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Chapters 6, 8, 9
Energy, Chemical Reactions, Acids and bases
| Question | Answer |
|---|---|
| Compressibility | A measure of the change in volume resulting from a pressure change. |
| Thermal Expansion | A measure of volume change resulting from a temperature change. |
| Kinetic Energy | Energy that matter possesses because of its motion. (Energy of Movement) |
| Potential Energy | Energy associated with forces of attraction between objects. (Energy of Position) |
| Electrostatic interactions | Attractions and repulsions that occur between charged particles. |
| Intermolecular Force | An attractive force that acts between a molecule and another molecule. How molecules are attracted to others when mixed. |
| Dipole-Dipole Interaction | An intermolecular force that occurs between polar molecules. (positive to negative)Relatively strong. |
| Hydrogen Bond | An extra strong dipole-dipole interaction between a hydrogen atom covalently bonded to a small, very electronegative atom (N,O,or F) and a lone pair of electrons to another small, very electronegative (N,O, or F). |
| Solid State | Physical state characterized by a dominance of potential energy over kinetic energy. |
| Liquid state | The physical state characterized by potential energy and kinetic energy of about the same magnitude. Randomly packed, but relatively close. |
| Gaseous State | The physical state characterized by a complete dominance of kinetic energy over potential energy. Move independently of one another. Fill their container. |
| Pressure | The force applied per unit area. The total force divided by the area of that surface. The particles banging into container. |
| Boyle's Law | Volume of a fixed amount of a gas in INVERSELY proportional to the pressure applied to the gas if the temperature is kept constant. P1 X V1 =P2 X V2 (Temp and Moles constant) |
| Charles's Law | Volume of a fixed amount of gas is DIRECTLY proportional to its Kelvin temp. if the pressure is kept constant. V1/T1=V2/T2 (pressure and moles constant) |
| Combined Gas Law | An expression obtained by combining Boyle's and Charles's laws. P1xV1/T1=P2xV2/T2(moles constant) |
| London Dispersion Force | A weak temporary intermolecular force that occurs between an atom or molecule (polar or nonpolar) and another atom or molecule (polar or nonpolar) Very Weak Bond. Temporary charge because constantly moving. |
| Ideal Gas Law | An equation that include the quantity of gas (moles) temp., pressure, and volume. PV=nRTR=0.0821 (contant) |
| Dalton's Law of Partial Pressures | Total pressure exerted by mixture of gases is the sum of the partial pressures of the individual gases. P(total)=P1+P2+P3.... |
| Partial pressure | Pressure that a gas would exert if it were present alone under the smae conditions. |
| Change of state | Process in which a subtance is transformed from one physical state to another. (6 Possible changes) |
| Sublimation | Direct change from the solid to Gaseous State. |
| Deposition | Direct change from the gaseous to the solid state. |
| Endothermic changes | Require input (absorption) of heat; Melting, evaporation, sublimation. |
| Exothermic changes | Release heat (heat given up); Freezing, condensation, deposition. |
| Evaporation | The process of molecules escaping from the liquid phase to the gas phase. |
| Thermodynamics | The amount of heat released or absorbed in a chemical reaction. |
| Equilibrium Rate | Two opposite processes that take place at equal rates. (Evaporation and Condensation) |
| Vapor | Gaseous molecules of a subtance at a temperature and pressure when normally thought of as liquid or solid, room temp. and atm. (molecules that escape water=water vapor) |
| Vapor Pressure | Pressure exerted by a vapor above a liquid when the liquid and vapor are in equilibrium. |
| Volatile substance | Substance that readily evaporates at room temperature because of a high vapor pressure. |
| Boiling | Form of evaporation where conversion from the liquid state to vapor state occurs and produces bubble formation. |
| Boiling point | Is the temperature at which the vapor pressure of a liquid becomes equal to the external (atmospheric) pressure exerted on the liquid. Fluctuates with atm. |
| Normal boiling point | The temperature at which a liquid boils under a pressure of 760 mm Hg. |
| Conditions that affect boiling point | atm, elevation, external pressure affect what? |
| Chemical Reaction | Process where at least one new product is produced as a result of chemical change |
| Combination/Synthesis Reaction | Single product produced from 2 (or more) reactants. X + Y = XY |
| Decompositon Reaction | Single reaction converted into two (or more)simpler substances (elements or compounds) XY = X + Y |
| Single Replacement Reaction | X + YZ = Y + XZ |
| Double Replacement Reaction | Two reactants exchange parts.XA + YB = XB + YA |
| Combustion Reaction | A reaction of a substance with oxygen (usually air) that proceeds with heat and usually flame. Combination reaction. Exothermic. Needs oxygen, creates H2O, and CO2. C3H2 +5O2 = 4CO2 + 2H2O |
