2.1 Energy Flashcards
Describe what a chemical reaction is, and characterize the reactants versus products for a given
reaction (e.g., bonds made/broken, relative energy states).
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Distinguish between the different types of energy
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Describe the forms of energy in biological systems.
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• State the first and second laws of thermodynamics, and explain how they relate to biological
systems.
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Explain how the change in Gibbs free energy for a chemical reaction determines if the reaction
can proceed.
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Differentiate between exergonic and endergonic reactions.
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Use the equation ∆G = ∆H – T∆S to describe biological systems.
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Explain the characteristics of ATP that account for the high free energy released during its
hydrolysis.
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Explain how coupling reactions to ATP hydrolysis helps drive reactions with a positive ∆G.
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Adenosine diphosphate (ADP)
nucleoside phosphate comprised of a ribonucleoside and two phosphate groups.
Adenosine triphosphate (ATP)
directly provide energy to chemical reactions
in life that need it
ATP hydrolysis
releases energy
Chemical energy
Energy released from a substance, or absorbed in the formation of a chemical compound, during a chemical reaction. The energy released from ATP or glucose during a chemical reaction is an example of chemical energy.
Chemical reaction
The change in the composition or distribution of atoms of a substance with consequent alterations in properties.
Electrical energy
a form of energy resulting from the flow of electric charge.
Endergonic
a reaction that releases free energy in the process of the reaction.
Energetic coupling
allows endergonic reactions to proceed using the energy
released from exergonic reactions
• Energy
The capacity to do work or move matter against an opposing force. The capacity to accomplish change in physical and chemical systems.
Enthalpy
The total energy of a system.
Entropy
A measure of the degree of disorder in any system. Spontaneous reactions in a closed system are always accompanied by an increase in entropy.
Exergonic
a chemical reaction where the change in the free energy is negative (there is a net release of free energy). This indicates a spontaneous reaction if the system is closed and initial and final temperatures are the same.
First law of thermodynamics
the first law expresses that energy can be transformed (i.e. changed from one form to another), but cannot be created or destroyed
Gibbs free energy
the energy in a system that is available to do work
Heat
the flow of thermal energy.
Hydrolysis reaction
se water to breakdown polymers into monomers and is the opposite of dehydration synthesis, which forms water when synthesizing a polymer from monomers. Hydrolysis reactions break bonds and release energy
Inorganic phosphate (Pi)
It is required in the ATP formation, kinase/phosphatase signalling and in the synthesis of lipids, carbohydrates and nucleic acids.
salts of phosphoric acid: inorganic phosphates are inorganic salts.
Kinetic energy
energy of movement
Light
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Mechanical energy
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Net reaction
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Nonspontaneous
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Phosphorylated intermediate
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Phosphorylation
Addition of a phosphate group.
Potential energy
stored energy
Product
molecules that result from the completion of a chemical reaction.
progesterone
Reactant
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Second law of thermodynamics
The principle that when energy is converted from one form to another, some of that energy becomes unavailable for doing work.
Spontaneous
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Substrate
(1) The molecule or molecules on which an enzyme exerts catalytic action. (2) The base material on which a sessile organism lives.
Temperature
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Thermal energy
he energy contained within a system that is responsible for its temperature.
