What are the Aluminum isotopes and their uses?
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Isotopes ;\nAluminium has nine isotopes. Only the stable isotope, Al-27 and the radioactive isotope, Al-26 occur naturally. Al-26 is produced from argon in the atmosphere by spallation caused by cosmic-ray protons. Aluminum isotopes have found practical application in dating marine sediments, manganese nodules, glacial ice, quartz in rock exposures, and meteorites. The ratio of Al-26 to beryllium-10 has been used to study the role of transport, deposition, sediment storage, burial times, and erosion on 105 to 106 year time scales.\n\nCosmogenic Al-26 was first applied in studies of the Moon and meteorites. Meteorite fragments, after departure from their parent bodies, are exposed to intense cosmic-ray bombardment during their travel through space, causing substantial Al-26 production. After falling to Earth, atmospheric shielding protects the meteorite fragments from further Al-26 production, and its decay can then be used to determine the meteorite's terrestrial age. Meteorite research has also shown that Al-26 was relatively abundant at the time of formation of our planetary system. Possibly, the energy released by the decay of Al-26 was responsible for the remelting and differentiation of some asteroids after their formation 4.6 billion years ago.
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The atomic number of gallium is 31. Therefore, there is 31 protons and 31 electrons. However, The mass number of gallium can be varied because gallium contains isotpes. Each isotope has the same atomic number but different mass number. The most abundance isotope of gallium has a mass number of 70. So there is (70 - 31) = 39 neutrons.
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Los Alamos national lab has a good periodic table/ elemental factoids.\n\nLanthanum is La.  It is the beginning of the "Lanthanides".
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check this site out\n\nhttp://www.chemicalelements.com/elements/al.html
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See the paragraph on applications here:\nhttp:http://en.wikipedia.org/wiki/Radium//en.wikipedia.org/wiki/Radium
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aluminum has 3 valence electrons
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copper, silver, aluminum, lead, magnesium, platinum and tungsten
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Aluminium is a chemical element and metal.\nAluminium nails would be nails made of this elements.\n\nCorrosion/rust is the contact of metals with oxygen (another chemical element and part of the air around us), the process is alled oxidation.\n\nThe best example is the metal iron reacting with oxygen from the air  and the result would be rust. (it works better with water as ths contains more of the element oxygen). The surface becomes reddish-brown and briddle, more oxygen can penetrate the metal and in the end the piece of metal breaks, "it rustes away".\n\nAlumumium does react withs oxygen but only on the surfcae, in common language you could say its "rusts". The surface than looks greyish.  But in comparison to iron this forms a protecting layer on the surface of the aluminum, no oxygen can get deeper and the aluminium stays stable.\n\nThat is one of the reason airplanes are made of a very pure aluminium. They should not rust.
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The question is either incomlete or it doesn´t make sense. Are you looking for the atomic mass, density or somethig else.\nAs it is, the best answer to your question would be: "depends on how much aluminum".
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Radium\nI  INTRODUCTION \n\nRadium (Latin, radius,”ray”), symbol Ra, chemically reactive, silvery-white, radioactive metallic element. In group 2 (or IIa) of the periodic table, radium is one of the alkaline earth metals. The atomic number of radium is 88.\n\nRadium was discovered in the ore pitchblende by the French chemists Marie Curie and Pierre Curie in 1898. They discovered that the ore was more radioactive than its principal component, uranium, and they separated the ore into many chemical fractions in order to isolate the unknown sources of radioactivity. One fraction, isolated by use of bismuth sulphide, contained a strongly radioactive substance that the Curies showed was a new element, polonium. A highly radioactive barium chloride fraction was treated to remove the radioactive substance, which was discovered to be a new element, radium.\n\nII  PROPERTIES AND OCCURRENCE \n\nRadium-226 metal melts at about 700° C (about 1292° F), and has a relative density of 5.5. The element oxidizes immediately upon exposure to air. The element is used and handled in the form of radium chloride or radium bromide and practically never in the metallic state.\n\nRadium is formed by the radioactive disintegration of uranium and is consequently found in all uranium ores. Radium is present in uranium ore to the extent of one part of radium to three million of uranium. It is extracted from the ore by the addition of a compound of barium that acts as a “carrier”. The chemical properties of radium are similar to those of barium, and the two substances are removed from the other components of the ore by precipitation of barium and radium sulphate. The sulphates are converted into carbonates or sulphides, which are then dissolved in hydrochloric acid. The radium is separated from the barium as the end result of successive crystallizations of the chloride solutions.\n\nOf the isotopes of radium, ranging in mass number from 206 to 232, the most abundant and most stable is the isotope of mass 226. Radium-226 is formed by the radioactive disintegration of the thorium isotope of mass 230, which is the fourth successive isotope in the decay series starting with uranium-238. The half-life of radium-226 is 1,620 years. It emits alpha particles, forming the gas radon.\n\nIII  USES \n\nRadiation from radium has a harmful effect upon living cells, and radium burns are caused by overexposure to the rays. Cancerous cells, however, are often more sensitive to radiation than normal cells, and such cells may be killed without seriously injuring healthy tissue by controlling the intensity and direction of the radiation. Radium is now used in the treatment of only a few kinds of cancer; radium chloride or radium bromide is enclosed in a sealed tube and inserted in the diseased tissue. When a radium salt is mixed with a substance such as zinc sulphide, the substance is caused to luminesce by the bombardment of the alpha rays emitted by the radium. Small amounts of radium were once used in the production of luminous paint, which was applied to clock dials, doorknobs, and other objects, to make them glow in the dark.
