what is the major difference between an element and its isotopes?
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Isotopes are atoms of the same element that have different numbers of neutrons but the same number of protons and electrons. The difference in the number of neutrons between the various isotopes of an element means that the various isotopes have different masses.
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Isotopes of an element have the same number of protons but different numbers of neutrons. Because the mass number is the sum of the atomic number (number of protons) and the number of neutrons, isotopes of the same element have different mass numbers.
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Because different isotopes have different numbers of neutrons, they do not all weigh the same or have the same mass. Different isotopes of the same element have the same atomic number. They have the same number of protons. The atomic number is decided by the number of protons.
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What makes one element different from another is the number of protons in the nucleus of its atoms. ... Atoms contain protons and neutrons in the nucleus and electrons outside the nucleus. Each element has a unique number of protons, known as its atomic number.
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A particular atom will have the same number of protons and electrons and most atoms have at least as many neutrons as protons. ... All isotopes of a particular element have the same number of protons, but can have different numbers of neutrons.
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Atoms of the same element that differ in their numbers of neutrons are called isotopes. ... Different isotopes of an element generally have the same physical and chemical properties. That's because they have the same numbers of protons and electrons.
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Atoms of the same element can differ in their mass which is the case if the number of neutrons in the atoms is not the same. These atoms with different mass are called isotopes.
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1) Two isotopes of a certain element have binding energies that differ by 5.03 MeV. The isotope with the larger binding energy contains one more neutron than the other isotope. Find the difference in atomic mass between the two isotopes.
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Isotopes have a same number of electrons and protons in all atoms. A . B . Isotopes : They are the atoms of a given element which have the same atomic number (Z) but different mass number (A) i.e. They have same Nuclear charge (Z) but different number of Neutrons (AZ).
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Isotopes are atoms that have the same numbers of protons but different numbers of neutrons. An ion is an atom that has gained or lost electrons, so it now has more or fewer electrons than it does protons. ... All atoms are isotopes and if an isotope gains or loses electrons it becomes an ion.
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Isotopes are atoms of the same element that contain an identical number of protons, but a different number of neutrons.
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Different isotopes of the same element have the same atomic number. They have the same number of protons. The atomic number is decided by the number of protons. Isotopes have different mass numbers, though, because they have different numbers of neutrons.
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Different isotopes of an element generally have the same physical and chemical properties because they have the same numbers of protons and electrons. ... For example, carbon with a mass number of 14 is called carbon-14. Atoms need a certain ratio of neutrons to protons to have a stable nucleus.
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Atoms of the same element that differ in their numbers of neutrons are called isotopes. Many isotopes occur naturally.
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The atomic number of an element is the number of protons in its nucleus. Neutrons are neutral particles having a mass slightly greater than that of the proton. Different isotopes of the same element contain the same number of protons but differing numbers of neutrons.
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Atoms of the same element can have different numbers of neutrons, however. Atoms of the same element (i.e., atoms with the same number of protons) with different numbers of neutrons are called isotopes. Most naturally occurring elements exist as isotopes.
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These different kinds of the same element are called isotopes. Isotopes are atoms that have the same atomic number (and are therefore of the same element) but different mass numbers. The composition of atoms of the naturally occurring isotopes of carbon are shown in Table 4.2.