Basic Concepts of Chemistry - JEE Main & Advanced
1. Matter and Its Classification
1.1 States of Matter
- Solid: Definite shape and volume
- Liquid: Definite volume but no fixed shape
- Gas: Neither definite shape nor volume
- Plasma: Ionized state of matter at high temperatures
- BEC (Bose-Einstein Condensate): State at extremely low temperatures
1.2 Classification of Matter
| Pure Substances | Mixtures |
|---|---|
|
|
Practice Questions (JEE Level)
Question 1:
The ratio of radii of second orbit of He⁺ to the first orbit of H atom is:
(a) 1:2 (b) 2:1 (c) 1:4 (d) 4:1
Answer: (b) 2:1
Question 2:
Which of the following has the highest electron affinity?
(a) F (b) Cl (c) Br (d) I
Answer: (b) Cl (Fluorine has lower EA than Cl due to small size and electron repulsion)
The landscape of competitive examinations for higher education is a complex and high-stakes arena, particularly in countries like India, where the pursuit of engineering and medical careers sees millions of aspirants vying for a limited number of coveted seats, and this ecosystem is primarily defined by a quartet of major assessments: the Joint Entrance Examination (JEE) Main, the National Eligibility cum Entrance Test (NEET), the Scholastic Assessment Test (SAT), and the JEE Advanced, each serving as a critical gateway to specific academic and professional futures, with the Jee main acting as the first and most significant hurdle for aspiring engineers across the nation, administered by the National Testing Agency (NTA), which oversees the entire process from the initial jee main registration to the final declaration of the jee main result, while for medical aspirants, the NEET examination, whose neet full form is National Eligibility cum Entrance Test, serves as the single window for undergraduate medical admissions, with the nta neet authority managing the examination process for neet ug candidates. The JEE Main is not a single event but a multi-session examination typically conducted twice a year, in January and April, allowing students multiple attempts to improve their scores, and the entire cycle for a given year, such as jee main 2025, begins months in advance with the official notification detailing the jee main 2025 exam date and opening the window for jee main 2025 registration on the official nta jee main portal, where candidates must meticulously fill out their application forms, upload required documents, and pay the requisite fees to complete the jee main registration process successfully, while for medical aspirants, the neet 2025 cycle follows a similar pattern with the announcement of the neet 2025 exam date and commencement of neet 2025 registration. Following the closure of the registration window, the nta jee main authority initiates the process of allocating exam centers, which is communicated to candidates through the jee main 2025 city intimation slip, a crucial document that informs them of the city where they are assigned to take the test, and this is followed by the release of the jee main admit card 2025, which is a mandatory document for entry into the examination hall, containing vital details such as the candidate's roll number, exam center address, and precise timings, and it is imperative for candidates to download their jee main admit card from the official website as soon as it is released, typically one week to 1 day before the exam, to avoid any last-minute technical glitches or panic, while for NEET aspirants, the neet admit card 2025 serves the same critical function. The jee main 2025 exam date is a nationally significant milestone, often spanning several days across both sessions, and the exam itself is conducted in a computer-based test (CBT) mode for most papers, featuring questions from Physics, Chemistry, and Mathematics designed to test a student's understanding of core concepts and their application, and the difficulty level can be considered Hard, demanding rigorous preparation and a strong conceptual foundation from the aspirants, whereas the neet exam date 2025 typically falls in May and the examination is conducted in pen-and-paper mode, testing candidates on Physics, Chemistry, and Biology. After the conclusion of the examination, the anxious wait for the jee main result begins, with the nta jee main authority taking approximately a week to ten days to process and declare the outcomes, and the jee main result 2025 is usually announced in the form of a scorecard that includes the candidate's NTA score, percentile, All India Rank (AIR), and category rank, which are pivotal for determining eligibility for the next stage, the JEE Advanced, or for admissions to various National Institutes of Technology (NITs), Indian Institutes of Information Technology (IIITs), and other Government Funded Technical Institutes (GFTIs), while for medical aspirants, the anticipation for the neet result 2025 builds up with the neet ug result date 2025 being announced by the NTA, and the neet 2025 result determines admission to MBBS, BDS, and other medical courses across India. Specifically, for the April session, students eagerly await the jee main session 2 result 2025, which, when combined with the January session scores, helps form the final rank list, and accessing the jee main result 2025 session 2 is a straightforward process through the official jee main result 2025 link provided by the NTA, where candidates must log in with their application number and date of birth to view and download their scorecards, while for NEET, there is only a single attempt per year, making the neet result even more crucial for medical aspirants. The declaration of the jee main session 2 result marks the culmination of the JEE Main cycle for that year, and for high-performers, it unlocks the gateway to register for the JEE Advanced, the second stage of the IIT entrance process, which is notably more challenging and conceptual than the JEE Main, whereas for medical postgraduates, the neet pg examination serves as the entrance test for MD/MS and other postgraduate courses, with neet pg 2025 being a crucial examination for medical graduates. Furthermore, for analysis and preparation purposes, the jee main 2025 question paper and its answer keys are released by the NTA shortly after the exam, allowing students to calculate their expected scores and file challenges in case of discrepancies. While the JEE Main and JEE Advanced form the bedrock of engineering admissions in India, the National Eligibility cum Entrance Test (NEET) occupies a parallel and equally formidable position for medical and dental aspirants, being the single, unified entrance examination for MBBS, BDS, and other undergraduate medical courses in all medical institutions across the country, including the prestigious AIIMS and JIPMER, which were brought under its umbrella, and the neet counselling 2024 process allocates seats based on the neet result and candidate preferences. Unlike the multi-session JEE Main, NEET is a single, pen-and-paper-based test conducted once a year, also by the NTA, and its syllabus is based on the NCERT curriculum for classes 11 and 12, covering Physics, Chemistry, and Biology (Botany and Zoology), with the competition being exceptionally fierce due to the sheer number of applicants and the limited number of seats available, and the neet exam date 2024 has already passed, while aspirants are now looking forward to the neet 2025 exam date. The preparation for NEET is a marathon of its own, requiring immense retention power, conceptual clarity in biology, and problem-solving skills in physics and chemistry, and success in NEET is the dream of every aspiring doctor in India, opening doors to top government and private medical colleges, and the neet 2025 result date is eagerly anticipated by lakhs of candidates. In a different vein, the Scholastic Assessment Test (SAT) serves as a critical standardized test for students aiming to pursue undergraduate studies, primarily in the United States and Canada, but its acceptance has grown globally, and the SAT is designed to assess a candidate's readiness for college through tested skills in Reading, Writing, and Mathematics, offering a different philosophy of assessment compared to the syllabus-intensive JEE Main and NEET. The SAT is conducted multiple times a year by the College Board, providing students with ample opportunities to take the test and improve their scores, and the registration process is entirely online, similar to the jee main registration and neet 2025 registration, but with a more international focus, and candidates need to Sign up on the College Board website. The SAT score is a key component of college applications abroad, alongside essays, letters of recommendation, and extracurricular activities, making it a holistic assessment tool rather than a sole determinant of one's academic future, unlike the JEE Advanced or NEET, which are predominantly rank-based. Returning to the Indian engineering context, the JEE Advanced is the ultimate challenge for IIT aspirants, a examination that only the top 2.5 lakh rank holders from the JEE Main are eligible to appear for, and it is conducted by one of the IITs on a rotational basis, featuring a pattern that is designed to test a student's analytical ability, comprehension, and scientific ingenuity at a much deeper level than the JEE Main. The questions in JEE Advanced are often unconventional, inter-disciplinary, and require a multi-step thought process to solve, truly separating the exceptional from the very good, and success in this exam secures a seat in the Indian Institutes of Technology, institutions synonymous with academic excellence and global recognition. The journey from starting preparation for the JEE Main to finally receiving an admission offer from an IIT or an NIT is a grueling multi-year endeavor that tests a student's perseverance, intellectual capacity, and emotional resilience, and it is a path walked by hundreds of thousands of young Indians each year, similarly, the path from neet 2025 registration to the declaration of neet result 2025 is equally challenging for medical aspirants. The importance of the jee main admit card or the jee main 2025 city intimation slip might seem like minor administrative details, but in the high-tension environment of these exams, they are critical documents that can mean the difference between taking the exam or being barred from the center, just as the timely announcement of the jee main result 2025 determines the future trajectory of a candidate's academic life, similarly, the neet admit card 2025 is equally important for medical aspirants. The digital infrastructure managed by the nta jee main and nta neet teams is therefore under immense scrutiny and pressure during these cycles, and any delays or technical issues can cause widespread anxiety among students and parents. For those targeting the April attempt, keeping track of the jee main 2025 exam date for session 2 and the subsequent release of the jee main session 2 result 2025 is paramount, as this result often provides a final chance to improve one's rank and secure a better college or qualification for JEE Advanced, while for medical postgraduates, the neet pg 2024 exam date has already passed and they are now preparing for neet pg 2025. After the exams are over, the jee main 2025 question paper becomes a valuable resource for future aspirants, providing insight into the trend and difficulty level of the examination, and coaching institutes and educators meticulously analyze these papers to guide their students more effectively for subsequent attempts. In conclusion, while the SAT represents a pathway to global education with a broader assessment model, the JEE Main, NEET, and JEE Advanced represent the pinnacle of a highly specialized, intensely competitive, and structurally rigid system of admissions in India, where a single rank, derived from a meticulously managed process from jee main registration to the final jee main result or from neet 2025 registration to the neet result 2025, can define a young individual's professional destiny, making the entire ecosystem surrounding these exams, from the release of the jee main admit card 2025 to the nervous click on the jee main result 2025 link or from the download of neet admit card 2025 to the announcement of neet 2025 result, a defining narrative in the lives of millions.
Atomic Structure - JEE Main & Advanced
1. Historical Development of Atomic Models
1.1 Dalton's Atomic Theory (1808)
- Matter composed of indivisible atoms
- Atoms of same element are identical
- Compounds form when atoms combine in fixed ratios
- Chemical reactions involve rearrangement of atoms
1.2 Thomson's Plum Pudding Model (1897)
- Discovered electrons using cathode ray tube
- Atom as positively charged sphere with embedded electrons
- Failed to explain atomic stability and spectral lines
Thomson's Model: ⊕⊕⊕⊕⊕ (positive sphere) with ••• (electrons)
Periodic Classification & Periodicity - JEE Main & Advanced
1. Historical Development of Periodic Table
1.1 Dobereiner's Triads (1829)
- Groups of 3 elements with similar properties
- Atomic weight of middle element ≈ average of other two
- Example: Li (7), Na (23), K (39)
- Limited to only a few elements
1.2 Newlands' Law of Octaves (1864)
- Every 8th element had similar properties
- Worked well for lighter elements only
1.3 Mendeleev's Periodic Table (1869)
- Arranged elements in increasing atomic weights
- Left gaps for undiscovered elements (Ga, Ge, Tc)
- Predicted properties of missing elements accurately
- Anomalies: Ar/K, Co/Ni, Te/I pairs
1.4 Modern Periodic Law (Moseley, 1913)
"The physical and chemical properties of elements are periodic functions of their atomic numbers."
2. Modern Periodic Table
2.1 Structure
| Block | Groups | Orbitals Filled | Elements |
|---|---|---|---|
| s-block | 1, 2 | ns¹⁻² | Alkali & Alkaline earth metals |
| p-block | 13-18 | np¹⁻⁶ | Metalloids, Non-metals, Halogens, Noble gases |
| d-block | 3-12 | (n-1)d¹⁻¹⁰ns⁰⁻² | Transition metals |
| f-block | - | (n-2)f¹⁻¹⁴(n-1)d⁰⁻¹ns² | Lanthanides & Actinides |
2.2 Special Groups
- Alkali Metals: Group 1 (ns¹)
- Alkaline Earth Metals: Group 2 (ns²)
- Chalcogens: Group 16 (ns²np⁴)
- Halogens: Group 17 (ns²np⁵)
- Noble Gases: Group 18 (ns²np⁶)
- Coinage Metals: Cu, Ag, Au (Group 11)
- Volatile Metals: Zn, Cd, Hg (Group 12)
3. Periodic Trends
3.1 Atomic Radius
| Type | Definition | Trend in Period | Trend in Group |
|---|---|---|---|
| Covalent Radius | ½ distance between nuclei of 2 bonded atoms | Decreases → | Increases ↓ |
| van der Waals Radius | ½ distance between nuclei of 2 adjacent atoms | Decreases → | Increases ↓ |
Exceptions: Noble gases have largest vdW radius in period
Anomalous Size: Lanthanide contraction (5d series ≈ 4d series size)
3.2 Ionization Energy (IE)
Energy required to remove most loosely bound electron from gaseous atom
X(g) → X⁺(g) + e⁻; ΔH = IE₁
| Order | Trend in Period | Trend in Group | Exceptions |
|---|---|---|---|
| IE₁ < IE₂ < IE₃... | Increases → | Decreases ↓ | Be > B, N > O, Mg > Al, P > S |
Example Problem:
Arrange in increasing order of IE₁: N, O, F
Answer: O < N < F (N has half-filled p-subshell stability)
3.3 Electron Affinity (EA)
Energy released when electron is added to gaseous atom
X(g) + e⁻ → X⁻(g); ΔH = -EA
| Trend in Period | Trend in Group | Exceptions |
|---|---|---|
| Increases → | Decreases ↓ | Cl > F (small size of F causes electron repulsion) |
3.4 Electronegativity (EN)
Tendency to attract shared electron pair (Pauling scale)
| Trend in Period | Trend in Group | Highest/Lowest |
|---|---|---|
| Increases → | Decreases ↓ | F (4.0) > O (3.5) > Cl (3.0); Cs (0.7) lowest |
3.5 Metallic Character
| Property | Trend in Period | Trend in Group |
|---|---|---|
| Electropositivity | Decreases → | Increases ↓ |
| Reducing Nature | Decreases → | Increases ↓ |
4. Other Periodic Properties
4.1 Valency
- s-block: Equal to group number
- p-block: 8 - group number (or group number for lower groups)
- d-block: Variable valency common
4.2 Oxidation States
- s-block: Fixed (+1 Group 1, +2 Group 2)
- p-block: Variable (except F always -1)
- Transition metals: Multiple oxidation states common
4.3 Melting/Boiling Points
- s-block: Decrease down group (except anomalous Li)
- p-block: Increase then decrease across period (peak at C/Si)
- d-block: Generally high, peak at middle of series
4.4 Diagonal Relationship
Similarities between 2nd period element and 3rd period element of next group:
| Pair | Similar Properties |
|---|---|
| Li-Mg | Form nitrides, carbonates decompose on heating |
| Be-Al | Amphoteric oxides, form polymeric hydrides |
| B-Si | Form acidic oxides, covalent compounds |
Practice Questions (JEE Level)
Question 1:
Which has highest first ionization energy?
