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Energy And Metabolism - SBI4U1 > Energy And Metabolism > Flashcards

Energy And Metabolism Flashcards

1
Q

What are catabolic reactions?

A

The breakdown of of complex and large substances/molecules

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2
Q

Examples of catabolic reactions

A
  • Breakdown of starch into glucose

- glucose into carbon dioxide and water

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3
Q

What are anabolic reactions?

A

Cells building complex substances from simpler subunits

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4
Q

Examples of anabolic reactions

A

Building of DNA from nucleotides

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5
Q

Define work

A

Happens when one object applies a force on another object and changes its position or state of motion

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6
Q

Examples of work

A
  • work/energy comes from your muscles (stored potential energy)
  • muscle movement
  • thinking a thought
  • heart contractions
  • active transport
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7
Q

Define kinetic energy

A

Energy possessed by moving objects possess kinetic energy

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8
Q

Define potential energy and explain the 4 types

A

Stored energy (4 types):

  1. Chemical (stored in muscles)
  2. Electrical (batteries)
  3. Gravitational (objects at a height)
  4. Elastic (rubber band or springs)
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9
Q

First Law of Thermodynamics?

A

The total amount of energy in the universe is constant

* energy cannot be created or destroyed, but can convert to other forms (to heat, sound energy etc.)

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10
Q

What is Bond Energy?

A

The measure of stability of a bond:

  • the energy required to break a bond
  • the energy released when bonds form
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11
Q

Sum of anabolic and catabolic reactions?

A

Metabolism

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12
Q

Describe the steps of energy conversion for a diver that is about to jump off a platform

A
  1. Starts with potential energy - due to the force of gravity and distance between him and the Earth
  2. He did not always have potential energy, he gained it from the work in his muscles lifting him to the present height
  3. As he dives, he gains kinetic energy as his speed increases, and lose potential energy as the distance between him and the water decreases
  4. Potential is converted to kinetic when he falls
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13
Q

What is activation energy?

A

The amount of energy needed to break the reactants bonds

  • it is equal to the difference between the potential energy level of transition state and the potential energy of the reactants
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14
Q

Energy absorbed when:

A

When reactant bonds break

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15
Q

Energy released when:

A

When product bonds form

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16
Q

What is the transition state of reactants?

A

It is a temporary condition in which:

  • bonds within reactants are breaking
  • bonds between products are forming
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17
Q

What happens when product bonds form?

A

Energy is released:

  • if bonds in products are more stable than those in reactants -> more energy is released during bond formation
  • this results in a net energy output (exothermic)
18
Q

Exothermic reaction

A

This reaction has a net release of energy (heat)

  • change in ENTHALPY between reactants and products yields a release of heat (negative numbers)
19
Q

Endothermic reaction

A

A net gain/absorption of energy (heat)

  • the amount of energy absorbed when breaking reactant bonds is greater than the energy released when forming product bonds
20
Q

What is the overall change in energy called? And what is the symbol?

A

Heat or enthalpy of reactions (symbol H)

H is (+) for endothermic reactions
H is (-) for exothermic reactions
21
Q

Examples of endothermic

A

Beaker experiment: beakers heat is taken by the chemicals that inside, wood is an insulator so it does not take heat

22
Q

Examples of exothermic

A

Anything that burns (gives off heat)

- burning wood

23
Q

What is the NET

A

change in enthalpy

24
Q

Enthalpy of reactants

A

The amount of energy required to break all reactant bonds

25
Q

Enthalpy of products

A

The amount of energy released after all product bonds form

26
Q

What is the Second Law of Thermodynamics

A
  • During every energy conversion, there is always some energy wasted as heat
  • This causes entropy of the universe to always increase
  • not all chemical is turned into potential
27
Q

Entropy

A

The measure of the disorder in a system

Ex: messy room, shuffling playing cards

Decrease disorder by organizing

28
Q

If a student organizes their room, does this break the 2nd law?

A

No, because entropy is still increasing in our body instead of the room

(Entropy of a person increases by a greater amount due to work being done to organize room)

29
Q

Entropy: liquid to solid

A

Entropy drops

30
Q

Entropy: gas to liquid

A

Entropy drops

31
Q

Entropy: liquid to gas

A

Entropy increases

32
Q

of molecules to entropy relationship

A

As # of molecules increase, the more disorder (entropy) (s-)

33
Q 
H +
H -
S +
S -
K
A 
(H) + is heat absorbed
(H) - is heat released
(S) + increase in entropy
(S) - decrease in entropy
(K) temperature
34
Q

Spontaneous change/reaction and examples

A

(Exergonic)
- a reaction where once started, will continue on its own and releases useful energy (free energy)

Ex: burning paper

35
Q

Non-spontaneous change and examples

A

(Endergonic)
- a reaction that constantly needs input of energy for completion

Ex: boiling water/cooking anything

36
Q

Free Energy (Gibb’s)

A

Energy in the body that is able to perform useful work in the body

  • the useful work requires an input of free energy
  • comes from the digestion of food

(Thinking a thought, breathing, etc)

37
Q

How does food convert to ATP?

A

Food —> free energy (ATP)
(chemical (digest) + heat (waste)
potential) (energy
conversion)

38
Q

Negative free energy (G)

A

Indicates the free energy of the products is less than the free energy of the reactants

  • energy released from this can be used to do work in other reactions

OCCUR SPONTANEOUSLY

39
Q

Positive free energy (G)

A

Indicates the products have more free energy than reactants

OCCUR NON-SPONTANEOUSLY

40
Q

Exergonic reactions

A
  • can do work because they act as a source of free energy
  • releases free energy
  • (G) value is negative
    (products contain less free energy)
41
Q

Endergonic reactions

A
  • products contain more free energy than reactants
  • (G) value is positive
  • reactants must ABSORB free energy from surroundings to transform into the products

Ex: conversion of carbon dioxide and water into glucose and oxygen gas
(This requires an input of free energy)

Energy And Metabolism - SBI4U1 (2 decks)

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