Chemistry booster series

https://t.me/+5VTfeOK6KxJkYWQ1

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263 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, 18:55

Chemistry booster series

https://t.me/+5VTfeOK6KxJkYWQ1

Old m Copyright aa gya 🙂again upload krenge 3500+ video

Btw share krdo needy students ko baad m link na milegi

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248 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, 18:55

Chemistry booster series

1️⃣ #MOLECULARORBITALTHEORY
📌 Molecular Orbital Theory (MOT) explains bonding, bond order and magnetic nature of molecules.
📌 Proposed by Hund and Mulliken.

2️⃣ #BASICIDEA
✔️ Atomic orbitals of bonded atoms combine to form molecular orbitals
✔️ Molecular orbitals belong to the entire molecule
✔️ Number of MOs formed = number of AOs combined

3️⃣ #CONDITIONSFORCOMBINATION
✔️ Comparable energy of AOs
✔️ Proper orientation
✔️ Significant overlap

4️⃣ #TYPESOFMOLECULARORBITALS
✔️ Bonding MO
✔️ Antibonding MO
✔️ Non-bonding MO (rare in diatomic molecules)

5️⃣ #BONDINGMO
✔️ Formed by constructive overlap
✔️ Lower energy than AOs
✔️ Increases stability
📌 Denoted by: σ, π

6️⃣ #ANTIBONDINGMO
✔️ Formed by destructive overlap
✔️ Higher energy
✔️ Decreases stability
📌 Denoted by: σ*, π*

7️⃣ #ELECTRONFILLINGRULES
✔️ Aufbau principle
✔️ Pauli exclusion principle
✔️ Hund’s rule of maximum multiplicity

8️⃣ #ENERGYORDEROFDIATOMICMOLECULES ⭐
📌 For B₂, C₂, N₂:
σ1s < σ1s < σ2s < σ2s < π2p < σ2p < π2p < σ2p
📌 For O₂, F₂, Ne₂:
σ1s < σ1s < σ2s < σ2s < σ2p < π2p < π2p < σ2p

9️⃣ #BONORDER (VERY IMP )
📌 Formula:
Bond order = (Nb − Na) / 2
✔️ Nb = bonding electrons
✔️ Na = antibonding electrons
📌 Interpretation:
✔️ Higher bond order → stronger bond
✔️ Bond order = 0 → molecule does not exist

🔟 #MAGNETICNATURE
✔️ Unpaired electrons → paramagnetic
✔️ All electrons paired → diamagnetic
📌 Example:
✔️ O₂ → paramagnetic
✔️ N₂ → diamagnetic

1️⃣1️⃣ #IMPORTANTEXAMPLES (NEET 🔥)
✔️ H₂ → bond order = 1
✔️ He₂ → bond order = 0 (does not exist)
✔️ O₂⁺ → bond order increases
✔️ O₂⁻ → bond order decreases

1️⃣2️⃣ #LIMITATIONSOFMOT
✔️ Complex for polyatomic molecules
✔️ Does not explain shape clearly

1️⃣3️⃣ #NEETIMPORTANTPOINTS
✔️ MOT explains paramagnetism of O₂
✔️ Energy order changes after N₂
✔️ Bond order decides stability

1️⃣4️⃣ #ONELINEREVISION
Molecular Orbital Theory explains bonding by delocalised molecular orbitals and predicts bond order and magnetic nature

@Ayano1me @Neetugpoll @Neetugquiz

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210 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, 03:17

Chemistry booster series

1️⃣ #VALENCEBONDTHEORY
📌 Valence Bond Theory (VBT) explains formation of covalent bonds by overlap of atomic orbitals.
📌 Proposed by Heitler and London.

