SHOBHIT NIRWAN's
DESIGNED
REDOX REACTIONS
NEW NOTES FOR CLASS 11 2022 EXAMS
, OVERVIEW OF THE CHAPTER
1. Uses of redox reaction.
2. Classical idea of redox reactions – oxidation and reduction reaction.
3. Redox reactions in terms of electron transfer reactions.
4. Competitive electron transfer reactions.
5. Oxidation number.
6. Types of Redox Reactions:
(i) Combination reactions
(ii) Decomposition reactions
(iii) Displacement reactions:
Metal displacement and non – metal displacement
7. Balancing of redox reactions:
(i) Oxidation number method
(ii) Half reaction method
8. Redox reactions as the basis for titrations.
9. Limitations of concept of oxidation number.
10. Redox Reactions & electrode process.
, 1. Uses of Redox Reaction:
a. Extensive use in pharmaceutical, biological, industrial, metallurgical and
agricultural areas.
b. Burning of different types of fuels for obtaining energy.
c. In electrochemical process for extraction of highly reactive metals and non-
metals.
d. Manufacturing of chemical compounds like caustic soda.
e. In dry & wet batteries.
f. Corrosion of metals.
g. Environment issues like use of hydrogen economy (use of liquid hydrogen as
fuel) & development of ‘ozone hole’ are under redox phenomenon)
2.Classical Idea of Redox Reactions – Oxidation &
Reduction Reaction:
(i)Oxidation: Oxygen का जुड़ना
Atmosphere म" dioxygen present है , तो काफ़* elements oxygen के साथ combine हो जाते
है l इसी वजह से 2यादातर elements atmosphere म" oxides के form म" पाए जाते ह8 l
Eg: 2Mg(s) +O2(g) 2MgO (s)
S(s) + O2(s) SO2 (s)
CH4(g) + 2O2(g) CO2(g) + 2H2O(l) → (i)
ऊपर के example से हम यह भी कह सकते ह8 ;क oxidation- removal of hydrogen भी होता है l
Eg: 2H2S (g) + O2(g) → 2S (s) + H2O (l) → (ii)
→ Removal of electropositive elements is also called as oxidation.
2K4 [Fe(CN)6] (aq) + H2O2 (aq) → 2K3 [Fe(CN)6] (aq) + 2KOH (aq)
→ Addition of electronegative element.
Mg (s) + F2 (g) → MgF2 (s)
Mg (s) + Cl2(g) → MgCl2 (s)
Mg (s) + S (g) → MgS (s)
DESIGNED
REDOX REACTIONS
NEW NOTES FOR CLASS 11 2022 EXAMS
, OVERVIEW OF THE CHAPTER
1. Uses of redox reaction.
2. Classical idea of redox reactions – oxidation and reduction reaction.
3. Redox reactions in terms of electron transfer reactions.
4. Competitive electron transfer reactions.
5. Oxidation number.
6. Types of Redox Reactions:
(i) Combination reactions
(ii) Decomposition reactions
(iii) Displacement reactions:
Metal displacement and non – metal displacement
7. Balancing of redox reactions:
(i) Oxidation number method
(ii) Half reaction method
8. Redox reactions as the basis for titrations.
9. Limitations of concept of oxidation number.
10. Redox Reactions & electrode process.
, 1. Uses of Redox Reaction:
a. Extensive use in pharmaceutical, biological, industrial, metallurgical and
agricultural areas.
b. Burning of different types of fuels for obtaining energy.
c. In electrochemical process for extraction of highly reactive metals and non-
metals.
d. Manufacturing of chemical compounds like caustic soda.
e. In dry & wet batteries.
f. Corrosion of metals.
g. Environment issues like use of hydrogen economy (use of liquid hydrogen as
fuel) & development of ‘ozone hole’ are under redox phenomenon)
2.Classical Idea of Redox Reactions – Oxidation &
Reduction Reaction:
(i)Oxidation: Oxygen का जुड़ना
Atmosphere म" dioxygen present है , तो काफ़* elements oxygen के साथ combine हो जाते
है l इसी वजह से 2यादातर elements atmosphere म" oxides के form म" पाए जाते ह8 l
Eg: 2Mg(s) +O2(g) 2MgO (s)
S(s) + O2(s) SO2 (s)
CH4(g) + 2O2(g) CO2(g) + 2H2O(l) → (i)
ऊपर के example से हम यह भी कह सकते ह8 ;क oxidation- removal of hydrogen भी होता है l
Eg: 2H2S (g) + O2(g) → 2S (s) + H2O (l) → (ii)
→ Removal of electropositive elements is also called as oxidation.
2K4 [Fe(CN)6] (aq) + H2O2 (aq) → 2K3 [Fe(CN)6] (aq) + 2KOH (aq)
→ Addition of electronegative element.
Mg (s) + F2 (g) → MgF2 (s)
Mg (s) + Cl2(g) → MgCl2 (s)
Mg (s) + S (g) → MgS (s)
