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T he Periodic Table

T he Periodic Table. Twelve elements have been known since ancient times. What do you think they are? (Name them, use your periodic table to help you.). T he Periodic Table. Twelve elements have been known since ancient times. What do you think they are?

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T he Periodic Table

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  1. The Periodic Table Twelve elements have been known since ancient times. What do you think they are? (Name them, use your periodic table to help you.)

  2. The Periodic Table Twelve elements have been known since ancient times. What do you think they are? (Name them, use your periodic table to help you.) carbon, sulfur, iron, copper, arsenic, silver, tin, antimony, gold, mercury, lead, bismuth

  3. The Periodic Table Why do you think these particular elements have been known for so long, while most elements were not discovered until the 1800s and 1900s?

  4. Overview of the Periodic Table

  5. Overview of the Periodic Table

  6. Trends of the Periodic Table “periodic” = repeating pattern Overall theme = electrons’ positions relative to each other and the nucleus determine the following properties: • Electron configuration • Ionic radius

  7. Electron Configuration Compare the charges on the ion list with the position of the element in the periodic table

  8. Electron Configuration Noble gas configuration = [core] e-’s ‘Outer’ electrons = valence e-’s Elements of groups 1A-8A have valence e-’s in s and p orbitals

  9. Periodic Trends The position of a valence electron and the ability to remove it from an atom are related to • the number of protons in the nucleus • the extent to which the valence electron is shielded from the positively-charged nucleus by the negatively-charged core electrons

  10. Isoelectronic Series = a group of ions and atoms that have the same electron configuration 1. Draw the electron configuration of each of the following elements. 2. What ions will they form? 3. When ions, how many electrons does each have? How many protons? 4. Predict the relative diameters of the members of this isoelectronic series.

  11. Isoelectronic Series Prediction: smallest to largest:

  12. Isoelectronic Series Prediction: smallest to largest: Mg2+ < Na+ < Ne < F-< O2-

  13. Reminder: Atomic Radius

  14. Ionic Radius • Cations (+) smaller than original atom • remove e-’s  greater pull from nucleus • Anions (-) larger than original atom • Increased repulsion swells the shell

  15. Ionic Radius

  16. Ionic Radius 1. In this table of ionic radii, how is the charge of the ions of elements in groups 1A-4A related to the group number?

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