Chapter 6 Biology 1610

Front 1

Metabolism

Back 1

the chemical processes that occur within a living organism in order to maintain life

Front 2

Catabolism

Back 2

we break stuff up

Front 3

Anabolim

Back 3

we take the smaller molecules and put them together

Front 4

Potential Energy

Back 4

potential energy is stored energy, we use heat or energy becomes un-usable

Front 5

Kinetic Energy

Back 5

Energy in motion

Front 6

How is potential energy stored in chemicals?

Back 6

we store it in a molecule called ATP

Front 7

Describe ATP and how it is used as an energy molecule

Back 7

Adenisine Triphosphate- the energy is stored in the bonds. If we want to get energy out of it we take the ATP and we break off phosphate. Now we are left with ADP and are able to use our energy

Front 8

Describe the first law of thermodynamics

Back 8

Energy cannot be created nor destroyed

Front 9

Describe the 2nd law of thermodynamics

Back 9

In any cyclic process the entropy will either increase or remain the same. Entropy: a state variable whose change is defined for a reversible process at T where Q is the heat absorbed. Entropy: a measure of the amount of energy which is unavailable to do work.

Front 10

Describe a reversible reaction

Back 10

is a chemical reaction where the reactants form products that, in turn, react together to give the reactants back.

Front 11

Exergonic Reaction

Back 11

a reaction that loses energy during the process of the reaction. Activation energy (1) catalyzes the reaction to occur in a spontaneous manner. The progress of the reaction is shown by the line.

Front 12

Endergonic Reaction

Back 12

a reaction that requires energy to be driven. The activation energy for the reaction is typically larger than the overall energy of the exergonic reaction

Front 13

Explain the equation ΔG =ΔH –TΔS

Back 13

ATP <----> ADP+P DELTA/TRIANGLE=CHANGE!!!!! ΔG= Gibbs free energy or the total available energy= the energy of product minus the energy of the reactants.If ΔG is negative then reaction is spontaneous, exergonic, release energyif ΔG is positive then reaction is nonspontaneous, requires energy-endergonic, require energyΔH= the total energy T= the temperatureΔS= entropy, unusable energyΔG =ΔH –TΔS

Front 14

Function of an enzyme

Back 14

help reactions occure more easily

Front 15

Enzyme Inhibitor

Back 15

compounds or agents that combine with an enzyme in such a manner as to prevent the normal substrate-enzyme combination and the catalytic reaction.

Front 16

Enzyme Activatior

Back 16

are molecules that bind to enzymes and increase their activity

Front 17

Reversible

Back 17

form weak bonds with enzymes and easily dissociat from them

Front 18

Irreversible Inhibitors

Back 18

usually form covalent bonds with enzymes and irreversibly inactivate them

Front 19

Competitive

Back 19

compete to bind against substrate or active site

Front 20

Non-competitive Inhibitors

Back 20

bind at an allsteric site; not the active site

Front 21

Allosteric enzymes

Back 21

change their shape or conformation on binding to a substrate, activator, or inhibitor and this change in shape in turn influences the activity of th enzyme, either activating or inhibiting it.

Front 22

Negative Feedback

Back 22

the final product inhibits the first step of the reaction

Front 23

Cofactors

Back 23

inorganic molecules bind with enzyme required for enzyme function