Nature of Oxides
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- True
- False
The formation of the oxide ion, O2−(g) from oxygen atom requires first an exothermic and then an endothermic step as shown below:
O(g)+e−→O−(g);ΔfH∘=−141 kJ mol−1O−(g)+e−→O2−(g);ΔfH∘=+780 kJ mol−1
Thus, process of formation of O2− in gas phase is unfavourable even though O2− is isoelectronic with neon. It is due to the fact that,
O− ion has comparatively smaller size than oxygen atom.
oxygen is more electronegative
addition of electron in oxygen results in larger size of the ion.
electron repulsion outweighs the stability gained by achieving noble gas configuration.
The formation of the oxide ion, O2−(g) from oxygen atom requires first an exothermic and then an endothermic step as shown below:
O(g)+e−→O−(g);ΔfH∘=−141 kJ mol−1O−(g)+e−→O2−(g);ΔfH∘=+780 kJ mol−1
Thus, process of formation of O2− in gas phase is unfavourable even though O2− is isoelectronic with neon. It is due to the fact that,
O− ion has comparatively smaller size than oxygen atom.
oxygen is more electronegative
addition of electron in oxygen results in larger size of the ion.
electron repulsion outweighs the stability gained by achieving noble gas configuration.
- Chemical formula of anion is O−2
- They are also called hyperoxide
- Both (A) and (B)
- None of these