Footnotes: reference "Nomenclature of Inorganic Chemistry: IUPAC Recommendations 2005" (Red Book)
(1) Historically, coordination compounds were considered to be formed by adding independently stable compounds to a simple central atom or ion.
Naming of these coordination compounds was therefore based on an additive principle whereby the names of added compounds and the central atom were combined.
In this tutorial we will name the complex ion using the oxidation state for the central metal atom.
This form of additive nomenclature has been in use for a very long time, but it has problems, notably it may not accurately reflect the distribution of electrons within the complex ion.
There are other, arguably better, systematic IUPAC ways to name a complex ion, for example, you could name the complex ion as an ion (see Naming cations and Naming Anions) in which case you enclose the charge on the ion in round brackets after the additive name (no need to try to determine the oxidation state of the metal and hence removes the problem of electron distribution).
(2) Previously, anionic ligands were named by removal of "ide" and replacement by "o", for example chloride became chloro, and, removal of "ate" and replacement with "o" for example sulfate became sulfo.
Note the changes: final "e" is removed and replaced by "o", chloride becomes chlorido and sulfate becomes sulfato.
Also note that hydride becomes hydrido when coordinating to all elements EXCEPT boron.
Coordinated cyanide is also named cyanido.
(3) The names of cationic ligands are also used without modification, even if the name ends in "ide", "ate" or "ite".
Note the change of name when water is a ligand from the previous "aquo" to the new "aqua".
(4) This is true for the names of simple ligands. For complex ligand names, the prefixes bis, tris, tetrakis etc are used with enclosing marks around the multiplicand in order to aviod ambiguity.
(5) If the metal has a negative oxidation state, then a minus sign is written to the left of the Roman numeral indicating its oxidation state, eg, Fe(-II)
If the oxidation state is zero, then an arabic 0 is placed in parentheses.
(6) If more than one type of ligand is present, the ligands are named in alphabetical order (disregard any multiplicative prefixes when determining that order),
eg, [CoCl(NH3)5]Cl2 is pentaaminechloridocobalt(2+) chloride.
(7) If more than one type of ligand is present, the symbols are given in alphabetical order, eg, if Cl- and NH3 both occur as ligands in the same coordination compound, then, because C occurs before N in the alphabet, so we write [CrCl2(NH3)4]+
Note that the ligand CO preceded the Cl ligand because single letter symbols preceded two letter symbols.
Note the change: previously we wrote the symbols for anionic ligands before the symbols for neutral ligands.
(8) This is NOT an exhaustive list of shapes, but these are the ones you are most likely to encounter in an introductory inorganic chemistry course.