Successfully reported this slideshow.
We use your LinkedIn profile and activity data to personalize ads and to show you more relevant ads. You can change your ad preferences anytime.

Chapter 5.3 : Electron Configuration and the Periodic Table


Published on

Published in: Education
  • Be the first to comment

Chapter 5.3 : Electron Configuration and the Periodic Table

  1. 1. Chapter 5.3<br />Electron Configurations and Periodic properties<br />
  2. 2. Objectives:<br />Define atomic radii and ionic radii, ionization energy, electron affinity, and electronegativity.<br />Compare periodic trends for these properties and state reasons for variations.<br />Define valence electrons, and state how many are present in atoms of each main-group element.<br /> Compare the these same properties of d-block elements with those of the main-group elements<br />
  3. 3. Atomic Radii<br />Defined as one-half the distance between the nuclei of identical atoms that are bonded together<br />Period trends<br />Decrease from left to right<br />Due to increasing positive charge<br /><ul><li>Group trends
  4. 4. Increase down a group
  5. 5. Due to occupying higher energy levels</li></li></ul><li>Atomic Radii<br />
  6. 6. Ionization Energy<br />Defined as energy required to remove one electron from a neutral atom of an element (IE)<br />A + energy A+ + e-<br /><ul><li>Ion – atom or group of bonded atoms that has a positive or negative charge.</li></li></ul><li>Ionization Energy<br />Period trends<br />Generally increase across a period<br />Due to increasing nuclear charge<br /><ul><li>Group trends
  7. 7. Generally decrease down a group
  8. 8. Due to electron shielding of outer electrons</li></li></ul><li>Electron Affinity<br />Defined as the energy change that occurs when an electron is acquired by a neutral atom<br />A +e- A- + energy <br /><ul><li>Quantity released represented by a negative number
  9. 9. Forced
  10. 10. Unstable</li></ul>A +e- + energyA-<br /><ul><li>Quantity absorbed represented by a positive number</li></li></ul><li>Ionic radii<br />Cation – positive ion<br />Formed by loss of one or more electrons<br />Smaller due to removal of electron & stronger pull by nucleus on remaining electrons<br /><ul><li>Anion– negative ion
  11. 11. Formed by gain of one or more electrons
  12. 12. Larger due to addition of electron & remaining electrons are not pulled as strongly by nucleus</li></ul>Ionic Radii<br />
  13. 13. Valence Electrons<br />Defined as the electrons available to be lost, gained, or shared in the formation of chemical compounds<br />Valence electron<br />Sodium atom<br />Chlorine atom<br />
  14. 14. Valence Electrons<br />1 2 3 4 5 6 7 8<br />
  15. 15. Electronegativity<br />Defined as the measure of the ability of an atom in a chemical compound to attract electrons<br />Want to gain electrons!!<br />Noble gases have very low electronegativity<br />Alkali metals are low as well<br />Halogens have the highest<br />Electronegativity<br /><ul><li>Period trends
  16. 16. Tend to increase across a period
  17. 17. Due to wanting to fill outer shell
  18. 18. Group trends
  19. 19. Tend to decrease down a group</li></li></ul><li>Electronegativity<br />