Exam 2 Flashcards
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Energy
The capacity to do work
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Types of Energy (2)
Kinetic: the energy of motion
Potential: stored energy
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What is the form of energy that most other forms can be converted to?
Heat energy
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What is heat energy measured in?
Calories
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Calories
One calorie = heat energy required to raise the temp of 1 g of water 1 degree C
1 kilocalorie (kcal) = 1000 calories = 1 food calorie
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How is potential energy, stored in chemical bonds, transferred from one molecule to another?
They are transferred by way of electrons
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Redox Reactions
First, remember that redox comes from reduction-oxidation (reduction-gaining an electron; oxidation-losing an electron)
This is both oxidation and reduction occurring at the same time
These reactions are always coupled to one another
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First Law of Thermodynamics
Energy cannot be created or destroyed, it can only be converted from one form to another
Ex: sunlight energy –> chemical energy
(through photosynthesis)
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Second Law of Thermodynamics
Without external energy input, all systems naturally become more disorderly over time
Ex: think of a room becoming messy over time-this seems to require zero energy, whereas cleaning it (making it orderly) requires work
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Entropy
Disorder
Written as “S”
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Free Energy
The energy available to do work
Written as “G” (Gibb’s Free Energy)
Free energy = Enthalpy – (Temp X Entropy)
G = H - TS
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Enthalpy
Energy contained in a molecule’s chemical bonds
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What effect do chemical reactions have on free energy?
Chemical reactions create changes in free energy
ΔG = ΔH - T ΔS
(Δ is the symbol “delta,” it represents a change)
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In a chemical reaction, what happens when the products have MORE free energy than the reactants?
ΔG is positive (the change in free energy is a positive change); energy is gained
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In a chemical reaction, what happens when the products contain LESS free energy than the reactants?
ΔG is negative (the change in free energy is negative); energy is lost
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Endergonic Reaction
Requires free energy (positive ΔG)
An “energy requiring” reaction
*ender/enter ~ energy enters
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Exergonic Reaction
releases free energy (negative ΔG)
An “energy yielding” reaction
*exo/exit ~ energy leaves
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Activation Energy
Energy needed to get a reaction started by destabilizing chemical bonds
*even exergonic reactions require some energy just to get started
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Catalysts
Substances that lower the activation energy of a reaction
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ATP
Adenosine triphosphate, the energy currency of the cells
Structure:
ribose (a 5-C sugar)
adenine (a nucleotide)
three phosphates
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Where does ATP store energy?
In its phosphate bonds
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Phosphates are highly _____
Phosphates are highly electronegative
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What happens because of the electronegativity in phosphates? (What are some characteristics/properties they have due to their electronegativity?) (3)
They naturally repel each other
Much energy is required to keep them bound to each other
Much energy is released when the P bonds are broken
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What happens when the bond between phosphates is broken by hydrolysis?
*First of all, hydrolysis is the chemical breakdown of a compound due to its reaction with water
When this occurs, energy is released
ATP = ADP + Pi