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Periodic Table of Elements

Periodic Table of Elements. Bohr Model: and Valence electrons http://youtu.be/trsln8RCEVo Casseopia http://youtu.be/5MMWpeJ5dn4 Dan Radcliffe http://youtu.be/rSAaiYKF0cs Bald Guy: http://youtu.be/nsbXp64YPRQ Song: http://youtu.be/afFw91fvNJM http://youtu.be/zGM-wSKFBpo.

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Periodic Table of Elements

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  1. Periodic Table of Elements

  2. Bohr Model: and Valence electrons • http://youtu.be/trsln8RCEVo Casseopia • http://youtu.be/5MMWpeJ5dn4 • Dan Radcliffe • http://youtu.be/rSAaiYKF0cs • Bald Guy: • http://youtu.be/nsbXp64YPRQ • Song: • http://youtu.be/afFw91fvNJM • http://youtu.be/zGM-wSKFBpo

  3. Dmitri Mendeleev • Russian chemist. • Created first version of the periodic table. • Predicted properties of elements yet to be discovered. Rockin the shaggy beard…

  4. Mendeleev arranged elements according to their atomic weights. • Today they are arranged by atomic number.

  5. Periodic Law • Properties of elements are periodic functions of their atomic numbers. • In other words, properties tend to repeat as you start a new period.

  6. Groups/Families • Columns on the table (1-18). • Elements have the same number of valence electrons. • Similar chemical properties. • Tend to form bonds in a similar way to get stable octet.

  7. Periods (1-7) • The rows on the table. • Have the same number of occupied energy levels. • They do not have similar properties.

  8. Get to Know Your Groups

  9. 1 valence electron Form +1 Ions Very reactive Found only in compounds. Alkali Metals

  10. Rubidium

  11. Comparing the Alkali Metals http://youtu.be/uixxJtJPVXk

  12. 2 valence electrons Form +2 ions Very reactive Found only in compounds Alkaline Earth Metals

  13. 7 valence electrons Form -1 ions Very reactive All nonmetals Halogens

  14. Gas Liquid Solid FLUORINE Extremely reactive gas IODINE solid → gas (sublimes)

  15. Inert Gases Not reactive Have stable octet (except He) Monoatomic gases Noble Gases

  16. s, p, d, f, “Blocks” • Indicates what sublevel is being filled last in the atom

  17. Metals in the “lower” columns. (d-block metals) “Inner” transition metals are the two bottom rows (f-block metals) Transition Metals

  18. Transition Metals • Form colored compounds and solutions.

  19. Metals/Nonmetals/Metalloids

  20. Metals • Have luster • Malleable • Ductile • Conduct heat and electricity • Tend to lose valence electrons and form positive ions • All solids (except Hg)

  21. Nonmetals • No luster • Brittle (if solid) • Don’t conduct • Tend to gain valence electrons and form negative ions • Can be solid ( I, C, P, S) , liquid (Br), or gases (F, Cl, N, O) • Hydrogen is considered a nonmetal

  22. Metalloids (Semimetals) • Most elements along the “staircase” • Can have properties of both metals and nonmetals. • B, Si, Ge, As, Sb, Te, At

  23. Trends in the Period Table

  24. Atomic Radius • Distance from the nucleus of an atom to the outer edge of it’s electron cloud.

  25. Get out Reference Table S

  26. Trends in Radius Li Na K Rb Cs Fr • Down a Group Ex: Group 1 What happens? • Across a Period Ex: Period 2 What happens? Li Be B C N O F Ne

  27. Down a Group • Size increases • Why? You add new energy levels • Across a Period • Size decreases • Why? Increasing nuclear charge pulls on the energy levels

  28. http://youtu.be/ba2yN2HtPTA

  29. Ionization Energy • Energy required to remove the outermost electron from an atom.

  30. Get out Reference Table S

  31. Trends in Ionization Energy • Down a Group Ex: Group 1 What happens? • Across a Period Ex: Period 2 What happens? Li Na K Rb Cs Fr Li Be B C N O F Ne

  32. What is the trend? Directly related to Atomic Radius. • Large Radius = Lower Ionization Energy Why? The further the outmost electron to the nuclear pull the easier to remove it.

  33. http://youtu.be/8F9nA4Fg3Rw

  34. Electronegativity • The relative attraction an atom has for electrons involved in bond formation.

  35. The higher the EN value the more the atom “pulls” on electrons involved in a bond. • This can result in “polar” and “nonpolar” bonds.

  36. Fluorine has the highest EN value = 4 (The EN scale was created by comparing other elements to Fluorine)

  37. Get out Reference Table S

  38. Trends in Electronegativity • Down a Group Ex: Group 1 What happens? • Across a Period Ex: Period 2 What happens? Li Na K Rb Cs Fr Li Be B C N O F Ne

  39. http://youtu.be/93G_FqpGFGY

  40. Metallic/NonMetallic Character • More “Metallic”: • Large radius • Low Ionization Energy • Low Electronegativity • More “Non Metallic”: • Small radius • High Ionization Energy • High Electronegativity

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