Energy, Chemical Reactions, Acids and bases
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| Compressibility | A measure of the change in volume resulting from a pressure change.
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| Thermal Expansion | A measure of volume change resulting from a temperature change.
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| Kinetic Energy | Energy that matter possesses because of its motion. (Energy of Movement)
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| Potential Energy | Energy associated with forces of attraction between objects. (Energy of Position)
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| Electrostatic interactions | Attractions and repulsions that occur between charged particles.
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| Intermolecular Force | An attractive force that acts between a molecule and another molecule. How molecules are attracted to others when mixed.
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| Dipole-Dipole Interaction | An intermolecular force that occurs between polar molecules. (positive to negative)Relatively strong.
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| 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).
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| Solid State | Physical state characterized by a dominance of potential energy over kinetic energy.
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| Liquid state | The physical state characterized by potential energy and kinetic energy of about the same magnitude. Randomly packed, but relatively close.
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| Gaseous State | The physical state characterized by a complete dominance of kinetic energy over potential energy. Move independently of one another. Fill their container.
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| Pressure | The force applied per unit area. The total force divided by the area of that surface. The particles banging into container.
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| 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)
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| 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)
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| Combined Gas Law | An expression obtained by combining Boyle's and Charles's laws. P1xV1/T1=P2xV2/T2(moles constant)
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| 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.
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| Ideal Gas Law | An equation that include the quantity of gas (moles) temp., pressure, and volume. PV=nRTR=0.0821 (contant)
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| 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....
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| Partial pressure | Pressure that a gas would exert if it were present alone under the smae conditions.
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| Change of state | Process in which a subtance is transformed from one physical state to another. (6 Possible changes)
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| Sublimation | Direct change from the solid to Gaseous State.
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| Deposition | Direct change from the gaseous to the solid state.
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| Endothermic changes | Require input (absorption) of heat; Melting, evaporation, sublimation.
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| Exothermic changes | Release heat (heat given up); Freezing, condensation, deposition.
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| Evaporation | The process of molecules escaping from the liquid phase to the gas phase.
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| Thermodynamics | The amount of heat released or absorbed in a chemical reaction.
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| Equilibrium Rate | Two opposite processes that take place at equal rates. (Evaporation and Condensation)
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| 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)
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| Vapor Pressure | Pressure exerted by a vapor above a liquid when the liquid and vapor are in equilibrium.
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| Volatile substance | Substance that readily evaporates at room temperature because of a high vapor pressure.
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| Boiling | Form of evaporation where conversion from the liquid state to vapor state occurs and produces bubble formation.
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| 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.
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| Normal boiling point | The temperature at which a liquid boils under a pressure of 760 mm Hg.
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| Conditions that affect boiling point | atm, elevation, external pressure affect what?
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| Chemical Reaction | Process where at least one new product is produced as a result of chemical change
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| Combination/Synthesis Reaction | Single product produced from 2 (or more) reactants. X + Y = XY
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| Decompositon Reaction | Single reaction converted into two (or more)simpler substances (elements or compounds) XY = X + Y
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| Single Replacement Reaction | X + YZ = Y + XZ
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| Double Replacement Reaction | Two reactants exchange parts.XA + YB = XB + YA
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| 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
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| Redox Reactions | Oxidation-Reduction Reactions
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| Oxidation-Oxygen based Redox | Process whereby a reactant in a chemical reaction gains one or more oxygen atoms.
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| Reduction-Oxygen based Redox | Process whereby a reactant in a chemical reaction loses one or more oxygen atoms
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| LEO goes GER (Electron Redox) | Lose electrons oxidation; Gain electrons Reduction
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| oxidation-reduction reaction | A chemical reaction in which there is a transfer of electrons between reactants
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| Non-oxidation-reduction reaction | A chemical reaction in which there is NO transfer of electrons between reactants
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| Oxidizing agent | Causes oxidation by accepting electron from other reactant. (GER, or reduced substance)
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| Reducing agent | Causes reduction by providing electrons for the other reactant to accept. (LEO, Oxidized subsantance)
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| 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
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| Activation Energy | Minimum combined kinetic energy that reactant particles must possess in order for collision to result in a reaction
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| Molecular collisions | Reactant particles must collide for reaction to occur.
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| Collision orientation | Molecules must line up right to collide.
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| Exothermic Reaction | Releases heat (kinetic energy) into the surroundings. Energy is released as reaction occurs.
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| Endothermic Reaction | Reaction that absorbs energy from the surroundings. Requires input of energy.
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| Heat | Actual kinetic energy.
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| 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
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| Temperature | A measure of the average kinetic energy of all the particles.
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| Catalyst | Substance that increases the reaction rate without being consumed in the reaction. Alternate route need lower activation energy. Enzymes are catalysts
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| Chemical equilirium | Two opposing chemical reactions occur simultaneously. Doesn't have to be 50/50 mix.
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| Reversible reaction | Used to discuss chemical equilibrium. Rate of forward reaction is equal to the rate of the reverse reaction-
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| 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.
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| Arrhenius Theory | Theory that:Acids donate [H+] protons and Bases donate [OH-] hydroxide
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| Bronsted & Lowry Theory | Acid: Donate [H+]=Proton DonorBase: Accept [H+]=Proton Acceptor
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| Ionization | Individual positive and negative ions are PRODUCED from a compund dissolved in solution.
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| Dissociation | Individual positive and negative ions are RELEASED from a compund dissolved in solution.
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| Arrhenius Acid | sour taste, blue paper red
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| Arrhenius Base | Bitter taste, Red paper turns blue
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| Conjugate Acid-base pair | Species that differ by one proton
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| Conjugate base | Species that remains when an acid loses a proton.
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| Conjugate Acid | Species formed when a base accepts a proton.
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| monoprotic acid | An acid that transfers one [H+] ion per molecule during an acid-base reaction
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| diprotic acid | an acid that transfers 2 [H+]ions per molecule during an acid-base reaction
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| triprotic acid | an acid that transfers 3 [H+]ions per molecule during an acid-base reaction
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| polyprotic acid | an acid that can transfer two or more [H+]ions per molecule during an acid-base reaction
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| Strong Acid | A substance that transfers 100% or very nearly 100% of its protons to water.
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| Weak Acid | A substance that transfers only a small % of its protons to water.
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| 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
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| Neutralization | the reaction between an acid and a hydroxide base to form a salt and water. (Either a double replacement or proton transfer reaction)
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| Acidic solution | solution where the concentration of H3O+ ions is higher than OH- ions.
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| Basic Solution | solution where the concentration of OH- ions is higher than H3O+ ions.
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| Neutral Solution | Equal concentrations of H30+ and OH- ions in a solution
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| pH | -log[H3O+] ;negative logarithum of solutions molar hydronium ion concentration.
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| 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.
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| 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
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| Indicator | A compound that exhibits different colors depending on the pH of its surroundings.
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