CHEM 480 1nd Edition Lecture 2 Outline of Last Lecture I. BondingII. Structure of Biological MoleculesIII. UnitsIV. EquilibriumV. Extensive vs. Intensive PropertiesVI. Equations of State VII. Standards Outline of Current Lecture I. EnergyII. States of MatterIII. Kinetic Molecular TheoryIV. Thermal EnergyV. Boltzmann DistributionCurrent LectureI. Energya. Capacity to do workb. F = mac. W = F*dd. Kinetic (KE) = ½ mv2 i. Energy of motione. Potential (PE) = mgh = Q+ Q- / 4πε0d where ε0 = 8.854 x 10-12 C2/J*mi. Energy of positionf. Conservation of energy: PE + KE = total energyII. States of mattera. Gas – liquid – solid b. Liquid and solid = condensed phasesc. Primary difference between states = Freedom of particles to move past one another ==> Average distance between particlesIII. Kinetic Molecular Theory (what happens to gas particles as environmental conditionschange)a. Gases consist of large numbers of molecules that are in continuous, random motionThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.b. The combined volume of all the molecules of the gas is negligible relative to the total volume in which the gas is containedi. Vmatter << Vgasc. Attractive and repulsive forces between gas molecules are negligibled. Energy can be transferred between molecules during collisions, but the average kinetic energy of the molecules does not change with time, as long as the temperature of the gas remains constante. The average kinetic energy of the molecules is proportional to the absolute temperatureIV. Thermal energya. Temperature is a measure of the average kinetic energy of a collection of particlesb. For a single particle, thermal energy = 3/2 kT where k = 1.381 x 10-23 J/Kc. For a mole of particles, thermal energy = 3/2 RT where R = NA*k = 8.314 J/K mold. The energy of a particle is distributed over several modes: Translation, Rotation, Vibration, Electronice. Rotation change in energy level < vibration < electronici. Smaller = more dense f. For any mode, as T increases, E increases, so additional energy levels can be populatedV. Boltzmann Distributiona. At a temperature Ti. The number of particles in state 1 with energy E1: N1=e-E1/KTii. And the number of particles in state 2 with energy E2: N2=e-E2/KTiii. Assume that, at this temperature, E2 > E1b. N2/N1 = e-(E2-E1)/KT=e-ΔE/KT (for molar quantities, sub R for K)c. As T increases, E increasesd. e. This distribution, with its dependence on ΔE and T, accounts for the stability of matter: at ordinary temperatures, very few molecules are found in highly excited statesf. Yet the possibility exists for reaction to occur (above T = 0) because there is a nonzero number of accessible excited statesg. Reaction rates increase with an increase in temperature because the excited states become more populatedh. The equilibrium constant – the ratio of products to reactants – depends on density of energy levels of both reactants and