Definitions for "Isotopes"
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Isotope , Nuclide, Mass number, Boson , Bosons, Atomic number, Atom, Fermion, Subatomic particle, Atoms, Elementary particle, Fermions, Proton, Hyperon, Antiparticle, Meson, Atomic nucleus, Nucleon number, Neutrons, Deuteron, Quarks, Nuclei, Neutron, Alpha particles, Protons, Electron, Baryons, Baryon, Lepton, Antimatter, Pion, Nucleon, Hadrons, Hadron, Qcd, Muon, Subatomic particles, Atomic mass, Quark , Hydrogen atom, Quantum chromodynamics, Deuterium, Pauli exclusion principle, Leptons, Neutrino, Electrons, Neutron number, Annihilation, Gluon, Higgs boson
different forms of an element that have the same number of protons in their nuclei, and thus the same atomic number, but that have different numbers of neutrons and thus different atomic masses. There are two kinds of isotopes, stable and unstable. Isotopes that are unstable are called radioactive and disintegrate at a constant decay rate. Examples of stable isotopes include carbon-12 and carbon-13. Carbon-14, and uranium-238 and -235, are examples of unstable isotopes.
Atoms of the same element having the same chemical properties but differing in mass and in the physical properties that depend on their mass.
atoms whose nuclei have the same atomic umber but different mass numbers
A form of an element in which the atoms have more (or less) than the usual number of neutrons. Isotopes of a given element have identical chemical propertied, but they differ in mass (weight, extra neutrons) as a result of the additional (or lesser) neutrons. Many isotopes are unstable and radioactive.
Isotopes are different forms of the same chemical element, which have different numbers of neutrons but the same number of protons in the nucleus of their atoms. A single element may have many isotopes. For example, stable iodine is iodine-127. Its radioactive isotopes include iodine-129 and iodine-131.
Atoms with the same atomic number, but different mass numbers (same number of protons but a different number of neutrons).
All elements have isotopes, some more than others. There are two kinds of isotope, stable and unstable. A stable isotope does not disintegrate and is therefore not radioactive. An unstable isotope is radioactive and disintegrates to form other elements. (see Elements, Atoms and Isotopes)
Atoms of the same element but with different mass numbers. They have the same number of protons in their nucleus but different numbers of neutrons. For example, helium-3, an isotope of helium, contains two protons and one neutron. Helium-4 has two protons and two neutrons.
Nuclides with the same number of protons, such as 12C, 13C, and 14C.
Atoms of the same element that have equal numbers of protons, but different numbers of neutrons. Isotopes of an element have the same atomic number by different atomic mass. For example, uranium-238 and uranium-235.
Isotopes are two or more nuclides with the same atomic number but different mass number . The term is sometimes used synonymously with nuclide, but it is preferable to reserve the word nuclide for a species of specific and .
different forms of an element (depending on the number of neutrons)
Two or more forms of a chemical element that have the same number of protons but different mass numbers because they have different numbers of neutrons in their nuclei.
atoms with nuclei possessing the same number of protons but different numbers of neutrons.
Forms of an element whose atoms contain the same number of protons but different numbers of neutrons (and thus differ in atomic weight).
3/4 Nuclides having the same atomic number but different mass numbers.
All elements have isotopes, some more than others. There are two kinds of isotope, stable and unstable. A stable isotope does not disintegrate and is therefore not radioactive. An unstable isotope is radioactive and disintegrates to form other elements. ilo (k) Thousand = 1000 = 103
Chemically identical atoms of the same element with different numbers of neutrons in their nuclei and thus different atomic masses (for example, U-238 and U-235).
Physically and chemically different atoms of the same element, resulting from differences in the number of neutrons in the atomic nuclei.
Nuclei containing the same number of protons but different numbers of neutrons. Most elements can exist in several isotopic forms. A common example of an isotope is deuterium, which differs from normal hydrogen by the presence of an extra neutron in the nucleus.
atoms of the same element with different numbers of neutrons in their nuclei, i.e. the same atomic numbers but different mass numbers.