(a) N (b) O (c) F (d) Ne
Answer: (d) Ne (noble gas configuration)
Question 2:
Correct order of atomic radii is:
(a) N < O < F (b) F < O < N (c) O < F < N (d) F < N < O
Answer: (b) F < O < N (size decreases across period)
Question 3:
Element with electronic configuration [Xe]4f¹⁴5d¹6s² belongs to:
(a) d-block (b) f-block (c) p-block (d) s-block
Answer: (a) d-block (last electron enters d-orbital)
Key Takeaways
- Memorize all periodic trends with exceptions
- Understand why anomalies occur (half-filled/filled subshell stability)
- Practice comparative questions (which is larger/higher EN etc.)
- Know special cases like lanthanide contraction
- Remember diagonal relationships
Chemical Bonding & Molecular Structure - JEE Main & Advanced
1. Types of Chemical Bonds
1.1 Ionic (Electrovalent) Bond
- Formed by complete electron transfer (metal → non-metal)
- Governed by Fajan's Rules
- Lattice Energy (U) = k(q⁺q⁻)/r₀
- Examples: NaCl, CaO, MgCl₂
Fajan's Rules for Covalent Character in Ionic Bonds:
- Small cation size → More polarization
- Large anion size → More polarization
- High charge on ions → More polarization
- Non-polarizable cations (Noble gas config) → Less covalent
1.2 Covalent Bond
- Formed by electron sharing (Lewis theory)
- Explained by Valence Bond Theory (VBT) and Molecular Orbital Theory (MOT)
- Examples: H₂, O₂, CH₄
1.3 Coordinate Bond
- Special covalent bond where both electrons come from one atom
- Represented by "→"
- Examples: H₃O⁺, NH₄⁺, SO₄²⁻
1.4 Metallic Bond
- "Sea of electrons" model
- Responsible for metallic properties (conductivity, malleability)
- Examples: Cu, Fe, Na
2. VSEPR Theory (Valence Shell Electron Pair Repulsion)
2.1 Basic Principles
- Electron pairs (bonding & lone pairs) arrange to minimize repulsion
- Order of repulsion: LP-LP > LP-BP > BP-BP
- Bond angles affected by lone pairs
2.2 Molecular Geometries
| Steric Number | Lone Pairs | Shape | Bond Angle | Examples |
|---|---|---|---|---|
| 2 | 0 | Linear | 180° | BeCl₂, CO₂ |
| 3 | 0 | Trigonal planar | 120° | BF₃, SO₃ |
| 3 | 1 | Bent/V-shape | <120° | SO₂, O₃ |
| 4 | 0 | Tetrahedral | 109.5° | CH₄, NH₄⁺ |
| 4 | 1 | Trigonal pyramidal | 107° | NH₃, PCl₃ |
| 4 | 2 | Bent/V-shape | 104.5° | H₂O, H₂S |
| 5 | 0 | Trigonal bipyramidal | 90°, 120° | PCl₅, PF₅ |
| 6 | 0 | Octahedral | 90° | SF₆, [AlF₆]³⁻ |
3. Hybridization
3.1 Concept
- Mixing of atomic orbitals to form new hybrid orbitals
- Explains molecular geometry and bond angles
- Hybridization = ½(V + M - C + A)
- Where V = valence e⁻, M = monovalent atoms, C = cation charge, A = anion charge
3.2 Types of Hybridization
| Hybridization | Geometry | Bond Angle | Examples |
|---|---|---|---|
| sp | Linear | 180° | C₂H₂, BeCl₂ |
| sp² | Trigonal planar | 120° | C₂H₄, BF₃ |
| sp³ | Tetrahedral | 109.5° | CH₄, NH₄⁺ |
| sp³d | Trigonal bipyramidal | 90°, 120° | PCl₅, SF₄ |
| sp³d² | Octahedral | 90° | SF₆, [Fe(CN)₆]³⁻ |
| dsp² | Square planar | 90° | [Ni(CN)₄]²⁻, XeF₄ |
Example Problem:
Determine hybridization in XeOF₄
Solution:
Steric number = 6 (1 Xe-O σ + 4 Xe-F σ + 1 lone pair)
Hybridization = sp³d² (octahedral geometry with 1 lone pair)
4. Molecular Orbital Theory (MOT)
4.1 Key Concepts
- Atomic orbitals combine to form molecular orbitals
- Bonding MO (σ, π): Lower energy than parent AOs
- Anti-bonding MO (σ*, π*): Higher energy than parent AOs
- Bond order = ½(Nb - Na)
4.2 MOT Diagrams
Homonuclear Diatomics (O₂, N₂):
σ2s ↑↓ σ*2s ↑↓ π2p ↑↓ ↑↓ σ2p ↑↓ π*2p ↑ ↑ (for O₂) σ*2p
4.3 Magnetic Properties
- Paramagnetic: Unpaired electrons (O₂, B₂)
- Diamagnetic: All electrons paired (N₂, H₂)
Important MOT Observations:
- O₂ is paramagnetic (2 unpaired e⁻ in π*2p)
- N₂ has triple bond (σ2p + π2p pair)
- Bond order predicts stability: Higher BO → More stable
5. Hydrogen Bonding
5.1 Characteristics
- Special dipole-dipole interaction (X-H···Y)
- X, Y = F, O, N (highly electronegative)
- Strength: 5-10% of covalent bond
5.2 Types
| Type | Description | Examples |
|---|---|---|
| Intermolecular | Between molecules | H₂O (ice), HF (liquid) |
| Intramolecular | Within same molecule | o-nitrophenol, salicylaldehyde |
5.3 Effects
- Increases boiling/melting points
- Increases solubility (e.g., ethanol in water)
- Affects density (ice less dense than water)
- Important in biological structures (DNA, proteins)
Practice Questions (JEE Level)
Question 1:
Which has maximum bond angle?
(a) NH₃ (b) NF₃ (c) NCl₃ (d) All equal
Answer: (a) NH₃ (F is more electronegative than H, pulls e⁻ density reducing bond angle)
Question 2:
Correct order of bond length in NO species is:
(a) NO⁻ < NO < NO⁺ (b) NO⁺ < NO < NO⁻ (c) NO < NO⁺ < NO⁻ (d) NO⁻ < NO⁺ < NO
Answer: (b) NO⁺ < NO < NO⁻ (Bond order: NO⁺=3, NO=2.5, NO⁻=2)
Question 3:
Hybridization of central atom in XeF₄ is:
(a) sp³ (b) sp³d (c) sp³d² (d) sp²d²
Answer: (c) sp³d² (Steric number = 6, square planar geometry)
Key Takeaways
- Memorize VSEPR geometries and bond angles
- Practice hybridization calculations for complex molecules
- Understand MOT diagrams for diatomic molecules
- Know exceptions to octet rule (PCl₅, SF₆ etc.)
- Remember effects of hydrogen bonding on physical properties
States of Matter: Gases & Liquids - JEE Main & Advanced
1. Gas Laws and Kinetic Theory
1.1 Fundamental Gas Laws
| Law | Equation | Conditions | Graph |
|---|---|---|---|
| Boyle's Law | P ∝ 1/V (T constant) | Isothermal | Hyperbola in P-V |
| Charles' Law | V ∝ T (P constant) | Isobaric | Straight line in V-T |
| Gay-Lussac's Law | P ∝ T (V constant) | Isochoric | Straight line in P-T |
| Avogadro's Law | V ∝ n (P,T constant) | - | Straight line in V-n |
Ideal Gas Equation:
PV = nRT
Where:
P = Pressure (atm), V = Volume (L), n = moles,
R = Universal gas constant = 0.0821 L·atm·K⁻¹·mol⁻¹,
T = Temperature (K)
1.2 Kinetic Theory of Gases
- Postulates: Point masses, random motion, elastic collisions
- PV = ⅓ mNū² (where ū = root mean square speed)
- Kinetic energy per mole = 3/2 RT
- Average KE per molecule = 3/2 kT (k = Boltzmann constant)
2. Gas Properties and Deviations
2.1 Molecular Speeds
| Speed Type | Formula | Ratio |
|---|---|---|
| Average speed (vav) | √(8RT/πM) | 1 : 1.128 : 1.224 |
| Root mean square speed (urms) | √(3RT/M) | (vav : urms : vmp) |
| Most probable speed (vmp) | √(2RT/M) |
Maxwell-Boltzmann Distribution:
Peak (vmp) < vav < urms
Curve shifts right and flattens with temperature increase
2.2 Real Gases and Deviations
- Deviation from ideal behavior at high P and low T
- van der Waals equation: (P + an²/V²)(V - nb) = nRT
- a = intermolecular forces correction, b = volume correction
- Boyle temperature (TB): Gas behaves ideally over widest P range
Compressibility Factor (Z = PV/nRT):
- Z = 1 for ideal gas
- Z < 1 at low P (attractive forces dominate)
- Z > 1 at high P (repulsive forces dominate)
3. Liquid State Properties
3.1 Surface Tension (γ)
- γ = F/l (N/m)
- Work done: W = γ·ΔA
- Capillary rise: h = 2γcosθ/rρg
- Effect of temperature: γ decreases with T
- Effect of additives: Surfactants decrease γ
3.2 Viscosity (η)
- F = ηA(dv/dx) (Poiseuille's law)
- SI unit: Pa·s (1 Poise = 0.1 Pa·s)
- Stokes' law: F = 6πηrv (for spherical particles)
- Effect of temperature: η decreases for liquids, increases for gases
3.3 Vapor Pressure
- Equilibrium pressure exerted by vapor at given T
- Clausius-Clapeyron equation: ln(P₂/P₁) = (ΔHvap/R)(1/T₁ - 1/T₂)
- Boiling point: When vapor pressure = atmospheric pressure
- Effect of temperature: Exponential increase with T
4. Phase Equilibria
4.1 Phase Diagrams
Water Phase Diagram:
- Triple point: 0.01°C, 4.58 mmHg (all 3 phases coexist)
- Critical point: 374°C, 218 atm (liquid-gas distinction disappears)
- Negative slope for solid-liquid line (ice less dense than water)
4.2 Azeotropes
| Type | Behavior | Examples |
|---|---|---|
| Minimum boiling | Boils at lower T than components | 95.6% ethanol + 4.4% water (78.1°C) |
| Maximum boiling | Boils at higher T than components | 68% HNO₃ + 32% water (122°C) |
Practice Questions (JEE Level)
Question 1:
The rms speed of O₂ at temperature T is v. At what temperature will the rms speed of SO₂ be v?
(a) T (b) 2T (c) T/2 (d) 4T
Answer: (b) 2T (v ∝ √(T/M), M(SO₂)=64, M(O₂)=32 ⇒ T₂ = 2T₁)
Question 2:
For a real gas at 25°C and high pressure, the compression factor is:
(a) =1 (b) <1 (c) >1 (d) Can't predict
Answer: (c) >1 (At high P, repulsive forces dominate causing Z > 1)
Question 3:
The surface tension of liquid at its boiling point:
(a) Becomes zero (b) Becomes infinite (c) Is same as at RT (d) None
Answer: (a) Becomes zero (At critical temperature, surface tension vanishes)
Key Takeaways
- Memorize all gas law relationships and their graphical representations
- Understand the significance of van der Waals constants a and b
- Know the three molecular speeds and their ratios
- Remember surface tension and viscosity formulas with units
- Practice phase diagram interpretation (especially water's anomalous behavior)
- Be thorough with azeotrope concepts and examples
Equilibrium - JEE Main & Advanced
1. Chemical Equilibrium
1.1 Law of Mass Action
For a reaction: aA + bB ⇌ cC + dD
Kc = [C]c[D]d/[A]a[B]b
Kp = (PC)c(PD)d/(PA)a(PB)b
Relation between Kp and Kc:
Kp = Kc(RT)Δng
Where Δng = (c+d) - (a+b) = moles gaseous products - moles gaseous reactants
1.2 Characteristics of Equilibrium
- Dynamic nature - forward and reverse reactions continue
- Macroscopic properties remain constant
- Achieved in closed system at constant temperature
- Independent of path taken
1.3 Le Chatelier's Principle
"When a system at equilibrium is disturbed, it shifts to counteract the change."
