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Electron Configuration and the Periodic Table

Electron Configuration and the Periodic Table. 5-2. 5-2 Learning Targets. Name, identify, and classify groups on the periodic table. Identify group, period and element based on electron configuration. Periods. Horizontal rows on PT

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Electron Configuration and the Periodic Table

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  1. Electron Configuration and the Periodic Table 5-2

  2. 5-2 Learning Targets • Name, identify, and classify groups on the periodic table. • Identify group, period and element based on electron configuration.

  3. Periods • Horizontal rows on PT • Period number corresponds to the highest principal quantum number (n) of the elements in the period • Sublevel blocks • Periodic table can be broken into blocks corresponding to s,p,d,f sublevels

  4. Blocks and Groups • s- block Groups 1 and 2 • Group 1- Alkali Metals • One s electron in outer shell • Soft, silvery metal of low density and low mp • Highly reactive with nonmetals • Reacts strongly with water to make hydrogen • Never found pure in nature • High reactivity

  5. Group 2- Alkaline Earth metals • Two s electrons in outer shell • Denser, harder, stronger, less reactive than group1 • Too reactive to be found pure in nature • High reactivity

  6. Hydrogen • Unique does not share properties of other elements in group 1

  7. Main group elements • s and p block elements • Groups 1,2, 13-18 • Also called representative elements

  8. d- block Groups 3-12 • Metals with typical metallic properties • Referred to as transition metals • Group number = sum of outermost s and d electrons • Less reactive than alkali or alkaline-earth metals (low reactivity) • Pd, Pt, and Au least reactive

  9. p- block Groups 13-18 • Along with s block called main group elements • All contain full s orbital • Properties vary greatly • Metals • Softer and less dense than d-block metals • Harder and more dense than s-block metals • All except Bi too reactive to be found alone in nature

  10. Metalloids • Brittle solids with some metallic and some nonmetallic properties • Semiconductors • Nonmetals • Halogens (group 17) are most reactive of nonmetals (high reactivity) • Noble Gas (group 18) not reactive (low reactivity)

  11. f- block Lanthanides and Actinides • f-block called Rare Earth Metals • Lanthanides are shiny metal similar in reactivity to group 2 metals • Actinides • All are reactive • Plutonium (94) trough Lawrencium (103) are man made High reactivity No group number assigned to f block elements

  12. Relationships Among Group #, blocks, and E configurations

  13. Relationship Between Periodicity and Electron Configurations

  14. Find the period, block, and group • [Ne] 3s1 • Period = # of s orbital • 3 • Block= what orbital is filling last (s,p,d,f) • s • Group= s + p (add d if present) • Remember f block elements don’t have group number • 1

  15. Find the period, block, and group • [Xe] 6s2 • 6th, s, 2 • [Kr] 5s1 • 5th, s, 1 • [Ar] 4s2 • 4th, s ,2 • [Ar] 4s2 3d8 • 4th, d, 10 • [Kr] 5s2 4d 10 • 5th, d, 12 • [Ar] 4s2 3d10 4p3 • 4th, p, 15 • [Ne]3s23p3 • 3rd, p, 15

  16. Find the period, block, and group Be able to identify element , type (metal, nonmetal, or metalloid), and reactivity (high or low) • [He] 2s2 2p3 • 2nd, p, 15 • Nitrogen, non, low • [Xe] 6s1 4f14 5d10 • 6th, d, 11 • Gold, trans metal, low • [Rn] 7s1 • 7,s, 1 • Francium, Alkali, high • [Ar] 4s2 3d10 4p5 • 4th, p, 17 • Bromine, halogen, high

  17. Find the period, block, and group Be able to identify element , type (metal, nonmetal, or metalloid), and reactivity (high or low) • [Xe] 6s2 4f6 • 6th, f, none • Nd, rare earth metal, high • [Xe] 6s1 4f145d9 • 6th, d, 10 • Pt, Transition metal, low

  18. [Ne] 3s2 3p5 • 3rd, p, 17 • Cl, Halogen, high • [Ne] 3s2 3p6 • 3rd, p, 18 • Ar, Noble gas, non reactive

  19. Write the outer electron configuration • Group 13, period 3 • 3s2 3p1 • Al • Group 17, period 2 • 2s2 2p5 • F • Group 16, period 4 • 4s2 3d104p4 • Se

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