Read the passage given below and answer the question that follow :
The distribution of electrons among various molecular orbitals is called the electronic configuration of the molecule which provides us the following very important information about the molecule.
(I)Stability of molecule : The molecule is stable if number of bonding molecular orbital electrons (N_b ) is greater than the number of anti bonding molecular orbital electrons(N_a).
(II)Bond order = 12 ( N_b – N_a )A positive bond order means a stable molecule while a negative or zero bond order means an unstable molecule.
(III)Nature of the bond : Bond order 1, 2 and 3 corresponds to single, double and triple bonds respectively.
(IV)Bond length : Bond length decreases as bond order increases.
(V)Magnetic nature : If molecular orbitals in a molecule are doubly occupied, the substance is diamagnetic and if one or more molecular orbitals are singly occupied, it is paramagnetic.

Solution

In which of the following pairs the two species are not isostructural ?

\(CO_{3}^{2-}\)and\(NO_{3}^{-}\)
\(PCl_{4}^{+}\) and \(SiCl_{4}^{+}\)
PF₅ and BrF₅
\(AlF_{6}^{3-}\) and SF6

Solution

The number of types of bonds between two carbon atoms in calcium carbide is

One sigma, One pi
Two sigma, one pi
Two sigma, two pi
One sigma, two pi

Solution

The bond dissociation energy of B – F in BF₃ is 646 kJ mol–1 where as that of C – F in CF₄ is 515 kJ mol–1. The correct reason for higher B – F bond dissociation energy as compared to that of C – F is

stronger ? bond between B and F in BF₃ as compared to that between C and F in CF₄.
significant p? – p? interaction between B and F in BF₃ whereas there is no possibility of such interaction between C and F in CF₄.
lower degree of p? – p? interaction between B and F in BF₃ than that between C and F in CF₄.
smaller size of B– atom as compared to that of C– atom.

Solution

Which of the following hydrogen bonds is the strongest?

O– H - - - F
O– H - - - H
F– H- -- F
O – H - - -O

Solution

Greater the difference between electro-negativity of bonded atoms, stronger will be the bond. Since F is most electronegative hence F – H ...... F is the strongest bond.

Bond order of 1.5 is shown by :

\(O_{2}^{+}\)
\(O_{2}^{+-}\)
\(O_{2}^{2-}\)
O₂

Solution

Solution

\(BF_{4}^{-}\) hybridisation sp³, tetrahedral structure.
\(NH_{4}^{+}\) hybridisation sp³, tetrahedral structure.

Solution

Which of the following has the minimum bond length ?

\(O_{2}^{+}\)
\(O_{2}^{-}\)
\(O_{2}^{2-}\)
O₂

Solution

Which of the two ions from the list given below have the geometry that is explained by the same hybridization of orbitals, \(NO_{2}^{-}\), \(NO_{3}^{-}\), \(NH_{2}^{-}\), \(NH_{4}^{+}\), SCN^– ?

\(NO_{2}^{-}\) and \(NO_{3}^{-}\)
\(NH_{2}^{-}\) and \(NO_{3}^{-}\)
SCN^- and \(NH_{2}^{-}\)
\(NO_{2}^{-}\) and \(NH_{2}^{-}\)

Solution

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