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Modern Periodic Table

Modern Periodic Table. Mrs. Coyle. Part I. Introduction. Periods and groups. Metals, nonmetals and metalloids. The Modern Periodic Table. The Periodic Table is a listing of all the known elements. The elements are organized by: Atomic number Chemical Properties. Groups and Periods.

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Modern Periodic Table

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  1. Modern Periodic Table Mrs. Coyle

  2. Part I • Introduction. • Periods and groups. • Metals, nonmetals and metalloids.

  3. The Modern Periodic Table • The Periodic Table is a listing of all the known elements. • The elements are organized by: • Atomic number • Chemical Properties

  4. Groups and Periods • Group( or Family): a vertical column. Elements in groups have similar chemical properties. • Period: a horizontal row.

  5. Groups and Periods are numbered. • There are 7 periods. • There are 18 numbered columns.

  6. IUPAC • International Union of Pure and Applied Chemistry • 1985 new system for labeling groups.

  7. Metals, Nonmetals and Metalloids • Elements can be classified into: • Metals • Nonmetals • Metalloids (semimetals)

  8. Nonmetals Metals Metalloids

  9. Actinides and Lanthanides

  10. Physical Properties of Metals • Good conductors of electricity and heat. • Malleable (can be hammered into sheets). • Ductile (can be drawn into wires). • Lustrous.

  11. Chemical Properties of Metals • Easily lose electrons. • Form positive (+) ions.

  12. Nonmetal Physical Properties • They do not have the properties of metals.

  13. Nonmetal Chemical Properties • Gain electrons. • Form negative ions.

  14. Part II • Valence Electrons • Group 1 • Group 2

  15. -Niels Bohr’s Model – Distinct Energy Levels

  16. Periods • The periods (rows) of the periodic table indicate the highest energy level occupied by one or more electrons.

  17. Valence Electrons • The electrons the occupy the highest energy level of an atom. • Valence electrons play a key role in the chemical properties of an element.

  18. “A” Groups (Old System) • The “A” groups are numbered 18. • The number of the “A” groups correspond to the number of valence electrons.

  19. Group 1- Alkali Metals • 1 valence electron (ns1) • Form a 1+ ion. • Note: Hydrogen, a nonmetal, is located in the first column because it has one valence electron.

  20. Group 1- Alkali Metals Lithium Sodium Potassium Rubidium Cesium Francium

  21. Sodium’s Reaction with H2O Produces Hydrogen

  22. Reactivity of Alkali Metals • Increases from top to bottom of the group. • Which is more reactive Cesium or Sodium?

  23. Note: • Sodium and Potassium are stored in oil to keep them from reacting with oxygen and water in the air. • Cesium is stored in glass tubes of argon gas( an inert gas).

  24. Group 2- Alkali Earth Metals Beryllium Magnesium Calcium Strontium Barium Radium

  25. Group 2- Alkali Earth Metals • Have 2 valence electrons. • Form 2+ ions.

  26. Group 2- Alkali Earth MetalsReactions with Water • Be does not react with water. • Mg reacts with hot water. • Ca, Sr, Ba react easily with cold water. • Which way along the group does reactivity increase?

  27. Notes: • There is Mg in chrolophyll C55H72O5N4Mg • Calcium is in your bones, chalk, limestone, toothpaste, pearl (all as calcium carbonate).

  28. The Periodic Table

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