second ionization energy

[MoooShuuu]

For the first ionization energy follow the trend, but to find which has a greater second ionization energy what do you do? Cations have a greater second ionization energy than neutral atoms, correct?

Do you look at for example Potassium and removing one electron (first ionization) would be easy because it wants to be in the stable Ar octet. But removing another (second IE) electron from Ar is much harder because it doesn't want to lose it's octet. Is this correct? Can anyone give some more examples of more difficult questions?

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[doc toothache]

http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch7/ie_ea.html

 

[zuma35]

Ionization energy is the energy needed to remove an electron. So for Na, for example, since removong one electron would give the stable noble gas configuration, the first ionizatiion energy is relatively small. The second ionization energy is drastically larger. For Mg, which is in group 2, removing two electrons would be relatively easy, and there would be a big jump in the 3rd ionization energy, and so forth. Also, IE increases as you remove more electons. So basically IE increases across the table. Also, it decreases down a row, bec since the atom is bigger, and the electrons are further from the nucleus, they are easier to remove.

 

[klutzy1987]

It follows the same rules as first ionization energy. The more protons something has the harder it is to abstract an electron. When something is in noble gas configuration the energy required skyrockets.