⚡ PW Style One-Page Mindmaps

Ek Page, Ek Chapter Khallas! (70/70 Strategy)

Chapter 1
💧 SOLUTIONS

1. Henry's vs Raoult's

  • Henry's Law: Dissolving Gas in Liquid. p = KH × χ (Higher KH = Less soluble)
  • Raoult's Law: Liquid in Liquid. Volatile components. P(Total) = P°A·χA + P°B·χB

2. Ideal & Non-Ideal

  • Ideal: ΔH=0, ΔV=0, follows Raoult's. (Benzene+Toluene)
  • +ve Deviation: Weaker forces, Higher VP. Minimum boiling azeotrope. (Ethanol+Water)
  • -ve Deviation: Stronger forces, Lower VP. Maximum boiling azeotrope. (HNO3+Water)

3. Colligative Properties

  • RLVP: (P° - P)/P° = χ(solute)
  • Elevation BP: ΔTb = Kb × m
  • Depression FP: ΔTf = Kf × m
  • Osmotic Pres.: π = CRT

4. Van't Hoff Factor (i)

  • Used when solute Associates (i < 1) or Dissociates (i> 1).
  • i = Normal M.Mass / Abnormal M.Mass
  • Multiply 'i' to all colligative formulas!
Chapter 2
⚡ ELECTROCHEMISTRY

1. Nernst Equation

  • Calculate EMF at any concentration.
  • Ecell = E°cell - (0.0591/n) log(Q)
  • At Equilibrium: Ecell = 0
    E°cell = (0.0591/n) log(Kc)
  • ΔG° = -n F E°cell

2. Faraday's Laws

  • First Law: Mass deposited ∝ Q. W = Z × I × t
  • Second Law: Same current, different cells. W1 / E1 = W2 / E2 (E=Eq. weight)

3. Kohlrausch's Law

  • Molar conductivity at infinite dilution (Λ°m).
  • Λ°m (AB) = λ°(A+) + λ°(B-)
  • Application: Finding Λ°m for Weak Electrolytes (like CH3COOH) using Strong ones.

4. Batteries

  • Primary: Non-rechargeable (Dry cell).
  • Secondary: Rechargeable. Lead Storage. Discharge Anode: Pb → PbSO4
  • Fuel Cell: H2-O2 (Apollo space program). 70% efficient, water is byproduct.
Chapter 3
⏱️ CHEMICAL KINETICS

1. Rate & Order

  • Rate Law: Rate = k[A]^x[B]^y
  • Order: x+y (Experimental, can be 0 or fraction)
  • Molecularity: Theoretical collisions. (1, 2, 3... never 0)
  • Unit of k: (mol/L)^(1-n) s^-1

2. Zero & First Order

  • Zero Order: k = (R0 - R)/t
    Graph of [R] vs t is straight line decreasing.
  • First Order (VVI): k = (2.303/t) log(R0/R)
    All radioactive decays follow 1st order.

3. Half Life (t1/2)

  • Zero Order: t1/2 = R0 / 2k (Depends on Initial Conc.)
  • First Order: t1/2 = 0.693 / k (Independent of Initial Conc.)

4. Arrhenius Equation

  • Effect of Temp on Rate (Rate doubles for 10°C rise).
  • k = A e^(-Ea/RT)
  • log(k2/k1) = (Ea / 2.303R) [1/T1 - 1/T2]
  • Catalyst lowers Activation Energy (Ea).
Chapter 4
🏔️ d & f BLOCK ELEMENTS

1. General Properties (d-Block)

  • Variable Ox. States: Due to small energy diff. between (n-1)d and ns orbitals.
  • Catalytic Prop: Can form variable ox. states & provide surface area for rxn.
  • Colored Ions/Para: d-d transitions & unpaired electrons. μ = √(n(n+2)) BM

2. Lanthanoid Contraction (f-Block)

  • What: Steady decrease in size due to poor shielding by 4f electrons.
  • Consequences: Zr (4d) and Hf (5d) have almost identical atomic radii.
  • High resemblance in chemical properties makes them hard to separate.

