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Chem unit 2 terms
| Question | Answer |
|---|---|
| limiting reactant | completely consumed in the reaction and limits the amount of product that can be made |
| excess reactant | reactant that is not completely consumed |
| Is the limiting reactant present in the fewest number of moles, or the least amount of mass? | moles |
| theoretical yield | amount of product that can be made from the limiting reactant |
| percent yield | the efficiency of a reaction |
| actual yield | the amount that is actually produced |
| percent yield equation | actual/theoretical x 100 |
| molecular formula | give the exact number of each type of element in a compound |
| empirical formula | give the simplest ratio of elements in a compound |
| percent composition of mass | list of the percent by mass of each element in a compound |
| limiting reactant | completely consumed in the reaction and limits the amount of product that can be made |
| excess reactant | reactant that is not completely consumed |
| Is the limiting reactant present in the fewest number of moles, or the least amount of mass? | moles |
| theoretical yield | amount of product that can be made from the limiting reactant |
| percent yield | the efficiency of a reaction |
| actual yield | the amount that is actually produced |
| percent yield equation | actual/theoretical x 100 |
| molecular formula | give the exact number of each type of element in a compound |
| empirical formula | give the simplest ratio of elements in a compound |
| percent composition of mass | list of the percent by mass of each element in a compound |
| What inherent relationships are contained in chemical formulas? | number of atoms and molecules and moles of atoms and molecules |
| What are the steps in determining the empirical formula from percent composition? | 1. assume 100 gram sample 2. convert grams to mole of each element 3. use # of moles as subscripts in empirical formula, dividing each subscript by the smallest subscript 4. convert any fractions to whole numbers |
| molar mass | the sum of the masses of all the atoms in the empirical formula |
| combustion analysis | a way to figure out what elements are in a substance by burning it and measuring what comes out |
| What type of solvent do polar molecules dissolve in? | polar solvents |
| hydration | polarity allowing water to attract ions and pull them from their crystal structure |
| dissociation | separating the ions from ionic compounds |
| What are chemical reactions that occur between substances dissolved in water? | aqueous solutions |
| solute | part of a solution that is being dissolved |
| solvent | part of a solution that dissolves the solute |
| When molecular compounds dissolve in water, what do they dissociate into? | individual compounds |
| When ionic compounds dissolve in water, what do they dissociate into? | ions |
| dilute solutions | amount of solute is small relative to the amount of solvent |
| concentrated solutions | large amount of solute relative to the amount of solvent |
| unsaturated solutions | contains less solute than the maximum amount that can dissolve at a given temperature |
| saturated solutions | contains the maximum amount of solute that can dissolve in a solvent at a given temperature |
| supersaturated solutions | solution that contains more dissolved solute than it should be able to hold at that temperature |
| precipitate | a solid that forms and separates out of a solution during a chemical reaction |
| solubility | maximum amount of a solute that can dissolve in a given amount of solvent at a specific temperature and pressure |
| dilution | reducing the concentration of a solute in a solution by adding more solvent |
| nonelectrolytes | substance that dissolves in water but does not form ions |
| electrolytes | substances that dissolve in water to produce ions, allowing the solution to conduct electricity |
| strong electrolytes | substance that completely dissolves into ions when dissolved in water |
| weak electrolytes | substance that dissolved in water but only partially ionizes |
| precipitation reaction | chemical reaction in which two aqueous ionic solutions are mixed and an insoluble solid forms |
| formula unit equation | standard balanced chemical equation written with complete, neutral chemical formulas |
| complete ionic equation | shows all strong electrolytes as the ions they form in a solution |
| net ionic equation | shows only the ions and molecules that actually participate in the chemical reaction |
| synthesis | type of chemical reaction in which two or more simple substances combine to form a single, more complex product |
| decomposition | chemical reaction in which one compound breaks down into two or more simpler substances |
| single replacement | reaction in which one element replaces another element in a compound |
| double replacement | reaction in which two ionic compounds in aqueous solution exchange ions, forming two new compounds |
| acids | substances increase the concentration of hydrogen ions (H⁺ or H₃O⁺) in aqueous solution |
| bases | substances that produce hydroxide ions (OH⁻) in water or accept protons (H⁺) |
| strong acids | HCL, HBr, Hl, HNO3, HClO3, HClO4, H2SO4 |
| strong bases | LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2 |
| acid anhydrides | non‑metal oxide that reacts with water to form an acid |
| basic anhydrides | metal oxide that reacts with water to form a base |
| neutralization reaction | acid–base reaction in which an acid donates H⁺ and a base donates OH⁻, and the two combine to form water |
| tritation | laboratory technique used to determine the concentration of an unknown solution by reacting it with a solution of known concentration |
| oxidation-reduction reactions | reactions in which electrons are transferred from one species to another |
| oxidation | loss of electrons by an atoms, ion, or molecule |
| reduction | gain of electrons by an atom, ion, or molecule |
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