Which statement correctly describes the trend of electronegativity on the periodic table?

• A. Electronegativity increases from left to right across a period and decreases from top to bottom down a group.
• B. Electronegativity increases from left to right across a period and increases from top to bottom down a group.
• C. Electronegativity remains constant across periods but increases down groups.
• D. Electronegativity decreases 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 tends to increase as you move from left to right across a period because atoms have more protons, increasing the 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 observations 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 evaluate the given statements and identify the one that correctly describes the trend of electronegativity on the periodic table.