The electron affinities of Be . Mg and noble gases are almost zero because both (Z=4:1s22s2)andMg(Z=12,1s22s22p63s2) are having s orbital fully filled in their valence shell . Fully filled orbitals are most stable due to symmetry. Therefore , these elements would be having least tendency to accept electron . Hence. Be and Mg would be having zero electron affinity Whereas
N(Z=7,1s22s22px12py12pz1)andP(Z=15)1s22s22p63s23p3 is having half filled 2p - subshell . Half filled sub shells are most stable due to symmetry (Hund 's rule). Thus , nitrogen and phosphorous are having least tendency to accept electron Hence ,have low electron affinity.
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Explanation:
The electron affinities of Be . Mg and noble gases are almost zero because both (Z=4:1s22s2)andMg(Z=12,1s22s22p63s2) are having s orbital fully filled in their valence shell . Fully filled orbitals are most stable due to symmetry. Therefore , these elements would be having least tendency to accept electron . Hence. Be and Mg would be having zero electron affinity Whereas
N(Z=7,1s22s22px12py12pz1)andP(Z=15)1s22s22p63s23p3 is having half filled 2p - subshell . Half filled sub shells are most stable due to symmetry (Hund 's rule). Thus , nitrogen and phosphorous are having least tendency to accept electron Hence ,have low electron affinity.