1 / 16

Periodic Trends

Periodic Trends. Periodic Trends. Periodic Trends are trends that occur across the periodic table and down the periodic table. Atomic Radius. Atomic Radius – size of the atom. . Decreases. Increases. . Atomic Radius. Radius decreases across a period

zelda-turner
Télécharger la présentation

Periodic Trends

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Periodic Trends

  2. Periodic Trends • Periodic Trends are trends that occur across the periodic table and down the periodic table

  3. Atomic Radius • Atomic Radius – size of the atom  Decreases Increases 

  4. Atomic Radius • Radius decreases across a period • Increased effective nuclear charge due to decreased shielding • Radius increases down a group • Addition of principal quantum levels

  5. Ionization Energy • _________________– the energy required to remove one mole of electrons, from one mole of gaseous atoms, to produce one mole of ions  Increases Decreases 

  6. Ionization Energy • First ionization energy • Second Ionization energy • Ionization energies are measure in KJ/mol • The have positive values showing that energy must be put in to remove an electron

  7. Ionization Energy • The magnitude of the ionization energy depends on 2 things… • The nuclear charge (how many protons are present) • The shielding effect of the inner electrons

  8. Ionization Energy • Across • increase because the nuclear charge increasesand the electrons are being removed from the same principal quantum level (shell), experiencing no extra shielding, and are therefore held more strongly. • (You’re trying to remove a more & more negatives, but still have the same number of positives pulling in on the electrons. They are pulling harder because there are few negatives)

  9. Ionization Energy • Down • decrease because the outer electrons are further away from the nucleus • Therefore the electrons are held less strongly.

  10. Example • Consider the following ionization energies • What is the predicted charge of this atom?

  11. Electron affinity • _________________– the energy change when one mole of gaseous atoms gains one mole of electrons , to form one mole of gaseous atoms  Increases Decreases 

  12. Electron affinity • Affinity tends to increase across a period • Affinity tends to decrease as you go down in a period • Electrons farther from the nucleus • experience less nuclear attraction

  13. Eelctronegativity • _________________ - A measure of the ability of an atom in a chemical compound to attract electrons  Increases Decreases 

  14. Metallic Character • _________________ – how much like a metal the element is  Decreases Increases 

  15. Ionic Radius • which will be larger: • Cl or Cl-1

  16. Ionic Radius • which will be larger: • Na or Na+1

More Related