2️⃣ #BASICIDEA
✔️ Atoms bond to achieve stable electronic configuration
✔️ Half-filled atomic orbitals overlap
✔️ Electrons pair with opposite spins
📌 Greater overlap → stronger bond

3️⃣ #CONDITIONSFOROVERLAP
✔️ Half-filled orbitals
✔️ Comparable energy of orbitals
✔️ Proper orientation

4️⃣ #TYPESOFOBOND
✔️ Sigma (σ) bond
✔️ Pi (π) bond

5️⃣ #SIGMABOND
✔️ Formed by head-on overlap
✔️ Stronger than π bond
✔️ Electron density along internuclear axis
📌 Overlap types:
✔️ s–s
✔️ s–p
✔️ p–p

6️⃣ #PIBOND
✔️ Formed by sidewise overlap
✔️ Weaker than σ bond
✔️ Electron density above & below axis
📌 Formed by p–p overlap only

7️⃣ #HYBRIDISATION
📌 Mixing of atomic orbitals of similar energy to form hybrid orbitals.
✔️ Number of hybrid orbitals = number of AOs mixed

8️⃣ #TYPESOFHYBRIDISATION
✔️ sp → linear → 180° → BeCl₂
✔️ sp² → trigonal planar → 120° → BF₃
✔️ sp³ → tetrahedral → 109.5° → CH₄
✔️ dsp² → square planar → [Ni(CN)₄]²⁻
✔️ d²sp³ → octahedral → [Co(NH₃)₆]³⁺

9️⃣ #VALENCEBONDTHEORYINCOORDINATIONCOMPOUNDS
✔️ Central metal provides empty orbitals
✔️ Ligands donate lone pair
✔️ Coordinate bond formed by overlap

🔟 #MAGNETICNATURE
✔️ Unpaired electrons → paramagnetic
✔️ Paired electrons → diamagnetic
📌 Example:
✔️ [Ni(CN)₄]²⁻ → diamagnetic
✔️ [NiCl₄]²⁻ → paramagnetic

1️⃣1️⃣ #LIMITATIONSOFVBT
✔️ Cannot explain colour of compounds
✔️ Cannot explain strong vs weak ligands clearly
✔️ No quantitative explanation of spectra

1️⃣2️⃣ #NEETIMPORTANTPOINTS
✔️ σ bond is stronger than π bond
✔️ Multiple bonds = 1 σ + remaining π
✔️ Hybridisation explains geometry

1️⃣3️⃣ #ONELINEREVISION
Valence Bond Theory explains bonding by orbital overlap and predicts bond type, strength and geometry.

@Ayano1me @Neetugpoll @Neetugquiz

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204 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, 03:19

Chemistry booster series

Q1.
Assertion (A): In O₂ molecule, two electrons remain unpaired in molecular orbitals.
Reason (R): The last electrons of O₂ occupy degenerate π* antibonding orbitals according to Hund’s rule.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true

Q2.
Assertion (A): Bond order of N₂ molecule is 3.
Reason (R): N₂ has more electrons in bonding molecular orbitals than in antibonding molecular orbitals.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true

Q3.
Assertion (A): He₂ molecule does not exist.
Reason (R): Number of electrons in bonding and antibonding orbitals of He₂ are equal.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true

Q1.
Assertion (A): According to VBT, a covalent bond is formed by overlap of half-filled atomic orbitals.
Reason (R): Overlap of orbitals increases electron density between two nuclei.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true

Q2.
Assertion (A): A σ-bond is stronger than a π-bond.
Reason (R): σ-bond is formed by head-on overlap whereas π-bond is formed by sidewise overlap.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true

Q3.
Assertion (A): Valence Bond Theory cannot explain paramagnetism of O₂ molecule.
Reason (R): VBT does not consider molecular orbitals and electron delocalisation.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true

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266 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, 03:21

Chemistry booster series

https://t.me/+5VTfeOK6KxJkYWQ1

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238 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, 03:30

Chemistry booster series

1️⃣ #KINETICTHEORYOFGASES
✔️ Explains macroscopic properties of gases
✔️ Based on molecular motion
✔️ Applies mainly to ideal gases

2️⃣ #BASICPOSTULATES
✔️ Gas consists of very large number of molecules
✔️ Molecules are point masses (negligible volume)
✔️ Distance between molecules ≫ molecular size
✔️ Molecules move randomly in all directions

3️⃣ #NATUREOFMOLECULARMOTION
✔️ Continuous
✔️ Random
✔️ Straight-line motion between collisions
📌 Velocity constantly changes due to collisions

4️⃣ #INTERMOLECULARFORCES
✔️ Negligible attractive forces
✔️ No repulsion except during collision
📌 Valid only for ideal gases

5️⃣ #COLLISIONS (VERY IMP 🔥)
✔️ Collisions are perfectly elastic
✔️ Occur between:
▪️ Molecule–molecule
▪️ Molecule–wall
📌 No loss of kinetic energy

