Explain the term radioisotopes.?
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Atoms of chemical elements may have many isotopes (different forms) with the same atomic numbers but different atomic weights / atomic mass numbers. If a nuclide is radioactive, it is sometimes referred to as a radionuclide or (when the atom in question is understood) a radioisotope.\n\nA radionuclide is an atom with an unstable nucleus. The radionuclide undergoes radioactive decay by emitting a gamma ray(s) and/or subatomic particles. Radionuclides may occur naturally, but can also be artificially produced.\n\nRadionuclides are often referred to by chemists and biologists as radioactive isotopes or radioisotopes, and play an important part in the technologies that provide us with food, water and good health. However, they can also constitute real or perceived dangers.
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Polonium:\n\npo·lo·ni·um (pə-lō'nē-əm) pronunciation\nn. (Symbol Po)\n\nA naturally radioactive metallic element, occurring in minute quantities as a product of radium disintegration and produced by bombarding bismuth or lead with neutrons. It has 27 isotopes ranging in mass number from 192 to 218, of which Po 210, with a half-life of 138.39 days, is the most readily available. Atomic number 84; melting point 254°C; boiling point 962°C; specific gravity 9.32; valence 2, 4.\n\n[From Medieval Latin Polōnia, Poland (the native country of Pierre and Marie Curie, the element's discoverers).]\nPolonium\n\nA chemical element, Po, atomic number 84. Marie Curie discovered the radioisotope 210Po in pitchblende. This isotope is the penultimate member of the radium decay series. All polonium isotopes are radioactive, and all are shortlived except the three ?-emitters, artificially produced 208Po (2.9 years) and 209Po (100 years), and natural 210Po (138.4 days). See also Periodic table.\n\nPolonium (210Po) is used mainly for the production of neutron sources. It can also be used in static eliminators and, when incorporated in the electrode alloy of spark plugs, is said to improve the cold-starting properties of internal combustion engines.\n\nMost of the chemistry of polonium has been determined using 210Po, 1 curie of which weighs 222.2 micrograms; work with weighable amounts is hazardous, requiring special techniques. Polonium is more metallic than its lower homolog, tellurium. The metal is chemically similar to tellurium, forming the bright red compounds SPoO3 and SePoO3. The metal is soft, and its physical properties resemble those of thallium, lead, and bismuth. Valences of 2 and 4 are well established; there is some evidence of hexavalency. Polonium is positioned between silver and tellurium in the electrochemical series.\n\nTwo forms of the dioxide are known: low-temperature, yellow, face-centered cubic (UO2 type), and high-temperature, red, tetragonal. The halides are covalent, volatile compounds, resembling their tellurium analogs.polonium (pəlō'nēəm) , radioactive chemical element; symbol Po; at. no. 84; mass no. of most stable isotope 209; m.p. 254°C; b.p. 962°C; sp. gr. about 9.4; valence +2 or +4. Polonium is an extremely rare element found in uranium ores (about 0.1 gram per ton). A product of radium decay, it is sometimes called radium F. In its physical and chemical properties it resembles tellurium (the element above it in Group 16 of the periodic table) and bismuth. Polonium has 34 isotopes, more than any other element. All of these isotopes are radioactive. The most stable, polonium-209, has a half-life of about 103 years. Polonium-208 (half-life about 3 years) is the only other polonium isotope with a half-life over one year. Although these two isotopes can be prepared in small quantities in a particle accelerator, they are very expensive to produce. All other polonium isotopes are short-lived except polonium-210 (half-life about 138 days), which is the most commonly used isotope. It is prepared by bombarding bismuth with neutrons in a nuclear reactor. It is a highly radioactive material. A milligram of polonium-210 emits as much alpha radiation as about 5 grams of radium, and enough gamma radiation to cause a blue glow in the air around it. It can be used as a heat source, since most of the energy of the alpha radiation is absorbed as heat within the polonium and its container. Polonium has found use in small portable radiation sources and in the control of static electricity. However, it is an extremely toxic substance and must be handled with great care. Polonium was the first element to be discovered because of its radioactivity; it was discovered in pitchblende in 1898 by Marie Curie and named for her native country, Poland.A naturally radioactive metallic element, occurring in minute quantities in uranium ores; its most readily available isotope is Po 210, with a half-life of 138.39 day
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Uranium enrichment is the process of making those little things called electrons that are in atoms to become more and more unstable thus creating a highly unstable substance that is used for the core of.. you guessed it! The A bomb! There are different isotopes of atoms, usually uranium, and the more electrons you make it lose the more unstable it gets, Plutonium is used in bombs, plutonium is made from uranium for example. Have a nice day.
