Assign a possible reason for the following : (a) Stability of + 5 oxidation state decreased and that of + 3 oxidation

(b)The elements of group 14 have 4 valence electrons. Therefore, the oxidation state of the group is +4. However, as a result of the inert pair effect, the lower oxidation...

[Hint  :  Due to increase in size and decrease in electronegativity down the groups.]

[Hint : NH3 > PH3 > AsH3 > SbH3 > BiH3]

[Hint : Due to inert pair effect.]

The lanthanides that exhibit +2 and +4 states are shown in the given table. The atomic numbers of the elements are given in the parenthesis. +2 +4 Nd (60) Ce (58) Sm (62) Pr (59) Eu (63) Nd...

(i) As the atomic size of nitrogen is smaller than phosphorus, therefore electron density on nitrogen atom is higher than that on phosphorus atom. Consequently the tendency of N in...

(i) This is because transition metals have strong metallic bonds as they have a large number of unpaired electrons. (ii) The catalytic activity of transition metals is attributed to the following...

(i) It is due to (a) Intermolecular hydrogen bonding in HF. (b) Higher H—F bond dissociation enthalpy than H—Cl. (ii) As P—P single bond (213 kJ mol-1) in P4 is much weaker than...

(i) In aqueous solution Cu+ undergoes disproportionation to form a more stable Cu2+ ion. 2Cu+(aq) → 2Cu2+(aq) + Cu(s) The higher stability of Cu2+ in aqueous solution may be attributed to its greater negative...

(i) This is because fluorine is most electronegative element and does not have d-orbitals in its valence shell.  (ii) Due to vary high ionisation enthalpy helium does not form any real...