Determine the oxidation number of the elements underline in the following ions or compounds.
a) PF3:Ox.# P=
B)S2O3: Ox.#S=
What do you not understand about how to do this? Here are the rules.
http://www.chemteam.info/Redox/Redox-Rules.html
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To determine the oxidation numbers of the elements in ions or compounds, you need to follow a set of rules:
1. The oxidation number of an element in its pure elemental form is always 0. For example, the oxidation number of sulfur (S) in S8 is 0.
2. The sum of all oxidation numbers in a neutral compound is always 0. For example, in PF3, the total sum of the oxidation numbers of the elements must be 0 because it is a neutral compound.
Now let's determine the oxidation number for each element:
a) PF3:
Since the compound is neutral, the sum of the oxidation numbers must be 0.
Let x be the oxidation number of phosphorus (P).
Thus, the oxidation number of each fluorine (F) atom must be -1, as it is a halogen.
The compound PF₃ contains three fluorine atoms, so the total oxidation number contributed by the fluorine atoms is -3.
Therefore, the sum of the oxidation numbers should be equal to zero:
x + (-3) = 0
Solving for x:
x = +3
So, the oxidation number of phosphorus (P) in PF3 is +3.
b) S2O3:
Similarly, the compound is neutral, so the sum of the oxidation numbers must be 0.
Let x be the oxidation number of sulfur (S).
Each oxygen atom (O) is assigned an oxidation number of -2, except in peroxides (-1) or when bonded to fluorine (+2).
The compound S₂O₃ contains three oxygen atoms, totaling -6 in oxidation number.
Therefore, the sum of the oxidation numbers should be equal to zero:
2x + (-6) = 0
Solving for x:
2x = 6
x = +3
So, the oxidation number of sulfur (S) in S2O3 is +3.