3. Potassium Permanganate (KMnO4)

  • Color: Intense purple (due to Charge Transfer). Strong Oxidizing Agent!
  • Acidic Med: MnO4⁻ + 8H⁺ + 5e⁻ → Mn²⁺ + 4H2O (Oxidizes Fe²⁺ to Fe³⁺, I⁻ to I2).

4. Potassium Dichromate (K2Cr2O7)

  • Chromate-Dichromate Interconn: Yellow CrO4²⁻ ⇌ Orange Cr2O7²⁻ (depends on pH).
  • Acidic Med: Cr2O7²⁻ + 14H⁺ + 6e⁻ → 2Cr³⁺ + 7H2O.
Chapter 5
🔗 COORDINATION CMPDS

1. Werner's Theory

  • Primary Valency: Ionizable (Oxidation state of Metal). Satisfied by -ve ions.
  • Secondary Valency: Non-ionizable (Coordination Number). Satisfied by ligands. Defines shape.

2. Isomerism

  • Structural: Linkage (ambidentate NO2/SCN), Ionization, Coordination, Solvate.
  • Stereo: Geometrical (Cis/Trans mainly in square-planar & octahedral) and Optical (d/l forms, common in [M(en)3]3+).

3. Valence Bond Theory (VBT)

  • Strong Ligands (CO, CN-): Force pairing of electrons. Form Inner orbital complexes (d2sp3, diamagnetic).
  • Weak Ligands (H2O, F-): No pairing. Form Outer orbital complexes (sp3d2, high spin).

4. Crystal Field Theory (CFT)

  • d-orbitals split into t2g (lower) and eg (higher) in octahedral fields.
  • If Δo > P : 4th electron pairs in t2g (Low Spin).
  • Colors arise from excitation of e- from t2g to eg (d-d transition).
Chapter 7
🍷 ALCOHOLS & PHENOLS

1. Acidity (Phenol vs Alcohol)

  • Phenol is more acidic due to resonance stabilization of Phenoxide ion.
  • EWG (-NO2) increases acidity. ERG (-CH3, -OCH3) decreases acidity.

2. Phenol Name Reactions

  • Reimer-Tiemann: Phenol + CHCl3 + aq.NaOH → Salicylaldehyde (ortho).
  • Kolbe's Rxn: Phenol + CO2 + NaOH → Salicylic Acid (ortho).

3. Alcohol Distinction

  • Lucas Test (ZnCl2/HCl): Distinction of 1°, 2°, 3° alcohols.
  • 3° Gives immediate turbidity. 2° takes 5 mins. 1° doesn't react at room temp.

4. Ethers (Williamson Syn)

  • Williamson Synthesis: RONa + R'X → R-O-R'
  • R'X (Alkyl Halide) MUST BE PRIMARY (1°). If 3°, elimination happens (alkene forms).
  • Cleavage with HI: I- goes to SMALLER alkyl group.
Chapter 6
🔄 HALOALKANES & ARENES

1. SN1 vs SN2 (VVI)

  • SN1 (Carbocation): 2 steps. Reactivity: 3° > 2° > 1°. Weak nucleophile, Polar protic solvent. Forms Racemic mixture.
  • SN2 (Transition State): 1 step. Reactivity: 1° > 2° > 3° (Steric). Strong nucleophile. Complete Inversion (Walden).

2. Name Reactions (Halogen Exch)

  • Finkelstein: Makes Alkyl Iodides. R-Cl + NaI (Dry Acetone) → R-I + NaCl(ppt)
  • Swarts: Makes Alkyl Fluorides. R-X + AgF → R-F + AgX

3. Addition to Alkenes

  • Markovnikov: H goes to carbon with MORE Hydrogens. Negative part goes to LESS H.
  • Peroxide Effect (Anti-Markov): ONLY with HBr + Peroxide. Reverse addition.

