RBSE SS Chemistry study plan

Assign oxidation states and hybridisation for the oxoacids of chlorine, sulphur and phosphorus, and sketch the structures of H2S2O7, H4P2O7, H3PO3 and H2S2O8 counting terminal and bridging bonds.

Predict and justify group trends in atomic radius, ionisation enthalpy and oxidising power across groups 15–18 using bond dissociation enthalpy, inert-pair effect and hydration enthalpy arguments.

Write balanced equations for the preparation, hydrolysis and disproportionation of XeF2, XeF4 and XeF6, and for the interhalogen reactions of ClF3 and ICl with water and alkali.

Explain the anomalous behaviour of fluorine, oxygen and nitrogen by citing three concrete pieces of evidence each, rather than listing labels.

Complete 30 timed MCQs on groups 15–18 and log each error against the sub-topic that caused it.

Apply the Nernst equation and the relation between EMF and Gibbs energy to calculate cell potential, equilibrium constant and spontaneity for a given cell at non-standard concentrations.

Use Kohlrausch's law and molar conductivity data to compute the degree of dissociation and dissociation constant of a weak electrolyte.

Calculate the mass deposited or gas liberated from a current–time electrolysis problem using Faraday's laws, showing unit conversions explicitly.

Compare the working of a fuel cell, a lead–acid accumulator and lithium-ion cells on electrolyte, electrode reactions and practical limitation.

Explain rusting and corrosion control methods (galvanising, cathodic protection, sacrificial anodes) using the electrochemical cell model.

Write the electronic configuration of every 3d series element and account for each anomaly of chromium and copper using exchange energy and stability arguments.

Explain the trends in metallic radius, melting point, ionisation enthalpy and oxidation state of the 3d series in terms of exchange pairing, effective nuclear charge and screening.

Assign the number of unpaired electrons, spin-only magnetic moment and expected colour of a complex ion or hydrated ion using crystal field or exchange-pairing reasoning.

Describe the preparation and characteristic reactions of KMnO4 and K2Cr2O7, assigning the oxidation-state change in each reaction medium.

Compare lanthanoids and actinoids, and derive three consequences of the lanthanoid contraction.

Name at least fifteen coordination compounds by IUPAC rules, including those with bridging ligands, anionic complex ions and hydrates.

Enumerate all possible stereoisomers and structural isomers for a stated formula such as [Co(NH3)4Cl2]+ or [Co(en)2Cl2]+ and label each type of isomerism.

Draw crystal-field splitting diagrams for octahedral and tetrahedral environments, then compute CFSE and predict high-spin or low-spin behaviour for a stated d configuration.

Use valence bond theory and crystal field theory side by side to explain the magnetic behaviour of [Fe(CN)6]3− versus [Fe(H2O)6]3+, and state where VBT fails.

Rank ligands by the spectrochemical series and explain the chelate effect and the thermodynamic origin of complex stability.

Select SN1, SN2, E1 or E2 for a given substrate, nucleophile, solvent and temperature, and justify the choice with at least two independent lines of evidence.

Draw curved-arrow mechanisms for Finkelstein, Swarts, Sandmeyer, Williamson ether synthesis, Reimer–Tiemann and Kolbe reactions.

Explain the relative acidity of phenol, o-nitrophenol and p-nitrophenol using resonance and inductive effects, and predict the product of phenol with Br2 water versus dilute HNO3.

Distinguish primary, secondary and tertiary alcohols by specific chemical tests, and give the reagent and observation for each test.

Predict the products of ether cleavage by HX and explain why aryl ethers resist cleavage.

Explain the mechanism of nucleophilic addition to a carbonyl group and rank formaldehyde, acetaldehyde and acetone by reactivity using steric and electronic factors.

Write products and name the reaction type for aldol condensation, Cannizzaro, Claisen–Schmidt, Hell–Volhard–Zelinsky, Clemmensen, Wolff–Kishner and haloform reactions.

Rank carboxylic acids and their derivatives (acid chloride, anhydride, ester, amide) by reactivity and justify the order by leaving-group ability and resonance.

Order amines, ammonia and substituted anilines by basicity in aqueous solution using solvation, steric and resonance effects, and test that order against a stated set of four compounds.

Describe the Hinsberg, carbylamine, Hoffmann bromamide and diazonium coupling reactions, giving the reagent, the visible observation and the product class.

Calculate relative lowering of vapour pressure, boiling-point elevation, freezing-point depression and osmotic pressure for electrolyte and non-electrolyte solutions, inserting the van't Hoff factor where required.

Interpret positive and negative deviations from Raoult's law and predict azeotrope formation for stated binary mixtures.

Determine the order of a reaction from initial-rate and concentration–time data, then write the corresponding rate law and unit of the rate constant.

Apply zero- and first-order integrated rate equations and half-life relations to numerical problems, and distinguish order from molecularity.

Use the Arrhenius equation to compute activation energy from two rate constants, and explain how a catalyst or a temperature rise changes rate without changing equilibrium position.

Compute packing efficiency, unit-cell edge length, density and number of formula units per cell for simple cubic, bcc, fcc and hcp structures.

Distinguish Schottky and Frenkel defects and predict which ionic solids adopt each, then relate the defect to density and electrical behaviour.

Compare physisorption and chemisorption and apply the Freundlich isotherm and Langmuir model to given adsorption data.

Classify carbohydrates, proteins and nucleic acids by structure and linkage, and distinguish addition from condensation polymers with two named examples of each.

Link drug classes, food preservatives and cleansing agents to their chemical structure and mode of action.