Phase 1: Understand Electronegativity Patterns
Within the periodic table:
- Electronegativity rises from left to right across a period, driven by increased nuclear charge.
- Electronegativity declines from top to bottom within a group, due to larger atomic radii and enhanced electron shielding.
Phase 2: Identify Elements on the Periodic Table
- Fluorine (F): Positioned in Group 17, Period 2
- Oxygen (O): Positioned in Group 16, Period 2
- Nitrogen (N): Positioned in Group 15, Period 2
- Chlorine (Cl): Positioned in Group 17, Period 3
All these elements are situated in the upper-right quadrant, the region characterized by the highest electronegativity.
Phase 3: Compare Electronegativity Values
Utilizing the Pauling scale with approximate values:
- Fluorine: 3.98
- Oxygen: 3.44
- Nitrogen: 3.04
- Chlorine: 3.16
Fluorine exhibits the most elevated value.
Phase 4: Analyze Trends
- Across Period 2 (N, O, F): Electronegativity demonstrates an increasing trend, thus establishing the order F>O>N.
- Down Group 17 (F, Cl): Electronegativity shows a decreasing trend, hence F>Cl.
Consequently, Fluorine is identified as the most electronegative element.
Phase 5: Conclusion
Fluorine possesses the highest electronegativity, aligning with option (1)