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

• A. As atomic radius increases, the ability to hold on to valence electrons decreases.
• B. Atomic radius has no effect on the ability to hold on to valence electrons.
• C. Atoms with smaller radii are less able to hold on to their valence electrons.
• D. As atomic radius increases, the ability to hold on to valence electrons increases.

Answer: (A)

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. Recognize that the force of attraction between the nucleus and valence electrons depends on the distance between them and the effective nuclear charge (the net positive charge experienced by electrons).
3. Recall Coulomb's law, which states that the force of attraction between two charged particles decreases as the distance between them increases, expressed as \(F = k \frac{q_1 q_2}{r^2}\), where \(r\) is the distance between charges.
4. Apply this concept to atoms: as atomic radius increases (meaning valence electrons are farther from the nucleus), the electrostatic attraction between the nucleus and valence electrons weakens, making it easier for the atom to lose or share these electrons.
5. Conclude that atoms with larger atomic radii hold their valence electrons less tightly, so the ability to hold on to valence electrons decreases as atomic radius increases.