Since the characters aren't enough for my real questions, I'll just put it here. My questions are about nuclear chemistry.\n\n1.What property should a radioisotope have if it is to be administered internally in a medical diagnostic procedure? Why?\n\n2.Of alpha radiation, beta radiation, and gamma radiation, which is most damaging to living things when it is emitted by a nearby, external force? Explain.\n\n3.Of the three, which is most dangerous to one thing when it is emitted by a radioisotope located within the body? Explain.\n\n4.Among the various proposals suggested for the disposal of high-level nuclear wastes, is there a possibility of sealing them in drums and transporting them by rocket to the moon, to remain on its surface forever? What would be the advantage of such a plan? What would be its drawbacks? Would you support a plan of this sort?
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http://www.gwu.edu/~nsarchiv/radiation/dir/mstreet/commeet/meet1/brief1/br1j.txt\n\nThe first 3 are covered there.
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Tritium.\n\nThat is the isotope of hydrogen with one proton and two neutron in the nucleus.  It is used as a low grade radio-active activator in phosphorescent paint, replacing radium which is much more dangerous.\n\n(Science Teacher below is wrong: deuterium is a stable nucleon, it is thus not radio active)
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radioactivity is the number of radioactive particle emitted in a unit of time.\nSo, the application are\nMedication- radioactive source that emits X-ray is used to scan bones. It also used to kill cancer cells(this technique is called the radiotheraphy)\nDating- Since there is C14 which is radioactive in almost every carbon based organism (include human and dinosour,n in fact in all organism), historian were able to determine the age of an artifact or bones.\nPaper production- using information that alpha particle cannot penetrate a thin sheet of paper, we are able to control the thickness of paper produced.\nsterilization- because radiation can kill cells, it is use to kill microbes to sterill things.
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In Singapore, for diagnostic imaging we use Iodine 123.\n\nI think actually Iodine 131 is used for radioablation too. We don't use the 127 isotope where I come from so can't help you with that.
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It kind of depends on exactly what the radiation was given to treat; they tell you not to handle patients who get "seeds" implanted because while the material is in their bodies, some of the contamination may leach out through pores in their skin and contaminate you.  If your cat had a thyroid problem, then radioactive iodine 131 was used to kill thyroid tissue, because the thyroid selectively collects iodine.  As a previous poster said, by the time you can get to a doctor, you're already going to absorb all you're probably going to get from this exposure, because iodine 131 has a half life of about a half an hour, so by the time three hours have passed, it's all decayed away to normal iodine.  The reason you found potassion iodide listed as a treatment is that if you take a tablet, it floods your system with more iodine than your thyroid can handle, and it won't accept any more; assuming you take it BEFORE or IMMEDIATELY after your exposure to radioactive iodine, it prevents your body from absorbing the radioactive stuff and it just flushes right out of your system.  \n\nIf, however, your cat was treated with something other than iodine, whatever isotope was used may have other effects on you (strontium deposits in bone, for instance, replacing calcium)  Only way to know for sure is to figure out what the treatment was and ask your doctor for advice.  It is probably nothing to worry about, but worth checking with a medical professional just to be sure.
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All things are radiocative. The only thing in this universe that isn't radioactive is the small amount of hydrogen that scientists have refined to not be radiocative.\n\nThis "radioactivity of everything" is what we call the background radiation level. It varies from place to place but everywhere has a background radiation level, and the insides of people or other organisms are no exception.\n\nFood is radiocative because the ground and air it came from is radiocative.\n\nThe ground is radioactive because the matter the Earth was made of came from a supernova. And supernova is just a really, really big atomic bomb.\n\nThe air is radioactive partly because of that supernova but mostly because the sun is also basically a really big nuclear bomb. On the ground we are protected from all the worst radaiation that bomb puts out. In the upper atmosphere the air is not protected. It gets zapped with masive amounts of radiation every day and is fairly radioactive as a result.\n\nWhen plants take minerals out of the soil those minerals are slightly radioactive from the supernova that created the Earth. When plants take carbon out of the air that carbon is radioactive from being zapped by nuclear radiatioon from the sun. When the plants use those things to build more plants the plants become radioactive. When animals eat the radioactive plants and use that material to build animal bodies the animals become radicoative.\n\nAnd when people eat radiocative plants and animals our bodies become radiocative.\n\nEverything in the universe is radiocative, even us. The only thing that varies is how radioactive they are.\n\nYoumay be interested in the link below. It explains how all food plants and all animals are radiocative, and how this  radiactivity of all living things forms the basis of radiocarbon dating techniques.
