The formation of the oxide ion O 2 − ( g ) requires first an exothermic and then an endothermic step as shown below O ( g ) + e − O − ( g ) Δ H ∘ = − 142 kJmol − 1 O − ( g ) + e − O 2 − ( g ) Δ H ∘ =

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The formation of the oxide ion O 2 − ( g ) requires first an exothermic and then an endothermic step as shown below O ( g ) + e − O − ( g ) Δ H ∘ = − 142 kJmol − 1 O − ( g ) + e − O 2 − ( g ) Δ H ∘ = 844 kJmol − 1

TestHub · Accepted Answer

O − 1 ( g ) + e ⟶ O − 2 ( g ) Due to the electronic repulsion, amount of the energy is needed to add electron

Chemistry - PERIODIC TABLE Question with Solution | TestHub

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