Pop quiz today -_-Chapter 8.1 and 8.2 METABOLISMTwo types of energy1. Kinetica. energy of motionb. Molecular level: thermal energy heat or lightc. Ex. Electrons falling to a lower energy shell2. Potential energya. Energy of position or configurationb. Molecular level: chemical energyi. Stored in the position of the electronii. If an electron is close to negative charges of other electrons and far from positive charges of nuclei potential energy is high because negative charges repel each otheriii. Outermost electron shell has highest potential energyiv. Can move shells in fluorescence and release a photon (energy)Laws of Thermodynamics- control reactions1. Energy is conserved- cannot be created or destroyed can only be transferred or transformed; mass is technically energya. you cannot have more energy in the products than the reactantsb. energy will always be lost in a reaction so no reaction will be perfectly efficient, theoretically perfect efficiency happens at absolute zero (0Kelvin) but at that pointeverything is dead so do you really want perfect efficiency?c. everything takes energy even after you die your body will still be involved in chemical reactions2. Chemical reactions involve such energy transformations3. Entropy always increases- in general physical and chemical processes proceed in the direction that results in lower potential energy enthalpy and increased disorder entropy which together are measured by free energy4. Free energy- (G) amount of energy available to do worka. ΔG is the change in free energy and it determines whether a reaction is spontaneous (happens randomly) or not (requires energy to start)b. Combined contribution in heat content (chemical potential energy and disorder of the system entropy as well as the overall temperatureFormula Δ g = Δ H -T Δ sc. If the G of the products is lower than the G of the reactants then the reaction is spontaneous ΔG<0d. If the G of the products is higher than the G of the reactants then the reaction is NOT spontaneous ΔG>0e. Endergonic- requires energyf. Exergonic- produces energy (doesn’t need any because it has extra)Enthalpy- measure of the total energy of a molecule involves- Potential energy- Pressure and volumeΔH is the charge in enthalpy always do products-reactants1. Entropy- S measure of disorder of a system- ΔS change in entropy- ΔS>0 then it’s an endergonic reactionIn the body energy can be released and then used to form ATPQUESTION: EXPLAIN WHY THE SAME RXN CAN BE NON-SPONTANEOUS AT ONE TEMPERATURE AND SPONTANEOUS AT ANOTHER- high temperature- molecules are moving around more and have more energy so the reactants will have more energy at a high temperature. At a higher temperature there is more energy in the system so the system is more disorderly and the free energy changes.At a low temperature molecules don’t move much and have low energy so they need extra to start a reaction.EXPLAIN WHY SOME EXOTHERMIC REACTIONS ARE NON-SPONATEOUS- some reactions require energy to get started and then release heat when they are doneSTATE WHEN THE OVERALL FREE ENERGY CHANGE IN A REATION IS MOST LIKELY TO BE NEGATIVE- free energy change will be negative when a reaction is spontaneous; the reactants had more energy than the products. The reaction will probably be endothermicNon-spontaneous reactions in cells are started in two ways- transfer of high energy electrons - Transfer of phosphate