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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Similar Questions
When a chloride ion is formed from an isolated gaseous chlorine atom,$3.8 \ eV$ of energy is released. This value is equal to the:
Medium
View SolutionThe amount of energy released due to the addition of an extra electron to the outermost orbit of a gaseous atom is called:
Easy
View SolutionExplain the periodicity of electron gain enthalpy of elements in the periodic table.
The process that is $NOT$ endothermic in nature is :-
The formation of the oxide ion $O^{2-}_{(g)}$ requires first an exothermic and then an endothermic step as shown below:
$O_{(g)} + e^{-} \to O^{-}_{(g)}; \Delta H = -142 \, kJ \, mol^{-1}$
$O^{-}_{(g)} + e^{-} \to O^{2-}_{(g)}; \Delta H = 844 \, kJ \, mol^{-1}$
This is because:
$O_{(g)} + e^{-} \to O^{-}_{(g)}; \Delta H = -142 \, kJ \, mol^{-1}$
$O^{-}_{(g)} + e^{-} \to O^{2-}_{(g)}; \Delta H = 844 \, kJ \, mol^{-1}$
This is because:
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