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Periodic Table

Periodic Table. Development of the Periodic Table. Classification – grouping elements based on similarities. Cross classification – grouping into more than one group @ a time. Purpose - organize, explain, & predict information about the elements. Mendeleev.

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Periodic Table

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  1. Periodic Table

  2. Development of the Periodic Table Classification – grouping elements based on similarities. Cross classification – grouping into more than one group @ a time. Purpose - organize, explain, & predict information about the elements

  3. Mendeleev • Dmitri Mendeleev (1869, Russian) • Organized elements by increasing atomic mass. • Elements with similar properties were grouped together. • There were some discrepancies.

  4. Mendeleev • Dmitri Mendeleev (1869, Russian) • Predicted properties of undiscovered elements.

  5. Moseley • Henry Mosely (1913, British) • Organized elements by increasing atomic number. • Resolved discrepancies in Mendeleev’s arrangement. • The modern periodic table is arranged in order of increasing atomic #

  6. Mendeleev’s Periodic Table Dmitri Mendeleev

  7. Modern Russian Table

  8. Stowe Periodic Table

  9. A Spiral Periodic Table

  10. “Mayan” Periodic Table

  11. The Periodic Table Period Group or Family Group or family Period

  12. 1 -Horizontal rows are called Periods or Series -There are 7 periods - Elements have the same # shells or Energy levels 2 3 4 5 6 7

  13. -Vertical columns are calledGroups or Families -Elements with same # of outer shell electrons -Elements are placed in columns by similar properties.

  14. Blocks • Main Group Elements • Transition Metals • Inner Transition Metals

  15. Main Families • Alkali Metals • Alkaline Earth Metals • Transition Metals • Halogens • Noble Gases

  16. 8A 1A 2A 3A 4A 5A 6A 7A The elements in the A groups are called the Representative Elements

  17. These are called the inner transition elements and they belong here The group B are called the Transition Metals

  18. Group 1A are the alkali metals Group 2A are the alkaline earth metals

  19. Group 7A is called the Halogens Group 8A are the Noble gases

  20. Metallic Character • Metals • Nonmetals • Metalloids

  21. Alkali Metals • All alkali metals have 1 valence electron • Alkali metals are NEVER found pure in nature; they are too reactive • Reactivity of these elements increases down the group • React with water to form a base Potassium, K reacts with water and must be stored in kerosene

  22. Alkaline Earth Metals • All alkaline earth metals have 2 valence electrons • Alkaline earth metals are less reactive than alkali metals • Alkaline earth metals are not found pure in nature; they are too reactive • The word “alkaline” means “basic” • common bases include salts of the metals Ca (OH)2 Mg (OH)2

  23. Transition MetalsCreate + ions, typically with more than one charge Copper, Cu, is a relatively soft metal, and a very good electrical conductor. Mercury, Hg, is the only metal that exists as a liquid at room temperature

  24. Examples of Metals Potassium, K reacts with water and must be stored in kerosene Copper, Cu, is a relatively soft metal, and a very good electrical conductor. Zinc, Zn, is more stable than potassium Mercury, Hg, is the only metal that exists as a liquid at room temperature

  25. Physical Properties of Metals • Metals are good conductors of heat and electricity • Metals are malleable • Metals are ductile • Metals have high tensile strength • Metals have luster • Are solids @ room temp.

  26. Chemical Properties of Metals • Tend to lose electrons easily • Form positive ions (cations) when combining with other atoms • Have Low ionization energy • Have Low electronegativity

  27. Nonmetals • Nonmetals are poor conductors of heat and electricity • Nonmetals tend to be brittle • Many nonmetals are gases at room temperature Carbon, the graphite in “pencil lead” is a great example of a nonmetallic element.

  28. Chemical Properties of Non metals • Tend to gain electrons • Form negative ions (anions) when combining with other atoms • Have High ionization energy • Have High electronegativity

  29. Examples of Nonmetals Microspheres of phosphorus, P, a reactive nonmetal Sulfur, S, was once known as “brimstone” Graphite is not the only pure form of carbon, C. Diamond is also carbon; the color comes from impurities caught within the crystal structure

  30. Properties of Metalloids • They have properties of both metals and nonmetals. • Metalloids are more brittle than metals, less brittle than most nonmetallic solids • Metalloids are semiconductors of electricity • Some metalloids possess metallic luster

  31. Silicon, Si – A Metalloid • Silicon has metallic luster • Silicon is brittle like a nonmetal • Silicon is a semiconductor of electricity Other metalloids include: • Boron, B • Germanium, Ge • Arsenic, As • Antimony, Sb • Tellurium, Te

  32. Halogens • Halogens all have 7 valence electrons, form anions by gaining electrons. • Halogens are never found pure in nature; they are very reactive • Halogens in their pure form are diatomic molecules (F2, Cl2, Br2, and I2) • They react with metals to form salts. Chlorine is a yellow-green poisonous gas

  33. Noble Gases • Noble gases have 8 valence electrons (except helium, which has only 2) • These elements do not easily combine with other elements– they are chemically un reactive. • Colorless, odorless and un reactive; they were among the last of the natural elements to be discovered

  34. Periodicity Explained • Valence = Outer shell electrons • The orbitals fill up in a regular pattern • The outer shell electron configuration repeats • The properties of atoms therefore repeat when placed in order of Atomic Number

  35. H 1 Li 3 Na 11 K 19 Rb 37 Cs 55 Fr 87 1s1 1s22s1 1s22s22p63s1 1s22s22p63s23p64s1 1s22s22p63s23p64s23d104p65s1 1s22s22p63s23p64s23d104p65s24d10 5p66s1 1s22s22p63s23p64s23d104p65s24d105p6 6s24f145d106p67s1

  36. He 1s2 2 Ne 1s22s22p63s23p64s23d104p6 1s22s22p63s23p64s23d104p65s24d105p6 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p6 1s22s22p6 10 Ar 1s22s22p63s23p6 18 Kr 36 Xe 54 Rn 86

  37. s - block s1 s2 • Alkali metals all end in s1 • Alkaline earth metals all end in s2 • really have to include He but it fits better later. • He has the properties of the noble gases.

  38. Transition Metals - d block d4 d9 d1 d2 d3 d5 d6 d7 d8 d10

  39. The p -block p1 p2 p6 p3 p4 p5

  40. f6 f13 f1 f2 f3 f4 f5 f7 f8 f10 f12 f14 f11 f9 f - block • inner transition elements

  41. Orbital filling table

  42. Writing Electron configurations the easy way

  43. Electron Configurations repeat • The shape of the periodic table is a representation of this repetition. • When we get to the end of the row the outermost energy level is full. • This is the basis for our shorthand.

  44. The Shorthand • Write the symbol of the noble gas before the element. • Then the rest of the electrons. • Aluminum - full configuration. • 1s22s22p63s23p1 • Ne is 1s22s22p6 • So… Al is [Ne] 3s23p1

  45. More examples • Ge = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2 • Ge = [Ar] 4s23d104p2 • Hf = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d2 • Hf = [Xe] 6s2 4f14 5d2

  46. The Shorthand Again Sn- 50 electrons The noble gas before it is Kr Takes care of 36 Next 5s2 Then 4d10 Finally 5p2 [ Kr ] 5s2 4d10 5p2

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