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question_answer1) A diatomic molecule has a dipole moment of 1.2 D, if the bond distance is 1\[\overset{o}{\mathop{A}}\,\], what percentage of electronic charge exists on each atom?
question_answer2) The dipole moments of a diatomic molecule AB is 0.41 D and bond distance is 2.82, calculate the % ionic character of AB.
question_answer3) The bond angle between two hybrid orbitals is \[105{}^\circ \]. Calculate the percentage of s-character of hybrid orbital.
question_answer4) In \[O_{2}^{-},{{O}_{2}}\] and \[O_{2}^{2-}\] molecular species. Find the total number of anti-bonding electrons.
question_answer5) There are two groups of compounds A and B. Group A contains three compounds \[P{{x}_{4}},Q{{y}_{3}},R{{z}_{2}},\] Group B also contains three compounds\[S{{x}_{4}},\,T{{y}_{3}},\,U{{z}_{2}}\]. Hybridization of each central atom of group A compounds is same as that of iodine in \[IBrC{{l}^{-}}\]while in group B compounds it is same as that of iodine in \[IBrC{{l}^{+}}\] Substituents X, Y and Z exhibit covalence of one in ground state. Then find the value of x/y. Where, x and y are total number of lone pairs present at central atoms of compounds of group A and B respectively.
question_answer6) Consider the following three compounds (i) \[AX_{2n}^{n-}\], (ii) \[A{{X}_{3n}}\] and (iii) \[AX_{4n}^{n+},\], where central atom A is 15th group element and their maximum covalency is 3n. If total number of proton in surrounding atom X is n and value of n is one, then calculate value of\[''{{x}^{3}}+{{y}^{2}}-z''\]. (Where x, y and z are total number of lone pair at central atom in compound (i), (ii) and (iii) respectively.
question_answer7) Calculate the value of "x+y-z" here x, y and z are total number of non-bonded electron pair(s), pie \[(\pi )\] bond (s) and sigma \[(\sigma )\] bonds in hydrogen phosphite ion respectively.
question_answer8) Consider the following compounds: (i) \[I{{F}_{5}}\] (ii) \[ClI_{4}^{-}\] (iii) \[Xe{{O}_{2}}{{F}_{2}}\] (iv) \[NH_{2}^{-}\] (v) \[BC{{l}_{3}}\] (vi) \[BeC{{l}_{2}}\] (vii) \[AsCl_{4}^{+}\] (viii) \[B{{(OH)}_{3}}\] (ix) \[NO_{2}^{-}\] (x) \[ClO_{2}^{+}\] The value of "x + y - z" is where x, y and z are total number of compounds in given compounds in which central atom used their all three p- orbitals, only two p-orbitals and only one p-orbital in hybridisation respectively.
question_answer9) Total number of species which used all three p-orbitals in hybridisation of central atoms and should be non-polar also are \[Xe{{O}_{2}}{{F}_{2}},SnC{{l}_{2}},I{{F}_{5}},I_{3}^{+},\,Xe{{O}_{4}},S{{O}_{2}},\,XeF_{7}^{+},Se{{F}_{4}}\]
question_answer10) Consider the following orbitals \[3s,2{{p}_{x}},4{{d}_{xy}},4d_{z}^{2},3{{d}_{{{x}^{2}}-{{y}^{2}}}},\,\,3{{p}_{y}},\,4s,\,4{{p}_{z}}\] and find total number of orbital(s) having even number of nodal plane.
question_answer11) For the following molecules: \[PC{{l}_{5}},Br{{F}_{3}},ICl_{2}^{-},XeF_{5}^{-},NO_{3}^{-},Xe{{O}_{2}}{{F}_{2}},\,PCl_{4}^{+},CH_{3}^{+}\] Calculate the value of \[\frac{a+b}{c}\] a = Number of species having \[s{{p}^{3}}\]d-hybridisation b = Number of species which are planar c = Number of species which are non-planar
question_answer12) Find total number of orbital which can overlap collaterally, (if inter nuclear axis is z) \[s,{{p}_{x}},{{p}_{y}},{{p}_{z}},{{d}_{xy}},{{d}_{yz}},{{d}_{xz}},{{d}_{{{z}^{2}}}},{{d}_{{{x}^{2}}-}}_{{{y}^{2}}}\]
question_answer13) The total number of lone-pairs of electrons in melamine is
question_answer14) Among the triatomic molecules/ions, \[BeC{{l}_{2}}\text{, }\] \[N_{3}^{-},\text{ }{{N}_{2}}O,\,NO_{2}^{+},{{O}_{3}},SC{{l}_{2}},ICl_{2}^{-},I_{3}^{-}\] and \[Xe{{F}_{2}},\] the total number of linear molecule(s)/ion(s) where the hybridization of the central atom does not have contribution from the d-orbital(s) is [Atomic number: S = 16, Cl = 17, I = 53 and Xe = 54]
question_answer15) The sum of the number of lone pairs of electrons on each central atom in the following species is \[{{[TeB{{r}_{6}}]}^{2-}},{{[Br{{F}_{2}}]}^{+}},SN{{F}_{3}}\] and \[{{[Xe{{F}_{3}}]}^{-}}\] (Atomic numbers: N=7, F=9, S=16, Br= 35, Te=52, Xe=54)
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