Ch 3 Notes/Definitions/Vocab Etc
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each of the black spaces below before clicking
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| Law of conservation of mass | mass is neither created not destroyed during ordinary chemical reactions or physical changes.
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| Law of definite proportions | the fact a chemical compound contains the same elements in exactly the same proportions by mass regardless of the size, sample, or source of the compound.
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| Law of multiple proportions | If 2 or more different compounds are composed of the same 2 elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always the ratio of small whole numbers.
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| Atom | smallest particle of an element that retains the chemical properties of that element
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| Nuclear forces | short-range proton-neutron, proton-proton, neutron-neutron, forces hold the nuclear particles together
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| Atomic Number | the # of protons of each atom of that element
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| Isotopes | atoms of the same element that have different masses
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| Mass number | total # of protons and neutrons that make up the nucleus of an isotope
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| Nuclide | general term for a specific isotope of an element
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| Atomic mass unit | 1amu is exactly 1/12 the mass of a carbon-12atom
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| Average atomic mass | the weighed average of the atomic masses of the naturally occurring isotopes of an element
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| Mole | amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon-12
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| Avagrado's Number | 6.022 x 10^23. The # of particles in exactly one mole of a pure substance
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| Molar Mass | mass of one mole of a pure substance
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