Question Analysis
This question evaluates the student's understanding of periodic trends in electronegativity, specifically how it changes across a period and down a group.
Key Concept Explanation
Electronegativity increases as you move from left to right across a period and decreases as you move down a group. This is due to the increasing nuclear charge and decreasing atomic radius across a period, and the increasing atomic radius outweighing the effect of increased nuclear charge down a group.
Step-by-step Solution
1. Identify the position of sulfur (S) in the periodic table: S is in period 3, group 16.
2. Compare the positions of the given elements with sulfur:
Phosphorus (P) is in period 3, group 15 (to the left of S).
Chlorine (Cl) is in period 3, group 17 (to the right of S).
Selenium (Se) is in period 4, ...
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