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Periodic trends

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Periodic trends

  1. 1. Periodic Trends<br />
  2. 2. CA Standards<br />Students know how to use the periodic table to identify trends in ionization energy, electronegativity, and the relative sizes of ions and atoms.<br />
  3. 3. Atomic Radius<br />Definition: Half of the distance between nuclei in covalently bonded diatomic molecule <br /><ul><li>Radius decreases across a period
  4. 4. Increased effective nuclear charge due to decreased shielding
  5. 5. Radius increases down a group
  6. 6. Each row on the periodic table adds a “shell” or energy level to the atom</li></li></ul><li>Table of Atomic Radii<br />
  7. 7. Period Trend:Atomic Radius<br />
  8. 8. Ionization Energy<br />Definition: the energy required to remove an electron from an atom<br /><ul><li>Tends to increase across a period
  9. 9. As radius decreases across a period, the electron you are removing is closer to the nucleus and harder to remove
  10. 10. Tends to decrease down a group
  11. 11. Outer electrons are farther from the nucleus and easier to remove</li></li></ul><li>Periodic Trend:Ionization Energy<br />
  12. 12. Electronegativity<br />Definition: A measure of the ability of an atom in a chemical compound to attract electrons<br /><ul><li>Electronegativity tends to increase across a period
  13. 13. As radius decreases, electrons get closer to the bonding atom’s nucleus
  14. 14. Electronegativity tends to decrease down a group or remain the same
  15. 15. As radius increases, electrons are farther from the bonding atom’s nucleus</li></li></ul><li>Periodic Table of Electronegativities<br />
  16. 16. Periodic Trend:Electronegativity<br />
  17. 17. Summary of Periodic Trends<br />
  18. 18. Ionic Radii<br /><ul><li>Positively charged ions formed when</li></ul> an atom of a metal loses one or <br /> more electrons<br />Cations<br /><ul><li>Smaller than the corresponding </li></ul> atom<br /><ul><li>Negatively charged ions formed </li></ul> when nonmetallic atoms gain one <br /> or more electrons<br />Anions<br /><ul><li> Larger than the corresponding </li></ul> atom <br />
  19. 19. Table of Ion Sizes<br />

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