Which of the following elements has a larger atomic radius than sulfur (S)?

• A. Sodium (Na)
• B. Chlorine (Cl)
• C. Phosphorus (P)
• D. Oxygen (O)

Answer: (A)

Verified step by step guidance

1. Recall that atomic radius generally decreases from left to right across a period in the periodic table due to increasing nuclear charge pulling electrons closer to the nucleus.
2. Recognize that sulfur (S) is located in period 3, group 16 of the periodic table.
3. Compare the positions of the given elements relative to sulfur: Sodium (Na) is in period 3, group 1; Phosphorus (P) is in period 3, group 15; Chlorine (Cl) is in period 3, group 17; Oxygen (O) is in period 2, group 16.
4. Understand that elements to the left of sulfur in the same period have larger atomic radii because they have fewer protons attracting the same number of electron shells, so Sodium (Na) will have a larger atomic radius than sulfur.
5. Conclude that among the options, Sodium (Na) has a larger atomic radius than sulfur due to its position further to the left in the same period.