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Welcome to Sonic and the world of Chemistry.

Topic:
Redox Reactions

First of all, let's just briefly build up on some of the basic
ideas of Redox Reactons.

A Redox Reaction is a reaction between two elements or
compounds in which a change in oxidation states occur.
The two elements or compounds (which we shall refer to as
reactants) experience a change in their oxidation states, as a
result of the reaction.

One of the reactants is oxidised during the reaction, meaning
its oxidation state increases; whereas the other reactant is
reduced, meaning its oxidation state decreases. Both of the
reactants play a part in either oxidising, or reducing the other
reactant. A name must be given to the reactant to describe its
role in the reaction.

The reactant that oxidises the other reactant is called the
"oxidising-agent", because that is its role in the reaction. The
other reactant (which is oxidised) is called the "reducing-
agent" respectively, because it reduces the oxidising agent. In
simple words, the oxidising-agent oxidises the reducing-
agent, and simultaneously the reducing-agent reduces the
oxidising-agent.

Just let all the knowledge sink in for a few seconds

Is that better?

The actual process that works behind a Redox reaction
involves a transfer of electrons. Electrons are extremely
miniscule particles that have a typical negative charge. We've
reduced Sonic in size so that he can examine the electrons
closer, and for your own sake too, so you can get an idea as
to what they may look like.

Consider this example of a straightforward chemical reaction,
which involves a change in oxidation states.

This beaker contains a solution (mixture) that is called
Copper(II)Sulphate.

The Redox reaction is triggered when this nail, composed of
iron in its standard metallic state, is dipped into the
Copper(II)Sulphate solution.

Keep watching the nail closely

The shiny orange/brown substance which
has formed on the iron nail is copper in its
metallic state.

For this redox reaction, what is oxidised
and what is reduced can be identified by
this observation. This means that the
oxidising-agent and the reducing-agent
can therefore be found.

In this solution of Copper(II)Sulfate, Copper is in
abundance as many Copper 2+ ions that co-exist with
many sulfate ions.

Don't worry if you are unfamiliar with what ions are, all
that has to be understood is the changes in oxidation
states. For this reaction, the copper 2+ ions have been
reduced to deposits of copper metal on the iron nail.

This reduction is attested by the fact that copper in its
metallic state has a lower oxidation state than copper in
its ionic form (the copper in solution). Since copper is
reduced in the reaction, it must be the oxidising-agent.
Recall that the oxidising-agent is reduced by the
reducing-agent.

The reducing-agent in the reaction, which is the reactant
that is oxidised by the copper 2+ ions in solution, is the
iron nail itself. The iron nail is steadily oxidised and
releases iron 2+ ions into the solution.

Before commencing this reaction, the aspect of electron
transfer in Redox reactions was briefly hinted at. Negatively
charged electrons like these form part of the atoms in many
elements, and the number of electrons in an atom depends on
the elemental type. In a redox reaction, the reducing-agent
loses some of its electrons to the oxidising-agent. It is this
exchange in electrons which influences the change in the
oxidation states of reactants.

Cu
2+

Fe
2+

Electrons lost by the iron in the nail are
gained by the copper 2+ ions. Some of
the copper 2+ ions are reduced to
copper metal from this acquisition.

After parts of the iron nail lose
electrons, they flow into the solution as
Iron 2+ ions (Fe2+).

Don't worry if you still haven't managed to grasp the
concept of Redox reactions. Hopefully the next
demonstrations with Sonic and Knuckles will help you
understand the important aspects more.

This combination of equipment makes up what is called a galvanic cell. A
galvanic cell is a practical setup in reality, but the setup you see here
should only be considered as an unreal example that works in the same
way as a real galvanic cell.

This combination of equipment makes up what is called a galvanic cell. A
galvanic cell is a practical setup in reality, but the setup you see here
should only be considered as an unreal example that works in the same
way as a real galvanic cell.

