Question

Arrange the following as stated: (i) N2, O2, F2, Cl2 (Increasing order of bond dissociation energy) (ii) F, Cl, Br, I (Increasing order of electron gain enthalpy) (iii) F2, N2, Cl2, O2 (Increasing order of bond length)

Find the molecule with the least bond angle

Arrange the following in the order of property indicated for each set: (i) O2, O2+, O2–, O22– (increasing stability) (ii) LiCl, NaCl, KCl, RbCl (decreasing covalent character) (iii) NO2, NO2+, NO2– (decreasing bond angle) (iv) H–F, H–Cl, H–Br, H–I (decreasing bond dissociation enthalpy)

Table shows the molecular orbital occupancy and molecular properties for B2, C2, N2, O2, F2. Observe this figure and answer the questions based on this diagram and related studied concepts. (a) Why is Ne2 not formed according to M.O. theory? (b) Arrange B2, C2, N2, O2, F2 in increasing order of bond length. (c) On the basis of fig and table given above, Why F2 diamagnetic whereas O2 paramagnetic? (d) Consider the table given above and answer, Why does bond enthalpy of N2 is higher than O2? (e) Why is F2 more reactive than O2?