Chemical Forums
1 Hour
1 Day
1 Week
1 Month
Forever
June 03, 2024, 06:02:47 PM
Forum Rules
: Read This Before Posting
Home
Help
Search
Login
Register
Chemical Forums
Chemistry Forums for Students
Undergraduate General Chemistry Forum
Why does the first energy of ionization of oxygen is lesser than of nitrogen?
« previous
next »
Print
Pages: [
1
]
Go Down
Topic: Why does the first energy of ionization of oxygen is lesser than of nitrogen? (Read 1196 times)
0 Members and 1 Guest are viewing this topic.
Blueberries116
Regular Member
Posts: 32
Mole Snacks: +0/-1
Gender:
Freelance scientist and learner
Why does the first energy of ionization of oxygen is lesser than of nitrogen?
«
on:
February 22, 2020, 04:17:57 AM »
The following question arises from a question I found in my book.
The problem states the following:
Experimentally it has been determined that the value of the first energy of ionization of oxygen is lesser than the first energy of ionization of nitrogen. Select the statement which explains this:
The alternatives given were:
[itex]\begin{array}{ll}
1.&\textrm{The higher electronegativity of oxygen}\\
2.&\textrm{The lesser electron affinity of nitrogen}\\
3.&\textrm{The lesser radius of oxygen}\\
4.&\textrm{The higher stability of nitrogen}\\
5.&\textrm{The higher electroaffinity of nitrogen}\\
\end{array}[/itex]
According to my book the answer is the fourth option, but I couldn't find a way to justify this. What sort of explanation can do this?.
My guess is that nitrogen forms a triple bond with itself which is higher than the oxygen and this makes the molecule more stable but I don't know if this can be translated into a higher energy of ionization nitrogen rather than the oxygen which does have a sigma and pi bonds. Am I right?. Can someone illustrate this or bring some sort of diagram with some values to justify this?. It would help a lot if an answer could help me why should I discard the second option?. Doesn't nitrogen has lesser electron affinity than the oxygen?.
Wouldn't it mean that having a lesser electron affinity cause to be easier to strip out an electron from its outher shell rather than the opposite as the question indicates?. Can someone really help me with this?.
Logged
Have a nice day!
Mr. Deeds
Regular Member
Posts: 10
Mole Snacks: +0/-0
Re: Why does the first energy of ionization of oxygen is lesser than of nitrogen?
«
Reply #1 on:
February 22, 2020, 09:00:12 AM »
Edit*
The e-config of Oxygen is paired as opposed to Nitrogen. This pairing allows for less energy required to ionize gaseous Oxygen atoms. I would have this makes Nitrogen more stable than Oxygen, but this is a special case. Look at Hund's Rule for more information about this special case.
«
Last Edit: February 22, 2020, 10:15:23 AM by Mr. Deeds
»
Logged
Enthalpy
Chemist
Sr. Member
Posts: 4040
Mole Snacks: +304/-59
Re: Why does the first energy of ionization of oxygen is lesser than of nitrogen?
«
Reply #2 on:
February 24, 2020, 01:12:04 PM »
Let's evacuate first the electron affinity. It characterises the energy that binds an
additional
electron. The ionization energy characterises the
loss
of an electron. These quantities differ, and are not clearly linked.
Do you know molecular orbitals? N
2
has all valence electrons on bonding orbitals, deep, hence is very stable and non-reactive, while O
2
has two more electrons that must go on anti-bonding orbitals, shallow.
https://en.wikipedia.org/wiki/Molecular_orbital_diagram#Dinitrogen
Logged
mjc123
Chemist
Sr. Member
Posts: 2060
Mole Snacks: +298/-12
Re: Why does the first energy of ionization of oxygen is lesser than of nitrogen?
«
Reply #3 on:
February 25, 2020, 04:54:38 AM »
As the question was stated, I assume it refers to atomic O and N, not the molecules, especially as the OP is also asking other questions about atomic electron configurations.
Logged
Print
Pages: [
1
]
Go Up
« previous
next »
Sponsored Links
Chemical Forums
Chemistry Forums for Students
Undergraduate General Chemistry Forum
Why does the first energy of ionization of oxygen is lesser than of nitrogen?