| Stress | Effect on Equilibrium |
|---|---|
| Concentration increase (reactant) | Shifts toward products |
| Pressure increase (gaseous) | Shifts toward side with fewer moles |
| Temperature increase (endothermic) | Shifts toward products |
| Catalyst added | No shift (speeds both forward and reverse) |
2. Acid-Base Equilibrium
2.1 Theories
| Theory | Acid Definition | Base Definition |
|---|---|---|
| Arrhenius | H⁺ producer | OH⁻ producer |
| Brønsted-Lowry | H⁺ donor | H⁺ acceptor |
| Lewis | e⁻ pair acceptor | e⁻ pair donor |
2.2 Ionization Constants
Ka × Kb = Kw = 10-14 (at 25°C)
pH = -log[H⁺], pOH = -log[OH⁻], pH + pOH = 14
2.3 pH Calculations
| Solution Type | pH Formula |
|---|---|
| Strong acid | pH = -log[H⁺] |
| Strong base | pOH = -log[OH⁻], then pH = 14 - pOH |
| Weak acid | pH = ½(pKa - log C) |
| Weak base | pOH = ½(pKb - log C), then pH = 14 - pOH |
| Buffer (acidic) | pH = pKa + log([salt]/[acid]) |
| Buffer (basic) | pOH = pKb + log([salt]/[base]) |
3. Solubility Equilibrium
3.1 Solubility Product (Ksp)
For salt AxBy(s) ⇌ xAy+(aq) + yBx-(aq)
Ksp = [Ay+]x[Bx-]y
3.2 Common Ion Effect
Solubility decreases when common ion is added
Example: Solubility of AgCl decreases in NaCl solution due to common Cl⁻ ion
3.3 Precipitation Condition
Ionic Product (IP) > Ksp → Precipitation occurs
IP = Ksp → Saturated solution
IP < Ksp → Unsaturated, no precipitation
3.4 Simultaneous Solubility
For salts with common ion (e.g., AgCl and AgBr):
[Ag⁺] = √(Ksp(AgCl) + Ksp(AgBr))
4. Salt Hydrolysis
4.1 Types of Salts
| Salt Type | Formed from | Nature | pH |
|---|---|---|---|
| Strong acid + Strong base | HCl + NaOH → NaCl | Neutral | 7 |
| Strong acid + Weak base | HCl + NH₄OH → NH₄Cl | Acidic | <7 |
| Weak acid + Strong base | CH₃COOH + NaOH → CH₃COONa | Basic | >7 |
| Weak acid + Weak base | CH₃COOH + NH₄OH → CH₃COONH₄ | Depends on Ka & Kb | ≈7 |
4.2 Degree of Hydrolysis
For salt of weak acid: h = √(Kw/KaC)
For salt of weak base: h = √(Kw/KbC)
For salt of weak acid & weak base: h = √(Kw/KaKb)
Practice Questions (JEE & NEET Level)
JEE Main Question:
For N₂(g) + 3H₂(g) ⇌ 2NH₃(g), ΔH = -92 kJ. Maximum yield of NH₃ is obtained at:
(a) High P, low T (b) Low P, high T (c) High P, high T (d) Low P, low T
Answer: (a) High P (fewer moles product side), low T (exothermic)
NEET Question:
pH of 0.01M CH₃COOH (Ka = 1.8×10-5) is:
(a) 2.37 (b) 3.37 (c) 4.37 (d) 5.37
Answer: (b) 3.37 (pH = ½(pKa - log C) = ½(4.74 - log0.01))
JEE Advanced Question:
Ksp of AgCl is 1.8×10-10. Its solubility in 0.1M NaCl is:
(a) 1.8×10-9 M (b) 1.8×10-10 M (c) 1.8×10-11 M (d) 1.8×10-12 M
Answer: (a) 1.8×10-9 M (Ksp = [Ag⁺][Cl⁻] ⇒ 1.8×10-10 = s × 0.1)
NEET Question:
The pH of 0.1M NH₄Cl solution (Kb for NH₃ = 1.8×10-5) is:
(a) 5.13 (b) 6.13 (c) 7.13 (d) 8.13
Answer: (a) 5.13 (pH = 7 - ½pKb - ½log C)
JEE Main Question:
For the reaction 2A(g) ⇌ B(g), Kp = 0.25 atm⁻¹. If initial pressure of A is 2 atm, equilibrium pressure of B is:
(a) 0.5 atm (b) 0.25 atm (c) 1 atm (d) 0.75 atm
Answer: (a) 0.5 atm
Key Takeaways
- Understand the dynamic nature of equilibrium
- Memorize Kp-Kc relationship
- Apply Le Chatelier's principle to predict shifts
- Know all pH calculation formulas
- Remember buffer action mechanism
- Practice solubility product problems
- Recognize common ion effect applications
- Understand salt hydrolysis concepts
Redox Reactions - JEE Main & Advanced
1. Introduction to Redox Reactions
1.1 Oxidation and Reduction
- Oxidation: Loss of electrons or increase in oxidation number
- Reduction: Gain of electrons or decrease in oxidation number
- Redox Reaction: Simultaneous oxidation and reduction
- Example: Zn + CuSO₄ → ZnSO₄ + Cu
1.2 Oxidizing and Reducing Agents
| Agent | Action | Examples |
|---|---|---|
| Oxidizing Agent | Accepts electrons, gets reduced | KMnO₄, K₂Cr₂O₇, O₃, H₂O₂ |
| Reducing Agent | Donates electrons, gets oxidized | Na, Mg, H₂, C, SO₂ |
2. Oxidation Number
2.1 Rules for Assigning Oxidation Numbers
- Free elements: 0 (e.g., Na, O₂, P₄)
- Monatomic ions: Equal to charge (e.g., Na⁺ = +1, Cl⁻ = -1)
- Hydrogen: +1 (except in metal hydrides = -1)
- Oxygen: -2 (except in peroxides = -1, superoxides = -½, OF₂ = +2)
- Fluorine: Always -1
- Sum of oxidation numbers in neutral compound = 0
- Sum of oxidation numbers in polyatomic ion = charge on ion
2.2 Calculating Oxidation Numbers
Example 1: Find oxidation number of Cr in K₂Cr₂O₇
2(+1) + 2x + 7(-2) = 0 ⇒ 2 + 2x - 14 = 0 ⇒ 2x = 12 ⇒ x = +6
Example 2: Find oxidation number of S in H₂SO₅ (Caro's acid)
2(+1) + x + 5(-2) = 0 ⇒ 2 + x - 10 = 0 ⇒ x = +8 (impossible)
Correction: One O-O bond exists, so oxidation number = +6
3. Balancing Redox Reactions
3.1 Oxidation Number Method
Steps:
- Assign oxidation numbers to all elements
- Identify oxidized and reduced elements
- Calculate change in oxidation numbers
- Balance electron loss and gain
- Balance atoms other than O and H
- Balance O atoms by adding H₂O
- Balance H atoms by adding H⁺
- For basic medium, add OH⁻ to both sides
3.2 Half-Reaction Method (Ion-Electron Method)
Example: Balance in acidic medium: MnO₄⁻ + Fe²⁺ → Mn²⁺ + Fe³⁺
Oxidation half: Fe²⁺ → Fe³⁺ + e⁻
Reduction half: MnO₄⁻ + 8H⁺ + 5e⁻ → Mn²⁺ + 4H₂O
Balanced: MnO₄⁻ + 5Fe²⁺ + 8H⁺ → Mn²⁺ + 5Fe³⁺ + 4H₂O
4. Types of Redox Reactions
4.1 Combination Reactions
2Mg + O₂ → 2MgO
H₂ + Cl₂ → 2HCl
4.2 Decomposition Reactions
2KClO₃ → 2KCl + 3O₂
2HgO → 2Hg + O₂
4.3 Displacement Reactions
- Metal displacement: Zn + CuSO₄ → ZnSO₄ + Cu
- Halogen displacement: Cl₂ + 2KBr → 2KCl + Br₂
- Hydrogen displacement: Zn + 2HCl → ZnCl₂ + H₂
4.4 Disproportionation Reactions
Same element is both oxidized and reduced
3Cl₂ + 6NaOH → 5NaCl + NaClO₃ + 3H₂O
2H₂O₂ → 2H₂O + O₂
4.5 Comproportionation Reactions
Different oxidation states of same element form intermediate state
NH₄NO₂ → N₂ + 2H₂O
5. Redox Titrations
5.1 Common Redox Titrations
| Titration | Indicator | Reaction | Application |
|---|---|---|---|
| KMnO₄ vs Oxalate | Self (KMnO₄) | 2MnO₄⁻ + 5C₂O₄²⁻ + 16H⁺ → 2Mn²⁺ + 10CO₂ + 8H₂O | Estimation of oxalic acid |
| K₂Cr₂O₇ vs Fe²⁺ | Diphenylamine | Cr₂O₇²⁻ + 6Fe²⁺ + 14H⁺ → 2Cr³⁺ + 6Fe³⁺ + 7H₂O | Estimation of iron |
| Iodometry | Starch | I₂ + 2S₂O₃²⁻ → 2I⁻ + S₄O₆²⁻ | Estimation of oxidizing agents |
5.2 Equivalent Weight in Redox
Equivalent weight = Molecular weight / Number of electrons gained or lost
Example: Equivalent weight of KMnO₄ in acidic medium
MnO₄⁻ → Mn²⁺ (5 electrons gained)
Eq. wt. = 158/5 = 31.6 g/equiv
6. Electrochemical Series
6.1 Standard Electrode Potentials
| Electrode Reaction | E° (V) |
|---|---|
| Li⁺ + e⁻ ⇌ Li | -3.04 |
| K⁺ + e⁻ ⇌ K | -2.93 |
| Zn²⁺ + 2e⁻ ⇌ Zn | -0.76 |
| Fe²⁺ + 2e⁻ ⇌ Fe | -0.44 |
| 2H⁺ + 2e⁻ ⇌ H₂ | 0.00 |
| Cu²⁺ + 2e⁻ ⇌ Cu | +0.34 |
| Ag⁺ + e⁻ ⇌ Ag | +0.80 |
| Au³⁺ + 3e⁻ ⇌ Au | +1.50 |
6.2 Applications of Electrochemical Series
- Predicting feasibility of redox reactions
- Determining stronger oxidizing/reducing agents
- Predicting displacement reactions
- Calculating EMF of electrochemical cells
Practice Questions (JEE & NEET Level)
JEE Main Question:
The oxidation number of phosphorus in Ba(H₂PO₂)₂ is:
(a) +3 (b) +2 (c) +1 (d) -1
Answer: (c) +1
NEET Question:
Which of the following is not a redox reaction?
(a) CaCO₃ → CaO + CO₂ (b) 2H₂O₂ → 2H₂O + O₂
(c) NaH + H₂O → NaOH + H₂ (d) MnO₂ + 4HCl → MnCl₂ + Cl₂ + 2H₂O
Answer: (a) CaCO₃ → CaO + CO₂ (No change in oxidation numbers)
JEE Advanced Question:
In the reaction: 3Br₂ + 6CO₃²⁻ + 3H₂O → 5Br⁻ + BrO₃⁻ + 6HCO₃⁻
What percentage of bromine is converted to bromide?
(a) 25% (b) 50% (c) 66.6% (d) 83.3%
Answer: (d) 83.3% (5 out of 6 Br atoms reduced)
NEET Question:
Equivalent weight of K₂Cr₂O₇ in acidic medium is (M = molecular weight):
(a) M/2 (b) M/3 (c) M/6 (d) M/1
Answer: (c) M/6 (Cr₂O₇²⁻ → 2Cr³⁺, gain of 6 electrons)
JEE Main Question:
In which of the following compounds, nitrogen exhibits highest oxidation state?
(a) N₂H₄ (b) NH₃ (c) N₃H (d) NH₂OH
Answer: (c) N₃H (Oxidation state = -1/3)
NEET Question:
The number of moles of KMnO₄ that will be needed to react with one mole of sulphite ion in acidic solution is:
(a) 2/5 (b) 3/5 (c) 4/5 (d) 1
Answer: (a) 2/5
JEE Advanced Question:
For the redox reaction: MnO₄⁻ + C₂O₄²⁻ + H⁺ → Mn²⁺ + CO₂ + H₂O
The correct coefficients of MnO₄⁻, C₂O₄²⁻ and H⁺ are respectively:
(a) 2, 5, 16 (b) 5, 2, 8 (c) 2, 5, 8 (d) 5, 2, 16
Answer: (a) 2, 5, 16
Key Takeaways
- Master oxidation number rules and calculations
- Practice both methods of balancing redox reactions
- Understand different types of redox reactions
- Memorize important redox titrations and their applications
- Know electrochemical series and its applications
- Calculate equivalent weights in redox reactions
- Practice disproportionation and comproportionation reactions
Hydrogen - JEE Main & Advanced
1. Position and Unique Properties of Hydrogen
1.1 Position in Periodic Table
- Resembles Alkali Metals (Group 1):
- Electronic configuration: 1s¹
- Forms H⁺ ion (like Na⁺, K⁺)
- Forms oxides, halides, and sulphides
- Resembles Halogens (Group 17):
- Diatomic molecule (H₂)
- Forms H⁻ ion (like F⁻, Cl⁻)
- High ionization enthalpy
- Forms covalent compounds
1.2 Physical Properties
| Property | Value |
|---|---|
| Atomic Number | 1 |
| Atomic Mass | 1.008 u |
| Electronic Configuration | 1s¹ |
| Ionization Enthalpy | 1312 kJ/mol |
| Electron Gain Enthalpy | -73 kJ/mol |
| Electronegativity | 2.1 |
| Melting Point | 13.96 K (-259°C) |
| Boiling Point | 20.39 K (-253°C) |
2. Isotopes of Hydrogen
| Isotope | Symbol | Protons | Neutrons | Natural Abundance | Applications |
|---|---|---|---|---|---|
| Protium | ¹H or H | 1 | 0 | 99.985% | Most common, forms H₂ gas |
| Deuterium | ²H or D | 1 | 1 | 0.015% | Heavy water (D₂O), NMR studies |
| Tritium | ³H or T | 1 | 2 | Trace (radioactive) | Radioactive tracer, β-emitter |
Key Differences:
- Protium: Ordinary hydrogen, non-radioactive
- Deuterium: Heavy hydrogen, stable isotope
- Tritium: Radioactive (β-emitter, t₁/₂ = 12.33 years)
3. Preparation of Dihydrogen
3.1 Laboratory Methods
- From Metals:
Zn + 2HCl → ZnCl₂ + H₂
2Al + 2NaOH + 2H₂O → 2NaAlO₂ + 3H₂
- From Metal Hydrides:
CaH₂ + 2H₂O → Ca(OH)₂ + 2H₂
- Electrolysis of Water:
2H₂O → 2H₂ + O₂ (with acid/alkali)
3.2 Commercial Methods
- Electrolysis of Brine:
2NaCl + 2H₂O → 2NaOH + Cl₂ + H₂
- Steam Reforming:
CH₄ + H₂O → CO + 3H₂ (at 1270K with Ni)
- Water Gas Shift Reaction:
CO + H₂O → CO₂ + H₂ (with Fe₂O₃/Cr₂O₃)
- From Coke:
C + H₂O → CO + H₂ (water gas)
4. Properties and Reactions of Dihydrogen
4.1 Physical Properties
- Colorless, odorless, tasteless gas
- Lightest known substance (density = 0.09 g/L)
- Highly combustible
- Slightly soluble in water (2% by volume)
4.2 Chemical Reactions
| Reaction Type | Reaction | Conditions |
|---|---|---|
| With Oxygen | 2H₂ + O₂ → 2H₂O | Burns with pale blue flame |
| With Halogens | H₂ + Cl₂ → 2HCl | Sunlight or heat |
| With Nitrogen | 3H₂ + N₂ → 2NH₃ | Haber process (Fe catalyst) |
| With Metals | H₂ + 2Na → 2NaH | Forms ionic hydrides |
| With Unsaturated Compounds | H₂ + CH₂=CH₂ → CH₃-CH₃ | Hydrogenation (Ni catalyst) |
| With Metal Oxides | CuO + H₂ → Cu + H₂O | Reducing agent |
5. Hydrides
5.1 Classification of Hydrides
| Type | Formed by | Nature | Examples | Properties |
|---|---|---|---|---|
| Ionic/Saline | s-block elements | Ionic, crystalline | NaH, CaH₂ | High melting points, electrolytic conductors |
| Covalent/Molecular | p-block elements | Volatile liquids/gases | CH₄, NH₃, H₂O | Low melting/boiling points, soft |
| Metallic/Interstitial | d-block elements | Non-stoichiometric | TiH₁.₇, PdH₀.₆ | Conduct electricity, metallic lustre |
5.2 Complex Hydrides
- Lithium Aluminium Hydride (LiAlH₄): Powerful reducing agent
- Sodium Borohydride (NaBH₄): Selective reducing agent
- Used in: Organic synthesis, fuel cells, hydrogen storage
6. Water and Heavy Water
6.1 Structure and Properties of Water
- Structure: Bent molecule (104.5° bond angle)
- Hydrogen Bonding: Extensive H-bonding network
- Anomalous Properties:
- High boiling point
- High specific heat capacity
- Maximum density at 4°C
- High surface tension
6.2 Heavy Water (D₂O)
| Property | H₂O | D₂O |
|---|---|---|
| Molecular Mass | 18 g/mol | 20 g/mol |
| Melting Point | 0°C | 3.8°C |
| Boiling Point | 100°C | 101.4°C |
| Density (at 20°C) | 0.998 g/mL | 1.105 g/mL |
Uses of Heavy Water:
- Moderator in nuclear reactors
- Tracer studies in chemical reactions
- NMR spectroscopy
- Study of reaction mechanisms
7. Hydrogen Peroxide (H₂O₂)
7.1 Preparation
- Laboratory Method:
BaO₂ + H₂SO₄ → BaSO₄ + H₂O₂
- Industrial Method (Auto-oxidation):
2-ethylanthraquinol + O₂ → 2-ethylanthraquinone + H₂O₂
7.2 Structure and Properties
- Structure: Non-planar, open book structure
- Physical Properties:
- Pale blue liquid (appears colorless in dilute solution)
- Miscible with water in all proportions
- Unstable and decomposes: 2H₂O₂ → 2H₂O + O₂
7.3 Chemical Properties
| Property | Reaction | Application |
|---|---|---|
| Oxidizing Agent | 2Fe²⁺ + 2H⁺ + H₂O₂ → 2Fe³⁺ + 2H₂O | Bleaching, antiseptic |
| Reducing Agent | 2MnO₄⁻ + 6H⁺ + 5H₂O₂ → 2Mn²⁺ + 8H₂O + 5O₂ | Reduces strong oxidizing agents |
| Bleaching Action | H₂O₂ → H₂O + [O] | Bleaching hair, textiles |
8. Hydrogen Economy
8.1 Concept
Using hydrogen as a low-carbon energy source to replace fossil fuels
8.2 Advantages
- Clean fuel (produces only water when burned)
- High energy content (142 kJ/g)
- Renewable and abundant
- Can be used in fuel cells
8.3 Challenges
- Storage and transportation difficulties
- High production costs
- Safety concerns (highly flammable)
- Infrastructure requirements
Practice Questions (JEE & NEET Level)
JEE Main Question:
Hydrogen peroxide oxidises [Fe(CN)₆]⁴⁻ to [Fe(CN)₆]³⁻ in acidic medium but reduces [Fe(CN)₆]³⁻ to [Fe(CN)₆]⁴⁻ in alkaline medium. The other products formed are, respectively:
(a) H₂O and (H₂O + O₂) (b) H₂O and (H₂O + OH⁻) (c) (H₂O + O₂) and H₂O (d) (H₂O + O₂) and (H₂O + OH⁻)
Answer: (a) H₂O and (H₂O + O₂)
NEET Question:
Which of the following statements is correct for hydrogen?
