#ELECTROMAGNETICRADIATION
Electromagnetic radiation is a form of energy propagated as waves with electric and magnetic fields oscillating perpendicular to each other.
#️⃣ 1️⃣ Characteristics of EM Radiation
⭐ Wave Nature
✔️ Travels in space as waves
✔️ Characterized by wavelength (λ), frequency (ν), speed (c)
✔️ Relationship: c = λν
⭐ Particle Nature
✔️ Light also behaves as particles (photons)
✔️ Energy of photon: E = hν
✔️ Momentum of photon: p = h/λ
📌 Constants
✔️ h = Planck’s constant = 6.626 × 10⁻³⁴ J·s
✔️ c = speed of light = 3 × 10⁸ m/s
📌 Constants
✔️ h = Planck’s constant = 6.626 × 10⁻³⁴ J·s
✔️ c = speed of light = 3 × 10⁸ m/s
2#TypesofElectromagneticRadiation (NCERT)
📌 Order of increasing wavelength / decreasing frequency:
γ-rays < X-rays < UV < Visible < IR < Microwaves < Radio waves
✔️ UV, Visible, IR → Important in Atomic Spectra
3️⃣ #ImportantRelations (Atom Chapter)
✔️ Energy of photon: E = hν = hc/λ
✔️ Frequency & wavelength inversely proportional: ν = c/λ
4️⃣ #NEETIMPORTANTPOINTS ⭐
✔️ EM radiation has dual nature → wave + particle
✔️ Wave nature → explains interference, diffraction, refraction
✔️ Particle nature → explains photoelectric effect, Compton effect
✔️ Photon energy proportional to frequency (E ∝ ν)
@Ayano1me @Neetugpoll @Neetugquiz
Electromagnetic radiation is a form of energy propagated as waves with electric and magnetic fields oscillating perpendicular to each other.
#️⃣ 1️⃣ Characteristics of EM Radiation
⭐ Wave Nature
✔️ Travels in space as waves
✔️ Characterized by wavelength (λ), frequency (ν), speed (c)
✔️ Relationship: c = λν
⭐ Particle Nature
✔️ Light also behaves as particles (photons)
✔️ Energy of photon: E = hν
✔️ Momentum of photon: p = h/λ
📌 Constants
✔️ h = Planck’s constant = 6.626 × 10⁻³⁴ J·s
✔️ c = speed of light = 3 × 10⁸ m/s
📌 Constants
✔️ h = Planck’s constant = 6.626 × 10⁻³⁴ J·s
✔️ c = speed of light = 3 × 10⁸ m/s
2#TypesofElectromagneticRadiation (NCERT)
📌 Order of increasing wavelength / decreasing frequency:
γ-rays < X-rays < UV < Visible < IR < Microwaves < Radio waves
✔️ UV, Visible, IR → Important in Atomic Spectra
3️⃣ #ImportantRelations (Atom Chapter)
✔️ Energy of photon: E = hν = hc/λ
✔️ Frequency & wavelength inversely proportional: ν = c/λ
4️⃣ #NEETIMPORTANTPOINTS ⭐
✔️ EM radiation has dual nature → wave + particle
✔️ Wave nature → explains interference, diffraction, refraction
✔️ Particle nature → explains photoelectric effect, Compton effect
✔️ Photon energy proportional to frequency (E ∝ ν)
@Ayano1me @Neetugpoll @Neetugquiz
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#PBLOCK ELEMENTSGROUP 14 (CARBON FAMILY)
Elements: C, Si, Ge, Sn, Pb
✔️ General electronic configuration: ns² np²
✔️ Valency: 4
✔️ Oxidation states: +4, +2
📌 Stability of +2 state increases down the group (inert pair effect)
1️⃣ #PHYSICALPROPERTIES
⭐ Atomic & Ionic Radii
✔️ Increases down the group (C < Si < Ge < Sn < Pb)
⭐ Ionisation Enthalpy
✔️ Decreases down the group
📌 Carbon has very high IE → strong covalent bonding
⭐ Electronegativity
✔️ Decreases down the group
📌 C highest, Pb lowest
⭐ Catenation (NEET HOT 🔥)
✔️ Ability to form long chains
📌 Order: C >> Si > Ge > Sn > Pb
📌 Strong C–C bond + small size
2️⃣ #ALLOTROPY
⭐ Carbon Allotropes
✔️ Crystalline → Diamond, Graphite, Fullerene
✔️ Amorphous → Coal, Coke, Charcoal
📌 Diamond
✔️ sp³ hybridised
✔️ Hardest substance
✔️ Electrical insulator
📌 Graphite
✔️ sp² hybridised
✔️ Good conductor of electricity
✔️ Layered structure
3️⃣ #CHEMICALPROPERTIES
⭐ Oxidation States
✔️ C, Si → mainly +4
✔️ Ge, Sn, Pb → +2 & +4
📌 +2 becomes more stable down the group (inert pair effect)
⭐ Inert Pair Effect
✔️ ns² electrons do not participate in bonding
📌 Maximum in Pb → Pb²⁺ more stable than Pb⁴⁺
4️⃣ #HYDRIDES (EH₄)
✔️ CH₄, SiH₄, GeH₄, SnH₄
📌 Trend:
✔️ Thermal stability ↓ down the group
✔️ Reducing character ↑ down the group
