the basis of oxidation number considerations, one of the following oxides would not react with molecular oxygen: NO, N2O, SO2, SO3, P4O6. Which one is it? Why?
SO3 will not react because O2 always exist in pairs that means SO3 wil not have excess electrons to oxidise
To determine which oxide would not react with molecular oxygen based on oxidation number considerations, we need to examine the oxidation state of the central atom in each compound.
Let's go through each oxide:
1. NO (nitric oxide): Nitrogen has an oxidation state of +2 in this compound. Since nitrogen already has a positive oxidation state, it can further oxidize to a higher oxidation state (+4) upon reaction with molecular oxygen.
2. N2O (nitrous oxide): Nitrogen atoms in N2O have an oxidation state of +1. Similarly, it can further oxidize to a higher oxidation state (+4 and +5) upon reaction with molecular oxygen.
3. SO2 (sulfur dioxide): The oxidation state of sulfur in SO2 is +4. Sulfur can further oxidize to a higher oxidation state (+6) upon reaction with molecular oxygen.
4. SO3 (sulfur trioxide): The oxidation state of sulfur in SO3 is +6. Since sulfur is already in its highest possible oxidation state, it cannot undergo further oxidation upon reaction with molecular oxygen.
5. P4O6 (phosphorus hexoxide): The oxidation state of phosphorus in P4O6 is +3. Phosphorus can oxidize to higher oxidation states (+4 and +5) upon reaction with molecular oxygen.
Therefore, the oxide that would not react with molecular oxygen based on oxidation number considerations is SO3, as sulfur is already in its highest oxidation state of +6, and it cannot further oxidize upon reaction with molecular oxygen.
To determine which one of the given oxides would not react with molecular oxygen based on oxidation number considerations, we need to analyze the oxidation states of the elements involved in each compound.
Here is the step-by-step explanation:
1. Recall that the oxidation number is a positive or negative charge assigned to an atom within a compound to indicate its electron distribution.
2. In each oxide, we know that oxygen always has an oxidation number of -2 since it is highly electronegative.
3. For NO, we can assign x as the oxidation number of nitrogen. Given that NO is a neutral compound, the sum of the oxidation numbers must equal zero. Hence, we have: x + (-2) = 0. Solving for x, we find that nitrogen has an oxidation number of +2 in NO.
4. For N2O, let's assign x as the oxidation number of nitrogen. Considering that the sum of the oxidation numbers must be zero, we have: 2x + (-2) = 0. Solving for x, we find that nitrogen has an oxidation number of +1 in N2O.
5. In SO2, sulfur's oxidation number is often +4, and oxygen's oxidation number is -2. Therefore, assigning x as sulfur's oxidation number, we get: x + 2(-2) = 0. Solving for x, sulfur has an oxidation number of +4 in SO2.
6. Finally, let's analyze SO3. Assuming x as sulfur's oxidation number, the equation becomes: x + 3(-2) = 0. Solving for x, sulfur has an oxidation number of +6 in SO3.
7. Regarding P4O6, it is composed of a polyatomic ion called phosphate (PO4) with an overall charge of -2. We divide this charge equally among the four phosphorus atoms, which makes the oxidation number of each phosphorus +5/3.
Based on the obtained oxidation numbers, the compound that would not react with molecular oxygen is N2O. This is because nitrogen in N2O has an oxidation number of +1, which suggests that it is already partially oxidized and does not have available electrons to react further with oxygen.
In conclusion, N2O is the oxide that would not react with molecular oxygen based on oxidation number considerations.