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Metabolic Processes Flashcards

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Biology 101 flashcards
1
Q

what is metabolism?

A

metabolism = anabolism (build-up) + catabolism (break down)

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2
Q

what is kinetic energy and potential energy?

A

energy of movement and stored energy. one form of energy can be transformed into another form

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3
Q

what is the 1st law of thermodynamics?

A

total energy in the universe is constant. energy cannot be created nor destroyed but may be changed from one form to another

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4
Q

where does all the energy come from?

A

the sun. photosynthesis needs the sun. we eat plants….

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5
Q

what is bond energy?

A

the amount of energy needed to break a bond (kJ/mol)

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6
Q

what happens when bonds are formed and broken?

A

when bonds are formed, energy is released on the product side.

when bonds are broken, energy is absorbed by breaking bonds on the reactant side

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7
Q

explain energy related to the cell respiration reaction? C6H12O6 + 6O2 –> 6CO2 +H2O?

A

the reactant have a higher amount of energy because it is stored in the bonds. the products have a lover energy stored in the bonds

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8
Q

what is an exothermic reaction?

A

an exothermic reaction gives off heat or energy. reactions where energy is released leave the products with less chemical PE compared to reactants. Heat tends to be released, leaving surroundings warm.

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9
Q

what is delta H. What is the difference between an exothermic and endothermic reaction?

A

delta H is the change in PE.

In an exothermic reaction, delta H is negative, and heat, light, or other energy is usually given off in this type of reactions. ex. respiration

In an endothermic reaction, delta H is positive, and the activation energy is large. ex. photosynthesis (energy from light)

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10
Q

what is an endothermic reaction?

A

reactions where energy is absorbed, leaving products with more chemical PE. Heat tends to be absorbed, leaving the surroundings cold.

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11
Q

what is activation energy and what does it tell us?

A

activation energy is the amount of energy needed to see a reaction through

it tells us how fast a reaction is.

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12
Q

what reactions are more common

A

exothermic reactions, they are considered spontaneous (means more likely to occur without assistance)

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13
Q

what is the most common form of energy released or absorbed in PE diagrams?

A

heat

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14
Q

what other factor is used to determine if a reaction will occur spontaneously?

A

entropy is the other factor, which is explained in the Second Law of Thermodynamics.

entropy means disorganization, randomness, chaos, disorder, mess. it is shown as delta S

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15
Q

what is the second law of thermodynamics?

A

the entropy of the universe increases when any change occurs. if it is getting organized somewhere, it is getting messy somewhere else

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16
Q

what is entropy? how does it apply to chemical reaction?

A

entropy is the measurement of disorder in a system.

the total entropy of a system and its surroundings increases whenever there is any change, such as a chemical reaction.

*basically, if entropy seems to decrease in a system, it’s at the expense of increasing somewhere else in the universe

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17
Q

what factors increase entropy within a system?

A

1) changes in state
2) liquids react to form gas products
3) changes in concentration (ie. total # of product molecules is greater than the total number of reactant molecules)

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18
Q

what is the relation between exothermic and entropy?

A

exothermic reactions are spontaneous at all temps. if the reaction leads to an increase in entropy. ex. cell respir.

not spontaneous at high temps if reaction leads to low entropy.`

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19
Q

relation between endothermic and entropy?

A

endothermic reactions are not spontaneous at low temps (only in high) when the reaction leads to an increase in entropy

not spontaneous at all temps, and only proceed given a net input of energy if entropy is decreasing

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20
Q

what does the second law of thermodynamics suggest?

A

every time energy is converted into a different form, then some of the energy becomes unstable and therefore causes an increase in the entropy of the universe

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21
Q

how can 1st and 2nd law of thermodynamics help us?

A

can be used to determine whether physical or chemical changes can occur spontaneously or without a continuous input of energy

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22
Q

spontaneous changes continue….

A

to progress forward on its own once it has begun. eg. lighting a match –> once lit, it continues burning after being struck

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23
Q

non-spontaneous changes….

A

cannout occur without a continual input of energy. eg. boiling a pot of water –> if the heat is removed, boiling stops.

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24
Q

how does the concept of spontaneity help?

A

can help determine how likely it is for certain reactions to take place and is important to biological systems where reactions need to be highly controlled

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25
Q

what is wood burning, food colouring dispersing in water an example of?

A

exothermic changes (favoured) and an increase in entropy (favoured)

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26
Q

what is sweat evaporating from skin or ice melting an example of?

A

endothermic changes (not favoured) and increase in entropy (favoured)

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27
Q

what is water freezing an example of?

A

exothermic changes (favoured) and decrease in entropy (not favoured)

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28
Q

what is plants making glucose or rolling a ball uphill an example of?

A

endothermic changes (not favoured) and decrease in entropy (not favoured)

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29
Q

who is the scientist that described free energy

A

josiah gibbs

30
Q

what is free energy

A

energy that is available to do useful work.

energy that is exchanged leads to a release of energy. some energy is not list but still available to do work in a given system. (ie. recaptured) . eg. toaster… light useless but is used to heat toast

in a living system it is used for chemical and physical work like anabolism, reproduction and movement

31
Q

what is the formula of Gibbs Free energy

A

pressure and volume must be constant

delta G = delta H x TdeltaS

the change in free energy represents the difference in free energy of the final state of the molecules compared to the initial

-ve delta G => free energy of products is less than that of reactants

+ve delta G => free energy of products is more than reactants

32
Q

what does -ve delta G indicate?

A

reaction will occur spontaneously and will give off free energy available to do work. in bio, energy might be used to produce ATP, which can be used to carry out cellular work. Exergonic reaction (when related to G)

33
Q

what does +ve delta G indicate?