(a) It can form bonds in +1 oxidation state (b) It has very high ionization enthalpy
(c) It has same electronegativity as halogens (d) All of the above
Answer: (d) All of the above
JEE Advanced Question:
The volume of strength of 10 volume H₂O₂ solution is:
(a) 3% (b) 30% (c) 6% (d) 12%
Answer: (a) 3% (10 volume means 1L gives 10L O₂ at STP)
NEET Question:
Heavy water is:
(a) H₂O₁₈ (b) Water at 4°C (c) D₂O (d) Water obtained by repeated distillation
Answer: (c) D₂O
JEE Main Question:
Hydrogen bond is strongest in:
(a) S-H---S (b) O-H---S (c) F-H---F (d) F-H---O
Answer: (c) F-H---F (Highest electronegativity difference)
Key Takeaways
- Understand hydrogen's unique position in periodic table
- Memorize properties and preparation methods of dihydrogen
- Know classification and properties of different hydrides
- Understand structure and anomalous properties of water
- Learn preparation and uses of hydrogen peroxide
- Remember applications of heavy water
- Be familiar with hydrogen economy concept
S-Block Elements - JEE Main & Advanced
1. Introduction to S-Block Elements
1.1 General Characteristics
- Elements in which last electron enters s-orbital
- Includes Group 1 (Alkali metals) and Group 2 (Alkaline earth metals)
- Highly reactive metals
- Form basic oxides and hydroxides
- Strong electropositive character
1.2 Electronic Configuration
| Group | General Configuration | Elements |
|---|---|---|
| 1 (Alkali Metals) | [Noble gas] ns¹ | Li, Na, K, Rb, Cs, Fr |
| 2 (Alkaline Earth Metals) | [Noble gas] ns² | Be, Mg, Ca, Sr, Ba, Ra |
2. Alkali Metals (Group 1)
2.1 Physical Properties
| Property | Trend | Reason |
|---|---|---|
| Atomic Radius | Increases down the group | Addition of new shells |
| Ionic Radius | Increases down the group | Increasing nuclear charge |
| Ionization Enthalpy | Decreases down the group | Increasing atomic size |
| Melting Point | Decreases down the group | Weak metallic bonding |
| Density | Increases down the group | Increase in mass predominates |
2.2 Chemical Properties
| Reaction | Equation | Remarks |
|---|---|---|
| With Oxygen | 4M + O₂ → 2M₂O (oxide) 2M + O₂ → M₂O₂ (peroxide) M + O₂ → MO₂ (superoxide) |
Li forms only oxide, Na forms peroxide, others form superoxides |
| With Water | 2M + 2H₂O → 2MOH + H₂ | Violent reaction, reactivity increases down the group |
| With Halogens | 2M + X₂ → 2MX | Form ionic halides |
| With Hydrogen | 2M + H₂ → 2MH | Form ionic hydrides |
| With Nitrogen | 6M + N₂ → 2M₃N | Only lithium reacts at room temperature |
3. Alkaline Earth Metals (Group 2)
3.1 Physical Properties
| Property | Comparison with Alkali Metals |
|---|---|
| Atomic Size | Smaller than corresponding alkali metals |
| Ionization Enthalpy | Higher than alkali metals |
| Melting and Boiling Points | Higher than alkali metals |
| Density | Higher than alkali metals |
| Electropositive Character | Less electropositive than alkali metals |
3.2 Chemical Properties
| Reaction | Equation | Remarks |
|---|---|---|
| With Oxygen | 2M + O₂ → 2MO | Form monoxides, except Ba forms peroxide |
| With Water | M + 2H₂O → M(OH)₂ + H₂ | Reactivity increases down the group |
| With Halogens | M + X₂ → MX₂ | Form ionic halides |
| With Hydrogen | M + H₂ → MH₂ | Form ionic hydrides |
| With Nitrogen | 3M + N₂ → M₃N₂ | Only Be and Mg form nitrides |
4. Anomalous Behavior and Diagonal Relationship
4.1 Anomalous Behavior of Lithium and Beryllium
| Property | Lithium (vs Other Alkali Metals) | Beryllium (vs Other Alkaline Earth Metals) |
|---|---|---|
| Size | Exceptionally small | Exceptionally small |
| Polarizing Power | High | High |
| Nature of Compounds | More covalent | More covalent |
| Hydration Enthalpy | Highest | Highest |
| Reaction with Nitrogen | Forms nitride | Forms nitride |
4.2 Diagonal Relationship
| Pair | Similar Properties |
|---|---|
| Li - Mg |
|
| Be - Al |
|
5. Important Compounds of S-Block Elements
5.1 Sodium Compounds
| Compound | Formula | Uses |
|---|---|---|
| Sodium Carbonate (Washing Soda) | Na₂CO₃·10H₂O | Water softening, glass manufacture, cleaning agent |
| Sodium Bicarbonate (Baking Soda) | NaHCO₃ | Antacid, baking powder, fire extinguisher |
| Sodium Hydroxide (Caustic Soda) | NaOH | Soap manufacture, petroleum refining, paper industry |
| Sodium Chloride (Common Salt) | NaCl | Essential for life, food preservation, chemical industry |
5.2 Calcium Compounds
| Compound | Formula | Uses |
|---|---|---|
| Calcium Oxide (Quick Lime) | CaO | Manufacture of cement, steel, glass |
| Calcium Hydroxide (Slaked Lime) | Ca(OH)₂ | White washing, soil treatment, mortar |
| Calcium Carbonate | CaCO₃ | Building material, antacid, toothpaste |
| Calcium Sulphate (Plaster of Paris) | CaSO₄·½H₂O | Plastering, surgical casts, statues |
6. Biological Importance
6.1 Sodium and Potassium
- Sodium (Na⁺):
- Regulates osmotic pressure
- Maintains fluid balance
- Essential for nerve impulse transmission
- Required for muscle contraction
- Potassium (K⁺):
- Activates many enzymes
- Essential for protein synthesis
- Maintains heartbeat rhythm
- Regulates blood pressure
6.2 Magnesium and Calcium
- Magnesium (Mg²⁺):
- Component of chlorophyll
- Activates enzymes in carbohydrate metabolism
- Required for bone formation
- Maintains normal muscle and nerve function
- Calcium (Ca²⁺):
- Major component of bones and teeth
- Essential for blood clotting
- Required for muscle contraction
- Activates certain enzymes
7. Industrial Applications
7.1 Metallurgical Applications
- Magnesium: Used in lightweight alloys for aircraft
- Calcium: Used as reducing agent in metallurgy
- Sodium: Used in extraction of titanium and zirconium
7.2 Chemical Industry
- Sodium hydroxide: Manufacture of soap, paper, rayon
- Sodium carbonate: Glass manufacturing, water softening
- Calcium compounds: Cement production, plaster
7.3 Medical Applications
- Antacids: Mg(OH)₂, CaCO₃, NaHCO₃
- Calcium supplements: For bone health
- Magnesium sulphate: Epsom salt for baths
8. Solubility Trends
8.1 Group 1 Elements
- All salts are generally soluble in water
- Solubility increases down the group for most salts
- Exception: Lithium salts have lower solubility
8.2 Group 2 Elements
| Salt Type | Solubility Trend | Reason |
|---|---|---|
| Hydroxides | Increases down the group | Decrease in lattice energy |
| Fluorides | Decreases down the group | Increase in lattice energy |
| Sulphates | Decreases down the group | Increase in lattice energy |
| Carbonates | Decreases down the group | High lattice energy |
Practice Questions (JEE & NEET Level)
JEE Main Question:
The solubility of the alkaline earth metal hydroxides in water increases down the group. This is due to:
(a) Decrease in lattice energy (b) Increase in lattice energy
(c) Decrease in hydration energy (d) Increase in hydration energy
Answer: (a) Decrease in lattice energy
NEET Question:
Which of the following alkali metals forms only normal oxide when heated with oxygen?
(a) K (b) Rb (c) Li (d) Cs
Answer: (c) Li
JEE Advanced Question:
Identify the correct statement:
(a) Mg²⁺ ions form complexes with EDTA
(b) Ca²⁺ ions are important in blood clotting
(c) Na⁺ ions are involved in transmission of nerve signals
(d) All of the above
Answer: (d) All of the above
NEET Question:
Which of the following has highest hydration energy?
