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I2? Second ionization energy?
I leave now, but please leave a response, thanks
Write the electron configuration of all the atoms. Then see which electron will be removed in the second ionization reaction. Then think about which electron would be the hardest to remove. I think you will see it. For example, K has to lose its s electron first and then it will lose an electron from a closed inner orbital, the p. Now do the same for the rest of the atoms.
Okay, I'll try that... thank you!
\[K:~ 1s^1~ 2s^2~ 2p^6~ 3s^2 ~3p^6~4s^1\]\[Ca:~1s^1~ 2s^2~ 2p^6~ 3s^2 ~3p^6 ~4s^2\]\[Sc:~1s^1 ~2s^2 ~2p^6 ~3s^2~ 3p^6 ~4s^2~ 3d^1\]\[Fe:~1s^1~ 2s^2 ~2p^6 ~3s^2~ 3p^6~ 4s^2~ 3d^6\] Would it be K?
@Australopithecus got anything?
Pretty sure Ionization energy is related to effective nuclear charge (electronegativity)
yes i believe so
Ca is more electronegative than K, (it is closer to the right the periodic table)
yea but it says SECOND Ionization energy so.. idk :\ im confused
Isn't there a law where available orbitals are filled with 1 electron before they are filled with 2
I think you are over thinking it
Anyways if something has a strong affinity for electrons (it is electronegative) it should take even more energy to pull the next electron off it
yea but we're talking about pulling the second electron off
let me read up on orbitals, I haven't done this stuff in ages
and wouldnt K use the most energy since its stable after the first electron being removed so it would take a lot more energy to remove a second one
what is the point of this question?
Which of the following has the largest I2? (Transition metals lose their s electrons before the d electrons) K Ca Sc Fe they want to know which element would have the largest second ionization energy
the more you go toward to the right, the ionization energy increases. so it's down to up left to right and diagonal right
there's a chart of a whole periodic table on this one. let me pull it up for you
I posted it I'm pretty sure @nincompoop
i answered Fe since its farthest to the right as would follow the rule but my teacher said to try again cuz that was wrong..so i honestly dont even know
that is because d orbitals dont hold electrons very well, wish I knew why tbh
It is why metals are conductive though
okay so Sc and Fe are ruled out, yea?
any way you can just link the index?
This looks like an interesting book, I really wish I could take inorganic chemistry and structure and bonding
tha pages end at 110..
you have to look at the displayed page on the book itself, don't follow how it shows on your browser or adobe. I took every chapter individually so it is easier for people to download or view
yea the individual page numbers end at 110
okay look at the upper right and upper left hand corners of the book, it tells you the actual page in the book itself.
I just got home, so let me settle down and I will help you later.
nin im not stupid...the header on the last page says: 110- Chapter Two Atomic Structure and Periodicity
Thanks nincompoop this is a great source
it is :)
umm...i think i got it, I'll put some more thought to it and ask my instructor again later Thanks guys!
Well p orbitals are higher energy than s orbitals
Which I should have remembered durp
s orbitals are closer to the nucleus than p orbitals, http://www.chembook.co.uk/fig2-3.jpg
These orbitals are just calculations of where you would most likely find the electron, based on the uncertainty principle.
I know the order of the orbitals.
so it would be potassium
what would really help is to read the whole chapter. either of the first link or the last link. you will get the whole picture, and it will help a lot in terms of their properties during bonding.
You are right, it seems interesting, I will probably read it right now ha Initial configuration of K 1s1 2s2 2p6 3s2 3p6 4s1 First electron withdrawn 1s1 2s2 2p6 3s2 3p5 4s1 second electron withdrawn 1s1 2s2 2p6 3s2 3p4 4s1 is this correct? It has been forever since I have done these
It sucks how little I remember from gen chem
lol how many joules does it require to remove one from the p block?
off hand I have no clue, I just remember hunds rule states that all higher orbitals should be filled with 1 electron before with 2 electrons
I may be mistaken I took gen chem 4 years ago
I know p orbitals hold onto electrons weaker than s orbitals. Its why organic compounds with greater s character are more acidic
or rather carbon atoms with greater s character are more acidic
yeah that's in terms of filling the space, but that has little to do with ionization. for the ionization you follow from right to left of the configuration so for a K, the first Ionization is the 4s1
So hunds rule just dictates the optimal electron configuration of an atom?
Hund's Rule is just a description of the behavior in terms of the Pauli Principle.
oh oh, I need to read that chapter I still dont really understand ha
so it would be Ca because the Sc and Fe d orbitals shield the protons, K only has one 4s1 electron to remove whereas Ca has 2 4s electrons to remove
ok ok downloading it now thanks for posting it :D
It would be K. The second electron is going from a complete orbital and that would require a lot of energy. So I2 would be pretty high. The transition metal orbitals are pretty close in energy so I2 would be pretty small.