The formation of the oxide ion O_{(g)}^{2-} r | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(A) The formation of $O_{(g)}^{2-}$ involves the addition of an electron to a negatively charged $O_{(g)}^{-}$ ion.Since both the incoming electron an

Vedclass · Accepted Answer

$O^{-}$ ion will tend to resist the addition of another electron

Vedclass · Answer

(A) The formation of $O_{(g)}^{2-}$ involves the addition of an electron to a negatively charged $O_{(g)}^{-}$ ion.Since both the incoming electron and the $O_{(g)}^{-}$ ion are negatively charged,there is a strong electrostatic repulsion between them.To overcome this repulsion and force the electron into the $O_{(g)}^{-}$ ion,energy must be supplied to the system,making the process endothermic.Therefore,the $O^{-}$ ion resists the addition of another electron.

The formation of the oxide ion $O_{(g)}^{2-}$ requires first an exothermic and then an endothermic step as shown below. This is because
$O_{(g)} + e^{-} \rightarrow O_{(g)}^{-}; \Delta H^{o} = -142 \ kJ \ mol^{-1}$
$O_{(g)}^{-} + e^{-} \rightarrow O_{(g)}^{2-}; \Delta H^{o} = 844 \ kJ \ mol^{-1}$

Similar Questions

Arrange $S$,$O$,and $Se$ in ascending order of electron affinity.

For the reaction $Cl_{(g)} + e^- \to Cl^-_{(g)}$,the value of $\Delta H$ is ...........

Which of the following species has the highest electron affinity?

In which of the following processes is the highest energy absorbed?

In which of the following processes is energy liberated?

Vedclass Test Series

Exam Paper Generator

Online Exam Module

The formation of the oxide ion $O_{(g)}^{2-}$ requires first an exothermic and then an endothermic step as shown below. This is because$O_{(g)} + e^{-} \rightarrow O_{(g)}^{-}; \Delta H^{o} = -142 \ kJ \ mol^{-1}$$O_{(g)}^{-} + e^{-} \rightarrow O_{(g)}^{2-}; \Delta H^{o} = 844 \ kJ \ mol^{-1}$