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1️⃣ #CHEMICALEQUILIBRIUM
✔️ State where forward & reverse reactions occur at same rate
✔️ Concentrations of reactants & products become constant
📌 Example:
N₂ + 3H₂ ⇌ 2NH₃


2️⃣ #EQUILIBRIUMCONSTANT (K)
✔️ Ratio of product concentrations to reactant concentrations
✔️ Each raised to power of stoichiometric coefficient
📌 General reaction:
aA + bB ⇌ cC + dD
📌 Expression:
Kc = [C]ᶜ[D]ᵈ / [A]ᵃ[B]ᵇ


3️⃣ #TYPESOFEQUILIBRIUMCONSTANT
✔️ Kc → concentration based
✔️ Kp → partial pressure based
📌 Relation:
Kp = Kc(RT)ⁿ
✔️ n = moles of gaseous products − moles of gaseous reactants


4️⃣ #SIGNIFICANCEOFK
✔️ Predicts extent of reaction
✔️ Tells position of equilibrium
📌 Values:
✔️ K ≫ 1 → Product favoured
✔️ K ≪ 1 → Reactant favoured
✔️ K ≈ 1 → Both present


5️⃣ #REACTIONQUOTIENT (Q)
✔️ Same expression as K
✔️ Calculated at any stage of reaction
📌 Comparison:
✔️ Q < K → reaction proceeds forward
✔️ Q > K → reaction proceeds backward
✔️ Q = K → equilibrium


6️⃣ #APPLICATION1DIRECTIONOFREACTION
✔️ Compare Q with K
✔️ Predict spontaneous direction
📌 Very important for numericals


7️⃣ #APPLICATION2DEGREEOFDISSOCIATION
✔️ Used for weak electrolytes
📌 Example:
HA ⇌ H⁺ + A⁻
K = α²C / (1 − α)
✔️ α = degree of dissociation
✔️ C = initial concentration


8️⃣ #APPLICATION3IONIZATIONOFWEAKELECTROLYTES
✔️ Acids & bases have small K value
📌 Example:
CH₃COOH ⇌ H⁺ + CH₃COO⁻
✔️ Small K → weak acid


9️⃣ #APPLICATION4CALCULATIONOFCONCENTRATION
✔️ Find unknown equilibrium concentration
✔️ Used in ICE table method
📌 Steps:
✔️ Initial concentration
✔️ Change
✔️ Equilibrium


🔟 #APPLICATION5EFFECTOFCHANGINGCONDITIONS
✔️ Temperature change affects K
✔️ Concentration & pressure do NOT change K
📌 Only temperature changes K value


1️⃣1️⃣ #EFFECTOFTEMPERATURE
✔️ Endothermic reaction:
Temperature ↑ → K ↑
✔️ Exothermic reaction:
Temperature ↑ → K ↓


1️⃣2️⃣ #RELATIONWITHGIBBSFREEENERGY
📌 Formula:
ΔG° = −RT ln K
✔️ ΔG° < 0 → K > 1 (spontaneous)
✔️ ΔG° > 0 → K < 1


1️⃣3️⃣ #HETEROGENEOUSEQUILIBRIUM
✔️ Solids & liquids not included in K
📌 Example:
CaCO₃(s) ⇌ CaO(s) + CO₂(g)
Kp = P(CO₂)


1️⃣4️⃣ #REVERSINGREACTION
✔️ K(reverse) = 1 / K(forward)


1️⃣5️⃣ #MULTIPLYINGREACTION
✔️ If reaction multiplied by n
✔️ New K = Kⁿ


1️⃣6️⃣ #NEET⚠️
✔️ K depends only on temperature
✔️ Catalyst does not change K
✔️ Pure solids not included
✔️ Units of K depend on reaction


1️⃣7️⃣ #ONELINEREVISION
✔️ K predicts extent of reaction
✔️ Q vs K gives direction
✔️ Only temperature affects K
✔️ Kp–Kc relation important

