Term
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Definition
| the rate of forward reaction is equal to the rate of the reverse reaction |
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Term
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Definition
| both the forward and reverse proccess are still occuring but at equal rates |
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Term
| product-favored reactions |
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Definition
| reactions in which reactants are completely or largely converted to products when equlibrium is reached |
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Term
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Definition
| 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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Term
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Definition
| homogenous mixture of two or more substances |
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Term
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Definition
| the median in wich the solute is dissolved |
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Term
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Definition
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Term
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Definition
| solutions in which water is the solvent |
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Definition
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Term
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Definition
| substances whose solutions are good electrical conductors owing to the presence of ions |
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Term
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Definition
| compunds who aqeous solutions do not conduct electricity |
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Term
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Definition
| when the compund is disolved in water only a small fraction of the kolecules forms ions. |
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Term
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Definition
| the ions of the reactants exchange partners |
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Term
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Definition
| produces a water insoluble solid product called a precipate |
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Term
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Definition
| a water insoluble solid product |
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Term
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Definition
| ions that appear on both sides of the equation that do not participate in the net reaction |
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Term
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Definition
| the balanced equation that results after leaving out the spectator ions |
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Term
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Definition
Hydrochlric acid
Strong acid |
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Term
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Definition
Hydrobromic acid
strong acid |
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Term
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Definition
Hydroiodic acid
Storng acid |
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Definition
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Definition
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Definition
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Term
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Definition
lithium hydroxide
strong base |
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Term
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Definition
Sodium hydroxide
strong base |
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Term
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Definition
potassium hydroxide
strong base |
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Term
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Definition
Barium hydroxide
strong base |
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Term
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Definition
strontium hydroxide
strong base |
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Term
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Definition
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Term
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Definition
| acids that ionize completely in water |
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Term
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Definition
| acids that incompletely ionize in water |
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Term
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Definition
| bases that ionize completely in water |
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Term
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Definition
| reactions between strong acids and bases |
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Term
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Definition
| oxides that can react with water to produce H3O+ |
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Term
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Definition
| oxides of metal that give basic solutions when dissolved in water |
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Term
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Definition
| the agent that brings about the reduction |
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Term
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Definition
| the agent responsible for oxidation |
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Term
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Definition
| when a substance loses electrons |
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Term
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Definition
| the charge an atom has or appears to have |
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Term
| Each atom in a pure elemnt has an oxidation number of zero |
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Definition
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Term
| For monatomic ions, the oxidation number is equal to the charge on the ion |
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Definition
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Term
| When combined with another element, flourine always has an oxidation number of -1 |
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Definition
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Term
| The oxidation number of O is -2 in most compounds |
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Definition
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Term
| Cl, Br, and I have oxidation numbers of -1 in compounds, except when combined with oxygen and flourine |
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Definition
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Term
| The oxidation number of H is +1 in most compunds |
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Definition
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Term
| 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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Definition
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Term
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Definition
| ions combine in solution to form an insoluble reaction product |
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Term
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Definition
| water is a product og many acid-bae reactions, and the cation of the base and the anion of the acid form a salt |
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