The electron affinity values of elements A, B, C and D are respectively –135, –60, –200 and–348 kJ mol–1. The outer electronic configuration of B is 3s23p5 3s23p3 3s23p1 3s23p2

It seems like there is some confusion in your question as the outer electronic configuration of element B is given multiple times. However, I can tell you that the electron affinity generally increases across a period from left to right and decreases down a group on the periodic table.

The electron affinity values you provided indicate how much energy is released when an electron is added to a neutral atom to form a negative ion. A higher value (more negative) means that more energy is released, indicating a higher electron affinity.

Based on the values you provided, element D has the highest electron affinity (-348 kJ mol–1), followed by C (-200 kJ mol–1), A (-135 kJ mol–1), and then B (-60 kJ mol–1).

As for the electronic configuration, if we assume the correct configuration for B is 3s23p5, this would suggest that element B is in the second to last column of the periodic table (the halogens), which are known for having high electron affinities. However, this seems to contradict the electron affinity value you provided for B, which is the lowest of the four elements.

Please check the details of your question and provide the correct information so I can give you a more accurate answer.