5️⃣ #HALIDES (MX₄ / MX₂)
⭐ Tetrahalides (MX₄)
✔️ CCl₄, SiCl₄ → covalent
✔️ Stability ↓ down the group
⭐ Dihalides (MX₂)
✔️ SnCl₂, PbCl₂ → more stable down the group
📌 Due to inert pair effect
📌 PbCl₄ unstable, PbCl₂ stable
6️⃣ #OXIDES (IMPORTANT 🔥)
✔️ CO₂, SiO₂ → Acidic
✔️ GeO₂ → Weakly acidic
✔️ SnO₂ → Amphoteric
✔️ PbO → Amphoteric / basic
📌 Acidity decreases down the group
7️⃣ #CARBONSPECIALCASE
⭐ Shows maximum catenation
⭐ Forms multiple bonds (C=C, C≡C)
⭐ Large number of organic compounds
⭐ No d-orbitals → strong π bonding
8️⃣ #COMPARISON ( NEET MCQ)
Property :Carbon :Lead
Catenation :Maximum :Negligible
Oxidation state :+4 :+2 more stable
Nature of oxide :Acidic :Amphoteric
Inert pair effect :Absent :Maximum
⚠️ #NCERTLINES
❌ Pb⁴⁺ more stable than Pb²⁺ → WRONG
✔️ CCl₄ does NOT hydrolyse
✔️ SiCl₄ hydrolyses easily
✔️ Graphite conducts electricity, diamond does not
@Ayano1me @Neetugpoll @Neetugquiz
Elements: C, Si, Ge, Sn, Pb
✔️ General electronic configuration: ns² np²
✔️ Valency: 4
✔️ Oxidation states: +4, +2
📌 Stability of +2 state increases down the group (inert pair effect)
1️⃣ #PHYSICALPROPERTIES
⭐ Atomic & Ionic Radii
✔️ Increases down the group (C < Si < Ge < Sn < Pb)
⭐ Ionisation Enthalpy
✔️ Decreases down the group
📌 Carbon has very high IE → strong covalent bonding
⭐ Electronegativity
✔️ Decreases down the group
📌 C highest, Pb lowest
⭐ Catenation (NEET HOT 🔥)
✔️ Ability to form long chains
📌 Order: C >> Si > Ge > Sn > Pb
📌 Strong C–C bond + small size
2️⃣ #ALLOTROPY
⭐ Carbon Allotropes
✔️ Crystalline → Diamond, Graphite, Fullerene
✔️ Amorphous → Coal, Coke, Charcoal
📌 Diamond
✔️ sp³ hybridised
✔️ Hardest substance
✔️ Electrical insulator
📌 Graphite
✔️ sp² hybridised
✔️ Good conductor of electricity
✔️ Layered structure
3️⃣ #CHEMICALPROPERTIES
⭐ Oxidation States
✔️ C, Si → mainly +4
✔️ Ge, Sn, Pb → +2 & +4
📌 +2 becomes more stable down the group (inert pair effect)
⭐ Inert Pair Effect
✔️ ns² electrons do not participate in bonding
📌 Maximum in Pb → Pb²⁺ more stable than Pb⁴⁺
4️⃣ #HYDRIDES (EH₄)
✔️ CH₄, SiH₄, GeH₄, SnH₄
📌 Trend:
✔️ Thermal stability ↓ down the group
✔️ Reducing character ↑ down the group
5️⃣ #HALIDES (MX₄ / MX₂)
⭐ Tetrahalides (MX₄)
✔️ CCl₄, SiCl₄ → covalent
✔️ Stability ↓ down the group
⭐ Dihalides (MX₂)
✔️ SnCl₂, PbCl₂ → more stable down the group
📌 Due to inert pair effect
📌 PbCl₄ unstable, PbCl₂ stable
6️⃣ #OXIDES (IMPORTANT 🔥)
✔️ CO₂, SiO₂ → Acidic
✔️ GeO₂ → Weakly acidic
✔️ SnO₂ → Amphoteric
✔️ PbO → Amphoteric / basic
📌 Acidity decreases down the group
7️⃣ #CARBONSPECIALCASE
⭐ Shows maximum catenation
⭐ Forms multiple bonds (C=C, C≡C)
⭐ Large number of organic compounds
⭐ No d-orbitals → strong π bonding
8️⃣ #COMPARISON ( NEET MCQ)
Property :Carbon :Lead
Catenation :Maximum :Negligible
Oxidation state :+4 :+2 more stable
Nature of oxide :Acidic :Amphoteric
Inert pair effect :Absent :Maximum
⚠️ #NCERTLINES
❌ Pb⁴⁺ more stable than Pb²⁺ → WRONG
✔️ CCl₄ does NOT hydrolyse
✔️ SiCl₄ hydrolyses easily
✔️ Graphite conducts electricity, diamond does not
@Ayano1me @Neetugpoll @Neetugquiz
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Chemistry booster series pinned «𝗧𝗢𝗣 𝟮𝟬 𝗛𝗜𝗚𝗛 𝗪𝗘𝗜𝗚𝗛𝗧𝗔𝗚𝗘 𝗧𝗢𝗣𝗜𝗖𝗦 — 𝗖𝗛𝗘𝗠𝗜𝗦𝗧𝗥𝗬 ⭐ #𝗣𝗛𝗬𝗦𝗜𝗖𝗔𝗟𝗖𝗛𝗘𝗠𝗜𝗦𝗧𝗥𝗬 𝗖𝗛𝗔𝗣𝗧𝗘𝗥 𝟭: 𝗦𝗢𝗟𝗨𝗧𝗜𝗢𝗡 ⭐ 𝗜𝗗𝗘𝗔𝗟 𝗦𝗢𝗟𝗨𝗧𝗜𝗢𝗡 ⭐ 𝗖𝗢𝗟𝗟𝗜𝗚𝗔𝗧𝗜𝗩𝗘 𝗣𝗥𝗢𝗣𝗘𝗥𝗧𝗜𝗘𝗦 𝗖𝗛𝗔𝗣𝗧𝗘𝗥 𝟮𝗘𝗟𝗘𝗖𝗧𝗥𝗢𝗖𝗛𝗘𝗠𝗜𝗦𝗧𝗥𝗬 ⭐ 𝗡𝗘𝗥𝗡𝗦𝗧 𝗘𝗤𝗨𝗔𝗧𝗜𝗢𝗡 ⭐ 𝗖𝗢𝗡𝗗𝗨𝗖𝗧𝗜𝗩𝗜𝗧𝗬 𝗖𝗛𝗔𝗣𝗧𝗘𝗥 𝟯: 𝗖𝗛𝗘𝗠𝗜𝗖𝗔𝗟 𝗞𝗜𝗡𝗘𝗧𝗜𝗖𝗦 ⭐ 𝗙𝗜𝗥𝗦𝗧 𝗢𝗥𝗗𝗘𝗥 𝗥𝗘𝗔𝗖𝗧𝗜𝗢𝗡𝗦 ⭐ 𝗔𝗥𝗥𝗛𝗘𝗡𝗜𝗨𝗦…»
Chemistry booster series
𝗧𝗢𝗣 𝟮𝟬 𝗛𝗜𝗚𝗛 𝗪𝗘𝗜𝗚𝗛𝗧𝗔𝗚𝗘 𝗧𝗢𝗣𝗜𝗖𝗦 — 𝗖𝗛𝗘𝗠𝗜𝗦𝗧𝗥𝗬 ⭐ #𝗣𝗛𝗬𝗦𝗜𝗖𝗔𝗟𝗖𝗛𝗘𝗠𝗜𝗦𝗧𝗥𝗬 𝗖𝗛𝗔𝗣𝗧𝗘𝗥 𝟭: 𝗦𝗢𝗟𝗨𝗧𝗜𝗢𝗡 ⭐ 𝗜𝗗𝗘𝗔𝗟 𝗦𝗢𝗟𝗨𝗧𝗜𝗢𝗡 ⭐ 𝗖𝗢𝗟𝗟𝗜𝗚𝗔𝗧𝗜𝗩𝗘 𝗣𝗥𝗢𝗣𝗘𝗥𝗧𝗜𝗘𝗦 𝗖𝗛𝗔𝗣𝗧𝗘𝗥 𝟮𝗘𝗟𝗘𝗖𝗧𝗥𝗢𝗖𝗛𝗘𝗠𝗜𝗦𝗧𝗥𝗬 ⭐ 𝗡𝗘𝗥𝗡𝗦𝗧 𝗘𝗤𝗨𝗔𝗧𝗜𝗢𝗡 ⭐ 𝗖𝗢𝗡𝗗𝗨𝗖𝗧𝗜𝗩𝗜𝗧𝗬 𝗖𝗛𝗔𝗣𝗧𝗘𝗥 𝟯: 𝗖𝗛𝗘𝗠𝗜𝗖𝗔𝗟 𝗞𝗜𝗡𝗘𝗧𝗜𝗖𝗦 ⭐ 𝗙𝗜𝗥𝗦𝗧 𝗢𝗥𝗗𝗘𝗥 𝗥𝗘𝗔𝗖𝗧𝗜𝗢𝗡𝗦 ⭐ 𝗔𝗥𝗥𝗛𝗘𝗡𝗜𝗨𝗦…
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#BOHRMODELOFHYDROGENATOM
Proposed by Niels Bohr (1913) to explain the line spectrum of hydrogen.