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Aluminium or aluminum is the chemical element in the periodic table that has the symbol Al and atomic number 13. It is a silvery and ductile member of the poor metal group of chemical elements. Aluminium is found primarily as the ore bauxite and is remarkable for its resistance to corrosion (due to the phenomenon of passivation) and its light weight. Aluminium is used in many industries to make millions of different products and is very important to the world economy. Structural components made from aluminium and its alloys are vital to the aerospace industry and very important in other areas of transportation and building in which light weight, durability, and strength are needed.\n\nAluminium is a soft and lightweight metal with a dull silvery appearance, due to a thin layer of oxidation that forms quickly when it is exposed to air. Aluminium is nontoxic (as the metal), non-magnetic, and non-sparking. Pure aluminium has a tensile strength of about 49 megapascals (MPa) and 400 MPa if it is formed into an alloy. Aluminium is about one-third as dense as steel or copper; is malleable, ductile, and easily machined and cast; and has excellent corrosion resistance and durability due to the protective oxide layer. Aluminium mirror finish has the highest reflectance of any metal in the 200-400 nm (UV) , and the 3000-10000 nm (far IR) regions, while in the 400-700 nm visible range it is slightly outdone by silver, and in the 700-3000 (near IR) by silver, gold and copper. It is the second most malleable metal (after gold) and the sixth most ductile. Aluminium is a good heat conductor which is why it is used to make saucepans.
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There are many different forms of Alum.\n\nAlum is a double Sulfate salk with a general formula of,\nM+M'3+ (SO4)2 * 12H2O\n\nA very common form of Alum involves Potassium and Aluminum ions as shown below, this would be the standard "Alum",\nKAl(SO4)2 * 12H2O\nThis can be made through a series of chemical reactions.  Start with some Aluminum , react it with a KOH solution to make Al(OH)3 and then slowly add some Sulfuric acid (H2SO4). \n\nIt is a multistep process, there iare certainly more thorough explanations to be found out there on the internet.
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I'll tell you and won't kill you.\n\nBut don't even think of trying this at home.\n\nThe ore (found in rocks, mines, mountains) contains a couple types (isotopes) of uranium, mainly  U-235 (the one for nuclear fuel) and U-238 (depleted uranium, for armor piercing rounds).\n\nThese have different weights, so you can use a centrifuge (same as the spinner that seperates blood cells from plasma based on weight) to seperate the lighter atoms of U-235 from the heavier U-238. Thus all the fuss about who may or may not be buying aluminum tubes in the middle east to make centrifuges.
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Protons, neutrons, and electrons.
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stable lutetium nuclides can be used as catalysts in cracking, alkylation, hydrogenation, and polymerization alloys.
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C, Al(OH)3...\nWould you like an explanation? Okay, I'm supposed to be learning about this in Chemistry right now, so, I think this is how it works...\n\nIf you study the periodic table of elements, then you will find the number of valence (or outer) electrons each element has. Al has 3, O has 6, and H has 1. Before we start, it is important to know that a filled orbital has 8 valence electrons... okay? \nO and H combine, so they have a total of 7 valence electrons. You can imagine this by thinking of the letters OH surrounded by 7 dots in a circle, 2 pairs of dots on each side and 1 alone (a filled orbital with have four pairs opposite each other). The lone pair needs an electron, so it can borrow one from aluminum, which has 3 electrons. Aluminum loses its electron, so now it has 2, and the OH is now full, because it has 8 electrons. However, the aluminum has to get rid of its other two electrons, so another OH is brought in. The aluminum gives up an electron and the second OH is now full. Finally, the last OH pair is brought in and the aluminum gives away its last electron. So now, it is empty and the OH's are full. I guess they're balanced. Anyway, you are now left with 1 Al and 3 OH's, making Al(OH)3. Do you understand now? \n\nAl (3), and OH (7) (because O=6 & H=1, which equals 7)...\nAl - 1 = (2), so now OH = (8) (now it's full)\nAl - 1 = (1), so a 2nd OH (7) is brought in, making it OH (8)\nAl - 1 = (0), so a 3rd OH (7) is brought in, making it OH (8)\n\nIt took 1 Al and 3 OH's, so the new compound is Al(OH)3\nHope this helps!!!\nP.S. sorry for any confusion earlier when I tried to "draw" them. The computer changed the spacing so all you could see was a mess of stars and stuff. : )
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The atomic number of Aluminum is 13 (look at a periodic table). This means 13 protons and 13 electrons (since these are oppositely charged they have to balance each other.) To find the number of neutrons you subtract the number of protons from the atomic mass (the atomic mass is 27). So 27-13= 14 neutrons