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Understanding Atomic Radius Trends in the Periodic Table

Learn how atomic radius changes with groups and periods in the periodic table, affecting the ability to gain or lose electrons. Get insights on electron gain and loss trends, along with nuclear charge influences. Improve your knowledge and mastery in chemistry.

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Understanding Atomic Radius Trends in the Periodic Table

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  1. Periodic Table Trends

  2. Atomic Radius Definition: The distance from center to the outermost orbit.

  3. Atomic Radius • Increases as you move down a group • # of orbits increase • Decreases as you move across a period • # of orbits stay the same but # of protons increase which pulls the electrons closer

  4. Atomic Radius

  5. Ability to gain electrons • Decreases as you move down a group • # of orbits increase, therefore inner electrons shield the attractive forces of the nucleus - attractive force not strong enough to gain electrons onto the outermost orbit • Increases as you move across a period • Stronger nuclear charge as the # of orbits stays the same but # of protons increase- allows for gain of electron on the outermost orbit

  6. Ability to gain electrons Electron gain

  7. Ability to lose electrons • Increases as you move down a group • # of orbits increase, therefore inner electrons shield the attractive forces of the nucleus - easier to loose an electron in the outermost orbit. • Decreases as you move across a period • Stronger nuclear charge as the # of orbits stays the same but # of protons increase- strong attractive forces prevent electron from being lost.

  8. Ability to lose electrons Electron loss Increases Decreases

  9. HOMEWORK • READ PG184-187 • DO Q 1-3,7,8,9 ON PG 187

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