1. INORGANIC CHEMISTRYACTINIDE SERIES OF PERIODIC TABLEPresented by :Pujiati (06121010018)Binti Uswatin (06121010021)Chemistry Education DepartmentSriwijaya UniversityIndralaya2012

2. Actinide seriesAtom number 89-103 3. 89 Actinium (Ac)90 Thorium (Th)91 Protactinium(Pa)92 Uranium (U)93 Neptunium(Np)94 Plutonium (Pu)95 Americium(Am)96 Curium (Cm)97 Berkelium (Bk)98 Californium (Cf)99 Einsteinium (Es)100 Fermium (Fm)101 Mendelevium(Md)102 Nobelium (No)103 Lawrencium (Lr)All of them areradioactive 4. ACTINIUM Its chemistry is dominated by (+3) O. S. Its compounds are colorless. There are 36 known isotopes. 227Ac is strongly radioactive and so are its decay components. Actinium metal is silvery solid; obtained by reduction of oxide,fluoride or chloride w/ Group 1 metals; and oxidized rapidly inmoist air. It forms insoluble fluoride and oxalate (Ac2(C2O4)3.10H2O)compounds Actinium is found in uranium ores 5. USES OF ACTINIUM Actiniums high activity level makes it valuable in producingneutrons. There has been some work done to use 225Ac in treatingcancer patients There are no practical commercial uses of actinium. Actinium of98 percent purity is prepared for research studies. 6. HEALTH EFFECTS OF ACTINIUMLike all radioactive materials, actinium is a health hazard. Iftaken into the body, it tends to be deposited in the bones, wherethe energy it emits damages or destroys cells. Radiation isknown to cause bone cancer and other disorders. 7. THORIUM It exhibits the +4 O.S. exclusively. The chemistry in the +2 and +3 O.S. is restricted to iodides likeThI2 and cyclopentadienyl Th(C5H5)3. It has wide coordination chemistry with oxygen donor ligands. Thorium metal is bright and silvery-white and tarnishes to a dullblack color when exposed to air. It is soft enough to be scratchedwith a knife and melts at 1750. It slowly dissolves in dilute withhydrogen evolution and can be pyrophoric as a powder. Thorium is weakly radioactive: all its known isotopes areunstable 8. USES OF THORIUMThorium is predicted to be able to replace uranium as nuclearfuel in nuclear reactors but no thorium reactors have yet beencompleted. 9. PROTACTINIUM It has been in existence longer than any other actinide. 231Pa has a half-life of 3.28*1014 which allows it to make chemicalstudy easy for it. It has -emission, so it has appropriate radiochemicalprecautions. The Pa metal is malleable, ductile, silvery, and has a meltingpoint of about 1565C. It is also a superconductor. 10. USES OF PROTACTINIUMProtactinium-231 arises from the decay of uranium-235 formedin nuclear reactors, and by the reaction 232Th + n 231Th + 2n andsubsequent beta decay. It may support a nuclear chain reaction,which could in principle be used to build nuclear weapons. 11. URANIUM Many compounds exist between the O.S. of +3 to +6. The main O.S. are +4 and +6. Stability of O.S.U3+ reduces to hydrogenU4+ stable in aqueous solution in the absence of airU5+ disproportionates rapidly into a mixture of U4+ and U6+ in aqueous solutionsU6+ stable in aqueous solutions When pure it has a silvery appearance. Reacts readily with hot water to prevent substances from coming into contact innuclear reactors 12. USES OF URANIUMuranium is an element found everywhere on Earth, but mainly intrace quantities. In 1938, German physicists Otto Hahn and FritzStrassmann showed that uranium could be split into parts toyield energy. Uranium is the principal fuel for nuclear reactorsand the main raw material for nuclear weapons. 13. NEPTUNIUM It was the first transuranium element to be discovered in 1940. There are 15 known isotopes, only 237Np, w/ half-life of2.14*106 years, is useful for chemical experiments. It exhibits O.S. of +3 to +7 in compounds. It is a silvery metal, with a melting point of 637C and a boilingpoint of 4174C. It has surface oxidation when exposed to air. It is converted to NpO2 at high temperatures 14. USES OF NEPTUNIUM Neptunium and its compounds of neptunium have been madefor research purposes. They are used in specialized detectiondevices and in nuclear reactors. Neither the element nor itscompounds have any commercial uses. Neptunium is a very hazardous material. It must be handled withgreat caution 15. PLUTONIUMThere are 15 known isotopes. The masses range from 232 to 246.The most important isotope is 239Pu because it is fissionable and has a half-life of 24,100years, which makes it easy for chemists to study.It exhibits O.S. from +3 to +7. The +3 and +4 O.S. are the most important, but compounds of the ions are well defined. Pu+7 only exists under very alkaline conditions.It has 6 allotropic metal forms, which makes it unusual. They can form at normal pressure between room temperature and its melting point,640C. It is dense, silvery and a reactive metal; more reactive than uranium or neptunium. When attacked by air, it forms a green-gray oxide coating. It reacts slowly with cold water, faster with dilute H2SO4, and dissolves quickly in dilutehydrochloric acid or hydrobromic acid. 16. USES OF PLUTONIUM The most important uses of plutonium depend on two of itsproperties. First, the radiation given off by plutonium occurs asheat. In fact, plutonium gives off so much heat that the metalfeels warm when it is touched. If a large piece of plutonium isplaced into water, the heat released can cause the water to boil. Plutonium provides electrical power on space probes and spacevehicles. 17. AMERICIUM It has 12 known isotopes. It was first made in 1944-1945 by Seaborg and his coworkers, where theydecayed 239Pu and 241Pu to 241Am, which has a half-life of 433 years.241Am and 243Am, which has a half-life of 7380 years are the most important isotopes,because their half-lives allow scientists to study their characteristics. The metal is a slivery, ductile and very malleable.It tarnishes in air slowly and dissolves in dilute hydrochloric acid quickly.It reacts with heating with oxygen, halogens, and other nonmetals 18. USES OF AMERICIUMThe vital ingredient of household smoke detectors is a very smallquantity of Am-241 as americium dioxide (AmO2). 19. LATER ACTINIDES (CM, BK, CF, ES, FM, MD, NO, AND LR) Their chemistry is of mostly the M+3 state. They all form binary compounds, such as trihalides. Oxidized by air to the oxide Electropositive Reacts with hydrogen on warming to form hydrides Yields compounds on warming with group 5 and group 6 non-metals