6️⃣ #PRESSUREOFGAS
✔️ Due to collision of gas molecules with container walls
✔️ More collisions → more pressure
📌 Pressure ∝ number of collisions

7️⃣ #KINETICENERGY
✔️ Average kinetic energy depends only on temperature
✔️ Independent of pressure & volume
📌 Formula:
Average K.E. = (3/2) kT (per molecule)
Average K.E. = (3/2) RT (per mole)

8️⃣ #TEMPERATURESIGNIFICANCE
✔️ Measure of average kinetic energy
✔️ At 0 K → molecular motion stops (ideal case)
📌 Higher T → higher molecular speed

9️⃣ #SPEEDOFGASMOLECULES
✔️ Three types:
▪️ Most probable speed (vₚ)
▪️ Average speed (vₐᵥ)
▪️ RMS speed (vᵣₘₛ)
📌 Relation:
vₚ < vₐᵥ < vᵣₘₛ

🔟 #SPEEDFORMULAE (NEET FAVORITE ❤️)
✔️ vₚ = √(2RT / M)
✔️ vₐᵥ = √(8RT / πM)
✔️ vᵣₘₛ = √(3RT / M)
📌 M in kg mol⁻¹

1️⃣1️⃣ #GRAHAMLAW (LINKED CONCEPT)
✔️ Rate ∝ 1 / √M
✔️ Lighter gas diffuses faster

1️⃣2️⃣ #DEVIATIONFROMIDEALBEHAVIOUR
✔️ Real gases deviate at:
▪️ High pressure
▪️ Low temperature
📌 Cause:
✔️ Finite molecular volume
✔️ Intermolecular attraction

1️⃣3️⃣ #LIMITATIONSOFKTG
❌ Cannot explain liquefaction
❌ Fails at high pressure
❌ Assumes zero molecular volume

1️⃣4️⃣ #NEETONELINERS
✔️ Pressure independent of mass of gas
✔️ KE ∝ absolute temperature
✔️ Elastic collision = KE conserved
✔️ At same T → all gases have same average KE

@Ayano1me @Neetugpoll @Neetugquiz

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280 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, 19:10

Chemistry booster series

Q1.
Assertion (A): Average kinetic energy of gas molecules is directly proportional to absolute temperature.
Reason (R): Increase in temperature increases the speed of gas molecules.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true

Q2.
Assertion (A): At constant temperature, pressure of a gas is inversely proportional to volume.
Reason (R): Number of collisions of gas molecules with container walls increases when volume decreases.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true

Assertion (A): Root mean square (rms) speed of gas molecules depends on the nature of gas.
Reason (R): rms speed is inversely proportional to the square root of molar mass.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true

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234 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, 19:11

Chemistry booster series

1️⃣ #THERMODYNAMICS
✔️ Branch of chemistry dealing with energy changes
✔️ Studies relation between heat, work & energy
✔️ Does NOT tell rate or mechanism of reaction

2️⃣ #THERMODYNAMICSYSTEM
✔️ Part of universe under study
📌 Types:
✔️ Open system → exchanges mass + energy
✔️ Closed system → exchanges only energy
✔️ Isolated system → no exchange

3️⃣ #SURROUNDINGS
✔️ Rest of universe except system
📌 Universe = System + Surroundings

4️⃣ #STATEFUNCTION
✔️ Depends only on initial & final state
✔️ Path independent
📌 Examples:
✔️ Internal energy (U)
✔️ Enthalpy (H)
✔️ Entropy (S)

5️⃣ #PATHFUNCTION
✔️ Depends on path followed
📌 Examples:
✔️ Heat (q)
✔️ Work (w)

6️⃣ #ZEROTHLAWOFTHERMODYNAMICS
✔️ If A is in thermal equilibrium with B
✔️ And B is in thermal equilibrium with C
✔️ Then A is also in thermal equilibrium with C
📌 Basis of temperature measurement

7️⃣ #FIRSTLAWOFTHERMODYNAMICS (VERY IMP )
✔️ Law of conservation of energy
✔️ Energy cannot be created or destroyed
📌 Mathematical form:
ΔU = q + w
✔️ ΔU = change in internal energy
✔️ q = heat absorbed by system
✔️ w = work done on system

