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question_answer1) Aluminium forms \[{{[Al{{F}_{6}}]}^{3-}}\] ion but boron does not form \[{{[B{{F}_{6}}]}^{3-}}\] ion. Explain.
question_answer2) Boron tribromide is a stronger acid than boron trifluoride. Assign reason.
question_answer3) \[p\pi -p\pi \] back bonding occurs in halides of boron and not in those of aluminium. Why?
question_answer4) Although first ionisation potential of boron \[(8.3\,\,eV)\] is less than that of gold\[(9.22\,\,eV)\] yet the former is a non-metal while the latter is a metal. Explain.
question_answer5) An aqueous solution of sodium hydroxide is added drop wise to solution of gallium chloride in water. A precipitate is initially formed which dissolves on further addition of NaOH solution. Write chemical equations.
question_answer6) Compounds of carbon are covalent while those of lead are generally ionic. Discuss.
question_answer7) Why is \[PbC{{l}_{2}}\] is more stable than\[PbC{{l}_{4}}\]?
question_answer8) Carbon and silicon are mainly tetravalent while germanium, tin and lead also show divalency. Explain.
question_answer9) Why is carbon dioxide a gas while silicon dioxide is a solid?
question_answer10) Trisilicylamine is a weaker base than trimethylamine. Explain.
question_answer11) Why is \[SiC{{l}_{4}}\] readily hydrolysed but \[CC{{l}_{4}}\] is resistant to hydrolysis?
question_answer12) Trisilicylamine is planar while trimethylamine is pyramidal. Explain.
question_answer13) Write the balanced equations for the following reactions. (i) SnO is treated with dilute \[HN{{O}_{3}}\] (ii) Tin is heated with excess of chlorine gas (iii) Lead sulphide is heated in air.
question_answer14) The +1 oxidation state is more stable than the + 3 oxidation state for thallium.
question_answer15) Assign reasons for each of the following : (i) + 1 gallium undergoes disproportionation reactions. (ii) Unlike \[\text{I}{{n}^{+}},\,\text{T}{{\text{l}}^{+}}\] is more stable with respect to disproportionation. (iii) \[\text{InCl}\] undergoes disproportionation but \[\text{TlCl}\] does not. (iv) In \[(III)\] is more stable than In \[(I)\] in aqueous solution.
question_answer16) Why does not boron form \[{{B}^{3+}}\] ions?
question_answer17) Why boron and aluminium tend to form covalent compounds?
question_answer18) Molten aluminium bromide is a poor conductor of electricity. Explain.
question_answer19) Why boron forms electron deficient compounds?
question_answer20) Why boron halides do not exist as dimers while \[AlC{{l}_{3}}\] exists as \[A{{l}_{2}}C{{l}_{6}}\]?
question_answer21) Aluminium chloride exists as a dimer. Give reasons.
question_answer22) Anhydrous aluminium chloride is used as a catalyst.
question_answer23) Why trihalides of Group 13 elements fume in the moist air?
question_answer24) \[BC{{l}_{3}}\] is trigonal planar while \[AlC{{l}_{3}}\] is tetrahedral in dimeric state. Explain.
question_answer25) Why \[BB{{r}_{3}}\] is a stronger Lewis acid as compared to \[B{{F}_{3}}\] though fluorine is more electronegative than bromine.
question_answer26) Why B-X bond distance in \[B{{X}_{3}}\] is shorter than theoretically expected value?
question_answer27) Properties of Be resemble with Al? Why?
question_answer28) Why boric acid acts as an acid through it does not give \[{{H}^{+}}\]ions?
question_answer29) C and Si are almost always tetravalent but Ge, Sn and Pb show divalency. Why? Or Why the tendency to exhibit + 2 oxidation state increases with increasing atomic number in group 14. Or +2 oxidation state of lead is more stable than +4 oxidation state. Give reasons.
question_answer30) Why carbon forms covalent compounds whereas lead forms ionic compounds?
question_answer31) Give one chemical reaction to show that: (i) Tin \[(II)\] is a reducing agent whereas Pb \[(II)\]is not. (ii) Tin \[(II)\] chloride is a reducing agent.
question_answer32) \[Pb{{O}_{2}}\] is a stronger oxidising agent than \[Sn{{O}_{2}}\]. Or \[Pb{{O}_{2}}\] can act as an oxidising agent.
question_answer33) Like CO why its analog of SiO is not stable.
question_answer34) Why \[N{{(C{{H}_{3}})}_{3}}\] is pyramidal but \[N{{(Si{{H}_{3}})}_{3}}\] is planar?
question_answer35) Why \[{{(Si{{H}_{3}})}_{3}}N\] is a weaker base than \[{{(C{{H}_{3}})}_{3}}N\]? or Why \[N{{(C{{H}_{3}})}_{3}}\] is more basic than \[N(SiM{{e}_{3}})\]?
question_answer36) Account for the following : (i) \[Pb{{X}_{2}}\] is more stable than \[Pb{{X}_{4}}\,(X=Cl,\,Br)\] (ii) \[PbC{{l}_{4}}\] is less stable than \[SnC{{l}_{4}}\] but\[PbC{{l}_{2}}\] is more stable than \[SnC{{l}_{2}}\]. (iii) \[PbC{{l}_{4}}\] is less stable than \[SnC{{l}_{4}}\]?
question_answer37) Why \[CC{{l}_{4}}\] is resistant to hydrolysis but \[SiC{{l}_{4}}\] is readily hydrolysed?
question_answer38) The tendency for catenation decreases down the group 14. Or Why carbon shows catenation but silicon does not Or In group 14, the tendency for catenation decreases with increasing atomic number.
question_answer39) Why does not silicon form an analogue of graphite? Or Why does elemental silicon not form graphite like structure as carbon does. Explain. Or No form of elemental silicon is comparable to graphite.
question_answer40) \[C{{O}_{2}}\] is a gas while \[Si{{O}_{2}}\] is a solid. Explain.
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