Understanding the Myriad of Inorganic chemistry

Did you know: What is Bond order of CO+?  Well, it’s 3.5

F2 is best oxidising agent? Well, it’s wrong. Check p-273, Q8.16 NCERT XI Chemistry.

Perxenate ion, (XeO6)4– is Stronger oxidising agent than F2.


  1. Solid PCl5, solid PBr5, solid GaCl2, solid XeF6, solid N2O5, solid N2O4, solid N2O3 , solid Cl2O6, solid I2Cl6, are ionic solids. Identify the ions.
  2. KHCO3 has dimeric hydrogen bonding (HCO3)- Whereas NaHCO3 has linear polymeric hydrogen Bonding hence KHCO3 is more soluble.
  3. I4O9 is an ionic solid, I(IO3)3.
  4. (XeF5)- has pentagonal planar geometry.
  5. I2Cl6 has all atoms in same plane.
  6. (CrO8)3– has four peroxy linkages (i.e, eight peroxy oxygens) and Cr (+5).
  7. Two sulfur of H2S2O3 are in -2 & +6 oxidation state.
  8. PH3, H2S and hydride of higher elements of group 15 and 16 have almost “no hybridisation”..
  9. Hybridisation in (CH5)+ is sp2 but carbon is pentavalent.
  10. PF5 has all bonds almost equivalent but PCl5 has two types of bonds.
  11. CH2=C=CH2 is non-planar molecule, CH2=C=C=CH2 is planar.
  12. CH3-CH=S=O & H2N2O2 has geometrical isomerism.
  13. Solid BeCl2 is sp3 hybridised linear polymeric solid but BeCl2(g) is sp hybridised.
  14. SnCl2 > SnCl4 is correct melting point order.
  15. Bond angle order is NF3 < NH3 but PF3 >PH3.
  16. Bond angle order is Cl2O > H2O > F2O.
  17. C-F bond length order is CH3F < CH2F2 < CHF3 < CF4.
  18. Bond angle order is SO2 = SO3.
  19. O-O bond length order is H2O2 > F2O2.
  20. CaC2 and BaC2 give different products with N2?
  21. Ortho-cyanophenol has no chelation.
  22. NCl3 + H2O gives NH3 and HOCl whereas PCl3 + H2O gives H3PO3 and HCl.
  23. Dipole moment order is HF > H2O > NH3 but boiling point order is H2O > HF > NH3.
  24. HF has zig zag hydrogen Bonding where one HF molecule forms only two hydrogen Bonding.
  25. Boiling point order is H2O> H2Te > H2Se > H2S but BiH3 > SbH3 > NH3 > AsH3 > PH3.
  26. If H2O had no hydrogen Bonding, its boiling point would have been 173 K.
  27. B2, C2 are examples of species having no sigma but only “pi” bonds.
  28. Ionisation energy order is N2 > O2 = Xe > NO.
  29. Maleic acid has lesser pKa1 and greater pKa2 as compared to that of fumaric acid & for the same reason, ortho- nitrophenol is more acidic than para isomer.
  30. Bond angle of NO2 is 115 degree and of (NO2)- is 136 degree.
  31. CF3 free radical & Bridhgehead free radicals are pyramidal but other organic free radical are trigonal planar. ClO3, ClO2, NO2 free radical are of bent shape & pyramidal.
  32. C3O2 and C2N4 are linear.
  33. (CN2)2-, cyanamide ion is isoelectronic and isostructural with CO2, N3–, N2O, (NO2)+.
  34. “All C-C bonds in naphtalene are identical” is a false statement.
  35. CaCO3, BaSO4, CsI, LiF etc. are ionic but water insoluble/sparingly soluble, why?
  36. BeO, MgO, Al2O3 etc. have appreciable covalent character but these are high melting solids, why?
  37. AgBr, AgI etc. are diamagnetic but colored due to greater polarization. Explain.
  38. KMnO4, K2Cr2O7 are diamagnetic but colored due to LMCT. Explain.
  39. The same reductant, thiosulphate react differently with iodine and bromine.
  40. Pb3O4, red lead reacts differently with HCl and with HNO3.
  41. CuSO4(aq) reacts similarly with KI and KCN and produces Cuprous salts and  I2 or (CN)2. Further I2 is estimated by titrating with hypo solution. Starch is used as the indicator.
  42. When concentrated sulphuric acid is added to an inorganic mixture containing chloride, we get colourless pungent smelling gas HCl, but if the mixture contains bromide then we get red vapour of bromine.
  43. Cl2 + KBr gives KBr and Cl2 whereas KClO3 + Br2 gives KBrO3 and Cl2.
  44. Sulfur undergoes disproportionation in alkaline medium to form sulfide ion and thiosulfate ion.
  45. Fluorine reacts with alkali to form Fluoride ion and OF2, but it is not a disproportionation reaction.
  46. Among the four oxoanions of chlorine, only perchlorate ion does not disproportionate. etc…

