Which of the following elements has the highest ionization energy?
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Ionization energy is the quantity of energy that an isolated, gaseous atom in the ground electronic state must absorb to discharge an electron, resulting in a cation
@Photon336 Can u handle this !!!!!!!! I have an emergency now
Not the answer you are looking for? Search for more explanations.
ionization energy = amount of energy you need to remove the least tightly bound electron from a neutral atom.
This is what you must know
ionization energy generally increases as you go fro left to right across a period. and decreases as you go down a group
Let's try to understand this first, (if you're interested in knowing more).
as you go form left to right across a period, you are adding a proton but not changing the number of shells.
so what this means is that the positive charge is getting bigger, and this is something called Zeff. effective nuclear charge is the pull of the nucleus on the electrons and as we go from left to right it becomes greater.
so what this means is two things: this greater pull from nucleus will mean that it will be harder to remove an electron, which means higher Ionization energy.
now as we go down a group, the number of shells increases. what happens here is that now the electrons are farther away from the nucleus and the pull isn't so great, so it's easier to remove an electron.
So what would the answer be? @Photon336
Sorry I wrote that as your thing was going through!
no problem i'm trying to look up the values for these to help
@mmazach which one do you think it is and why?
Cl 1251.2 Kj/mol
Se 941 kj/mol
Si 786.5 kj/mol
from this table we can see that chlorine has the highest ionization energy