In a galvanic cell, a redox reaction takes place. However, instead of the
transfer happening in a standard chemical reaction, the transfer occurs
electrically between the oxidising-agent and the reducing-agent.

In a galvanic cell, a redox reaction takes place. However, instead of the
transfer happening in a standard chemical reaction, the transfer occurs
electrically between the oxidising-agent and the reducing-agent.

What this means is that the electrons from one reactant can be
transferred through this wire to the other reactant, even when the
reactants are not in contact with each other chemically.

What this means is that the electrons from one reactant can be
transferred through this wire to the other reactant, even when the
reactants are not in contact with each other chemically.

The transfer of electrons cannot be seen of course when the external
power supply is turned on, so deductions on which reactant is oxidised
and which is reduced must be concluded by observing the two half-cells.

The transfer of electrons cannot be seen of course when the external
power supply is turned on, so deductions on which reactant is oxidised
and which is reduced must be concluded by observing the two half-cells.

What a half-cell is exactly is the combination of two of the same
reactants, but they differ in oxidation states. One of the reactants is in its
reduced form, whereas the other is in its oxidised form.

What a half-cell is exactly is the combination of two of the same
reactants, but they differ in oxidation states. One of the reactants is in its
reduced form, whereas the other is in its oxidised form.

This can be thought of as the Sonic half-cell. The half-cell beaker contains
the same Sonic reactants which are in different oxidation states.

This can be thought of as the Sonic half-cell. The half-cell beaker contains
the same Sonic reactants which are in different oxidation states.

The Sonic reactant that is in its reduced form is the blue metallic, Super
Sonic electrode. The electrode in a half-cell completes the overall
galvanic cell by sending, or recieving the electrons which are transferred
through the wire.

The Sonic reactant that is in its reduced form is the blue metallic, Super
Sonic electrode. The electrode in a half-cell completes the overall
galvanic cell by sending, or recieving the electrons which are transferred
through the wire.

This faintly blue coloured solution is made up of many Sonic ions. A
Sonic ion has a higher oxidation state than the metallic, Super Sonic
electrode. Thus, the sonic ions in solution are the oxidised form of the
Sonic reactant. Obviously, ions are far too small to be seen by the human
eye, but have been included as a representation anyway.

This faintly blue coloured solution is made up of many Sonic ions. A
Sonic ion has a higher oxidation state than the metallic, Super Sonic
electrode. Thus, the sonic ions in solution are the oxidised form of the
Sonic reactant. Obviously, ions are far too small to be seen by the human
eye, but have been included as a representation anyway.

The reason why this solution is only faintly coloured is because it has
been diluted. This condition will serve as the starting for an important
observational change, which will you will see after the power has been
turned on.

The reason why this solution is only faintly coloured is because it has
been diluted. This condition will serve as the starting for an important
observational change, which will you will see after the power has been
turned on.

This is the Knuckles half-cell. Its setup is practically the same as the
Sonic half-cell, except the reactant type is different.

This is the Knuckles half-cell. Its setup is practically the same as the
Sonic half-cell, except the reactant type is different.

The Knuckles reactant in its reduced form is the Super Knuckles
electrode. The corresponding oxidised form are the Knuckles ions in
solution. This solution is more concentrated than the Sonic solution,
which is why it is more deeply coloured.

The Knuckles reactant in its reduced form is the Super Knuckles
electrode. The corresponding oxidised form are the Knuckles ions in
solution. This solution is more concentrated than the Sonic solution,
which is why it is more deeply coloured.

This green coloured material is called the salt bridge. It is an integral
component of the galvanic cell because it stabilizes the overall transfer of
electrons. Its use will be looked at more after the reaction takes place.

This green coloured material is called the salt bridge. It is an integral
component of the galvanic cell because it stabilizes the overall transfer of
electrons. Its use will be looked at more after the reaction takes place.

For a redox reaction in a galvanic cell, one half-cell will experience
oxidation occuring at its electrode, and the other half-cell will experience
reduction in its solution.

