Atomic size generally increases down a group from "summary" of The Periodic Table: A Very Short Introduction by Eric R. Scerri
The size of an atom is a fundamental property that influences its chemical behavior. In the periodic table, atomic size generally increases as you move down a group. This trend is due to the increasing number of energy levels or shells occupied by electrons in each successive element. As you go down a group, each new element has an additional energy level that is farther away from the nucleus. Electrons in these outer energy levels experience weaker attraction to the nucleus, leading to an increase in atomic size. This is because the outermost electrons are shielded from the positive charge of the nucleus by the inner electron shells. The increase in atomic size down a group is not uniform, as the addition of a new energy level does not always result in a proportional increase in atomic size. For example, the atomic size of elements in the transition metals group may not follow this trend due to the complex interplay of electron-electron repulsions and attractions. The concept of atomic size increasing down a group is a useful tool in predicting the chemical properties of elements. Larger atoms have more electron shells and therefore are more likely to lose electrons to form positive ions. In contrast, smaller atoms tend to gain electrons to achieve a full outer electron shell and form negative ions. Understanding the trend of atomic size down a group also helps explain the reactivity of elements. Larger atoms have more loosely held electrons, making them more reactive in forming chemical bonds with other elements. This trend in atomic size provides a valuable framework for organizing and understanding the behavior of elements in the periodic table.
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