Ionization Energy Trends

Ionization Energy Trends - IonizationEnergyTrends

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
Ionization Energy Trends in the Periodic Table The ionization energy of an atom is the amount of energy  required  to remove an  electron from the gaseous form of that atom or ion. 1 st  ionization energy -  The energy required to remove the highest energy electron from  a neutral gaseous atom. For Example: Na (g) Na + (g) + e - I 1 = 496 kJ/mole Notice that the ionization energy is positive. This is because it  requires  energy to remove  an electron. 2 nd  ionization energy -  The energy required to remove a  second  electron from a singly  charged gaseous cation. For Example: Na + (g) Na 2+ (g) + e - I 2 = 4560 kJ/mole The second ionization energy is almost  ten times  that of the first because the number of  electrons causing repulsions is reduced. 3 rd  ionization energy -  The energy required to remove a  third  electron from a doubly  charged gaseous cation. For Example:
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Image of page 2
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 11/22/2011 for the course CHEMISTRY CHM1025 taught by Professor Laurachoudry during the Fall '10 term at Broward College.

Page1 / 4

Ionization Energy Trends - IonizationEnergyTrends

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online