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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 dont 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