What is the difference between isomers and isotopes?
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Isomers are molecules with the same chemical formula but different structures.  Isotopes are atoms of the same element but have different numbers of neutrons.  The right one for carbon is isomer
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technically, a system that consists of homogeneous atoms or molecules bonded to each other is called a "lattice," or a "crystal lattice."  The difference is that, with a molecule, splitting it or removing components of it would change its chemical properties, whereas with a lattice, splitting it causes no chemical changes and only reduces its size.  Therein lies the difference.
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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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Electron configuration is related to the number of protons in the nucleus, hence, the element. In theory, all isotopes of a certain element should have the same electron configuration.\n\nWhat u were asking for is an electron configuration for oxygen anion, it has the same electron configuration as Neon\n\nelectron configuartion of O^2- = [Ne] (Neon core) = 1s^2 2s^2 2p^6
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Isomers\n\nIn chemistry, isomers are molecules with the same chemical formula and often with the same kinds of bonds between atoms, but in which the atoms are arranged differently. That is to say, they have different structural formulae. Many isomers share similar if not identical properties in most chemical contexts. This should not be confused with a nuclear isomer, which involves a nucleus at different states of excitement.\n\nA simple example of isomerism is given by propanol: it has the formula C3H8O (or C3H7OH) and two isomers Propan-1-ol (n-propyl alcohol; I) and Propan-2-ol (isopropyl alcohol; II)
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Isotopes: Protium, Deuterium, Tritium (naturally occurring)\nOther isotopes (synthesized):\n\n============================================================\nIsotopes\nMain Article: Isotopes of hydrogen \nHydrogen is the only element that has different names for its isotopes. (During the early study of radioactivity, various heavy radioactive isotopes were given names, but such names are no longer used, although one element, radon, has a name that originally applied to only one of its isotopes.) The symbols D and T (instead of 2H and 3H) are sometimes used for deuterium and tritium, although this is not officially sanctioned. (The symbol P is already in use for phosphorus and is not available for protium.)\n\n1H \nThe most common isotope of hydrogen, this stable isotope has a nucleus consisting of a single proton; hence the descriptive, although rarely used, name protium. The spin of a protium atom is 1/2+. [6]\n\n2H \nThe other stable isotope is deuterium, with an extra neutron in the nucleus. Deuterium comprises 0.0184%–0.0082% of all hydrogen (IUPAC); ratios of deuterium to protium are reported relative to the VSMOW standard reference water. The spin of a deuterium atom is 1+.\n\n3H \nThe third naturally occurring hydrogen isotope is the radioactive tritium. The tritium nucleus contains two neutrons in addition to the proton. It decays through beta decay and has a half-life of 12.32 years. Tritium occurs naturally due to cosmic rays interacting with atmospheric gases. Like ordinary hydrogen, tritium reacts with the oxygen in the atmosphere to form T2O. This radioactive "water" molecule constantly enters the Earth's seas and lakes in the form of slightly radioactive rain, but its half-life is short enough to prevent a buildup of hazardous radioactivity. The spin of a tritium atom is 1/2+.\n\n4H \nHydrogen-4 was synthesized by bombarding tritium with fast-moving deuterium nuclei. It decays through neutron emission and has a half-life of 9.93696x10-23 seconds. The spin of a hydrogen-4 atom is 2-.\n\n5H \nIn 2001 scientists detected hydrogen-5 by bombarding a hydrogen target with heavy ions. It decays through neutron emission and has a half-life of 8.01930x10-23 seconds.\n\n6H \nHydrogen-6 decays through triple neutron emission and has a half-life of 3.26500x10-22 seconds.\n\n7H \nIn 2003 hydrogen-7 was created (article) at the RIKEN laboratory in Japan by colliding a high-energy beam of helium-8 atoms with a cryogenic hydrogen target and detecting tritons—the nuclei of tritium atoms—and neutrons from the breakup of hydrogen-7, the same method used to produce and detect hydrogen-5.\n============================================================\n\nWater: H2O (one).
