Final answer:
The correct order from greatest to least tendency to accept an electron, considering electron affinity and electronegativity trends, is Cl > F > O > N, with chlorine having the highest tendency to accept an electron among the elements listed.
Step-by-step explanation:
The question asks to arrange elements F (fluorine), Cl (chlorine), O (oxygen), and N (nitrogen) from greatest to least tendency to accept an electron. This property is closely related to the concept of electron affinity, which typically increases across a period. However, the electron affinities of elements in the second row of the periodic table (such as F), are less negative than those immediately below them in the third row (such as Cl) due to increased electron-electron repulsions in the 2p orbitals. Therefore, Cl tends to accept an electron more readily than F. Between O and N, oxygen has a slightly higher electronegativity, suggesting a stronger tendency to attract electrons compared to nitrogen. Following these trends, the correct order from greatest to least tendency to accept an electron is Cl > F > O > N.