September 25th 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) • REMINDER: Quest: matter and trends, next Tuesday October the 1st
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.
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.
More energy to remove electron from group 8 and less energy for the group 1.
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.
Visual Trend in Periodic Table Lowest Highest Highest Lowest
Periodic Table Trends: Ionization Energyby: Khanacademty http://www.youtube.com/watch?v=ywqg9PorTAw