Elements with the same number of protons but have different numbers of neutrons, and thus different masses. Back to .
All atoms of the same element posses the same no. of protons and electrons but not neccarily the same no. of neutrons. So all atoms of an element will react in the same way, but they can differ in their molecular masses. Atoms of the same element with different masses are known as isotopes. Hydrogen has three isotopes. 99.98% of all hydrogen has one proton and one electron, while 0.02% of hydrogen has one proton, one neutron and one electron. This isotope is called deuterium. There is also a trace of a third isotope, tritium, which has two neutrons in its nucleus.
forms of the same chemical element that differ only in terms of the number of neutrons in their nucleus.
Nuclides having the same number of protons in the nuclei, and hence having the same atomic number, but differing in the number of neutrons, and therefore in mass number. Almost identical chemical properties exist among isotopes of a particular element.
Forms of a single element that differ in atomic mass due to a different number of neutrons in the nucleus.
Two or more nuclides having the same atomic number, thus constituting the same element, but differing in the mass number. Isotopes of a given element have the same number of nuclear protons but differing numbers of neutrons. Naturally occurring chemical elements are usually mixtures of isotopes so that observed (non-integer) atomic weights are average values for the mixture.
Atoms of the same element which have the same number of protons but a different number of neutrons in the nuclei.
Nuclides that have the same number of protons. Isotopes of a nuclide have nearly the same chemical properties, but somewhat different physical properties.
Atoms of the same element but which differ in the numbers of neutrons in their nuclei (or, have different mass numbers).
Atomic species differing in mass number but having the same atomic number. (Grant & Hackh's Chemical Dictionary, 5th ed)
Atoms having different atomic masses or mass numbers, but the same atomic number.
Different forms of the same chemical element that differ only by the number of neutrons in their nucleus. Most elements have more than one naturally occurring isotope. Many isotopes that do not exist in nature have been produced in reactors and particle accelerators.
Atoms with the same number of protons (and electrons) but different masses.
members of a chemical-element family with the same number of protons in its nucleus, but a different number of neutrons, so that while they have the same chemical attributes, they often display different physical attributes. For example, U-235, which can maintain a nuclear chain-reaction, and U-238, which can not, are different isotopes of uranium.
Forms of a chemical element that have the same number of protons and electrons, but differ in the number of neutrons contained in the atomic nucleus. Unstable isotopes undergo a transition to a more stable form with the release of radioactivity.
Forms of an element in which atoms have the same number of protons but different numbers of neutrons.
One of two or more atoms having the same atomic number but different mass numbers.
Nuclides with the same number of protons but different numbers of neutrons. Nuclides with the same number of protons but different numbers of neutrons. Not a synonym for nuclide.
Atoms that have an equal number of protons, and hence are of the same element, but differ in their number of neutrons. This results in a difference ofmass. Isotopes may be either stable or unstable—that is, radioactive.
Two or more forms of atoms of the same element with different masses; atoms containing the same number of protons but different numbers of neutrons.
Various forms of a chemical element (e.g., carbon) that have different numbers of neutrons and therefore different atomic mass.
Nuclides with the same number of protons, but different numbers of neutrons, e.g. U-235 (92 protons and 143 neutrons) and U-238 (92 protons and 146 neutrons). The number of neutrons in an atomic nucleus, while not significantly altering its chemistry, does alter its properties in nuclear reactions.
Different forms of the same element. Isotopes of an element have different numbers of neutrons in the nuclei of their atoms, but the same number of protons. Some isotopes, called radioisotopes, are unstable and emit radiation.
Forms of the same element that have different numbers of neutrons (p.208-209).
Atoms of the same element that have different numbers of neutrons are called isotopes. Classifying materials
atoms of the same element (the same number of protons) that have different numbers of neutrons. They have identical atomic numbers but different mass numbers.
Atoms that have an equal number of protons, and hence are of the same element, but differ in their number of neutrons. This results in a difference of mass. An isotope may either be stable or radioactive.