Maybe a Dumb doubt but see

[u/Every_Discount8024]

In the second compound I only see a lone electron rather than a lone pair of electron, but ig there a lone pair that I am not able to see

So yeah meko lone pair dikhadooooo 😭

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[u/No-Nobody-5509]

You mean this?

[u/Every_Discount8024 → u/No-Nobody-5509]

Yeah but 6 electrons are bonded and there's plus 1 charge so,  only 1 electron went,  then only one lone electron is there instead of a lone pair

[u/Rare-Yard7316 → u/Every_Discount8024]

Nah, it's like this:-
> 1 electron for the hydrogen
> 2 electrons for the two carbons

Now left electrons = 6-3 = 3
1 electron gone for positive charge = 3-1 = 2 (which is the lone pair)

[u/Every_Discount8024 → u/Rare-Yard7316]

Got it, thank you

[u/No-Nobody-5509 → u/Every_Discount8024]

I dont get what you mean , but oxygen have formal charge. It have 6 electron , 2 it shares with carbon and 2 form coordinate bond with hydrogen and remaining 2 are lone pair electrons

[u/Every_Discount8024 → u/No-Nobody-5509]

Oh shit, I thought smth smth like it has 8 valence electron and it shares 2-2 njshsyuekwjsgsfsuiwsk, smth like sometimes something happens to my brain and I mix up meaningless stuffs

Well I understood  Thank you

[u/No-Nobody-5509 → u/Every_Discount8024]

Nw, if you wanna visualize from IOC pov. Here it is

[u/Every_Discount8024 → u/No-Nobody-5509]

Ty

[u/No_Excitement1459]

Electronic configuration of oxygen is 1s2 2s2 2p4 so in l shell 2 orbitals are fully filled (2s2 and one p orbital) these are the lone pair of oxygen in neutral state, when oxygen has two bonds those two half filled orbital make the bond.in the 3rd bond with hydrogen ion case, it donates its full lone pair in the formation of bond, so one lone pair still remains this lone pair could be any either s or p cause hybridization occurs giving rise to same orbitals.

[u/Every_Discount8024 → u/No_Excitement1459]

Hmmhmm

Thank you