Question

The oxidation state of a transition metal can be determined by looking at the ligands bonded to the metal. Every bond to a transitie by +1. For example in CoBry, there are two bromines bonded to the cobalt, and the cobalt will have a +2 oxidation state (Co?"). W to the metal, they do not change the oxidation state of the metal. For example the palladium in Pd(PP), has an oxidation state Determine the oxidation state of the metal in each of the following. NaO P(tu) Pd(OAc)2 1)---NH2 - Pd(OAC)2 Pd R-N---Pd NaO PitBug b CODE

Answer 1

# Let the oxidation state of Pb ben. a) pdcoAo - n+ 2(-1) = 0 = x -2=0 (2= +2 Note Chy cooo is a negative tigand. b). ona T - Pd COAC. ed coach NHL > With NZONA J2 Since the ligand is neutral therefore the oxidation state of Pd would remain +2. I - N+2(-1) + 2(0) = 0 & The bulky ligand is? Caneutel U lisand 21=+2) c) (tau) p....pd...... p lt Bu, The Phosphorous or phosphonium ligands are nackalı - pd (2x x + 2(o)=0 Hence, oxidation state of (Pd is zero ph R-NH...... pd N+(+)+(-1)=0 = (2=+2 Here Br is a negative ligand and this also negative as Carbon has donatio eletrons to Pd and N4 is a neutral ligand