Atomic Size and Ionization Trends
Atomic size is one of the key properties that changes systematically across the periodic table. Scientists measure atomic radius (half the distance between nuclei of two bonded atoms) to determine an atom's size, often in picometers (pm).
Notice these clear patterns: atoms get larger as you move down a group (column) because more energy levels are being added. As you move across a period (row), atoms get smaller because the stronger nuclear charge pulls electrons closer. These patterns will help you predict relative sizes of any elements!
When atoms gain or lose electrons, they form ions with charges. Metals typically lose electrons to form positively charged cations (like Na⁺), while nonmetals usually gain electrons to form negatively charged anions (like Cl⁻). The energy needed to remove an electron is called ionization energy, which decreases down a group and increases across a period.
Remember this! First ionization energy shows opposite trends from atomic radius - when atoms get smaller, ionization energy gets larger (and vice versa).