Learn to identify a redox reaction and balance its chemical equation using our extensive library of interactive content to learn everything you need to know (and more) about oxidation-reduction reactions!

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General Physics 

Biology

Physics

## INTRODUCTION
Whenever we see a physical or chemical change in any object near us, we automatically conclude that some reaction has occurred. Have you ever wondered which reaction is taking place when we burn a matchstick? 

![role-of-redox-reaction-in-combustion](//images.ctfassets.net/4yflszkpcwkt/7KLDmM7vhDxYRsQoCtPqjg/3245204b36543114efbd6ff6cb148fcd/role-of-redox-reaction-in-combustion.jpg)
[Source](https://studiousguy.com/examples-redox-reactions-everyday-life/)

In real life, combustion is a famous example of redox processes. When we think of combustion, though, we normally think of it as a physical rather than a chemical process. Another significant example of redox reactions is burning organic matter and hydrocarbons in fossil resources. 

The oxygen in the atmosphere reacts with the carbon and hydrogen in the chemical being burnt, forming a bond. Oxygen in the atmosphere is reduced throughout combustion, while the chemical being burned is oxidized. Well now, we have talked a lot about redox reactions! But what exactly is a redox reaction?

### WHAT IS A REDOX REACTION?
All chemical processes in which atoms' oxidation states are altered are referred to as redox (oxidation-reduction) reactions. The loss of electrons—or the rise in oxidation state—by a molecule, atom, or ion is called oxidation. A molecule, atom, or ion gains electrons—or decreases its oxidation state—during reduction. 

Every chemical reaction is represented in the form of equations and it is very important for both scientific and academic purposes that these equations are balanced.

### BALANCING OF REDOX REACTIONS: 
To balance the overall reaction in an alkaline medium, OH ions and water are introduced to half of the reactions. Take the interaction involving potassium permanganate and sodium sulfite, for example: 

MnO₄– + SO₃²⁻ + H₂O → MnO₂ + SO₄²⁻ + OH–

The imbalanced reaction may be split into two halves, each of which represents reduction or oxidation. 

- Reduction: 3 e− + 2 H₂O + MnO₄– → MnO₂ + 4 OH−
- Oxidation: 2 OH− + SO₃²⁻ → SO₄²⁻ + H₂O + 2 e−

### STEPS TO BALANCING A REDOX REACTION:

1. Write the imbalanced ionic equation. 
2. Separate half-reactions should be written for the oxidation and reduction events. 
3. Apart from hydrogen and oxygen, counterbalance the atoms in the half-reactions. 
4. Water molecules are added to the appropriate end of the equation to equalize oxygen atoms. 
5. The hydrogen atoms must then be balanced. 
6. By giving electrons to every other half-reaction, the charges are balanced. 
7. Then, by multiplying it all in one or even both equations by a coefficient, equalize the electrons. 
8. Combine the two half-reactions. The electrons must balance each other out. By inspecting the remaining ingredients, you may find out whether there are any that need to be balanced H2O or H that occur on both sides should be canceled if required. 
9. The hydroxide ions will then be added. 
10. Making water by merging hydrogen and hydroxide ions. 
11. To reach the final equation, eliminate the water molecules over both sides. 

By following the above rules, we reach the final balanced reaction of potassium permanganate and sodium sulfite: 

2 MnO₄– + 3 SO₃²⁻ + H₂O → 2 MnO₂ + 3 SO₄²⁻ + 2 OH–

![balanced reaction of potassium permanganate and sodium sulfite](//images.ctfassets.net/4yflszkpcwkt/3QUnaKlphb5GfFjQmDyomZ/0a7f523da4274bbc4ab905d318478c19/balanced_reaction_of_potassium_permanganate_and_sodium_sulfite.png)

## CONCLUSION: 
- All chemical processes in which atoms' oxidation states are altered are redox reactions. 
- The type of reaction determines which balancing approach should be used. 
- The half-reaction approach for balancing redox is more adaptable, and it works well for ions in aqueous solution interactions.

### FAQs:  

__1. How do you know if a redox reaction is acidic or basic?__

It's an acidic medium if H is present throughout the reaction's balance, and it's a basic media if OH- is present. 

__2. How do you balance redox reactions in acidic and basic mediums?__

- Identify the half-reactions.
- Balance the components that aren't O and H. 
- Use H2O to restore oxygen equilibrium. 
- Insert protons (H) to balance hydrogen. 
- Use electrons to equalize the charge of each equation. 
- Equalize the electrons in the processes by scaling them. 