4. Aryl Halides

  • Less reactive towards Nucleophilic substitution due to partial double bond character (resonance).
  • Wurtz-Fittig: Ar-X + R-X + Na → Ar-R
  • Fittig: Ar-X + Ar-X + Na → Biphenyl
Chapter 8
🍋 ALD, KETONES & CARBOXYLIC

1. Distinction Tests

  • Tollens' Test: Ag(NH3)2+. Gives Silver Mirror. (+ve for ALL Aldehydes).
  • Fehling's Test: Cu2+. Gives Red ppt. (+ve for Aliphatic Aldehydes ONLY).
  • Iodoform: For CH3-C=O or CH3-CH(OH)-. Yellow ppt (CHI3).

2. Alpha-Hydrogen Rxns

  • Aldol: Ald/Ket WITH α-H (Dil. NaOH) → β-hydroxy → Heat → α,β-unsaturated.
  • Cannizzaro: Aldehydes WITHOUT α-H (HCHO). Conc. NaOH → Self oxidation-reduction → Alcohol + Acid salt.

3. Reductions

  • Rosenmund: Acid Chloride → Aldehyde (H2/Pd-BaSO4).
  • Clemmensen: C=O → CH2 (Zn-Hg / conc. HCl).
  • Wolff-Kishner: C=O → CH2 (NH2NH2 / KOH, Glycol).

4. Carboxylic Acids

  • More acidic than Phenols (carboxylate ion has two equivalent resonance structures).
  • HVZ Reaction: Acid with α-H + X2/Red P → α-Haloacid.
Chapter 9
🐟 AMINES

1. Basic Character

  • Gas Phase: 3° > 2° > 1° > NH3 (+I effect)
  • Aqueous (Methyl): 2° > 1° > 3° > NH3
  • Aqueous (Ethyl): 2° > 3° > 1° > NH3
  • Aniline is weakest base (Lone pair in resonance).

2. Preparation

  • Gabriel Phthalimide: ONLY prepares pure 1° Aliphatic Amines.
  • Hoffmann Bromamide (VVI): Amide + Br2 + 4NaOH → 1° Amine (Steps down 1 Carbon).

3. Distinction Tests

  • Carbylamine: ONLY 1° Amines + CHCl3 + KOH → Isocyanide (Foul odor).
  • Hinsberg (Benzene sulphonyl chloride): 1° → Soluble in NaOH.
    2° → Insoluble in NaOH.
    3° → No reaction.

4. Diazonium Salts

  • Sandmeyer: CuCl/HCl or CuBr/HBr.
  • Gattermann: Cu powder / HCl.
  • Azo Dye Test: Aniline reacts with Diazonium salt to form Yellow dye.
Chapter 10
🧬 BIOMOLECULES

1. Carbohydrates

  • Reducing Sugars: Have free ald/ketonic group. Reduce Tollens/Fehlings. (Glucose, Fructose). Sucrose is NON-reducing.
  • Glucose Rxns: (+ HI/Red P) → n-hexane (proves straight chain). (+ Br2 water) → Gluconic acid (proves Aldehyde).
  • Anomers: Alpha & Beta glucose (differ at C1).

2. Proteins

  • Amino Acids: Zwitterions (+/- charges). Link via Peptide bonds.
  • Denaturation: On heating/pH change. 2° and 3° structures destroyed, 1° remains intact. (Ex: Boiling egg).

3. Vitamins

  • Fat Soluble: A, D, E, K. (Stored in adipose tissue).
  • Water Soluble: B, C. (Excreted in urine). Exception: Vit B12 is stored in liver.
  • Deficiencies: Vit A (Night blindness), Vit C (Scurvy).

4. Nucleic Acids

  • DNA: Deoxyribose sugar. Bases: A, G, C, T (Thymine). Double Helix. Stores genetic info.
  • RNA: Ribose sugar. Bases: A, G, C, U (Uracil). Single strand. Protein synthesis.