Oxidation-Reduction and Solution Formulas

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Formula Sheet for Oxidation-Reduction and Solution

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Oxidation Reaction in which	Reduction Reaction in which
1. there is a ↑ in O or Electronegative element or compound (S, Cl, F, Br, I) in any element or compound	1. there is a ↑ in El or Electro positive element in any element or compound
2. ↓ of H or electropositive element.	2. ↓ of O or electronegative element.
3. any atom or ion gives e^– (s) ie., DE-ELECTRONATION	3. any atom or ion accepts e^– (s) ie., ELECTRONATION
4. Positive valency of element ↑	4. Positive valency of element ↓
5. Negative valency of element ↓	5. Negative valency of element ↑
6. there is a ↑ in O.N. (Oxidation no.) of element.	6. there is a ↓ in O.N. (Oxidation no.) of element.

2. Oxidant itself is reduced (gives O₂)
Or Oxidant → e^– (s) Acceptor
Reductant itself is oxidised (gives H₂)
Or Reductant → e^–(s) Donor

3. (a) List of common oxidising agents:

O₂
O₃
H₂O₂
H₂SO₄
HNO₃
HCIO₄
KClO₃
(K₂Cr₂O₇/H₂SO₄)
(KMnO₄/H₂SO₄)
(KMnO₄/KOH)
F₂, Cl₂, Br₂

(b) List of Common Reductants:

H₂
HI
H₂S
LiAlH₄
NaBH₄
SO₂,
C
O₃
H₂O₂
(Sn/HCl)
(Na/C₂H₅OH)
Metallic Salts (Ous) like SnCl₂, FeSO₄

(c) Substance acting as oxidant as well as Reductant:
HNO₂, O₃, H₂O₂, SO₂ etc.

4. (i) Strongness of acid oc oxidation number
(ii) Strongness of base ∝ \(\frac{1}{\text { oxidation number }}\)

5. Equivalent Weight of compound = Mol. weight / Total Charge in O.N. per molecule
Note: – Equivalent weight of KMnO₄ (Mol.wt. 158) in acidic, alkaline & neutral media is respectively : 31.6, 158, 52.6

6. TABLE: – Important Oxidation & Reduction Part (a):

Oxidation Part (Half reaction)
1. Fe²⁺ – Fe³⁺	8. S₂O₃^2- – S₄O₆^2-
2. H₂O₂ – O₂(basic med.)	9. I₂ – IO₃^–
3. Zn – Zn²⁺	10. ASO₃^3- – ASO₄^3-
4. SO₃^2-– SO₄^2-	11. Sn²⁺ – Sn⁴⁺
5. Cl^– – Cl₂ (Or X^–→ X₂)	12. Cu⁺ – Cu⁺²
6. S^2- – S	13. U⁴⁺ – UO₂²⁺
7. C₂O₄^2- – CO₂	14. SO₂ – SO₄^2-

(b)

Reduction Part (Half Reaction)
1. Fe³⁺ – Fe²⁺	8.MnO₄^– – MnO₂(ln alkaline & neutral medium)
2. H₂O₂ – H₂O	9. I₂ – IO^–(Or X₂ → X^–)
3. CrO₄^2- – Cr³⁺	10. MnO₄^– – Mn⁺²(In acidic med.)
4. SO₄^2- – SO₂	11. MnO₄^– – Mn⁺⁴ (In alkaline & neutral medium)
5. OCl^– – Cl^–	12. CIO₃^– – Cl^–
6. [Fe(CN)₆]^3- – [Fe(CN)₆]^4-	13. VO²⁺ – V₂O₃
7. Cr₂O₇^2- – Cr³⁺ (Acidic medium)	14. NO₃^– – NO₂ (In Conc.HNO₃)
	15. NO₃^– – NO (In dil. HNO₃)

7. (a) Electro-Chemical Series:
Li, K, Ba, Sr, Ca, Na, Mg, Al, Mn, Zn, Cr, Fe, Cd, Co, Ni, Sn, Pb, H₂, Cu, Fig, Ag, Pt, Au.

(b) As we move from top to bottom in this series:-

Standard Reduction Potential ↑
Standard Oxidation Potential ↓
Reducing Capacity ↓
IP ↑
Reactivity ↓

8. Some other important points:

Formal charge = Group No. – [No. of bonds + No. of non-bonded electrons]
At Anode → Oxidation, Cathode → Reduction
For aqua-regia (HNO₃ + 3HCl) → Cl acts as an oxidant
Starch iodide paper is used for the identification of an oxidant
ON of any element remains in between n → n – 8 where n = group no.
SO₂ decolourlise the colour of flower by reduction & Cl₂ by oxidation.

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