__3. What is a redox reaction?__

Redox reactions are oxidation-reduction chemical processes in which the oxidation states of the reactants change. 

*We hope you enjoyed studying this lesson and learned something cool about __Balancing redox reactions__! Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our App to experience our fun, VR classrooms - we promise, it makes studying much more fun!* 😎  

## SOURCES: 
1. Balancing Redox Reactions: Half-Reaction Method in Basic Solution. https://www.ck12.org/c/chemistry/balancing-redox-reactions:-half-reaction-method-in-basic-solution/lesson/Half-Reaction-Method-in-Basic-Solution-CHEM/. Accessed 27 Jan, 2022.
2. Balancing Redox Equations. https://courses.lumenlearning.com/introchem/chapter/balancing-redox-equations-2/.  Accessed 27 Jan, 2022.


All chemical processes in which atoms' oxidation states are altered are redox (oxidation-reduction) reactions. 

Balancing Redox Reactions: Half-Reaction Method in Basic Solution Study Guide

## INTRODUCTION
Corrosion is a prevalent occurrence in metal items and surfaces. It occurs when metal reacts with substances in the environment, causing slow disintegration. It erodes the metal, leaving visible holes and altering the chemical composition. While all types of corrosion have this impact, galvanic corrosion is especially troublesome because it can induce different levels of damage between two metals.

![Corrosion](//images.ctfassets.net/4yflszkpcwkt/1f3P0UfY7xPkwHaLCaf96J/ba8e7ff79dc539a2ea3284af85fd51a8/330px-Nandu_River_Iron_Bridge_corrosion_-_03.jpg)
[Source](https://en.wikipedia.org/wiki/Pitting_corrosion)

### WHAT IS GALVANIC CORROSION?

- Galvanic corrosion, also called bimetallic erosion, occurs when two different metals are exposed to an electrolyte. 
- When this happens, one of the metals starts to rust, whereas the other remains safe. 
- The node is the metal that erodes throughout galvanic corrosion. The cathode is a metal that does not rust.
- The Statue of Liberty is a well-known case of galvanic corrosion.

![Statue of Liberty](//images.ctfassets.net/4yflszkpcwkt/1RIBia58iXo02R7kxWd82S/793d936a4b1c039e11efd13c9901f680/f-d_12897d11d2f56a42f2a2ea9ec046e68347494967c1fc7fec9a8e857a_IMAGE_THUMB_POSTCARD_TINY_IMAGE_THUMB_POSTCARD_TINY.1)
[Source](https://www.ck12.org/c/chemistry/corrosion/rwa/Preserving-the-Statue/) 

### STATUE OF LIBERTY CORROSION

- The statue of liberty wasn't green when it was first shipped from France. The color of its copper "skin" was brown. So, how did the hue of the Statue of Liberty change? Corrosion was the cause of the color change. 
- The copper, which is the statue's main component, oxidized over time due to exposure to the air. 
- The copper metal undergoes a series of oxidation-reduction reactions in the environment. 
- Copper metal oxidizes to copper(I) oxide, a reddish-brown color, and subsequently to copper (II) oxide, a blackish-brow color.

2Cu(s)+ ½ O₂(g) ⟶ Cu₂O(s) (red)
Cu₂O(s)+ ½ O₂(g) ⟶ 2CuO(s) (black)

- Coal, frequently heavy in sulfur, was widely burned in the early twentieth century. Sulfur trioxide, carbon dioxide, and water all interacted with the CuO as a consequence.

2CuO(s) + CO₂(g) + H₂O(l) ⟶ Cu₂CO₃(OH)₂(s) (green)
3CuO(s) + 2CO₂(g)+ H₂O(l) ⟶ Cu₂(CO₃)₂ (OH)₂(s) (blue)
4CuO(s) + SO₃(g) + 3H₂O(l) ⟶ Cu₄SO₄(OH)₆(s) (green)

- The striking blue-green patina visible today is due to these three chemicals. Fortunately, the patina formed a protective covering on the exterior, preventing the copper skin from eroding further.

![Statue of Liberty Corrosion](//images.ctfassets.net/4yflszkpcwkt/31C7xak0WaRLzRrM8zn1G1/3e48724990b2cd37553115094c9aca5b/CNX_Chem_17_06_Statue.jpg)
[Source](https://courses.lumenlearning.com/chemistryatomsfirst/chapter/corrosion/)

## CONCLUSION

- The Statue of Liberty is a prominent example of galvanic corrosion.
- In conjunction with the copper skin, the Statue of Liberty's iron framework created a classic galvanic corrosion condition.
- The exterior of the Statue of Liberty is composed of copper, which has oxidized to a shade of green.

