Which of the following elements has the strongest attraction for electrons (i.e., the highest electronegativity)?

• A. F (fluorine)
• B. N (nitrogen)
• C. Cl (chlorine)
• D. O (oxygen)

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 from left to right across a period and decreases from top to bottom within a group.
3. Identify the positions of the given elements on the periodic table: N (period 2, group 15), O (period 2, group 16), F (period 2, group 17), and Cl (period 3, group 17).
4. Compare the elements based on their group and period: since F and Cl are in the same group, but F is in a higher period (period 2 vs period 3), F will have a higher electronegativity than Cl; similarly, O is to the right of N in the same period, so O has higher electronegativity than N.
5. Conclude that fluorine (F), being in period 2 and group 17, has the highest electronegativity among the options because it is the most to the right and highest up in the periodic table.