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Unformatted text preview: Electron affinity decreases or increases across a period depending on electronic configuration. This occurs because of the same subshell rule that governs ionization energies. Example: Since a half-filled "p" subshell is more stable, carbon has a greater affinity for an electron than nitrogen. Obviously, the halogens, which are one electron away from a noble gas electron configuration, have high affinities for electrons: (More negative energy = greater affinity) Element Electron Affinity I-295.2 kJ/mole Br-324.5 kJ/mole Cl-348.7 kJ/mole F *-327.8 kJ/mole * Fluorine's electron affinity is smaller than chlorine's because of the higher electron - electron repulsions in the smaller 2p orbital compared to the larger 3p orbital of chlorine....
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