Summary
NCERT Class 11 Chemistry Chapter 7 covers redox reactions — processes where oxidation and reduction occur simultaneously, including definitions, oxidation numbers, electron transfer, and their applications in everyday phenomena like burning fuel, metal extraction, and battery operation.
Redox reactions are fundamental chemical processes where simultaneous oxidation and reduction occur. The chapter explains classical definitions (addition/removal of oxygen or hydrogen), electron-transfer concepts (loss and gain of electrons), and oxidation number methods for tracking electron shifts. It covers four types: combination reactions (elements forming compounds), decomposition (compounds breaking apart), displacement (one element replacing another), and disproportionation (single element both oxidized and reduced). The chapter demonstrates how redox reactions balance using oxidation numbers and half-reaction methods, their role in titrations with color indicators, and electrode processes underlying galvanic cells like the Daniell cell.
Key points & formulas
- 01Redox reactions occur when oxidation and reduction happen simultaneously; oxidation is electron loss, reduction is electron gain
- 02Oxidation numbers are assigned per element using six rules, with changes indicating redox processes and balancing equations
- 03Four types of redox reactions: combination (synthesis), decomposition, displacement (metals or non-metals), and disproportionation
- 04Half-reaction method separates redox into oxidation and reduction steps, balancing each independently then combining
- 05Redox titrations use color-change indicators (self-indicators like MnO₄⁻, or external indicators like diphenylamine) to detect equivalence points
- 06Electrode potentials measure redox couple tendency; negative E° indicates stronger reducing agents than hydrogen, positive E° indicates weaker reducing agents
Frequently asked questions
01What is the difference between oxidation and reduction in redox reactions?
Oxidation is the loss of electrons by a species (increase in oxidation number), while reduction is the gain of electrons (decrease in oxidation number). The oxidizing agent accepts electrons and is reduced; the reducing agent donates electrons and is oxidized. These processes always occur together in redox reactions.
02How do you balance redox equations using the oxidation number method?
Step 1: Assign oxidation numbers to all elements. Step 2: Identify which elements change oxidation state. Step 3: Calculate increase/decrease per atom and balance by multiplying coefficients so total increase equals total decrease. Step 4: In aqueous reactions, add H⁺ (acidic) or OH⁻ (basic) to balance charges. Step 5: Add H₂O molecules to balance hydrogen atoms.
03What are the four types of redox reactions with examples?
Combination: C(s) + O₂(g) → CO₂(g). Decomposition: 2H₂O(l) → 2H₂(g) + O₂(g). Displacement: Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s). Disproportionation: 2H₂O₂(aq) → 2H₂O(l) + O₂(g), where the same element exhibits multiple oxidation states.
04Is the NCERT Class 11 Chemistry Chapter 7 PDF free to download?
Yes, the NCERT Class 11 Chemistry Chapter 7 PDF is free to download. NCERT textbooks are published by the Government of India and freely distributed to support students' learning across all classes.
More chapters in Chemistry Part II
This is the complete Chemistry Part II Chapter 7 as published by NCERT — every diagram, solved example, and exercise included, free. Browse all NCERT Class 11 textbooks.
Read offline with notes, solutions & mock tests
CBSE Prepmaster — free on iOS & Android