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your first question is somewhat political so i am not answering that but your second question ,that's physics so i will answer that.\nthe radioactive elements have this special property called half-life.\ni will use this eg to explain it.\nthink that you have in your hand 1kg of uranium(dont show that to bush)and assuming its half-life to be around  thousand years ,you will find that after 1000years the uranium in your hand will have decayed and only 0.5kg of the total will be left.and it keeps on like that.so it kinda never ends.Hope you understood.
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Take radium and subtract two from its atomic number. Then find the element with that result as its atomic number. I'm too lazy to see what that is right now.
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Radioactive Isotopes - are called  the "Clocks in Rocks" and these are used for calculating the Numerical and Relative Ages for Rocks \nIn Numerical dating,  - radioactive isotopes ("parents") that spontaneously decay to form new isotopes ("daughters") while releasing energy. For example, decay of the parent isotope Rb-87 (Rubidium) produces a stable daughter isotope, Sr-87 (Strontium), while releasing a beta particle (an electron from the nucleus). ("87" is the atomic mass number = protons + neutrons.) \nMany minerals contain radioactive isotopes. In theory, the age of any of these minerals can be determined by \n1) counting the number of daughter isotopes in the mineral, and  \n2) using the known decay rate to calculate the length of time required to produce that number of daughters. \nSO TO SUM UP THE PARENTS PRODUCE DAUGHTERS BECAUSE UNLIKE THE PARENTS THE DAUGHTER CAN NOT PRODUCE ANOTHER DAUGHTER WITHOUT ABSORBING    ANOTHER ELECTRON INTO ITS NUCLEUS WHICH HAS TO COME FROM ANOTHER PARTICLE somewhat like impregnation and that is probably why they are called daughters.
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the proton\n\nelements with different amounts of neutrons are isotopes of the same element and elements of different amounts of electrons are ions of that element. only if you change the number of protons will you have an different element.
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YES.\n\nthere are always "isotopes" of common elements in the body such as carbon, nitrogen, oxygen, etc.  present at any given time.\n\nisotopes are chemically identical to their "regular" counterpart elements but differ by one or two neutrons in their atoms.  this makes some isotopes radioactive ( a fact which can be measured as in carbon-14 dating ).  \n\nthe effect of this radiation is exceedingly small and of no concern to life.
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A substance whose atoms all have the same number of protons. Neutron numbers may vary (these are called "isotopes"). In a neutral (non-charged) atom, the number of electrons equals the number of protons.
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Because even though it is a radioactive element it's half-life will be over 1/2 million years making it a stable element.  It has what is termed in physics as an 'island of stability' which describes the possibility of elements which have stable 'magic numbers' of protons and neutrons.
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Measuring the background radiation.\nCalculations involving half life.\nCalculating the energy of fusion and fission reactions.
