Complex Ion Formation 

yeah this one was a bit throwaway, i made it years ago for a company and the exclusivity clause ran out so i decided to post it, but i'll do more like it soon.

@@ProfessorDaveExplains thank you. Waiting for more:)

@@ProfessorDaveExplains thanks

Yeah yeah I agree! Please tell your friends!

Almost there now

thank you Chemistry Jesus lol

i'm going to do a few on that this year!

NH3 is a neutral molecule, the lone pairs do not add extra charge. It has the same number of protons and electrons overall, so it is neutral. Ag ion has +1 charge. So when you combine a +1 charged ion with 2 neutral molecules, you'd end up with +1 charged complex ion. Remember, charges must be balanced on each side of the equation. Ag^+ + 2NH3 --> Ag(NH3)2 ^+

​@@dr.oztekchemistrychannel9668 I don't understand why 2NH3? why not 4NH3 or any number? how to determine this number?

@@crieliocriel the number of ligands surrounding a metal ion in a complex is dependent on the SIZE of the central metal ion AND also the SIZE of the ligands around it. In this case, silver Ag+ ion is a very big ion (in second row of transition elements/d block or period 5). So it can ONLY fit two ligands around it forming a linear complex [Ag(NH3)2]+. Most complex ions can fit 6 or 4 (monodentate) ligands eg H20, NH3, Cl-, around their central metal ion. Silver is exception due to its large size. Also When you add chloride ions to a solution of copper ions, there is a change in coordination number from 6 to 4 since Cl- ions are bigger than H20 molecules so can only fit 4Cl- ions around the central metal ion : [Cu(H20)]2+ + 4Cl- = [CuCl4]2- + 6H20. In this case, the change in shape of complex/coordination number is caused by change in SIZE of surrounding ligands in complex ion.

Just keep putting out as much content as I can! Also I have a book coming out.

@@ProfessorDaveExplains Oh wow! which genre book? Science-related or something else?

Social commentary about public science literacy! I'll make a formal announcement on the channel.

nope they are coordinate covalent bonds

sorry i don't really tutor anymore!

No I'm just very busy with the channel and other projects.

yes and also the identity of the metal cation

Professor Dave Explains I see. Do transition metals behave similarly? Is copper unique in any way?

they all have their own properties!

Professor Dave Explains ok thank you

no it's not the size of the ligand it's how you use it

but dissolution is always entropically favorable, so if something is insoluble, enthalpy must be the reason

@@ProfessorDaveExplains Hi Dave :) I find it necessary to add to the discussion that dissolution is not always entropically favorable. This may make an exothermic dissolution process nonspontaneous, if the TΔS term is larger than the ΔH term.For example compounds that contain ions with large magnitude of charge, such as aluminum chloride, have negative entropy of solution (-250 J/mol.K). The highly charged ions immobilize water molecules more than ions with low charges would. So although the ionic compound experiences an increase in entropy, the solvent experiences a larger decrease in entropy, and the overall process will have ΔS

interesting i was not aware!

correct me if i am wrong... if + the ligand will be 2.. if 2+ the ligand will be 4.. and so on??

@Khush Bakht Khan hahaha

i already got it though..

Give this guy a Nobel prize

@@tyrekeholness1687 hey really???

What's the Indian channel

Why the hate?