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LCCC Chem 2 Final
LCCC Mr. Hiner's Chem 2 Final
| Term | Definition |
|---|---|
| Intermolecular Forces | Fixed- keeps shape when placed in a container, Indefinite- takes the shape of the container |
| Solid Intermolecular Forces | very strong forces, particles are packed close together and can only vibrate and are incompressible |
| Liquid Intermolecular Forces | particles are packed close together but have the ability to move from place to place, and are incompressible |
| Gas Intermolecular Forces | cohesive, complete freedom of motion and aren't held together, but flow and no shape and can't be compressed |
| State of Matter | Depends on: The amount of kinetic energy the particles possess, the strength of attraction between molecules |
| Gas Kinetic Energy | their kinetic energy overcomes the attractive forces between molecules |
| Forces of Attraction | the particles are attracted to each other by electrostatic forces (strength varies, depends on kinds of particles) |
| Specific Heat (c) | amount of energy needed to raise 1 gram of water 1 degree Celcius |
| Q=mc(delta T) | heating of a substance |
| Q=mQf Heat of fusion(Qf) | Heat of fusion= 79.7cal/gm or 334kJ/kg |
| Q=mQvap Heat of Vaporization(Qvap) | Heat of Vaporization=539 cal/gm or 2260kJ/kg |
| Heating Water | 100 cal/gm or 418.6 kJ/kg to heat water 0 degrees --> 100 degrees |
| Intermolecular Attractions | attractive forces between opposite charges, H bonding especially strong |
| London Dispersion Forces | nonpolar molecules-very weak |
| Dipole-Dipole | polar molecules, strong alignment |
| H-bonding | O-H, N-H, F-H |
| Ion-Dipole Forces | In a mixture, ions from an ionic compound are attracted to the dipole in polar molecules. |
| Viscosity | resistance of a liquid to flow, raising temperature reduces viscosity |
| Capillary Action | is the ability of a liquid to flow up a thin tube |
| Super Critical Fluid | A point at which you get one state (liquid and gas blur) |
| Boiling Point | the temperature at which the vapor pressure equals external atmosphere pressure |
| Dynamic Equilibrium | rate of evaporation=rate of condensation |
| Heat of Vaporization | the amount of heat energy required to vaporize one mole of the liquid |
| Vapor Pressure and Temperature | as the temperature increases, the vapor pressure increases, increasing the temperature increases number of molecules escaping a liquid |
| Clausis-Clapeyron Equation | ln(P2/P1)=(Hvap/R)((1/T1)-(1/T2)) |
| Crystalline Solids | particles are in highly ordered arrangements |
| Amorphous Solids | no particular order in the arrangement of particles |
| Ionic Crystals | ions pack themselves so as to maximize the attractions and minimize repulsions |
| Homogeneous Solutions | A mixture of two or more substances |
| Solvent | majority component of a solution |
| Solute | minority component of a solution |
| Soluble | when a solute dissolves in a solvent |
| Entropy | measure of randomness |
| Solubility | the maximum amount of solute that can be dissolved in a given amount of solvent (temperature dependent) |
| Lattice Energy | attractive forces between ions |
| Saturated Solutions | the solvent holds as much solute as is possible at that temperature |
| Unsaturated Solutions | less solute than can dissolve in the solvent at that temperature is dissolved in the solvent |
| Henry's Law | Sg=kPg, Sg=solubility of gas, k=Henry's Law Constant, Pg=partial pressure of gas above liquid, (S1/P1)=(S2/P2) |
| Concentration | amount of solute in a given amount of solution |
| Part of a whole | amount of solute in a given amount of solution %=(amount of solute/ amount of solution) x 100 |
| Molarity | M=(mass of solute)/((Molar Mass)(V of solution in liters)) |
| Molality | m=(moles of solute)/(mass of solvent in kilograms) |
| Mole Fraction | Xa=moles of solute/total number of moles |
| Density | D=M/V |
| Colligative Properties | vapor pressure of a solvent above a solution is lower than the vapor pressure of the pure solvent |
| Raoult's Law | P solvent in solution= X solvent (pressure of gas at standard conditions) |
| Boiling Point Elevation | Delta Tb=Kb(m) Kb=molal boiling point Delta Tb=added to the normal boiling point |
| Freezing Point Elevation | Delta Tf=Kf(m) |
| Van't Hoff Effect | Delta Tf=Kf(mi) mi=number of particles in an electrolyte |
| Osmosis | is the flow of solvent from a solution of low concentration into a solution of high concentration |
| Semipermeable Membrane | allows solvent to flow through it, but not solute |
| Osmotic Pressure | amount of pressure needed to keep osmotic flow from taking place, II=MRT |
| Isotonic | exerts the same osmotic pressure as body fluids such as red blood cells (RBCs) |
| Hypertonic | has a lower solute concentration than RBCs, water goes out of cells by osmosis |
| Hypotonic | has higher solute concentration than RBCs, water goes out of cells by osmosis |