### FAQs: 

__1. Is the Statue of Liberty corroded?__

The node is the metal that corrodes throughout galvanic corrosion. The Statue of Liberty is a typical example of galvanic corrosion.

__2. What causes the corrosion of the Statue of Liberty?__

In conjunction with the copper skin, the Statue of Liberty's iron framework created a classic galvanic corrosion condition. When two or more metals are electrically linked in the same electrolyte, this form of deterioration happens.

__3. Will the Statue of Liberty continue to erode?__

Despite all efforts to protect the monument, copper and iron cannot resist the "radical" character of oxygen, and the Statue of Liberty will never be free of corrosion.

__4. Why is the Statue of Liberty green?__

The outside of the Statue of Liberty is composed of copper, which has oxidized to a shade of green.

*We hope you enjoyed studying this lesson and learned something cool about the __Corrosion__! Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our app to experience our fun VR classrooms - we promise it makes studying much more fun!* 😎 

## SOURCES:
1. Preserving the Statue: https://www.ck12.org/c/chemistry/corrosion/rwa/Preserving-the-Statue/ Accessed 27 Feb 2022
2. Corrosion: https://courses.lumenlearning.com/chemistryatomsfirst/chapter/corrosion/ Accessed 27 Feb 2022.


The Statue of Liberty is a well-known case of galvanic corrosion.

Corrosion Study Guide

## INTRODUCTION

A new object made of iron is initially grey, but it will develop a reddish appearance if left in the open for a long time. This is due to the oxidation of iron, also known as rusting. This is a typical example of the redox reaction that we see in our everyday lives. So, are you wondering what a redox reaction is? 🤔

![Corrosion - Redox Reaction](//images.ctfassets.net/4yflszkpcwkt/1vcowPxaj7oJ9myO2N4Fs9/03168915958846f582967b588776b876/GettyImages-548553969-56a134395f9b58b7d0bd00df.jpg)
[Source](https://www.thoughtco.com/how-rust-works-608461)

### REDOX REACTIONS: 

Redox reactions are oxidation-reduction chemical processes in which the oxidation states of the reactant changes. (The degree of oxidation for an atom in a chemical compound is indicated by its oxidation state, which is the imaginary charge that an atom would have if all links to atoms of various elements were entirely ionic.)

- The loss of electrons or a rise in the oxidation state of an atom, an ion, or specific atoms in a molecule is referred to as oxidation.
- The gaining of electrons or a drop in the oxidation state of an atom, an ion, or specific atoms in a molecule is referred to as reduction (a reduction in the oxidation state).
- In a redox reaction, the oxidation and reduction processes always happen simultaneously. 

### IDENTIFYING REDOX REACTION:

Because two separate elements appear as free elements (oxidation number of 0) (zinc and copper in the example below) on one side of the equation and as components of a molecule on the other, single-replacement processes like the one given below, are redox reactions. As a result, the oxidation number of the substance must change.

                   Zn (s) + CuSO₄ (aq) → ZnSO₄ (aq) + Cu (s)

Oxidation half-reaction: Zn → Zn²⁺ + 2e–

Reduction half-reaction: Cu²⁺ + 2e– → Cu

Because elemental oxygen (O2) functions as the oxidizing agent and is reduced, combustion processes are redox reactions.

                       S(s) + O₂ (g) → SO₂ (g)

Because elements are generally changed into compounds, and vice versa, most combination and decomposition processes are redox reactions.

                           2H₂O → 2H₂ + O₂

Here, H+ is oxidized, and O- is reduced.

![Redox-Reaction](//images.ctfassets.net/4yflszkpcwkt/7BdZQMM8WpKypuT5F4ulSb/6d81ccc423b1c1b22859bd6d3f8393d9/Redox-Reaction.jpg)
[Source](https://www.chemistrylearner.com/chemical-reactions/redox-reaction)

### NOW LET’S LOOK AT A FEW REACTIONS THAT ARE NOT REDOX:

Because ions are merely merged without any electron transfer, double-replacement events like those below aren't redox reactions.

               BaCl₂ (aq) + Na₂SO₄ (aq) → BaSO₄ (s)+ 2NaCl(aq)

If you calculate the oxidation numbers on all the ions, you will realize that the oxidation number of all the elements remains unchanged after the reaction.

![Double-Replacement-Reaction](//images.ctfassets.net/4yflszkpcwkt/pGdnBDyqNqhuRSYriSXsm/edb0ad0ddbc56ea517a4161d59d479b5/Double-Replacement-Reaction.jpg)

[Source](https://sciencenotes.org/double-replacement-reaction-definition-and-examples/)

Instead of an electron, a hydrogen ion is transferred in acid-base reactions. Acid base reactions, such as the one beneath, are not redox reactions.

