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III. Periodic Trends p. 140 - 154

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III. Periodic Trends p. 140 - 154

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    1. III. Periodic Trends (p. 140 - 154) Ch. 5 - The Periodic Table

    2. A. Periodic Law When elements are arranged in order of increasing atomic #, elements with similar properties appear at regular intervals.

    3. B. Chemical Reactivity Families Similar valence e- within a group result in similar chemical properties

    4. B. Chemical Reactivity Alkali Metals Alkaline Earth Metals Transition Metals Halogens Noble Gases

    5. Atomic Radius size of atom C. Other Properties

    6. Atomic Radius D. Atomic Radius

    7. Atomic Radius D. Atomic Radius

    8. Why larger going down? Higher energy levels have larger orbitals Shielding - core e- block the attraction between the nucleus and the valence e- Why smaller to the right? Increased nuclear charge without additional shielding pulls e- in tighter D. Atomic Radius

    9. First Ionization Energy E. Ionization Energy

    10. First Ionization Energy E. Ionization Energy

    11. Why opposite of atomic radius? In small atoms, e- are close to the nucleus where the attraction is stronger Why small jumps within each group? Stable e- configurations don�t want to lose e- E. Ionization Energy

    12. Successive Ionization Energies E. Ionization Energy

    13. Successive Ionization Energies E. Ionization Energy

    14. Melting/Boiling Point F. Melting/Boiling Point

    15. Ionic Radius G. Ionic Radius

    16. Which atom has the larger radius? Examples

    17. Which atom has the higher 1st I.E.? Examples

    18. Which atom has the higher melting/boiling point? Examples

    19. Which particle has the larger radius? Examples

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