Which of the following diagrams correctly depicts the general trend in electronegativity across the periodic table?

• A. Electronegativity increases from left to right across a period and decreases from top to bottom down a group.
• B. Electronegativity decreases from left to right across a period and increases from top to bottom down a group.
• C. Electronegativity remains constant across periods and groups.
• D. Electronegativity increases from left to right across a period and increases from top to bottom down a group.

Answer: (A)

Verified step by step guidance

1. Understand that electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond.
2. Recall the general trend of electronegativity on the periodic table: it increases as you move from left to right across a period because atoms have more protons, increasing the effective nuclear charge and attracting electrons more strongly.
3. Recognize that electronegativity decreases as you move down a group because atoms have more electron shells, which increases the distance between the nucleus and the valence electrons, reducing the nucleus's pull on bonding electrons.
4. Combine these two trends to conclude that electronegativity increases from left to right across a period and decreases from top to bottom down a group.
5. Use this understanding to identify the correct diagram or statement that matches this trend among the given options.