • 例题KCl is also used as a raw material in the manufacture of KOH,KNO3,and other industrially important potassium compounds（Potassium nitrate） • 例题Sodium carbonate is used primarily in the manufacture of glass.The NaCO3 produced in the United States now comes mostly from natural sources,such as the mineral trona,NaCO3.NaHCO3.nH2O. • In the past sodium carbonate was manufactured mostly from NaCl,CaCO3,and NH3,using a process introduced by the Belgian chemist Ernest Solvay in 1863. • ['trəunə]天然碱 • 例题The sodium bicarbonate can be isolated and converted to sodium carbonate by heating Sodium hydrogen carbonate • 例题Sodium sulfate :is obtain partly from natural sources,partly from neutralization reactions,and partly through a process discovered by Johann Rudolf Glauber in 1625. • H2SO4(concd)+NaCl(s) → NaSO4(s)+HCl(g) • The strategy behind reactions is the production of a volatile acid(HCl) by heating one of its salts(NaCl) with a nonvolatile acid(H2SO4) ['vɔlətail] • 例题Na2S is produced by the reduction of NaSO4 with carbon • NaSO4+C→ Na2S+CO . • 例题Sodium hydroxides is produced commercially by the electrolysis of NaCl. Cl- is oxidized to Cl2;and H2O is reduced to H2. • Alkali metal hydroxides can also be prepared by the reaction of the group1 metals with water. • 例题The preferred method of producing the group 2 metals(except Mg)is by reducing their salts with other active metals. • beryl is the natural source of beryllium compounds.This mineral is processed to produce BeF2,which is then reduced with Mg. 例题Calcium and magnesium are particularly abundant.Even beryllium,the least abundant member of group 2,is accessible because it occurs in deposits of the mineral beryl,3BeO.Al2O3.6SiO2。绿柱石 • 例题Calcium,strontium,and barium are obtained by the reduction of their oxides with aluminum; • Ca and Sr also can be obtained by electrolysis of their molten chlorides. • 例题Magnesium metal is obtained by electrolysis of the molten chloride in the Dow process .The source of magnesium is seawater or natural brines. • The abundance of Mg in seawater is about 1350mg/L. 例题Preparation of magnesium。The first step is the precipitation of Mg(OH)2 with slaked lime Ca(OH)2 as the source of OH-. Slaked lime is formed by the reaction of quicklime CaO with water. The precipitated Mg(OH)2 is washed,filtered,and dissolved in HCl.The resulting concentrated MgCl2 is dried by evaporation, melted,and electrolyzed,yielding pure Mg metal and Cl2.The Cl2 is converted to HCl,which is recycled. 例题Calcium metal is used primarily as a reducing agent to prepare,from their oxides or fluorides,other metals such as U,Pu,and most of the lanthanides. [lænθə`naid]镧系元素 • 例题Three steps are required to obtain pure CaCO3 from limestone(1)thermal decomposition of limestone(2)reaction of CaO with water and (3)conversion of an aqueous suspension of Ca(OH)2 to precipitated CaCO3.悬浮液 • 例题CaO called quicklime is produced by the calcination of limestone.This reaction is reversible at room temperature;the reverse reaction occurs almost exclusively. • So in the calcination of CaCO3,a high temperature must be used and the CO2 produced must be continuously exhausted from the furnace in which the reaction occurs. • The most familiar is CaCO3,the principal component of the rock limestone.If a limestone contains more than 5%MgCO3,it is usually called dolomite. • The primary use of limestone(about 70%)is as a building stone.Among other applications,limestone is used in the manufacture of quicklime and slaked lime. • 