(a) Li⁺ (b) Na⁺ (c) K⁺ (d) Rb⁺
Answer: (a) Li⁺ (Smallest size, highest charge density)
JEE Main Question:
The compound that is used in borex bead test is:
(a) Na₂B₄O₇ (b) NaBO₂ (c) Na₂B₄O₇·10H₂O (d) Na₂B₄O₇·5H₂O
Answer: (c) Na₂B₄O₇·10H₂O (Borax)
NEET Question:
Dead burnt plaster is:
(a) CaSO₄ (b) CaSO₄·½H₂O (c) CaSO₄·H₂O (d) CaSO₄·2H₂O
Answer: (a) CaSO₄
Key Takeaways
- Understand periodic trends in s-block elements
- Memorize chemical reactions of alkali and alkaline earth metals
- Know anomalous behavior of lithium and beryllium
- Remember diagonal relationships (Li-Mg, Be-Al)
- Learn important compounds and their uses
- Understand biological importance of s-block elements
- Practice solubility trends and their explanations
P-Block Elements - JEE Main & Advanced
1. Introduction to P-Block Elements
1.1 General Characteristics
- Elements in which last electron enters p-orbital
- Includes Groups 13 to 18
- Show variable oxidation states
- Form covalent compounds predominantly
- Show inert pair effect in heavier elements
1.2 Electronic Configuration and Groups
| Group | General Configuration | Common Name | Elements |
|---|---|---|---|
| 13 | ns²np¹ | Boron Family | B, Al, Ga, In, Tl |
| 14 | ns²np² | Carbon Family | C, Si, Ge, Sn, Pb |
| 15 | ns²np³ | Nitrogen Family | N, P, As, Sb, Bi |
| 16 | ns²np⁴ | Oxygen Family | O, S, Se, Te, Po |
| 17 | ns²np⁵ | Halogen Family | F, Cl, Br, I, At |
| 18 | ns²np⁶ | Noble Gases | He, Ne, Ar, Kr, Xe, Rn |
2. Group 13: Boron Family
2.1 Atomic and Physical Properties
| Property | Trend | Anomalous Behavior of Boron |
|---|---|---|
| Atomic Radius | Increases down the group | Very small atomic radius |
| Ionization Enthalpy | Decreases down the group | Very high ionization enthalpy |
| Electronegativity | Decreases down the group | High electronegativity |
| Melting Point | Decreases down the group | Very high melting point |
2.2 Chemical Properties
- Oxidation States: +3 (common), +1 (Tl due to inert pair effect)
- Reactivity: Increases down the group
- Nature: Boron - metalloid, Others - metals
2.3 Important Compounds
| Compound | Formula | Properties and Uses |
|---|---|---|
| Borax | Na₂B₄O₇·10H₂O | Flux in welding, borax bead test, antiseptic |
| Boric Acid | H₃BO₃ | Weak monobasic acid, antiseptic, eye wash |
| Diborane | B₂H₆ | Electron-deficient compound, bridged structure |
| Aluminium Chloride | AlCl₃ | Lewis acid, Friedel-Crafts catalyst |
3. Group 14: Carbon Family
3.1 Atomic and Physical Properties
| Property | Trend | Anomalous Behavior of Carbon |
|---|---|---|
| Atomic Radius | Increases down the group | Very small atomic radius |
| Ionization Enthalpy | Decreases down the group | Very high ionization enthalpy |
| Electronegativity | Decreases down the group | High electronegativity |
| Catenation | Decreases down the group | Maximum catenation in carbon |
3.2 Allotropes of Carbon
| Allotrope | Structure | Properties |
|---|---|---|
| Diamond | Tetrahedral, 3D network | Hardest natural substance, insulator |
| Graphite | Hexagonal layers | Soft, good conductor, lubricant |
| Fullerene | Spherical molecules (C₆₀) | Soccer ball structure, semiconductor |
| Graphene | Single layer of graphite | Strongest material, excellent conductor |
3.3 Important Compounds
| Compound | Formula | Properties and Uses |
|---|---|---|
| Carbon Monoxide | CO | Poisonous gas, reducing agent, coordination complexes |
| Carbon Dioxide | CO₂ | Greenhouse gas, fire extinguisher, refrigerant |
| Silicon Dioxide | SiO₂ | Quartz, glass manufacture, semiconductor |
| Silicones | (R₂SiO)ₙ | Heat resistant, water repellent, lubricants |
4. Group 15: Nitrogen Family
4.1 Atomic and Physical Properties
| Property | Trend | Anomalous Behavior of Nitrogen |
|---|---|---|
| Atomic Radius | Increases down the group | Very small atomic radius |
| Ionization Enthalpy | Decreases down the group | Very high ionization enthalpy |
| Electronegativity | Decreases down the group | High electronegativity |
| Catenation | Decreases down the group | Limited catenation in nitrogen |
4.2 Allotropes of Phosphorus
| Allotrope | Structure | Properties |
|---|---|---|
| White Phosphorus | P₄ tetrahedral | Highly reactive, poisonous, glows in dark |
| Red Phosphorus | Polymeric chains | Less reactive, non-poisonous, used in matches |
| Black Phosphorus | Layered structure | Most stable, conductor of electricity |
4.3 Important Compounds
| Compound | Formula | Properties and Uses |
|---|---|---|
| Ammonia | NH₃ | Basic gas, fertilizer, refrigerant |
| Nitric Acid | HNO₃ | Strong acid, oxidizing agent, explosives |
| Phosphine | PH₃ | Poisonous gas, garlic odor, fumigant |
| Phosphorus Halides | PCl₃, PCl₅ | Chlorinating agents, catalyst in organic synthesis |
5. Group 16: Oxygen Family
5.1 Atomic and Physical Properties
| Property | Trend | Anomalous Behavior of Oxygen |
|---|---|---|
| Atomic Radius | Increases down the group | Very small atomic radius |
| Ionization Enthalpy | Decreases down the group | Very high ionization enthalpy |
| Electronegativity | Decreases down the group | High electronegativity (second to fluorine) |
| Melting/Boiling Point | Increases then decreases | Low melting/boiling point |
5.2 Allotropes of Oxygen and Sulphur
| Element | Allotropes | Properties |
|---|---|---|
| Oxygen | O₂ (dioxygen), O₃ (ozone) | O₃ is pale blue gas, powerful oxidizing agent |
| Sulphur | Rhombic, Monoclinic, Plastic | Different crystalline forms, S₈ ring structure |
5.3 Important Compounds
| Compound | Formula | Properties and Uses |
|---|---|---|
| Sulphur Dioxide | SO₂ | Acidic oxide, bleaching agent, preservative |
| Sulphuric Acid | H₂SO₄ | King of chemicals, dehydrating agent, fertilizer |
| Ozone | O₃ | Allotrope of oxygen, oxidizing agent, UV absorber |
6. Group 17: Halogen Family
6.1 Atomic and Physical Properties
| Property | Trend | Anomalous Behavior of Fluorine |
|---|---|---|
| Atomic Radius | Increases down the group | Very small atomic radius |
| Ionization Enthalpy | Decreases down the group | Very high ionization enthalpy |
| Electronegativity | Decreases down the group | Highest electronegativity |
| Oxidizing Power | Decreases down the group | Strongest oxidizing agent |
6.2 Chemical Properties
- Oxidation States: -1 (common), positive states for Cl, Br, I
- Reactivity: Decreases down the group
- Nature: All are non-metals
6.3 Important Compounds
| Compound | Formula | Properties and Uses |
|---|---|---|
| Hydrochloric Acid | HCl | Strong acid, pickling of metals, laboratory reagent |
| Bleaching Powder | Ca(OCl)Cl | Oxidizing agent, disinfectant, bleaching |
| Interhalogen Compounds | ClF, BrF₃, IF₇ | Formed between different halogens, powerful fluorinating agents |
7. Group 18: Noble Gases
7.1 Atomic and Physical Properties
| Property | Trend | Remarks |
|---|---|---|
| Atomic Radius | Increases down the group | Largest in respective periods |
| Ionization Enthalpy | Decreases down the group | Highest in respective periods |
| Boiling Point | Increases down the group | Very low boiling points |
| Density | Increases down the group | All are monoatomic gases |
7.2 Chemical Properties
- Generally inert due to stable electronic configuration
- Xenon forms compounds with fluorine and oxygen
- Compounds include XeF₂, XeF₄, XeF₆, XeO₃, XeO₄
7.3 Uses of Noble Gases
| Gas | Uses |
|---|---|
| Helium | Balloons, deep sea diving, cryogenics |
| Neon | Advertising signs, voltage regulators |
| Argon | Welding, incandescent lamps |
| Krypton & Xenon | Photography flash lamps, lasers |
8. Inert Pair Effect
8.1 Definition and Explanation
The reluctance of s-electrons to participate in bond formation in heavier elements of p-block
8.2 Examples
| Group | Element | Stable Oxidation State | Due to Inert Pair Effect |
|---|---|---|---|
| 13 | Tl | +1 | More stable than +3 |
| 14 | Pb | +2 | More stable than +4 |
| 15 | Bi | +3 | More stable than +5 |
Reason for Inert Pair Effect:
- Poor shielding by d and f electrons
- Increased effective nuclear charge
- Greater stability of ns² configuration
Practice Questions (JEE & NEET Level)
JEE Main Question:
Which of the following statements is correct for p-block elements?
(a) They include metals, non-metals and metalloids
(b) They show variable oxidation states
(c) They form covalent compounds predominantly
(d) All of the above
Answer: (d) All of the above
NEET Question:
In borax bead test, which compound is formed?
(a) Metal borate (b) Metal metaborate (c) Metal tetraborate (d) Metal orthoborate
Answer: (b) Metal metaborate
JEE Advanced Question:
The correct order of catenation is:
(a) C > Si > Ge ≈ Sn (b) C > Si > Ge > Sn (c) Si > C > Ge > Sn (d) Ge > Si > C > Sn
Answer: (a) C > Si > Ge ≈ Sn
NEET Question:
Which of the following oxides is amphoteric?
(a) SiO₂ (b) CO₂ (c) SnO₂ (d) CaO
Answer: (c) SnO₂
JEE Main Question:
The compound that does not exist is:
(a) XeF₂ (b) XeF₄ (c) XeF₆ (d) XeCl₆
Answer: (d) XeCl₆
Key Takeaways
- Understand periodic trends in all p-block groups
- Memorize anomalous behavior of first elements
- Know important compounds and their uses
- Learn allotropes of carbon, phosphorus, oxygen, and sulphur
- Understand inert pair effect and its consequences
- Remember preparation and properties of important compounds
- Practice chemical reactions of p-block elements
Organic Chemistry - Some Basic Principles - JEE Main & Advanced
1. Introduction to Organic Chemistry
1.1 Definition and Scope
- Organic Chemistry: Study of carbon compounds (except CO, CO₂, carbonates, bicarbonates, cyanides)
- Vital Force Theory: Proposed by Berzelius, disproved by Wöhler's synthesis of urea
- Modern Definition: Chemistry of hydrocarbons and their derivatives
1.2 Unique Properties of Carbon
| Property | Significance |
|---|---|
| Catenation | Ability to form chains and rings of carbon atoms |
| Tetravalency | Forms four covalent bonds |
| Multiple Bond Formation | Forms double and triple bonds |
| Isomerism | Same molecular formula but different structures |
2. Classification of Organic Compounds
2.1 Based on Carbon Skeleton
| Type | Description | Examples |
|---|---|---|
| Acyclic (Open Chain) | Straight or branched chains | CH₄, CH₃-CH₃, CH₃-CH₂-CH₃ |
| Cyclic (Closed Chain) | Ring structures | Cyclohexane, Benzene |
2.2 Based on Functional Groups
| Functional Group | Formula | Suffix/Prefix | Example |
|---|---|---|---|
| Alkane | -C-C- | -ane | CH₄ (Methane) |
| Alkene | C=C | -ene | CH₂=CH₂ (Ethene) |
| Alkyne | C≡C | -yne | HC≡CH (Ethyne) |
| Alcohol | -OH | -ol | CH₃OH (Methanol) |
| Aldehyde | -CHO | -al | HCHO (Methanal) |
| Ketone | >C=O | -one | CH₃COCH₃ (Propanone) |
| Carboxylic Acid | -COOH | -oic acid | HCOOH (Methanoic acid) |
| Amine | -NH₂ | -amine | CH₃NH₂ (Methanamine) |
3. IUPAC Nomenclature
3.1 Fundamental Principles
- Longest Chain Rule: Select the longest continuous carbon chain
- Lowest Number Rule: Number the chain to give lowest numbers to substituents
- Alphabetical Order: Name substituents in alphabetical order
- Multiple Same Groups: Use di-, tri-, tetra- prefixes
3.2 Step-by-Step Naming Procedure
Example: Name the compound CH₃-CH₂-CH(CH₃)-CH₂-CH₂-CH₃
- Longest chain: 6 carbons (hexane)
- Numbering: From right gives methyl at C3
- Name: 3-Methylhexane
3.3 Common vs IUPAC Names
| Common Name | IUPAC Name | Formula |
|---|---|---|
| Acetic acid | Ethanoic acid | CH₃COOH |
| Acetone | Propanone | CH₃COCH₃ |
| Formaldehyde | Methanal | HCHO |
| Isopropyl alcohol | Propan-2-ol | (CH₃)₂CHOH |
4. Isomerism
4.1 Structural Isomerism
| Type | Description | Example |
|---|---|---|
| Chain Isomerism | Different carbon skeletons | Butane vs 2-Methylpropane |
| Position Isomerism | Different positions of functional group | Propan-1-ol vs Propan-2-ol |
| Functional Isomerism | Different functional groups | Ethanol vs Dimethyl ether |
| Metamerism | Different alkyl groups on either side of functional group | Methoxyethane vs Ethoxyethane |
| Tautomerism | Dynamic equilibrium between isomers | Keto-enol tautomerism |
4.2 Stereoisomerism
| Type | Description | Example |
|---|---|---|
| Geometrical Isomerism | Different spatial arrangements due to restricted rotation | cis-trans But-2-ene |
| Optical Isomerism | Non-superimposable mirror images | Lactic acid |
| Conformational Isomerism | Different arrangements by rotation around single bonds | Staggered and eclipsed ethane |
5. Electronic Effects in Organic Molecules
5.1 Inductive Effect
- Permanent polarization of σ-bond due to electronegativity difference
- -I Effect: Electron withdrawing groups (NO₂, CN, CHO, COOH)
- +I Effect: Electron donating groups (CH₃, C₂H₅)
- Decreases with distance from the group
5.2 Resonance (Mesomeric Effect)
- Delocalization of π-electrons in conjugated systems
- -M Effect: Electron withdrawing (NO₂, CN, CHO, COR)
- +M Effect: Electron donating (OH, NH₂, OCH₃)
- Examples: Benzene, carboxylate ion, nitrobenzene
5.3 Hyperconjugation
- Delocalization of σ-electrons into empty p-orbital
- Also called no-bond resonance
- Stabilizes carbocations and free radicals
- Number of hyperconjugative structures = number of α-hydrogens + 1
5.4 Electromeric Effect
- Temporary effect observed in presence of attacking reagent
- Complete transfer of π-electrons to one atom
- Observed in multiple bonds
6. Reaction Mechanisms
6.1 Types of Bond Fission
| Type | Description | Products | Example |
|---|---|---|---|
| Homolytic Fission | Equal sharing of electrons | Free radicals | Cl-Cl → 2Cl• |
| Heterolytic Fission | Unequal sharing of electrons | Ions (carbocation/carbanion) | CH₃-Br → CH₃⁺ + Br⁻ |
6.2 Types of Reagents
| Reagent Type | Definition | Examples |
|---|---|---|
| Nucleophile | Electron pair donor | OH⁻, CN⁻, NH₃, H₂O |
| Electrophile | Electron pair acceptor | H⁺, NO₂⁺, CH₃⁺, AlCl₃ |
| Free Radical | Species with unpaired electron | Cl•, CH₃• |
6.3 Types of Organic Reactions
| Reaction Type | Description | Example |
|---|---|---|
| Substitution | Replacement of atom/group by another | CH₄ + Cl₂ → CH₃Cl + HCl |
| Addition | Addition of molecules to unsaturated compounds | CH₂=CH₂ + H₂ → CH₃-CH₃ |
| Elimination | Removal of atoms/groups to form multiple bonds | CH₃-CH₂Br → CH₂=CH₂ + HBr |
| Rearrangement | Migration of atom/group within molecule | Pinacol-Pinacolone rearrangement |
7. Purification Methods
7.1 Common Purification Techniques
| Method | Principle | Application |
|---|---|---|
| Crystallization | Difference in solubility | Purification of solids |
| Sublimation | Direct solid to vapor transition | Camphor, naphthalene, benzoic acid |
| Distillation | Difference in boiling points | Purification of liquids |
| Fractional Distillation | Small difference in boiling points | Separation of petroleum fractions |
| Steam Distillation | Immiscible liquid mixture | Essential oils, aniline |
7.2 Chromatography
| Type | Principle | Application |
|---|---|---|
| Adsorption Chromatography | Different adsorption on stationary phase | Separation of coloured compounds |
| Partition Chromatography | Different partition coefficients | Amino acids, sugars |
| Thin Layer Chromatography (TLC) | Adsorption on thin layer | Quick separation, identification |
| Column Chromatography | Adsorption in column | Separation of mixtures |
8. Qualitative Analysis
8.1 Detection of Elements
| Element | Test | Observation |
|---|---|---|
| Carbon & Hydrogen | Heating with CuO | CO₂ turns lime water milky, H₂O turns anhydrous CuSO₄ blue |
| Nitrogen | Lassaigne's test | Prussian blue colour with FeSO₄ + FeCl₃ + HCl |
| Sulphur | Lassaigne's test | Violet colour with sodium nitroprusside |
| Halogens | Lassaigne's test | White ppt with AgNO₃ (Cl), pale yellow (Br), yellow (I) |
8.2 Detection of Functional Groups
| Functional Group | Test | Observation |
|---|---|---|
| Alkene | Bromine water test | Decolorization of bromine water |
| Alkyne | Ammoniacal AgNO₃ | White ppt with terminal alkynes |
| Alcohol | Ceric ammonium nitrate | Red colour |
| Aldehyde | Tollen's test | Silver mirror |
| Ketone | 2,4-DNP test | Yellow/orange ppt |
| Carboxylic Acid | NaHCO₃ test | Effervescence of CO₂ |
9. Quantitative Analysis
9.1 Carbon and Hydrogen
Liebig's Method: Organic compound burned in copper oxide, CO₂ and H₂O absorbed and weighed
9.2 Nitrogen
| Method | Principle | Application |
|---|---|---|
| Dumas Method | Heating with CuO in CO₂ atmosphere | All nitrogen compounds |
| Kjeldahl's Method | Digestion with conc. H₂SO₄ | Compounds where N is in -3 oxidation state |
9.3 Halogens
Carius Method: Heating with fuming HNO₃ and AgNO₃, precipitate of AgX weighed
9.4 Sulphur and Phosphorus
Carius Method: Heating with fuming HNO₃, converted to H₂SO₄ and H₃PO₄ respectively
Practice Questions (JEE & NEET Level)
JEE Main Question:
The IUPAC name of CH₃-CH₂-CH(CH₃)-CH₂-CHO is:
(a) 2-Methylpentanal (b) 3-Methylpentanal (c) 2-Ethylbutanal (d) 3-Ethylbutanal
Answer: (b) 3-Methylpentanal
NEET Question:
Which of the following shows metamerism?
