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How the +2 oxidation state of nitrogen is stable.derive briefly
Accepted Answer
Nitrogen's +2 oxidation state is relatively unstable. Here's why:
1. Electron Configuration: Nitrogen has 5 valence electrons. Achieving a +2 oxidation state means losing two electrons, leaving it with a 2p3 configuration. This configuration is not particularly stable due to having three unpaired electrons, making it highly reactive.
2. Ionic Radius: Nitrogen's small size and high electronegativity make it difficult to form stable +2 ions. The loss of two electrons would result in a very small and highly charged cation, making it susceptible to strong electrostatic attractions and potentially unstable.
3. Common Oxidation States: Nitrogen's most common oxidation states are -3, +3, +4, and +5. The +2 oxidation state is less frequently encountered, as it is more likely to either gain or lose more electrons to achieve a more stable configuration.
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