 Living organisms require energy to perform functions. They:  Kidney cells: › to transports materials  Digestive tract: › break macromolecules  Heart: › to pump

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Metabolism : Anabolism : Catabolism : 4

Energy : Energy can take many forms: mechanicalelectric current heat light All energy can be classified as: - kinetic energy : - potential energy : 5

 stored energy. › ___________________________________ 6

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Potential energy stored in chemical bonds can be transferred from one molecule to another by way of electrons. oxidation : reduction : redox reactions 8

 Energy of motion › ________________________________________ 9

c04r9E 10

 Study of heat and energy flow within chemical reactions 11

First Law of Thermodynamics – For example: sunlight energy chemical energy photosynthesis 12

 Exercise to lose weight › produce heat and you sweat › heats the air around you.  When you eat a pizza › energy from the chemical bonds in the bread, cheese, etc. is broken down › converted into ATP molecules through cellular respiration. 13

 _______________________________________ _______________________________________  The enthalpy change (ΔH) › amount of heat released or absorbed when a chemical reaction occurs at a constant pressure. › ΔH formation = _____________________________ 14

 Reactants:  Activation energy (Ea):  Transition state:  Products: 15

 some of the reactant's potential energy is released into the surroundings as heat.  enthalpy of the products is ____________________  energy is _____________  ΔH is ____________ 16

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Second Law of Thermodynamics : entropy : The 2 nd Law of Thermodynamics states that entropy is always increasing. 22

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Free energy : -denoted by the symbol G (Gibb’s free energy) enthalpy : free energy = enthalpy – (entropy x temp.) G = H - TS 24

 Chemical reactions can create changes in free energy.  When products contain more free energy than reactants  G is positive.  When reactants contain more free energy than products  G is negative. 25

Chemical reactions can be described by the transfer of energy that occurs: endergonic reaction : exergonic reaction : 26

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Most reactions require some energy to get started. activation energy : catalysts : 28

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C6H12O6 + O2 → CO2 + H2O + Energy (as ATP) ΔG = kJ/mol of glucose  release of energy  an increase in entropy  This reaction tends to proceed spontaneously. 30

Photosynthesis Chemical Equation CO2 + H2O + Energy → C6H12O6 + O2 ΔG = kJ/mol of glucose  energy is absorbed  a decrease in entropy  This reaction does not proceed spontaneously as energy is needed to drive the reaction. 31

ATP = adenosine triphosphate ATP structure: 32

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Adenosine Triphosphate (ATP) Section 9.1 P P A P

Mono = One phosphate group Di = Two phosphate groups Tri = three phosphates groups Adenosine Triphosphate (ATP) Section 9.1 P P A P

The battery of the cell Section 9.1

When the bond between phosphates is broken: ATP ADP + P i energy is released ADP = adenosine diphosphate P i = inorganic phosphate This reaction is reversible. 37

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 Section 1.3, p.68 1, 2, 5, 10, 11 40