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Periodic Table

This guide explores the Periodic Table's history and structure, detailing how elements are arranged by atomic number and mass. It distinguishes between groups (columns) and periods (rows) based on electron configurations. Key element classifications—metals, nonmetals, metalloids, and noble gases—are discussed alongside their unique properties, including conductivity, ionization energy, and reactivity trends. The document highlights the increasing atomic radius down groups and the changes in metallic/nonmetallic character across periods, providing a comprehensive overview of elemental trends.

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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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