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14 Cards in this Set
- Front
- Back
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mass is neither created nor destroyed during an ordinary chemical reaction or physical changes
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Law of conservation of mass
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a chemical compound contains the same elements in exactly the same proportions by mass regardless of the size of the elements or source
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Law of definite proportions
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If two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always a ratio of small whole numbers
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Law of multiple proportions
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the smallest particle of an element that remains the chemical properties of that element
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Atom
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the short-range proton-neutron, proton-proton, and neutron forces hold the nuclear particles together
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Nuclear forces
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the number of protons of each atom of that element
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Atomic number
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atoms of the same element that have different masses (i.e. different #of nuetrons)
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Isotope
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the total number of protons + nuetrons that make up the nucleus
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Mass number
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general term for a specific isotope of an element
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Nuclide
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exactly 1/12 of the mass of a carbon-12 atom
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Atomic mass unit (AMU)
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the weighted average of the atomic masses of the naturally occuring isotopes of an element
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Average atomic mass
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the amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon-12
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Mole (mol)
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6.022 X 10^23 - is the number of particles in exactly one mole of a pure substance
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Avogadro's number
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the mass of one mole of a pure substance. Written as g/mol.
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Molar mass
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