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 __________________

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.

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.