                    CH₃COOH + NH₃ ⇌ CH₃COO– + NH₄+

## CONCLUSION

- Redox reactions are oxidation-reduction chemical processes in which the oxidation states of the reactant changes.
- Decomposition, combustion, Disproportionation, Displacement & Combination Reactions are the 5 major types of redox reactions.
- Because ions are merely recombined without any electron transfer, double-replacement processes are not redox.

### FAQs: 

__1. What is the definition of redox?__

All chemical processes in which atoms' oxidation states are altered are redox (oxidation-reduction) reactions. The loss of electrons—or the rise in oxidation state—by a molecule, atom, or ion is called oxidation. During reduction, a molecule, atom, or ion gains electron—or decreases its oxidation state.

__2. What is an example of redox reaction?__

H₂ + F₂ → 2HF. Following that, the hydrogen and fluorine ions unite to produce hydrogen fluoride. F₂ is an oxidizing agent, whereas H₂ is a reducing agent in this reaction.

__3. What types of reactions are redox reactions?__

Decomposition Reaction, combustion reactions, Disproportionation Reaction, Displacement Reaction & Combination Reactions are the 5 major types of redox reactions. 

*We hope you enjoyed studying this lesson and learned something cool about __Identifying Redox Reactions__! Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our App to experience our fun, VR classrooms - we promise, it makes studying much more fun!* 😎 

## SOURCES:
1. Identifying Redox Reactions. https://www.ck12.org/c/chemistry/identifying-redox-reactions/lesson/Identifying-Reaction-Types-CHEM/. Accessed 7 Feb 2022.
2. Acid-Base Reactions. https://courses.lumenlearning.com/boundless-chemistry/chapter/acid-base-reactions/. Accessed 7 Feb 2022.


Redox reactions are oxidation-reduction chemical processes in which the oxidation states of the reactant changes.

Identifying Redox Reactions Study Guide

# Introduction
A redox reaction is commonly known as a reduction-oxidation process. These reactions often take place in acidic solutions and occasionally occur in solutions that are basic. Balancing a redox reaction in a basic solution can easily be done using the half-reaction method. To understand this in detailed form, let's start with its basics.

## WHAT IS A REDOX REACTION?
- An oxidation-reduction reaction, commonly known as a redox reaction, is any chemical process in which the oxidation number of a participating chemical species changes. 
- An oxidation-reduction reaction is any chemical reaction in which the oxidation number of a molecule, atom, or ion changes as a result of gaining or losing an electron. 
- The creation of hydrogen fluoride is an example of a redox reaction. 
- We should break down the reaction to investigate the oxidation and reduction of reactants.

![redox](//images.ctfassets.net/4yflszkpcwkt/1ZIfHgJ1akLXO42TvWultn/e83501f08f9710640cbd322f2296b9f1/news3_redox.jpg)
[Source](http://1.bp.blogspot.com/-WDcUevXBgzM/TfsHYouxWVI/AAAAAAAAAjs/MOsTe4fdbHo/s1600/news3%20redox.jpg) 

## BALANCING REDOX REACTIONS

Balancing of redox reactions happens in two categories. If the solution is acidic, it is treated differently, and if basic, the process of balancing may vary. 

## BALANCING REDOX REACTION IN BASIC SOLUTION
Balancing redox reactions in a basic solution is slightly more difficult than the balancing redox reactions in an acidic solution. In the basic solution, we add up __H+ and OH-__ in every half-equation. 

## STEPS OF BALANCING 
To balance the redox reaction in a basic medium, OH ions and water are added to half of the reactions. 

Take the reaction between potassium permanganate and sodium sulfite, for example:

__MnO4– + SO32- + H2O → MnO2 +SO42- + OH–__

The imbalanced reaction can be divided into two half-reactions, each representing either reduction or oxidation, just as it can in acidic media.

__Reduction: 3 e− + 2 H2O + MnO4− → MnO2 + 4 OH−__

__Oxidation: 2 OH− + SO32− → SO42− + H2O + 2 e−__

When the number of electrons in the two half-reactions are balanced, the result is:

__6 e− + 4 H2O + 2 MnO4− → 2 MnO2 + 8 OH−__

__6 OH− + 3 SO32− → 3 SO42− + 3 H2O + 6 e−__

The balanced equation is obtained by adding these two half-reactions together:

__2 MnO4– + 3 SO32- + H2O → 2 MnO2 + 3 SO42- + 2 OH–__

# SUMMARY 
- The loss of electrons due to the transfer of electrons in the oxidation state is called oxidation. In contrast, the gain of electrons in the oxidation state is said to be the reduction process. 
- The electron acceptor always undergoes a reduction process called an oxidizing agent. The electron donor undergoes an oxidation process in a redox reaction called a reducing agent.
-  We add up OH- ions to the equation when the redox reaction is in a basic solution. 
- The half reaction method is more versatile if no acid or bases are present. 

