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Biology - Metabolic Processes > Introduction to Metabolism > Flashcards

Introduction to Metabolism Flashcards

1
Q

Metabolism=

A

Anabolism + Catabolism

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2
Q

What is anabolism?

A

Build up or create molecules

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3
Q

What is catabolism?

A

Break down of molecules

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4
Q

What is energy?

A

The ability to do work

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5
Q

What is kinetic energy?

A

Energy of movement

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6
Q

What is potential energy?

A

Stored energy

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7
Q

Note about energy

A

Energy can be transformed into other forms of energy

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8
Q

What must food energy be transformed into?

A
  • Mechanical energy
  • Heat energy
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9
Q

1st Law of Thermodynamics

A
  • Total amount of 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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10
Q

1st Law of Thermodynamics used to explain bond energy

A

“Bond energy” is the amount of energy needed to break a bond measured in KJ/mol

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11
Q

When Bonds are formed…

A

Energy is released to the environment (on the product side)

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12
Q

When Bonds Break…

A

Energy is absorbed by the breaking bonds (on the reactant side)

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13
Q

What does the reactant side do?

A

Break bonds to make energy available

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14
Q

What does the product side do

A

Form new bonds

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15
Q

Exothermic Reaction

A
  • Reactions where energy is released
  • Leaves the products with less chemical potential energy compared to the reactants
  • Heat tends to be released
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16
Q

What is △H in exothermic reactions?

A
  • The change in potential energy is negative
  • Heat, light or other energy is usually given off in this type of reaction
17
Q

Exothermic Reaction Example

A
  • Respiration
  • Makes ATP at the expense of a small investment
18
Q

What does △H stand for?

A
  • Change in enthalpy
  • Change in heat
19
Q

What does H stand for?

A

Enthalpy

20
Q

What does Ea stand for?

A

Activation energy

21
Q

Endothermic Reactions

A
  • Reactions where energy is absorbed
  • Leaves the products with more chemical potential energy compared to the reactants
  • Heat tends to be absorbed, leaves surroundings cool
22
Q

What is the △H in endothermic reactions?

A
  • △H is positive
  • The energy of activation is large
23
Q

Endothermic Reaction Example

A
  • Photosynthesis is an endothermic process
24
Q

What type of reaction (endothermic or exothermic) requires less energy?

A
  • Exothermic reactions
  • The overall amount of energy is always lower
25
Q

What type of reaction (endothermic or exothermic) is more common?

A
  • Exothermic reactions
  • They are always considered “spontaneous”
  • These reactions are more likely to occur without too much work
26
Q

What is the most common type of energy to be released or absorbed in potential energy diagrams?

A

Heat

27
Q

Factors that determine whether a chemical reaction will occur

A
  • Energy
  • Entropy
28
Q

What is entropy?

A
  • The measurement of disorder in a system
29
Q

What is △S?

A
  • Entropy
  • Change in order
30
Q

The Second Law of Thermodynamics?

A
  • The Entropy of the universe increases when any change occurs
  • Some energy becomes unuseful with every change
31
Q

Note about entropy

A

The total entropy of a system and its surrounding increases whenever there is any change, such as a chemical reaction

32
Q

What types of molecules have less entropy?

A

Complex, organized molecules

33
Q

What types of molecules have more entropy?

A

Small, gaseous molecules

34
Q

Factors that increase entropy

A
  • Changes in state
  • Changes in concentration
35
Q

Change in state
(Factor that increases entropy)

A
  • When solids react to form liquids or gases
  • When liquids react to form gaseous products
36
Q

Change in concentration
(Factor that increases entropy)

A
  • When the total number of product molecules is greater than the total number of reactant molecules

Biology - Metabolic Processes (14 decks)

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