Complex Ions, Ligands, & Coordination Compounds, Basic Introduction Chemistry

This chemistry video tutorial provides a basic introduction into complex ions, ligands, and coordination compounds. A complex ion typically consist of a transition metal cation bounded to ligands which can be neutral molecules or ions. The number of ligands attached to the transition metal ion is known as the coordination number. This video explains how to determine the oxidation state of the transition metal ion in a complex ion and within a coordination compound. A coordination compound consist of a complex ion and a counterion. The counterion may be a cation or an anion. This video briefly discusses werner's theory of coordination compounds and the concept of primary valence and secondary valence as it relates to the transition metal ions in complex ions.
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[@TheOrganicChemistryTutor]

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[@huzbinaru]

In most part of the video, you kept saying that coordination number is the number of ligands attached but it's somewhat an incorrect definition, y'know. Coordination number depends on the number of dative bonds central metal ion is attached to, so let's say if a hexadentate ligand (a molecule or ion that can form six dative bonds) attaches itself with a transition metal ion, it's coordination number will be six depending on what I said and would be one from what you have explained, which would be wrong.

[@user-ow4zi1sv6n]

This is what I couldn’t understand in class. Thanks soo much

[@antham8112]

at 11:52, shouldn't you have bracketed the (CN) at the top so it looks like (CN)3? otherwise it looks like 1 carbon and 3 nitrogens.

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[@nasserBack]

Do u have anything on Fac-mer isomers? They are in the same chapter as this one. Thanks

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This is also a great recap video

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[@sofiahassan5572]

do we have to memorise the coordination number of each ion? I don't get how he got them from 6:55. Someone please help

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[@ahmedsarker3555]

1:25 how do you know whether the compound is ligand just by looking at the equation.....also sir for 8:05 as the charge increases, isn't the coordination number generally decreasing? for 10:07 why did you have to draw zinc when carbon is already bonded with two oxygen atoms [or ions].......11:42 i do not see chromium having 3 atoms of it

[@rwayle]

Ligands are the groups bonded to the metal ion, so in Zn(H2O)6 2+ there are 6 H2O ligands bonded to Zn 2+ For coordination number you need to look at that data again. But it's only a general rule, you'll find transition metals form many different complexes. He's drawing the bonds between the oxalate ion and the zinc metal... He didn't say there's 3 atoms of Cr, look at the formula, he's saying it has a +3 charge because of the 3 x CN- counter ions. Based on your questions I think you should watch this one again and maybe check out some other transition metal videos too.

[@grandpasuho]

how do i tell when to use a tetrahedral or a square planar since those are the two options for a coordination number of 4?

[@doonyah.3959]

I thought there's no lone pairs for the tetrahedral complex, but I'm probably wrong.

[@louisg7062]

depends of the ligand structure i think.

[@ximelp7268]

It depends on how many clouds of lone electrons (electrons that aren't participating in bonds) there are. When looking at the molecular geometry is really important to count ALL electron clouds. There are two types of these, the electrons that are participating in bonding and the lone pairs of electrons. A molecule or compound that has tetrahedral geometry has 4 electron clouds, all participating in bonding. Since all the four bonds are identical it forms a tetrahedron which is the shape that allows for all bonds to be the same. A molecule that has square planar geometry does NOT have 4 electron clouds. In fact, it has 6 electron clouds, four of them participating in bonding and the other two are lone pair of electrons. The lone pairs have the most steric hindrance out of all the electron clouds. Because of this, the lone pairs of electrons positions themselves exactly above and below the molecule and the 4 remaining bonds have to position themselves on the "equator" of the molecule. This makes the four bonds form a square in the middle of the molecule and this is what we see. Hope this helps.

[@sunnywinker1805]

fruitloops It depends on how many lone pairs are on the metal

[@aminad1938]

If it’s sp3 (or d3s) => tetrahedral. If it’s dsp2 => sqare planar. You basically need to do the hybridation of the metal

[@zero-one3599]

u just saved me a lot of time......tyvm...so good explanation

[@mddulumia9206]

Sir,pls tell me that, how can I identify the situation of the ligand in complex compound??? Is it cation ,anion or neutral???

[@amirhamzah9332]

You have to add the charges from each ion, if total charge is +ve, cation, if -ve, anion and if total charge 0, it is neutral

[@millermason2068]

Thank you for doing all your videos with a black background

[@jiahan4492]

having final tomorrow and finally know what is going on in my chemistry class

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Thank you for an excellent presentation!

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LOVED THIS THOUGH ! THANKYOU

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i swear to god that u are better than my school teacher and tuition teacher

[@sabahmunir2851]

hey! when you talk about bidentates, you use zinc ion as an example. Zinc ion can not form a complex ion as it has a complete 3-d orbital....