## FAQs

__1. How do you balance a redox reaction by the half-reaction method?__

1. First, split up the equation into two halves.
2. Balance each half-equation for its charge and mass.
3. Evaluate the number of electrons and then combine both equations.

__2. How do you balance redox reactions by the ion-electron method in a basic medium?__

- Divide the reaction into two halves to balance in basic solution.
- Balance each reaction with O- rather than H+ in H2O
- Balance the hydrogen atom with H+
- Add OH- ions on both sides to neutralize the equation.
- Combine OH- and H+ to create H2O
- Simplify the equation 
- Combine both half equations. 

__3. How do you balance half equations?__

Balancing half equations can be done by balancing the atoms separately. The number of electrons lost is equalized to the number of electrons gained. 

__4. What is step 1 in the ion-electron method for balancing redox reactions?__

Writing down the unbalanced equations and then separating the reactions into two halves as per their undergoing process. 

*We hope you enjoyed studying this lesson and learned something cool about __Redox Reaction In Basic Solutions!__ Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our app to experience our fun VR classrooms - we promise it makes studying much more fun!😎*

## REFERENCES 
1. Balance Redox Reaction in basic Solution: https://socratic.org/questions/how-do-you-balance-redox-reactions-in-basic-solution. Accessed 3rd March 2022. 
2. How to Balance Redox Reactions: https://blog.cambridgecoaching.com/how-to-balance-redox-reactions-in-acidic-and-basic-solutions. Accessed 3rd March 2022.
3. Balancing Redox Reactions: https://flexbooks.ck12.org/cbook/ck-12-chemistry-flexbook-2.0/section/22.11/primary/lesson/half-reaction-method-in-basic-solution-chem/. Accessed 3rd March 2022.
4. Balancing Redox Equations: https://courses.lumenlearning.com/introchem/chapter/balancing-redox-equations-2/. Accessed 3rd March 2022.
5. Balancing Redox Reactions: https://www.ck12.org/c/chemistry/balancing-redox-reactions%3A-half-reaction-method-in-basic-solution/lesson/Half-Reaction-Method-in-Basic-Solution-CHEM/.Accessed 3rd March 2022.


A redox reaction is also known as a reduction-oxidation reaction. Often, these reactions take place in acidic solutions, although sometimes they can also occur in basic solutions.


Redox Reaction In Basic Solution Study Guide

# Introduction
- Redox reaction or oxidation-reduction reaction includes the transfer of particles during a chemical reaction. 
- Balancing redox reaction includes several methods, such as half-reaction, where one is done through oxidation, and another half represents the reduction. And then, the half-reactions are added together, resulting in the entire balanced equation. 

## WHAT IS REDOX REACTION BALANCING?
Redox equations are said to be more complex than the standard reaction. 
This balancing includes a half-reaction table and is often split up into two parts to get one net balanced equation. 

- The loss of electrons due to the transfer of electrons in the given reactant and the increase of the reactant in the oxidation state is called oxidation. 
- In contrast, the gain of electrons and the decrease of reactants in the oxidation state is said to be the reduction process. 
- The accepting electrons always undergoes a reduction in redox reactions and are thus called oxidizing agents. 
- The donor of the electron undergoing an oxidation process in a redox reaction is called a reducing agent. 

## HOW TO BALANCE A REDOX REACTION (HALF-REACTION METHOD)?
- We divide the equation into two half in this procedure. 
- After that, we split the two portions of the reaction and balance them independently. 
- Finally, we combine them to get a balanced equation. 

We'll use an example to show the procedures involved in balancing redox reactions using the half-reaction approach.

In an acidic solution, for example, Fe2+ ions are transformed into Fe3+ ions by dichromate ions. 
In the process, dichromate ions (Cr2O72–) are reduced to Cr3+ ions. 
The redox process described above must be balanced. 
The following are the steps to balancing this equation.

