0:00
Hello there.
00:02
So in this given question we have given four species.
00:06
Okay.
00:07
Oxygen fluoride, boron molecule, hydrogen molecule and c22 negative.
00:13
And okay.
00:14
Here in this question we have to find out which one has strong bond strength after one.
00:39
Removal of one electron fine so here we use moat according to molecular orbital theory here we will found out bond orders okay bond order is equals to electron in bonding orbital minus electron in anti -bonding orbitals divided by, that is the formula will be here, bo is equal to bo minus abo divided by, fine, okay, so let's check all these four given species one by one.
01:43
First we have here, h2 molecule, hydrogen, okay, if i write sigma, means, bonding orbital and if i write sigma star it is anti -bonding orbital.
02:12
Bonding orbital promote stronger bonds or stronger molecule, anti -bonding promote weaker bonds.
02:22
Fine.
02:22
So this is anti -bonding and bonding orbitals.
02:25
Now let's start solving our question.
02:28
We have two hydrogen atoms in this molecule.
02:33
The electron configuration of one hydrogen atom is 1s1.
02:41
So for the formation of h2 molecule, each hydrogen has given one electron.
02:48
So for h2 molecule we have two electrons and filling is like sigma 1s2.
02:57
So here we have only sigma 1s.
03:02
Sigma 1s orbital now check bond order bonding electron bonding orbital electron minus anti -bonding orbital electrons divided by 2 here hydrogen molecule have only bonding orbital in which it has two electrons minus 0 divided by 2 that is bond order is 1 fine and we have to find the species which on removing one electron get stronger bond fine so if i remove one electron from here if one electron is removed so only sigma 1 s 1 left now the bond order is 1 divided by 2 minus 0 that is bond order in this case is 0 .5.
04:14
So now we have an important information here.
04:19
If electron removed from bonding electron, bond order will get decreased, as happened in h2 molecule.
04:49
Earlier it was 1 and now is 0 .5.
04:52
So h2 is not our answer.
04:55
This is not our answer.
04:58
Now move to of molecule.
05:04
Here is, now let's count the total electron.
05:07
Oxygen will give 8 electrons.
05:11
Fluorine will give 9 electrons.
05:14
So here we have total 8 plus 9.
05:23
That is 17 electrons.
05:27
Now let's start filling this.
05:29
Sigma 1 is 2, sigma star 1 is 2, sigma 2 is 2, sigma star 2 is 2, sigma 2p z 2, pi 2p x 2 is equal to pi 2 p p y 2 now let's count the electron 2 4 6 8 10 10 12 14 now move further pi star 2 p x pi star 2 p 2 electron in each orbital now again count 2 4 6 8 8 10 10 10 12, 14, 16 extra electron.
06:28
I have filled the extra electron.
06:30
Remove this.
06:35
17 total.
06:36
So what i have said, this star is anti -bonding orbital and this is bonding orbital.
06:47
Now let's calculate our bond order.
06:50
Here we have bonding orbital 2, 4, 6, 8, 2, 4, 6, 8, 10.
07:04
Fine, we have 10 bonding orbital electrons minus 2, 4, 6 and 7.
07:15
We have 7 anti -bonding electrons divided by 2.
07:22
Minus 7 is 3, 3 divided by 2 is 1 .5...