A

reaction must gain free energy from another source in order to occur… non-spontaneous. in bio, these types of reactions might consume ATP to move forward. called endergonic reactions when related to G

34
Q

exergonic reaction?

A

a chemical reaction that releases free energy and the products have less free energy than the reactants.

reaction - spontaneous
energy - released (some can be recaptured)
delta G < 0

35
Q

endergonic reaction?

A

a chemical reaction that absorbs free energy and products have more free energy than reactant

reaction - not spontaneous
energy - absorbed
delta G > 0

36
Q

what is free energy used for?

A

allow living organisms to carry out routine processes like cell respiration (Exergonic reaction)

37
Q

what do enzymes do?

A

enzyme don’t change the value of delta G; they only lower the activation energy…. speeding up reversible reactions

38
Q

how do enzymes work to lower activation energy?

A

1) orienting substrates correctly
2) straining substrate bonds
3) providing favorable microenvironments (appropriate polarity charges) to make substrates react/ interact

39
Q

catalysis in the enzyme active system. what happens?

A

the substrate bind to the active site of the enzyme and the active site helps to orient substrates correctly or strain substrate bonds, and/ or provide favourable microenvironments to make substrates react or interact

40
Q

effects on enzymes (Temp., ph, substrate concentrations, and enzyme concentration)

A

enzymes have an optimal pH and temp which it can function

optimal conditions favour the more active shape for the enzyme molecule

enzymes have saturation points if high concentrations of substrate are present.

enzymes don’t saturate if increasingly high concentrations of enzyme are present.

41
Q

all enzymes are happiest at what temperature for human?

A

36 degrees (Aka body temp)

something like a fever can denature the enzymes

42
Q

cell respir. and photosynthesis are…

A

coexistent and are ultimately dependent of each other

chloroplast and mitochondria exchange energy

43
Q

what are metabolic reactions?

A

most metabolic reactions are exothermic or exergonic and rely on enzyme action

44
Q

some processes are endothermic/ endergonic, which require?

A

energy to be driven forward

45
Q

what is energy coupling?

A

when exergonic reaction is used to drive endergonic reactions.

and reactions involved in this type of energy cycling are called coupled reactions

46
Q

coupled reactions?

A

where an energetically favourable reaction (spontaneous) like ATP hydrolysis is able to drive an energetically unfavourable reaction forward (non-spontaneous)

47
Q

what molecule usually helps in biological reaction with coupling?

A

ATP

48
Q

what is ATP?

A

adenosine triphosphate - the primary source of free energy for endothermic reactions to occur in cells

49
Q

why is ATP made of the same building blocks as ATP?

A

it is hard to make these precious materials, so they reused bits and pieces of precious molecules to make other precious molecules

50
Q

what is ATP like?

A

a rechargeable battery

51
Q

how is ATP regenerated?

A

by coupling ATP and it’s related to ADP.

we use the energy from breaking apart the food to rejoin ADP + Pi to make ATP. it will be added with enzymes through phosphorylation.

by living, we hydrolyze ATP.

coupling is used to use ATP and build it back up

52
Q

what does -ase mean?

A

ending indicated enzymes most of the time

53
Q

what is ATPase?

A

an enzyme that hydrolyzes the last phosphate and removes it from ATP when the cell requires Gibbs free energy to do work

54
Q

what is free energy used for?

A

to drive many kinds of cell processes that require work

55
Q

when does something become phosphorylated?

A

the inorganic phosphate attaches to the molecule that is to be energized

56
Q

what is phosphorylation?

A

the addition of inorganic phosphate (Pi) to a molecule. the phosphorylated molecules become more reactive molecules

57
Q

where do ATP exist?

A

ATP molecules exist in all cells, but some cells possess more than others Eg. muscles, nerve cells, sperm cells

58
Q

how is energy transferred from one molecule to another?

A

we must consider the atomic level like to movement of electrons (REDOX rxn)

59
Q

what is reduction oxidation?

A

when biochemical reactions involve the transferring of electrons (H - hydrogen atom) from one molecule to another (Redox rxn)

60
Q

reduction?

A

process of gaining electrons (often in the form of hydrogen atoms)

61
Q

why is hydrogen atom (H) considered an electron?

A

hydrogen has one electron… an electron in bio

62
Q

why is a hydrogen ion (H+) considered a proton?

A

it is positively charged…. a proton in bio

63
Q

oxidation?

A

process of losing electrons (often hydrogen atoms in biological systems)

64
Q

LEO the lion says GER

A

Lose Electrons = Oxidation
Gain Electrons = Reduction

65
Q

reducing agent?

A

the substance that loses electrons (ie becomes oxidized => causes reducation)

66
Q

oxidizing agent?

A

the substance gains electrons (ie. becomes reduced => causes oxidation)

67
Q

what is an example of a redox rxn?

A

burning or combustion is a redox reactions because oxygen steals electrons from fuel; therefore a decreasing the potential energy of the transferred electrons and releasing of free energy.

cell resp. is a slow, controlled redox rxn

68
Q

explain the following reaction:

CH4 + 2 O2 —> CO2 + 2 H2O + energy

A

carbon is the reducing agent
oxygen is oxidizing agent

carbon becomes oxidized because it loses electrons in the form of H+

oxygen gets reduced because it gains electrons in the form of H+

69
Q

coupled redox processess?

A

in some biochemical rxns, a series of redox of rxns occue where electrons are lost, gained, lost, gained, lost, gained,….. until the final product is reduced (gains electrons)

this process is sort of like hot potato where the electron is the potato and each oxidation agent in the series of rxns possesses a

70
Q

if you have unlimited supply on enzymes….

A

no saturation occurs

71
Q

if substrate supply is unlimited…..

A

it will eventually level out (graph) because all the active sites are used

bio (1 decks)

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