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question_answer1) A molecule of \[{{H}_{2}}\] exists while that of the\[H{{e}_{2}}\] does not. Explain.
question_answer2) \[NaCl\] gives a white precipitate with\[AgN{{O}_{3}}\] solution but \[CC{{l}_{4}}\] does not. Why?
question_answer3) \[Be{{F}_{2}}\] and \[{{H}_{2}}O\] are both tri-atomic molecules but have different shapes. Discuss.
question_answer4) Bond angle in \[N{{H}_{3}}\] is more than in \[P{{H}_{3}}\]. Explain.
question_answer5) Why is\[HCl\]predominantly covalent in the gaseous state but is ionic in aqueous solution?
question_answer6) Can a non-polar molecule have polar covalent bonds?
question_answer7) Sigma bond is stronger than the pi bond. Explain.
question_answer8) A molecule of\[PC{{l}_{5}}\] exists while that of\[NC{{l}_{5}}\] does not.
question_answer9) o-nitrophenol is steam volatile while p-nitrophenol is not. Discuss.
question_answer10) \[KH{{F}_{2}}\] exists while \[KHC{{l}_{2}}\] does not. Explain.
question_answer11) You are given the electronic configuration of five neutral atoms - A, B, C, D and E. \[A-1{{s}^{2}}\,2{{s}^{2}}\,2{{p}^{6}}\,3{{s}^{2}};\]\[B-1{{s}^{2}}2{{s}^{2}}\,2{{p}^{2}}\,3{{s}^{1}};\]\[C-1{{s}^{2}}2{{s}^{2}}2{{p}^{1}};\]\[D-1{{s}^{2}}\,2{{s}^{2}}\,2{{p}^{5}};\]\[E-1{{s}^{2}}\,2{{s}^{2}}\,2{{p}^{6}}\]. Write the empirical formula for the substances containing (i) A and D (ii) B and D (iii) only D (iv) only E.
question_answer12) Boiling point of ethane is more than that of methane. Assign reason.
question_answer13) Which compound from each of the following pairs is more covalent and why? (a) CuO or CuS (b) \[AgCl\] or \[AgI\] (c) \[PbC{{l}_{2}}\] or \[PbC{{l}_{4}}\] (d) \[BeC{{l}_{2}}\] or \[MgC{{l}_{2}}\]
question_answer14) The bond angles in \[NH_{4}^{+}\] and \[C{{H}_{4}}\] are same but \[N{{H}_{3}}\] has different bond angle. Why?
question_answer15) Predict which out of the following species are planar. (i)\[NH_{4}^{+}\] (ii)\[CH_{3}^{+}\] (iii)\[S{{F}_{4}}\] (iv)\[O{{F}_{2}}\] (v)\[{{H}_{2}}O\]
question_answer16) Why is \[MgC{{l}_{2}}\] molecule linear whereas the molecule of \[SnC{{l}_{2}}\] chloride has angular shape?
question_answer17) The hybridisation of oxygen in both water and diethyl ether molecules is the same but they differ in their bond angles. Explain.
question_answer18) Both Na and H occur in group 1 of the periodic table ; yet melting point of\[NaCl\] is \[800{}^\circ C\] while that of\[HCl\] is\[-114{}^\circ C\]. Why?
question_answer19) Write the Lewis dot symbols and predict the valencies you expect for the following elements: Nitrogen, Fluorine and Neon
question_answer20) Out of \[NaCl\] and \[MgO\], which has higher lattice energy and why?
question_answer21) Out of \[MgO,\] and \[CaO,\] which one is more hard and why?
question_answer22) Why an ionic bond is formed between two elements having large difference in their electro negativity?
question_answer23) Is \[Ca{{F}_{2}}\] linear or bent or neither of the two? Justify.
question_answer24) Why \[NaCl\] gives a white precipitate with \[AgN{{O}_{3}}\] solution but \[CC{{l}_{4}}\] does not?
question_answer25) Define lattice enthalpy. How is it related to the stability of an ionic compound?
question_answer26) Why is solubility of \[MgC{{l}_{2}}\] much greater than that of \[Mg{{F}_{2}}\]?
question_answer27) Draw the Lewis structures of the following molecules and ions and tell in which case/cases the octet rule is violated \[C{{O}_{2}},\,S{{O}_{2}},\,BeC{{l}_{2}},\,N{{H}_{3}},\,AlC{{l}_{3}},\,PC{{l}_{5}},\,CO_{3}^{2-}\]
question_answer28) On the basis of VSEPR theory, predict the shapes of the following molecules/ions? (i) \[Si{{F}_{4}}\] (ii) \[NH_{2}^{-}\] (iii) \[NH_{4}^{+}\] (iv) \[{{C}_{2}}{{H}_{2}}\] (v) \[{{H}_{3}}{{O}^{+}}\] (vi) \[{{F}_{2}}O\] (vii) \[PC{{l}_{3}}\] (viii) \[P{{F}_{5}}\].
