How does electronegativity change from left to right across a period?

In the context of chemistry, electronegativity—defined as the ability of an atom to attract shared electrons in a chemical bond—typically increases as you move from left to right across a period in the periodic table.12

This trend occurs because, as you move across a period, the nuclear charge increases due to the addition of more protons. While the number of electrons also increases, the outer-shell electrons are pulled more closely toward the nucleus by this stronger positive charge, resulting in a smaller atomic radius and a greater affinity for electrons. Consequently, elements on the right side of the periodic table (excluding noble gases) exhibit higher electronegativity values compared to those on the left.312