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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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Agricultural Applications - radioactive tracers\n\n\nRadioisotopes can be used to help understand chemical and biological processes in plants. This is true for two reasons: 1)radioisotopes are chemically identical with other isotopes of the same element and will be substituted in chemical reactions and 2)radioactive forms of the element can be easily detected with a Geiger counter or other such device.\nExample:\nA solution of phosphate, containing radioactive phosphorus-32, is injected into the root system of a plant. Since phosphorus-32 behaves indentically to that of phosphorus-31, the more common and non-radioactive form of the element, it is used by the plant in the same way. A Geiger counter is then used to detect the movement of the radioactive phosphorus-32 throughout the plant. This information helps scientists understand the detailed mechanism of how plants utilized phosphorus to grow and reproduce.
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ASTATINE AT A GLANCE \nName: From the Greek astatos, unstable.  \nAtomic mass: (210) \nHistory: First produced in 1940 by Dale R. Corson, K. R. MacKenzie, and Emilio Segrè at the University of California, Berkeley, by bombarding a bismuth isotope with  particles. \nOccurrence: The rarest of the 92 naturally occurring elements; less than 30 g exists on Earth at any one time as a natural by-product of uranium and thorium decay. \nAppearance: Solid nonmetal of unknown color at room temperature. \nBehavior: Highly radioactive; decays very quickly. \nUses: None.
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Atom  \n\nThe smallest unit matter can be divided into whilst still retaining its chemical identity. Atoms are not single particles but complex arrangements of three types of particles. The subatomic particles, protons, neutrons and electrons, combine to form atoms. The protons and neutrons provide the bulk of an atom's mass and are concentrated into a tiny central region known as the atomic nucleus. The nucleus is held together by the strong nuclear force which acts between the constituent particles (termed nucleons ). The protons are positively charged and so mutually repel each other, but it is not until there are many of them that they overcome the nuclear force. Thus there is only one stable element beyond lead (Z=82). Whilst the radius of an atom is in the region of 10-10 metres, the atomic nucleus is about ten thousand times smaller at 10-14 metres. The volume surrounding the nucleus is where the electrons exist. They are much lighter than the protons and neutrons and carry a negative electrical charge. Being opposite in charge to the nucleus, the electrons are held in orbits around it by the force of electromagnetism. The electrons exist in electron orbitals around the nucleus. These orbitals are grouped into shells. Within each shell are energy levels which allow the electrons to exist in unique quantum states, depending upon their angular momentum (hence energy), in accordance with Pauli's exclusion principle . In a neutral atom the number of electrons equals the number of protons. When ionisation occurs, one or more electrons are provided with enough energy to escape the atom altogether. What remains is known as an ion because it is now positively charged and will behave in a different way chemically from neutral atom. The number of protons in the nucleus of an atom (the atomic number , Z) defines which chemical element it is. There are just over 110 known chemical elements and these can be arranged in a classification sequence known as the periodic table. The number of neutrons in any given atomic nucleus can also vary. The total number of protons + neutrons is termed the atomic mass number (A). Most atoms have a prefered number of neutrons at which their nuclei are stable. Atoms with more or less neutrons than the stable configuration are known as isotopes and will often undergo radioactive decay. The simplest of all atoms is hydrogen and is a special case which has a nucleus of one solitary proton and a single electron in orbit around it. It is the only nuclide (species of nucleus) with no neutron. A stable isotope of hydrogen is called deuterium which has one neutron in its nucleus; tritium is an unstable (radioactive) isotope of hydrogen and has two neutrons. See also atomic absorption , atomic emission , atomic number , molecule .
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The atomic number tells you how many protons there are in the nucleus, and that's what identifies the element.  Subtract that number from the atomic weight and you get the number of neutrons.  Uranium has 92 protons and 143 neutrons (U235) or 146 neutrons (U238).  The different weights are called isotopes.  In an electrically neutral atom the number of electrons is the same as the number of protons.  Strip a few electrons away you get an ion (an ionized atom).  It's the structure of the electrons that strongly influences the chemical properties of the element.
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This word is an adjective usually used in "physics."\n\nIt means that something is capable of nuclear fission: fissile material.\n\nWhile fission means the act ir process splitting the Nucleus (=central part) of an atom, when a large amount of energy is released.