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Atomic mass depends on the element. It accounts for all isotopes and does a sort of weighted average, depending on how often the isotope occurs in nature.\nMass number depends on the isotope.\n\nFor example, atomic mass of hydrogen is 1.0079. The mass number of most hydrogen atoms is 1. Deuterium is an isotope with a neutron in its nucleus, so its mass number is 2. Tritium is an isotope with two neutrons, so its mass number is 3.
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Isotopes of the same element have *almost* identical chemical properties. They can be distinguished because they have different masses (from a different number of neutrons in the nucleus). But this effect is usually very small. One exception is hydrogen. The isotope consisting of one protoon and one neutron in the nucleus (deuterium) has double the mass of a regular hydrogen atom, and this can have observable effects even on the chemistry.
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The atomic number equals the number of protons.  Electrons should equal the number of protons, but may not if it's an ion.  Neutrons vary as to the specific isotope of the atom.\n\nExample:\nHydrogen, atomic number = 1.  Therefore, 1 proton, 1 electron.\nIt has three isotopes:\nH-1 (1 proton, 1 electron, no neutrons)\nH-2 (1 proton, 1 electron, 1 neutron)\nH-3 (1 proton, 1 electron, 2 neutrons).\n\nYou might check the section you are asking this in, though.  This is the Religion section.
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they have the same number of protons and electrons but differing numbers of neutrons.  Since it is the electrons that determin the chemical properties of an element, two isotopes will react the same chemically, but may react differently nuclearly
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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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Same number of protons\n\ndifferent number of neutrons
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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.
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if u bombard the nucleus of one element with protons or neutrons the elements can change so they are basically interchangeable while cells are at much more complex level of differentiation
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Iso- as a prefix means "the same". Thus isobar (same pressure), isosceles triangle (two sides the same length) and isotope two or more versions of the same element which all have the same number of protons (or it would be a different element!) but varying numbers of neutrons in the nucleus.\n\nAs protons are positively charged and neutrons have no charge (electrons have a negative charge) neutrons are needed as "packing materials" to help keep the positive charges fom repelling one another and making the nucleus unstable.\n\nWith elements of low atomic number, the number of neutrons will be the same or just greater than the number of protons. But with elements of high atomic number, more packing materials are needed, and the ratio of neutrons to protons begins to climb towards 1.5:1\n\nThere is only a narrow range of options for that ratio for isotpes that are stable. Those with too few or too many neutrons, iutside that range, are unstable and decay.\n\nCompare Carbon 12 and Carbon 14 with Uranium 235 and Uranium 238\n\nCarbon 12 has 6 protons and 6 neutrons and is stable\n\nCarbon 14 has 6 protons and 8 neutrons and is unstable, it decays\n\nU235 has 92 protons, 143 neutrons and is unstable.\n\nU238 has 92 protons, 146 neutrons and is unstable\n\nAs regards silver (Ag) oy has two stable isotopes Ag 107 (47p, 60n) and Ag 109 (47p, 62n) But very short-lived isotopes varying in atomic mass from the neutron-deficient Ag 93 (47p, 46 n) to Ag 123 (47p 76n) also exist.
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Trans- isomers are more stable than cis- isomers because they keep similar groups farther apart.  For example, trans- and cis- dichloro-ethene:\n\nTrans- vs. Cis- dichloroethene:\ntrans:\nhttp://shrimpandgrits.rickandpatty.com/blogfiles/transdce.png\ncis:\nhttp://shrimpandgrits.rickandpatty.com/blogfiles/cisdce.png\n\nObviously, in trans, the two Cl's are farther apart.  The story of stability in chemistry and materials is that alike things don't like to be by each other (like 2 positive charges or 2 magnetic norths repeling each other).  In organics, like groups close to each other experience what's called steric interactions, which make a molecule more unstable than the two alike groups being as far away as possible.
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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.