1. #POSTULATES OF BOHR MODEL
✔️ Atom has a small, positively charged nucleus at the centre
✔️ Electron revolves around nucleus in fixed circular orbits (stationary states)
✔️ Each orbit has a definite energy
✔️ Electron does not radiate energy while revolving in a permitted orbit
📌 Allowed orbits → n = 1, 2, 3, 4…
✔️ Angular momentum of electron is quantised:
📌 mvr = n(h / 2π)
2. #ENERGYOFELECTRON IN HYDROGEN ATOM
✔️ Energy of electron in nth orbit:
📌 Eₙ = −13.6 / n² eV
✔️ Negative sign → electron is bound to nucleus
📌 Ground state (n = 1):
E₁ = −13.6 eV
📌 Excited state (n > 1):
Energy becomes less negative
3. #RADIUSOFBOHRORBIT
✔️ Radius of nth orbit:
📌 rₙ = 0.529 × n² Å
📌 For ground state (n = 1):
r₁ = 0.529 Å
✔️ Radius increases as n²
4. #SPECTRALLINES (EMISSION & ABSORPTION)
✔️ Electron jumps from higher to lower orbit → emission of energy
✔️ Electron jumps from lower to higher orbit → absorption of energy
📌 Energy difference:
📌 ΔE = E₂ − E₁ = hν
5 #HYDROGENEMISSION SPECTRUM (IMPORTANT )
✔️ Spectrum consists of discrete lines
📌 Series based on final orbit:
Slines :Final n :Region
Lyman: 1 :UV
Balmer :2 :Visible
Paschen :3 :IR
Brackett :4 :IR
Pfund :5 :IR
📌 Balmer series → only visible series
6. #RYDBERGEQUATION
✔️ Explains wavelength of spectral lines:
📌 1/λ = R (1/n₁² − 1/n₂²)
✔️ n₂ > n₁
📌 R = 1.097 × 10⁷ m⁻¹
7. #SUCCESSOFBOHRMODEL
✔️ Explains hydrogen line spectrum
✔️ Explains stability of hydrogen atom
✔️ Gives correct values of energy & radius for H atom
8. #LIMITATIONSOFBOHRMODEL (VERY IMP ⚠️)
❌ Cannot explain spectra of multi-electron atoms
❌ Cannot explain Zeeman effect
❌ Cannot explain Stark effect
❌ Violates Heisenberg uncertainty principle
9. #NCERT ONELINEFACTS (NEET DIRECT)
✔️ Valid only for one-electron systems (H, He⁺, Li²⁺)
✔️ Energy levels are quantised
✔️ Lower n → more stability
✔️ Higher n → larger orbit, higher energy
#IMP
Electron radiates energy in stationary orbit → WRONG
✔️ Ground state has minimum energy
✔️ Transition n=3 → n=2 → Balmer series
@Ayano1me @Neetugpoll @Neetugquiz
Proposed by Niels Bohr (1913) to explain the line spectrum of hydrogen.
1. #POSTULATES OF BOHR MODEL
✔️ Atom has a small, positively charged nucleus at the centre
✔️ Electron revolves around nucleus in fixed circular orbits (stationary states)
✔️ Each orbit has a definite energy
✔️ Electron does not radiate energy while revolving in a permitted orbit
📌 Allowed orbits → n = 1, 2, 3, 4…
✔️ Angular momentum of electron is quantised:
📌 mvr = n(h / 2π)
2. #ENERGYOFELECTRON IN HYDROGEN ATOM
✔️ Energy of electron in nth orbit:
📌 Eₙ = −13.6 / n² eV
✔️ Negative sign → electron is bound to nucleus
📌 Ground state (n = 1):
E₁ = −13.6 eV
📌 Excited state (n > 1):
Energy becomes less negative
3. #RADIUSOFBOHRORBIT
✔️ Radius of nth orbit:
📌 rₙ = 0.529 × n² Å
📌 For ground state (n = 1):
r₁ = 0.529 Å
✔️ Radius increases as n²
4. #SPECTRALLINES (EMISSION & ABSORPTION)
✔️ Electron jumps from higher to lower orbit → emission of energy
✔️ Electron jumps from lower to higher orbit → absorption of energy
📌 Energy difference:
📌 ΔE = E₂ − E₁ = hν
5 #HYDROGENEMISSION SPECTRUM (IMPORTANT )
✔️ Spectrum consists of discrete lines
📌 Series based on final orbit:
Slines :Final n :Region
Lyman: 1 :UV
Balmer :2 :Visible
Paschen :3 :IR
Brackett :4 :IR
Pfund :5 :IR
📌 Balmer series → only visible series
6. #RYDBERGEQUATION
✔️ Explains wavelength of spectral lines:
📌 1/λ = R (1/n₁² − 1/n₂²)
✔️ n₂ > n₁
📌 R = 1.097 × 10⁷ m⁻¹
7. #SUCCESSOFBOHRMODEL
✔️ Explains hydrogen line spectrum
✔️ Explains stability of hydrogen atom
✔️ Gives correct values of energy & radius for H atom
8. #LIMITATIONSOFBOHRMODEL (VERY IMP ⚠️)
❌ Cannot explain spectra of multi-electron atoms
❌ Cannot explain Zeeman effect
❌ Cannot explain Stark effect
❌ Violates Heisenberg uncertainty principle
9. #NCERT ONELINEFACTS (NEET DIRECT)
✔️ Valid only for one-electron systems (H, He⁺, Li²⁺)
✔️ Energy levels are quantised
✔️ Lower n → more stability
✔️ Higher n → larger orbit, higher energy
#IMP
Electron radiates energy in stationary orbit → WRONG
✔️ Ground state has minimum energy
✔️ Transition n=3 → n=2 → Balmer series
@Ayano1me @Neetugpoll @Neetugquiz
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1️⃣ #PBLOCKGROUP15 ⭐ (Nitrogen Family / Pnictogens)
📌 Group members:
✔️ Nitrogen (N)
✔️ Phosphorus (P)
✔️ Arsenic (As)
✔️ Antimony (Sb)
✔️ Bismuth (Bi)
📌 General electronic configuration:
✔️ ns² np³
NEET point:
✔️ 5 valence electrons → trivalent nature common
2️⃣ #GENERALTRENDS ⭐
📌 Atomic & ionic size:
✔️ Increases down the group
📌 Ionisation enthalpy:
✔️ Decreases down the group
✔️ Nitrogen → highest (small size)
📌 Electronegativity:
✔️ Decreases down the group
📌 Metallic character:
✔️ Increases down the group
✔️ N & P → non-metals
✔️ As & Sb → metalloids
✔️ Bi → metal
3️⃣ #OXIDATIONSTATES ⭐
✔️ Common oxidation states: –3, +3, +5
📌 Trends:
✔️ –3 → stability decreases down the group
✔️ +5 → stability decreases down the group
✔️ +3 → stability increases down the group
🧠 Reason:
✔️ Inert pair effect increases down the group
📌 Examples:
✔️ N₂O₅ → +5 (stable)
✔️ Bi³⁺ → more stable than Bi⁵⁺
4️⃣ #HYDRIDES (NH₃ TYPE) ⭐
📌 General formula:
✔️ EH₃
📌 Bond angle:
✔️ NH₃ > PH₃ > AsH₃ > SbH₃ > BiH₃
📌 Basic nature:
✔️ NH₃ → most basic
✔️ Basicity decreases down the group
Reason:
✔️ Lone pair availability decreases
📌 Thermal stability:
✔️ Decreases down the group
5️⃣ #OXIDES ⭐
✔️ Form E₂O₃ and E₂O₅
📌 Nature of oxides:
✔️ N₂O₅, P₂O₅ → acidic
✔️ As₂O₃ → amphoteric
✔️ Bi₂O₃ → basic
Trend:
✔️ Acidic → basic character increases down the group
6️⃣ #HALIDES ⭐
📌 Trihalides (EX₃):
✔️ All elements form EX₃
📌 Pentahalides (EX₅):
✔️ Formed by P, As, Sb
✔️ Nitrogen ❌ (no d-orbitals)
✔️ Bi ❌ (inert pair effect)
Important:
✔️ PCl₅ → exists as solid (ionic) & gas (covalent)
7️⃣ #ANOMALOUSBEHAVIOUROFNITROGEN ⭐
✔️ Small size
✔️ High electronegativity
✔️ High ionisation enthalpy
✔️ Absence of d-orbitals
📌 Results:
✔️ N₂ has strong triple bond
✔️ Limited oxidation states
✔️ Different properties from rest of group
8️⃣ #IMPORTANTCOMPOUNDS
✔️ Ammonia (NH₃):
• Basic gas
• Forms hydrogen bonding
✔️ Phosphine (PH₃):
• Weak base
• Toxic gas
✔️ P₂O₅:
Strong dehydrating agent
#NEETTAKEAWAY
✔️ Inert pair effect → key to oxidation states
✔️ NH₃ strongest base in group
✔️ Acidic → basic oxide trend important
✔️ Nitrogen always exceptional
@Ayano1me @Neetugpoll @Neetugquiz
📌 Group members:
✔️ Nitrogen (N)
✔️ Phosphorus (P)
✔️ Arsenic (As)
✔️ Antimony (Sb)
✔️ Bismuth (Bi)
📌 General electronic configuration:
✔️ ns² np³
NEET point:
✔️ 5 valence electrons → trivalent nature common
2️⃣ #GENERALTRENDS ⭐
📌 Atomic & ionic size:
✔️ Increases down the group
📌 Ionisation enthalpy:
✔️ Decreases down the group
✔️ Nitrogen → highest (small size)
📌 Electronegativity:
✔️ Decreases down the group
📌 Metallic character:
✔️ Increases down the group
✔️ N & P → non-metals
✔️ As & Sb → metalloids
✔️ Bi → metal
3️⃣ #OXIDATIONSTATES ⭐
✔️ Common oxidation states: –3, +3, +5
📌 Trends:
✔️ –3 → stability decreases down the group
✔️ +5 → stability decreases down the group
✔️ +3 → stability increases down the group
🧠 Reason:
✔️ Inert pair effect increases down the group
📌 Examples:
✔️ N₂O₅ → +5 (stable)
✔️ Bi³⁺ → more stable than Bi⁵⁺
4️⃣ #HYDRIDES (NH₃ TYPE) ⭐
📌 General formula:
✔️ EH₃
📌 Bond angle:
✔️ NH₃ > PH₃ > AsH₃ > SbH₃ > BiH₃
📌 Basic nature:
✔️ NH₃ → most basic
✔️ Basicity decreases down the group
Reason:
✔️ Lone pair availability decreases
📌 Thermal stability:
✔️ Decreases down the group
5️⃣ #OXIDES ⭐
✔️ Form E₂O₃ and E₂O₅
📌 Nature of oxides:
✔️ N₂O₅, P₂O₅ → acidic
✔️ As₂O₃ → amphoteric
✔️ Bi₂O₃ → basic
Trend:
✔️ Acidic → basic character increases down the group
6️⃣ #HALIDES ⭐
📌 Trihalides (EX₃):
✔️ All elements form EX₃
📌 Pentahalides (EX₅):
✔️ Formed by P, As, Sb
✔️ Nitrogen ❌ (no d-orbitals)
✔️ Bi ❌ (inert pair effect)
Important:
✔️ PCl₅ → exists as solid (ionic) & gas (covalent)
7️⃣ #ANOMALOUSBEHAVIOUROFNITROGEN ⭐
✔️ Small size
✔️ High electronegativity
✔️ High ionisation enthalpy
✔️ Absence of d-orbitals
📌 Results:
✔️ N₂ has strong triple bond
✔️ Limited oxidation states
✔️ Different properties from rest of group
8️⃣ #IMPORTANTCOMPOUNDS
✔️ Ammonia (NH₃):
• Basic gas
• Forms hydrogen bonding
✔️ Phosphine (PH₃):
• Weak base
• Toxic gas
✔️ P₂O₅:
Strong dehydrating agent
#NEETTAKEAWAY
✔️ Inert pair effect → key to oxidation states
✔️ NH₃ strongest base in group
✔️ Acidic → basic oxide trend important
✔️ Nitrogen always exceptional
@Ayano1me @Neetugpoll @Neetugquiz
🔥3👌3❤1🕊1😍1
𝘾𝙝𝙚𝙢𝙞𝙨𝙩𝙧𝙮 𝙍𝙖𝙣𝙠 𝘽𝙤𝙤𝙨𝙩𝙚𝙧 𝙇𝙀𝙏’𝙎 𝘾𝙍𝘼𝘾𝙆 𝙄𝙏 𝙉𝙊𝙏𝙀𝙎 ⚕️ 𝙒𝙖𝙮 𝙩𝙤 𝙨𝙪𝙘𝙘𝙚𝙨𝙨:
1️⃣ #PERIODICCLASSIFICATIONOFELEMENTS ⭐
✔️ Elements ko increasing atomic number ke order me arrange karna
✔️ Purpose → study of properties in a systematic way
📌 Modern periodic law:
✔️ Physical & chemical properties of elements are periodic functions of their atomic numbers
#NEETpoint:
✔️ Atomic number (Z) is basis, not atomic mass
2️⃣ #HISTORICALDEVELOPMENT ⭐
✔️ Dobereiner’s Triads
• Middle element mass ≈ average of other two
✔️ Newlands’ Law of Octaves
• Every 8th element similar properties
✔️ Mendeleev’s Periodic Table
• Based on atomic mass
• Left gaps for undiscovered elements
✔️ Modern Periodic Table (Moseley)
• Based on atomic number
#NEETIMP
✔️ Anomalies of Mendeleev solved by modern table
3️⃣ #MODERNPERIODICTABLE ⭐
📌 Structure:
✔️ 7 periods (horizontal rows)
✔️ 18 groups (vertical columns)
📌 Blocks:
✔️ s-block
✔️ p-block
✔️ d-block
✔️ f-block
#NEETpoint:
✔️ Period number = highest principal quantum number (n)
4️⃣ #PERIODICITYINPROPERTIES ⭐
✔️ Repetition of properties at regular intervals
📌 Important properties:
✔️ Atomic radius
✔️ Ionisation enthalpy
✔️ Electron affinity
✔️ Electronegativity
✔️ Metallic & non-metallic character
5️⃣ #ATOMICRADIUS ⭐
📌 Trend:
✔️ Decreases across a period → left to right
✔️ Increases down a group
#Reason:
✔️ Effective nuclear charge ↑ across period
✔️ New shell added down the group
📌 Ionic radius:
✔️ Cation < atom
✔️ Anion > atom
6️⃣ #IONISATIONENTHALPY ⭐
✔️ Energy required to remove an electron
📌 Trend:
✔️ Increases across a period
✔️ Decreases down a group
#Exceptions (NEET favourite 🔥):
✔️ Be > B
✔️ N > O
7️⃣ #ELECTRONAFFINITY ⭐
✔️ Energy released when electron is added
📌 Trend:
✔️ Increases across a period
✔️ Decreases down a group
#NEETpoint:
✔️ Halogens → highest electron affinity
✔️ Noble gases → ~0
8️⃣ #ELECTRONEGATIVITY ⭐
✔️ Tendency to attract shared electron pair
📌 Trend:
✔️ Increases across a period
✔️ Decreases down a group
⭐NEETpoint:
✔️ Fluorine → most electronegative
9️⃣ #METALLICCHARACTER ⭐
📌 Trend:
✔️ Decreases across a period
✔️ Increases down a group
⭐NEETclarity:
✔️ Metals → lose electrons
✔️ Non-metals → gain electrons
🔟 #ANOMALOUSBEHAVIOUR ⭐
✔️ First element of each group shows different properties
📌 Reason:
✔️ Small size
✔️ High electronegativity
✔️ Absence of d-orbitals
⭐Example:
✔️ Li ≠ Na
✔️ Be ≠ Mg
1️⃣1️⃣ #NEETONELINERS🔥
✔️ Basis of modern periodic table → atomic number
✔️ Periodicity due to electronic configuration
✔️ s-block → highly electropositive
✔️ p-block → variable oxidation states
✔️ d-block → transition elements
1️⃣2️⃣ #SUMMARY ⭐
✔️ Periodic table = map of chemistry
✔️ Trends help predict properties
✔️ Exceptions are more important for NEET
@Ayano1me @Neetugpoll @Neetugquiz
1️⃣ #PERIODICCLASSIFICATIONOFELEMENTS ⭐
✔️ Elements ko increasing atomic number ke order me arrange karna
✔️ Purpose → study of properties in a systematic way
📌 Modern periodic law:
✔️ Physical & chemical properties of elements are periodic functions of their atomic numbers
#NEETpoint:
✔️ Atomic number (Z) is basis, not atomic mass
2️⃣ #HISTORICALDEVELOPMENT ⭐
✔️ Dobereiner’s Triads
• Middle element mass ≈ average of other two
✔️ Newlands’ Law of Octaves
• Every 8th element similar properties
✔️ Mendeleev’s Periodic Table
• Based on atomic mass
• Left gaps for undiscovered elements
✔️ Modern Periodic Table (Moseley)
• Based on atomic number
#NEETIMP
✔️ Anomalies of Mendeleev solved by modern table
3️⃣ #MODERNPERIODICTABLE ⭐
📌 Structure:
✔️ 7 periods (horizontal rows)
✔️ 18 groups (vertical columns)
📌 Blocks:
✔️ s-block
✔️ p-block
✔️ d-block
✔️ f-block
#NEETpoint:
✔️ Period number = highest principal quantum number (n)
4️⃣ #PERIODICITYINPROPERTIES ⭐
✔️ Repetition of properties at regular intervals
📌 Important properties:
✔️ Atomic radius
✔️ Ionisation enthalpy
✔️ Electron affinity
✔️ Electronegativity
✔️ Metallic & non-metallic character
5️⃣ #ATOMICRADIUS ⭐
📌 Trend:
✔️ Decreases across a period → left to right
✔️ Increases down a group
#Reason:
✔️ Effective nuclear charge ↑ across period
✔️ New shell added down the group
📌 Ionic radius:
✔️ Cation < atom
✔️ Anion > atom
6️⃣ #IONISATIONENTHALPY ⭐
✔️ Energy required to remove an electron
📌 Trend:
✔️ Increases across a period
✔️ Decreases down a group
#Exceptions (NEET favourite 🔥):
✔️ Be > B
✔️ N > O
7️⃣ #ELECTRONAFFINITY ⭐
✔️ Energy released when electron is added
📌 Trend:
✔️ Increases across a period
✔️ Decreases down a group
#NEETpoint:
✔️ Halogens → highest electron affinity
✔️ Noble gases → ~0
8️⃣ #ELECTRONEGATIVITY ⭐
✔️ Tendency to attract shared electron pair
📌 Trend:
✔️ Increases across a period
✔️ Decreases down a group
⭐NEETpoint:
✔️ Fluorine → most electronegative
9️⃣ #METALLICCHARACTER ⭐
📌 Trend:
✔️ Decreases across a period