__Step 1:__ First, we must express the equation in its simple ionic form.

__Fe2+9aq) + Cr2O72-(aq) -> Fe3+9aq) + Cr3+(aq)__

__Step 2:__ Split the equation into two halves, one for oxidation and one for reduction.

__Fe2+(aq) -> Fe3+9aq)  Oxidation Half__

__Cr2O72-(aq) -> Cr3+(aq)  Reduction Half__

__Step 3:__ We shall balance the atoms present in each half of the reaction excluding O and H atoms in the third phase of balancing redox reactions using the __half-reaction method__.

- The oxidation phase of the reaction in terms of Fe atoms is already balanced in the example question. 
- As a result, we'll only balance the reaction's reduction phase. 
- To balance the Chromium atoms in this example, we shall multiply Cr3+ by 2.

__Cr2O72-(aq) -> 2Cr3+(aq)__

__Step 4:__ We know that the reaction occurs in an acidic environment. 
As a result, we must add water molecules (H2O) to balance the O atoms in the equation, as well as H+ to balance the H atoms. 

The equation is now: __Cr2O72-(aq) + 14H+(aq) -> 2Cr3+(aq) + 7H2O (1)__

__Step 5:__ Now we must balance the charges in both halves of the reaction. 

- As a result, we must multiply the appropriate number by one or both halves of the reaction to equalize the number of electrons. 
- The oxidation portion of the reaction must be balanced.

__Fe2+(aq) -> Fe3+(aq) + e-__

- There are 12 positive charges on the left side of the equation for the reduction half and 6 positive charges on the right side of the equation for the reduction half. 
- To balance the reduction half, we must add 6 extra electrons to the left side of the equation.

__Cr2O72-(aq) + 14H+(aq) + 6e_ -> 2cr3+(aq) + 7H2O (1)__

- We'll double 6 in the oxidation half-reaction to equalize the electrons in the two parts of the reaction. As a result,

__Step 6:__ To complete the total reactions, the two halves of the equations are joined together. 

- Cancel the electrons on both sides after adding the two reaction halves. The net ionic equation is as follows:

__6Fe2+(aq) + Cr2O72-(aq) + 14H+(aq) -> 6Fe3+(aq) + 2Cr3+(aq) + 7H2O(1)__

__Step 7:__ Finally, we must ensure that both sides of the equation have the same type, quantity, and charges. Furthermore, in terms of atoms and charges, the equation is perfectly balanced.

In the case of a basic solution, we must balance the atoms in the same way that we would in an acidic solution. Then, in both half of the equation, an equal number of OH– ions are added for each H+ ion. When H+ and OH– ions are present on the same side of the equation, the ions must be combined to form H2O.

# SUMMARY 
- Any chemical reaction in which oxidation and reduction both processes take place simultaneously is know as a redox reaction.
- The half-reaction method is a way to balance redox reactions. It involves breaking the overall equation down into an oxidation part and a reduction part. 

## FAQ’s 

__1. What are 2 ways of balancing redox reactions?__

Two ways are:
- Oxidation number method 
- Half reaction method

__2. How do you balance redox reactions Class 11?__

- To balance the redox reaction, first check the nature of the reaction. 
- If the reaction is of acidic nature, balance the charges by adding H ions. 
- For basic nature, add OH- ions. 
- Then, balance the deficient side of oxygen atoms by adding the required molecules. This way, you get balanced redox equations.

__3. What is Ncert Class 10 redox?__

A redox reaction is a reaction in which one reactant undergoes a reduction process, and the other gets oxidized during the reaction. It is termed a reduction-oxidation reaction. 

__4. How do you balance redox reactions fast?__

- Divide the equation into two halves 
- Balance each half-equation for mass and charge
- Equalize the electron numbers and then mix both the equations.

*We hope you enjoyed studying this lesson and learned something cool about __Balancing Redox Reactions!__ Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our app to experience our fun VR classrooms - we promise it makes studying much more fun!😎*

## Sources 

1. Balancing Redox Reaction: https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Supplemental_Modules_(Analytical_Chemistry)/Electrochemistry/Redox_Chemistry/Balancing_Redox_reactions.Accessed 28 Feb 2022. 
2. Balancing Redox Reaction: https://courses.lumenlearning.com/introchem/chapter/balancing-redox-equations-2/. Accessed 28 Feb 2022.
3. Redox Reactions: https://byjus.com/jee/redox-reactions/. Accessed 28 Feb 2022.
4. Balancing Redox Reaction: https://opentextbc.ca/introductorychemistry/chapter/balancing-redox-reactions/. Accessed 28 Feb 2022.

Balancing redox reactions includes oxidation and reduction processes that take place simultaneously. 

