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Electron Affinity

Which of the ...

Question

Which of the following process involves absorption of energy?

A

C l (g) + e^{-} ⟶ {C l}^{-} (g)

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B

O^{-} (g) + e^{-} ⟶ O^{2 -} (g)

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C

O (g) + e^{-} ⟶ O^{-} (g)

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D

S (g) + e^{-} ⟶ S^{-} (g)

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Solution

The correct option is B $O^{-} (g) + e^{-} ⟶ O^{2 -} (g)$
Solution:-
The process ${O^{-}}_{(g)} + e^{-} ⟶ {O^{2 -}}_{(g)}$ involves absorption of energy.
When a neutral atom gains an electron, energy is released. When an anion (having unit negative charge) gains an electron, energy is absorbed. This is due to the repulsion between the additional electron and negatively charged anion.

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Similar questions

Q. Consider the following reactions :

O_{(g)} + e^{-} \to O_{(g)}^{-}, Δ H_{1}

F_{(g)} + e^{-} \to F_{(g)}^{-}, Δ H_{2}

C l_{(g)} + e^{-} \to C l_{(g)}^{-}, Δ H_{3}

O_{(g)}^{-} + e^{-} \to O_{(g)}^{2 -}, Δ H_{4}

The correct statement(s) is/are

O_{(g)} + e^{-} \to O_{(g)}^{-} Δ H_{1}

O_{(g)}^{-} + e^{-} \to O_{(g)}^{- 2} Δ H_{2}

O_{2 (g)} \to O_{2 (g)}^{+} + e^{-} Δ H_{3}

O_{(g)} \to O_{(g)}^{+} + e^{-} Δ H_{4}

H_{2 (g)} \to H_{2 (g)}^{+} + e^{-} Δ H_{5}

H_{(g)} \to H_{(g)}^{+} + e^{-} Δ H_{6}

O_{(g)} + 2 e^{-} \to O^{- 2} Δ H_{7}

Which of the following option(s) is/are correct?

Q. 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 k J / m o l

.

O^{-} (g) + e ⟶ O^{2 -} (g)

Δ H = 844 k J / m o l

.
This is because:

Q. 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 k J / m o l

O^{-} (g) + e^{-} ⟶ O^{2 -} (g)

Δ H = 844 k J / m o l

This is because:

Q. 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^{0} = - 142 k J m o l^{- 1}

O^{-} (g) + e^{-} = O^{2 -} (g), Δ H^{0} = + 844 k J m o l^{- 1}

This is because :

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