energy and the cell
DESCRIPTION
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. - PowerPoint PPT PresentationTRANSCRIPT
![Page 1: Energy and the Cell](https://reader036.vdocuments.net/reader036/viewer/2022081603/568140b7550346895dac7b66/html5/thumbnails/1.jpg)
Energy and the Cell
![Page 2: Energy and the Cell](https://reader036.vdocuments.net/reader036/viewer/2022081603/568140b7550346895dac7b66/html5/thumbnails/2.jpg)
What do you know…
• About energy?
• Is it matter?
• What kinds are there?
• Can it be transformed to other forms?
![Page 3: Energy and the Cell](https://reader036.vdocuments.net/reader036/viewer/2022081603/568140b7550346895dac7b66/html5/thumbnails/3.jpg)
What is energy?
• “Capacity to do work”
• Do living organisms need energy?
• YES!!!!!!!!!
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Contrast
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Explain potential and kinetic energy of the roller coaster
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Two Types of Energy
• Kinetic
• Actually doing work (moving)
• Potential
• Stored energy
• Due to location or arrange-
• ment (of atoms)
0-C-0
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Examples
• Kinetic• Pedaling a bike
• Heat = moves molecules
• electron jumps
• (go to Bohr’s quantum behavior of an atom)
ICE
STEAM
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Potential Energy
• Potential• Water behind a dam
• Electron’s position in an atom
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Name the type:
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What’s the most important type to living organisms?
•Chemical• The energy in food molecules can
be stored in the bonds
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Explain the energy transfers:
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When you break bonds…
• You release the energy that held the bonds together
• This energy can do work in the body.
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Thermodynamics
• laws governing energy transfer
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First Law of thermodynamics
• in closed system, energy can neither be created nor destroyed, only changed in form.
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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)
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How does this explain energy transfers?
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What energy transfers are occurring?
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Second Law of Thermodynamics
• energy transformations inevitably involve increased disorder or entropy.
• NOTE: it is the environment that is increasing disorder, not the cell
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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.
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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
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Second Law
• energy of all kinds in our material
world disperses or
dissipates if it is not hindered from doing so
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Must be spontaneous
• All spontaneous happenings in the material world are examples of the second law because they involve energy dispersing.
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Could you explain that in other words?
• heat flows from hot (more energy) to cold (less energy)
• diffusion leads to substances becoming uniformly dispersed
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• You could think of cells as
• “Islands of Low Entropy”
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Is the transformation perfect?
• A cell cannot transfer or transform energy with 100% efficiency.
• Where does the lost energy go?
• Mostly lost as heat.
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NOT Just organizing your desk
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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
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Exergonic Reaction
• Releases Energy
• Begins with reactants whose covalent bonds contain more energy than its products
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Exergonic: Releasing Energy
• Burning
• One big step
• Breaking bonds
• Many smaller steps
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Exergonic Example
• Glucose (reactant) breaks down into carbon dioxide and water (products)
• C6H12O6 CO2 + H2O
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“Cellular Respiration”
• Breaking glucose molecules to release energy and store it in a form the cell can use (ATP molecules)
• “slow burn”
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Endergonic Reaction
• The products have more energy than the reactants
• Requires an input of energy
• Usually in the form of ATP
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Endergonic Reaction
• Carbon dioxide and water combine to form glucose
CO2 + H2O C6H12O6
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“Cellular Metabolism”
• Sum of exergonic and endergonic reactions of cells
• CO2 + H2O C6H12O6
• Less energy more energy molecules molecules
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ATP
• No…not the new rock band from Japan
• Well, what is it?
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ATP
• Adenosine Triphosphate
• “cell’s batteries”
• “energy currency”
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ATP
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How are they different?
• Adenosine triphosphate
• Adenosine diphosphate
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Third Phosphate
• Acts as an energy shuttle
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Making ADP + Pi
• ATP is energy rich and breaks down into ADP and Pi (inorganic phosphate) + energy
• is exergonic
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Making ATP
• energy + ADP + Pi -> ATP is endergonic
• requiring the input of energy.
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Which has more energy?
• ATP or ADP?
• Answer: ATP
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Phosphorylation
• Adding of a phosphate group to a molecule
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Energy Coupling
• Energy released from exergonic reactions drive endergonic reactions
ADP + Pi <=> ATP+
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REACTIONS
• The end products of a reaction may have more (endergonic) or less (exergonic) energy than the substrate molecules.
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REACTIONS
• Most reactions are reversible, occur in both directions -
• reactants -> end products
• AND end products -> reactants.
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REACTIONS
• Reversible reactions move
toward an equilibrium, a state in which the reaction
occurs at about the same rate in both directions.
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So...
•ATP is like money in a checking account
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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)
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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)
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ATP
• Breaks down readily
• Would break down spontaneously except for the energy barrier
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If entropy is spontaneous…• Why aren’t we all just
spontaneously combusting?
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Energy of Activation EA
• The amount of energy that reactants must absorb to start a chemical reaction
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But what if…
• The barrier is too great and the reaction cannot go…
• Use ENZYMES
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Enzymes
• “Biological Catalysts”• (speed up a reaction without being changed themselves)
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Enzymes
• Usually end in –ase
• Usually named for what they work on
• EXAMPLE: Lipase works on Lipids
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How do enzymes work?
•Each enzyme has a specific shape, which will determine which reactants it will work on
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• Active Site- small area where enzyme and substrate work
•Substrate=A substance that the enzyme acts on
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Induced Fit
• Slight change in the shape of the active site of an enzyme as it embraces its substrate (like grasping hands)
• Enzyme animation
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Is an enzyme…
• Able to be used over and over?
• YES!!!!!!!!!
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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
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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
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Cofactores
• Nonprotein helpers
• EXAMPLES:
• Zn, Fe, Cu (inorganic ones)
• Vitamins like B6 (organic ones)=also called coenzymes
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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
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Negative Feedback
• When a cell’s supply exceeds the demand
• Negative Feedback animation