✔️ Increases down a group
⭐NEETclarity:
✔️ Metals → lose electrons
✔️ Non-metals → gain electrons
🔟 #ANOMALOUSBEHAVIOUR ⭐
✔️ First element of each group shows different properties
📌 Reason:
✔️ Small size
✔️ High electronegativity
✔️ Absence of d-orbitals
⭐Example:
✔️ Li ≠ Na
✔️ Be ≠ Mg
1️⃣1️⃣ #NEETONELINERS🔥
✔️ Basis of modern periodic table → atomic number
✔️ Periodicity due to electronic configuration
✔️ s-block → highly electropositive
✔️ p-block → variable oxidation states
✔️ d-block → transition elements
1️⃣2️⃣ #SUMMARY ⭐
✔️ Periodic table = map of chemistry
✔️ Trends help predict properties
✔️ Exceptions are more important for NEET
@Ayano1me @Neetugpoll @Neetugquiz
❤4🕊2🎉1🤩1🙏1💘1
Q1. (Assertion–Reason type)
Assertion (A): Atomic radius generally decreases from left to right in a period.
Reason (R): Nuclear charge increases while number of shells remains same.
Options:
(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.
Which element has maximum electronegativity?
(1) Oxygen
(2) Nitrogen
(3) Fluorine
(4) Chlorine
Question:3 Which of the following has largest atomic size?
(1) Na
(2) Mg
(3) Al
(4) Si
Question 4
Assertion (A): Ionization enthalpy generally increases from left to right in a period.
Reason (R): Atomic size decreases and nuclear charge increases across a period.
(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
Question:5
Assertion (A): Electron affinity of halogens is high.
Reason (R): Halogens have one electron less than noble gas configuration.
(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
Question:6
Assertion (A): Metallic character increases down a group.
Reason (R): Atomic size increases and ionization enthalpy decreases down the group.
(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
🔥3🥰3🤩1
1️⃣ #DUALBEHAVIOUROFMATTER ⭐
✔️ Matter shows dual nature:
👉 Particle nature
👉 Wave nature
✔️ This concept proved that classical physics fails at atomic scale
NEET point:
✔️ Dual behaviour mainly observed for microscopic particles (electron, proton)
2️⃣ #PARTICLENATUREOFMATTER ⭐
✔️ Matter consists of discrete particles
✔️ Particle nature supported by:
👉 Photoelectric effect
👉 Compton effect
📌 Evidence:
✔️ Emission of electrons only when threshold frequency is reached
3️⃣ #WAVENATUREOFMATTER ⭐
✔️ Proposed by de Broglie
✔️ Every moving particle behaves like a wave
📌 de Broglie hypothesis:
✔️ λ ∝ 1/p
📌 de Broglie wavelength:
✔️ λ = h / mv
Where:
✔️ h = Planck’s constant
✔️ m = mass
✔️ v = velocity
NEET point:
✔️ Wave nature important for electrons
4️⃣ #ELECTROMAGNETICRADIATION ⭐
✔️ Energy travels as waves
✔️ Does not require medium
📌 Examples:
✔️ Radio waves
✔️ Microwaves
✔️ Infrared
✔️ Visible light
✔️ UV, X-rays, γ-rays
📌 Relation:
✔️ c = νλ
5️⃣ #PHOTOELECTRICEFFECT ⚡ ⭐
✔️ Emission of electrons when light falls on metal surface
📌 Key observations:
✔️ Threshold frequency (ν₀) exists
✔️ No emission below ν₀
✔️ Intensity ↑ → number of electrons ↑
✔️ Frequency ↑ → kinetic energy ↑
📌 Einstein’s photoelectric equation:
✔️ hν = hν₀ + ½mv²
NEET trap
✔️ KE depends on frequency, NOT intensity
6️⃣ #WAVEPARTICLEDUALITY ⭐
✔️ Light behaves as:
👉 Wave → interference, diffraction
👉 Particle → photoelectric effect
✔️ Matter behaves as:
👉 Particle → mass, momentum
👉 Wave → de Broglie wavelength
NEET clarity:
✔️ Dual behaviour is complementary, not simultaneous
7️⃣ #IMPORTANCEOFDEBROGLIEWAVE ⭐
✔️ Basis of Bohr’s model modification
✔️ Explains stability of orbits
✔️ Used in electron microscope
📌 Special cases:
✔️ For electron (accelerated by V):
λ = h / √(2meV)
8️⃣ #NEETONELINERS
✔️ Dual nature → matter + radiation
✔️ Threshold frequency → metal dependent
✔️ de Broglie wavelength inversely ∝ velocity
✔️ Electron shows wave nature more clearly
9️⃣ #FORMULASUMMARY (MUST REVISE )
✔️ λ = h / mv
✔️ c = νλ
✔️ E = hν
✔️ hν = hν₀ + ½mv²
✔️ λ = h / √(2meV)
🔟 #REAL_SENSESUMMARY ⭐
✔️ Classical physics ❌ at atomic scale
✔️ Quantum ideas ✔️ required
✔️ Wave nature dominates for small particles
✔️ Foundation of modern chemistry & physics
@Ayano1me @Neetugpoll @Neetugquiz
✔️ Matter shows dual nature:
👉 Particle nature
👉 Wave nature
✔️ This concept proved that classical physics fails at atomic scale
NEET point:
✔️ Dual behaviour mainly observed for microscopic particles (electron, proton)
2️⃣ #PARTICLENATUREOFMATTER ⭐
✔️ Matter consists of discrete particles
✔️ Particle nature supported by:
👉 Photoelectric effect
👉 Compton effect
📌 Evidence:
