Which of the following periodic trends generally occurs as you move from top to bottom within a group on the periodic table?

• A. Electronegativity increases
• B. Ionization energy increases
• C. Atomic radius increases
• D. Electron affinity becomes more negative

Answer: (C)

Verified step by step guidance

1. Understand that periodic trends describe how certain properties of elements change as you move across periods (rows) or down groups (columns) in the periodic table.
2. Focus on the trend moving from top to bottom within a group. As you move down a group, new electron shells are added, increasing the distance between the nucleus and the outermost electrons.
3. Recognize that increased distance and additional electron shells cause the atomic radius to increase because the outer electrons are farther from the nucleus and experience more shielding from inner electrons.
4. Recall that electronegativity and ionization energy generally decrease down a group because the outer electrons are less tightly held due to increased shielding and distance from the nucleus.
5. Note that electron affinity does not consistently become more negative down a group; it varies depending on the element's electron configuration.