Nitrogen has lower electron affinity than its preceding element carbon because
- AElectron affinity decreases along a period
- BElectron affinity generally increases along a period
- CNitrogen atom has half-filled $p$-orbital
- DNitrogen is a $p$-block element
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The second electron gain enthalpies (in $kJ \ mol^{-1}$) of oxygen and sulphur respectively are
Difficult
View SolutionWhich element has maximum electron affinity?
Easy
View SolutionIn which of the following is the electron gain enthalpy of elements correctly arranged?
The formation of the oxide ion $O_{(g)}^{2-}$ requires first an exothermic and then an endothermic step as shown below. This is because
$O_{(g)} + e^{-} \rightarrow O_{(g)}^{-}; \Delta H^{o} = -142 \ kJ \ mol^{-1}$
$O_{(g)}^{-} + e^{-} \rightarrow O_{(g)}^{2-}; \Delta H^{o} = 844 \ kJ \ mol^{-1}$
$O_{(g)} + e^{-} \rightarrow O_{(g)}^{-}; \Delta H^{o} = -142 \ kJ \ mol^{-1}$
$O_{(g)}^{-} + e^{-} \rightarrow O_{(g)}^{2-}; \Delta H^{o} = 844 \ kJ \ mol^{-1}$
MediumAIEEE 2004
View SolutionWhat is electron gain enthalpy?
Easy
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