⃣ #SOLUBILITYPRODUCT
✔️ Solubility product = product of molar concentrations of ions in saturated solution
✔️ Each concentration raised to power of its stoichiometric coefficient
📌 For salt: AₓBᵧ
Ksp = [A⁺]ˣ [B⁻]ʸ


2️⃣ #CONDITIONOFAPPLICABILITY
✔️ Salt must be sparingly soluble
✔️ Solution must be saturated
✔️ At constant temperature

.
3️⃣ #IONICDISSOCIATION
✔️ AB(s) ⇌ A⁺ + B⁻
✔️ A₂B(s) ⇌ 2A⁺ + B²⁻
✔️ AB₂(s) ⇌ A⁺ + 2B⁻
.

4️⃣ #MOLARSOLUBILITY (S)
✔️ Molar solubility = moles dissolved per litre to form saturated solution
📌 Units: mol L⁻¹


⭐⭐5️⃣ #KspINTERMSSOLUBILITY (VERY IMP )

5️⃣1️⃣ For AB
AB ⇌ A⁺ + B⁻
Ksp = S²
S = √Ksp

5️⃣2️⃣ For A₂B
A₂B ⇌ 2A⁺ + B²⁻
Ksp = (2S)²(S) = 4S³
S = (Ksp / 4)¹ᐟ³

5️⃣3️⃣ For AB₂
AB₂ ⇌ A⁺ + 2B⁻
Ksp = S(2S)² = 4S³
S = (Ksp / 4)¹ᐟ³

5️⃣4️⃣ For A₃B
A₃B ⇌ 3A⁺ + B³⁻
Ksp = (3S)³(S) = 27S⁴


6️⃣ #IONICPRODUCT (IP)
✔️ IP = product of ionic concentrations at any instant
📌 Comparison:
✔️ IP < Ksp → Unsaturated
✔️ IP = Ksp → Saturated
✔️ IP > Ksp → Precipitation
.
7️⃣ #COMMONIONEFFECT (NEET )
✔️ Solubility decreases in presence of common ion
📌 Example:
AgCl solubility ↓ in NaCl solution
📌 Reason: Equilibrium shifts backward


8️⃣ #EFFECTOFPHONCOMMONION
✔️ Solubility increases if no common ion present


9️⃣ #SELECTIVEPRECIPITATION
✔️ Salt with lower Ksp precipitates first
📌 Used in qualitative analysis


🔟 #RELATIONBETWEENSOLUBILITYANDKsp
✔️ Higher Ksp ≠ higher solubility always
✔️ Depends on stoichiometry of salt


1️⃣1️⃣ #SOLUBILITYINPRESENCEOFCOMMONION
For AB in presence of B⁻ concentration = C
Ksp = S × C
S = Ksp / C
📌 Used in buffer & salt solutions


1️⃣2️⃣ #SOLUBILITYINPRESENCEOFPH
✔️ For salts of weak acids → solubility increases in acidic medium
✔️ For salts of weak bases → solubility increases in basic medium
📌 Example:
CaCO₃ dissolves more in acidic solution


1️⃣3️⃣ #TEMPERATUREEFFECT
✔️ Ksp increases with temperature (usually)
✔️ Endothermic dissolution favoured


1️⃣4️⃣ #UNITOFKsp
✔️ Depends on stoichiometry
✔️ No fixed unit
📌 NEET note: Ksp has no unit


1️⃣5️⃣ #COMPARISONOFKspVALUES
✔️ Compare only salts with same formula type
✔️ Otherwise comparison invalid


1️⃣6️⃣ #PRECIPITATIONCONDITION
✔️ Precipitation starts when IP just exceeds Ksp


1️⃣7️⃣ #SOLUBILITYORDER
✔️ Lower Ksp → lower solubility (for same type salts)