生石灰和熟石灰 白云石 ['dɔləmait] 例题The most important metal of the group is aluminum.The third most abundant element,aluminum comprises 8.3% by mass of Earth’s solid crust. • The chief ore,bauxite,contains Fe2O3 as an impurity that must be removed.The principle used in the separation is that Al2O3 is an amphoteric oxide and dissolves in NaOH,whereas the iron oxide is a basic oxide and does not. [æmfə`terik]两性的 铝土矿 [`bɔ:k,saɪt] • When the solution containing [Al(OH)4]- is slightly acidified,Al(OH)3 precipitates.Pure Al2O3 is obtained by heating the Al(OH)3. • Al2O3 can be dissolved in the molten mineral cryolite,Na3AlF6,at about 10000C.The liquid is a good electrical conductor,so the electrolysis of Al2O3 is accomplished in molten cryolite. Hexafluoroaluminate [`kraiəulait ]冰晶石 例题Aluminum sulfate is the most important aluminum compound used commercially.It is prepared by the reaction of hot concentrated H2SO4 on Al2O3.The product that crystallizes from solution is Al2(SO4)3.18H2O.octadecahydrate • When an aqueous solution of equimolar amounts of Al2(SO4)3 and K2SO4 is allowed to crystallize,the crystals obtained are of potassium aluminum sulfate,KAl(SO4).12H2O.This is just one of a large class of double salts called alums. • Dodecahydrate 明矾 [ə`lʌm] • 例题The chief tin ore is tin(IV),SnO2,known as cassiterite. • After purification,the tin(IV)oxide is reduced with carbon to produce tin metal. [kə`sitə,rait]锡石矿 • Tin forms two primary oxides,SnO and SnO2.By heating SnO in air, it can be converted to SnO2.One use of SnO2 is as a jewelry abrasive. • Both chlorides of tin—SnCl2 and SnCl4__ have important uses.Tin(II) chloride,SnCl2 is a good reducing agent and is used in the quantitative analysis iron ores to reduce Fe(III) to Fe (II) in aqueous solution. • Tin(IV) chloride SnCl4 is formed by the direct reaction of tin and Cl2 ;it is the form in which tin is recovered from scrap tinplate.Tin (II) fluride SnF2 (stannous fluoride),has an important use as an anticavity additive to toothpaste. 预防蛀牙 • 例题Lead is found chiefly as lead(II) sulfide PbS,an ore known as galena. • The lead(II) sulfide is first converted to lead(II) oxide by strongly heating it in air,a process called roasting.焙烧 The oxide is then reduced with coke to produce the metal.焦炭 [ɡə`li:nə]方铅矿 • One of the few soluble lead compounds is lead(II) nitrate Pb(NO3)2.It is formed in the reaction of PbO2 with nitric acid. • Pb(IV) compounds tend to undergo reduction to compounds of Pb(II) and therefore good oxidizing agents.PbO2 is a better oxidizing agent than Cl2 and nearly as good as MnO4-.PbO2 can oxidize HCl to Cl2. • Addition of a soluble chromate salt to Pb(NO3)2 produces the pigment lead chromate .Another lead –based pigment used in ceramic glazes and once extensively used in the manufacture of paint is white lead,a basic lead carbonate 例题For zinc ,the commercially important ores are ZnCO3(smithsonite)and ZnS(sphalerite). [sfælərait]闪锌矿['smiθsənait]菱锌矿。 • ZnCO3 decomposes to ZnO and CO2 when it is strongly heated.When strongly heated in air,ZnS reacts with O2,producing ZnO and SO2.The reduction of ZnO is carried out at about 11000C in which C(coke) or CO act as reducing agents. • 例题Titanium metal cannot be produced by reduction of TiO2 with carbon because the metal and carbon react to form titanium carbides. The first step in the production of Ti is the conversion of rutile ore (TiO2) to TiCl4 by reaction with carbon and Cl2. 