1 / 8

Successive Ionization Energies

September 25 th 2013. Successive Ionization Energies . Notes by: Sarah Elsarty . Homework. Read pages 36-41 (Periodic Trends in Atomic properties) Hw: finish all worksheets pgs. 47 #1-18 (review) Pgs. 48 #1-19, 31, 47,55, 57,66-69 (review)

tricia
Download Presentation

Successive Ionization Energies

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. September 25th 2013 Successive Ionization Energies Notes by: Sarah Elsarty

  2. Homework • Read pages 36-41 (Periodic Trends in Atomic properties) • Hw: finish all worksheets • pgs. 47 #1-18 (review) • Pgs. 48 #1-19, 31, 47,55, 57,66-69 (review) • REMINDER: Quest: matter and trends, next Tuesday October the 1st

  3. What are ionization energies The energy it takes to remove and electron from an atom, in the gaseous state, to become a cation. Cation: a passively charged atom.

  4. Textbook Summary (Pg. 38-9) • Ionization energy: quantity of energy required to remove a single valence electron from an atom or ion in the gaseous state. • General ionization equation: X(g)+energy X+(g)+e • specific example: Li(g)+520 Kj/mol Li+(g)+e- • the unit used is kilojoules per mole.

  5. More energy to remove electron from group 8 and less energy for the group 1.

  6. Worksheet summary • Less energy is required to remove the outermost electrons. (First IE) • Requires more energy for each successive ionization energy. (second IE, third IE and so on) • It take more energy to remove the electron closer to the nucleuses. • Noticeable jump in IE once the atom have reached a noble gas configuration. • Once valence electrons have been removed the radius decreases.

  7. Visual Trend in Periodic Table Lowest Highest Highest Lowest

  8. Periodic Table Trends: Ionization Energyby: Khanacademty http://www.youtube.com/watch?v=ywqg9PorTAw

More Related