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PERIODIC TABLE

PERIODIC TABLE. The Language of Chemistry. CHEMICAL ELEMENTS - pure substances that cannot be decomposed by ordinary means to other substances. Aluminum. Bromine. Sodium. The Language of Chemistry. The elements, their names, and symbols are given on the PERIODIC TABLE.

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PERIODIC TABLE

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  1. PERIODIC TABLE

  2. The Language of Chemistry • CHEMICAL ELEMENTS - • pure substances that cannot be decomposed by ordinary means to other substances. Aluminum Bromine Sodium

  3. The Language of Chemistry • The elements, their names, and symbols are given on thePERIODIC TABLE

  4. The Periodic Table Dmitri Mendeleev (1834 - 1907) arranged elements in order of increasing atomic mass.

  5. Groups in the Periodic TableVertical columns Elements in groups react in similar ways! Have similar chemical and physical properties

  6. Periods in the Periodic TableHorizontal rows = 7

  7. Regions of the Periodic Table 3 classes of elements Metals Nonmetals metalloids

  8. METALS • 80% of elements are metals • Metallic lust, shiny • Good conductors (heat, electricity) • Solid at room temperature (except Hg) • Ductile – can be pulled through wires • Malleable

  9. NonMetals • Most are gases at room temperature • Dull color if solid • P and S are solids • Br - liquid • Poor conductors of heat and temperature • Carbon is the exception

  10. METALLOIDS • Have characteristics of metals and nonmetals • Can be metallic • Brittle (not malleable or ductile • Semiconductors ( Si)

  11. Group 1A: Alkali Metals Silvery colored Very Reactive http://www.youtube.com/watch?v=QSZ-3wScePM Malleable, ductile good conductors soft Cutting sodium metal

  12. Group 2A: Alkaline Earth Metals Magnesium Magnesium oxide Very reactive

  13. Transition Elements Lanthanides and actinides Malleable Good conductors of electricity and heat Iron, Cobalt and Nickel can create magnetic fields Can have several oxidation (Lose Electrons) states

  14. Group 7A: The Halogens (salt makers) F, Cl, Br, I, At Non Metals Extremely reactive/Dangerous Forms salts (NaCl) Forms Acids (HF) Used in: lamps (halogen), Teflon (Flourine + Carbon) http://www.youtube.com/watch?v=u2ogMUDBaf4&feature=related

  15. XeOF4 Group 8A: The Noble (Inert) GasesHe, Ne, Ar, Kr, Xe, Rn • Lighter than air balloons • “Neon” signs • Very Unreactive because they have full electron shells

  16. The Periodic Table -Review 1. Name group 1 2. Name group 7 3. 2 Characteristics of metals 4. 2 characteristics of nonmetals

  17. PERIODIC TRENDS • Atomic size- Increase in atomic number draws electrons closer to the nucleus = smaller

  18. Ionization Energy • The energy required to remove an electron from an atom in order to form an ion • Easy to remove electrons from group 1A more difficult to remove electrons across a row

  19. IONS • IONSare atoms or groups of atoms with a positive or negative charge. • Taking away an electron from an atom gives a CATION with a positive charge • Adding an electron to an atom gives an ANION with a negative charge. • To tell the difference between an atom and an ion, look to see if there is a charge in the superscript! Examples: Na+ Ca+2 I- O-2 Na Ca I O

  20. Forming Cations & Anions A CATION forms when an atom loses one or more electrons. An ANION forms when an atom gains one or more electrons F + e- --> F- Mg --> Mg2+ + 2 e-

  21. PREDICTING ION CHARGES In general • metals (Mg) lose electrons ---> cations • nonmetals (F) gain electrons ---> anions

  22. -3 -2 -1 +1 +2 Charges on Common Ions By losing or gaining e-, atom has same number of e-’s as nearest Group 8A atom.

  23. Ionic Size • Cations are always smaller than the atoms they form • Anions are always larger than the atoms from which they form

  24. Electronegativity • Ability of an atom in an element to attract electrons when the atom is in a compound

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