[@mithiahmed3335]

But zinc is not a transition metal, but why do we calculate the coordination number in this case.

[@amnanavid]

Zinc IS a transition metal it is just ‘non-typical’ transition metal

[@mithiahmed3335]

@@amnanavid well, in our book, the definition is given that any d block metal that forms any ion which has 1-9 e- in its d orbital. but Zn doesn't seem to comply to that,so I said so

[@tremeramcbean3719]

Great video thank you! I have a quiz on Wednesday so I'm trying to get ahead on studying.

[@saliasuale3523]

So well explained. Do you have any videos on Ligand Field Theory?

[@thisismychild.7753]

I might not have time to look at the video right now (will do later) but I was wondering why the metal within complex ions was drawn with dashed bonds and the ligants still had their electron pairs draw right between the bond and the atom? Is it related to resonance form in any way or are the bonds just conventionally drawn that way? I have to ''discuss'' the metal's geometry in EDTA-Ca^2- for a lab report, it obviously looks like an octahedron but you never know.

[@thisismychild.7753]

Oh nevermind, it was just coordinate covalent bonds, I had no clue lol

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You sir are a legend. Thank you

[@HouseOfTrona]

OMG this is so good I understand it perfectly!

[@hasanmahmud6547]

why you donot use third bracket as it is complex !!!

[@cheimaachimikaa4984]

Sir, pls tell me that, how Can i determinat the number a in this complexe {Cu(NH3)a}2+ pls help me because i have a test !!!!!!

[@leonatomy]

Great explanations, thank you!!

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[@elizabetholabisi3847]

Please how do we calculate the overall charge of a coordination complex

[@anushmargaryan7788]

You are such a savior

[@ahmedhass146]

but what about the charge of the diamine silver cation at the beginning od the video can some one explain it to me please ??

[@SamFarr1]

The amine molecules are both neutral but each has a lone pair of electrons that interact. The silver ion in the complex has a 1+ charge, so because this charge is not balanced with a 1- charge, the overall complex charge remains 1+

[@faria93]

What is the name of [Fe(CN)6]3- please?

[@bennydalton8652]

Sir can you say when the NO3 acts as counter ion

[@collinsomurunga4811]

Nice work from you,,,, chemistry made easy

[@phyaunna1329]

Why can't the lone pairs of the other two oxygens interact ? (in the bidentate example)

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I’m gonna write this on all your videos I watch

[@steveh6612]

6:18 this is where i get a bit confused. What dictates Td or D4h shapes

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grateful for such amazing videos always

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Thank u sir for your beautifull explanation

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Great thanks

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Please do a video on activation complex

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thanks for the great job and please can you make a video for order of reactions??

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Thank you so much for the work done .

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[@tahsinnawar9847]

Can anyone kindly tell me the difference between complexation and chelation

[@russellanawan8116]

this is very helpful. thanks for the info

[@danielnorris4848]

coordination number is not the number of ligands but the number of coordinate bonds attached to the central metal ions. Bidentate ligands bind to the central ion twice and so coordinate number will increase by two for every bidentate ligand.

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[@antham8112]

Wouldn't the secondary valence be affected by what the charge of the ligands are? Wouldn't the Fe+3 sometimes for complexes with a different number of ligands, or is it always 6?

[@Vanlalmuanpuii]

🤣i have the same question ! Somebody answer plss

[@alicechromatica9125]

Primary valence only talks about oxidation state. Secondary valence only talks about coordination number. The charge of complex ion, in the video which is -3, does not depends on secondary valence. [Fe(CN)6]3- Primary valence: +3 Secondary valence: 6 Charge of ligand: -1 (because Fluorine needs 1 electron and once it receives, it becomes -1) To get the charge of complex ion: 1. Charge of ligand × Secondary valence So, -1 × 6 = -6 2. Product of number 1 + Charge of metal ion So, -6 + 3 = -3 This is why Fe(CN)6]3-.

[@Chelsea-gs7qj]

how did you know that the CN's each had a reacting charge of -1? what if you got the molecule [Cu(NH3)4]^2+? what is the charge of Cu?

[@YummyhenIsBeast]

charge is 2+ coz nh3 neutral. and CN just draw its structure lone pair on C: 5 bonds

[@fytonchem7945]

Thank you

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You are amazing.👌

[@paperinashes]

Is there a playlist for coordination chemistry?

[@21Bammy]

Thank you ❤

[@inathiinathi8683]

Can you please explain covalent bond classification (MLX classes )

[@ghadeerbadr7242]

THANK YOU!!!!! I'm so grateful..

[@Mattyalmighty]

how can Ag attached to 2 ligands since there's only 1 valence electron

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wishing you succeed.