8️⃣ #SIGNCONVENTION (NEET ⚠️)
✔️ Heat absorbed → q = +ve
✔️ Heat released → q = –ve
✔️ Work done on system → w = +ve
✔️ Work done by system → w = –ve

9️⃣ #WORKDONEINGASEXPANSION
✔️ w = –PΔV
📌 Expansion (ΔV +ve) → w –ve
📌 Compression (ΔV –ve) → w +ve

🔟 #SPECIALCASES
✔️ At constant volume
w = 0
ΔU = q
✔️ At constant pressure
qₚ = ΔH

1️⃣1️⃣ #ENTHALPY
✔️ Heat content of system
✔️ H = U + PV
📌 Change in enthalpy:
ΔH = ΔU + Δ(PV)

1️⃣2️⃣ #SECONDLAWOFTHERMODYNAMICS
✔️ Natural processes occur in direction of increase in entropy
✔️ Total entropy of universe always increases
📌 ΔS(universe) > 0 → spontaneous
📌 ΔS(universe) = 0 → equilibrium

1️⃣3️⃣ #ENTROPY
✔️ Measure of randomness or disorder
✔️ Higher disorder → higher entropy
📌 Solid < Liquid < Gas

1️⃣4️⃣ #GIBBSFREEENERGY ( IMPORTANT )
✔️ G = H – TS
📌 Change in Gibbs energy:
ΔG = ΔH – TΔS
✔️ ΔG < 0 → spontaneous
✔️ ΔG = 0 → equilibrium
✔️ ΔG > 0 → non-spontaneous

1️⃣5️⃣ #THIRDLAWOFTHERMODYNAMICS
✔️ Entropy of perfectly crystalline solid at 0 K is zero
📌 S = 0 at 0 K

1️⃣6️⃣ #NEETONELINERS
✔️ Internal energy is state function
✔️ Heat & work are path functions
✔️ First law is special case of energy conservation
✔️ Entropy predicts spontaneity
✔️ Gibbs energy decides feasibility

@Ayano1me @Neetugpoll @Neetugquiz

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301 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, edited 03:01

Chemistry booster series

Q1. Zeroth Law
Assertion (A): If two systems are separately in thermal equilibrium with a third system, they are in thermal equilibrium with each other.
Reason (R): All systems in thermal equilibrium have the same temperature.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true

Q2. First Law
Assertion (A): Internal energy of an isolated system remains constant.
Reason (R): Energy can neither be created nor destroyed, only converted from one form to another.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true

Q3. Second Law
Assertion (A): Heat cannot spontaneously flow from a colder body to a hotter body.
Reason (R): Total entropy of an isolated system always increases for a spontaneous process.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true

Q4. Third Law
Assertion (A): Entropy of a perfectly crystalline substance is zero at absolute zero temperature.
Reason (R): At absolute zero, only one microstate is possible.
(1) A & R both true and R is correct explanation
(2) A & R both true but R is not correct explanation
(3) A true, R false
(4) A false, R true

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277 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, 03:02