✔️ Emission of electrons only when threshold frequency is reached
3️⃣ #WAVENATUREOFMATTER ⭐
✔️ Proposed by de Broglie
✔️ Every moving particle behaves like a wave
📌 de Broglie hypothesis:
✔️ λ ∝ 1/p
📌 de Broglie wavelength:
✔️ λ = h / mv
Where:
✔️ h = Planck’s constant
✔️ m = mass
✔️ v = velocity
NEET point:
✔️ Wave nature important for electrons
4️⃣ #ELECTROMAGNETICRADIATION ⭐
✔️ Energy travels as waves
✔️ Does not require medium
📌 Examples:
✔️ Radio waves
✔️ Microwaves
✔️ Infrared
✔️ Visible light
✔️ UV, X-rays, γ-rays
📌 Relation:
✔️ c = νλ
5️⃣ #PHOTOELECTRICEFFECT ⚡ ⭐
✔️ Emission of electrons when light falls on metal surface
📌 Key observations:
✔️ Threshold frequency (ν₀) exists
✔️ No emission below ν₀
✔️ Intensity ↑ → number of electrons ↑
✔️ Frequency ↑ → kinetic energy ↑
📌 Einstein’s photoelectric equation:
✔️ hν = hν₀ + ½mv²
NEET trap
✔️ KE depends on frequency, NOT intensity
6️⃣ #WAVEPARTICLEDUALITY ⭐
✔️ Light behaves as:
👉 Wave → interference, diffraction
👉 Particle → photoelectric effect
✔️ Matter behaves as:
👉 Particle → mass, momentum
👉 Wave → de Broglie wavelength
NEET clarity:
✔️ Dual behaviour is complementary, not simultaneous
7️⃣ #IMPORTANCEOFDEBROGLIEWAVE ⭐
✔️ Basis of Bohr’s model modification
✔️ Explains stability of orbits
✔️ Used in electron microscope
📌 Special cases:
✔️ For electron (accelerated by V):
λ = h / √(2meV)
8️⃣ #NEETONELINERS
✔️ Dual nature → matter + radiation
✔️ Threshold frequency → metal dependent
✔️ de Broglie wavelength inversely ∝ velocity
✔️ Electron shows wave nature more clearly
9️⃣ #FORMULASUMMARY (MUST REVISE )
✔️ λ = h / mv
✔️ c = νλ
✔️ E = hν
✔️ hν = hν₀ + ½mv²
✔️ λ = h / √(2meV)
🔟 #REAL_SENSESUMMARY ⭐
✔️ Classical physics ❌ at atomic scale
✔️ Quantum ideas ✔️ required
✔️ Wave nature dominates for small particles
✔️ Foundation of modern chemistry & physics
@Ayano1me @Neetugpoll @Neetugquiz
❤3🥰2🕊2💋2
1️⃣ #DIPOLEMOMENT
📌 Measure of polarity of a bond or molecule
2️⃣ #DEFINITION
✔️ Product of magnitude of charge (q) and distance (d) between centres of +ve and −ve charges
✔️ μ = q × d
✔️ Vector quantity
✔️ Direction → from negative to positive charge
3️⃣ #UNITS
✔️ SI unit → Coulomb metre (C·m)
✔️ Practical unit → Debye (D)
📌 1 Debye = 3.336 × 10⁻³⁰ C·m
4️⃣ #BONDDIPOLEMOMENT
✔️ Due to electronegativity difference
✔️ Greater ΔEN → greater dipole moment
📌 H–Cl > H–Br > H–I
5️⃣ #MOLECULARDIPOLEMOMENT
✔️ Vector sum of all bond dipoles
✔️ Depends on molecular shape & symmetry
6️⃣ #EFFECTOFSHAPE
✔️ Symmetrical molecule → μ = 0
✔️ Unsymmetrical molecule → μ ≠ 0
📌 Examples:
✔️ CO₂ → μ = 0 (linear)
✔️ BF₃ → μ = 0 (trigonal planar)
✔️ H₂O → μ ≠ 0 (bent)
✔️ NH₃ → μ ≠ 0 (pyramidal)
7️⃣ #APPLICATIONS
✔️ Polarity determination
✔️ Molecular geometry
✔️ Ionic character
✔️ Distinguishing cis–trans isomers
📌 cis → μ ≠ 0
📌 trans → μ = 0
8️⃣ #IMPORTANTNCERTPOINTS
✔️ Lone pair increases dipole moment
✔️ Symmetry can cancel dipole moment
✔️ Polar bonds may give zero μ
9️⃣ #NEETTRAPS
❌ Polar bond ≠ polar molecule
❌ Zero μ ≠ non-polar bonds
❌ Shape ignored = wrong answer
HF>HCL but ch3cl>ch3F ( DM)
@Ayano1me @Neetugpoll @Neetugquiz
📌 Measure of polarity of a bond or molecule
2️⃣ #DEFINITION
✔️ Product of magnitude of charge (q) and distance (d) between centres of +ve and −ve charges
✔️ μ = q × d
✔️ Vector quantity
✔️ Direction → from negative to positive charge
3️⃣ #UNITS
✔️ SI unit → Coulomb metre (C·m)
✔️ Practical unit → Debye (D)
📌 1 Debye = 3.336 × 10⁻³⁰ C·m
4️⃣ #BONDDIPOLEMOMENT
✔️ Due to electronegativity difference
✔️ Greater ΔEN → greater dipole moment
📌 H–Cl > H–Br > H–I
5️⃣ #MOLECULARDIPOLEMOMENT
✔️ Vector sum of all bond dipoles
✔️ Depends on molecular shape & symmetry
6️⃣ #EFFECTOFSHAPE
✔️ Symmetrical molecule → μ = 0
✔️ Unsymmetrical molecule → μ ≠ 0
📌 Examples:
✔️ CO₂ → μ = 0 (linear)
✔️ BF₃ → μ = 0 (trigonal planar)
✔️ H₂O → μ ≠ 0 (bent)
✔️ NH₃ → μ ≠ 0 (pyramidal)
7️⃣ #APPLICATIONS
✔️ Polarity determination
✔️ Molecular geometry
✔️ Ionic character
✔️ Distinguishing cis–trans isomers
📌 cis → μ ≠ 0
📌 trans → μ = 0
8️⃣ #IMPORTANTNCERTPOINTS
✔️ Lone pair increases dipole moment
✔️ Symmetry can cancel dipole moment
✔️ Polar bonds may give zero μ
9️⃣ #NEETTRAPS
❌ Polar bond ≠ polar molecule
❌ Zero μ ≠ non-polar bonds
❌ Shape ignored = wrong answer
HF>HCL but ch3cl>ch3F ( DM)
@Ayano1me @Neetugpoll @Neetugquiz
😍2❤1👍1🔥1🙏1
1️⃣ #VSEPRTHEORY
📌 VSEPR = Valence Shell Electron Pair Repulsion theory
📌 Used to predict shape of molecules and ions.
