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| the study of the properties and the composition of matter |
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| a pure substance that cannot be broken into simpler substances by chemical means |
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| a pure substance that can be broken down by chemical means to produce two or more pure substances |
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| when elements are arranged in order of increasing atomic number, their properties show a periodic recurrence and gradual change |
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| atoms of the same element that have the same number of protons but different number of neutrons |
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| isotopes that are unstable giving off radiation |
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| the distance from the center of the nucleus to the valence electron |
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| the amount of energy required to remove the most weakly held electron from a neutral atom |
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| the amount of energy given off when an electron is accepted by an atom in the gaseous state |
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| a number that describes the relative ability of an atom to attract electrons when bonding |
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| the force of attraction holding atoms or ions together |
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| the attraction between oppositely charged ions in a compound |
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| the attractive force between two atoms that result when electrons are shared |
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| illustrations of molecules formed from covalent bonding and using Lewis symbols |
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| a covalent bond with unequal sharing of electron in the bond |
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| attractive forces between atoms and ions within a compound (these are bonds) |
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| attractive forces between molecules |
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| International Union of Pure and Applied Chemistry |
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| a covalently bonded group of atoms, possessing a net charge |
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| polyatomic ions that contain oxygen and have a negative charge |
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| law of conservation of mass |
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Definition
| during a chemical reaction, the total mass of the reactants is always equal to the total mass of the products |
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| the law of definite proportions |
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| a specific compound always contains the same elements in definite proportions by mass |
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| the amount of substance containing 6.02 x 1023 entities |
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| the mass, in grams, of one mole of a substance |
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| shows the simplest whole number ratio of atoms or ions in a compound |
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| gravimetric stoichiometry |
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| the procedure for calculating the masses of reactants or products in a chemical reaction |
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| the reactant that is completely consumed in a chemical reaction |
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| the reactant that is present in more than the required amount for complete reaction |
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| the amount of product that is actually obtained experimentally |
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| the amount of product that we predict will be obtained, calculated using stoichiometry |
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| a homogeneous mixture of substances composed of at least one solute and one solvent |
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| a uniform mixture of only one phase (visible part) |
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| a non-uniform mixture of two or more phases |
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| a substance that is dissolved in a solvent |
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| the medium in which a solute is dissolved |
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| the quantity of a given solute in a given amount of solution |
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| having a relatively small concentration |
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| a solution for which the precise concentration is known |
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| a solution containing less than the maximum quantity of a solute at specific temperature and pressure conditions |
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| a solution containing the maximum quantity of a solute at specific temperature and pressure conditions |
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| the state of a solution when the solution contains more than the maximum quantity of a solute at specific temperature and pressure conditions |
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| the amount of solute that can dissolve in a certain amount of solvent at a specific temperature and pressure |
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| the insoluble solid formed in a chemical reaction involving two solutions |
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| when two liquids do not form a homogeneous mixture when added together (do not form a solution when mixed) |
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| when two liquids form a homogeneous mixture when added together (forms a solutions when mixed in any proportion) |
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| any substance that produces hydrogen ions in water |
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| any substance that produces hydroxide ions in water |
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| the production of ions from a neutral molecule |
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| mainly vibrational motion so particles stay relatively close together |
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| have some of each type of motion |
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| have all types of motion but translation motion is predominate |
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| particles can have three main types of motion: translational (straight line), rotational (spinning), and vibrational (back and forth motion of atoms within the molecule) |
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| At a constant temperature, the volume of a fixed mass of gas in inversely proportional to its pressure |
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| At a constant pressure, the volume of a fixed mass of gas is directly proportional to its Kelvin temperature. |
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| At a constant volume, the pressure of a fixed mass of gas is directly proportional to its Kelvin temperature. |
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| the volume occupied by one mole of a substance |
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| equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. |
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| compounds that contain carbon, except CO, CO2, and ionic compounds with carbon |
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| organic compounds containing only one carbon and hydrogen atoms |
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| a compound with the same molecular formula as another compound, but a different structural formula |
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