For a redox reaction in a galvanic cell, one half-cell will experience
oxidation occuring at its electrode, and the other half-cell will experience
reduction in its solution.

Observing both of the half-cells when the reaction starts can show what
is reduced and what is oxidised, but this can be predicted beforehand. To
predict which half-cell experiences oxidation, and which experiences
reduction, the half-cell potentials can be looked at.

Observing both of the half-cells when the reaction starts can show what
is reduced and what is oxidised, but this can be predicted beforehand. To
predict which half-cell experiences oxidation, and which experiences
reduction, the half-cell potentials can be looked at.

A half-cell potential indicates the oxidising, and reducing strength of a
particular half-cell. Half-cell potentials are measured in Volts (V). In
Chemistry, the half-cell potentials of many elements and compounds have
been experimentally determined in the past.

A half-cell potential indicates the oxidising, and reducing strength of a
particular half-cell. Half-cell potentials are measured in Volts (V). In
Chemistry, the half-cell potentials of many elements and compounds have
been experimentally determined in the past.

Let's just say the Sonic half-cell has a half-cell potential of -1.20V, and the
Knuckles half-cell a potential of 0.80V

Let's just say the Sonic half-cell has a half-cell potential of -1.20V, and the
Knuckles half-cell a potential of 0.80V

Whether the half-cell contains the oxidising agent, or the reducing agent
depends on its cell pontential. In a galvanic cell setup like this one, the
half-cell with the more positive cell potential is the oxidising agent, and
the half-cell with the more negative cell potential is the reducing agent.

Whether the half-cell contains the oxidising agent, or the reducing agent
depends on its cell pontential. In a galvanic cell setup like this one, the
half-cell with the more positive cell potential is the oxidising agent, and
the half-cell with the more negative cell potential is the reducing agent.

This rule is generally accepted on the official scale of half-cell potentials.
The higher up a half-cell is on the scale, i.e. the more positive it is, the
stronger it is an oxidising agent, and inversely the weaker it is as a
reducing agent.

This rule is generally accepted on the official scale of half-cell potentials.
The higher up a half-cell is on the scale, i.e. the more positive it is, the
stronger it is an oxidising agent, and inversely the weaker it is as a
reducing agent.

This device is a Voltmetre. It measures the overall cell potential of the
reaction, which is the difference between both of the half-cells' potentials.
This will be looked at more closely later. One thing to note, this is a
fictional Voltmetre that gives a digital reading.

This device is a Voltmetre. It measures the overall cell potential of the
reaction, which is the difference between both of the half-cells' potentials.
This will be looked at more closely later. One thing to note, this is a
fictional Voltmetre that gives a digital reading.

Based on what you now know about the half-cell potential scale, and the
potentials of the half-cells in this reaction, can you predict which half-cell
undergoes oxidation, and which one reduction? Remember, the potential
of the Knuckles half-cell is 0.80V, and the Sonic half-cell is -1.20V

Based on what you now know about the half-cell potential scale, and the
potentials of the half-cells in this reaction, can you predict which half-cell
undergoes oxidation, and which one reduction? Remember, the potential
of the Knuckles half-cell is 0.80V, and the Sonic half-cell is -1.20V

Power on

Power on

0.00

0

.

1.04

4.75

4.62

9.62

4.21

2.00

The redox reaction has successfully commenced in a spontaneous
manner. The voltmetre shows that the overall cell potential of this
galvanic cell is 2.00

The redox reaction has successfully commenced in a spontaneous
manner. The voltmetre shows that the overall cell potential of this
galvanic cell is 2.00

Let's go back to the point just before when the reaction started. By
focusing on both of the half-cells in turn during the reaction, it will be
easier to attest any identifications of what is oxidised and what is reduced.

Let's go back to the point just before when the reaction started. By
focusing on both of the half-cells in turn during the reaction, it will be
easier to attest any identifications of what is oxidised and what is reduced.

