Oxidation Numbers

The oxidation number of sulfur (S) in S2O3 is +2. This is because oxygen always has an oxidation number of -2, and since there are three oxygen atoms in S2O3, the total oxidation number of oxygen will be -6. The sum of the oxidation numbers in the compound must equal zero, so the oxidation number of sulfur is +2.

1. The oxidation number of an atom in its elemental form is 0.
2. In a compound, the sum of oxidation numbers must equal the overall charge of the compound.
3. In a polyatomic ion, the sum of oxidation numbers must equal the charge of the ion.
4. Some elements have fixed oxidation numbers (e.g., alkali metals +1, alkaline earth metals +2).

Rb has an oxidation number of +1, Cl has an oxidation number of -1, and O has an oxidation number of -2 based on common rules. Therefore, the oxidation number for RbClO would be +1 for Rb, -1 for Cl, and -2 for O.

The oxidation number for Ni in NiO2 is +4. Nickel is known to have variable oxidation states, and in this compound, it is bonded to two oxygen atoms which have an oxidation number of -2 each. The overall charge of the compound is neutral.

The oxidation number of chlorine in the compound PbCl is -1. Lead (Pb) has an oxidation number of +2, so the overall charge of the compound is neutral. Chlorine typically has an oxidation number of -1 in binary compounds.

The oxidation number of B in B4O7 is +3. This can be determined by assigning oxygen an oxidation number of -2, then setting up an equation to solve for the oxidation number of B.

+1 for each H

-2 for each O

+4 for each S

The oxidation number of O in any elemental form (e.g. O2, O3) is zero. Typically in chemical compounds the oxidation number of O is -2 (oxide ion)

Hydrogen has -1 and +1 oxidation numbers.

Other elements have +1 only

The sum of the oxidation numbers of all the atoms in C6H5CHO is equal to zero. This is because in a neutral molecule like C6H5CHO, the total oxidation number must balance out to zero.

In the compound NO, nitrogen (N) has an oxidation number of +2 and oxygen (O) has an oxidation number of -2. This is because oxygen usually has an oxidation number of -2 in compounds, and since NO is a neutral molecule, the oxidation numbers must balance out to zero.

The oxidation number of iron (Fe) in FeBr3 is +3. This is because each bromine atom (Br) has an oxidation number of -1, and since there are three bromine atoms in FeBr3, the overall charge must be balanced by a +3 charge on the iron atom.

In chromium(III) oxide, the oxidation number of chromium is +3 and the oxidation number of oxygen is -2. This compound has the chemical formula Cr2O3.

The oxidation number of Se in K2SeO4 is +6. This is determined by considering the oxidation numbers of K(+1) and O(-2) in the compound and using the overall charge of the compound (zero) to calculate the oxidation number of Se.

The oxidation number of zinc increasing by 2 indicates that zinc is being oxidized. This means it is losing electrons during the reaction.

The oxidation numbers of halogens can vary because they have seven valence electrons, making it possible for them to gain or lose different numbers of electrons to attain a stable electron configuration. This flexibility allows halogens to exhibit a range of oxidation states in chemical compounds, such as -1, +1, +3, +5, +7.

Vanadium is an element that commonly exhibits an oxidation state of +5.

To find the oxidation number of phosphorus in phosphate (PO4), consider that oxygen typically has an oxidation number of -2. Since there are four oxygen atoms in phosphate, their total charge is -8. The overall charge of the phosphate ion is -3, so the oxidation number of phosphorus can be calculated as +5 to balance the charges.

The increase in oxidation number indicates loss of electrons, while a decrease indicates gain of electrons. For example, if an atom's oxidation number increases from +2 to +4 in a reaction, it has lost two electrons. Conversely, if the oxidation number decreases from +4 to +2, it has gained two electrons.

The oxidation number of the ion is -1. Oxygen atoms have -2 oxidation number each. Nitrogen's oxidation number is +3: 4 covalent bonds with oxygen yields +4 and the central negative charge yields -1.

The sum of oxidation numbers in a compound is zero. In Sb2O5, oxygen typically has an oxidation number of -2. By setting up the equation: 2x + 5(-2) = 0, solving for x gives the oxidation number of Sb as +5.

Nitrogen is more electronegative than Hydrogen.

So +1 for each hydrogen and -3 for nitrogen

In SO3, sulfur has an oxidation number of +6 and each oxygen atom has an oxidation number of -2. The sum of the oxidation numbers must equal the overall charge of the molecule, which in this case is 0.

In SO3, sulfur has an oxidation number of +6 and each oxygen atom has an oxidation number of -2.

Carbon has an oxidation number of -4 in compounds like methane (CH4) or other similar hydrides. This occurs because carbon is more electronegative than hydrogen, causing it to attract the electrons and have a partial negative charge.