Question

3 would you expect an atom further down in a group to have a higher electron affinity or a lower electron affinity than the atoms above it? explain your answer

Explanation:

Electron affinity is the energy change when an atom gains an electron. As we go down a group in the periodic table, the atomic radius increases (because new electron shells are added). A larger atomic radius means the outermost electrons are farther from the nucleus, and the nuclear attraction for an incoming electron is weaker. So, an atom further down a group will have a lower electron affinity than the atoms above it because it’s less likely to attract and hold an additional electron due to increased atomic size and reduced nuclear attraction.

Answer:

An atom further down in a group is expected to have a lower electron affinity than the atoms above it. This is because as we move down a group, the atomic radius increases (due to the addition of electron shells), so the outermost electrons are farther from the nucleus. The nuclear attraction for an incoming electron is weaker, making it less favorable to gain an electron, thus resulting in a lower electron affinity.