1️⃣8️⃣ #NEET⚠️TRAPS
✔️ Ksp valid only for saturated solution
✔️ Ksp ≠ solubility
✔️ Common ion reduces solubility
✔️ Ksp independent of initial concentration
✔️ Compare Ksp only at same temperature


1️⃣9️⃣ #NUMERICALSHORTCUT
✔️ If Ksp = 10⁻¹⁰ for AB
S ≈ 10⁻⁵
✔️ If Ksp = 4×10⁻¹² for AB₂
S ≈ 10⁻⁴


2️⃣0️⃣ #ONELINEREVISION
✔️ Ksp = ionic product at saturation
✔️ Precipitation when IP > Ksp
✔️ Common ion ↓ solubility
✔️ Same Ksp ≠ same solubility

Q1
Assertion (A): Solubility of AgCl decreases on addition of NaCl.
Reason (R): Addition of NaCl increases concentration of Cl⁻ ions.


Q2
Assertion (A): Larger the value of Ksp, higher is the solubility of a salt.
Reason (R): Ksp is directly proportional to solubility for all salts


Q3
Assertion (A): Precipitation occurs when ionic product exceeds Ksp.
Reason (R): Solution becomes supersaturated under this condition.


Q4
Assertion (A): Solubility of BaSO₄ increases in presence of dilute HCl.
Reason (R): H⁺ ions react with SO₄²⁻ ions to form HSO₄⁻.


Q5
Assertion (A): Two salts having same Ksp may have different solubilities.
Reason (R): Solubility depends on number of ions produced on dissociation

.

1️⃣ #WEAKELECTROLYTES
✔️ Weak acids & weak bases ionise partially in aqueous solution
✔️ Establish equilibrium between ionised & unionised form
📌 Examples:
✔️ Weak acid → CH₃COOH
✔️ Weak base → NH₄OH


2️⃣ #IONISATIONOFWEAKACID
✔️ Partial dissociation in water
📌 General reaction:
HA + H₂O ⇌ H₃O⁺ + A⁻
📌 Example:
CH₃COOH + H₂O ⇌ H₃O⁺ + CH₃COO⁻


3️⃣ #ACIDDISSOCIATIONCONSTANT (Ka)
✔️ Measure of strength of weak acid
✔️ Higher Ka → stronger acid
📌 Expression:
Ka = [H⁺][A⁻] / [HA]
✔️ Unit: mol L⁻¹


4️⃣ #DEGREEOFIONISATION (α)
✔️ Fraction of total molecules ionised
📌 Formula:
α = Number of molecules ionised / Total molecules
✔️ For weak acids → α ≪ 1


5️⃣ #RELATIONBETWEENKaANDα (NEET FAV )
For weak acid of concentration C:
📌 Formula:
Ka = Cα²
📌 Therefore:
α = √(Ka / C)
✔️ Ionisation increases on dilution


6️⃣ #pKaCONCEPT
✔️ pKa = –log Ka
✔️ Lower pKa → stronger acid
📌 Relation:
Strong acid → small pKa
Weak acid → large pKa


7️⃣ #pHOFWEAKACID
For weak acid of concentration C:
📌 Formula:
[H⁺] = √(Ka × C)
📌 pH formula:
pH = ½ ( pKa – log C )
✔️ Very important for numericals


8️⃣ #IONISATIONOFWEAKBASE
✔️ Partial dissociation in water
📌 General reaction:
BOH ⇌ B⁺ + OH⁻
📌 Example:
NH₄OH ⇌ NH₄⁺ + OH⁻


9️⃣ #BASEDISSOCIATIONCONSTANT (Kb)
✔️ Measure of strength of weak base
✔️ Higher Kb → stronger base
📌 Expression:
Kb = [B⁺][OH⁻] / [BOH]


🔟 #RELATIONBETWEENKbANDα
For weak base of concentration C:
📌 Formula:
Kb = Cα²
📌 Therefore:
α = √(Kb / C)


