Answer
See explanation
Work Step by Step
Electronegativity trends: Across a row of the periodic table (from left to right), electronegativity generally increases. This is because as you move across a row, the number of protons in the nucleus increases, leading to a stronger attractive force for electrons in the same energy level. Down a column (group), electronegativity generally decreases. This is due to the increase in atomic size and the shielding effect of inner electrons, which reduces the attraction for outer electrons.
Comparison with ionization energies and atomic radii: Ionization energy follows a similar trend to electronegativity across a row, as elements with higher electronegativity require more energy to remove an electron. Atomic radii, on the other hand, increase across a row (due to increased nuclear charge) and increase down a column (due to additional energy levels). Larger atomic radii are associated with lower electronegativity, as electrons are farther from the nucleus and experience weaker attraction.
