1. IIIIII Ch. 4 - The Periodic Table 1. History and Organization of Elements (pp. 111 - 124) PT Rap PT Song PT Rap PT Song

2. I. History of Periodic Table z1700’s – scientists had identified only about 30 elements z1865 – Newlands – The Law of Octaves. With only 62 elements known, he noticed a repeating pattern every 8 elements when they were arranged in order of increasing atomic mass. They had similar chemical and physical properties.

3. A. Mendeleev zDmitri Mendeleev (1869) – 1 st orderly arrangement yOrganized 63 elements by increasing atomic mass yElements with similar properties were grouped together in columns. yThere were some discrepancies.

4. A. Mendeleev zDmitri Mendeleev (1869, Russian) yPredicted properties of undiscovered elements; empty spaces in his table.

5. B. Moseley zHenry Mosely (1913) yOrganized elements by increasing atomic number. yResolved discrepancies in Mendeleev’s arrangement by studying spectral lines that correlated to atomic # not atomic mass yApprox. 80 elements known at this time

6. B. Moseley z IUPAC recommended table yInternational Union of Pure and Applied Chemistry yPeriodic Law – the physical and chemical properties of the elements are periodic functions of their atomic numbers.

7. C. Periodic Tables zUse the blank table for the next sections of notes. Some of the following information will be put on your tables and some will be copied in your notes. zBOTH periodic tables will be reference materials.

8. Extended Version

9. Pages 114-115

10. zMain Group Elements (the purple ones on the left, s orbital, and right, p orbital) yRepresentative elements, outline zTransition Metals (the yellow section in the middle, d orbital) zInner Transition Metals (the green ones, f orbital) yLanthanide Series – shiny, reactive, irregular electron configuration yActinide Series - radioactive D. Blocks – Don’t color these, just bracket them or outline them.

11. E. Labeling zGroups: Write “group” above 1A. The columns are called groups or families – there are 18 of them. Label 1A thru 8A. Common properties Same number of valance shell electrons Add common ion charges to table zPeriods: These are rows going across – there are 7 of them. Please label 1-7 and write periods at the top. zPut in the bolded stairstep – what does this mean?

12. zUse the key in your book to help you color and label the different groups! zMetals (77% of the elements) All are solids except mercury which is a liquid (locate it on the red/white/blue p.t. Note what else is a liquid) Good conductors of electricity zNonmetals (15%) – most gasses, highlight the elements H He N O F Ne Cl Ar Kr Xe Rn as gasses zMetalloids or semiconductors (properties of both metals and nonmetals) (8%) F. Metallic Character pp.164-167

13. G. Special Groups zAlkali Metals (1A) zAlkaline Earth Metals (2A) zHalogens (7A) zNoble Gases (8A)

14. Alkali Metals zGroup 1A zList 7 properties: zWhat does alkaline mean? zWhat makes them so reactive?

15. Alkaline Earth zGroup 2A zLose 2 electrons zList 5 basic properties: zList uses of Magnesium and Calcium

16. Halogens zGroup 7A “salt former” zCombine with metals to produce a salt yMost reactive nonmetals yNeed one electron to be stable, -1 charge

17. Noble Gasses zGroup 8A zUsed to be called inert because they were thought to be unreactive. zThe outermost shell is filled in an octet, what does that mean? zList several uses for noble gases

18. H. Extra’s to Label zSolids, Liquids, Gases (Key at the bottom of red/white and blue p.t.) zSynthetic: Elements 93 and greater +43, 61 (key at the bottom of p.t.) zRadioactive: Elements 83 and greater