1️⃣1️⃣ #pKbCONCEPT
✔️ pKb = –log Kb
✔️ Lower pKb → stronger base


1️⃣2️⃣ #pHOFWEAKBASE
For weak base of concentration C:
📌 [OH⁻] = √(Kb × C)
📌 pOH formula:
pOH = ½ ( pKb – log C )
📌 pH = 14 – pOH


1️⃣3️⃣ #DILUTIONEFFECT (VERY IMP 🔥)
✔️ On dilution → degree of ionisation increases
✔️ But total ions per unit volume decrease
📌 Ostwald’s dilution law applies


1️⃣4️⃣ #COMMONIONEFFECT
✔️ Ionisation of weak electrolyte decreases
✔️ Presence of common ion shifts equilibrium backward
📌 Example:
CH₃COOH + CH₃COONa → ionisation decreases


1️⃣5️⃣ #WEAKACIDVSWEAKBASE
✔️ Weak acid → H⁺ producing
✔️ Weak base → OH⁻ producing
✔️ Both show partial ionisation


1️⃣6️⃣ #NEET⚠️KEYPOINTS
✔️ Ka & Kb are temperature dependent
✔️ α increases with dilution
✔️ pH of weak acid > strong acid (same concentration)
✔️ pH of weak base < strong base (same concentration)


1️⃣7️⃣ #ONELINEREVISION
✔️ Weak electrolytes ionise partially
✔️ Ka = Cα²
✔️ [H⁺] = √(Ka × C)
✔️ pH weak acid = ½ (pKa – log C)
✔️ Dilution increases ionisation

1️⃣ #REDOXREACTION
✔️ Redox reaction = reaction involving simultaneous oxidation and reduction
✔️ Oxidation → loss of electrons
✔️ Reduction → gain of electrons
📌 Example:
Zn + Cu²⁺ → Zn²⁺ + Cu
✔️ Zn → Zn²⁺ + 2e⁻ (Oxidation)
✔️ Cu²⁺ + 2e⁻ → Cu (Reduction)


2️⃣ #OXIDATIONNUMBERCONCEPT
✔️ Oxidation number (ON) = hypothetical charge if all bonds ionic
✔️ Increase in ON → oxidation
✔️ Decrease in ON → reduction
📌 Rules:
✔️ Element in free state → ON = 0
✔️ Monatomic ion → ON = charge
✔️ Oxygen → usually –2
✔️ Hydrogen → usually +1
✔️ Sum of ONs in molecule → 0
✔️ Sum of ONs in polyatomic ion → ion charge


3️⃣ #TYPESOFREDOXREACTIONS
✔️ Combination reaction → A + B → AB
✔️ Decomposition → AB → A + B
✔️ Displacement → A + BC → AC + B
✔️ Disproportionation → X → Xⁿ⁺ + Xᵐ⁻
📌 Example:
2H₂O₂ → 2H₂O + O₂
✔️ O in H₂O₂: –1 → 0 & –2 (disproportionation)


4️⃣ #OXIDISINGAGENT
✔️ Substance that accepts electrons
✔️ Causes oxidation of other species
📌 Example:
✔️ Cu²⁺ in Zn + Cu²⁺ → Cu²⁺ is oxidising agent


5️⃣ #REDUCINGAGENT
✔️ Substance that donates electrons
✔️ Causes reduction of other species
📌 Example:
✔️ Zn in Zn + Cu²⁺ → Zn is reducing agent


6️⃣ #ELECTRONBALANCEMETHOD (NEET FAV )
✔️ Step 1 → Write oxidation & reduction half-reactions
✔️ Step 2 → Balance atoms other than O & H
✔️ Step 3 → Balance O by H₂O
✔️ Step 4 → Balance H by H⁺ (acidic) or OH⁻ (basic)
✔️ Step 5 → Balance electrons
✔️ Step 6 → Combine half-reactions


