Final answer:
The element with the most negative electron affinity is Fluorine, represented by the electron configuration 1s²2s²2p⁵. This occurs because Fluorine, having a strongly attracting incomplete valence shell, seeks to gain one additional electron to fill it.
Step-by-step explanation:
The question is asking about the electron configuration of an element with the most negative electron affinity. Electron affinity generally increases across the periodic table and up the groups, meaning that as we move to the right of a period and towards the top of a group, atoms tend to attract additional electrons more strongly. Therefore, the element with the most negative electron affinity would be the one that is closest to completing its valence shell.
The ground-state electron configurations given are:
- a. 1s²2s²2p¹: This represents the element Boron (B).
- b. 1s²2s²2p⁴: This represents the element Oxygen (O).
- c. 1s²2s²2p⁵: This represents the element Fluorine (F).
- d. 1s²2s²2p³: This represents the element Nitrogen (N).
Out of these elements, Fluorine has the highest electronegativity and is known for having the most negative electron affinity because it is only one electron away from completing its valence shell. Thus, the correct answer is c. 1s²2s²2p⁵, which represents Fluorine.