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Answer :
Final answer:
Nitrogen's positive electron affinity is due to the stability of its five valence electrons and the electron configuration it achieves without the addition of extra electrons. Generally, elements gain electrons to reach a stable electronic configuration, but for nitrogen, its half-filled p orbitals in the valence shell are already stable, negating the need to add extra electrons for stability.
Explanation:
Nitrogen has a positive electron affinity because it already has five valence electrons in its outer shell, which results in a stable electron configuration that does not release energy when an additional electron is added. This unique situation arises from nitrogen's position in the periodic table (group 15), which normally would suggest it forms anions. However, in the case of nitrogen, the addition of an electron to form an anion such as N³⁻ is not energetically favorable due to repulsion between the electrons and the stability of the half-filled p orbital. Therefore, nitrogen's electron affinity is approximately zero, highlighting that no significant energy change occurs on gaining an electron.
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