金红石['ru:ti:l] • TiO2+2C +2Cl2 →TiCl4+2CO • The purified TiCl4 is reduced to Ti with a good reducing agent.The kroll process uses Mg. • TiCl4+2Mg → Ti+2MgCl2 • The MgCl2 is removed and electrolyzed to produce Cl2 and Mg,which are recycled in reactions,respectively. • The Ti is obtained as a fused mass called titanium sponge. • The kroll process is slow;because it requires high-temperature vacuum distillation to remove the Mg and MgCl2 from the titanium. • Recently ,an electrolytic process has been suggested for the production of Ti from rutile. TiO2 are placed at the cathode of an electrolytic cell containing molten calcium chloride,The Ti(IV) is reduced at the cathode. • 例题The most important compound of vanadium is the pentoxide,V2O5, used mainly as a catalyst,as in the conversion of SO2 to SO3 in the contact method for the manufacture of sulfuric acid. [və`neidiəm] 例题A better source of chromium compounds than the pure metal is the alkali metal chromates,which contain Cr(VI) and can be obtained directly from chromite ore . Fe(CrO2)2 [`krəumait]铬铁矿 • 4Fe(CrO2)2+8Na2CO3+7O2→ 2Fe2O3+8Na2CrO4+8CO2 • The sodium chromate produced by this reaction is the source of many industrially important chromium compounds. • I t is possible to crystallize a dichromate salt from from a water solution of CrO3.If the solution is made basic,the color turns from orange to yellow. • Fom basic solutions,only chromate salts can be crystallized.Thus whether a solution cotains Cr(VI) as Cr2O72-or CrO42- or a mixture of the two depends on the PH. • The forward reaction of is favored in acidic solutions and the predominant Cr(VI) species is Cr2O72-. • In basic solution,H+ ions are removed and the reverse is favored,forming CrO42-as the principal species,Careful control of the PH is necessary when Cr2O72- is used as an oxidizing agent or CrO42- as a precipitating agent. 2CrO42-+2H+→ Cr2O72-+H2O • Chromium ion in basic solution can be used to precipitate metal chromates such as BaCrO4 and PbCrO4. It is not a good oxidizing agent, it is not readily reduced. • Dichromates are easily reduced to Cr2O3.In the case of ammonium dichromate, simply heating the compound produces Cr2O3 in a dramatic reaction. • Pure Cr can be obtained in small amounts by reducing Cr2O3 with Al in a reaction similar to be thermite reaction. • 例题Manganese is a fairly abundant element,cnstituting about 1%of Earth’s crust.Its principal ore is pyrolusite软锰矿,MnO2.Like V and Cr,Mn is most important in steel production as the iron-manganese alloy. Ferromanganese can be obtained by the reduction of a mixture of pyrolusite and hematite （['hɛmə,taɪt ]赤铁矿 ）iron ores with carbon. • MnO2+Fe2O3+5C → Mn+2Fe+5CO • [fɛro'mæŋgə,nis] [词典释义] 【冶】铁锰合金 • Mn participates in the purification of iron by reacting with sulfur and oxygen and removing them through slag formation. • In addition,Mn increases the hardness of steel.Steel containing high proportions of Mn is extremely tough and wear-resistant • Manganese dioxide is used in dry cell batteries ,in glass and ceramic glazes, and as a catalyst; I is also the principal source of manganese compounds . • When MnO2 is heated in the presence of an alkali and an oxidizing agent,a manganate salt is produced. 