How does the atomic radius of an atom affect its ability to attract additional electrons?

• A. Atoms with a larger atomic radius have a weaker attraction for additional electrons.
• B. Atomic radius does not affect an atom's ability to attract additional electrons.
• C. Atoms with a smaller atomic radius have a weaker attraction for additional electrons.
• D. Atoms with a larger atomic radius have a stronger attraction for additional electrons.

Answer: (A)

Verified step by step guidance

1. Understand that atomic radius refers to the size of an atom, typically measured from the nucleus to the outer boundary of the electron cloud.
2. Recall that the attraction an atom has for additional electrons depends largely on the effective nuclear charge (the net positive charge experienced by electrons) and the distance between the nucleus and the incoming electron.
3. Recognize that as atomic radius increases, the outer electrons are farther from the nucleus, which reduces the electrostatic attraction between the nucleus and any additional electrons.
4. Consider that a larger atomic radius means the nucleus has less pull on extra electrons due to increased distance and electron shielding by inner electrons.
5. Conclude that atoms with a larger atomic radius have a weaker attraction for additional electrons, while atoms with a smaller atomic radius have a stronger attraction.