Which of the following options correctly describes the general trends in electronegativity across the periodic table?

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

Answer: (C)

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 across a period (left to right) in the periodic table: electronegativity increases because atoms have more protons, increasing the nuclear charge and attracting electrons more strongly.
3. Recall the general trend down a group (top to bottom): electronegativity decreases because additional electron shells increase the distance between the nucleus and the valence electrons, reducing the nucleus's pull on bonding electrons.
4. Compare the given options with these trends: the correct description should state that electronegativity increases from left to right across a period and decreases from top to bottom within a group.
5. Conclude that the correct answer is the one that matches these trends, which is: 'Electronegativity increases from left to right across a period and decreases from top to bottom within a group.'