Chemistry booster series

⭐ 𝗖𝗜𝗘 𝗪EE (𝗗𝗡, 𝗗𝗝, 𝗠𝗝 𝗦𝗧𝗔𝗥, 𝗠𝗞𝗚 & so on) 𝟮𝟬𝟮𝟲

⭐ 𝗢𝗟𝗗 𝗟𝗘𝗖𝗧𝗨𝗥𝗘𝗦 — 𝗨𝗡𝗗𝗠𝗬 + 𝗟𝗡 𝗞@𝗧𝗔 + 𝗦@𝗩@𝗠 + 𝗢𝗧𝗛𝗘𝗥 𝗧𝗢𝗣 𝗧𝗘𝗔𝗖𝗛𝗘𝗥𝗦

⭐ 𝗨𝗡𝗗𝗠𝗬 (𝗧𝗡𝗠, 𝗥𝗗, 𝗬𝗦𝗬, 𝗔𝗖𝗜𝗗, 𝗦𝗧 𝗦𝗜𝗥, 𝗜𝗡𝗦𝗔𝗙 𝗔𝗟𝗜 𝗦𝗜𝗥 & So On ) 𝟮𝟬𝟮𝟲

⭐ 𝗦@𝗩@𝗠 (𝗔𝗚 𝗦𝗜𝗥, 𝗔𝗦𝗛𝗜𝗦𝗛 𝗕𝗔𝗝𝗣𝗘𝗬𝗜 𝗦𝗜𝗥, 𝗣𝗔𝗥𝗩𝗘𝗭 𝗞𝗛𝗔𝗡, 𝗩𝗞
𝗦𝗜𝗥 & 𝗦𝗢 𝗢𝗡) 𝟮𝟬𝟮𝟲

⭐ 𝗖𝗢𝗣𝗬𝗥𝗜𝗚𝗛𝗧 𝗕𝗔𝗖𝗞𝗨𝗣 𝗢𝗙 𝗔𝗟𝗟 𝗢𝗙 𝗧𝗛𝗜𝗦

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303 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, 03:23

Chemistry booster series

⭐ 𝗖𝗜𝗘 𝗪EE (𝗗𝗡, 𝗗𝗝, 𝗠𝗝 𝗦𝗧𝗔𝗥, 𝗠𝗞𝗚 & so on) 𝟮𝟬𝟮𝟲 ⭐ 𝗢𝗟𝗗 𝗟𝗘𝗖𝗧𝗨𝗥𝗘𝗦 — 𝗨𝗡𝗗𝗠𝗬 + 𝗟𝗡 𝗞@𝗧𝗔 + 𝗦@𝗩@𝗠 + 𝗢𝗧𝗛𝗘𝗥 𝗧𝗢𝗣 𝗧𝗘𝗔𝗖𝗛𝗘𝗥𝗦 ⭐ 𝗨𝗡𝗗𝗠𝗬 (𝗧𝗡𝗠, 𝗥𝗗, 𝗬𝗦𝗬, 𝗔𝗖𝗜𝗗, 𝗦𝗧 𝗦𝗜𝗥, 𝗜𝗡𝗦𝗔𝗙 𝗔𝗟𝗜 𝗦𝗜𝗥 & So On ) 𝟮𝟬𝟮𝟲 ⭐ 𝗦@𝗩@𝗠 (𝗔𝗚 𝗦𝗜𝗥, 𝗔𝗦𝗛𝗜𝗦𝗛 𝗕𝗔𝗝𝗣𝗘𝗬𝗜 𝗦𝗜𝗥, 𝗣𝗔𝗥𝗩𝗘𝗭 𝗞𝗛𝗔𝗡, 𝗩𝗞 𝗦𝗜𝗥 & 𝗦𝗢 𝗢𝗡) 𝟮𝟬𝟮𝟲 ⭐ 𝗖𝗢𝗣𝗬𝗥𝗜𝗚𝗛𝗧…

Join kr lena all bcz in sbke full lec + crash course+ handwriting notes +short notes + test All in one milega

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246 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, 05:00

Chemistry booster series

1️⃣ #GIBBSFREEENERGY
✔️ Thermodynamic state function
✔️ Determines spontaneity of process
✔️ Denoted by G
📌 Relation:
G = H − TS

2️⃣ #TERMSINFORMULA
✔️ H → Enthalpy
✔️ T → Absolute temperature (K)
✔️ S → Entropy
📌 Unit of G → Joule

3️⃣ #CHANGEINGIBBSENERGY
📌 Formula:
ΔG = ΔH − TΔS
✔️ Applies at constant T & P

4️⃣ #SIGNIFICANCEOFΔG (VERY IMP )
✔️ ΔG < 0 → Spontaneous process
✔️ ΔG = 0 → Equilibrium
✔️ ΔG > 0 → Non-spontaneous

5️⃣ #CASESBASEDONΔHANDΔS
✔️ ΔH < 0 and ΔS > 0
Process spontaneous at all temperatures
✔️ ΔH > 0 and ΔS < 0
Process non-spontaneous at all temperatures
✔️ ΔH < 0 and ΔS < 0
Spontaneous at low temperature
✔️ ΔH > 0 and ΔS > 0
Spontaneous at high temperature

6️⃣ #TEMPERATUREEFFECT
✔️ Increase in T increases importance of entropy term
✔️ TΔS dominates at high temperature

7️⃣ #GIBBSENERGYATEQUILIBRIUM
✔️ At equilibrium:
ΔG = 0
📌 Relation with equilibrium constant:
ΔG° = −RT ln K

