Ionization energy

[anteater85]

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nitrogen's first IE is higher than Oxygen.Why?

 

[dfymarine]

lol, this is the most basic stuff! you'd better get cracking at it!


anyways, as you go from the left to right and down to up, the IE increases.

by definition, it is the energy needed to remove the electron, so which means as you go from left to right, the Atomic # is increased to hold the electron more tightly to the nucleus, thus making it hard to remove the electron!

i think that answer is wrong! lol

 

[joonkimdds]

nitrogen's first IE is higher than Oxygen.Why?

really?

Anyway, when it comes to periodic table trend, there are many ways to come up with reasoning that explains why it inc or dec this or that way.

But I highly doubt that DAT will ask for the reasoning.

Just know 4 facts; atomic size, electronegativity, electron affinity, and ionization energy.

And atomic size is the only one that inc down and left.
The other 3 inc up and right. (But electronegativity inc stops at group 7)

Besides these, also learn which one has bigger ionic size and which one forms acidic/basic anhydride....etc.

 

[dfymarine]

really?

Anyway, when it comes to periodic table trend, there are many ways to come up with reasoning that explains why it inc or dec this or that way.

But I highly doubt that DAT will ask for the reasoning.

Just know 4 facts; atomic size, electronegativity, electron affinity, and ionization energy.

And atomic size is the only one that inc up and right.
The other 3 inc left and downward.

Besides these, also learn which one has bigger ionic size and which one forms acidic/basic anhydride....etc.

wrong! it's the other way around.

 

[anteater85]

Can someone also tell me why nitrogen has a smaller radius and higher IE than Oxygen and carbon?

 

[UCB05]

nitrogen's first IE is higher than Oxygen.Why?

Ionization energy follows the general trend of decreasing as you go left along a period. However, you also have to look at the orbital configurations. O is 2s2, 2p4. Nitrogen is 2s2, 2p3. If you remember, p3 is one of those semi-stable states where all 3 p orbitals are half-filled. That's why N has a higher IE than Oxygen, which has one filled p orbital and 2 half-filled orbitals.

The same phenomenon happens between Be vs B. Be is 2s2, whereas B is 2s2, 2p1. Be has the higher IE because it has a semi-stable filled s orbital.

Edit*
googled: 1st IE N=1402.3 kJ/mol, O=1313.0 kJ/mol

 

[joonkimdds]

wrong! it's the other way around.

ahahahaha!!!

 

[yumi43]

whoa, someone got to it already, but atomic radius increases to the LEFT and DOWN, while electronegativity, electron affinity, and ionization energy increase UP and to the RIGHT.

i almost thought i was losing my mind there for a sec! 😛

 

[joonkimdds]

Can someone also tell me why nitrogen has a smaller radius and higher IE than Oxygen and carbon?

as it moves to right side, u have more proton and electrons thus they can pull stronger thus smaller.

ionization energy is the energy to remove electron.
When you have octet, it's super stable so why would you wanna remove it? right? thus removing it requires high energy.

if atom is at group 1, it is so close to become an octet which is super stable? right? so it wants to lose electron ASAP to be happy and stable octet and that's why it's so easy to give it up.

This trend continues~

 

[anteater85]

lol, this is the most basic stuff! you'd better get cracking at it!


anyways, as you go from the left to right and down to up, the IE increases.

by definition, it is the energy needed to remove the electron, so which means as you go from left to right, the Atomic # is increased to hold the electron more tightly to the nucleus, thus making it hard to remove the electron!

i think that answer is wrong! lol

I'm ok in Chem but this Cliff Ap chemistry is throwing me off. It has some weirt question. I guess if i see of more these question i'm going to stop reading it. Since I already understood everything from the kaplan

 

[anteater85]

Ionization energy follows the general trend of decreasing as you go left along a period. However, you also have to look at the orbital configurations. O is 2s2, 2p4. Nitrogen is 2s2, 2p3. If you remember, p3 is one of those semi-stable states where all 3 p orbitals are half-filled. That's why N has a higher IE than Oxygen, which has one filled p orbital and 2 half-filled orbitals.

The same phenomenon happens between Be vs B. Be is 2s2, whereas B is 2s2, 2p1. Be has the higher IE because it has a semi-stable filled s orbital.