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I'm not directly giving you the answers, you have to know how to do this stuff, but I'll give you the process to get to each.\n\n9: Americium and Curium (wikipedia!)\n\n10: Potassium ion wants to be like the noble gas closest to it (the one right before it), so it loses 1e- to get there and be K+.  If that's not a choice, then look for another ion, positive or negative, that adds up to the electronic configuration of the aforementioned noble gas. (1s2 2s2 2p6 3s2 3p6), 18 total e-'s...\n\n11: Mg is in column 2, things in the same period tend to be chemically similar.  Find the other one in the choices that's in that column\n\n12: U235 and U238 are isotopes, same atomic number, different weight.  If you change the number of protons, you change the atomic number, so that wouldn't be U anymore.  Changing electrons can make ions, but not change weight.  So different number of neutrons for the same element makes an isotope.\n\n13: Same explanation as above, it'll also be Hydrogen's atomic number because it's an isotope.\n\n14: shell 2 contains the 2s and 2p subshells.  2s can hold 2 because it's an s orbital.  2p can hold 2 per p orbital, and a p subshell has 3 p orbitals, so 6.  Total would then be...\n\n15: If an atom loses electrons, it's LOSING -1 per electron lost, so it's becoming more positive.\n\n16: Which element in that list only has 1s shell? Which one has a  stable ion as just a proton or with a configuration like Helium (1s2)?\n\n17: Inert elements are on the far right of the periodic table.  They are inert because they have 8 valence (outer shell) electrons (or 2 in Helium's case) so they can't take anymore and are stable.  Look at your periodic table or count up electrons for each of those atomic numbers.  Only one of them will have 8 in the outer shell...
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For the first question, , I think C is the least correct.  Alpha and beta emissions are particles, not rays.  B is also suspect, because not all radioactive emiissions are both particulate and energy.\n\nFor your true/false question, the answer is FALSE.  An alpha emission reduces the atomic number by 2, and reduces the atomic weight by 4.
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1) is false, all the elements in living things can be found in non-living things\n\n2) this more tricky, what are these 4 elements most common in plants? I'm guessing: Hydrogen and Oxygen, (from water) Carbon, and . . .nitrogen???\nall these can be found in animals\nare you sure the question is asking about elements? elements in living things are pretty common to another. Its the compounds (hemoglobin, chlorophyll, etc) that get rather unique\n\ndo a little research, if some one cannot explain how they got the answer to a T/F question, you can't be sure they are just guessing
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ignoring radioactivity(which deals with unstable isotopes) the elements are indestructible and will last forever.\nthe law of conservation of matter says matter can never be created nor destroyed.( we can destroy matter in nuclear bombs but otherwise...).\nAs long as atoms exist, which is forever, the periodic table will tell you what to expect.
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1.what is the most heat resisstant materian on earth?\n(clue:used by NASA for ther Stardust Sattelite)\nYet NASA plans to do just that, using a lightweight insulating material called aerogel. Composed of over 95 percent air, aerogel is the lightest man-made material on earth. And although aerogel will be used in the depths of space to conduct research in astrophysics, it has hundreds of down-to-earth applications, as well.\n\n2.Where is Yahoo!'s headquarter?(clue: CA)\nnorth Sunnyvale, CA\nhttp://www.svcn.com/archives/sunnyvalesun/02.16.00/yahoo-0007.html\n\n3.tell me 2 diffrences between Plutonium and Uranium(clue: BOOM!!, Krrrttzzz rrrtzz..)\n\nPlutonium\n\nPlutonium was discovered, secretly, in 1940 by Glenn Seaborg with Wahl and Kennedy at Berkeley and publicly reported in 1946. Plutonium was extracted from uranium ore in 1947. Until recently the major use of plutonium has been for nuclear weaponry, it now finds its best use in deep space probe electricity sources . \nAtomic number-94Densityg/mL19.8\nAtomic weightu244Melting pointK913\nBonding radiusA-Boiling pointK3503\nAtomic radiusA-Heat of vaporizationkJ/mol344\nIonization PotentialV6.06Heat of fusionkJ/mol2.84\nElectronegativity-1.28Specific heatJ/gK0.13\nThe oxide is amphoteric.\nCrystal are monoclinic.\n\nUranium\nUranium oxide has been used since Roman times for yellow pigments in glass. The element was discovered in 1789 by a German chemist, Martin Klaproth, who named it for the newly observed seventh planet. In 1841, French chemist Eugene Peligot extracted pure uranium metal, which caused little interest until March 1, 1869, when French physicist, Henry Becquerel serendipidously discovered radioactivity in uranium salts - suddenly uranium was hot stuff!\nAlthough only mildly radioactive, uranium compounds are toxic. \n\nAtomic number-92Densityg/mL18.9\nAtomic weightu238.029Melting pointK1405\nBonding radiusA1.42Boiling pointK4407\nAtomic radiusA-Heat of vaporizationkJ/mol477\nIonization PotentialV6.05Heat of fusionkJ/mol8.52\nElectronegativity-1.38Specific heatJ/gK0.12\nThe oxide is amphoteric.\nCrystal are orthorhombic.\nhttp://chemlab.pc.maricopa.edu/periodic/U.html