3MnO2+6KOH+KClO3→ 3K2MnO4+KCl+3H2O • K2MnO4 is extracted from the fused mass with water and then be oxidized to KMnO4 potassium permanganate. • Potassium permanganate is an important laboratory oxidizing agent.I t is generally used in acidic solutions in which it is reduced to Mn2+. • In the analysis of iron by MnO4-,a sample of Fe2+ is prepared by dissolving iron in an acid and reducing any Fe3+back to Fe2+.Then the sample is titrated with MnO4- 例题Bromine can be extracted from seawater or from inland brine solutions.The seawater or brine solution is adjusted to pH3.5 and treated with Cl2,which oxidizes Br-to Br2 in this displacement reaction • Certain marine plants,such as seaweed,absorb and concentrate I- selectively in the presence of Cl- and Br-. • Iodine is obtaied in small quantities from such plants . • Another abundant natural source of iodine is NaIO3,found in large deposits in chile. • Iodate • Because the oxidation state of iodine must be reduced from +5 in IO3- to 0 in I2,the conversion of IO3- to I2 requires the use of a reducing agent.Aqueous sodium hydrogen sulfite (bisulfite) is used as the reducing agent in the first step ,followed by the reaction of I- with additional IO3-to produce I2. • IO3-+3HSO3-→ I-+3SO42-+3H+ • 5I-+IO3-+6H+ → 3I2+3H2O • In aqueous solution ,they are called the hydrohalic acids.Excepts for HF,hydrohalic acids are strong acids in water. [`haidrə`hælik] [`hælaid] • Hydrogen fluoride Hydrogen halides HF hydrogen fluoride HCl hydrogen chloride HBr hydrogen bromide HI hydrogen iodide H2S hydrogen sulfide HCl: hydrochloric acid HBr Hydrobromic acid HCl: hydrochloric acid HBr hydrobromic acid HI hydroionic acid HF hydrofluoric acid When a halide salt (such as fluorite,CaF2)is heated with a nonvolatile acid,such as concentrated H2SO4,a sulfate salt and the volatile hydrogen halide are produced The method works for preparing HCl (g)but not for HBr or HI.That is because concentrated H2SO4 is a sufficiently strong oxidizing agent to oxidize Br- to Br2and I- to I2. • 2NaBr+2H2SO4 → Na2SO4+2H2O+Br2+SO2 • With H2 and Cl2 ,the reaction proceeds rapidly explosively in the presence of light,and some HCl is made this way commercially. • With Br2 and I2,the reaction occurs more slowly and a catalyst is required. • An easily prepared oxidizing agent for use in the laboratory is an aqueous solution of chlorine.The solutions is not just one of Cl2, • The Cl2 disproportionates into HOCl and HCl. HClO （hypochlorous acid） • HOCl is an effective germicide used in water purification and the treatment of swimming pools.Aqueous solutions of hypochlorite salts(NaOCl) are used as common household bleaches. [haipəu`klɔ:rait ] • Chlorine dioxide is an important bleach for paper and fibers.Its reduction with peroxide ion in aqueous solution produces chlorite salt.sodium chlorite is used as a bleaching agent for textiles.[`klɔ:rait ] • Chlorate salts form when Cl2 disproportionates in hot, concentrated alkaline solutions. • Hypochlorites form in cold ,dilute alkaline solutions. [klɔ:rit] 氯酸盐 • Chlorate are good oxidizing agents.Solid chlorates produce oxygen gas when they decompose ,which makes them useful in matchs and fireworks. • A simple laboratory method of producing O2 involves heating KClO3 in the presence of MnO2,a catalyst. • 2KClO3→ 2KCl+3O2 • Perchlorate salts are prepared mainly by electrolyzing chlorate solutions.Oxidation of ClO3- occurs at a Pt anode .platinum [`æn,əʊd] • Compared with the other oxoacid salts,perchlorates are relatively stable. • They do not disproportionate,because no oxidation state higher than +7 is available to chlorine. • At elevated temperature or in the presence of a readily oxidizable compound,perchlorate salts may react explosively. • Mixtures of ammonium perchlorate and powdered aluminum are utilized as the propellant in some solid rockets,such as those used on the space shuttle.