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RESOURCES - chem imp sovind sir, Schemes and Mind Maps of Chemistry

California Institute of Technology (Caltech)Chemistry

ALL RESOURCES FOR CHEMISTRY(which I could humanly give)

Typology: Schemes and Mind Maps

2025/2026

Available from 04/26/2026

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SOLID STATE
1. distinguish between ionic solid and metallic solid.
2. explain the simple unit cell, body centred cell and face centred cell.
3. derive the relationship among molar mass, density of the substance and unit cell
edge length.
4. explain two-dimensional crystal in –
a) square close packing
b) hexagonal close packing
5. what is packing efficiency? find the packing efficiency of simple cubic cell.
6. calculate the packing efficiency of body centred and face centred cells.
7. explain –
a) frenkel defect b) schottky defect
c) self-interstitial defect d) impurity defect
8. define –
a) diamagnetic solid
b) paramagnetic solid
c) ferromagnetic solid.**
SOLUTIONS
1. state henry’s law. what is henry constant?
2. explain raoult’s law with graphical representation.
3. write four differences between ideal and non-ideal solution.
4. explain two types of deviation of non-ideal solution.
5. explain why vapour pressure lowering is a colligative property.
6. what is relative lowering of vapour pressure? derive the expression for molar
mass of solute from vapour pressure lowering.
7. explain boiling point elevation as a consequence of vapour pressure lowering.
8. what is freezing point depression? derive the expression for molar mass using
boiling point elevation.
9. define –
a) ebullioscopic constant
b) cryoscopic constant
10. what is isotonic, hypotonic and hypertonic solution?
11. what is osmotic pressure? derive the relation of osmotic pressure with molar
mass.
12. explain reverse osmosis with diagram.
13. what is van’t hoff factor? derive the relation between van’t hoff factor and degree
of dissociation.
IONIC EQUILIBRIA
1. explain –
a) bronsted–lowry proton transfer theory b) lewis theory for acid and base
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SOLID STATE

  1. distinguish between ionic solid and metallic solid.
  2. explain the simple unit cell, body centred cell and face centred cell.
  3. derive the relationship among molar mass, density of the substance and unit cell edge length.
  4. explain two-dimensional crystal in – a) square close packing b) hexagonal close packing
  5. what is packing efficiency? find the packing efficiency of simple cubic cell.
  6. calculate the packing efficiency of body centred and face centred cells.
  7. explain – a) frenkel defect b) schottky defect c) self-interstitial defect d) impurity defect
  8. define – a) diamagnetic solid b) paramagnetic solid c) ferromagnetic solid.**

SOLUTIONS

  1. state henry’s law. what is henry constant?
  2. explain raoult’s law with graphical representation.
  3. write four differences between ideal and non-ideal solution.
  4. explain two types of deviation of non-ideal solution.
  5. explain why vapour pressure lowering is a colligative property.
  6. what is relative lowering of vapour pressure? derive the expression for molar mass of solute from vapour pressure lowering.
  7. explain boiling point elevation as a consequence of vapour pressure lowering.
  8. what is freezing point depression? derive the expression for molar mass using boiling point elevation.
  9. define – a) ebullioscopic constant b) cryoscopic constant
  10. what is isotonic, hypotonic and hypertonic solution?
  11. what is osmotic pressure? derive the relation of osmotic pressure with molar mass.
  12. explain reverse osmosis with diagram.
  13. what is van’t hoff factor? derive the relation between van’t hoff factor and degree of dissociation.

IONIC EQUILIBRIA

  1. explain – a) bronsted–lowry proton transfer theory b) lewis theory for acid and base

c) amphoteric nature of water d) ostwald’s dilution law of weak base e) hydrolysis of salt of strong acid and weak base f) hydrolysis of salt of weak acid and strong base

  1. define – a) conjugate acid–base pair b) ph of a solution c) poh of a solution d) hydrolysis of salt e) common ion effect
  2. what is ionic product of water?
  3. show that ph + poh = 14.
  4. what is buffer solution? explain the types of buffer solution.
  5. write applications of buffer solutions.

