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Introduction to Metabolism

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Presentation on theme: "Introduction to Metabolism"— Presentation transcript:

1 Introduction to Metabolism
Section 1.3

2 ENERGY Living organisms must continually capture, store, and use energy in order to function ENERGY: __________________________. Organisms do all of their work at the ____________ level. Needed for catabolic reactions: Amylose  ______________  _________ + _______ Needed for anabolic reactions: Phosphate + sugar + ______________  nucleotide  ___ METABOLISM: sum of all __________________ and ___________________ reactions in a cell or organism.

3 TYPES OF ENERGY All forms of energy can be classified as KINETIC or POTENTIAL energy. Kinetic energy: energy possessed by moving objects. Examples? Thermal energy: random motion of particles Mechanical energy: coordinated motion of particles Electromagnetic energy: motion of light Electrical energy: motion of charged particles. Potential energy: stored energy An object possesses potential energy because of its position within an attractive or repulsive force field. Gravitational potential energy: attraction between two objects Chemical potential energy: attraction of electrons to protons in a chemical bond.

4 THE DIVER A diver on a diving board possesses _____________ energy because of the force of _____________ between him/her and the Earth, and the distance between the two. The diver must have done __________ to gain this ________________ energy. When the diver dives, the ________________ energy is converted to _________________ energy.

5 The First Law of Thermodynamics
Total amount of energy in the Universe is constant Energy cannot be created or destroyed, only ___________ from one form into another.

6 Usable Energy In organisms, energy is usually stored before being used. Ex// plants capture ___________ energy and convert it to chemical potential energy in _______________ and may be stored in that form before being used. Through the reactions of cellular respiration, the chemical energy in ____________ is passed on to ______. ATP: the primary energy-transferring compound. ATP may be used to activate protein carriers which transport ions through a cell membrane ______________ the concentration gradient, building up ______________ potential energy.

7 Bond Energy Molecules possess stability because of the chemical bonds between their atoms. The atoms achieve a greater stability by attaining a stable ___________________ electron configuration. Bond Energy: measure of the stability of a covalent bond. ATOMS NOT IN A BOND CONTAIN MORE ENERGY THAN ATOMS IN A BOND. Equal to the minimum amount of energy needed to break the bond between two atoms. Equal to the amount of energy released when a bond is formed. ENERGY IS __________________ WHEN REACTANT BONDS BREAK AND ENERGY IS __________________ WHEN PRODUCT BONDS FORM.

8 POTENTIAL ENERGY DIAGRAMS
Shows the changes in potential energy during a chemical reaction. ACTIVATION ENERGY: amount of energy needed to break the bonds between reactants. TRANSITION STATE: temporary condition in which the bonds within the reactants are breaking and bonds between products are forming. ENTHALPY OF REACTION: ∆H: overall change in energy that occurs in a chemical reaction (the ‘system’). Deals with the NET ENERGY input or output. If bonds in products more stable than those in reactants: net energy ______________. This type of reaction is called an __________________________ reaction. The system ________ energy, meaning that ∆H is __________________. If bonds in products less stable than those in reactange: net energy ______________. This type of reaction is called an __________________________ reaction. The system ________ energy, meaning that ∆H is __________________

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10 ENTROPY Measure of the disorder in energy or in a collection of objects. Increases when disorder increases. In chemical reactions, entropy increases when: Solid  ________  _______ Fewer moles of reactant molecules form greater number of moles of product molecules: Complex molecules become simpler molecules: ______________________________________________. Diffusion: solutes move from an area of _____ concentration to an area of ______ concentration.

11 Gibbs Free Energy energy that can do USEFUL work.
There is a relationship between the energy change, entropy change, and temperature of a reaction. Predicts if a reaction will proceed spontaneously or not.

12 DIFFERENCE BETWEEN ENERGY AND FREE ENERGY?
Aquarium example: PURPOSE: to turn the blades of the fan. Both aquariums start with same amount of total energy. Aquarium 1: water moves from more ordered state (low entropy, higher free energy) to less ordered state (high entropy, lower free energy)  release of free energy. Aquarium 2: blade does not move: contains ENERGY, but does not contain FREE ENERGY. Thermal energy: molecules are moving, but are not doing any ‘useful’ work.

13 SPONTANEOUS REACTIONS
If decrease in Gibbs free energy  spontaneous. Gibbs free energy: ∆G Change in Gibbs free energy: ∆G = Gfinal – Ginitial If ∆G is negative, ___________________ reaction. If ∆G is positive, ___________________ reaction. A spontaneous reaction is ________________________ in the reverse reaction. Aquarium example: work must be done to reestablish the conditions of aquarium 1 (more order, more free energy) From another reaction!!!

14 SECOND LAW OF THERMODYNAMICS
The entropy of the universe increases with any change that occurs. Example: Geevithan eats a potato chip: Getting chip to mouth: increase in gravitational potential energy, decrease in entropy (more ordered)  increase in Gibbs: needs energy to do work. Energy for the work is derived from converting ordered nutrients (glucose) into more disordered carbon dioxide, water molecules, and other wastes: _________________ reactions. In the end, amount of disorder created in the ‘reaction’ is greater than order  net amount of disorder in universe.

15 DEFINITIONS: EXERGONIC: a chemical reaction in which the energy of the products is less than the energy of the reactants; chemists call this an ___________________ reaction. Is spontaneous: ∆G is _____________________. ENDERGONIC: a chemical reaction in which the energy of the products is more than the energy of the reactants; chemists call this an ________________ reaction. Is nonspontaneous: ∆G is ________________________.

16 SPONTANEOUS CHANGE, FREE ENERGY, AND WORK

17 Yeah... So? COOOOOOOOOOOOOOOOOOOOOOL.

18 Metabolic Reactions Reactions of metabolism are ENZYME CATALIZED and are all reversible. When a reversible reaction reaches equilibrium, its ∆G is zero. No free energy = ________________ cell.

19 ATP  OUR HERO!!!! ATP: primary source of free energy in living cells.
Made of: _________________, _________________, and ___________________. When a cell requires free energy to drive an ______________________ reaction, an enzyme called ATPase catalyzes the ______________ of the terminal _______________ of an ATP molecule, resulting in _____________ and _____. 31 kj/mol of free energy is released.

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21 The free energy released during the hydrolysis of ATP is not heat... Why?
A single working muscle cell uses about _____________________________ ATP molecules per minute. An active body consumes _________________ in ATP per day.

22 Phosphorylation Phosphate group attached to an organic molecule (like ADP or a protein pump)

23 HOMEWORK: Read section on Redox Reactions (page 66-67)
PPs pg. 68 #1-10.


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