BITSAT (Birla Institute of Technology and Science Admission Test) is a speed test which requires conceptual clearness in maximum strength, particularly in Chemistry where there are numerous direct but lengthy questions. This guide identifies the most expected topics in tables and to-the-point points for instant yet effective revision. Revise this before your mocks, and you will be entering sharper and more confident!
1. Basic Concepts & Atomic Structure
Atomic structure forms the foundation of chemistry and is examined frequently.
- Atomic models include the quantum mechanical model (orbitals), Rutherford's nuclear model, Bohr's quantized orbits, Thomson's plum pudding, and Dalton's atomic indivisibility.
- Quantum numbers: Describe the electron's location and energy. Spin (s), magnetic (m), azimuthal (l), and principal (n).
- Electronic Configuration: Fill the orbitals using the Pauli Exclusion Principle, Hund's Rule, and Aufbau Principle.
- Isotopes: Same atomic number, but different mass (e.g., ¹H, ²H, ³H).
- Oxidation States: Familiar with common states such as Fe²⁺ (ferrous), Fe³⁺ (ferric)
2. Periodic Table & Periodicity
Identifying trends enables you to make rapid predictions of reactivity and properties.
- Modern Table: Elements arranged by atomic number.Blocks: s, p, d, f.
- Trends:
- Atomic radius decreases down a period but increases down a group.
- Ionization energy and electronegativity increase up periods but decrease down groups.
- Electron affinity tends to increase down periods.
- Diagonal Relationship: Lithium is analogous to magnesium; beryllium is analogous to aluminum — watch out for this MCQ trap!
3. Chemical Bonding & Molecular Structure
This chapter is accountable for determining molecular geometry, polarities, and strengths of bonds.
- Types of Bonds:
- Ionic (NaCl), covalent (H₂O), metallic (Fe).
- Covalent bonds are polar (HCl) or non-polar (O₂).
- VSEPR Theory explains molecular shape because of electron pair repulsion.
- Hybridization tells us about bonding orbitals:
- sp (linear), sp² (trigonal planar), sp³ (tetrahedral).
- Intermolecular Forces: H-bonding (strongest), dipole-dipole, Van der Waals (weakest).
- Bond Strength: Shorter bonds are stronger (triple > double > single).
4. States of Matter & Gas Laws
Numericals that occur quite frequently include gas laws and solid state principles.
- Ideal Gas Equation: PV = nRT
- Laws:
- Boyle's: P ∝ 1/V (T constant)
- Charles's: V ∝ T (P constant)
- Dalton's Law: P_total = P₁ + P₂ +
- Real Gases: Low temperature, high pressure.
- Solids: Crystalline (NaCl) or amorphous (glass).
5. Thermodynamics & Equilibrium
These are principles that predict direction and probability of reactions.
- First Law: Energy is conserved (ΔU = q + w).
- Enthalpy (ΔH): Heat at constant pressure.
- Entropy (ΔS): Measure of disorder.
- Gibbs Free Energy (ΔG): Used to determine spontaneity.
Delta G =Delta H - T\Delta S
- Equilibrium Constant (K): Product concentration to reactant concentration ratio at equilibrium.
- Le Chatelier's Principle: System shifts to oppose change (pressure, temp, concentration).
6. Electrochemistry
A combination of redox with potential calculations — a BITSAT favorite!
- Redox: Oxidation = loss of electrons, Reduction = gain of electrons.
- Nernst Equation:
E=E∘−n0.0591 log Q
- Galvanic Cells: Electrical energy from chemical energy (e.g., Daniell cell: Zn | Zn²⁺ || Cu²⁺ | Cu).
- Corrosion: Rusting of iron by electrochemical reaction; prevented by sacrificial anodes (zinc coating).
7. Chemical Kinetics & Surface Chemistry
Time-based questions of this chapter.
- Rate Law: Rate = k[A]ᵐ[B]ⁿ
- Order of Reaction: Sum of exponents in rate law.
- Arrhenius Equation:
k=Ae−RT/Ea
- Catalysis: Accelerates reactions without being consumed.
Homogeneous (same phase), Heterogeneous (different phase).
- Adsorption:
Physical (Van der Waals) vs Chemical (formation of bonds).
8. Main Group & p-Block Elements
- Group 1 & 2: Alkali (Li, Na, K) and alkaline earth metals (Mg, Ca). Extremely reactive, give strong bases.
- p-Block: Boron group to noble gases.
- Familiarity with boron hydrides, aluminum halides, oxides of nitrogen and sulfur.
9. d- and f-Block Elements
They are the causes of color, magnetism, and complex formation.
- Transition Metals: Exhibit variable oxidation states (Fe²⁺/Fe³⁺), have colored ions. (Cu²⁺ blue, Fe³⁺ yellow-brown).
- Lanthanides/Actinides: f-block, utilized in magnets, lasers.
10. Coordination Compounds
Frequent BITSAT concepts are isomerism and nomenclature.
- Ligands: Neutral (H₂O), anionic (Cl⁻), cationic (NO⁺).
- Coordination Number: Donor atoms (e.g., 6 in [Fe(CN)₆]³⁻).
- Isomerism: Stereoisomerism (geometrical, optical) and structural.
11. Organic Chemistry
Usually has 20-25% weight in BITSAT chemistry!
- Concepts: Hybridization, resonance, inductive/mesomeric effects.
- Isomerism:
- Structural: Chain, position, functional group.
- Stereo: Geometric (cis-trans), optical (chiral centers).
- Reactions:
- Substitution: SN1, SN2
- Addition: Electrophilic, nucleophilic
- Elimination: E1, E2
- Functional Groups: Alcohols, ethers, aldehydes, ketones, acids, esters, amines.
12. Hydrocarbons & Derivatives
- Alkanes (CnH2n+2): Substitution reactions, saturated.
- Alkenes (CnH2n): Addition reactions, unsaturated.
- Alkynes (CnH2n-2): Triple bond, acidic hydrogen.
- Aromatic Compounds: Benzene undergoes electrophilic substitution (nitration, halogenation).
13. Environmental Chemistry & Everyday Life
- Pollutants: CO₂, SO₂, NOₓ (acid rain), CFCs (depletion of the ozone layer)
- Green Chemistry: Environmentally friendly chemical design (12 principles).
- Drugs: Antacids (aluminum hydroxide), analgesics (aspirin).
Final BITSAT Chemistry Tips:
Learn periodic trends and exceptions — they tend to crop up time and again.
- Practice numericals daily from gas laws, thermodynamics, and kinetics.
- Go through key organic mechanisms: SN1/SN2, E1/E2, addition reactions.
- Practice names and structures of coordination compounds.
- Attempt at least 10 full-length mock tests prior to D-day.
Best of luck! Concepts + practice = success in BITSAT Chemistry!