(a) CH₃OH (b) C₂H₅OH (c) CH₃OCH₃ (d) CH₃OC₂H₅
Answer: (d) CH₃OC₂H₅
JEE Advanced Question:
The number of hyperconjugative structures of isopropyl carbocation is:
(a) 6 (b) 7 (c) 8 (d) 9
Answer: (b) 7 (6 α-hydrogens + 1)
NEET Question:
In Dumas method, the nitrogen present in organic compound is converted into:
(a) NH₃ (b) N₂ (c) NO₂ (d) (NH₄)₂SO₄
Answer: (b) N₂
JEE Main Question:
The most stable carbocation among the following is:
(a) CH₃⁺ (b) (CH₃)₂CH⁺ (c) (CH₃)₃C⁺ (d) C₆H₅CH₂⁺
Answer: (c) (CH₃)₃C⁺ (Maximum hyperconjugation)
Key Takeaways
- Master IUPAC nomenclature rules
- Understand different types of isomerism
- Learn electronic effects and their applications
- Know reaction mechanisms and types of reactions
- Remember purification and analysis methods
- Practice qualitative and quantitative analysis
- Understand the importance of functional groups
Organic Chemistry - Some Basic Principles - JEE Main & Advanced
1. Introduction to Organic Chemistry
1.1 Definition and Scope
- Organic Chemistry: Study of carbon compounds (except CO, CO₂, carbonates, bicarbonates, cyanides)
- Vital Force Theory: Proposed by Berzelius, disproved by Wöhler's synthesis of urea
- Modern Definition: Chemistry of hydrocarbons and their derivatives
1.2 Unique Properties of Carbon
| Property | Significance |
|---|---|
| Catenation | Ability to form chains and rings of carbon atoms |
| Tetravalency | Forms four covalent bonds |
| Multiple Bond Formation | Forms double and triple bonds |
| Isomerism | Same molecular formula but different structures |
2. Classification of Organic Compounds
2.1 Based on Carbon Skeleton
| Type | Description | Examples |
|---|---|---|
| Acyclic (Open Chain) | Straight or branched chains | CH₄, CH₃-CH₃, CH₃-CH₂-CH₃ |
| Cyclic (Closed Chain) | Ring structures | Cyclohexane, Benzene |
2.2 Based on Functional Groups
| Functional Group | Formula | Suffix/Prefix | Example |
|---|---|---|---|
| Alkane | -C-C- | -ane | CH₄ (Methane) |
| Alkene | C=C | -ene | CH₂=CH₂ (Ethene) |
| Alkyne | C≡C | -yne | HC≡CH (Ethyne) |
| Alcohol | -OH | -ol | CH₃OH (Methanol) |
| Aldehyde | -CHO | -al | HCHO (Methanal) |
| Ketone | >C=O | -one | CH₃COCH₃ (Propanone) |
| Carboxylic Acid | -COOH | -oic acid | HCOOH (Methanoic acid) |
| Amine | -NH₂ | -amine | CH₃NH₂ (Methanamine) |
3. IUPAC Nomenclature
3.1 Fundamental Principles
- Longest Chain Rule: Select the longest continuous carbon chain
- Lowest Number Rule: Number the chain to give lowest numbers to substituents
- Alphabetical Order: Name substituents in alphabetical order
- Multiple Same Groups: Use di-, tri-, tetra- prefixes
3.2 Step-by-Step Naming Procedure
Example: Name the compound CH₃-CH₂-CH(CH₃)-CH₂-CH₂-CH₃
- Longest chain: 6 carbons (hexane)
- Numbering: From right gives methyl at C3
- Name: 3-Methylhexane
3.3 Common vs IUPAC Names
| Common Name | IUPAC Name | Formula |
|---|---|---|
| Acetic acid | Ethanoic acid | CH₃COOH |
| Acetone | Propanone | CH₃COCH₃ |
| Formaldehyde | Methanal | HCHO |
| Isopropyl alcohol | Propan-2-ol | (CH₃)₂CHOH |
4. Isomerism
4.1 Structural Isomerism
| Type | Description | Example |
|---|---|---|
| Chain Isomerism | Different carbon skeletons | Butane vs 2-Methylpropane |
| Position Isomerism | Different positions of functional group | Propan-1-ol vs Propan-2-ol |
| Functional Isomerism | Different functional groups | Ethanol vs Dimethyl ether |
| Metamerism | Different alkyl groups on either side of functional group | Methoxyethane vs Ethoxyethane |
| Tautomerism | Dynamic equilibrium between isomers | Keto-enol tautomerism |
4.2 Stereoisomerism
| Type | Description | Example |
|---|---|---|
| Geometrical Isomerism | Different spatial arrangements due to restricted rotation | cis-trans But-2-ene |
| Optical Isomerism | Non-superimposable mirror images | Lactic acid |
| Conformational Isomerism | Different arrangements by rotation around single bonds | Staggered and eclipsed ethane |
5. Electronic Effects in Organic Molecules
5.1 Inductive Effect
- Permanent polarization of σ-bond due to electronegativity difference
- -I Effect: Electron withdrawing groups (NO₂, CN, CHO, COOH)
- +I Effect: Electron donating groups (CH₃, C₂H₅)
- Decreases with distance from the group
5.2 Resonance (Mesomeric Effect)
- Delocalization of π-electrons in conjugated systems
- -M Effect: Electron withdrawing (NO₂, CN, CHO, COR)
- +M Effect: Electron donating (OH, NH₂, OCH₃)
- Examples: Benzene, carboxylate ion, nitrobenzene
5.3 Hyperconjugation
- Delocalization of σ-electrons into empty p-orbital
- Also called no-bond resonance
- Stabilizes carbocations and free radicals
- Number of hyperconjugative structures = number of α-hydrogens + 1
5.4 Electromeric Effect
- Temporary effect observed in presence of attacking reagent
- Complete transfer of π-electrons to one atom
- Observed in multiple bonds
6. Reaction Mechanisms
6.1 Types of Bond Fission
| Type | Description | Products | Example |
|---|---|---|---|
| Homolytic Fission | Equal sharing of electrons | Free radicals | Cl-Cl → 2Cl• |
| Heterolytic Fission | Unequal sharing of electrons | Ions (carbocation/carbanion) | CH₃-Br → CH₃⁺ + Br⁻ |
6.2 Types of Reagents
| Reagent Type | Definition | Examples |
|---|---|---|
| Nucleophile | Electron pair donor | OH⁻, CN⁻, NH₃, H₂O |
| Electrophile | Electron pair acceptor | H⁺, NO₂⁺, CH₃⁺, AlCl₃ |
| Free Radical | Species with unpaired electron | Cl•, CH₃• |
6.3 Types of Organic Reactions
| Reaction Type | Description | Example |
|---|---|---|
| Substitution | Replacement of atom/group by another | CH₄ + Cl₂ → CH₃Cl + HCl |
| Addition | Addition of molecules to unsaturated compounds | CH₂=CH₂ + H₂ → CH₃-CH₃ |
| Elimination | Removal of atoms/groups to form multiple bonds | CH₃-CH₂Br → CH₂=CH₂ + HBr |
| Rearrangement | Migration of atom/group within molecule | Pinacol-Pinacolone rearrangement |
7. Purification Methods
7.1 Common Purification Techniques
| Method | Principle | Application |
|---|---|---|
| Crystallization | Difference in solubility | Purification of solids |
| Sublimation | Direct solid to vapor transition | Camphor, naphthalene, benzoic acid |
| Distillation | Difference in boiling points | Purification of liquids |
| Fractional Distillation | Small difference in boiling points | Separation of petroleum fractions |
| Steam Distillation | Immiscible liquid mixture | Essential oils, aniline |
7.2 Chromatography
| Type | Principle | Application |
|---|---|---|
| Adsorption Chromatography | Different adsorption on stationary phase | Separation of coloured compounds |
| Partition Chromatography | Different partition coefficients | Amino acids, sugars |
| Thin Layer Chromatography (TLC) | Adsorption on thin layer | Quick separation, identification |
| Column Chromatography | Adsorption in column | Separation of mixtures |
8. Qualitative Analysis
8.1 Detection of Elements
| Element | Test | Observation |
|---|---|---|
| Carbon & Hydrogen | Heating with CuO | CO₂ turns lime water milky, H₂O turns anhydrous CuSO₄ blue |
| Nitrogen | Lassaigne's test | Prussian blue colour with FeSO₄ + FeCl₃ + HCl |
| Sulphur | Lassaigne's test | Violet colour with sodium nitroprusside |
| Halogens | Lassaigne's test | White ppt with AgNO₃ (Cl), pale yellow (Br), yellow (I) |
8.2 Detection of Functional Groups
| Functional Group | Test | Observation |
|---|---|---|
| Alkene | Bromine water test | Decolorization of bromine water |
| Alkyne | Ammoniacal AgNO₃ | White ppt with terminal alkynes |
| Alcohol | Ceric ammonium nitrate | Red colour |
| Aldehyde | Tollen's test | Silver mirror |
| Ketone | 2,4-DNP test | Yellow/orange ppt |
| Carboxylic Acid | NaHCO₃ test | Effervescence of CO₂ |
9. Quantitative Analysis
9.1 Carbon and Hydrogen
Liebig's Method: Organic compound burned in copper oxide, CO₂ and H₂O absorbed and weighed
9.2 Nitrogen
| Method | Principle | Application |
|---|---|---|
| Dumas Method | Heating with CuO in CO₂ atmosphere | All nitrogen compounds |
| Kjeldahl's Method | Digestion with conc. H₂SO₄ | Compounds where N is in -3 oxidation state |
9.3 Halogens
Carius Method: Heating with fuming HNO₃ and AgNO₃, precipitate of AgX weighed
9.4 Sulphur and Phosphorus
Carius Method: Heating with fuming HNO₃, converted to H₂SO₄ and H₃PO₄ respectively
Practice Questions (JEE & NEET Level)
JEE Main Question:
The IUPAC name of CH₃-CH₂-CH(CH₃)-CH₂-CHO is:
(a) 2-Methylpentanal (b) 3-Methylpentanal (c) 2-Ethylbutanal (d) 3-Ethylbutanal
Answer: (b) 3-Methylpentanal
NEET Question:
Which of the following shows metamerism?
(a) CH₃OH (b) C₂H₅OH (c) CH₃OCH₃ (d) CH₃OC₂H₅
Answer: (d) CH₃OC₂H₅
JEE Advanced Question:
The number of hyperconjugative structures of isopropyl carbocation is:
(a) 6 (b) 7 (c) 8 (d) 9
Answer: (b) 7 (6 α-hydrogens + 1)
NEET Question:
In Dumas method, the nitrogen present in organic compound is converted into:
(a) NH₃ (b) N₂ (c) NO₂ (d) (NH₄)₂SO₄
Answer: (b) N₂
JEE Main Question:
The most stable carbocation among the following is:
(a) CH₃⁺ (b) (CH₃)₂CH⁺ (c) (CH₃)₃C⁺ (d) C₆H₅CH₂⁺
Answer: (c) (CH₃)₃C⁺ (Maximum hyperconjugation)
Key Takeaways
- Master IUPAC nomenclature rules
- Understand different types of isomerism
- Learn electronic effects and their applications
- Know reaction mechanisms and types of reactions
- Remember purification and analysis methods
- Practice qualitative and quantitative analysis
- Understand the importance of functional groups
Introduction
The pursuit of academic excellence through competitive examinations such as JEE, NEET, and SAT has become a crucial step for students aspiring to secure admission into prestigious institutions. These exams not only evaluate a student’s knowledge but also test analytical thinking, problem-solving skills, and time management under pressure. Understanding the nuances of each examination is essential for a well-rounded preparation strategy. While JEE primarily targets engineering aspirants in India, NEET caters to students aiming for medical courses. The SAT, in contrast, serves as a gateway for international education, particularly in the United States. This guide aims to provide a detailed, notes-style exposition of each examination, covering syllabus, exam pattern, subject-wise preparation, study strategies, sample questions, FAQs, and references to essential notes like JEE Chemistry, JEE Physics, and JEE Math.
