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The Formation of the oxide ion, O²⁻ from oxygen atom requires first an exothermic and then an endothermic step as shown below:
O(g) + e⁻ → O⁻(g) ; Δf H° = -141 kJ mol⁻¹
O⁻(g) + e⁻ → O²⁻(g) ; Δf H° = +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,
Options
(a) O⁻ ion has comparatively smaller size than oxygen atom
(b) oxygen is more electronegative
(c) addition of electron in oxygen results in larger size of the ion
(d) electron repulsion outweighs the stability gained by achieving noble gas configuration
Correct Answer:
electron repulsion outweighs the stability gained by achieving noble gas configuration
Explanation:
No explanation available. Be the first to write the explanation for this question by commenting below.
Related Questions: - Rutherford’s experiment led to the discovery of
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Topics: P Block Elements in Group 15
(89)
Subject: Chemistry
(2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
- Rutherford’s experiment led to the discovery of
- The compressibility factor of an ideal gas is
- The fractional distillation is used in
- The heat of combustion of carbon to CO₂ is -393.5 kJ/mol. The heat released
- Which of the following is not true
Topics: P Block Elements in Group 15 (89)
Subject: Chemistry (2512)
Important MCQs Based on Medical Entrance Examinations To Improve Your NEET Score
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