7️⃣ #IONICEQUATIONEXAMPLE
✔️ Fe²⁺ + Cr₂O₇²⁻ → Fe³⁺ + Cr³⁺ (acidic medium)
📌 Half-reactions:
Fe²⁺ → Fe³⁺ + e⁻
Cr₂O₇²⁻ + 14H⁺ + 6e⁻ → 2Cr³⁺ + 7H₂O
📌 Multiply Fe reaction by 6 → 6Fe²⁺ → 6Fe³⁺ + 6e⁻
📌 Combine → 6Fe²⁺ + Cr₂O₇²⁻ + 14H⁺ → 6Fe³⁺ + 2Cr³⁺ + 7H₂O


8️⃣ #DISPROPORTIONATIONREACTIONS
✔️ Same element undergoes oxidation & reduction simultaneously
📌 Example:
3Cl₂ + 6OH⁻ → 5Cl⁻ + ClO₃⁻ + 3H₂O
✔️ Cl → –1 & +5


9️⃣ #NEET⚠️KEYPOINTS
✔️ Redox can occur in acidic or basic medium
✔️ Use oxidation number method for quick identification
✔️ Disproportionation = special redox with same element
✔️ Oxidising & reducing agents always appear on opposite sides


1️⃣0️⃣ #ONELINEREVISION
✔️ Redox = Oxidation + Reduction
✔️ Oxidation → loss e⁻, ON ↑
✔️ Reduction → gain e⁻, ON ↓
✔️ Oxidising agent → gains e⁻
✔️ Reducing agent → loses e⁻
✔️ Use half-reaction method for balancing

All cyclic compound ❤

Periodic table order
Exceptional like
1st ⭐#Radii grp 13 p block al>Ga
d series mn 3d5 sw so vahi sw reverse then fe=co=ni then cu<zn
2nd ⭐ #IE 3d<4d<5d but in 4th to 12th grp
4d=5d (appro) LC.
In grp 13 Beet, GAI
14th pb>sn
3rd ⭐EA : 2nd period se 3rd vale ki hmesha jyada
Highest Cl
Oxygen family M O last m

1️⃣ #CARBONFAMILY
✔️ Group number → 14
✔️ General electronic configuration:
📌 ns² np²
✔️ Members:
✔️ Carbon (C)
✔️ Silicon (Si)
✔️ Germanium (Ge)
✔️ Tin (Sn)
✔️ Lead (Pb)


2️⃣ #POSITIONINPERIODICTABLE
✔️ Lies between Boron family (13) & Nitrogen family (15)
✔️ First group containing non-metal → metalloid → metal trend
📌 Nature trend:
✔️ C → Non-metal
✔️ Si, Ge → Metalloids
✔️ Sn, Pb → Metals


3️⃣ #ATOMICANDPHYSICALPROPERTIES
✔️ Atomic radius ↑ down the group
✔️ Ionisation enthalpy ↓ down the group
✔️ Electronegativity ↓ down the group
📌 Density:
✔️ Increases downwards (exception: Pb irregularity)


4️⃣ #COVALENTCHARACTER
✔️ Strong covalent bonding (especially C, Si)
✔️ Due to:
✔️ Small size
✔️ High electronegativity
📌 Carbon shows maximum covalency (4)


5️⃣ #OXIDATIONSTATES ⭐ VERY IMP
✔️ Common oxidation states:
✔️ +4 and +2
📌 Stability trend:
✔️ +4 stable for C, Si
✔️ +2 stability ↑ down the group
📌 Reason:
✔️ Inert pair effect (Sn, Pb)
📌 Examples:
✔️ CO₂ → +4
✔️ CO → +2
✔️ SnCl₂ (+2) more stable than SnCl₄


6️⃣ #INERTPAIREFFECT
✔️ Poor shielding of d & f electrons
✔️ ns² electrons less available for bonding
📌 Order:
C < Si < Ge < Sn < Pb
✔️ Pb shows strongest inert pair effect


