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The Periodic Table

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The Periodic Table

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    1. The Periodic Table Method of organization 1869—Dmitri Mendeleev Predicted the properties of elements and predicted the discovery of other elements based on the trends in the table. Mendeleev’s table was based on atomic mass. Moseley discovered that a more appropriate basis was atomic number. Periodic Law—When elements are arranged in order of increasing atomic number, their physical and chemical properties show a periodic pattern.

    2. Periodic Table Groups or families Periods Roman numeral column labels IUPAC labels Common Names Alkali metals Alkaline Earth metals Halogens Noble gases Transition Metals Inner transition metals Lathanides Actinides

    3. Periodic Table

    4. Periodic Table Metals Luster/shine Good conductors of heat and electricity. Malleable Ductile All are solids except for Mercury Nonmetals No luster Poor conductors Not malleable or ductile Many are gases; Bromine is a liquid; some are solids Semimetals or metalloids

    5. Electron Configurations Valence Electrons Using American Column labels If elements have the same # of valence electrons, they will have similar chemical properties. Abbreviated electron configurations Noble Gas Inner Core

    6. S, p, d, and f blocks

    7. Periodic Trends Properties of elements change in a periodic way as you move through the periodic table Examples Atomic Radius—increases as you move down a group. Decreases as you move from left to right across a period. WHY?

    9. Periodic Trends Ion Size Increases as you move down a group. Metal atoms tend to become smaller when they form ions. Nonmetal atoms tend to become larger when they form ions. WHY??

    12. Ionization Energy Amount of energy needed to remove an electron from an atom. Decrease as you move down a group. Increase as you move from left to right across a period. WHY??? Successive Ionization Energies What’s the pattern? WHY???

    15. Electron Affinity Energy change that occurs when an atom gains an electron. What do the negative numbers mean? Irregular periodic trend. Nonmetals usually have a more negative electron affinity than do metals. Noble gases have very high electron affinities. Octet Rule

    16. Electron Affinity

    17. Electronegativity Ability to attract electrons in a chemical bond. Increases from left to right across a period. Decreases as you move down a group. Exclude the noble gases. WHY???

    19. Periodic Trends Density—Increases as you move down a group. Increases as you move right to left across a period. Melting and Boiling Points decrease as you move down a group and increase as you move across a period.

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