| Colloids | have medium-size particles, cannot be filtered, can be seperated by semipermeable membrane |
| Suspensions | very large particles, settle out, can be filtered, must be stirred to stay suspended |
| Soaps | Ionic heads (hydrophilic), nonpolar tails (hydrophobic) |
| Reaction Rate | the speed of a chemical reaction |
| Rate | how much a quantity changes in a given period of time Rate=change of something/delta t |
| Rate Equation | Rate=-1/a delta A/delta t=etc. |
| Polarimetry | measures the change in the degree of rotation of plane polarized light caused by one of the components over time |
| Spectrophotometry | this measures the amount of light of a particular wavelength absorbed by one component over time |
| Catalyst | affect speed of reaction without being consumed |
| The Rate Law | Rate=k[A]^n |
| Zero Order | rate is always the same/don't change rate |
| First Order | rate is directly proportional to reactant concentration |
| Second Order | rate is directly proportional to the square of the reactant concentrations/ double concentration=quadruple the rate |
| Integrated Rate Laws | zero=line, drop down, first=straight sloped line, slight bow, Second=bent line, big bow |
| Zeroth Order | [A]=-kt+[A]initial |
| First Order Half Life | 0.693/rate |
| First Order | ln([At]/[Ao])=-kt |
| Second Order | 1/[A]=kt+(1/[A]initial) |
| Second Order Half Life | 1/k[Ao] |
| Activation Energy (Ea) | minimum amount of energy required for reaction |
| Activation Energy Equation | ln(k2/k1)=(Ea/R)((1/T1)-(1/T2)) |
| Mechanism | sequence of events that are a road map of bond breaking and making |
| Le Chatelier's Principle | If a system at equilibrium is disturbed by a change in temperature, pressure, or the concentration of one of the components it will shift its equilibrium to counteract the effect of disturbance |
| Arrhenius Acid | a substance that when dissolved in water, increases the concentration of hydrogen ions |
| Arrhenius Base | a substance that when dissolved in water, increasing the concentration of hydroxide ions |
| Bronsted-Lowry | acid=proton donor/must have a removable protein, base=proton acceptor/must have pair of nonbonding electrons |
| Lewis Acid | species that can form a covalent bond by accepting an electron pair |
| Lewis Base | an electron pair donator |
| Acids | strong acids completely dissociate, weak acids don't |
| Kw | Kw=Ka x Kb, Kw=1.0x10^-14 |
| Equilibrium Expression | Kc=[H3O+][OH-] |
| pH | pH=-log[H3O+] pH=pKa+log([base]/[acid]) |
| pOH | pOH=-log[OH-] |
| pKa | pKa=-log[Ka] |
| Salt Anions | bases that can react with water in a hydrolysis reaction to form OH- and the conjugate acid |
| Salt Cations | with acidic protons will lower the pH of a solution, most metal cations when hydrated in solution also lower the pH |
| Buffers | resist changes in pH when an acid or base is added |
| Equivalence Point | where stiochiometric equality |
| End Point | where indicator changes color and allows you to end titration |
| Common-Ion Effect | If one of the ions in a solution equilibrium is already dissolved in the solution, the equilibrium will shift to the left and the solubility of the salt will decrease |
| First Law of Thermodynamics | Energy cannot be created nor destroyed. Therefore total energy of the universe is a constant. |
| Spontaneous Processes | are those that can proceed without any outside intervention, processes spontaneous forward are not reverse |
| Irreversible Processes | cannot be undone by exactly reversing the change to the system |
| Entropy Equation | S=entropy Delta S=Sfinal-Sinitial S-klogW Delta S= Delta Hvap/T |
| Second Law of Thermodynamics | Entropy of universe increases for spontaneous processes, but doesn't change for reversible processes |
| Third Law of Thermodynamics | The entropy of a pure crystalline substance at absolute zero is 0 |
| Gibb's Free Energy | Delta G= Delta H- T Delta S |
| Voltaic Cells | In spontaneous oxidation-reduction (redox) reactions, electrons are transferred and energy is released |
| Electromotive Force (emf) | the potential difference between the anode and cathode in a cell Wmax=-nFEcell |
| Oxidizing and Reducing Agents | The strongest oxidizers have the most positive reduction potentials and vice versa |
| Free Energy | Delta G=-nFE Ecell=(0.592)logK/n E=E(circle)-(0.0592/n)logQ |
| Radioactive Decays | Alpha, Beta, Gamma,Electron Capture (K-capture), Positron Emmission |
| Alpha Decay | mass number decrease by 4, atomic number decrease by 2 |
| Beta Decay | mass number stays the same, atomic number increase by 1 |
| Positron Emmission | mass number stays the same, atomic number decrease by 1 |
| Gamma Decay | gives off m (meta) in decay |
| Electron Capture (K-Capture) | proton meets electron to make neutron |
| Nuclear Kinetics | Nuclear transmutation is a first order process |
| Nuclear Rate | Rate=kNt Nt=number of radionuclei at any time |
| Curie | 1 Curie=3.7x10^10 nuclei/s |
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