question_answer29) Arrange the following in order of decreasing bond angle, giving reason : \[N{{O}_{2}},\,NO_{2}^{+},\,NO_{2}^{-}\]
question_answer30) Explain how the valence bond theory accounts for (i) a carbon-carbon double bond (C = C) (ii) a carbon-carbon triple bond \[(C\equiv C)\]
question_answer31) Explain how VB theory differs from Lewis concept.
question_answer32) Out of \[\sigma \] and \[\pi \]-bonds, which one is stronger and why?
question_answer33) What is the total number of sigma and pi bonds in the following molecules? (a)\[{{C}_{2}}{{H}_{3}}Cl\] (b)\[C{{H}_{2}}C{{l}_{2}}\] (c)\[{{H}_{3}}C-\overset{\begin{smallmatrix} H \\ | \end{smallmatrix}}{\mathop{C}}\,=\overset{\begin{smallmatrix} H \\ | \end{smallmatrix}}{\mathop{C}}\,-C\equiv C-H\]
question_answer34) What order of \[C-H\] bond lengths do you expect in \[{{C}_{2}}{{H}_{6}},\,{{C}_{2}}{{H}_{4}}\] and \[{{C}_{2}}{{H}_{2}}\] and why?
question_answer35) Which bond do you expect to be stronger in each of the following cases and why? (i) \[H-H,\,Cl-Cl\] (ii) \[{{O}_{2}},\,{{N}_{2}}\] (iii) \[F-F,\,Cl-Cl\]
question_answer36) Arrange the following single bonds in order of bond energy giving reasons: C - C, N - N, O - O, F - F
question_answer37) Explain why dipole moment of hydrogen halides decreases from HF to HI.
question_answer38) Represent diagrammatically the bond moments and the resultant dipole moments in (i) \[S{{O}_{2}}\] (ii) \[cis\] and trans forms of \[{{C}_{2}}{{H}_{2}}C{{l}_{2}}\]
question_answer39) Predict which out of the following molecules will have higher dipole moment and why? \[C{{S}_{2}}\] and \[OCS\]
question_answer40) Indicate whether the following statement is TRUE or FALSE. Justify your answer in not more than three lines: The dipole moment of \[C{{H}_{3}}F\] is greater than that of \[C{{H}_{3}}Cl\]
question_answer41) Which is more polar \[-C{{O}_{2}}\] or \[{{N}_{2}}O\]? Give reason.
question_answer42) Why reaction between \[NaCl\] and \[AgN{{O}_{3}}\] is very fast but reaction between \[{{H}_{2}}\] and \[C{{l}_{2}}\] is slow?
question_answer43) Why \[Al{{F}_{3}}\] is a high melting solid whereas \[Si{{F}_{4}}\] is a gas?
question_answer44) Draw the shapes of the following hybrid orbitals ; \[sp,\,s{{p}^{2}}\] and \[s{{p}^{3}}\]
question_answer45) Name the type of hybridisation of each C-atom in a molecule of (i) propylene (propene) (ii) propyne. How many \[\sigma \] and \[\pi \]-bonds are present in each case?
question_answer46) Why \[N{{F}_{3}}\] is pyramidal but \[B{{F}_{3}}\] is triangular planar?
question_answer47) Out of p-orbital and sp-hybrid orbital which has greater directional character and why?
question_answer48) What angles are associated with the following orbitals? \[sp,\,s{{p}^{2}}\] and \[s{{p}^{3}}\]
question_answer49) Which d-orbital is involved in \[s{{p}^{3}}d\] hybridisation and why?
question_answer50) Which d-orbital is involved in \[ds{{p}^{2}}\] hybridisation and why?
question_answer51) In the following molecule: \[C{{H}_{3}}-C\equiv \overset{1}{\mathop{C}}\,-\overset{2}{\mathop{C}}\,{{H}_{2}}-\overset{\begin{smallmatrix} O \\ 3|| \end{smallmatrix}}{\mathop{C}}\,-OH\] arrange the carbon atoms numbered\[C-1,\,C-2\] and\[C-3\] in the decreasing order of s-character.
question_answer52) What is the hybrid state of \[BeC{{l}_{2}}\]? What will be the change in the hybrid state of\[BeC{{l}_{2}}\] in the solid state?
