CHEM 106 1nd Edition Lecture 7Outline of Last Lecture I. Alcohols + EtherII. Aldehydes + KetonesIII. EstersIV. Amides + PolymersOutline of Current Lecture II. ProteinsIII. ChiralityIV. Fatty acidsV. Thermodynamicsa. Entropy, spontaneous reactions, non-spontaneous reactionsCurrent LectureChapter 13: Organic Chemistry (continued)Single monomer with 2 different functional groupsProteins (amide is also called a peptide bond)R= H, CH3, -CH2, many more13.8 ChiralityReview 9.6 Optical isomers, not superimposable on their mirror imageChiral molecules: chirality is certain if there are 4 different substituents on a C Fig. 9.39A ring, a little more subtle case Fig. 13.51 Fig. 9.38Fatty AcidsOleic acid – C18cisLauric acid (coconut) – C10Glycerol TriglycerideEster of glycerol with 3 fatty acidsChapter 14: Thermodynamics-spontaneous processes, entropy + free energy-review chapter 51st law of thermodynamics: energy is not created or destroyed, only transferred between the system and surroundings14.1 Spontaneous Reactions + EntropySpontaneous: process occurs without outside intervention, often exothermic(ΔH < 0) but not necessarily soNonspontaneous: process occurs only with the continuous input of energyEx:CH4(g) + 2O2(g) → CO2(g) + H2o(l) ΔH < 0 (spontaneous)NH4NO3(s) → NH4NO3(aq) ΔH > 0 (spontaneous) cold packFe(s) at high T + H2O(l) at low T → Fe(s) + H2O(l) at intermediate T (spontaneous)A balloon full of Ar pops + the Ar spreads out in a room (spontaneous)Entropy (s)A measure of the distribution of energy at a specific T2nd law of thermodynamics: the total entropy of the universe increases in any spontaneous reaction.Statistical Entropy:Flat tire example → a tire filled with an ideal gas has a leak and goes flat all at constant T (spontaneous)Forms of Kinetic energyTranslational, rotational, vibrational-only certain energy states are possible (energy states are quantized)Fig. 14.3Levels are closely spaced vibrational +
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