Firstly, concentrate on what is observed in the Sonic half-cell as the
reaction takes place.

Firstly, concentrate on what is observed in the Sonic half-cell as the
reaction takes place.

From the reaction, the bottom of the Super Sonic electrode has been
steadily dissolving, and is releasing more Sonic ions into the solution,
making the solution slightly more concentrated than it initially was before.

From the reaction, the bottom of the Super Sonic electrode has been
steadily dissolving, and is releasing more Sonic ions into the solution,
making the solution slightly more concentrated than it initially was before.

If you predicted that the Sonic half-cell would undergo oxidation you are
correct. What this observation shows is that the bottom of the Super Sonic
electrode is gradually being oxidised by losing electrons, and the Sonic
ions are the result of this increase in oxidation state.

If you predicted that the Sonic half-cell would undergo oxidation you are
correct. What this observation shows is that the bottom of the Super Sonic
electrode is gradually being oxidised by losing electrons, and the Sonic
ions are the result of this increase in oxidation state.

The electrons that are given up by the Super Sonic electrode travel in this
direction through the wired connection, and at the end are acquired by the
Super Knuckles electrode.

The electrons that are given up by the Super Sonic electrode travel in this
direction through the wired connection, and at the end are acquired by the
Super Knuckles electrode.

For a conventional represenation of a galvanic cell, the half-cell that
experiences oxidation is normally shown on the left, instead of on the
right like how we have shown it. It does not really matter either way.

For a conventional represenation of a galvanic cell, the half-cell that
experiences oxidation is normally shown on the left, instead of on the
right like how we have shown it. It does not really matter either way.

Seeing as the Sonic half-cell undergoes oxidation, the Kunckles half-cell
obviously undergoes reduction because it gains the electrons from the
Sonic half-cell.

Seeing as the Sonic half-cell undergoes oxidation, the Kunckles half-cell
obviously undergoes reduction because it gains the electrons from the
Sonic half-cell.

Although oxidation and reduction happen simultaneously in the reaction,
the Knuckles half-cell here has been shown in its initial state to begin with,
so that its observations under reduction can be focused on.

Although oxidation and reduction happen simultaneously in the reaction,
the Knuckles half-cell here has been shown in its initial state to begin with,
so that its observations under reduction can be focused on.

The observations of this half-cell are clearly the opposite to the
observations of the Sonic half-cell. On the bottom of the Super Knuckles
electrode, a build up of red metal has formed.

The observations of this half-cell are clearly the opposite to the
observations of the Sonic half-cell. On the bottom of the Super Knuckles
electrode, a build up of red metal has formed.

The electrons being received by the Super Knuckles electrode are
distributed into the solution containing Knuckles ions. The Knuckles ions
that do happen to recieve these electrons attain a lower oxidation state, and
are deposited as red metal on the electrode. The resulting solution
becomes less concentrated.

The electrons being received by the Super Knuckles electrode are
distributed into the solution containing Knuckles ions. The Knuckles ions
that do happen to recieve these electrons attain a lower oxidation state, and
are deposited as red metal on the electrode. The resulting solution
becomes less concentrated.

To conclude this demonstration and to summarise, the Sonic half-cell is
oxidised because it has the lower half-cell potential of -1.20V, whereas the
Knuckles half-cell potential is 0.80V so it is reduced.

To conclude this demonstration and to summarise, the Sonic half-cell is
oxidised because it has the lower half-cell potential of -1.20V, whereas the
Knuckles half-cell potential is 0.80V so it is reduced.

The Sonic half-cell potential is more negative, so it is lower down on the
scale making it a stronger reducing-agent than the Knuckles half-cell,
which is inversely the stronger oxidising-agent because it is higher up on
the scale and more positive.

The Sonic half-cell potential is more negative, so it is lower down on the
scale making it a stronger reducing-agent than the Knuckles half-cell,
which is inversely the stronger oxidising-agent because it is higher up on
the scale and more positive.