7️⃣ #CATABENATION (NEET FAV )
✔️ Ability to form long chains
📌 Order:
C >>> Si > Ge > Sn > Pb
📌 Reason:
✔️ Strong C–C bond
✔️ Small atomic size
✔️ Carbon forms:
✔️ Straight chains
✔️ Branched chains
✔️ Rings


8️⃣ #ALLOTROPY
✔️ Carbon shows extensive allotropy
📌 Allotropes of carbon:
✔️ Diamond → hardest, sp³
✔️ Graphite → conductor, sp²
✔️ Fullerene (C₆₀)
✔️ Si, Ge show limited allotropy


9️⃣ #HYDRIDES
✔️ General formula: MH₄
📌 Examples:
✔️ CH₄ → Methane
✔️ SiH₄ → Silane
📌 Stability:
CH₄ > SiH₄ > GeH₄ > SnH₄
✔️ Reducing character ↑ down group


1️⃣0️⃣ #HALIDES
✔️ General formula: MX₄
📌 Examples:
✔️ CCl₄
✔️ SiCl₄
📌 Hydrolysis:
✔️ CCl₄ → no hydrolysis
✔️ SiCl₄ → hydrolyses easily
📌 Reason:
✔️ Availability of vacant d-orbitals in Si


1️⃣1️⃣ #OXIDES
✔️ General formula: MO₂
📌 Nature:
✔️ CO₂ → acidic
✔️ SiO₂ → weakly acidic
✔️ SnO₂, PbO₂ → amphoteric
📌 Acidity ↓ down the group


1️⃣2️⃣ #ANOMALOUSBEHAVIOUROFCARBON
✔️ Small size
✔️ High electronegativity
✔️ Strong pπ–pπ bonding
✔️ Maximum catenation
✔️ No d-orbitals
📌 Hence carbon differs from rest of group


1️⃣3️⃣ #USES (NEET RELEVANT)
✔️ Carbon → fuels, organic compounds
✔️ Silicon → semiconductors, glass
✔️ Tin → coating (tin cans)
✔️ Lead → batteries, radiation shielding


1️⃣4️⃣ #NEETKEYPOINTS
✔️ +2 oxidation state stability ↑ down group
✔️ Inert pair effect strongest in Pb
✔️ Carbon shows maximum catenation
✔️ CO₂ acidic, PbO₂ amphoteric


1️⃣5️⃣ #ONELINEREVISION
✔️ Group 14 → ns² np²
✔️ C non-metal → Pb metal
✔️ Oxidation states +4, +2
✔️ Inert pair effect important
✔️ Carbon is exceptional

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Okay abse memes bhi dalna start kr dunga channel pr

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Apko observe krke meri observation change ho gyi 🙂

1️⃣ #ISOMERISM
✔️ Compounds having same molecular formula
✔️ But different arrangement of atoms
✔️ Hence different properties
📌 Types:
✔️ Structural isomerism
✔️ Stereoisomerism


2️⃣ #STRUCTURALISOMERISM
✔️ Difference in connectivity of atoms
📌 Types:
✔️ Chain isomerism
✔️ Position isomerism
✔️ Functional isomerism
✔️ Metamerism
✔️ Tautomerism


3️⃣ #CHAINISOMERISM
✔️ Different carbon chain arrangement
📌 Example:
✔️ n-Butane & isobutane (C₄H₁₀)
✔️ Seen in alkanes


4️⃣ #POSITIONISOMERISM
✔️ Same functional group
✔️ Different position on carbon chain
📌 Example:
✔️ 1-butanol & 2-butanol


5️⃣ #FUNCTIONALISOMERISM ⭐
✔️ Different functional groups
📌 Example:
✔️ Alcohol (C₂H₆O) ↔ Ether (C₂H₆O)
✔️ Aldehyde ↔ Ketone
✔️ Very common NEET MCQ


