Introduction To Metabolism (Ap Biology)

Front 1

Define "Metabolism"

Back 1

The totality of an organism's internal chemical reactions.

Front 2

what word means "the totality of an organism's internal chemical reactions."?

Back 2

Metabolism

Front 3

Metabolism contains these kinds of pathways in which a certain molecule is converted again and again until it becomes the final, desired product.

Back 3

Metabolic pathways.

Front 4

In metabolic pathways, molecules are ______ again and again until it becomes the final, desired product.

Back 4

In metabolic pathways, molecules are CONVERTED again and again until it becomes the final, desired product.

Front 5

State and define the two kinds of metabolic pathways.

Back 5

Catabolic pathways - (sounds like "catastrophe") molecules break down into simpler pieces.

Anabolic pathways - Energy is consumed in order TO BUILD a larger molecule.

Front 6

Define "Bioenergetics".

Back 6

The study of how organisms manage energy resources.

Front 7

What is defined as "The study of how organisms manage energy resources."?

Back 7

Bioenergetics

Front 8

What is defined as "The capacity to cause change."?

Back 8

Energy

Front 9

What are the two types of energy?

Back 9

Kinetic energy (relative motion)
Potential energy (based on location)

Front 10

What's the sub-type of kinetic energy and define it.

Back 10

Heat/Thermal Energy - Kinetic associated with the random movement of molecules.

Front 11

What's the sub-type of potential energy and define it.

Back 11

Chemical Energy - Energy for release in a chemical reaction.

Front 12

List the types of energy and their sub-types.

Back 12

- Kinetic
- - Heat/Thermal

- Potential
- - Chemical

Front 13

Thermodynamics is the study of energy ______________.

Back 13

Thermodynamics is the study of energy TRANSFORMATION.

Front 14

What is the first law of Thermodynamics?

Back 14

Energy can be transferred and transformed but not created or destroyed. (Also known as the conservation of energy)

Front 15

What is the second law of Thermodynamics?

Back 15

Every energy transfer or transformation increases the entropy of the system/universe.

Front 16

Define "Entropy".

Back 16

Entropy: Disorder in the universe.

Front 17

In what form does energy tend to be lost in reactions?

Back 17

Energy tends to be lost in the form of HEAT in reactions.

Front 18

We can NEVER _____ of energy input to energy output.

Back 18

We can NEVER 100% of energy input to energy output.

Front 19

Define "Free Energy".

Back 19

Free Energy measures the portion of a system's energy that can perform work when conditions are uniform (inside of a cell).

Front 20

What is "free energy" in a nutshell?

Back 20

Energy available to perform work.

Front 21

ONLY processes with a negative ∆G are ________ (require ____ input of energy).

Back 21

ONLY processes with a negative ∆G are SPONTANEOUS (require NO input of energy).

Front 22

Processes that require NO input of energy (such as rolling a ball down a hill) are spontaneous/instantaneous.

Back 22

Processes that require NO input of energy (such as rolling a ball down a hill) are spontaneous.

Front 23

Describe a spontaneous event.

Back 23

It is not immediate; we can predict or foresee it's impending arrival or happening. Instinctive or involuntary.

Front 24

A positive/negative ∆G value indicates that there must be an input of energy to drive the reaction.

Back 24

A positive ∆G value indicates that there must be an input of energy to drive the reaction.

Front 25

What equation is used to determine the ∆G value?

Back 25

∆G = Gf - Gi

(f = final state ; i = initial state)

Front 26

All systems want to be in a stable state, or _______.

Back 26

All systems want to be in a stable state, or EQUILIBRIUM.

Front 27

Very unstable systems will have a ______ G value.

Back 27

Very unstable systems will have a HIGH G value.

Front 28

Systems that have a high G value tend to be stable/unstable.

Back 28

Systems that have a high G value tend to be unstable.

Front 29

Anything that has high potential energy, has a high _________.

Back 29

Anything that has high potential energy, has a high G value.

Front 30

Do potential energy and G values go hand-in-hand?

Back 30

Yes.

Front 31

Systems that have a low G value tend to be stable/unstable.

Back 31

Systems that have a low G value tend to be stable.

Front 32

Anything that requires energy is/isn't spontaneous.

Back 32

Anything that requires energy isn't spontaneous, or non-spontaneous.

Front 33

An exergonic reaction absorbs/releases free energy.

Back 33

An exergonic reaction releases free energy.

Front 34

In exergonic reactions, ∆G increases/decreases.

Back 34

In exergonic reactions, ∆G decreases.

