chemistry-class-11-unit-08-chapter-01-redox-reactions-l-1-3-muwmhlnfstu

### <Success style="font-size:25px"> Redox Reactions L-1 </Success>
### <primary style="font-size:24px"> Redox reactions </primary>
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* $Fe_2$ $O_3$ $\leftarrow$ Fe +  $O_2$
* Oxidation - removal $e^-$
* Reduction - add $e^-$
* Increase in oxidation state
 - Fe $\xrightarrow {-3e^-}$ $Fe^{3+}$ - ox
* Decrease in oxidation state
 - O $\xrightarrow {+2e^-}$ $O^{2-}$ - Red
* Common fire 'c'
 - $KMnO_4$ + $\underbrace{H_2O_2}_{\text{EtOH}}$ $\rightarrow$ $MnO_2$ + $0_2$ + $H_2O$ + $HO^-$
* Oxidation agent
 - $KMnO_4$ Powder

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<footer style = "font-size: 18px">Redox reactions $\rightarrow$ Redox reactions $\rightarrow$ <span style = "color:blue"> Redox reactions </span> $\rightarrow$ Redox reactions $\rightarrow$ Redox reactions </footer>

### <Success style="font-size:25px"> Redox Reactions L-1 </Success>
### <primary style="font-size:24px"> Redox reactions </primary>
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* Rust is an iron oxide, usually red and formed by the redox reaction of iron and oxygen in the presence of water or moisture rust consists of hydrated iron(III) oxides

* $\mathrm{O}_2+4 \mathrm{e}^{-}+2 \mathrm{H}_2 \mathrm{O} \rightarrow 4 \mathrm{HO}^{-}$

* $\mathrm{Fe} \rightarrow \mathrm{Fe}^{2+}+2 \mathrm{e}^{-}$

* $4 \mathrm{Fe}^{2+}+\mathrm{O}_2 \rightarrow 4 \mathrm{Fe}^{3+}+2 \mathrm{O}^{2-}$

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### <Success style="font-size:25px"> Redox Reactions L-1 </Success>
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* $Fe_2O_3 .nH_2O$- red

* $O_2(O=O)\xrightarrow {e^-} O_2^{-} \xrightarrow {e^-} O_2^{2-} \rightarrow HO^-$

* Least electronegative element - Cs 0.79

* Most electronegative element - F 3.98

* $A+H_2O \rightarrow Cl^-+H_3O^+$

* $A = H^{+1}Cl^{-1}$

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### <Success style="font-size:25px"> Redox Reactions L-1 </Success>
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* Linas pauling scale of electronegativity and chemical bonds

|   Difference in electronegativity         |   Corresponding type of bond      |
| ----------------------------------------- | --------------------------------- |
| 0-0.5                                     | Non-polar covalent                |
| 0.6-1.9                                   | Polar covalent                    |
| 2.0 and above                             | Ionic                             |

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### <Success style="font-size:25px"> Redox Reactions L-1 </Success>
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* Dependence of bond type on two parameters electronegativity difference $(\Delta \chi)$ and average electronegativity ( $\chi$ av)

* Ionic character is governed by the partial charges of the bonded atoms, and metallic character by the HOMO LUMO band gap

* The nature of the dependence allows rationalization of the variation of bond type

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### <Success style="font-size:25px"> Redox Reactions L-1 </Success>
### <primary style="font-size:24px"> Redox reactions </primary>
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- **Interhalogen compouds**
 - $Cl^{1+}F^{1-}$
 - $Br^{1+}Cl^{1-}$

- **Water oxidation**
 - $2H_2O \rightarrow O_2+4H+4e$ Oxidation
 - $4H+4e \rightarrow 2H_2$ Reduction
 - $2H_2O \rightarrow 2H_2+O_2$ Total

- This process occurs naturally in photosystem II of plants to provide protons and electrons for the photosynthesis process and release oxygen to the atmosphere

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### <Success style="font-size:25px"> Redox Reactions L-1 </Success>
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* Materials that have the ability to oxidize other substances are said to be oxidative or oxidizing and are known as oxidizing agents, oxidants, or oxidizers It removes electrons from another substance, and is thus itself reduced

* Oxidants are usually chemical substances with elements in high oxidation states $\left(\mathrm{MnO}_4^{-}, \mathrm{CrO}_3, \mathrm{Cr}_2 \mathrm{O}_7{ }^{2-}, \mathrm{OsO}_4\right)$, or else highly electronegative elements $\left(\mathrm{O}_2, \mathrm{~F}_2, \mathrm{Cl}_2, \mathrm{Br}_2\right)$ that can gain extra electrons by oxidizing another substance

* Reductants - Electropositive metals like $\mathrm{Li}, \mathrm{Na}, \mathrm{Mg}, \mathrm{Fe}, \mathrm{Zn}$, and $\mathrm{Al}$ Can donate electrons readily

* Hydride transfer reagents, such as $\mathrm{NaBH}_4$ and $\mathrm{LiAlH}_4$, are used in organic chemistry

* $\mathrm{H}_2$ gas with a palladium, platinum, or nickel catalyst

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### <Success style="font-size:25px"> Redox Reactions L-1 </Success>
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* The term corrosion refers to the electrochemical oxidation of metals in reaction with an oxidant such as oxygen rusting, the formation of iron oxides, is a well-known example of electrochemical corrosion

* $4 \mathrm{Fe}+3 \mathrm{O}_2 \rightarrow 2 \mathrm{Fe}_2 \mathrm{O}_3$

* Corrosion is a natural process, and it converts a refined metal to a more chemically-stable form, such as its oxide, hydroxide, or sulfide

* $\Delta$ Gradual destruction of materials (usually metals) by chemical and/or electrochemical reaction with their environment

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