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- The different possible versions of each element are called isotopes(/ahy-suh-tohp/). Atoms of the same element can have different numbers of neutrons. For example, the most common isotope of hydrogen has no neutrons at all; there's also a hydrogen isotope called deuterium, with one neutron, and another, tritium, with two neutrons. Another example that you can take is of Carbon, there are a lot of carbon (C) atoms in the Universe. The normal ones, that exist in abundance on earth, are carbon-12. Those atoms have 6 neutrons. There are a few atoms that don't have 6. Those odd ones may have 7 or even 8 neutrons. Carbon-14 actually has 8 neutrons. C-14 is considered an isotope of the element carbon.
- Isotopes are variations of the same element with the same atomic number but a different atomic mass. Isotopes of an element have the same number of protons but a different number of neutrons - which is why their atomic mass is different. On the Periodic Table, the relative atomic mass is featured which is a weighted average from all the abundant isotopes of an element. The isotopes of some elements occur naturally and are said to be 'stable'; others are unstable, meaning that they only exist in a state of decay.
- Isotope is a semi-avid internet roleplayer who started roleplaying in NationStates. After moving to CN, his true love of the roleplay began. His first nation was the Republic of Oasis (he was RPing under the name, King Monster Gup). Not only does he roleplay in Cyber Nations, Isotope also roleplays on many offsite forums under pseudonyms.
- Isotope is a Raven in Armored Core 2. His rank is #6 in the Arena.
- Isotopes are any of the different chemical species of a chemical element each having different atomic mass (mass number).
- Isotopes are variants of elements in which the atoms have the same atomic number but different atomic masses. Different isotopes of an element have the same number of protons in the nucleus but a different number of neutrons.
- Isotopes are atoms of a chemical element whose nuclei have the same atomic number, Z, but different atomic weights, A. The word isotope, meaning at the same place, comes from the fact that isotopes are located at the same place on the periodic table. Collectively, the isotopes of the elements form the set of nuclides. A nuclide is a particular type of nucleus (characterised by A and Z). Strictly speaking, we should say that an element such as fluorine consists of one nuclide rather than that it has one isotope. Similarly, the tables at the foot of this article are tables of nuclides.
- An isotope is an atom with a different number of neutrons. The charge is still 0, unlike ions. There are radioactive isotopes, which are used in nuclear reactions. In radioactivity, only the nucleus is important. Add in extra neutrons, and the atom is heavier. It is still the same element. Take a neutron out, making it lighter, and it's still the same element. This is called an "isotope". Isotopes are the reason why some elements have a relative atomic mass that is not a whole number. The RAM is calculated with the natural abundance of each isotope. Example:
- Isotopes are atoms of a chemical element that have the same atomic number (making them essentially the same element) but different mass numbers (resulting in different properties) due to a different number of neutrons in the atom's nucleus. For example, hydrogen has three isotopes: protium (one proton), deuterium (one proton and one neutron), and tritium (one proton and two neutrons). In the 2060s, Earth's atmosphere was irradiated with radioactive isotopes in the aftermath of World War III. (Star Trek: First Contact) Caatati technology was dependant on thorium isotopes. (VOY: "Day of Honor")
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| - [[Category:/Creator]] [[Category:/Creator]] [[Category:/Creator]] [[Category:/Creator]] [[Category:/Creator]] [[Category:Characters by Name ]]
- An isotope is an atom with a different number of neutrons. The charge is still 0, unlike ions. There are radioactive isotopes, which are used in nuclear reactions. In radioactivity, only the nucleus is important. Add in extra neutrons, and the atom is heavier. It is still the same element. Take a neutron out, making it lighter, and it's still the same element. This is called an "isotope". Isotopes are the reason why some elements have a relative atomic mass that is not a whole number. The RAM is calculated with the natural abundance of each isotope. Example: Chlorine has 2 main isotopes 35Cl occurring 75% of the time, and 37Cl occurring 25% of the time. Cl ((35*75)+(37*25))/100=35.5 RAM or Ar is simply how heavy atoms are compared with 1/12 Carbon-12 however isotopes do not beahve any different in chemical reactions There are many types of Hydrogens e.g. deuterium and tritium. Tritium has an unstable nucleus - the forces holding the proton and neutrons together are weak. They will decay, so are radioactive. Radioactive isotopes are sometimes called radioisotopes.
- Isotopes are atoms of a chemical element that have the same atomic number (making them essentially the same element) but different mass numbers (resulting in different properties) due to a different number of neutrons in the atom's nucleus. For example, hydrogen has three isotopes: protium (one proton), deuterium (one proton and one neutron), and tritium (one proton and two neutrons). In the 2060s, Earth's atmosphere was irradiated with radioactive isotopes in the aftermath of World War III. (Star Trek: First Contact) In 2151, the Malurians were secretly mining the Akaali homeworld for veridium isotopes. (ENT: "Civilization") A gas giant investigated by Enterprise NX-01 in 2152 had many moons with atmospheres containing selenium isotopes. These isotopes interfered with sensors, hampering the search for Charles Tucker when his shuttlepod was shot down over one of the moons. (ENT: "Dawn") In the mid-24th century, the Haakonians used Metreon isotopes in the metreon cascade, a weapon used on the Talaxian moon, Rinax. (VOY: "Jetrel") Caatati technology was dependant on thorium isotopes. (VOY: "Day of Honor") Trilithium isotopes are used in Romulan plasma torpedoes. (DS9: "Image in the Sand")
- The different possible versions of each element are called isotopes(/ahy-suh-tohp/). Atoms of the same element can have different numbers of neutrons. For example, the most common isotope of hydrogen has no neutrons at all; there's also a hydrogen isotope called deuterium, with one neutron, and another, tritium, with two neutrons. Another example that you can take is of Carbon, there are a lot of carbon (C) atoms in the Universe. The normal ones, that exist in abundance on earth, are carbon-12. Those atoms have 6 neutrons. There are a few atoms that don't have 6. Those odd ones may have 7 or even 8 neutrons. Carbon-14 actually has 8 neutrons. C-14 is considered an isotope of the element carbon.