8️⃣ #STANDARDGIBBSFREEENERGY
✔️ Measured at:
✔️ 1 bar pressure
✔️ 298 K temperature
📌 Formula:
ΔG° = ΔH° − TΔS°

9️⃣ #REACTIONQUOTIENTRELATION
📌 Formula:
ΔG = ΔG° + RT ln Q
✔️ Q = reaction quotient
📌 At equilibrium Q = K

🔟 #MAXIMUMWORKCONCEPT
✔️ ΔG gives maximum non-expansion work
✔️ Useful in electrochemistry
📌 Electrical work = −ΔG

1️⃣1️⃣ #GIBBSENERGYINELECTROCHEMISTRY
📌 Relation:
ΔG° = −nFE°
✔️ n = number of electrons
✔️ F = Faraday constant
✔️ E° = standard emf

1️⃣2️⃣ #UNITSOFΔG
✔️ Joule
✔️ kJ mol⁻¹ (mostly used in chemistry)

1️⃣3️⃣ #NEET
✔️ ΔG decides feasibility, not rate
✔️ Spontaneous ≠ fast
✔️ ΔG depends on T, P & composition
✔️ ΔG is state function

1️⃣4️⃣ #ONELINEREVISION
✔️ Gibbs free energy predicts spontaneity
✔️ ΔG = 0 at equilibrium
✔️ Negative ΔG → feasible process
✔️ ΔG° related to K and E°

🔥2👍1😍1

264 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, 09:20

Chemistry booster series

⭐ 𝗖𝗜𝗘 𝗪EE 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 (𝗗𝗡, 𝗗𝗝, 𝗠𝗝 𝗦𝗧𝗔𝗥, 𝗠𝗞𝗚 & so on) 𝟮𝟬𝟮𝟲

⭐ 𝗢𝗟𝗗 𝗟𝗘𝗖𝗧𝗨𝗥𝗘𝗦 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘— 𝗨𝗡𝗗𝗠𝗬 + 𝗟𝗡 𝗞@𝗧𝗔 + 𝗦@𝗩@𝗠 + 𝗢𝗧𝗛𝗘𝗥 𝗧𝗢𝗣 𝗧𝗘𝗔𝗖𝗛𝗘𝗥𝗦

⭐ 𝗨𝗡𝗗𝗠𝗬 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 (𝗧𝗡𝗠, 𝗥𝗗, 𝗬𝗦𝗬, 𝗔𝗖𝗜𝗗, 𝗦𝗧 𝗦𝗜𝗥, 𝗜𝗡𝗦𝗔𝗙 𝗔𝗟𝗜 𝗦𝗜𝗥 & So On ) 𝟮𝟬𝟮𝟲

⭐ 𝗦@𝗩@𝗠 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘(𝗔𝗚 𝗦𝗜𝗥, 𝗔𝗦𝗛𝗜𝗦𝗛 𝗕𝗔𝗝𝗣𝗘𝗬𝗜 𝗦𝗜𝗥, 𝗣𝗔𝗥𝗩𝗘𝗭 𝗞𝗛𝗔𝗡, 𝗩𝗞
𝗦𝗜𝗥 & 𝗦𝗢 𝗢𝗡) 𝟮𝟬𝟮𝟲

⭐ 𝗖𝗢𝗣𝗬𝗥𝗜𝗚𝗛𝗧 𝗕𝗔𝗖𝗞𝗨𝗣 𝗢𝗙 𝗔𝗟𝗟𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 𝗢𝗙 𝗧𝗛𝗜𝗦

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282 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, 09:21

