Energy and the Cell
What do you know…
• About energy?
• Is it matter?
• What kinds are there?
• Can it be transformed to other forms?
What is energy?
• “Capacity to do work”
• Do living organisms need energy?
• YES!!!!!!!!!
Contrast
Explain potential and kinetic energy of the roller coaster
Two Types of Energy
• Kinetic
• Actually doing work (moving)
• Potential
• Stored energy
• Due to location or arrange-
• ment (of atoms)
0-C-0
Examples
• Kinetic• Pedaling a bike
• Heat = moves molecules
• electron jumps
• (go to Bohr’s quantum behavior of an atom)
ICE
STEAM
Potential Energy
• Potential• Water behind a dam
• Electron’s position in an atom
Name the type:
What’s the most important type to living organisms?
•Chemical• The energy in food molecules can
be stored in the bonds
Explain the energy transfers:
When you break bonds…
• You release the energy that held the bonds together
• This energy can do work in the body.
Thermodynamics
• laws governing energy transfer
First Law of thermodynamics
• in closed system, energy can neither be created nor destroyed, only changed in form.
First Law of Thermodynamics Examples
• Light energy to chemical energy (from sun to sugar in a plant)
• Water behind a dam (potential) is released (kinetic)
How does this explain energy transfers?
What energy transfers are occurring?
Second Law of Thermodynamics
• energy transformations inevitably involve increased disorder or entropy.
• NOTE: it is the environment that is increasing disorder, not the cell
Entropy…what is that?
• Living things use this energy to create order (reduce entropy) locally, but the overall entropy of the solar system invariably increases.
In other words…
• If a particular system becomes more ordered, its surrounding become more disordered
• A cell makes organelles to increase order, but its surroundings become less orderly
Second Law
• energy of all kinds in our material
world disperses or
dissipates if it is not hindered from doing so
Must be spontaneous
• All spontaneous happenings in the material world are examples of the second law because they involve energy dispersing.
Could you explain that in other words?
• heat flows from hot (more energy) to cold (less energy)
• diffusion leads to substances becoming uniformly dispersed
• You could think of cells as
• “Islands of Low Entropy”
Is the transformation perfect?
• A cell cannot transfer or transform energy with 100% efficiency.
• Where does the lost energy go?
• Mostly lost as heat.
NOT Just organizing your desk
Do Worksheet
• Hot pans of water
• Water on Niagara
• Air in tires that got a puncture
• Speeding car hits a brick wall
• Spark in contact with gasoline
• Sun’s energy hits the ocean
• Huge earthquake under the ocean
Exergonic Reaction
• Releases Energy
• Begins with reactants whose covalent bonds contain more energy than its products
Exergonic: Releasing Energy
• Burning
• One big step
• Breaking bonds
• Many smaller steps
Exergonic Example
• Glucose (reactant) breaks down into carbon dioxide and water (products)
• C6H12O6 CO2 + H2O
“Cellular Respiration”
• Breaking glucose molecules to release energy and store it in a form the cell can use (ATP molecules)
• “slow burn”
Endergonic Reaction
• The products have more energy than the reactants
• Requires an input of energy
• Usually in the form of ATP
Endergonic Reaction
• Carbon dioxide and water combine to form glucose
CO2 + H2O C6H12O6
“Cellular Metabolism”
• Sum of exergonic and endergonic reactions of cells
• CO2 + H2O C6H12O6
• Less energy more energy molecules molecules
ATP
• No…not the new rock band from Japan
• Well, what is it?
ATP
• Adenosine Triphosphate
• “cell’s batteries”
• “energy currency”
ATP
How are they different?
• Adenosine triphosphate
• Adenosine diphosphate
Third Phosphate
• Acts as an energy shuttle
Making ADP + Pi
• ATP is energy rich and breaks down into ADP and Pi (inorganic phosphate) + energy
• is exergonic
Making ATP
• energy + ADP + Pi -> ATP is endergonic
• requiring the input of energy.
Which has more energy?
• ATP or ADP?
• Answer: ATP
Phosphorylation
• Adding of a phosphate group to a molecule
Energy Coupling
• Energy released from exergonic reactions drive endergonic reactions
ADP + Pi <=> ATP+
REACTIONS
• The end products of a reaction may have more (endergonic) or less (exergonic) energy than the substrate molecules.
REACTIONS
• Most reactions are reversible, occur in both directions -
• reactants -> end products
• AND end products -> reactants.
REACTIONS
• Reversible reactions move
toward an equilibrium, a state in which the reaction
occurs at about the same rate in both directions.
So...
•ATP is like money in a checking account
P P P
Adenosine triphosphate (ATP)Adenosine triphosphate (ATP)
P P P++
Adenosine diphosphate (ADP)Adenosine diphosphate (ADP)
Hydrolysis of ATP•ATP + H2O ADP + P (exergonic)
HydrolysisHydrolysis(add water)(add water)
P P P
Adenosine triphosphate (ATP)Adenosine triphosphate (ATP)
P P P++
Adenosine diphosphate (ADP)Adenosine diphosphate (ADP)
Dehydration of ATP•ADP + P ATP + H2O (endergonic)
Dehydration synthesisDehydration synthesis (remove water)(remove water)
ATP
• Breaks down readily
• Would break down spontaneously except for the energy barrier
If entropy is spontaneous…• Why aren’t we all just
spontaneously combusting?
Energy of Activation EA
• The amount of energy that reactants must absorb to start a chemical reaction
But what if…
• The barrier is too great and the reaction cannot go…
• Use ENZYMES
Enzymes
• “Biological Catalysts”• (speed up a reaction without being changed themselves)
Enzymes
• Usually end in –ase
• Usually named for what they work on
• EXAMPLE: Lipase works on Lipids
How do enzymes work?
•Each enzyme has a specific shape, which will determine which reactants it will work on
• Active Site- small area where enzyme and substrate work
•Substrate=A substance that the enzyme acts on
Induced Fit
• Slight change in the shape of the active site of an enzyme as it embraces its substrate (like grasping hands)
• Enzyme animation
Is an enzyme…
• Able to be used over and over?
• YES!!!!!!!!!
Most enzymes…
• Work best at what temperature?
• 35-40oC
• What happens at high temperatures?
• Denatures them (unravels)
• Why is salty bad?
• Salt ions interfere with chemical bonds
Most enzymes…
• What is the optimal pH?
• 6-8
• What does too low (too acidic) of pH do to enzymes?
• Extra H+ ions interfere with chemical bonds
Cofactores
• Nonprotein helpers
• EXAMPLES:
• Zn, Fe, Cu (inorganic ones)
• Vitamins like B6 (organic ones)=also called coenzymes
Enzyme Inhibition
• Competetive inhibitor• Resembles the enzyme and competes for
the active site
• Noncompetetive inhibitor• Does not enter the activ site• Binds somewhere outside the active site• Inhibitor animations
Negative Feedback
• When a cell’s supply exceeds the demand
• Negative Feedback animation
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