how many isotopes does cobalt have?
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Webelements says there is only one naturally-occurring isotope of cobalt (Co-59).  It also list about 7 or 8 radioisotopes.
146629
The sodium atom has the atomic number of 11.  This means that it has 11 protons in the nucleus and 11 electrons in the space around it.\nThe most abundant isotope of sodium has an atomic weight of 23, this means that there are (23 - 11 = 12) 12 neutrons also in the nucleus.\nThe sodium atom has 11 protons, 12 neutrons and 11 electrons.\nThe sodium ion has a positive charge by loosing one of its electrons.  So the ion has 11 protons, 12 neutrons and 10 electrons.
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cobalt, metallic chemical element; symbol Co; at. no. 27; at. wt. 58.9332; m.p. 1,495°C; b.p. about 2,870°C; sp. gr. 8.9 at 20°C; valence +2 or +3. Cobalt is a silver-white, lustrous, hard, brittle metal. It is a member of group VIII of the periodic table. Like iron, it can be magnetized. It is similar to iron and nickel in its physical properties. The element is active chemically, forming many compounds, e.g., the series of cobaltous and cobaltic salts and the complex cobalt ammines derived from cobaltic salts and ammonia. Cobalt yellow, green, and blue are pigments of high quality that contain cobalt; another blue pigment, smalt, is made by powdering a fused mixture of cobalt oxide, potassium carbonate, and sand; these pigments are often used for coloring glass and ceramics. Cobalt chloride, used as an invisible ink, is almost colorless in dilute solution when applied to paper. Upon heating it undergoes dehydration and turns blue, becoming colorless again when the heat is removed and water is taken up. The element rarely occurs uncombined in nature but is often found in meteoric metal. It is a constituent of the minerals cobaltite and smaltite and of other ores, usually in association with other metals. Pure cobalt metal is prepared by reduction of its compounds by aluminum (the Goldschmidt process), by carbon, or by hydrogen. It is a component of several alloys, including the high-speed steels carboloy and stellite, from which very hard cutting tools are made. It is a component of some stainless steels, and of high-temperature alloys for use in jet engines. Alnico, an alloy of cobalt, aluminum, nickel, and other metals, is used to make high-strength, permanent magnets. As an element in the diet of sheep, cobalt prevents a disease called swayback and improves the quality of the wool. A radioactive isotope, cobalt-60 (with gamma ray emission 25 times that of radium), is prepared by neutron bombardment. It is used for cancer therapy and in industry for detecting flaws in metal parts. See hydrogen bomb. Cobalt was discovered in 1735 by Georg Brandt, a Swedish chemist.
213411
Atomic Number 3\nhttp://www.jergym.hiedu.cz/~canovm/vyhledav/varianty/litva.gif
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Are you talking of naturally occuring Radio isotopes like Carbon-14 or the synthesized ones like Cobalt-60 or krypton:\n\nAnyway, I will try!\n\n1. Carbon Dating: Living things absorb a certain amount of carbon-14 as long as they are living. When they die the Carbon-14 starts to decay at a half-life of 5730 yrs, by measuring the amount of the residue Carbon-14,the time since their death can be determined.\n\n2. In medicine:Positron emission Tomography PET uses radio isotopes to collect a tracer on brain activity including cerebral metabolism and oxygen use, while Nuclear magnetic Resonance is used to collect images of tissues that a more precise than CAT scans\n\n3. In industry, cobalt 60 is used to detect flaws in steel as thick as 6 inches, by picking up beta and gamma radiation on a photographic film emitted after radiating a cobalt wire.\n\n4.Nuclear Power production:Water heated due to radioactive decay produces steam to turn turbines that turn massive electric generators!\n\n5.Least desirable use: Nuclear weapons use the chain reaction properties to unleash megajoules of destructive energy!
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Answers:\n\n(a) Thorium-234>Proactinium-234 = -1e (beta decay)\n\n(b) Hydrogen + Hydrogen > Helium (fusion)\n\n(c) Uranium-238 > Thorium-234 + Helium-4 (alpha decay)
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Carbon's atomic number is six.  The innermost shell contains two electrons.  The next shell needs eight to be complete, but carbon has only four left.  Therefore, it needs four additional electrons to complete the shell.
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Same number of protons\n\ndifferent number of neutrons
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cobalt-60 may be used to control or eliminate cancerous growth caused by rapidly dividing cells by irradiating the area of the growth. \nI-131 is used to treat thyroid cancer and non malignant thyroid disorders.\nIr-192 implants are used specially for the head and the breasts.\nMost therauptic methods are generally used to relieve pain,strontium-89 and samarium-153 are used for relief of cancer-induced bone pain.\nOne more isotope used widely in medicine is technitium-99.Tc is one of the artificially prepared elements.\ntry this site,it gives u the details as to how these radioisotopes are used in medicine.
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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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235 Uranium + 1 neutron --> 140 Cesium + 93 Rubidium + 3 neutrons
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The mass of a nucleus indicates the number of protons and neutrons present in the nucleus. An element can have more than one isotope eg Carbon 12 and Carbon 14. The former has 6 protons and 6 neutrons, The latter 6 protons and 8 neutrons. \n\nThe atomic weight of an isotope refers to the numbers of protons AND neutrons present. The atomic number of an element refers to the number of protons in all its isotopes.\n\nHydrogen, though normally just a solo proton in its nucleus, does have two isotopes, deuterium, with 1 neutron, and tritium with two neutrons.\n\nA recent question asked about silver, how many of each in its nucleus. Its atomic number is 47, so clearly 47 protons. Naturally-occurring silver is given as having  an atomic weight of 108, so answerers answered 61 neutrons.\n\nHowever there is a subtlety they missed..\n\nNaturally-occurring silver is a mixture of Ag 107 (60 neutrons) and Ag 109 (62 neutrons). (Slightly more than 50% of the former.).\n\nSo the average atomic weight of the two isotopes is 108. But there is no Ag 108 isotope present. The wrong inference was drawn.\n\nSeveral people above are confusing atomic weight and atomic number, and what they each mean. So if you don't understand several of the answers it is because they are jumbled versions of the true picture.
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atomic mass unit, 1/12 of the mass the carbon 12, the most common carbon isotope. Try a periodic table.\n\n\n**** \n1 atomic mass unit = 1.66053886 × 10-27 kilograms
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Yes, you are correct. The atomic number of Molybdenum is 42.
878474
Um, there's over a hundred elements.  I'm not going to name them all for you.  Look at a periodic table.  I'm sure there's one in your chemistry book.
649511
A carbon atom is one that has 6 proton in the nucleus. If it is uncharged, there will also be 6 electrons. The number of neutrons varies depending on the isotope. The most common isotope has 6 neutrons. There is another stable isotope with 7 neutrons and a radioactive one with 8.
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It would be either an isotope or an ion depending on the number of neutrons or electrons in the atom.\nA good example of this for isotopes is hydrogen:\nWhen there is no neutrons it is H1 or just plain hydrogen\nWhen there is 1 neutron it is Deuterium or H2 also called heavy hydrogen\nWhen there is 2 neutrons it is called tritium or H3\n\nIf the only difference is the addition or removal of one or more electrons it is an Ion.