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Understanding Periodic Table and Chemical Periodicity

Explore the periodicity of elements in Mendeleev's table and learn about groupings such as alkali metals, noble gases, and halogens. Understand electron configurations, atomic radii, ionization energy, and electronegativity trends. Dive into the role of electrons in chemical behavior and the patterns in the periodic table.

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Understanding Periodic Table and Chemical Periodicity

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  1. Chemical Periodicity?What?

  2. Periodicity • When elements are organized • in order of  atomic mass, and • grouped by similarities of chemical properties, • a certain “pattern” or periodicity • of properties becomes evident Draft for first version of Mendeleev's periodic table (17 February 1869).

  3. Review of the Periodic Table

  4. Group IA – alkali metals Review of the Periodic Table

  5. Group IA – alkali metals H1 - 1s1 Li3 - 1s22s1 Na11 - 1s22s22p63s1 K19 - 1s22s22p63s23p64s1 Rb37 - 1s22s22p63s23p63d104s24p65s1 Cs55 - 1s22s22p63s23p63d104s24p64d105s25p66s1 Fr87 - 1s22s22p63s23p63d104s24p64d104f145s25p65 d106s26p67s1

  6. Group IIA – alkaline earth metals Review of the Periodic Table

  7. Group IIA – alkaline earth metals Be4 - 1s2 2s2 Mg12 - 1s22s22p63s2 Ca20 - 1s22s22p63s23p64s2 Rb38 - 1s22s22p63s23p63d104s24p65s2 Cs55 - 1s22s22p63s23p63d104s24p64d105s25p66s2 Fr87 - 1s22s22p63s23p63d104s24p64d104f145s25p65 d106s26p67s2

  8. Group VIII – Noble Gases Review of the Periodic Table

  9. Group VIII – Noble Gases He2 - 1s2 Ne10 - 1s22s22p6 Ar18 - 1s22s22p63s23p6 Kr36 - 1s22s22p63s23p63d104s24p6 Cs54 - 1s22s22p63s23p63d104s24p64d105s25p6 Rn86 - 1s22s22p63s23p63d104s24p64d104f145s25p65 d106s26p6

  10. Group VII – Halogens Review of the Periodic Table

  11. Group VII – Halogens F9 - 1s22s22p5 Cl17 - 1s22s22p63s23p5 Br35 - 1s22s22p63s23p63d104s24p5 I53 - 1s22s22p63s23p63d104s24p64d105s25p5 At85 - 1s22s22p63s23p63d104s24p64d104f145s25p65 d106s26p5

  12. Review of the Periodic Table Group VI

  13. Group VI O8 - 1s22s22p4 S16 - 1s22s22p63s23p4 Se34 - 1s22s22p63s23p63d104s24p4 Te52 - 1s22s22p63s23p63d104s24p64d105s25p4 Po84 - 1s22s22p63s23p63d104s24p64d104f145s25p65 d106s26p4

  14. Electron’s Role in Chemical Behavior • Atoms are most stable when their outermost “s” and “p” subshells are filled. – “the rule of 8” • Electron’s in the outermost shell determine chemical reactivity

  15. Periodic Table and e- config. 1 2 3 4 5 6 7 Increasing energy level (shell) px1 py1 pz1 px2 py2 pz2 s1 s2 Increasing energy sublevel (subshell)

  16. Periodic Patterns - Atomic Radii 2r

  17. Atomic Radii

  18. Periodicity and Atomic Radius • In group: • atomic radius increases as you move down the column • Across period: • Atomic radius decreases as you • Move from left to right • Rationale: • group – adding outermost electron shell • row –  pulling in with  nuclear charge

  19. Ionic Radius 97pm vs 181pm 190pm vs 102pm

  20. Periodic Patterns and Ionic Radius • In group: • ionic radius increases as you move down the column • Across period: • Ionic radius is max in group 5 • Lower on left and right • Rationale: • group –outermost shell • row – transition between losing and gaining electrons to reach stability

  21. Ionic Radius

  22. Periodic Patterns and Ionization Energy • Ionization energy ≡ energy needed to remove an electron from an atom or ion • first ionization energy - energy needed to remove an electron from a neutral atom • second ionization energy - energy needed to remove a second electron from a positively charged ion

  23. Ionization Energy

  24. Periodic Patterns and Ionization Energy • In group: • ionization energy  as you move down the column • Across period: • Ionization energy  as you move from left to right • Rationale: • group –outermost shell electrons • farther away from nucleus • row – outermost electron more tightly • held

  25. Ionization Energy

  26. Periodicity and Electronegativity • Electronegativity ≡ a measure of how tightly held an electron is.

  27. Electronegativity

  28. Periodicity and Electronegativity • In group: • electronegativity  as you move down the column • Across period: • Electronegativity  as you move from left to right • Rationale: • group –atoms more willing to accept another electrons due to  nuclear charge and shielding • row – atoms move closer to completed “s” and “p” orbitals and stability

  29. Electronegativity

  30. Periodic Trends – Summary Decreasing Atomic Radii Decreasing Ionic Size Increasing Ionization Energy Increasing Electronegativity Increasing Atomic Radii Increasing Ionic Radius Decreasing Ionization Energy Decreasing Electronegativity

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