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BIOSC 0150 > 2.1 Energy > Flashcards

2.1 Energy Flashcards

1
Q

Describe what a chemical reaction is, and characterize the reactants versus products for a given
reaction (e.g., bonds made/broken, relative energy states).

A

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2
Q

Distinguish between the different types of energy

A

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3
Q

Describe the forms of energy in biological systems.

A

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4
Q

• State the first and second laws of thermodynamics, and explain how they relate to biological
systems.

A

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5
Q

Explain how the change in Gibbs free energy for a chemical reaction determines if the reaction
can proceed.

A

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6
Q

Differentiate between exergonic and endergonic reactions.

A

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7
Q

Use the equation ∆G = ∆H – T∆S to describe biological systems.

A

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8
Q

Explain the characteristics of ATP that account for the high free energy released during its
hydrolysis.

A

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9
Q

Explain how coupling reactions to ATP hydrolysis helps drive reactions with a positive ∆G.

A

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10
Q

Adenosine diphosphate (ADP)

A

nucleoside phosphate comprised of a ribonucleoside and two phosphate groups.

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11
Q

Adenosine triphosphate (ATP)

A

directly provide energy to chemical reactions

in life that need it

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12
Q

ATP hydrolysis

A

releases energy

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13
Q

Chemical energy

A

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.

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14
Q

Chemical reaction

A

The change in the composition or distribution of atoms of a substance with consequent alterations in properties.

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15
Q

Electrical energy

A

a form of energy resulting from the flow of electric charge.

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16
Q

Endergonic

A

a reaction that releases free energy in the process of the reaction.

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17
Q

Energetic coupling

A

allows endergonic reactions to proceed using the energy

released from exergonic reactions

18
Q

• Energy

A

The capacity to do work or move matter against an opposing force. The capacity to accomplish change in physical and chemical systems.

19
Q

Enthalpy

A

The total energy of a system.

20
Q

Entropy

A

A measure of the degree of disorder in any system. Spontaneous reactions in a closed system are always accompanied by an increase in entropy.

21
Q

Exergonic

A

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.

22
Q

First law of thermodynamics

A

the first law expresses that energy can be transformed (i.e. changed from one form to another), but cannot be created or destroyed

23
Q

Gibbs free energy

A

the energy in a system that is available to do work

24
Q

Heat

A

the flow of thermal energy.

25
Q

Hydrolysis reaction

A

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

26
Q

Inorganic phosphate (Pi)

A

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.

27
Q

Kinetic energy

A

energy of movement

28
Q

Light

A

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29
Q

Mechanical energy

A

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30
Q

Net reaction

A

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31
Q

Nonspontaneous

A

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32
Q

Phosphorylated intermediate

A

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33
Q

Phosphorylation

A

Addition of a phosphate group.

34
Q

Potential energy

A

stored energy

35
Q

Product

A

molecules that result from the completion of a chemical reaction.
progesterone

36
Q

Reactant

A

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37
Q

Second law of thermodynamics

A

The principle that when energy is converted from one form to another, some of that energy becomes unavailable for doing work.

38
Q

Spontaneous

A

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39
Q

Substrate

A

(1) The molecule or molecules on which an enzyme exerts catalytic action. (2) The base material on which a sessile organism lives.

40
Q

Temperature

A

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41
Q

Thermal energy

A

he energy contained within a system that is responsible for its temperature.

BIOSC 0150 (16 decks)

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