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Three basic concepts apply to all types of ionizing radiation. When we develop regulations or standards that limit how much radiation a person can receive in a particular situation, we consider how these concepts might affect a person's exposure.  \n\nTime \nThe amount of radiation exposure increases and decreases with the time people spend near the source of radiation. \n\nIn general, we think of the exposure time as how long a person is near radioactive material. It's easy to understand how to minimize the time for external (direct) exposure. Gamma and x-rays are the primary concern for external exposure.\n\nHowever, if radioactive material gets inside your body, you can't move away from it. You have to wait until it decays or until your body can eliminate it. When this happens, the biological half-life of the radionuclide controls the time of exposure. Biological half-life is the amount of time it takes the body to eliminate one half of the radionuclide initially present. Alpha and beta particles are the main concern for internal exposure. \n\nDistance   \nThe farther away people are from a radiation source, the less their exposure. \nHow close to a source of radiation can you be without getting a high exposure? It depends on the energy of the radiation and the size (or activity) of the source. Distance is a prime concern when dealing with gamma rays, because they can travel long distances. Alpha and beta particles don't have enough energy to travel very far. \nAs a rule, if you double the distance, you reduce the exposure by a factor of four.  Halving the distance, increases the exposure by a factor of four.\n\nThe greater the shielding around a radiation source, the smaller the exposure. \n\nShielding simply means having something that will absorb radiation between you and the source of the radiation (but using another person to absorb the radiation doesn't count as shielding). The amount of shielding required to protect against different kinds of radiation depends on how much energy they have. \n\n \n(Alpha)\n\n A thin piece of light material, such as paper, or even the dead cells in the outer layer of human skin provides adequate shielding because alpha particles can't penetrate it. However, living tissue inside body, offers no protection against inhaled or ingested alpha emitters.\n    \n \n(Beta)\n\n Additional covering, for example heavy clothing, is necessary to protect against beta-emitters. Some beta particles can penetrate and burn the skin.\n   \n \n(Gamma) \n Thick, dense shielding, such as lead, is necessary to protect against gamma rays. The higher the energy of the gamma ray, the thicker the lead must be. X-rays pose a similar challenge, so x-ray technicians often give patients receiving medical or dental X-rays a lead apron to cover other parts of their body. \n\nSo in short the lead or other materials absorb the radiation vs. it being absorbed by your body.
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Hmm, the basic principle is that it excites the water molecules in food which creates heat energy. Don't know about putting a radioactive element in there...
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Change into a different element altogether.\n\nNatural decay of heavy elements occurs sending off alpha- or beta-particles, i.e. helium4-cores or electrons.\n\nIn the case of alpha radiation, the element will move two positions down in the periodic system, in case of beta radiation it will move one position up.\n\nUranium 238 emits alpha-radiation, forming Thorium 234. See the link below for consecutive decay reactions.
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http://www.burtonreport.com/InfForensic/HumanExperPlutonium.htm\n\n\nhttp://www.gwu.edu/~nsarchiv/radiation/dir/mstreet/commeet/meet10/brief10/tab_i/br10i2j.txt
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Ok I think that what you don't understand and what really has not been pointed out yet is that radiation is produced by the decay ( or breakdown) of atoms in the nuclear material.\n\nSay you have a few pounds of nuclear waste. You have Billions and billions and billions of atoms. Remember Avogadro's number? That is the number in just a mole of material. Now imaging that number multiplied by the number of moles in a few pounds! That's a lot of atoms.\n\nNow a fire burns out because it runs out of material to burn. However with all those billions of atoms it could take tens of thousands of years for all the material to be used up.\n\nie if the half life is 10,000 years, that means we have only used up half the material in 10,000 years. So if we had 10 pounds of nuclear waster, in 10,000 years we would still be left with 5 pounds!\n\nNow think of Einsteins famous equation E=mc2.\nm is the mass, c is the speed of light squared, and E is the\nenergy you get out of it. As you can see, even in a very small amount of mass there is tremendous energy.\n\nSo sum it up, even though very small amounts are decaying and giving off large amounts of energy. It is going to take thousand and thousands of years before it is used up.that is why it lasts so long.
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Right answer is F) because is given off by alpha (electrons), beta and gamma rays (photons) and breaks molecular bonds.\n\nThat´s it!\n\nGood luck!