Why is it generally easier for an atom to lose an electron if its atomic radius is larger?

• A. Because atoms with larger radii have higher ionization energies.
• B. Because the outermost electron is farther from the nucleus and experiences weaker electrostatic attraction.
• C. Because the electron cloud is denser, making it easier for electrons to escape.
• D. Because a larger atomic radius means the atom has more protons, which repel electrons.

Answer: (B)

Verified step by step guidance

1. Understand that ionization energy is the energy required to remove an electron from an atom.
2. Recognize that the electrostatic attraction between the nucleus and an electron depends on the distance between them; this is described by Coulomb's law, where force decreases as distance increases.
3. Note that a larger atomic radius means the outermost electron is farther from the nucleus, so the electrostatic attraction holding that electron is weaker.
4. Since the attraction is weaker, less energy (lower ionization energy) is needed to remove the electron, making it easier for the atom to lose an electron.
5. Therefore, the key reason is that the outermost electron experiences weaker electrostatic attraction due to being farther from the nucleus in atoms with larger atomic radii.