The oxidation no of phosphorus is +3 and that of chlorine is -1.
Phosphorus = +5
Chlorine = -1
-2 oxidation state
PCl5 Phosphorous pentachlorideP for Phosphorous and 5 Cl for chloride= PCl5 College Chemistry student
Mg = +2 oxidation state P = +5 oxidation state O = -2 oxidation state
O = -2 oxidation state P = +5 oxidation state
-2 oxidation state
+5 oxidation state
The oxidation state of phosphorous in PCl5 is +5.The valence shell has 5 electrons.It therefore cannot increase its oxidation state more than 5.Therefore PCl5 cannot act as a reducing agent as it cannot donate electrons.The oxidation state can be decreased to +3 by gaining electrons. There for PCl5 can act as a oxidizing agent.A example is given below along with the change in oxidation states of phosphorous.
Phosphorus in PCl5 Nitrogen in Nitrate (NO3-) ion
Phosphorous, or P, has a zero oxidation number in the element. Common oxidation numbers are:- It has a -3 in phosphides, where it forms the P3- ion It has a +3 in oxidation number in for example P4O6, and PCl3 It has a +5 oxidation number in for example P4O10 and PCl5
phosphorus as well as the PIII oxidation state has an oxidation state of PV. Its the +5 oxidation state we need to bond 4 chlorines to phosphorus. So we also need another monovalent atom e.g. a halogen to balance up the oxidation state. One possibility for a neutral compound would be a mixed halide e.g. FPCl4 This compound is known and is usually called phosphorus tetrachloride fluoride. A cheeky answer would be PCl5 it has four chlorine atoms too!
ionic, [PCl4]+ [PCl6]-
-2 oxidation state
PCl5 Phosphorous pentachlorideP for Phosphorous and 5 Cl for chloride= PCl5 College Chemistry student
K = +1 oxidation state Cl = +3 oxidation state O = -2 oxidation state
Fe = +3 oxidation state Cl = -1 oxidation state
O = -2 oxidation state H = +1 oxidation state
Mg = +2 oxidation state P = +5 oxidation state O = -2 oxidation state