THERMODYNAMICS

  1. define – a) extensive property b) intensive property c) state function d) path function
  2. write the features of reversible process.
  3. derive the expression for pressure–volume work.
  4. derive the expression for maximum work done.
  5. state first law of thermodynamics. write the effect of different processes on it.
  6. derive the relation between Δh and Δu.
  7. define – a) bond enthalpy b) enthalpy of fusion c) enthalpy of solution
  8. state hess’s law and give its application.
  9. what is entropy? state the relation between change in entropy and temperature.
  10. state thermodynamics second law. derive the relation between Δg and Δs.
  11. write the condition for spontaneity with respect to entropy and gibbs energy.
  12. derive the expression for gibbs function and equilibrium constant.

ELECTORCHEM

  1. define – a) conductance b) conductivity c) molar conductivity d) cell constant
  2. state kohlrausch’s law of independent migration of ions.
  3. explain electrolysis of molten sodium chloride.
  4. define – mole ratio.
  5. explain salt bridge and its function.
  6. find the overall reaction of – ni(s) | ni²⁺(aq) || al³⁺(aq) | al(s).
  7. derive the expression for nernst equation.
  8. derive the relation between standard potential difference and change in gibbs energy.
  9. write the relation between standard cell potential and equilibrium constant.
  10. define – reference electrode.

D BLOCK

  1. explain interhalogen compounds.
  2. write characteristics of interhalogen compounds.
  3. write uses of inert gases.why does chromium show abnormal electronic configuration?
  4. explain the oxidation states of first transition series elements.
  5. find the magnetic moment of – a) mn²⁺ b) ni²⁺ c) v²⁺
  6. what is an interstitial compound? write four properties of interstitial compounds.
  7. why are most transition elements remarkably coloured?
  8. explain alloys and their types.
  9. write the uses of alloys.
  10. explain the following zones in the blast furnace – a) zone of combustion b) zone of reduction c) zone of slag formation
  11. write the electronic configuration of – a) fe³⁺ b) eu²⁺ c) yb²⁺
  12. explain lanthanoid contraction with its cause.
  13. write the uses of – a) lanthanoids b) actinoids
  14. write three similarities and differences between lanthanoids and actinoids.
  15. explain transuranic elements.

COORDINATION

  1. what is ligand? write the classification of ligands.
  2. define – a) coordination number b) coordination sphere
  3. distinguish between double salt and coordination complex.
  4. write the postulates of werner’s theory.
  5. explain the classification of coordination compounds on the basis of – a) types of ligands b) charge on the complex
  6. write the iupac names of the following – a) ag[al(c₂o₄)₂] b) [pt(en)₂(scn)₂] c) [fe(co)₅] d) [co(h₂o)₄(nh₃)₂]
  7. what is the effective atomic number? write its rule. find the ean of the following compounds – a) k₄[fe(cn)₆] b) [co(nh₃)₆]³⁺
  8. explain cis–trans isomerism in – a) octahedral complexes b) square planar complexes
  9. explain – a) linkage isomerism b) ionization isomerism
  10. explain valence bond theory.
  1. write the limitations of valence bond theory.
  2. write the factors affecting crystal field splitting parameter.
  3. write the applications of coordination compounds.

HALOGEN

  1. how will you prepare – a) ethyl chloride using thionyl chloride b) methyl iodide using finkelstein reaction
  2. write a short note on swarts reaction.
  3. define – a) plane polarized light b) optical activity
  4. convert – a) methyl bromide to methyl acetate b) ethyl chloride to ethyl isocyanide
  5. prepare – ethanenitrile using alkyl halide.
  6. explain – a) sn2 mechanism b) sn1 mechanism
  7. distinguish between sn1 and sn2 mechanism.
  8. prepare – ethene from ethyl bromide.
  9. write a short note on wurtz reaction.
  10. prepare – biphenyl from chlorobenzene.
  11. write a short note on wurtz–fittig reaction.
  12. what is the action of acetyl chloride on chlorobenzene?
  13. write the uses and environmental effects of – a) chloroform b) ddt.**

