Organometallic Chemistry Basics I: The 18 Electron Rule 

The titanium atom doesn't have a charge of 0; contributes 0 electrons. Titanium is a d4 metal; the 2 cyclopentadienyl (Cp) and 2 chlorine (Cl) ligands are all anionic, and thus influence the oxidation state of the titanium from d4 to d0, which is why it only contributes 0 electrons.

There are plenty of organometallic platinum species. A very famous example is Zeise's salt, which features a platinum bonded to ethene. While platinum metal is generally unreactive (I'm assuming that's what you mean by 'strong'), you can get it to react. You just have to use some forcing conditions.

CO is a neural ligand if we were to remove it, it would be neural CO

The number of electrons should be 16, because this is a square planar structure. Octahedral complexes usually contain 18 electrons, but these numbers can vary from time to time depending on the ligands, such as with olefins. He did count the Cl electrons; he write 2(Cl-) = 4 e's.

d7 is representing the number of valence e-

When transition metals are bonded the 3d orbitals get occupied first, the 3d orbital becomes lower in energy than the 4s.

@@jakesmith6544 I'm studying for a test and bewildered by this because I haven't come across it in my lecture notes.

he made a little mistake, its supposed to be Pb not Pd

Thank you for your comment - I couldn't understand why he would call Palladium a p-block element.

Me tooo 😂