+5
The oxidation state of K in K2O2 is +1. In this compound, each K atom has a +1 oxidation state and each O atom has a -1 oxidation state.
In molybdenum disulfide (MoS2), molybdenum typically has an oxidation state of +4, and sulfur has an oxidation state of -2. Each Mo atom contributes a +4 oxidation state, while each S atom contributes a -2 oxidation state, which balances the overall charge of the compound.
If you mean SO3^-2 (the sulfite anion), then S has an oxidation number of 4+, since each O atom is 2-. In sulfur trioxide, SO3, the S atom has an oxidation number of 6+.
In silver sulfide (Ag2S), each silver (Ag) atom has an oxidation state of +1, and each sulfur (S) atom has an oxidation state of -2. This arrangement balances out the charges to form a neutral compound.
The oxidation state of sulfur in SO2Cl2 is +4. In this molecule, each oxygen atom has an oxidation state of -2, each chlorine atom has an oxidation state of -1, and the overall charge of the molecule is 0, which means the oxidation state of sulfur must be +4 to balance the charges.
The oxidation state of K in K2O2 is +1. In this compound, each K atom has a +1 oxidation state and each O atom has a -1 oxidation state.
In molybdenum disulfide (MoS2), molybdenum typically has an oxidation state of +4, and sulfur has an oxidation state of -2. Each Mo atom contributes a +4 oxidation state, while each S atom contributes a -2 oxidation state, which balances the overall charge of the compound.
If you mean SO3^-2 (the sulfite anion), then S has an oxidation number of 4+, since each O atom is 2-. In sulfur trioxide, SO3, the S atom has an oxidation number of 6+.
The sulfate ion is SO42 -. The oxidation state of the sulfur is +6 (work it out!); therefore, the ion is more properly named the sulfate(VI) ion. The sulfite ion is SO32-. The oxidation state of the sulfur is +4.
In silver sulfide (Ag2S), each silver (Ag) atom has an oxidation state of +1, and each sulfur (S) atom has an oxidation state of -2. This arrangement balances out the charges to form a neutral compound.
The oxidation state of sulfur in SO2Cl2 is +4. In this molecule, each oxygen atom has an oxidation state of -2, each chlorine atom has an oxidation state of -1, and the overall charge of the molecule is 0, which means the oxidation state of sulfur must be +4 to balance the charges.
With a few exceptions that do not apply to this formula, oxygen is always assigned a formal oxidation number of -2 per atom, and hydrogen is assigned +1 per atom. The compound as a whole must always be electrically neutral. Therefore, in this molecule, the oxidation number of the single sulfur atom must be -[-2(4) +2] or +6.
The oxidation state for sulfur (S) in SO3 is +6. Each oxygen atom in SO3 has an oxidation state of -2, and since the overall molecule is neutral, the sum of the oxidation states must equal zero. Therefore, sulfur must have an oxidation state of +6 to balance the -6 from the three oxygen atoms.
The oxidation number of S in HSO3- is +4. This is determined by assigning a -1 oxidation state to the hydrogen atom and a -2 oxidation state to the oxygen atoms, which leaves sulfur with a +4 oxidation state to balance the overall charge of -1 for the ion.
The oxidation number of Sulfur (S) in Na2S2O3 is +2. This is because the overall charge of the compound is zero, and since each Sodium (Na) atom has an oxidation state of +1, the oxidation state of Sulfur must be +2 to balance the charges in the compound.
The oxidation state of S in SO42- is +6. Each oxygen atom has an oxidation state of -2, so the total charge of -2 for sulfate ion requires sulfur to have an oxidation state of +6 to balance the charge.
S = +4 oxidation state O = -2 oxidation state