To be Expanded…..

Module 1 -Chemical bonding, Periodic properties, s-block. 

  1. Exceptional electronic configurations
  2. Shielding effect and Effective nuclear charge
  3. Periodic properties and its exceptional behaviors
  4. Covalent character in ionic compounds (Fajan Rule)
  5. VSEPR theory
  6. Drago rule and Bent’s rule
  7. Back bonding, pπ-pπ and pπ-dπ bonds and its applications
  8. Exceptional orders in bond length, bond length, bond angle and dipole moment order and their reasoning
  9. Formal charge, resonance and bond order
  10. MOT
  11. Hydrogen bonding, chelation and its applications
  12. Important questions on factors affecting lattice energy, hydration energy, melting point, solubility of s-block compounds
  13. Important questions on factors affecting order of acidic and basic character
  14. Flame test, Solutions of alkali metals in liquid ammonia
  15. Anomalous behavior of first element of group, Diagonal relationships and examples etc.

Module 2

Redox reactions, Electrochemistry, p-block complete, Hydrogen- (Also recall free energy, entropy, spontaneity- helps in understanding ellingham diagram etc). Here learn about

  1. Structures of lot variety compounds-make a list whenever you find new one
  2. Oxidation state
  3. Oxidising agents, reducing agents – Comparison of behavior of Important ones
  4. Concept of n-factor and its use in balancing and where it fails and why
  5. Law of equivalents- applications and where it fails and why
  6. Electrode potential and factors affecting it
  7. Activity series and its wide applications to predict feasibilty of various reactions
  8. Nernst equation (helps you undertstand the effect of using dil vs conc and effect of temperature on feasibilty)
  9. Electrolysis and over potential (helps you to understand downs cell, nelson cell, castner kellner cell, mercury cell, electrolytic reduction and refining etc)
  10. Inert pair effect and its applications
  11. Inorganic reactions -there you can classify into three (not mutually exclusive) types- hydrolysis reactions, decomposition reactions,acid base reactions and other redox reactions, make a list of all reactions and then find similarities)
  12. Inorganic compound -common names
  13. Different processes – name and use (Deacon’s process, contact process,
  14. Structure of different oxyacids– Ortho, meta, hypo, pyro etc
  15. Effect of heat on different compounds
  16. Nature of oxides – Amphoteric oxides
  17. 3c-2e and 3c-4e bonds
  18. Silicates, Silicones, Zeolites
  19. Borax, Boric acid, Diborane
  20. Thermite reaction
  21. Ostwald process, Contact process, Deacon process etc
  22. Disproportionation reactions etc.

Module 3

Metallurgy, d,f-block, coordination compounds, Qualitative Salt analysis

  1. Size, Melting point, Electrode potentials trends in 3d series
  2. Charge transfer examples
  3. KMnO4 and K2Cr2O7- properties
  4. Lanthanoid contraction and its consequences
  5. Hybridisation and Stereoisomerism in coordination compounds
  6. Crystal field theory and its applications
  7. Synergic bonding in metal carbonyls etc.

Now you must have an idea of variety of most important problems of inorganic chemistry.

 

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