6️⃣ #METAMERISM
✔️ Different alkyl groups around polyvalent atom
📌 Example:
✔️ Ethers, amines


7️⃣ #TAUTOMERISM ⭐⭐
✔️ Dynamic equilibrium between two structures
✔️ Differs in position of H and double bond
📌 Example:
✔️ Keto ⇌ Enol
✔️ Acid/base catalysed
✔️ Keto form usually more stable


8️⃣ #STEREOISOMERISM
✔️ Same structural formula
✔️ Different spatial arrangement
📌 Types:
✔️ Geometrical isomerism
✔️ Optical isomerism


9️⃣ #GEOMETRICALISOMERISM
✔️ Due to restricted rotation (C=C)
📌 Conditions:
✔️ Each C of double bond attached to two different groups
📌 Types:
✔️ cis
✔️ trans
📌 Example:
✔️ cis-2-butene & trans-2-butene


🔟 #OPTICALISOMERISM
✔️ Due to chiral carbon (asymmetric C)
📌 Chiral carbon:
✔️ Carbon attached to 4 different groups
📌 Property:
✔️ Rotates plane polarized light
✔️ d- & l- forms
PART–B : REACTION MECHANISM


1️⃣1️⃣ #REACTIONMECHANISM
✔️ Step-by-step description of how reaction occurs
✔️ Shows movement of electrons


1️⃣2️⃣ #BOND_FISSION
✔️ Breaking of covalent bond
📌 Types:
✔️ Homolytic
✔️ Heterolytic


1️⃣3️⃣ #HOMOLYTICFISSION
✔️ Equal bond breaking
✔️ Each atom gets one electron
📌 Forms:
✔️ Free radicals
📌 Example:
✔️ Cl₂ → 2Cl•
✔️ Occurs in UV / heat


1️⃣4️⃣ #HETEROLYTICFISSION
✔️ Unequal bond breaking
✔️ One atom gets both electrons
📌 Forms:
✔️ Carbocation
✔️ Carbanion
📌 Example:
✔️ CH₃–Cl → CH₃⁺ + Cl⁻


1️⃣5️⃣ #REACTIONINTERMEDIATES ⭐
✔️ Short-lived species
📌 Types:
✔️ Free radicals
✔️ Carbocation
✔️ Carbanion


1️⃣6️⃣ #CARBOCATION
✔️ Positively charged carbon
✔️ sp² hybridised
📌 Stability order:
✔️ 3° > 2° > 1° > CH₃⁺
✔️ Shows rearrangement


1️⃣7️⃣ #CARBANION
✔️ Negatively charged carbon
✔️ sp³ hybridised
📌 Stability order:
✔️ CH₃⁻ > 1° > 2° > 3°


1️⃣8️⃣ #FREERADICAL
✔️ Neutral species with unpaired electron
📌 Stability order:
✔️ 3° > 2° > 1° > CH₃

1️⃣9️⃣ #NUCLEOPHILE
✔️ Electron-rich species
✔️ Donates electron pair
📌 Examples:
✔️ OH⁻, CN⁻, NH₃


2️⃣0️⃣ #ELECTROPHILE
✔️ Electron-deficient species
✔️ Accepts electron pair
📌 Examples:
✔️ H⁺, NO₂⁺, BF₃


2️⃣1️⃣ #NEET⚠️IMPORTANTPOINTS
✔️ Functional isomerism very common
✔️ Tautomerism = dynamic equilibrium
✔️ Stability of carbocation frequently asked
✔️ Identify nucleophile/electrophile carefully


2️⃣2️⃣ #ONELINEREVISION
✔️ Same formula, different structure → isomerism
✔️ Keto–enol = tautomerism
✔️ Chiral carbon → optical activity
✔️ Carbocation most stable = 3°
✔️ Nucleophile = electron donor

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