1. Metabolism and Energy
Metabolism is the sum of all chemical reactions in an organism.
Energy is the ability to do work
How do these work together?

2. Metabolism in a nutshell 
WOW There is a lot going on!

3. What is energy Many forms… Chemical Electrical Mechanical Light
Energy is used anytime work is performed
Climb a mountain
Car travels down the road
Link amino acids together
Pump sucrose across a membrane
Many forms…
Chemical
Electrical
Mechanical
Light
Thermal
Regardless of the form, energy exists in one of two states…
Kinetic Energy
Stored Energy- Potential energy

4. Kinetic vs. Potential Energy
Kinetic Energy
energy of motion
Performs work by making things move
Potential Energy
stored energy
chemical potential/gravitational energy

5. The First Law of Thermodynamics The total amount of energy in any closed system is constant. Energy cannot be created or destroyed; it can only be converted from one form to another. If a physical system gains an amount of energy, another physical system must experience a loss of energy of the same amount.

6. BOND ENERGY
A measure of the strength or stability of the covalent bond
Measured in KJ/mol (equal to amount of energy absorbed per mole when the bond between atoms is broken(energy is needed to be put into the breaking of the bonds))
Important
Energy is absorbed by the bonds as energy is put in to break them and energy is released Question -
How will this affect the net amount of energy absorbed or released in the overall reaction?

7. Endothermic vs. Exothermic
Energy Diagrams…
the y-axis indicates the level of potential energy for the reactants before the reaction and the products after the reaction has occurred
If energy is released, the reaction is EXOTHERMIC
If energy is absorbed, the reaction is ENDOTHERMIC
Bond energy and Potential energy have an inverse relationship
The weaker the bond, the higher the potential energy
The stronger the bond, the lower the potential energy

8. Enthalpy (∆ H) The measure of the energy of a system usually measured using heat released or absorbed by a system overall. This is calculated by using the following formula; ∆ H total = ∆ H final - ∆ H initial Exothermic Reaction have a - ∆ H Endothermic Reactions have a + ∆ H

9. The second Law of Thermodynamics
In every energy transfer or conversion, some of the useful energy in the system becomes unusable and increases the entropy of the universe.
So what is Entropy?? 
Entropy is a measurement of the disorder in a system. 
CHAOS…..
In chemical reactions entropy actually increases when
Solids react to form liquids or gases
Liquids react to form gases
The total number of product molecules is greater than the total number of reactant molecules 
There is energy expended to maintain the living structures in all living things. This allows order to be established even when there is disorder (entropy).
Spontaneous change is a change that will, once begun, continue on its own under a given set of conditions and it will not require a continuous supply of energy.
So a non spontaneous reaction is one that needs continual energy input to continue.

10. STUDY BOOK Gibbs Free Energy: What is this?? What is the equation?
Define exergonic and endergonic reactions. P
Compare and contrast
Kinetic and Potential energy
Exothermic and Endothermic reactions