Knowing
the electron gain enthalpy values for O → O−
and O → O2−
as −141
and
702 kJ mol−1
respectively, how can you account for the formation of a
large
number of oxides having O2−
species and not O−?
(Hint:
Consider lattice energy factor in the formation of compounds).
Knowing the electron gain enthalpy values for O → O− and O → O2− as −141
and 702 kJ mol−1 respectively, how can you account for the formation of a
large number of oxides having O2− species and not O−?
(Hint: Consider lattice energy factor in the formation of compounds).
Stability
of an ionic compound depends on its lattice energy. More the lattice
energy of a compound, more stable it will be.
Lattice
energy is directly proportional to the charge carried by an ion. When
a metal combines with oxygen, the lattice energy of the oxide
involving O2−
ion is much more than the oxide involving O−
ion. Hence, the oxide having O2−
ions are more stable than oxides having O−.
Hence, we can say that formation of O2−
is energetically more favourable than formation of O−.
Stability of an ionic compound depends on its lattice energy. More the lattice energy of a compound, more stable it will be.
Lattice energy is directly proportional to the charge carried by an ion. When a metal combines with oxygen, the lattice energy of the oxide involving O2− ion is much more than the oxide involving O− ion. Hence, the oxide having O2− ions are more stable than oxides having O−. Hence, we can say that formation of O2− is energetically more favourable than formation of O−.
