SUCCESSIVE IONIZATION ENERGIES

Notes by: Sarah Elsarty

September 25th 2013

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

Lowest

Highest

http://www.youtube.com/watch?v=ywqg9PorTAw

Periodic Table Trends: Ionization Energyby: Khanacademty