There are a number of rules for calculating oxidation numbers.

The oxidation number of an element is equal to its combining power with oxygen.

Note that fractional oxidation numbers should not be used in naming.

The oxidation number on all atoms in such a reaction remains unchanged.

This is proved by the oxidation number of +2 for the oxygen atom.

The properties of the atoms involved can be understood using concepts such as oxidation number.

All atoms of free elements have an oxidation number of 0.

In disulfide, sulfur is only reduced to a state with oxidation number 1.

Valencies sometimes have the same numerical values as oxidation numbers - but not always.

Iron (Fe) has been oxidized because the oxidation number increased.

The oxidation number of the most common chalcogen compounds with positive metals is 2.

Other oxidation numbers, such as 1 in pyrite and peroxide, do occur.

When the metal has more than one possible ionic charge or oxidation number the name becomes ambiguous.

Phosphorus has an oxidation number of -3 in phosphine.

Table 4.23 compares the valency and oxidation numbers of carbon in five compounds.

It is a strong oxidizing agent as the osmium has an oxidation number of +8.

In most of its compounds, Gallium is found with an oxidation number of 3+.

It may also be helpful to indicate the oxidation number of a metal cation, where appropriate.

Assign oxidation numbers for each atom in the following compounds:

Note in some cases the oxidation number of the metal is give [e.g.

It shows reluctance to acquire "the high positive oxidation numbers characteristic of nonmetals".

Sulfur is usually assigned to the reduced oxidation number 2, described as S and called sulfide.

Elements in both ionic and covalent compounds can have oxidation numbers.

The sum of the oxidation numbers of the elements in a compound is zero.

Superoxides are compounds in which the oxidation number of oxygen is .

Most common are those in the 2+ oxidation state, as illustrated below.

Many elements can exist in more than one oxidation state.

Chemistry in the 0 oxidation state is far more limited.

As such, it almost always assumes the oxidation state +3.

It is composed of lead in its +4 oxidation state.

For each oxidation state use the parameters from the table shown below.

The status of the +1 oxidation state is still tentative.

The oxidation state of the metal is important in the reactions.

All elements in their standard form have the oxidation state zero.

These can most easily occur when the metal is in a high oxidation state.

The plutonium at this point is in the +4 oxidation state.

This is the definition in the current gold book for "oxidation state".

Most of the silver compounds are in the +1 oxidation state.

These chemical compounds are only in one oxidation state: +2.

For the most stable complex the metal is in oxidation state 0 or +1.

Most of them have more than one oxidation state.

The oxidation state of the iron atom changes between the +2 and +3 states.

A few of these are known to have yttrium in the oxidation state 0.

Often the technique is used to determine the oxidation state of iron.

Elements, even in molecular form, always have an oxidation state of zero.

The oxidation state of sulfur in this compound is +6.

Simple functional groups can be arranged in order of increasing oxidation state.

In this compound magnesium has an oxidation state of 2.

Elements in a high oxidation state can have a valence higher than four.