2️⃣ #BASICIDEA
✔️ Electron pairs in valence shell repel each other
✔️ They arrange themselves to minimise repulsion
✔️ Shape depends on number of electron pairs around central atom
3️⃣ #TYPESOFELECTRONPAIRS
✔️ Bond pair (BP) – shared electrons
✔️ Lone pair (LP) – unshared electrons
📌 Lone pair occupies more space than bond pair
4️⃣ #ORDEROFREPULSION (VERY IMP 🔥)
✔️ LP–LP > LP–BP > BP–BP
📌 This order decides distortion in shape
5️⃣ #ELECTRONGEOMETRYVS MOLECULARGEOMETRY
✔️ Electron geometry → arrangement of all electron pairs
✔️ Molecular geometry → arrangement of atoms only
📌 Lone pairs affect molecular shape, not electron geometry
6️⃣ #IDEALGEOMETRIES (NO LONE PAIR)
✔️ 2 BP → Linear → 180° → BeCl₂
✔️ 3 BP → Trigonal planar → 120° → BF₃
✔️ 4 BP → Tetrahedral → 109.5° → CH₄
✔️ 5 BP → Trigonal bipyramidal → PCl₅
✔️ 6 BP → Octahedral → SF₆
7️⃣ #EFFECTOFLONEPAIR
✔️ Lone pair reduces bond angle
✔️ More lone pairs → more deviation from ideal shape
📌 Examples:
✔️ CH₄ → 109.5°
✔️ NH₃ → 107°
✔️ H₂O → 104.5°
8️⃣ #SPECIALCASESTRIGONALBIPYRAMIDAL
✔️ Axial positions → more repulsion
✔️ Equatorial positions → less repulsion
📌 Lone pair occupies equatorial position first
📌 Example:
✔️ SF₄ → seesaw
✔️ ClF₃ → T-shape
✔️ XeF₂ → linear
9️⃣ #SPECIALCASEOFOCTAHEDRAL
✔️ One lone pair → square pyramidal
✔️ Two lone pairs → square planar
📌 Examples:
✔️ BrF₅ → square pyramidal
✔️ XeF₄ → square planar
🔟 #NEETIMPORTANTPOINTS 🚨
✔️ Lone pair causes maximum repulsion
✔️ Shape decided by LP + BP count
✔️ VSEPR explains shape, not bonding strength
✔️ Used mainly for p-block compounds
1️⃣1️⃣ #LIMITATIONSOFVSEPR
✔️ Cannot explain bond length accurately
✔️ Not applicable for transition metals
✔️ Fails for odd-electron molecules
1️⃣2️⃣ #ONELINEREVISION
Molecular shape is decided by repulsion between electron pairs around the central atom.
@Ayano1me @Neetugpoll @Neetugquiz
📌 VSEPR = Valence Shell Electron Pair Repulsion theory
📌 Used to predict shape of molecules and ions.
2️⃣ #BASICIDEA
✔️ Electron pairs in valence shell repel each other
✔️ They arrange themselves to minimise repulsion
✔️ Shape depends on number of electron pairs around central atom
3️⃣ #TYPESOFELECTRONPAIRS
✔️ Bond pair (BP) – shared electrons
✔️ Lone pair (LP) – unshared electrons
📌 Lone pair occupies more space than bond pair
4️⃣ #ORDEROFREPULSION (VERY IMP 🔥)
✔️ LP–LP > LP–BP > BP–BP
📌 This order decides distortion in shape
5️⃣ #ELECTRONGEOMETRYVS MOLECULARGEOMETRY
✔️ Electron geometry → arrangement of all electron pairs
✔️ Molecular geometry → arrangement of atoms only
📌 Lone pairs affect molecular shape, not electron geometry
6️⃣ #IDEALGEOMETRIES (NO LONE PAIR)
✔️ 2 BP → Linear → 180° → BeCl₂
✔️ 3 BP → Trigonal planar → 120° → BF₃
✔️ 4 BP → Tetrahedral → 109.5° → CH₄
✔️ 5 BP → Trigonal bipyramidal → PCl₅
✔️ 6 BP → Octahedral → SF₆
7️⃣ #EFFECTOFLONEPAIR
✔️ Lone pair reduces bond angle
✔️ More lone pairs → more deviation from ideal shape
📌 Examples:
✔️ CH₄ → 109.5°
✔️ NH₃ → 107°
✔️ H₂O → 104.5°
8️⃣ #SPECIALCASESTRIGONALBIPYRAMIDAL
✔️ Axial positions → more repulsion
✔️ Equatorial positions → less repulsion
📌 Lone pair occupies equatorial position first
📌 Example:
✔️ SF₄ → seesaw
✔️ ClF₃ → T-shape
✔️ XeF₂ → linear
9️⃣ #SPECIALCASEOFOCTAHEDRAL
✔️ One lone pair → square pyramidal
✔️ Two lone pairs → square planar
📌 Examples:
✔️ BrF₅ → square pyramidal
✔️ XeF₄ → square planar
🔟 #NEETIMPORTANTPOINTS 🚨
✔️ Lone pair causes maximum repulsion
✔️ Shape decided by LP + BP count
✔️ VSEPR explains shape, not bonding strength
✔️ Used mainly for p-block compounds
1️⃣1️⃣ #LIMITATIONSOFVSEPR
✔️ Cannot explain bond length accurately
✔️ Not applicable for transition metals
✔️ Fails for odd-electron molecules
1️⃣2️⃣ #ONELINEREVISION
Molecular shape is decided by repulsion between electron pairs around the central atom.
@Ayano1me @Neetugpoll @Neetugquiz
🔥2😎2❤1💋1
Chemistry booster series
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💯4❤2🕊1😍1
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
📌 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
🥰2❤1💯1
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
📌 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
🔥2🏆1🙈1
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
❤1👏1🐳1🏆1
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
✔️ 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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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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