| Redox Reactions | Oxidation-Reduction Reactions |
| Oxidation-Oxygen based Redox | Process whereby a reactant in a chemical reaction gains one or more oxygen atoms. |
| Reduction-Oxygen based Redox | Process whereby a reactant in a chemical reaction loses one or more oxygen atoms |
| LEO goes GER (Electron Redox) | Lose electrons oxidation; Gain electrons Reduction |
| oxidation-reduction reaction | A chemical reaction in which there is a transfer of electrons between reactants |
| Non-oxidation-reduction reaction | A chemical reaction in which there is NO transfer of electrons between reactants |
| Oxidizing agent | Causes oxidation by accepting electron from other reactant. (GER, or reduced substance) |
| Reducing agent | Causes reduction by providing electrons for the other reactant to accept. (LEO, Oxidized subsantance) |
| Collision Theory- | Conditions must be met before a chmical reaction will take place (3)1. Where two things must slam together for a reaction to occur.2. Activation energy-needed for reaction (heat)3. Orientation-particles must line up for collision to occur |
| Activation Energy | Minimum combined kinetic energy that reactant particles must possess in order for collision to result in a reaction |
| Molecular collisions | Reactant particles must collide for reaction to occur. |
| Collision orientation | Molecules must line up right to collide. |
| Exothermic Reaction | Releases heat (kinetic energy) into the surroundings. Energy is released as reaction occurs. |
| Endothermic Reaction | Reaction that absorbs energy from the surroundings. Requires input of energy. |
| Heat | Actual kinetic energy. |
| Rate of chemical reaction | Rate reactants are consumed or products are produced. 1. nature of reactants (state, and size) 2. Concentration (increase concentration, increases rate of reaction.) 3. Temperature (heat) 4. Catalyst |
| Temperature | A measure of the average kinetic energy of all the particles. |
| Catalyst | Substance that increases the reaction rate without being consumed in the reaction. Alternate route need lower activation energy. Enzymes are catalysts |
| Chemical equilirium | Two opposing chemical reactions occur simultaneously. Doesn't have to be 50/50 mix. |
| Reversible reaction | Used to discuss chemical equilibrium. Rate of forward reaction is equal to the rate of the reverse reaction- |
| Le Chatelier's principle | If a stress is applied to a system at equlibrium, the system will work to counteract that change and reestablish equilibrium. |
| Arrhenius Theory | Theory that:Acids donate [H+] protons and Bases donate [OH-] hydroxide |
| Bronsted & Lowry Theory | Acid: Donate [H+]=Proton DonorBase: Accept [H+]=Proton Acceptor |
| Ionization | Individual positive and negative ions are PRODUCED from a compund dissolved in solution. |
| Dissociation | Individual positive and negative ions are RELEASED from a compund dissolved in solution. |
| Arrhenius Acid | sour taste, blue paper red |
| Arrhenius Base | Bitter taste, Red paper turns blue |
| Conjugate Acid-base pair | Species that differ by one proton |
| Conjugate base | Species that remains when an acid loses a proton. |
| Conjugate Acid | Species formed when a base accepts a proton. |
| monoprotic acid | An acid that transfers one [H+] ion per molecule during an acid-base reaction |
| diprotic acid | an acid that transfers 2 [H+]ions per molecule during an acid-base reaction |
| triprotic acid | an acid that transfers 3 [H+]ions per molecule during an acid-base reaction |
| polyprotic acid | an acid that can transfer two or more [H+]ions per molecule during an acid-base reaction |
| Strong Acid | A substance that transfers 100% or very nearly 100% of its protons to water. |
| Weak Acid | A substance that transfers only a small % of its protons to water. |
| Salt | An ionic compound containing a metal or polyatomic ion as the positive ion and a non-metal or polyatomic ion (except OH-) as the negative |
| Neutralization | the reaction between an acid and a hydroxide base to form a salt and water. (Either a double replacement or proton transfer reaction) |
| Acidic solution | solution where the concentration of H3O+ ions is higher than OH- ions. |
| Basic Solution | solution where the concentration of OH- ions is higher than H3O+ ions. |
| Neutral Solution | Equal concentrations of H30+ and OH- ions in a solution |
| pH | -log[H3O+] ;negative logarithum of solutions molar hydronium ion concentration. |
| Buffer | A solution that resist major changes in pH when small amounts of acid or base are added to it. Will resist pH change until you overcome it. |
| acid-base titration | A measured volume of an acid or a base of known concentration is exactly reacted with a measured volume of a base or an acid of unknown concentration |
| Indicator | A compound that exhibits different colors depending on the pH of its surroundings. |
Created by:
janybee
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