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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[@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.

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[@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.

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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.

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

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

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