Front 35

When ∆G decreases, as in an exergonic reaction, the difference is usually positive/negative, which means it is spontaneous/non-spontaneous.

Back 35

When ∆G decreases, as in an exergonic reaction, the difference is usually negative, which means it is spontaneous.

Front 36

In an exergonic reaction, the greater the decrease of ∆G, the greater amount of _______ is produced.

Back 36

In an exergonic reaction, the greater the decrease of ∆G, the greater amount of ENERGY is produced.

Front 37

Describe a situation where the ∆G increases and is positive.

Back 37

When the ∆G increases and is positive, the situation is non-spontaneous; energy is required; and it is endergonic.

Front 38

When the ∆G of a situation is negative or decreasing, describe it.

Back 38

When the ∆G of a situation is negative or decreasing, that situation is exergonic, spontaneous, and no energy is required for it to occur.

Front 39

Cellular respiration is exergonic. Why?

Back 39

In the cellular respiration equation: Cv6Hv12Ov2 + Ov2 → 6 COv2 + Hv2O, the [Cv6Hv12Ov2 + Ov2] part has a high G value, which makes it unstable. The reaction that takes place is exergonic because the G value is going from high to low, indicating that it is going to equilibrium. The reaction is spontaneous, bound to happen, and no energy is required.

Front 40

Describe endergonic reactions.

Back 40

Endergonic reactions absorb free energy from the surrounding material. In these reactions, ∆G increases and it positive. It is a non-spontaneous reaction. It's like pushing a ball up a hill.

Front 41

Once something has reached equilibrium, all ______ ends.

Back 41

Once something has reached equilibrium, all WORK ends.

Front 42

Keeping our molecular selves our of equilibrium ultimately does what since cells which have achieved equilibrium are already dead?

Back 42

Keeping our molecular selves our of equilibrium ultimately keeps us alive.

Front 43

There is a constant flow of energy into and out of our system. Describe what happens, using G value levels, when cellular respiration occurs.

Back 43

When cellular respiration occurs, the input is oxygen and glucose, with high G values, and the output is carbon dioxide & water with low G values.

Front 44

What are the three types of work that's going on inside of a cell?

Back 44

Mechanical - Muscle cells, cilia
Transport work - Pumping across a membrane
Chemical work - Pushing of endergonic reactions for synthesis (anabolic)

Front 45

Describe energy coupling.

Back 45

When an exergonic reaction is used to drive an endergonic reaction. It's seen frequently with ATP.

Front 46

What is described as an exergonic reaction that is used to drive an endergonic reaction. And is frequently seen with ATP.

Back 46

Energy coupling.

Front 47

Exergonic _______ energy, and endergonic _______ energy.

Back 47

Exergonic CREATES energy, and endergonic REQUIRES energy.

Front 48

What are the three components that make up ATP?

Back 48

Ribose sugar, adenine, and a chain of phosphorous.

Front 49

When hydrolyzed, ATP produces how much kcal of energy per mole?

Back 49

When hydrolyzed, ATP produces -7.3 kcal of energy per mole?

Front 50

ATP + Hv2O → ___________

Back 50

ATP + Hv2O → ADP = Pvi

Front 51

What is the most visual way of seeing our body use hydrolysis on ATP?

Back 51

Shivering.

Front 52

When an inorganic phosphorous leaves ATP due to hydrolysis, what occurs next?

Back 52

When an inorganic phosphorous leaves ATP due to hydrolysis, that phosphorus goes through phosphorylation and attaches to another molecule involved in an endergonic reaction, make it more unstable, and movement of that protein or molecule is produced.

Front 53

How does ADP become ATP again?

Back 53

Through an endergonic reaction, it is possible to regenerate ATP.

Front 54

What is the purpose of enzymes?

Back 54

To speed up spontaneous reactions.

Front 55

What is a catalyst?

Back 55

A chemical agent that speeds up a reaction WITHOUT BEING CONSUMED!

Front 56

Any biological or chemistry term ending in "-ase" is most likely what?

Back 56

An enzyme.

Front 57

What is Activation Energy?

Back 57

Energy needed to start a reaction.

Front 58

The most unstable condition a molecule can be in is known as the ______ state.

Back 58

The most unstable condition a molecule can be in is known as the transition state.

Front 59

What usually provides activation energy? Why can't biological systems always use this?

Back 59

Heat usually provides activation energy, but biological systems, such as the human body, cannot rely on this because too much heat causes proteins to denature and will also break bonds that aren't meant to be broken.