Is Tin-106 a stable nuclide and if why?
484798
Stable? An isotope stable? Relative to other other isotopes maybe.
605534
TrueGentalman, Actually Such element DOES Exist.  Read on...\n\nErbuim has the atomic number of 68, but its Mass is not 68 amu.  It is actually 167.26 amu or 167.26g/mol.  Although it appears that no element has the exact mass of 68 amu in periodic table, Zinc having mass of 65.39 has a mass very close to 68.\n\nThe fact that Zinc has mass with a decimal suggests that it has isotopes and Zinc indeed has many isotopes.  \n\nThe TRUE answer to this question is Zinc-68.  It is a naturally occurring stable isotope of Zinc having atomic mass of exactly 68 amu.  \n\nI hope this helps.
300254
None of them.  \nTechnetium has been observed both in spectral star signatures, and in very small quantities in pitchblende.  To quote from Wickepedia "In 1962, technetium-99 was isolated and identified in pitchblende from the Belgian Congo in very small quantities (about 0.2 ng/kg); there it originates as a spontaneous fission product of uranium-238. This discovery was made by B.T. Kenna and P.K. Kuroda."
438964
For the Molybdenum 93 Isotope (synthetic radioisotope) 4,000 years.\nFor the Molybdenum 99 Isotope (synthetic radioisotope) it is 65.94hours.\nFor the Molybdenum 100 Isotope it is 7.8x10^18 years.\nAll other Isotopes of Molybdenum (92,94,95,96,97) are stable Isotopes.
1116618
It has a 2 microsecond half life, so it is not abundant anywhere. You can hardly keep it in a jar.\n\nIt is made at supercolliders, such as CERN.
450990
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.
1106952
There are 24 isotopes of potassium (atomic number 19), ranging in atomic mass from 32 to 54 amu.\n\nThe most abundant isotope, K39 (which comprises 93.26% of all potassium known), is stable, as is the next most abundant isotope, K41 (6.73%).  So the stable isotopes make up 99.99% of all the potassium in the world.\n\nOne other stable isotope, K32, is present in vanishingly small portions. \n\nHowever, that remaining 0.01% consists of the other 21 known isotopes, all of which are radioactive to some degree:\n\nK33 has a half-life less than 25 nanoseconds.\nK34 has a half-life less than 40 nanoseconds.\nK35 is a positron/gamma emitter with a half-life  of 0.19 seconds.\nK36 is a positron/gamma emitter with a half-life of 0.342 seconds.\nK37 is a positron/gamma emitter with a half-life of 1.23 seconds.\nK38m is a positron emitter with a half-life of 0.924 seconds.\nK38 is a positron/gamma emitter with a half-life of 7.63 minutes.\nK39 is stable.\nK40 is 0.01% of the total, and is a beta/gamma emitter with a half-life of 1.26x10^9 years.\nK41 is stable.\nK42 is a beta/gamma emitter with a half-life of 12.36 hours.\nK43 is a beta/gamma emitter with a half-life of 22.3 hours.\nK44 is a beta/gamma emitter with a half-life of 22.1 minutes.\nK45 is a beta/gamma emitter with a half-life of 17.8 minutes.\nK46 is a beta/gamma emitter with a half-life of  1.8 minutes.\nK47 is a beta/gamma emitter with a half-life of 17.5 seconds.\nK48 is a beta/gamma emitter with a half-life of 6.8 seconds.\nK49 is a beta/gamma emitter with a half-life of 1.26 seconds.\nK50 is a beta emitter with a half-life of 0.472 seconds.\nK51 is a beta emitter with a half-life of 0.365 seconds.\nK52 is a beta emitter with a half-life of 0.105 seconds.\nK53 is a beta emitter with a half-life of 30 milliseconds.\nK54 is a beta emitter with a half-life of 10 milliseconds.
244528
There are some numbers such as 20, 82, etc. which signifyu that if the difference between the number of protons and neutrons or the umber of protons or the number of neutrons are equal to that number then the nucleus is especially stable. No exact scientific reason is present to explain this effect. So these are called magic numbers.
796089
if neutron proton ratio is 1 or less than 1.5 then the metal is stable but if the ratio is higher than 1.5 then the substance is not stable.
1047499
If it existed, it would be boron pentafluoride, but as far as I know, this is not a stable molecule.\n\nAre you sure you don't mean BrF5 (bromine pentafluoride), which does exist as a stable molecule?
59635
Elements with octet configuration are more stable because the last layer of electrons is complete, so it doesn't have empty spaces to be filled by other elements (not easily). It is not impossible, but hard and not likely to happen under normal conditions. Under special circumstances, I suppose they do mix, like your case with Xenon.
399354
Yes.The six noble gases are found in group 18 of the periodic table. These elements were considered to be inert gases until the 1960's, because their oxidation number of 0 prevents the noble gases from forming compounds readily. All noble gases have the maximum number of electrons possible in their outer shell (2 for Helium, 8 for all others), making them stable. \n\nHelium \nNeon \nArgon \nKrypton \nXenon \nRadon
742905
Yes it's the same element,except that in the human body it's an ionized form,not a metallic form, only traces are required or else it would cause severe poisoning causing CNS and liver malfunction.
139410
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.
547737
kiki is right, and most other answers wrong. 'Decay' is only applied to radioactive elements, and not all elements are radioactive. Many have *isotopes* that are radioactive, but aren't the stable form of the element. For example, carbon 14 is radioactive carbon and decays; Carbon 13, the stable version, will never do so. \n\nStable elements can go through fusion or fission, effectively changing them into something else (for example, carbon fuses at about 600 million degrees K), but that is *not* decay, since decay involves *spontaneous* emission of radiation, and that event only involves external factors, like a star exploding, and is not a property of the element - so, again, that can't be called 'decay'.\n\nSo, no, not all elements decay over time, only the ones that have no stable isotope - all elements above 83, bismuth.
165489
The half-life of a radioactive element is the time it takes for half of its atoms to decay into something else. \n\nFor example, the half-life of I-125 is 60 days. Therefore, in 60days, one gram of I-125 will turn into half a gram of I-125  and half a gram of something else (the radioactive decay products of Iodin). After another 60 days have elapsed, only a quarter of a gram of the original I-125 will remain.\n\nThe radio active decay product of I-125 is tellurium-125 which is a stable. These elements decay by emitting radiations or capturing electron from near bys shells in order to become stable.
290665
3.45×10^−25 kg = Lead-208 atom, the heaviest stable isotope known\n\ncheck here http://en.wikipedia.org/wiki/Orders_of_magnitude_(mass) good luck