ALCOHOL

  1. convert – a) alkene to propan-1-ol b) methanal to ethanol c) acetic acid to ethanol d) isopropyl alcohol to tert-butyl alcohol
  2. what is the action of – a) lucas reagent on isopropyl alcohol b) acetic acid on methyl alcohol
  3. prepare – ethanoic acid to ethyl acetate.
  4. prepare – ethanal from ethanol.
  5. obtain – aspirin using salicylic acid.
  6. how will you prepare – i) carbolic acid from cumene ii) phenol from aniline
  7. how will you prepare – a) phenol from chlorobenzene b) phenol from benzene sulphonic acid
  8. what is the action of – a) bromine water on phenol b) nitrating mixture on anisole
  9. prepare – carbolic acid to picric acid.
  10. write a short note on – i) riemer–tiemann reaction ii) kolbe’s reaction
  11. what will happen when chromic anhydride reacts with phenol?

AMINES

  1. write a short note on ammonolysis.
  2. explain mendius reaction.
  3. how will you prepare ethyl amine using gabriel phthalimide?
  4. prepare – aniline using hoffmann bromamide degradation.
  5. explain – a) hoffmann exhaustive alkylation b) hoffmann elimination reaction
  6. prepare – a) n-methyl ethanamide using acylation of amine b) n,n-dimethyl acetamide using acylation of amine
  7. what is the action of nitrous acid on aniline?
  8. what is the action of amine on alcoholic koh and chcl₃?
  9. prepare – a) bromobenzene using sandmeyer’s reaction b) chlorobenzene using gattermann reaction
  10. prepare benzene using ethanol.
  11. explain the distinction between 1°, 2° and 3° amines by hinsberg’s reagent.
  12. prepare – a) p-bromoaniline using acetic anhydride b) p-nitroaniline using acetyl chloride
  13. explain zwitter ion.

BIOMOLECULES

  1. explain the classification of carbohydrates.
  2. how is glucose prepared?
  3. what is the action of – a) hydroiodic acid on glucose b) acetic anhydride on glucose c) dilute nitric acid on glucose
  4. write the reaction which confirms the presence of – a) carbonyl group b) aldehyde group
  5. explain the structure of – a) sucrose b) maltose c) lactose
  6. write the distinction between amylose and amylopectin.
  7. explain the classification of proteins on the basis of molecular shape.
  8. what is denaturation of protein?
  9. explain the mechanism of enzyme catalysis with the help of diagram.
  10. define – a) nucleoside b) nucleotide
  11. write the bases present in – a) purine b) pyrimidine.

POLYMER

  1. explain condensation polymers with example.
  2. distinguish between thermoplastic and thermosetting polymer.
  3. define – a) homopolymer b) copolymer
  4. explain vulcanization of rubber.
  5. write the uses of – a) ldp b) hdp c) teflon d) nylon-6, e) neoprene f) buna-s
  6. name the following – a) catalyst used in hdp b) monomer of teflon c) monomer of orlon d) catalyst used in terylene
  7. prepare – a) nylon-6,6 b) nylon- c) terylene d) buna-s e) phbv**

NANOCHEMISTRY

  1. define – a) green chemistry b) sustainable development
  2. write the names of 12 principles applied in green chemistry.
  3. explain the atom economy with an example.
  4. name the compound used in place of ddt.
  5. write the uses of pete, pp and ps.
  6. define – a) nanoscience b) nanotechnology
  7. what is nanomaterial? explain the types of nanomaterial.
  8. name the nanoparticles used as an effective bacterial disinfectant for water.
  9. write the information obtained by the following techniques – a) uv visible spectroscopy b) x-ray diffraction c) scanning electron microscopy d) ftir (fourier transform infrared spectroscopy)
  10. name the nanostructured material used to increase the life of a car tyre.
  11. write the advantages and disadvantages of nanoparticles and nanotechnology.