How does the atomic radius of an atom affect its ability to hold on to its valence electrons?

• A. As atomic radius decreases, the ability to hold on to valence electrons decreases because the electrons are more tightly bound.
• B. Atomic radius has no effect on an atom's ability to hold on to its valence electrons.
• C. As atomic radius increases, the ability to hold on to valence electrons decreases because the electrons are farther from the nucleus and experience less electrostatic attraction.
• D. As atomic radius increases, the ability to hold on to valence electrons increases because the electrons are closer to the nucleus.

Answer: (C)

Verified step by step guidance

1. Understand that atomic radius refers to the average distance from the nucleus to the outermost electrons (valence electrons) in an atom.
2. Recall that the electrostatic attraction between the positively charged nucleus and the negatively charged valence electrons depends on the distance between them; this attraction follows Coulomb's law, which states that force decreases as distance increases.
3. Recognize that as atomic radius increases, valence electrons are located farther from the nucleus, which reduces the electrostatic attraction holding them in place.
4. Conclude that with weaker attraction due to increased distance, the atom's ability to hold on to its valence electrons decreases as atomic radius increases.
5. Therefore, the correct relationship is: as atomic radius increases, the ability to hold on to valence electrons decreases because the electrons are farther from the nucleus and experience less electrostatic attraction.