Edit*
googled: 1st IE N=1402.3 kJ/mol, O=1313.0 kJ/mol

THank you...that makes sence now

 

[joonkimdds]

Ionization energy follows the general trend of decreasing as you go left along a period. However, you also have to look at the orbital configurations. O is 2s2, 2p4. Nitrogen is 2s2, 2p3. If you remember, p3 is one of those semi-stable states where all 3 p orbitals are half-filled. That's why N has a higher IE than Oxygen, which has one filled p orbital and 2 half-filled orbitals.

The same phenomenon happens between Be vs B. Be is 2s2, whereas B is 2s2, 2p1. Be has the higher IE because it has a semi-stable filled s orbital.

Edit*
googled: 1st IE N=1402.3 kJ/mol, O=1313.0 kJ/mol

Hm...this is something new.
how about N vs. F?

 

[UCB05]

Hm...this is something new.
So should we ignore the trend and use the configuration rule?

I doubt the DAT is going to try to trick people with an exception-to-the-rule question like this. As far as I remember, all the questions were very straightforward.

1st IE of N is still much smaller than F. As much as N might like its half filled orbitals, F HATES losing electrons being so close to [Ne] configuration 😛

 

[anteater85]

Hm...this is something new.
how about N vs. F?

well again I got these guestions from the Cliff Ap chemistry and it goes to details. I studied Kaplan 3 times already and never saw anything like that. I'm gonna go with the kaplan rules🙂

 

[sixkiller]

Yeah, I'm like 99 percent sure that the DAT won't test this.

This is more applicable for the chemistry gre or the chemistry olympiad exam.

 

[anteater85]

what else do u guys suggest to use for G-chem other than kaplan and destroyer to get 20s

 

[UCB05]

what else do u guys suggest to use for G-chem other than kaplan and destroyer to get 20s

Do you have time? If so you can probably find Schaum's Gen Chem at Borders/B&N. The problem is that it's basically a textbook printed on cheap stock. It has all you need to know, but it's dense.

 

[joonkimdds]

I have a question.
what's electron configuration for Fe2+?
Does it lose 2 electrons from S first?
or Does it lose 1 from each to form half filled D orbital which is supposed to be very stable?

 

[UCB05]

I have a question.
what's electron configuration for Fe2+?
Does it lose 2 electrons from S first?
or Does it lose 1 from each to form half filled D orbital which is supposed to be very stable?

Nah, it loses its two 4s electrons since they're in the highest-energy orbital. Fe3+ gets the half-filled d orbitals, though.

 

[sixkiller]

Joon,

Aren't you taking your DAT tomorrow? You should just go to sleep or something.

 

[anteater85]

Do you have time? If so you can probably find Schaum's Gen Chem at Borders/B&N. The problem is that it's basically a textbook printed on cheap stock. It has all you need to know, but it's dense.

I'll check it out becuase i don't like the cliff AP chem book. thx

 

[joonkimdds]

Joon,

Aren't you taking your DAT tomorrow? You should just go to sleep or something.

I will sleep at 3am, wake up at 8am~ i got test at 12:30.

 

[anteater85]

I will sleep at 3am, wake up at 8am~ i got test at 12:30.

Good luck bro....I'm sure u'll do great....post up ur scores tomorrow before u get drunk

 

[joonkimdds]

If I do well, I will definitely post it.
If u don't see my score within next 20 hrs, assume that I failed it.

 

[UCB05]

If I do well, I will definitely post it.
If u don't see my score within next 20 hrs, assume that I failed it.

Dude, go to bed. Get a good night's sleep or you're going to be sitting there burnt out and tired on the QR section.

 

[Pat Kelly]

Nah, it loses its two 4s electrons since they're in the highest-energy orbital. Fe3+ gets the half-filled d orbitals, though.

3d energy shells are higher in energy, and 3d5 half filled shells may be more stable than stripping 2 4s electrons - I am not sure about that.

edit - it is indeed 3d6. (Chemistry - McMurry and Fay pg 866). sorry for the confusion

 

[UCB05]

3d energy shells are higher in energy, and 3d5 half filled shells may be more stable than stripping 2 4s electrons - I am not sure about that.

I meant principle quantum level energy. Fe preferentially loses the 4s electrons first, and a 3d electron third. You can look it up

 

[Shinpe]

When filling up electrons, you will always fill up s first then d (with half-filled exceptions like 4s13d5 and 4s13d10 instead of 4s23d4 and 4s23d9)

When taking electrons out, you will always take out the s electrons before getting to d electrons.