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Fatty Acids

Fatty Acids. This picture is WRONG—always cis double bonds. Fats. Monoglycerides Diglycerides Triglycerides. Saturated Unsaturated. Structural lipids. Glycerophospholipids (Phosphoglycerides) Sphingolipids Sphingomyelin Neutral glycolipids Gangliosides Cholesterol. Phospholipids.

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Fatty Acids

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  1. Fatty Acids This picture is WRONG—always cis double bonds

  2. Fats Monoglycerides Diglycerides Triglycerides Saturated Unsaturated

  3. Structural lipids • Glycerophospholipids (Phosphoglycerides) • Sphingolipids • Sphingomyelin • Neutral glycolipids • Gangliosides • Cholesterol

  4. Phospholipids Common head group ( R ): choline sphingomyelin

  5. Glycolipids (glycosphingolipids) • Neutral glycolipids • Neutral sugars • Gangliosides • Charged sugars

  6. Genetic Diseases • Neimann-Pick Disease • sphingomyelin accumulation • mental retardation • early death • Tay-Sachs Disease • 1:28 American Jews are carriers • Ganglioside accumulation • death by age 3

  7. Cholesterol

  8. Biological Function • Steroid hormones • Vitamins • Eicosanoids • Others

  9. Vitamins • A • D • E • K

  10. Rickets (age 2.5) After treatment with Vitamin D (age 5)

  11. Eicosanoids

  12. Bioenergetics

  13. Uses of energy • Synthetic work • Concentration work • Mechanical work • Electrical work • Heat production • Bioluminescence

  14. Where does the energy come from? • Sun—common • Phototrophs • Chemotrophs • Geothermal sources—rare • Chemotrophs

  15. Where does the energy go?

  16. Thermodynamics: energy and energy flow Bioenergics: thermodynamics of living things

  17. Thermodynamic terms • System—what we're looking out • Surroundings—everything else • Open system—exchanges between system and surroundings • Closed system • State—the physical properties of the system, e.g. temp, pressure, conc. etc. • Work—use of energy to do something (except produce heat)

  18. First Law of Thermodynamics Energy can change forms, but can neither be created nor destroyed

  19. Internal energy (E) Or, for a chemical reaction:

  20. Enthalpy (H)heat content But DV for biological (aqueous) systems is zero, so DHDE

  21. Change in enthalpy is easily measured DH > 0: endothermic DH < 0: exothermic

  22. Usefulness of DH DH is a "state function", determined by change in state, not pathway between states DH = -673 kcal/mol True in either a calorimeter (easily measured) or a cell (very hard to measure)

  23. Not all processes occur • Can't be explained just by 1st law

  24. Second law of thermodynamics • The universe always tends toward greater disorder • Entropy (S) is measure of disorder

  25. Gibb's free energy Combines both enthalpy (H) and entropy (S) and thus combines 1st and 2nd laws of thermodynamics At constant temperature, volume, and pressure

  26. Thermodynamic spontaneity

  27. Spontaneous means a reaction CAN happen, not that it WILL • G is state function: pathway independent • Rate of a reaction: pathway dependent • kinetics DG = -686 kcal/mol

  28. Reversible Reactions

  29. Keq and G Std. Conditions: 25 C, 1 M conc., 1 atm., pH 7.0

  30. G's are additive

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