Chemistry booster series

⭐ 𝗖𝗜𝗘 𝗪EE 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 (𝗗𝗡, 𝗗𝗝, 𝗠𝗝 𝗦𝗧𝗔𝗥, 𝗠𝗞𝗚 & so on) 𝟮𝟬𝟮𝟲 ⭐ 𝗢𝗟𝗗 𝗟𝗘𝗖𝗧𝗨𝗥𝗘𝗦 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘— 𝗨𝗡𝗗𝗠𝗬 + 𝗟𝗡 𝗞@𝗧𝗔 + 𝗦@𝗩@𝗠 + 𝗢𝗧𝗛𝗘𝗥 𝗧𝗢𝗣 𝗧𝗘𝗔𝗖𝗛𝗘𝗥𝗦 ⭐ 𝗨𝗡𝗗𝗠𝗬 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 (𝗧𝗡𝗠, 𝗥𝗗, 𝗬𝗦𝗬, 𝗔𝗖𝗜𝗗, 𝗦𝗧 𝗦𝗜𝗥, 𝗜𝗡𝗦𝗔𝗙 𝗔𝗟𝗜 𝗦𝗜𝗥 & So On ) 𝟮𝟬𝟮𝟲 ⭐ 𝗦@𝗩@𝗠 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘(𝗔𝗚 𝗦𝗜𝗥, 𝗔𝗦𝗛𝗜𝗦𝗛 𝗕𝗔𝗝𝗣𝗘𝗬𝗜…

Join kr lena all bcz in sbke full lec + crash course+ handwriting notes +short notes + test All in one milega
Haar batch ka even more then batch content

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335 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, 09:21

Chemistry booster series

Q1.
Assertion (A): For a spontaneous process at constant temperature and pressure, ΔG is negative.
Reason (R): Spontaneous processes occur with decrease in Gibbs free energy.
Options:
(1) A & R true, R correct explanation
(2) A & R true, R not explanation
(3) A true, R false
(4) A false, R true

Q2.
Assertion (A): When ΔG = 0, the system is at equilibrium.
Reason (R): At equilibrium, forward and backward reaction rates are equal

Q3.
Assertion (A): A reaction with ΔH < 0 and ΔS < 0 is spontaneous at all temperatures.
Reason (R): Decrease in enthalpy always favours spontaneity.

Q5. (Numerical concept)
Assertion (A): If ΔH = −40 kJ and ΔS = −100 J K⁻¹, reaction is spontaneous at low temperature.
Reason (R): Negative ΔS disfavors spontaneity at high temperature

🕊1😍1🐳1

305 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, 09:23

Chemistry booster series

https://t.me/+Ea3TDyh0GIw5OTg0

𝙎𝙩𝙪𝙙𝙮 𝙁𝙤𝙧𝙜𝙚 chat

You’ve been invited to join this group on Telegram.

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237 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, 13:16

Chemistry booster series

❤2🔥1🙏1

328 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, 15:50

Chemistry booster series

⭐ 𝗖𝗜𝗘 𝗪EE 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 (𝗗𝗡, 𝗗𝗝, 𝗠𝗝 𝗦𝗧𝗔𝗥, 𝗠𝗞𝗚 & so on) 𝟮𝟬𝟮𝟲 ⭐ 𝗢𝗟𝗗 𝗟𝗘𝗖𝗧𝗨𝗥𝗘𝗦 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘— 𝗨𝗡𝗗𝗠𝗬 + 𝗟𝗡 𝗞@𝗧𝗔 + 𝗦@𝗩@𝗠 + 𝗢𝗧𝗛𝗘𝗥 𝗧𝗢𝗣 𝗧𝗘𝗔𝗖𝗛𝗘𝗥𝗦 ⭐ 𝗨𝗡𝗗𝗠𝗬 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘 (𝗧𝗡𝗠, 𝗥𝗗, 𝗬𝗦𝗬, 𝗔𝗖𝗜𝗗, 𝗦𝗧 𝗦𝗜𝗥, 𝗜𝗡𝗦𝗔𝗙 𝗔𝗟𝗜 𝗦𝗜𝗥 & So On ) 𝟮𝟬𝟮𝟲 ⭐ 𝗦@𝗩@𝗠 𝗗𝗥𝗘𝗔𝗠 𝗙𝗢𝗥𝗚𝗘(𝗔𝗚 𝗦𝗜𝗥, 𝗔𝗦𝗛𝗜𝗦𝗛 𝗕𝗔𝗝𝗣𝗘𝗬𝗜…

Krdo request send jisko bhi need ho bcz ab iske baad link nhi krunga m upload 3 baar copyright aa gya h inme
Link night 12 pr delete

❤‍🔥4❤2🥰1

283 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, 15:50

Chemistry booster series

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

❤3👍2👌2💯1

346 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, 08:06

Chemistry booster series

⃣ #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

❤2💯2😎1

283 views𝘼𝙮𝙖𝙣𝙤𝙠𝙤𝙟𝙞 🇮🇳, 06:02

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