- Isotopes are atoms of a chemical element whose nuclei have the same atomic number, Z, but different atomic weights, A. The word isotope, meaning at the same place, comes from the fact that isotopes are located at the same place on the periodic table. The atomic number corresponds to the number of protons in an atom. Thus, isotopes of a particular element contain the same number of protons. The difference in atomic weights results from differences in the number of neutrons in the atomic nuclei. In scientific nomenclature, isotopes are specified by the name of the particular element by a hyphen and the number of nucleons (protons and neutrons) in the atomic nucleus (e.g., helium-3, carbon-12, carbon-14, iron-57, uranium-238). In symbolic form, the number of nucleons is denoted as a superscripted prefix to the chemical symbol (e.g., 3He, 12C, 14C, 57Fe, 238U). Collectively, the isotopes of the elements form the set of nuclides. A nuclide is a particular type of nucleus (characterised by A and Z). Strictly speaking, we should say that an element such as fluorine consists of one nuclide rather than that it has one isotope. Similarly, the tables at the foot of this article are tables of nuclides. In a neutral atom, the number of electrons equals the number of protons. Thus, isotopes of a given element also have the same number of electrons and the same electronic structure. Because the chemical behavior of an atom is largely determined by its electronic structure, isotopes exhibit nearly identical chemical behavior. The primary exception is that, due to their larger masses, heavier isotopes tend to react somewhat more slowly than lighter isotopes of the same element. This "mass effect" is most pronounced for protium (1H) and deuterium (the common name of 2H), because deuterium has twice the mass of protium. For heavier elements the relative mass difference between isotopes is much less, and the mass effect is usually negligible. Although isotopes exhibit nearly identical electronic and chemical behavior, their nuclear behavior varies dramatically. Atomic nuclei consist of protons and neutrons bound together by the strong nuclear force. Because protons are positively charged, they repel each other. Neutrons, which are electrically neutral, allow some separation between the positively charged protons, reducing the electrostatic repulsion and stabilizing the nucleus. For this reason neutrons are necessary for two or more protons to be bound into a nucleus. As the number of protons increases, additional neutrons are needed to form a stable nucleus, for example, although the neutron/proton ratio of 3He is 1/2, the neutron/proton ratio of 238U is >3/2. However, if too many neutrons are present, the nucleus becomes unstable. Because isotopes of a given element have different numbers of neutrons they also have different neutron/proton ratios. This affects the nuclear stability, with the result that some isotopes are subject to nuclear decay. The decay of these radioactive isotopes (radioisotopes for short) is an important topic in nuclear physics. By studying the manner in which this decay occurs, physicists gain insight into the properties of the atomic nucleus. In general, several isotopes of each element can be found in nature. Stable isotopes are by far the most abundant; however, significant quantities of long-lived unstable isotopes, such as uranium-238, can also be found. Small amounts of short-lived radioactive isotopes are also present in nature. These arise as products of the decay of larger long-lived radioactive nuclei. The atomic mass for an element in the periodic table is the average of the natural abundance of the isotopes of that element. The amounts of the various isotopes on earth is ultimately the result of the amounts formed in stars and supernovae, and the subsequent decay patterns of the radioactive nuclei formed in these processes. After that, the formation of the solar system also influenced heavily on the proportions of different isotopes found here, since lighter nuclei was more easily blown away towards the outer parts of the solar system, by the solar wind immediately after the sun was formed. This is also why the gas giants are located further from the sun.
- Isotopes are variations of the same element with the same atomic number but a different atomic mass. Isotopes of an element have the same number of protons but a different number of neutrons - which is why their atomic mass is different. On the Periodic Table, the relative atomic mass is featured which is a weighted average from all the abundant isotopes of an element. The isotopes of some elements occur naturally and are said to be 'stable'; others are unstable, meaning that they only exist in a state of decay.
- Isotope is a semi-avid internet roleplayer who started roleplaying in NationStates. After moving to CN, his true love of the roleplay began. His first nation was the Republic of Oasis (he was RPing under the name, King Monster Gup). Not only does he roleplay in Cyber Nations, Isotope also roleplays on many offsite forums under pseudonyms.
- Isotope is a Raven in Armored Core 2. His rank is #6 in the Arena.
- Isotopes are any of the different chemical species of a chemical element each having different atomic mass (mass number).
- Isotopes are variants of elements in which the atoms have the same atomic number but different atomic masses. Different isotopes of an element have the same number of protons in the nucleus but a different number of neutrons.
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