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Periodic Table

Periodic Table. Unit IV. Mendeleev Arranged elements by their masses Moseley Arranged elements by their atomic number Modern periodic table. I History. Groups Columns on the table Contain the same number of valence electrons Periods Rows on the table Use the same energy levels.

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Periodic Table

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  1. Periodic Table Unit IV

  2. Mendeleev • Arranged elements by their masses • Moseley • Arranged elements by their atomic number • Modern periodic table I History

  3. Groups • Columns on the table • Contain the same number of valence electrons • Periods • Rows on the table • Use the same energy levels II Arrangement of the Periodic Table

  4. Groups Periods

  5. III Types of Elements

  6. Location • Lower left side of the table • Properties • Metals are malleable and ductile • Metals are solids at room temperature except mercury • Metals have luster • Metals are good conductors • Metals have low ionization energy and low electronegativity • Metals lose electrons and form positive ions A. Metals

  7. Location • Upper right side of the table • Properties • Nonmetals are brittle • Nonmetals are gases or molecular solids at room temperature except bromine which is a liquid • Nonmetals are dull • Nonmetals are insulators • Nonmetals have high ionization energy and high electronegativity • Nonmetals gain electrons and form negative ions B. Nonmetals

  8. Location • Groups 3 through 12 • Properties • Series of elements that fill the d-sublevel • Transition metals have multiple oxidation states • Transition metals form colored ions C. Transition Metals

  9. Location • On the “stairs” plus Ge and Sb • Properties • Metalloids are brittle • Metalloids are solid at room temperature • Metalloids have luster • Metalloids are semi-conductors • Metalloidshave middle ionization energy and electronegativity values • Metalloids gain or lose electrons D. Metalloids

  10. Location • Noble Gases are in Group 18 • Properties • Noble gases are inert which means they do not react • Noble gases are monatomic • Noble gases have filled outer energy levels E. Noble Gases

  11. Ionization Energy (IE) • Amount of energy to remove an electron Atomic Radius • ½ distance between two nuclei Ionic Radius • Metals decrease in size • Nonmetals increase in size Electronegativity (EN) • Attraction for electrons Reactivity • Metal activity increases as you go left and down • Nonmetallic activity increases as you go up and to the right IV Properties of Elements

  12. Hydrogen Alkali Metals • Group 1 • Explosive in water Alkaline Earth Metals • Group 2 Halogens • Group 17 • All nonmetals • All phases of matter • F2 and Cl2 (gas) Br2 (liquid) I2 (solid) Noble Gases • Group 18 • Do not react except the largest members V Groups

  13. As you go across a period Atomic number increases Mass increases Valence electrons increase Energy level is constant Metallic character decreases Nonmetallic character increases Radius decreases IE and EN increase As you go down a group • Atomic number increases • Mass increases • Valence electrons remain the same • Energy levels increase • Metallic character increases • Nonmetallic character decreases • Radius increases • IE and EN decrease VI Trends

  14. Notable Observations

  15. s-electrons p-electrons NONMETAL SIDE d-electronss Metalloids METAL SIDE f-electrons

  16. s-electrons 2s 3s 4s 5s 6s 7s

  17. p-electrons 2p 3p 4p 5p 6p 7p

  18. d-electrons 3d 4d 5d 6d

  19. f-electrons 4f 5f

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