Balancing Redox Reactions Study Guide

# Introduction
Have you seen that there is a layer of rust forming on the surface of any of the metal rods around you? Most often metal surfaces are painted, or a coating is applied to decrease rusting. Have you ever wondered why? It is because the metals get oxidized and develop rust when left untreated. Let’s learn about oxidation in this guide. 

![number](//images.ctfassets.net/4yflszkpcwkt/4HEoLc3ZwdhWgAiDVGDg2f/c98959fb73b709351917dde08be1bda7/common-most-stable-oxidation-number-state.png)
[Source](https://www.priyamstudycentre.com/2019/05/oxidation-number-of-elements.html)

## RULES FOR ASSIGNING OXIDATION NUMBERS
Here are some of the rules for assigning oxidation numbers. They are as follows:

1. The pattern is that the cation is always written first in a formula, which is then followed by the anion. 

2. The oxidation number of any free element always remains 0. 

3. The oxidation number in the case of a monatomic ion is always equal to the value of the charge of the ion. For instance, the oxidation number of Na3- is 3-.

4. The expected oxidation number of hydrogen is plus 1. The oxidation number of hydrogen remains -1 in compounds, including elements that have less electronegativity than hydrogen, as in NaH.

5. The oxidation number of oxygen in the case of compounds is typically -2. Anomalies include OF2 because F turns out to be more electronegative than O, and BaO2, due to the construction of the peroxide ion, which can be expressed as (O-O)2-.

6. The oxidation number of elements in Group IA in a compound is +1.

7. The oxidation number of elements present in Group IIA in a compound is +2.

8. The oxidation number of elements present in Group VIIA in a compound is -1, except for the case when that element is conjoined with one having a higher value of electronegativity. The oxidation number of Cl turns out to be -1 in HCl, but this number becomes +1 in HOCl.

9. The sum of the value of oxidation numbers of all the present atoms in any neutral compound is 0.

10. Also, the sum of the value oxidation numbers in any given polyatomic ion is always equal to the value of the charge of the ion. For instance, the sum of the value of oxidation numbers for SO42- is -2.

![oxidation](//images.ctfassets.net/4yflszkpcwkt/1V1P4ZHyRYPpfvyK54B0xe/757e4aa3f590b29d702fb4fcc9ba296e/Vq10aqY.png)
[Source](https://www.brainkart.com/article/Oxidation-Number_34651/)

## FAQs

__1. What are the rules related to assigning oxidation numbers?__

If you want to know how to assign oxidation numbers, you need to know some rules of oxidation numbers. Some of them are:
- The pattern is that the cation is expressed first in a formula, and then the anion is written.
- The oxidation number of any given free element always has to be 0.
- The oxidation number of a monatomic ion equals the value of the charge of the ion.

__2. What is the easiest way to determine oxidation numbers?__

The easiest way to determine the oxidation number is by dividing the total charge by two.

__3. How do you find the oxidizing agent?__

To find an oxidizing agent, you need to check the oxidation number of an atom that is before and after the chemical reaction. If the oxidation number is higher in the product, then it has lost electrons, and the substance went through oxidization. If the oxidation number is less, then it has gained electrons and was reduced.

*We hope you enjoyed studying this lesson and learned something cool about __Rules for Oxidation Numbers!__ Join our Discord community to get any questions you may have answered and to engage with other students just like you! Don't forget to download our App to experience our fun VR classrooms - we promise it makes studying much more fun!😎* 

## SOURCES
1. Assigning Oxidation Numbers: https://www.ck12.org/c/chemistry/assigning-oxidation-numbers/lesson/Assigning-Oxidation-Numbers-CHEM/. Accessed 7th March 2022.
2. Rules for Assigning Oxidation Numbers: https://www.toppr.com/ask/question/write-the-rules-for-assigning-oxidation-number/. Accessed 7th March 2022.

The oxidation number is defined as the total number of electrons an atom gains or losses in a chemical reaction to form a bond. It follows a set of oxidation number rules.


Rules for Oxidation Numbers Study Guide

## INTRODUCTION 

Did you ever wonder about the cause of rusting? It happens due to weathering. What is it? It is the breakdown or dissolution of rocks and minerals on the Earth's surface. There are three types of weathering. These are- mechanical, chemical, and lastly, biological.

### WHAT IS MECHANICAL WEATHERING?

Mechanical weathering happens due to external factors like rain, thawing, wind, freezing, sand, and other natural forces that hold power to alter rock physically. 

### WHAT IS BIOLOGICAL WEATHERING? 

Plants and animals cause biological weathering as they tend to grow, burrow, and nest. 
And now, the core topic of this discussion is chemical weathering, of which the Statue of Liberty chemical weathering is a prime example of this.