航天飞机 • Ammonium perchlorate is especially dangerous to handle,because an explosive reaction may occur when the oxidizing agent ClO4- acts on the reducing agent NH4+ • 例题The main commercial methods of producing SO2 are the direct combustion of sulfur and the roasting of metal sulfides.(ZnS) • In the presence of a catalyst,SO2 is converted to SO3 • The main use of SO2 is in the systhesis SO3 to make sulfuric acid H2SO4. • In the modern process,the contact process SO2 is formed by the direct combustion of sulfur and the roasting of metal sulfides. • Then sulfur trioxide is produced by oxidizing SO2 in an exothermic ,reversible reaction.Reaction occurs very slowly unless catalyzed. • The principal catalyst is V2O5mixed with alkali metal sulfates.The catalysis involves adsorption of SO2and O2 on the catalyst,followed by reaction at active sites and desorption of SO3. • SO3 reacts with water to form H2SO4. The SO3 readily dissolves in the sulfuric acid and reacts with the small amount water present to increase the concentration of the sulfuric acid.The result is a form of sulfuric acid sometimes called oleum but more commonly called fuming sulfuric acid. [əuliəm ]发烟硫酸 When SO2 reacts with water,it produces H2SO3,but this acid,sulfurous acid has never been isolated in pure form.Salts of sulfurous acid,sulfites,are good reducing agents and easily oxidized by O2.But they also act as oxidizing agents as in the reaction with H2S. • 例题Sulfate and sulfite salts have a number of important uses.Calcium sulfate dihydrate is used to make the hemihydrate for the building industry. • Aluminum sulfate is used in water treatment and in sizing paper.Copper(II) sulfate is employed as a fungicide and algicide and in electroplating. 杀真菌剂 [`ældʒisaid ]杀藻剂 • The chief application of sulfites is in the pulp and paper industry.sulfite solubilize lignin ,a polymeric substance that coats the cellulose fibers in wood.This treament frees the fibers for processing into wood pulp and then paper.Sulfites are used as reducing agents,such as in photography and as scavengers of O2 in treating boiler water. • 例题Thiosulfate can be prepared by boiling elemental sulfur in an alkaline solution of sodium sulfite .The sulfur is oxidized and the sulfite ion is reduced . • Thiosulfate solutions are important in photographic processing.They are also common analytical reagents,often used in conjunction with iodine. • For example,on one method of analysis for copper,an excess of iodide is added to Cu2+,producing CuI and triiodide. • Chlorate are good oxidizing agents.Solid chlorates produce oxygen gas when they decompose ,which makes them useful in matchs and fireworks. • A simple laboratory method of producing O2 involves heating KClO3in the presence of MnO2,a catalyst. • 2KClO3 → 2KCl+3O2 • Perchlorate salts are prepared mainly by electrolyzing chlorate solutions.Oxidation of ClO3-occurs at a Pt anode .platinum • Compared with the other oxoacid salts,perchlorates are relatively stable. • They do not disproportionate,because no oxidation state higher than +7 is available to chlorine. • At elevated temperature or in the presence of a readily oxidizable compound,perchlorate salts may react explosively. • Mixtures of ammonium perchlorate and powdered aluminum are utilized as the propellant in some solid rockets,such as those used on the space shuttle.