question_answer53) Arrange the following in order of decreasing bond angles (i)\[C{{H}_{4}},\,N{{H}_{3}},\,{{H}_{2}}O,\,B{{F}_{3}},\,{{C}_{2}}{{H}_{2}}\] (ii) \[N{{H}_{3}},\,NH_{2}^{-},\,NH_{4}^{+}\]
question_answer54) Write the structure of an anion which is isostructural with \[B{{F}_{3}}\] and the structure of a cation which is isostructural with \[C{{H}_{4}}\]
question_answer55) In \[S{{F}_{4}}\] molecule, the lone pair of electrons occupies an equatorial position rather than axial position in the overall trigonal bipyramidal arrangement. Why?
question_answer56) Why axial bonds of \[PC{{l}_{5}}\] are longer than equatorial bonds?
question_answer57) Why bond angle in \[{{H}_{2}}O\] is nearly \[104\cdot 5{{{}^\circ }^{{}}}\] but that in \[{{H}_{2}}S,\] it is nearly 90°?
question_answer58) Which of the following species have same shape/same bond order? \[N_{3}^{-},\,NO_{2}^{-},\,C{{O}_{2}},\,{{O}_{3}}\]
question_answer59) Write two resonating structures of \[{{N}_{2}}O\] that satisfy the octet rule.
question_answer60) Taking Z-axis as the inter nuclear axis, explain why \[2{{p}_{x}}\] or \[2{{p}_{y}}\] orbital does not combine with 2s orbital to form molecular orbitals?
question_answer61) Explain why\[{{N}_{2}}\] has greater bond dissociation energy than \[N_{2}^{+}\] whereas \[O_{2}^{+}\] has greater bond dissociation energy than \[{{O}_{2}}\].
question_answer62) Can we have a diatomic molecule with its ground state molecular orbitals full with electrons? Give a reason for your answer.
question_answer63) Out of H and \[{{H}_{2}},\] the latter has higher first ionization energy while out of \[O\] and \[{{O}_{2}},\] the former has higher first ionization energy. Explain why.
question_answer64) Give reason for the following: \[H_{2}^{+}\] and \[H_{2}^{-}\] ions have the same bond order but \[H_{2}^{+}\] ions are more stable than \[H_{2}^{-}\].
question_answer65) Compare the relative stabilities of \[O_{2}^{-}\] and \[N_{2}^{+}\] and comment on their magnetic (paramagnetic or diamagnetic) behaviour.
question_answer66) (a) How bond energy varies from \[N_{2}^{-}\] to \[N_{2}^{+}\] and why? (b) On the basis of molecular orbital theory what is similarity between (i) \[{{F}_{2}},\,O_{2}^{--}\] (ii) \[CO,\,{{N}_{2}},\,N{{O}^{+}}\]?
question_answer67) \[{{N}_{2}}\] has higher bond order than NO. Explain.
question_answer68) Why \[KH{{F}_{2}}\] exists but \[KHC{{l}_{2}}\] does not?
question_answer69) When we move from \[HF\] to \[HCl,\] the boiling point drops sharply but on moving further to \[HBr\] and \[HI\] the boiling point increases. Why? or Out of \[HF\],\[HCl,\]\[HBr\] and \[HI\], which has lowest boiling point and why?
question_answer70) Ethanol has higher boiling point than diethyl ether or ethyl amine. Why?
question_answer71) Why water has maximum density at 277 K?
question_answer72) How many H-bonds are formed by each \[{{H}_{2}}O\] molecule and how many water molecules are attached to each water molecule and in what direction?
question_answer73) Out of o-nitro phenol and p-nitro phenol, which has higher boiling point and why?
question_answer74) Though Cl has nearly same electro negativity as N, yet there is no H-bonding in HCl. Why?
question_answer75) Why glucose, fructose, sucrose etc. are soluble in water though they are covalent compounds?
question_answer76) Explain why HF is less viscous than \[{{H}_{2}}O\].
question_answer77) From each of the following pairs, select the molecule with higher value of the property mentioned against each pair: (i)\[N{{H}_{3}},\,P{{H}_{3}}\]: bond angle (ii) \[N{{F}_{3}},\,N{{H}_{3}}\]: dipole moment (iii) \[MgO,\,CaO\]: hardness (iv) \[HCl,\,HBr\]: ionic character
question_answer78) Account for the following: The experimentally determined \[N-F\] bond length in \[N{{F}_{3}}\] is greater than the sum of the single covalent radii of N and F.
question_answer79) Why \[NaCl\] is a bad conductor of electricity in the solid state?
question_answer80) Why two hydrogen atoms combine to form \[{{H}_{2}}\] but two helium atoms do not combine to form \[H{{e}_{2}}\]?
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