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| study of carbon compounds |
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| study of compounds that do not contain carbon |
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| mechanism, rate, and energy changes in matter |
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| states of matter (speed of molecules help determine) |
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| the same throughout a sample |
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| center placement of atom. determines what element an atom will be. +1 charge |
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| defines the element. number of protons in the element. |
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| also in the center. no charge, but hold the protons together in the nucleus. |
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| Smallest of three, always moving, -1 charge, moves from one atom to another or be shared between separate atoms. |
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| graphs of the phases of matter for a substance vs temperature and pressure |
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| time it takes for half of a radioisotope to decay |
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| splitting of a nucleus into smaller parts |
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| inspired by Dimitri Mendeleev, increasing atomic number arrangement. Rows are periods, groups are families |
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| soft, reactive, react with halogens |
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| some do not react, compounds are colorful |
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| most active non-metals, reacts with metals to form salts |
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| stable octet, non reactive |
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| half the distance between the nuclei of identical atoms that are bonded together |
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| energy required to remove one electron from a neutral atom |
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| measure of the ability of an atom to attract electrons closer to it |
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| positive ion. forms when an atom loses electrons |
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| negative ion. forms when an atom gains electrons |
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| form when electrons are transferred. metals and non metals |
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| visual representations of valence electrons |
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| show the kinds and numbers of atoms |
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| groups of covalently bonded atoms with an overall charge |
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| do not use criss cross method |
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| valence electron pairs repel each other |
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| assume the geometry that minimizes electrostatic repulsion |
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| have no partially charged regions, so the electrons are equally shared in bonds |
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| occur between molecules with permanent opposite charges |
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| strongest of intermolecular bonds |
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| weakest of intermolecular force |
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| moles to atoms, moles to moles, moles to mass, mass to moles, moles to volume |
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| empirical formula shows only lowest whole number ratio of elements |
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| molecular formulas are whole number multiples of empirical formula |
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| uses mole ratios from the balanced equation |
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| can be made out of any combination of coefficients and formulas |
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