About JEE
What is JEE Main?
The JEE Main examination is conducted by the National Testing Agency (NTA) for students seeking admission to undergraduate engineering programs at National Institutes of Technology (NITs), Indian Institutes of Information Technology (IIITs), and other centrally funded technical institutions. The exam tests students in three subjects: Physics, Chemistry, and Mathematics. Candidates aspiring to qualify for JEE Advanced, which leads to the Indian Institutes of Technology (IITs), must perform exceptionally well in JEE Main. The examination is computer-based, typically consisting of multiple-choice and numerical questions with a total score of around 300 marks. Understanding the detailed syllabus, practicing previous years’ papers, and managing time effectively are key to achieving high scores.
What is JEE Advanced?
JEE Advanced is the next stage for students who have cleared the JEE Main with top scores. It is considered one of the most challenging engineering entrance examinations globally. The exam pattern varies each year but usually includes two papers comprising multiple-choice questions, numerical problems, and conceptual analytical questions. Unlike JEE Main, which tests fundamental understanding, JEE Advanced assesses a deeper application of concepts. Preparation requires rigorous practice, conceptual clarity, and frequent mock tests. Reference notes like JEE Chemistry, JEE Physics, and JEE Math play a vital role in preparation.
JEE Syllabus & Preparation
The JEE Syllabus spans the entire NCERT Class 11 and 12 curriculum in Physics, Chemistry, and Mathematics. Important chapters in Physics include Mechanics, Electricity and Magnetism, Thermodynamics, and Modern Physics. Chemistry is divided into Physical, Organic, and Inorganic, while Mathematics covers Algebra, Calculus, Trigonometry, and Coordinate Geometry. Effective preparation involves daily practice, topic-wise revision, solving previous years’ questions, and taking sectional and full-length mock tests. Structured study plans, time management, and consistent revision using resources like JEE Chemistry notes, JEE Physics notes, and JEE Math notes ensure comprehensive coverage and readiness for both JEE Main and JEE Advanced.
Subject Wise Notes
Physics: Focus on conceptual clarity, formulas, and numerical problem-solving. Regular practice using JEE Physics notes helps build confidence and accuracy. Chemistry: Emphasis should be placed on understanding mechanisms, reactions, and problem-solving strategies. JEE Chemistry notes are critical for revising key concepts. Mathematics: Develop problem-solving speed and accuracy through consistent practice, using JEE Math notes for reference. Integrate formula sheets, previous years’ questions, and timed mock tests to enhance performance.
About NEET
NEET Exam Details
The NEET (National Eligibility cum Entrance Test) is the sole medical entrance examination in India for admission into MBBS, BDS, and other allied medical courses. Conducted annually, NEET evaluates students in Physics, Chemistry, and Biology, primarily based on the NCERT syllabus of Classes 11 and 12. The examination is generally pen-and-paper-based and includes 180 multiple-choice questions, with a total score of 720 marks. Proper understanding of concepts, diagrammatic learning for Biology, and extensive practice in Physics and Chemistry numerical problems are essential for excelling in NEET.
Biology, Physics, Chemistry Preparation
Biology forms the core of NEET, with approximately 50% weightage. Students should focus on Botany, Zoology, Genetics, Human Physiology, and Ecology, making use of charts and diagrammatic representations for faster recall. Physics and Chemistry require problem-solving skills and conceptual understanding. Consistent practice using previous years’ papers and mock tests enhances accuracy and time management. NCERT textbooks and reference materials, coupled with dedicated coaching or self-study, form a comprehensive preparation strategy.
About SAT
Exam Overview and Strategy
The SAT is an internationally recognized standardized test primarily used for undergraduate admissions in the United States and other countries. It evaluates students in two main areas: Evidence-Based Reading and Writing, and Mathematics. The SAT requires strong analytical reasoning, problem-solving ability, and time management. Unlike JEE or NEET, the SAT emphasizes logical reasoning and comprehension rather than rote memorization. Preparation involves practice tests, reviewing official SAT sample questions, and developing strategies to tackle time constraints efficiently. Aspirants may supplement preparation with online resources and guided study plans. Understanding your strengths and weaknesses is crucial for devising a personal study schedule, optimizing preparation, and achieving competitive scores.
Comparative Analysis (NEET vs JEE vs SAT)
Choosing between NEET, JEE, and SAT depends on career aspirations. NEET is specifically designed for medical aspirants, emphasizing biological sciences, while JEE caters to engineering aspirants with a strong focus on Physics, Chemistry, and Mathematics. SAT, on the other hand, is geared toward international university admissions and emphasizes critical thinking, quantitative skills, and language comprehension. Time management, disciplined study routines, and targeted practice are universal strategies applicable to all these examinations. Comparative analysis of syllabus, exam pattern, preparation methods, and required skill sets helps students make informed decisions based on their strengths and career goals.
Preparation Strategy
A structured preparation strategy is essential for success in competitive examinations. For JEE and NEET, aspirants should begin with a thorough understanding of the NCERT syllabus, reinforced by notes such as JEE Chemistry, JEE Physics, and JEE Math. Students should create a timetable that balances concept learning, problem-solving, revision, and mock tests. Mock tests should be analyzed critically to identify weak areas and improve accuracy and speed. For SAT, practice with official sample questions and timed tests is crucial. Maintaining health, consistent sleep, and stress management are equally important. Interactive learning methods, peer discussions, and guided mentorship can enhance retention and application of knowledge. Revisiting difficult topics regularly, maintaining error logs, and creating summary sheets ensure comprehensive preparation.
FAQs
Which exam should I choose?
Selection between NEET, JEE, and SAT depends on individual career goals. Medical aspirants should focus on NEET, engineering aspirants on JEE, and students seeking international admissions should prepare for SAT. Overlaps exist in Physics and Chemistry for NEET and JEE, but Biology and Mathematics content differs significantly.
How many hours per day should I study?
Quality of study is more important than quantity. Aim for 6–8 focused hours daily, divided into concept learning, practice, revision, and mock tests. Incorporate short breaks, adequate sleep, and recreational activities to maintain mental health and sustained performance.
How to use mock tests effectively?
Take mock tests under real exam conditions, analyze errors meticulously, identify weak topics, and adjust your study plan accordingly. Use error logs, summary notes, and past papers for focused practice. Time management and accuracy improvement are key outcomes of regular mock testing.
Conclusion
Excelling in competitive examinations such as JEE, NEET, and SAT requires a blend of conceptual understanding, consistent practice, disciplined time management, and strategic revision. Utilizing resources like JEE Chemistry notes, JEE Physics notes, and JEE Math notes, following a structured study schedule, and engaging in regular mock tests will enhance preparation quality. Understanding exam patterns, practicing previous years’ questions, and staying motivated are crucial to success. Additionally, maintaining physical and mental well-being, and seeking guidance through contact channels or mentorship, ensures a holistic preparation approach. For more detailed guidance, students may refer to the JEE Overview, the complete JEE Syllabus, or navigate back to Home for structured resources. Always remember that perseverance, consistency, and strategic planning are the key pillars to achieving excellence in any competitive examination while complying with best practices outlined in the Privacy Policy.
Hydrocarbons - JEE Main & Advanced
1. Introduction to Hydrocarbons
1.1 Definition and Classification
- Hydrocarbons: Compounds containing only carbon and hydrogen atoms
- Classification:
- Aliphatic: Open chain compounds
- Saturated: Alkanes
- Unsaturated: Alkenes, Alkynes
- Aromatic: Benzene and its derivatives
- Alicyclic: Cyclic aliphatic compounds
- Aliphatic: Open chain compounds
1.2 General Formula
| Hydrocarbon Type | General Formula | Hybridization | Bond Angle |
|---|---|---|---|
| Alkanes | CnH2n+2 | sp³ | 109.5° |
| Alkenes | CnH2n | sp² | 120° |
| Alkynes | CnH2n-2 | sp | 180° |
| Cycloalkanes | CnH2n | sp³ | Varies with ring size |
2. Alkanes (Paraffins)
2.1 Preparation Methods
| Method | Reaction | Conditions/Remarks |
|---|---|---|
| Hydrogenation of Alkenes/Alkynes | R-CH=CH₂ + H₂ → R-CH₂-CH₃ | Ni/Pt/Pd catalyst, 200-300°C |
| Wurtz Reaction | 2R-X + 2Na → R-R + 2NaX | Dry ether, gives alkane with even number of carbons |
| Decarboxylation | R-COONa + NaOH → R-H + Na₂CO₃ | Soda lime, heat |
| Kolbe's Electrolysis | 2R-COO⁻ → R-R + 2CO₂ | Aqueous sodium/potassium salt |
| Reduction of Alkyl Halides | R-X + 2[H] → R-H + HX | Zn/HCl, LiAlH₄, or Zn-Cu/ethanol |
2.2 Chemical Properties
| Reaction Type | Reaction | Mechanism | Remarks |
|---|---|---|---|
| Halogenation | CH₄ + Cl₂ → CH₃Cl + HCl | Free radical substitution | Sunlight/heat, follows reactivity order: F₂ > Cl₂ > Br₂ > I₂ |
| Combustion | CH₄ + 2O₂ → CO₂ + 2H₂O + Heat | Oxidation | Complete combustion gives CO₂ + H₂O |
| Isomerization | n-butane → iso-butane | Rearrangement | AlCl₃/HCl catalyst |
| Aromatization | n-hexane → benzene | Cyclization and dehydrogenation | Cr₂O₃/Al₂O₃, 773K |
2.3 Conformations of Alkanes
- Ethane: Staggered (more stable) and Eclipsed conformations
- Butane: Anti (most stable), Gauche, Eclipsed conformations
- Energy Difference: Staggered to Eclipsed = 12.5 kJ/mol for ethane
3. Alkenes (Olefins)
3.1 Preparation Methods
| Method | Reaction | Conditions/Remarks |
|---|---|---|
| Dehydration of Alcohols | CH₃-CH₂-OH → CH₂=CH₂ + H₂O | Conc. H₂SO₄, 443K |
| Dehydrohalogenation | CH₃-CH₂-Br → CH₂=CH₂ + HBr | Alcoholic KOH, heat |
| Dehalogenation | CH₂Br-CH₂Br + Zn → CH₂=CH₂ + ZnBr₂ | Zn, alcohol |
| Partial Hydrogenation | HC≡CH + H₂ → CH₂=CH₂ | Lindlar's catalyst (Pd/BaSO₄) |
3.2 Chemical Properties
| Reaction Type | Reaction | Mechanism | Regioselectivity |
|---|---|---|---|
| Addition of Hydrogen | R-CH=CH₂ + H₂ → R-CH₂-CH₃ | Catalytic hydrogenation | - |
| Addition of Halogens | R-CH=CH₂ + Br₂ → R-CHBr-CH₂Br | Electrophilic addition | Anti addition |
| Addition of HX | R-CH=CH₂ + HBr → R-CHBr-CH₃ | Electrophilic addition | Markovnikov's rule |
| Addition of H₂O | R-CH=CH₂ + H₂O → R-CH(OH)-CH₃ | Electrophilic addition | Markovnikov's rule |
| Ozonolysis | R-CH=CH-R' → R-CHO + R'-CHO | Cleavage of double bond | - |
| Oxidation | R-CH=CH₂ → R-COOH + CO₂ | Oxidative cleavage | Hot KMnO₄ (Baeyer's reagent) |
3.3 Markovnikov's Rule and Anti-Markovnikov Addition
Markovnikov's Rule:
"In the addition of unsymmetrical reagents to unsymmetrical alkenes, the negative part of the addendum goes to the carbon atom with lesser number of hydrogen atoms."
