Electron affinity is defined as the energy released when an electron is added to a neutral atom to form a negative ion.


The electron affinity order for Ne, Be, and N is as follows:

1. Ne (Neon): Neon has the highest electron affinity among the three elements. This is because neon has a completely filled valence shell, and adding an electron to it would result in a stable noble gas configuration. The energy released when an electron is added to neon is the highest among the three elements.

2. N (Nitrogen): Nitrogen has a higher electron affinity than beryllium because it has a partially filled valence shell. When an electron is added to nitrogen, it completes its valence shell and forms a stable ion. The energy released during this process is less than that of neon but higher than that of beryllium.

3. Be (Beryllium): Beryllium has the lowest electron affinity among the three elements. This is because beryllium has a completely filled 2s subshell and adding an electron to it would result in an unstable configuration. The energy released in this process is the lowest among the three elements.


The electron affinity of an element depends on its electronic configuration. An element with a completely filled or half-filled valence shell has a higher electron affinity than an element with a partially filled valence shell. This is because adding an electron to an element with a completely filled or half-filled valence shell results in a stable configuration, whereas adding an electron to an element with a partially filled valence shell results in an unstable configuration. The energy released during this process is the highest for elements with a completely filled valence shell and the lowest for elements with a partially filled valence shell.