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| process that takes place naturally with no apparent stimulus |
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| Process that gives up energy as it takes place |
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| Process that gains or accepts energy as it takes place |
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| exothermic or endothermic |
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| If the energy changes in chemical processes involve heat they are referred to ___________ and ____________ |
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| Measurement or indication of disorder in the system. The more disorderly a system, the higher its entropy |
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| Substance that does not undergo spontaneous changes under the surrounding conditions |
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| Speed of a reaction. In experiments, you determine the change in concentration of a reactant or product and divide it by the time it takes for this change to occur |
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| Detailed explanation of how a reaction actually takes place |
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| Energy associated with vibrations within molecules. (Heat causes molecules to vibrate more vigorously) |
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| Energy needed to start some spontaneous processes. Once started, the processes continue without further stimulus or energy from an outside source. |
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Definition
| graphing of energy and reaction times |
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| Factors that Influence Reaction Rates |
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Definition
Nature of the reactants
Concentration of the reactants
Temperature of the reactants
Presence of catalysts |
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Definition
| Collision that causes a reaction to occur between the colliding molecules |
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| Substance that changes reaction rates without being used up in the reaction |
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| Substance that decreases reaction rates |
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| Catalytic substance that is distributed uniformly throughout the reaction mixture |
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| Hetergeneous or surface catalyst: |
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Definition
| Catalytic substance normally used in the form of a solid with a large surface area on which reactions take place |
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Definition
| Condition in a reaction system when the rates of the forward and reverse reactions are equal. |
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| Equilibrium concentrations |
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Definition
| Unchanging concentrations of reactants and products in a reaction system that is in a state of equilibrium. |
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| An indication of the relative amounts of reactants and products present at equilibrium |
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| Le Chatelier’s principle. |
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Definition
| Position of an equilibrium shifts in response to changes made in factors of equilibrium |
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Definition
| Any substance that provides H+ ions when dissolved in water. |
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| Any substance that provides OH- (hydroxide) ions when dissolved in water |
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| Any hydrogen-containing substance that is capable of donating a proton (H+) to another substance |
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| Any substance capable of accepting a proton from another substance |
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| Species (atoms, molecules, ions) remaining when a BrØnsted acid donates a proton |
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Definition
| A BrØnsted acid and its conjugate base |
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| Term used to describe any water solution in which the concentrations of H3O+ (hydronium ion) and OH- (hydroxide ion) are equal. Also, a water solution with a pH=7. |
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Definition
| Equilibrium constant for the dissociation of pure water into H3O+ and OH-. |
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Definition
| A solution in which the concentrations of H3O+ is greater than the concentration of OH-. Also, a solution in which pH is less than 7. |
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| Basic or alkaline solution |
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Definition
| A solution in which the concentrations of OH- is greater than the concentration of H3O+. Also, a solution in which pH is greater than 7. |
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Term
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Definition
| Negative logarithm of the molar concentration H+ (H3O+), or hydronium ion, in a solution |
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Term
| All acids have the following properties in common: |
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Definition
1.They taste sour
2.Produce H3O+ ions when dissolved in water
3.Undergo double-replacement reactions with solid oxides, hydroxides, carbonates, and bicarbonates
4.React with (and dissolve) certain metals to yield hydrogen gas |
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Definition
| Tabular representation of the tendencies of metals to react with H+ |
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Definition
| Reaction in which an acid and base react completely, leaving a solution that contains only a salt and water. |
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| Solid crystalline ionic compound at room temperature that contains the cation of a base and anion of an acid |
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| Salt that contains specific numbers of water molecules as part of the solid crystalline structure |
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Definition
| Water retained as part of the solid crystalline structure of some salts. |
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Term
| Strong acids and strong bases: |
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Definition
| Acids and bases that dissociate (ionize) essentially completely when dissolved to form a solution. |
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Term
| Weak (or moderately weak) acids and bases |
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Definition
| Acids and bases that dissociate (ionize) less than completely when dissolved to form a solution. |
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Term
| Acid dissociation constant |
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Definition
| Equilibrium constant for the dissociation of an acid |
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Definition
| Acid that gives up only one proton (H+) per molecule when dissolved. |
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Definition
| Acid that gives up two protons (H+) per molecule when dissolved. |
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Definition
| Acid that gives up three protons (H+) per molecule when dissolved. |
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Definition
| Analytical procedure in which one solution (often a base) of known concentration is slowly added to a measured volume of an undknown solution (often an acid). The volume of the added solution is measured with a buret. |
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Term
| Equivalence point of a titration |
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Definition
| Point at which the unknown solution has exactly reacted with the known solution. Neither is in excess. |
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Definition
| Point at which the titration is stopped on the basis of an indicator color change or pH meter reading. |
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Definition
| Any reaction with water. For salts it is a reaction of the acidic cation and/or basic anion of the salt with water. |
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Definition
| Solution with ability to resist changing pH when acids or bases are added. |
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