Anti-Markovnikov Addition (Peroxide Effect):
In presence of peroxides, HBr adds contrary to Markovnikov's rule
CH₃-CH=CH₂ + HBr → CH₃-CH₂-CH₂Br (with peroxide)
Only for HBr, not for HCl or HI
4. Alkynes
4.1 Preparation Methods
| Method | Reaction | Conditions/Remarks |
|---|---|---|
| Dehydrohalogenation | CH₃-CHBr₂ → HC≡CH | Alcoholic KOH, heat |
| From Calcium Carbide | CaC₂ + 2H₂O → HC≡CH + Ca(OH)₂ | Industrial method for acetylene |
| Kolbe's Electrolysis | 2CH₂(COOK)₂ → HC≡CH + 2CO₂ | From potassium salts of dicarboxylic acids |
4.2 Chemical Properties
| Reaction Type | Reaction | Remarks |
|---|---|---|
| Acidic Character | HC≡CH + Na → HC≡CNa + ½H₂ | Only terminal alkynes show acidic character |
| Addition Reactions | HC≡CH + 2H₂ → CH₃-CH₃ | Complete hydrogenation to alkane |
| Addition of Halogens | HC≡CH + 2Br₂ → CHBr₂-CHBr₂ | Stepwise addition |
| Addition of Water | HC≡CH + H₂O → CH₃-CHO | HgSO₄/H₂SO₄ catalyst, gives acetaldehyde |
| Oxidation | HC≡CH → CO₂ + H₂O | Hot KMnO₄ gives complete oxidation |
| Ozonolysis | R-C≡C-R' → R-COOH + R'-COOH | Oxidative cleavage |
4.3 Polymerization
- Linear Polymerization: HC≡CH → (CH=CH)ₙ (Polyacetylene)
- Cyclic Polymerization: 3HC≡CH → C₆H₆ (Benzene)
- Uses: Acetylene used in welding, chemical synthesis
5. Aromatic Hydrocarbons
5.1 Benzene Structure and Aromaticity
- Kekulé Structure: Alternating single and double bonds
- Resonance: Delocalized π-electron cloud
- Aromaticity Criteria (Hückel's Rule):
- Planar cyclic molecule
- Complete delocalization of π-electrons
- (4n + 2) π-electrons
- Bond Length: All C-C bonds equal (1.39 Å)
5.2 Preparation Methods
| Method | Reaction | Conditions/Remarks |
|---|---|---|
| Cyclic Polymerization | 3C₂H₂ → C₆H₆ | Red hot iron tube, 873K |
| Decarboxylation | C₆H₅-COONa + NaOH → C₆H₆ + Na₂CO₃ | Soda lime, heat |
| Reduction of Phenol | C₆H₅-OH + Zn → C₆H₆ + ZnO | Zinc dust |
5.3 Electrophilic Substitution Reactions
| Reaction | Reagent | Product | Catalyst/Conditions |
|---|---|---|---|
| Nitration | HNO₃ | C₆H₅-NO₂ | Conc. H₂SO₄, 330K |
| Sulphonation | H₂SO₄ | C₆H₅-SO₃H | Conc. H₂SO₄ or oleum |
| Halogenation | X₂ | C₆H₅-X | FeX₃ or Fe |
| Friedel-Crafts Alkylation | R-X | C₆H₅-R | Anhydrous AlCl₃ |
| Friedel-Crafts Acylation | R-CO-X | C₆H₅-COR | Anhydrous AlCl₃ |
5.4 Directive Influence of Substituents
| Type of Substituent | Effect | Orientation | Examples |
|---|---|---|---|
| Ortho-para directing activators | +I or +M effect | o-, p- | -OH, -NH₂, -OCH₃, -CH₃ |
| Ortho-para directing deactivators | -I effect > +M effect | o-, p- | -F, -Cl, -Br, -I |
| Meta directing deactivators | -I and -M effect | m- | -NO₂, -CN, -CHO, -COOH |
6. Carcinogenicity and Toxicity
6.1 Carcinogenic Hydrocarbons
- Benzopyrene: Found in coal tar, cigarette smoke
- Benzanthracene: Potent carcinogen
- Chrysene: Found in coal tar
6.2 Environmental Impact
- Polycyclic aromatic hydrocarbons (PAHs) are environmental pollutants
- Formed during incomplete combustion of organic matter
- Can contaminate air, water, and soil
Practice Questions (JEE & NEET Level)
JEE Main Question:
Which of the following will not form yellow precipitate on heating with iodine in presence of NaOH?
(a) CH₃CH₂OH (b) CH₃CH₂CH₂OH (c) CH₃COCH₃ (d) CH₃CH(OH)CH₃
Answer: (a) CH₃CH₂OH (Only methyl carbinol gives iodoform test)
NEET Question:
The compound that will react most readily with gaseous bromine has the formula:
(a) C₃H₆ (b) C₂H₂ (c) C₄H₁₀ (d) C₂H₄
Answer: (d) C₂H₄ (Alkenes react faster than alkynes with Br₂)
JEE Advanced Question:
In the reaction: CH₃-C≡CH → X → Y, where X is obtained by reaction with NaNH₂ and Y is obtained by reaction with CH₃Br. Y is:
(a) Propene (b) 1-Butyne (c) 1-Butene (d) 2-Butyne
Answer: (b) 1-Butyne
NEET Question:
Which of the following is an aromatic compound?
(a) Cyclopentadienyl cation (b) Cycloheptatrienyl cation
(c) Cyclooctatetraene (d) Cycloheptatrienyl anion
Answer: (b) Cycloheptatrienyl cation (6π electrons)
JEE Main Question:
In the reaction: C₆H₅CH₃ + Cl₂ → X (in presence of light), X is:
(a) o-chlorotoluene (b) p-chlorotoluene (c) Benzyl chloride (d) m-chlorotoluene
Answer: (c) Benzyl chloride (Side chain chlorination)
Key Takeaways
- Understand preparation methods for different hydrocarbons
- Memorize chemical reactions and their mechanisms
- Know Markovnikov's rule and exceptions
- Learn aromaticity criteria and electrophilic substitution
- Understand directive influence of substituents
- Practice conformational analysis
- Remember environmental and health impacts
Environmental Chemistry - JEE Main & Advanced
1. Introduction to Environmental Chemistry
1.1 Definition and Scope
- Environmental Chemistry: Study of chemical and biochemical phenomena occurring in the environment
- Components of Environment:
- Atmosphere
- Hydrosphere
- Lithosphere
- Biosphere
- Pollutant: Substance present in concentration higher than natural levels and causes harmful effects
- Contaminant: Substance that does not occur in environment but when added, changes its quality
1.2 Segments of Environment
| Segment | Composition | Thickness/Volume |
|---|---|---|
| Atmosphere | N₂ (78%), O₂ (21%), Ar (0.9%), CO₂ (0.03%) | ~1000 km |
| Hydrosphere | Oceans, seas, rivers, lakes, groundwater | ~1.4 billion km³ |
| Lithosphere | Rocks, minerals, soil | ~100 km thick |
| Biosphere | All living organisms | Zone where life exists |
2. Atmospheric Pollution
2.1 Tropospheric Pollution
| Pollutant | Sources | Effects | Control Measures |
|---|---|---|---|
| Carbon Monoxide (CO) | Incomplete combustion of fuels, automobile exhaust | Binds with hemoglobin, causes suffocation, headache | Catalytic converters, proper combustion |
| Sulphur Dioxide (SO₂) | Burning of coal and petroleum, smelting | Respiratory problems, acid rain, corrosion | Scrubbers, use of low sulphur fuels |
| Nitrogen Oxides (NO, NO₂) | Automobile exhaust, power plants | Acid rain, smog, respiratory issues | Catalytic converters, selective catalytic reduction |
| Hydrocarbons | Incomplete combustion, petroleum refining | Smog formation, carcinogenic | Vapor recovery systems |
| Particulate Matter | Dust, smoke, fly ash | Respiratory diseases, reduced visibility | Electrostatic precipitators, bag filters |
2.2 Stratospheric Pollution
- Ozone Layer: O₃ in stratosphere (15-35 km altitude)
- Function: Absorbs harmful UV radiation (200-315 nm)
- Ozone Depletion: Caused by CFCs, NO, CCl₄
- Mechanism:
CF₂Cl₂ → CF₂Cl• + Cl•
Cl• + O₃ → ClO• + O₂
ClO• + O → Cl• + O₂
- Effects: Skin cancer, cataract, damage to plants
3. Greenhouse Effect and Global Warming
3.1 Greenhouse Gases
| Gas | Sources | Global Warming Potential | Atmospheric Lifetime |
|---|---|---|---|
| Carbon Dioxide (CO₂) | Respiration, combustion, deforestation | 1 | 50-200 years |
| Methane (CH₄) | Rice fields, livestock, landfills | 25 | 12 years |
| Nitrous Oxide (N₂O) | Fertilizers, combustion | 298 | 114 years |
| Chlorofluorocarbons (CFCs) | Refrigerants, aerosols | 4750-14400 | 45-1700 years |
3.2 Effects of Global Warming
- Rise in sea level (melting of glaciers)
- Changes in weather patterns
- Impact on agriculture and food production
- Extinction of species
- Spread of tropical diseases
3.3 Control Measures
- Reducing fossil fuel consumption
- Afforestation and reforestation
- Using renewable energy sources
- Energy conservation
- International agreements (Kyoto Protocol, Paris Agreement)
4. Water Pollution
4.1 Types of Water Pollutants
| Pollutant Type | Examples | Effects |
|---|---|---|
| Pathogens | Bacteria, viruses, protozoa | Water-borne diseases (cholera, typhoid) |
| Organic Wastes | Sewage, animal waste, food processing waste | Oxygen depletion, eutrophication |
| Chemical Pollutants | Heavy metals, pesticides, fertilizers | Toxicity, bioaccumulation |
| Sediments | Soil erosion, construction | Turbidity, habitat destruction |
| Radioactive Substances | Nuclear power plants, medical waste | Genetic mutations, cancer |
| Heat | Thermal power plants | Decreased oxygen solubility |
4.2 Water Quality Parameters
| Parameter | Definition | Significance |
|---|---|---|
| Dissolved Oxygen (DO) | Oxygen dissolved in water | Indicator of water quality, >4 mg/L for aquatic life |
| Biochemical Oxygen Demand (BOD) | Oxygen required by microorganisms to decompose organic matter | Measure of organic pollution, < 5 mg/L for clean water |
| Chemical Oxygen Demand (COD) | Oxygen required to chemically oxidize organic matter | Measure of total organic content |
| pH | Acidity or alkalinity | 6.5-8.5 for most aquatic life |
4.3 Eutrophication
- Definition: Excessive growth of algae and aquatic plants due to nutrient enrichment
- Causes: Runoff containing fertilizers, sewage discharge
- Effects: Oxygen depletion, fish kills, loss of biodiversity
- Control: Proper wastewater treatment, reduced fertilizer use
5. Soil Pollution
5.1 Major Soil Pollutants
| Pollutant | Sources | Effects |
|---|---|---|
| Pesticides | Agriculture, vector control | Bioaccumulation, toxicity to non-target organisms |
| Heavy Metals | Industrial waste, mining | Toxicity, soil infertility |
| Industrial Wastes | Chemical industries, manufacturing | Soil degradation, groundwater contamination |
| Plastics | Packaging, consumer products | Non-biodegradable, affects soil structure |
| Radioactive Materials | Nuclear accidents, medical waste | Long-term contamination, health hazards |
5.2 Effects of Soil Pollution
- Reduced soil fertility
- Contamination of groundwater
- Bioaccumulation in food chain
- Health problems in humans and animals
- Loss of biodiversity
5.3 Control Measures
- Proper waste management
- Use of biodegradable products
- Organic farming
- Bioremediation
- Afforestation
6. Industrial Waste Management
6.1 Types of Industrial Waste
| Waste Type | Examples | Treatment Methods |
|---|---|---|
| Inorganic Waste | Acids, alkalis, heavy metals | Neutralization, precipitation, ion exchange |
| Organic Waste | Solvents, oils, pesticides | Incineration, biological treatment |
| Gaseous Waste | SO₂, NOₓ, CO₂ | Scrubbing, adsorption, catalytic conversion |
| Hazardous Waste | Toxic chemicals, radioactive materials | Secure landfill, chemical treatment |
6.2 Waste Treatment Technologies
- Physical Methods: Sedimentation, filtration, flotation
- Chemical Methods: Neutralization, oxidation, precipitation
- Biological Methods: Aerobic and anaerobic treatment
- Thermal Methods: Incineration, pyrolysis
7. Green Chemistry
7.1 Principles of Green Chemistry
- Prevention: Better to prevent waste than to treat it
- Atom Economy: Maximize incorporation of all materials into final product
- Less Hazardous Synthesis: Use and generate non-toxic substances
- Designing Safer Chemicals: Maintain efficacy while reducing toxicity
- Safer Solvents: Avoid using auxiliary substances
- Energy Efficiency: Conduct reactions at ambient conditions
- Renewable Feedstocks: Use renewable raw materials
- Reduce Derivatives: Avoid unnecessary derivatization
- Catalysis: Prefer catalytic over stoichiometric reagents
- Design for Degradation: Products should break down to harmless substances
- Real-time Analysis: Develop analytical methods for pollution prevention
- Inherently Safer Chemistry: Minimize potential for accidents
7.2 Examples of Green Chemistry
| Traditional Process | Green Alternative | Benefits |
|---|---|---|
| Chlorine for bleaching | Hydrogen peroxide | No toxic chlorinated compounds |
| Phosgene for polycarbonates | Diphenyl carbonate | Eliminates highly toxic phosgene |
| CFCs as refrigerants | HFCs, natural refrigerants | No ozone depletion |
| Organic solvents | Supercritical CO₂ | Non-toxic, recyclable |
8. Strategies for Pollution Control
8.1 Air Pollution Control
| Technology | Principle | Applications |
|---|---|---|
| Electrostatic Precipitator | Charged particles attracted to oppositely charged plates | Thermal power plants, cement industries |
| Scrubber | Gas passed through liquid to remove pollutants | Removal of SO₂ from flue gases |
| Catalytic Converter | Catalyst converts pollutants to harmless gases | Automobile exhaust treatment |
| Bag Filter | Fabric filters trap particulate matter | Dust collection in various industries |
8.2 Water Pollution Control
- Primary Treatment: Physical removal of suspended solids
- Secondary Treatment: Biological degradation of organic matter
- Tertiary Treatment: Chemical treatment for specific pollutants
- Advanced Methods: Reverse osmosis, activated carbon adsorption
8.3 Solid Waste Management
- Reduce: Minimize waste generation
- Reuse: Use items multiple times
- Recycle: Convert waste into new products
- Recover: Extract energy from waste
- Dispose: Safe disposal of residual waste
Practice Questions (JEE & NEET Level)
JEE Main Question:
Which of the following is not a greenhouse gas?
(a) CO₂ (b) CH₄ (c) O₂ (d) CFCs
Answer: (c) O₂
NEET Question:
The gas which is mainly responsible for ozone depletion is:
(a) CO₂ (b) SO₂ (c) CFCs (d) CO
Answer: (c) CFCs
JEE Advanced Question:
In the context of 'green chemistry', the term 'atom economy' refers to:
(a) Cost of atoms used (b) Efficiency of atom usage in reaction
(c) Number of atoms in product (d) Molecular weight of product
Answer: (b) Efficiency of atom usage in reaction
NEET Question:
Biochemical Oxygen Demand (BOD) is a measure of:
(a) Industrial waste poured into water bodies
(b) Amount of oxygen needed by green plants during night
(c) Amount of oxygen required by bacteria to decompose organic waste
(d) Amount of oxygen needed by phosphates in water
Answer: (c) Amount of oxygen required by bacteria to decompose organic waste
JEE Main Question:
Which of the following is not a component of photochemical smog?
(a) O₃ (b) NO₂ (c) SO₂ (d) Unsaturated hydrocarbons
Answer: (c) SO₂ (SO₂ causes classical smog, not photochemical smog)
Key Takeaways
- Understand different types of environmental pollution
- Learn sources and effects of major pollutants
- Know greenhouse effect and ozone depletion mechanisms
- Understand water quality parameters (BOD, COD, DO)
- Memorize principles of green chemistry
- Learn pollution control technologies
- Understand waste management strategies