航天飞机 • Ammonium perchlorate is especially dangerous to handle,because an explosive reaction may occur when the oxidizing agent ClO4- acts on the reducing agent NH4+ • Although oxygen is obtained to a limited extent by the decomposition of oxygen –containing compounds and the electrolysis of water.the principal commercial souce of oxygen is the fractional distillation of liquid air. • The main commercial methods of producing SO2 are the direct combustion of sulfur and the roasting of metal sulfides.(ZnS) • In the presence of a catalyst,SO2 is converted to SO3 • The main use of SO2 is in the systhesis SO3 to make sulfuric acid H2SO4. • In the modern process,the contact process SO2 is formed by the direct combustion of sulfur and the roasting of metal sulfides. • Then sulfur trioxide is produced by oxidizing SO2 in an exothermic ,reversible reaction. • Reaction occurs very slowly unless catalyzed. • The principal catalyst is V2O5 mixed with alkali metal sulfates.The catalysis involves adsorption of SO2and O2 on the catalyst,followed by reaction at active sites and desorption of SO3. • SO3 reacts with water to form H2SO4. • The SO3 readily dissolves in the sulfuric acid and reacts with the small amount water present to increase the concentration of the sulfuric acid.The result is a form of sulfuric acid sometimes called oleum[əuliəm ]发烟硫酸 but more commonly called fuming sulfuric acid. • When SO2 reacts with water,it produces H2SO3,but this acid,sulfurous acid has never been isolated in pure form.Salts of sulfurous acid,sulfites,are good reducing agents and easily oxidized by O2 .But they also act as oxidizing agents as in the reaction with H2S. • O2+2SO32- → 2SO42- • Sulfate and sulfite salts have a number of important uses.Calcium sulfate dihydrate is used to make the hemihydrate for the building industry. • Aluminum sulfate is used in water treatment and in sizing paper.Copper(II) sulfate is employed as a fungicide and algicide and in electroplating. 杀真菌剂 [`ældʒisaid ]杀藻剂 • The chief application of sulfites is in the pulp and paper industry.sulfite solubilize lignin ,a polymeric substance that coats the cellulose fibers in wood.This treament frees the fibers for processing into wood pulp and then paper.Sulfites are used as reducing agents,such as in photography and as scavengers of O2 in treating boiler water. • Thiosulfate can be prepared by boiling elemental sulfur in an alkaline solution of sodium sulfite .The sulfur is oxidized and the sulfite ion is reduced . • Thiosulfate solutions are important in photographic processing.They are also common analytical reagents,often used in conjunction with iodine. • For example,on one method of analysis for copper,an excess of iodide is added to Cu2+,producing CuI and triiodide. • The excess iodine is then titrated with a standard solution of NaS2O3 ,froming I-and S4O62-,the tetrathionate ion.连四硫酸盐 [,tetrə`θaiə,neit] 窗体顶端 • •无机物的制备 例题锂和钠生产进行约6000C electrolysis.The氯化钠电解熔融氯化物。氯化钠的熔点8010C，开展这项电解economically.Adding氯化钙的混合物降低了熔点过高的温度。 •例题金属钾是由液态钠减少熔融的氯化钾 •。氯化钾+娜→盐+ K •反应是可逆的低temperatures.At 8500C，但是，平衡是流离失所远的权利为K逃脱从熔融混合物 •由于钠反应，其最重要的用途是作为还原剂，在获得金属，如钛，锆，铪。 例题在化学工业中，氯化钠的许多化学物质，包括金属钠，氯气，盐酸，氢氧化钠和的来源。 [hai'drɔksaid] •例题氯化钾是从自然产生的盐水（盐的集中解决 方案 气瓶 现场处置方案 .pdf气瓶 现场处置方案 .doc见习基地管理方案.doc关于群访事件的化解方案建筑工地扬尘治理专项方案下载 ）。，它是应用最广泛的植物肥料，因为钾是植物生长的主要的基本要素。[大脑]盐水 例题氯化钾也被用作原料，在氢氧化钾，硝酸钾生产和其他重要的工业钾化合物（硝酸钾） 例题碳酸钠主要用于制造在美国生产的玻璃。NaCO3的，现在大多是来自从天然来源，如矿产天然碱，NaCO3.NaHCO3.nH2O。 在过去的碳酸钠的生产大多来自氯化钠，碳酸钙和NH3，使用，由比利时的化学家欧内斯特苏威于1863年推出的一个过程。 •['trəunə]天然碱 •例题碳酸氢钠可以隔离和转换加热碳酸氢钠，碳酸钠 •例题硫酸钠：是获得部分从自然来源，部分来自中和反应，部分是通过由约翰鲁道夫芒硝在1625年发现的一个过程。 •H2SO4（concd）+盐（S）→NaSO4（S）+盐酸（G） •反应背后的战略是挥发性酸（盐酸）生产加热及其盐（氯化钠）与非易失性酸（H2SO4）['vɔlətail] •例题硫化钠是生产NaSO4与减碳 •NaSO4 +→硫化钠+ CO。 •例题钠氢氧化物是商业化生产的电解氯化钠。氯离子被氧化氯;和H2O减少至H2。 •碱金属氢氧化物也可以group1的金属与水反应的准备。 •例题生产的第2组金属（镁除外）的首选方法是通过减少与其他活性金属及其盐类。 •绿柱石是铍compounds.This矿物的天然来源是加工生产BeF2，然后用镁减少。 例题钙和镁是特别abundant.Even的铍，2组最丰富的成员，访问，因为它发生的矿物绿柱石，3BeO.Al2O3.6SiO2存款。绿柱石 •例题钙，锶，钡铝及其氧化物的减少; •钙，锶，也可以通过电解熔融氯化物。 •例题金属镁是通过电解熔融氯化道琼斯指数过程中，镁的来源是海水或天然卤水。 •镁在海水中的丰度约1350mg / L。 例题镁的制备，第一步是对Mg（OH）2作为源的OH -与熟石灰的Ca（OH）2沉淀。熟石灰是由曹生石灰与水反应。沉淀为Mg（OH）2，洗涤，过滤，并导致集中氯化镁溶解在HCl.The干燥蒸发，熔化，电解，产生纯镁金属和Cl2.The Cl2的转换，这是回收的盐酸。 例题金属钙是主要用作还原剂准备，从他们的氧化物或氟化物，其他金属，如铀，钚，和大多数镧系元素。 [lænθə`NAID]镧系元素 •例题三个步骤需要从石灰石（1）石灰石（2）热分解反应的CaO与水（3）转换的Ca（OH）2悬浮液中获得的纯碳酸钙沉淀碳酸钙悬浮液 •例题所谓limestone.This反应煅烧生产生石灰是氧化钙是可逆的，在室温下发生逆反应几乎完全。 •因此，在碳酸钙煅烧，必须使用高温和产生的二氧化碳，必须不断从反应发生炉排出。 •最熟悉的是碳酸钙，石灰石含有超过5％MgCO3岩石limestone.If的主要组成部分，它通常被称为白云石。 •石灰石的主要用途（约70％）是作为一个stone.Among其他应用程序的建设，石灰石是制造生石灰和熟石灰。 •生石灰和熟石灰白云石[“dɔləmait] 例题本集团的最重要的金属是第三个最丰富的元素，铝aluminum.The包括地球固体地壳质量的8.3％。 •行政矿石，铝矾土，包含必须removed.The分离的原则是Al2O3是两性氧化物，在NaOH溶解，而氧化铁是碱性氧化物和不作为杂质Fe2O3的。 [æmfə`terik]两性的铝土矿[`bɔ：K，saɪt] •当溶液中含有的Al（OH）4] - 稍微酸化，获得的Al（OH）3 precipitates.Pure氧化铝是通过加热的Al（OH）3。 •氧化铝约10000C.The液体可以溶解在熔融矿物冰晶石Na3AlF6，在良好的电导体，所以电解氧化铝在熔融冰晶石完成。六氟[`kraiəulait]冰晶石 例题硫酸铝是最重要的铝复合使用commercially.It是准备Al2O3.The产品热浓硫酸反应，从溶液中结晶，是AL2（SO4）3.18H2O.octadecahydrate •当摩尔AL2（SO4）3和硫酸钾水溶液结晶，得到的晶体硫酸铝钾，KAL（SO4）0.12 H2O.This仅仅是一个大的双盐类称为校友。 •十二水合明矾[ə`lʌm] •例题行政锡矿是锡（IV），二氧化锡，锡石称为。 •净化后，锡氧化物（四）生产锡金属与碳减少。 [kə`sitə，rait]锡石矿 •田形成两个主要的氧化物，SNO和SnO2.By加热空气中的二氧化锡，它可以被转换为SnO2.One SnO2的使用是作为一个珠宝研磨。 •既锡，氯化亚锡和SnCl4__氯化物重要uses.Tin（二）氯化，氯化亚锡是一个很好的还原剂，在定量 分析 定性数据统计分析pdf销售业绩分析模板建筑结构震害分析销售进度分析表京东商城竞争战略分析 的铁矿石，以减少在水溶液中铁（Ⅲ），铁（II）。 •田（四）四氯化锡氯化锡和氯气直接反应形成的，它是其中锡回收废tinplate.Tin（二）fluride SNF2（氟化亚锡）的形式，已作为anticavity添加剂的重要使用牙膏。预防蛀牙 •例题铅是主要为铅（II）硫化物PBS，为方铅矿矿石。 •铅（II）硫醚是先转换导致（二）氧化物在空气中强烈加热，这一过程称为焙烧焙烧与焦炭生产的金属氧化物减少焦炭[ɡə`李：nə]。方铅矿 •一些可溶性铅化合物之一是铅（II）硝酸铅（NO3）2.It是在二氧化铅与硝酸反应形成的。 •铅（IV）的化合物倾向于接受减少铅（II）的化合物，因此良好的氧化agents.PbO2是一个比Cl2和近MnO4 - .PbO2更好的氧化剂氧化盐酸氯。 •一种可溶性铬盐对Pb（NO3）2除了产生色素铬酸铅另一种铅基颜料在陶瓷釉料和一次广泛用于制造油漆用白铅，碱式碳酸铅。 例题锌，重要商业价值的矿石ZnCO3（菱锌矿）和硫化锌（闪锌矿）。 [sfælərait]闪锌矿“smiθsənait]菱锌矿。 •ZnCO3分解为氧化锌和二氧化碳时，强烈强烈heated.When在空气中加热，硫化锌与氧气发生反应，产生氧化锌和氧化锌减少SO2.The是C（焦炭）或CO法减少约11000C代理商。 •不能减少二氧化钛与碳产生的例题钛金属，因为金属和碳发生反应，形成钛碳化物。 在钛生产的第一步是金红石矿（二氧化钛）的转换，以四氯化钛与碳和Cl2反应。金红石[“RU：TI：L] •二氧化钛+2 C +2 CL2→四氯化钛2 CO •纯化的四氯化钛是钛与一个很好的减少agent.The Kroll的过程中使用镁。 •四氯化钛2毫克→钛2氯化镁 •氯化镁是电解生产氯气和镁，这是循环反应，分别。 •钛得到海绵钛的融合质量。 •克罗尔过程是缓慢的，因为它需要高温真空蒸馏除去钛镁和MgCl2。 •近日，电解过程中曾建议从金红石生产的钛。二氧化钛是放置在阴极电解熔融氯化钙细胞，德州仪器（四）减少在阴极。 •例题，最重要的钒化合物的五氧化二钒，五氧化二钒，主要用作催化剂在SO2转化成SO3的制造硫酸的接触方法，。 [və`neidiəm] 例题一个更好的源代码比纯金属的铬化合物是碱金属的铬酸盐，其中包含铬（VI），可直接从铬铁矿。铁（CrO2）2 [`krəumait]铬铁矿 •4FE（CrO2）2 8碳酸钠7 O2→2Fe2O3 +8 Na2CrO4 8二氧化碳 •这种反应所产生的铬酸钠是许多重要的工业铬化合物的来源。 •我T是可能的重铬酸钾盐结晶，从一个解决方案解决方案是基本CrO3.If水一个，颜色由橙色变成黄色。 •FOM基本解决方案，仅铬盐可crystallized.Thus cotains铬（VI）Cr2O72 -或CrO42或两者的混合物的PH值取决于是否一个解决方案。 •正向反应是在酸性溶液中的青睐，主要铬（VI）物种是Cr2O72。 •在碱性溶液中，H +离子被删除，反向的青睐，形成CrO42，作为主要品种，需要仔细控制的PH时Cr2O72用于作为氧化剂或作为沉淀剂，CrO42。 2CrO42 - +2 H +→Cr2O72 - + H2O •铬离子在碱性溶液可用于金属沉淀，如BaCrO4和PbCrO4铬酸盐。这不是一个良好的氧化剂，它是不容易降低。 •重铬酸盐很容易减少Cr2O3.In重铬酸铵的情况下，只需加热复合在一个戏剧性的反应产生的Cr2O3。 •纯铬可少量减少类似的反应，铝热反应的Cr2O3与Al。 •例题锰是一种相当丰富的元素，cnstituting地球crust.Its主要矿石约1％是软锰矿软锰矿，MnO2.Like V和铬，锰最重要的是，在钢铁，锰合金生产。锰铁可减少软锰矿和赤铁矿的混合物（['hɛmə，taɪt]赤铁矿）铁与碳的矿石。 •二氧化锰+ Fe2O3的5彗星→锰2铁5二氧化碳 •[fɛro'mæŋgə，NIS] [词典释义]【冶此页】铁锰合金 •锰参与净化铁，硫和氧反应，除去渣形成。 •此外，锰增加steel.Steel含有锰的比例很高的硬度是非常艰难和耐磨 •二氧化锰干电池，玻璃和陶瓷釉料和作为催化剂;我也是锰的化合物的主要来源。 •当加热二氧化锰是碱和氧化剂的存在，锰盐生产。 3MnO2 6 KOH +氯酸钾→3K2MnO4 +氯化钾3 H2O •K2MnO4是从与水的融合质量和提取，然后被氧化，高锰酸钾高锰酸钾。 •高锰酸钾氧化agent.I吨一般是在酸性溶液中使用它减少到Mn2 +的一个重要的实验室。 •在分析铁MnO4 -，Fe2 +的样本准备，由溶解在酸性铁和降低任何FE3 +为Fe2 +，然后样品滴定MnO4 例题，可以从海水中或从内陆盐水solutions.The海水或盐水中提取溴调整PH3.5和氯气，氧化溴到BR2在此置换反应处理 •某些海洋植物，如海藻，吸收和集中在我的存在，选择性氯和溴。 •碘是从这种植物的少量obtaied。 •另一种丰富的天然碘源NaIO3，发现在智利的大型矿床。 •碘 •由于碘的氧化状态，必须从5降低IO3 - 0，在I2，IO3 - I2的转换需要减少agent.Aqueous氢钠亚硫酸盐（亚硫酸氢钠）用作还原剂第一步，其次是我额外的IO3生产碘的反应。 •IO3 - 3 HSO3 -→我的3 SO42 - 3 H + •5I - + IO3 - +6 H +→3I2 +3 H2O •在水溶液中，它们被称为高频hydrohalic acids.Excepts，hydrohalic酸在水中的强酸。[`haidrə`hælik] [`hælaid] •氟化氢 卤化氢 HF氟化氢 盐酸氢氯 HBR溴化氢 HI碘化氢 硫化氢硫化氢 HCL：盐酸 HBR氢溴酸酸 HCL：盐酸 HBR氢溴酸酸 您好hydroionic酸 HF氢氟酸 当加热与非易失性酸，如浓硫酸，硫酸盐和卤化物产生的挥发性氢卤化物盐（如萤石，氟化钙） 该方法的工程，因为浓硫酸是一个足够强氧化剂氧化溴Br2and我至i2的准备，但不HBR或HI.That盐酸（G）。 •2NaBr +2 H2SO4→硫酸钠+2 H2O + Br2的二氧化硫 •与H2和Cl2反应进行迅速爆炸，在光的存在，一些盐酸是这样的商业。 •随着Br2和I2，发生反应比较缓慢，需要一种催化剂。 •轻松准备在实验室中使用的氧化剂水溶液chlorine.The解决方案不只是氯气之一， •氯气成次氯酸与盐酸disproportionates。 HCLO（次氯酸） •次氯酸是一种有效的杀菌剂，用于水的净化和游泳次氯酸钠盐的pools.Aqueous解决方案的治疗（次氯酸钠）是常见的家用漂白剂使用的。 [haipəuklɔ：rait] •二氧化氯是一种重要的漂白剂，纸张和fibers.Its减少与过氧化氢离子在水溶液中产生绿泥石salt.sodium绿泥石是作为一个纺织品的漂白剂使用[`klɔ：rait]。 •氯酸钠盐的形式时，CL2 disproportionates在高温，浓碱的解决方案。 •冷，稀碱溶液中的次氯酸盐形式。 [klɔ：RIT]氯酸盐 •氯酸盐良好agents.Solid氯酸盐氧化时产生氧气分解，这使得它们在配和烟花。 •一个简单的实验室方法生产O2加热氯酸钾在二氧化锰催化剂。 •2KClO3→2KCl +3 O2 •高氯酸盐盐主要由铂阳极电解氯酸盐ClO3发生solutions.Oxidation准备。白金[`AEN，əʊd] •相比与其他ox​​oacid盐，高氯酸盐是相对稳定的。 •他们不相称，因为无氧化状态比7更高的可用氯。 •在高温或易氧化物化合物的存在，高氯酸盐盐的反应可能爆炸。 •高氯酸铵和铝粉的混合物利用一些固体火箭推进剂，如航天飞机上使用的，航天飞机。 •高氯酸铵是特别危险的处理，因为可能发生爆炸性反应时氧化剂ClO4的行为减少代理铵+ •例题的主要生产二氧化硫的商业方法是直接燃烧硫和金属硫化物焙烧（硫化锌）。 •在催化剂存在下，二氧化硫转化为三氧化硫 •SO2的主要用途是在systhesis三氧化硫，使硫酸硫酸。 •在现代化过程中，接触的过程中直接​​燃烧含硫和金属硫化物焙烧的二氧化硫是形成。 •然后通过一个放热反应，可逆reaction.Reaction SO2氧化产生三氧化硫发生非常缓慢，除非催化。 •V2O5mixed与碱金属sulfates.The催化涉及SO2and氧的吸附在催化剂上的，在活跃的网站和三氧化硫的脱附反应的主要催化剂。 •SO3的反应，形成硫酸与水。 三氧化硫容易溶解在硫酸和少量水存在的反应，以增加浓度硫酸acid.The结果是硫酸的形式，有时也被称为发烟硫酸，但更常见的称为发烟硫酸。 [əuliəm]发烟硫酸 当二氧化硫与水反应，生成H2SO3，但这种酸，硫酸从未在纯硫酸，亚硫酸盐form.Salts分离，是良好的还原剂，很容易被O2.But氧化，他们还充当氧化剂与H2S的反应。 •例题硫酸盐和亚硫酸盐盐有一些重要的uses.Calcium二水硫酸是用来做建筑行业的半水。 •硫酸铝是在水处理和浆纱paper.Copper（二）使用硫酸作为一种杀真菌剂和灭藻剂和电镀聘用。 杀真菌剂[`ældʒisaid]杀藻ㄩ •亚硫酸盐的行政应用程序是在纸浆和造纸industry.sulfite溶解木质素，高分子物质，大衣wood.This treament纤维素纤维释放到处理的木浆纤维，然后paper.Sulfites作为还原剂使用，如在摄影和氧气治疗锅炉水的拾荒者。 •例题硫代​​可以将沸腾硫元素在碱性溶液中的亚硫酸钠准备，硫被氧化，减少亚硫酸盐离子。 •硫代解决方案是重要的，摄影processing.They还共同分析试剂，经常与碘结合使用。 •例如，一铜的分析方法，碘过量添加Cu2 +的，生产崔碘化。 •氯酸盐良好agents.Solid氯酸盐氧化时产生氧气分解，这使得它们在配和烟花。 •O2涉及加热KClO3in MnO2的存在，催化剂的生产简单的实验室方法。 •2KClO3→2KCl +3 O2 •高氯酸盐盐是准备主要由铂阳极电解氯酸盐ClO3发生solutions.Oxidation铂 •相比与其他ox​​oacid盐，高氯酸盐是相对稳定的。 •他们不相称，因为无氧化状态比7更高的可用氯。 •在高温或易氧化物化合物的存在，高氯酸盐盐的反应可能爆炸。 •高氯酸铵和铝粉的混合物利用一些固体火箭推进剂，如航天飞机上使用的，航天飞机。 •高氯酸铵是特别危险的处理，因为可能发生爆炸性反应时氧化剂ClO4的行为减少代理铵+ •虽然氧气是获得含氧化合物和氧气的商业water.the主要烃源电解分解在有限的范围内是液态空气分馏。 •主要生产二氧化硫的商业方法是直接燃烧硫和金属硫化物焙烧（硫化锌）。 •在催化剂存在下，二氧化硫转化为三氧化硫 •SO2的主要用途是在systhesis三氧化硫，使硫酸硫酸。 •在现代化过程中，接触的过程中直接​​燃烧含硫和金属硫化物焙烧的二氧化硫是形成。 •三氧化硫产生氧化放热反应，可逆反应SO2。 •反应速度非常慢，除非发生催化。 •五氧化二钒与碱金属sulfates.The催化混合涉及SO2and氧的吸附在催化剂上的，在活跃的网站和三氧化硫的脱附反应的主要催化剂。 •SO3的反应，形成硫酸与水。 •三氧化硫容易溶解在硫酸和少量水存在的反应，以增加浓度硫酸acid.The结果是硫酸的形式，有时也被称为发烟硫酸[əuliəm]发烟硫酸，但通常称为发烟硫酸。 •当二氧化硫与水反应，生成H2SO3，但这种酸，硫酸从未在纯硫酸，亚硫酸盐form.Salts分离，是良好的还原剂，很容易被O2氧化，但他们也作为氧化剂作为在与H2S反应。 •O2 +2 SO32 -→2SO42 •硫酸和亚硫酸盐有一个重要的uses.Calcium二水硫酸是用来做建筑行业的半水。 •硫酸铝是在水处理和浆纱paper.Copper（二）使用硫酸作为一种杀真菌剂和灭藻剂和电镀聘用。 杀真菌剂[`ældʒisaid]杀藻ㄩ •亚硫酸盐的行政应用程序是在纸浆和造纸industry.sulfite溶解木质素，高分子物质，大衣wood.This treament纤维素纤维释放到处理的木浆纤维，然后paper.Sulfites作为还原剂使用，如在摄影和氧气治疗锅炉水的拾荒者。 •硫代可以准备在碱性溶液中的亚硫酸钠煮沸元素硫，硫被氧化，减少亚硫酸盐离子。 •硫代解决方案是重要的，摄影processing.They还共同分析试剂，经常与碘结合使用。 •例如，一铜的分析方法，碘过量添加Cu2 +的，生产崔碘化。 •碘过量是那么的NaS2O3标准溶液滴定，froming我和S4O62，tetrathionate离子，连四硫酸盐，tetrə`θaiə，neit] 窗体底端