1 / 6

Periodicity

How are the electron configurations related to the atomic radius, ionization energy, and all the other “facts” about atoms?. Periodicity. Atomic radius – half the distance between the nuclei of two adjacent atoms. Periodicity- rEpeating properties.

brone
Download Presentation

Periodicity

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. How are the electron configurations related to the atomic radius, ionization energy, and all the other “facts” about atoms? Periodicity

  2. Atomic radius – half the distance between the nuclei of two adjacent atoms. Periodicity- rEpeating properties As you go across a period, no new layers are added. Each atom has progressively more protons to attract the electrons. As you go across a period the atomic size decreases. Shielding is constant. Nuclear charge increases. H = 1s Li = 1s 2s Mg = 1s2s 3s Na = 1s2s 3s Al = 1s2s 3s As you go down a period, you add layers. Each layer increases shielding, and increases the size of the atom.

  3. Ionization energy– The amount of energy required to remove an electron from a gaseous element. Periodicity- rEpeating properties As you go across a period, no new layers are added. Each atom has progressively more protons to attract the electrons. As you go across a period the ionization energy increases. Shielding is constant. Nuclear charge increases. H = 1s Li = 1s 2s Mg = 1s2s 3s Na = 1s2s 3s Al = 1s2s 3s As you go down a period, you add layers. Each layer increases shielding, and decreases the ionization energy.

  4. Tightly held electrons are difficult to remove – high energy. The more nuclear charge, and/or the smaller the atom, the more tightly held the electrons will be. General Trends in electronegativity • The greater nuclear charge and the smaller the atom, the more likely an electron will be accepted into an atom.

  5. Summary

  6. Which is larger (higher atomic radius? Same sheilding, greater nuclear charge.

More Related