What general trend does electronegativity follow in the Periodic Table?

The correct choice highlights that electronegativity increases from left to right across a periodic table and also increases as you move up within a group. This trend can be understood through the underlying principles of atomic structure and electron interaction.

As you move from left to right across a period, atoms have an increasing number of protons in their nucleus, which enhances the positive charge that holds the electrons in the outer shells. This increased nuclear charge attracts the bonding electrons more strongly, leading to higher electronegativity values for elements found toward the right side of the periodic table, such as the nonmetals.

Moving from the bottom to the top of a group, the outer electrons are located in shells that are closer to the nucleus due to fewer electron shells. This proximity results in a stronger nuclear attraction for the bonding electrons compared to elements lower down in the group, where additional electron shells shield the nucleus’s positive charge. Consequently, electronegativity values increase as you ascend a group.

This consistent trend in electronegativity is pivotal for understanding chemical bonding and reactivity among different elements in various periods and groups, influencing how they interact to form compounds.