### THE DIFFERENT TYPES OF CHEMICAL WEATHERING 

![Examples-of-chemical-weathering](//images.ctfassets.net/4yflszkpcwkt/4q1S8R83VBpR5hLUdmkDh4/258013a2bfeefec454e976c6678b899b/examples-of-chemical-weathering-607608_FINAL-54f8c4d63ed94e0eab454dc5e96cabff.png)
[Source](https://www.thoughtco.com/examples-of-chemical-weathering-607608)

### CHEMICAL WEATHERING DUE TO WATER

Water not only causes chemical weathering but mechanical too. The major difference? Mechanical weathering due to water happens when it drips or flows over rocks for a prolonged period; an example would be the Grand Canyon. Chemical weathering occurs when water dissolves minerals in rocks, resulting in new compounds. This is also known as hydrolysis. 

An example would be when water comes in the proximity of granite. Feldspar crystals present inside the rock react chemically, forming clay minerals. Water also reacts with calcites in caves and causes dissolving. Calcite in dripping water is known to build up over several years and create stalagmites and stalactites.

### OXYGEN IS THE REASON BEHIND CHEMICAL WEATHERING

Oxygen is a reactive element, and it reacts with rocks as per a phenomenon known as oxidation. Rust formation is a prime example of chemical weathering due to oxygen. Observe the Statue of Liberty before rusting and after rusting, and you will know the difference. In this weathering, oxygen reacts with iron, forming iron oxide. Rust is the reason behind the change in rock color, and iron oxide makes it more fragile. 

![Chemical Weathering From Oxygen](//images.ctfassets.net/4yflszkpcwkt/6cHzCpjFg2iEDti5B8YgMl/48f81ba1e19fcf88725395bb1aecf03e/ArizonaVermilionCliffsNationalMonument-5c6a3133c9e77c000119fb52.jpg)
[Source](https://www.thoughtco.com/examples-of-chemical-weathering-607608)

### CHEMICAL WEATHERING DUE TO ACID 

When minerals and rocks get altered due to hydrolysis, they could produce acid. Acid is also produced when water undergoes reactions in the atmosphere, and acid rain is one example. When carbon dioxide mixes with water, a weak acid is produced. Calcite often dissolves due to this type of chemical weathering. 

### CHEMICAL WEATHERING DUE TO LIVING ORGANISMS 

Here, living organisms grow, nest, and burrow; therefore, performing chemical reactions to acquire minerals from rocks and soils. 

### HOW WAS THE STATUE OF LIBERTY BEFORE CORROSION? 
You have seen the Statue of Liberty in the picture and maybe in real life too, and by now, its blue-green color is an iconic combination. However, it was not always blue-green; when unveiled in 1886, the Statue of Liberty was a shiny brown color before turning green. However, the color changed because the outer layer of the statue is covered in hundreds of thin copper sheets, which reacted with air to form patina or verdigris, which protects the underlying metal. The three main components that form the patina would be:

- Cu₄SO₄(OH)₆ (green)
- Cu₂CO₃(OH)₂ (green)
- Cu₃(CO₃)₂(OH)₂ (blue)

## CONCLUSION:  

1. Weathering is the breakdown or dissolving of rocks and minerals on the Earth's surface.
2. Weathering can be divided into mechanical, chemical, and biological. 
3. Chemical weathering happens when rocks undergo a complete chemical reaction resulting in new minerals.

### FAQs: 

__1. Does the Statue of Liberty corrode?__

Statue Of Liberty is an example of galvanic corrosion. 

__2. What happened to the copper on the Statue Of Liberty?__

Copper reacts with air to form patina or verdigris, protecting the underlying metal.

*We hope you enjoyed studying this lesson and learned something cool about Different Types Of Chemical Weathering! Join our Discord community to get any questions you may have answered and engage with other students like you! Don't forget to download our app to experience our fun VR classrooms - we promise it makes studying much more fun!* 😎

## SOURCES:
1. Examples of Chemical Weathering: https://www.thoughtco.com/examples-of-chemical-weathering-607608. Accessed 28 Feb 2022.
2. Why Statue of Liberty is Green? https://www.thoughtco.com/why-statue-of-liberty-is-green-4114936. Accessed 28 Feb 2022.
3. Preserving the Statue: https://www.ck12.org/c/chemistry/direct-redox-reactions/rwa/Preserving-the-Statue/. Accessed 28 Feb 2022.


Chemical weathering is when rocks undergo chemical reactions to form an entirely different mineral. An example would be the Statue of Liberty rusting. 