A. Consider the following neutral electron configurations in which n has a constant value. Which configuration would belong to the element with the most negative electron affinity, Eea? 1. 2s2
2. 2s2 2p2
3. 2s2 2p5
4. 2s2 2p6
B. Arrange the following elements from greatest to least tendency to accept an electron.
Rank from greatest to least tendency to accept an electron. To rank items as equivalent, overlap them.
1. Sr
2. Sn
3. Rb
4. Te
5. I

2s2 2p5

Rb < Sr< Sn< Te<I

Explanation:

Electron affinity is the ability of an atom to accept electrons to form negative ions.

Electron affinity is a periodic trend that decreases down the group but increases across the period.

This accounts for the trends observed in the answer. The atom having the electronic configuration, 2s2 2p5 must be a halogen and it exhibits the highest value of electron affinity.

Also, since electron affinity increases across the period, the electron affinities of the elements increases. Therefore, the arrangement of atoms as shown in the answer depends on increasing electron affinity.

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