As previously mentioned, the salt bridge plays a crucial role in stabilising
the oxidation and reduction processes. The salt bridge contains
compounds sustained in a jelly/agar like substance.

As previously mentioned, the salt bridge plays a crucial role in stabilising
the oxidation and reduction processes. The salt bridge contains
compounds sustained in a jelly/agar like substance.

Every Sonic ion in this solution has a positive charge associated with it.
Due to the loss of electrons from the Super Sonic electrode, more of these
ions are formed, thus a more positive charge will start to strengthen in this
half-cell. This build up of positive charge is not favourable because it will
prevent the galvanic cell from working properly.

Every Sonic ion in this solution has a positive charge associated with it.
Due to the loss of electrons from the Super Sonic electrode, more of these
ions are formed, thus a more positive charge will start to strengthen in this
half-cell. This build up of positive charge is not favourable because it will
prevent the galvanic cell from working properly.

A similar problem exists in this half-cell. The Super Knuckles electrode is
recieving more and more electrons from the Super Sonic electrode. Recall
that electrons have a negative charge associated with them.

Since the Super Knuckles electrode is gaining more electrons, it is causing
an unfavourable negative charge to build up, which will also prohibit the
galvanic cell from working properly.

Since the Super Knuckles electrode is gaining more electrons, it is causing
an unfavourable negative charge to build up, which will also prohibit the
galvanic cell from working properly.

The salt bridge balances and stabilizes this build up of unfavourable charge
in both half-cell solutions. Ions of opposite charge to the unfavourable
charge flow from the salt bridge into both half-cell solutions.

The salt bridge balances and stabilizes this build up of unfavourable charge
in both half-cell solutions. Ions of opposite charge to the unfavourable
charge flow from the salt bridge into both half-cell solutions.

Ions that have a negative charge associated with them flow into the
solution composed of Sonic ions, and balance the growing positive charge.
On the other hand, ions with an associated positive charge also flow from
the salt bridge into the Knuckles solution, where they balance the growing
negative charge respectively.

Ions that have a negative charge associated with them flow into the
solution composed of Sonic ions, and balance the growing positive charge.
On the other hand, ions with an associated positive charge also flow from
the salt bridge into the Knuckles solution, where they balance the growing
negative charge respectively.

Well, that wraps up the simple demonstration of a redox reaction in a
galvanic cell. There are many other specifications of this experiment and
that of redox reactions, which were not mentioned in order to keep
simplicity and not a long-winded movie. Read more into the topic of redox
reactions in Chemistry if you're interested in knowing more.

Well, that wraps up the simple demonstration of a redox reaction in a
galvanic cell. There are many other specifications of this experiment and
that of redox reactions, which were not mentioned in order to keep
simplicity and not a long-winded movie. Read more into the topic of redox
reactions in Chemistry if you're interested in knowing more.

Sonic demonstrates the principles of
acid and base reactions.

Knuckles = Acid

Tails = Proton

Sonic = Base

Art&Animation
and sprite editing

Written material

Sprite resources

Ren's Comic zone

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The People's Sprites

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(Hyperlinks)

Game Sprite Archives

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The Shyguy Kingdom

The Shyguy Kingdom

Music (in order of occurence)

Ghouls 'N Ghosts Poltergeist Mix - Binster

STH2 Welcome to the Metropolis - S|r NutS

Sonic3D Blissful Eruption - LeeBro

STH3 Aquatic Pressure - Red Tailed Fox

Special thanks to

All sprite rippers

Friends and family

My 2005 Chemistry teacher, for making
the subject enjoyable.

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Instance Names

"bar"Symbol 38 MovieClip Frame 1Symbol 34 MovieClip

Labels

"loaded"Symbol 38 MovieClip Frame 3




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Created: 9/8 -2019 20:47:29 Last modified: 9/8 -2019 20:47:29 Server time: 14/05 -2024 23:17:01