Chapter 3 – Chemistry Answers – Flashcards
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| Chemical Equilibrium |
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| the rate of forward reaction is equal to the rate of the reverse reaction |
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| Dynamic Equillibrium |
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| both the forward and reverse proccess are still occuring but at equal rates |
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| product-favored reactions |
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| reactions in which reactants are completely or largely converted to products when equlibrium is reached |
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| reactant favoured |
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| the opposite of product-favored reactions the reactions lead to the conversion of only a small amount of the reactants to products |
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| solution |
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| homogenous mixture of two or more substances |
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| Solvent |
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| the median in wich the solute is dissolved |
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| solute |
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| the dissolved sobstance |
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| aqueos solutions |
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| solutions in which water is the solvent |
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| electrodes |
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| conductor of electricity |
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| strong electrolyte |
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| substances whose solutions are good electrical conductors owing to the presence of ions |
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| non electrolytes |
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| compunds who aqeous solutions do not conduct electricity |
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| weak electrylites |
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| when the compund is disolved in water only a small fraction of the kolecules forms ions. |
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| exchange reactions |
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| the ions of the reactants exchange partners |
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| precipation reaction |
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| produces a water insoluble solid product called a precipate |
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| precipate |
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| a water insoluble solid product |
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| spectator ions |
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| ions that appear on both sides of the equation that do not participate in the net reaction |
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| net ionic equation |
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| the balanced equation that results after leaving out the spectator ions |
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| HCl |
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Hydrochlric acid Strong acid |
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| HBr |
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Hydrobromic acid strong acid |
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| HI |
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Hydroiodic acid Storng acid |
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| HNO3 |
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Nitric Acid storng acid |
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| HClO4 |
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Perchlric acid Strong |
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| H2SO4 |
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Sulfuric acid strong |
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| HF |
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hydroflouric acid weak |
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| H3PO4 |
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Phosphoric acid weak |
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| H2CO3 |
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Carbonic acid weak |
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| CH3CO2H |
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Acetic Acid Weak |
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| H2C2O4 |
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Oxalic Acid weak |
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| H2C4H4O6 |
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Tartaric Acid weak |
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| H3C6H5O7 |
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Citric Acid Weak acid |
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| HC9H7O4 |
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Aspirin Weak acid |
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| LiOH |
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lithium hydroxide strong base |
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NaOH
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Sodium hydroxide strong base |
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| KOH |
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potassium hydroxide strong base |
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| Ba(OH)2 |
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Barium hydroxide strong base |
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Sr(OH)2
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strontium hydroxide strong base |
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| NH3 |
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Ammonia weak base |
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| strong acid |
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| acids that ionize completely in water |
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| weak acids |
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| acids that incompletely ionize in water |
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| strong bases |
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| bases that ionize completely in water |
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| neutralization reaction |
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| reactions between strong acids and bases |
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| acidic oxide |
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| oxides that can react with water to produce H3O+ |
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| basic oxides |
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| oxides of metal that give basic solutions when dissolved in water |
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| reducing agent |
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| the agent that brings about the reduction |
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| oxidizing agent |
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| the agent responsible for oxidation |
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| oxidized |
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| when a substance loses electrons |
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| oxidation number |
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| the charge an atom has or appears to have |
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| Each atom in a pure elemnt has an oxidation number of zero |
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| For monatomic ions, the oxidation number is equal to the charge on the ion |
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| When combined with another element, flourine always has an oxidation number of -1 |
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| The oxidation number of O is -2 in most compounds |
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| Cl, Br, and I have oxidation numbers of -1 in compounds, except when combined with oxygen and flourine |
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| The oxidation number of H is +1 in most compunds |
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| The algebraic sum of oxidation numbers for the atoms in a neutral cmpound must be zero; in a polyatomic ion, the sum must be equal to the ion charge. |
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| precipitation reactions |
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| ions combine in solution to form an insoluble reaction product |
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| acid-base reactions |
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| water is a product og many acid-bae reactions, and the cation of the base and the anion of the acid form a salt |
