As you move down a group (family) on the periodic table, how does electronegativity typically change?

• A. Electronegativity first increases, then decreases.
• B. Electronegativity increases.
• C. Electronegativity decreases.
• D. Electronegativity remains constant.

Answer: (C)

Verified step by step guidance

1. Understand that electronegativity is a measure of an atom's ability to attract electrons in a chemical bond.
2. Recall the periodic trends: as you move across a period from left to right, electronegativity generally increases due to increasing nuclear charge and decreasing atomic radius.
3. Focus on the trend down a group (family): as you move down, atoms have more electron shells, increasing the atomic radius and shielding effect.
4. Recognize that the increased distance between the nucleus and valence electrons, along with shielding, reduces the nucleus's pull on bonding electrons, causing electronegativity to decrease.
5. Conclude that the typical trend down a group is a decrease in electronegativity.