Oxidation Numbers

The oxidation of any element, by itself, is zero.

The oxidation number of an atom states how it shares its valence electrons with other elements (or ions or compounds). A neutral atom always has its oxidation number 0: it does not share any electrons. A cation has a positive oxidation number and that of anion is negative because they donate and attract electrons respectively.

The Oxidation number for Kr which is krypton is 2. The Oxidation number for Kr which is krypton is 2. The Oxidation number for Kr which is krypton is 2.

The oxidation number of KF is +1 for potassium (K) and -1 for fluorine (F). This is because alkali metals like potassium typically have an oxidation state of +1, while halogens like fluorine have an oxidation state of -1 in ionic compounds.

Element Phosphorus has an oxidation state of -4.

No element has oxidation state of +4.

Phosphorus is denoted by "P".

The oxidation state of Hydrogen in the hydronium ion is 1+ and the oxidation state of oxygen is 2-

The oxidation number of Fe in Fe2S3 is +3. This is because the overall charge of the Fe2S3 compound is 0, and since there are 2 Fe atoms each with an unknown oxidation number "x" and 3 S atoms each with an oxidation number of -2, the sum of the oxidation numbers must equal 0. Solving for x gives +3 for the oxidation number of Fe.

In per chloric acid HClO4, the oxidation number of chlorine is +7.

+3 for Cr and -2 for O

The oxidation number of xenon can vary depending on the compound it is in. Xenon typically has an oxidation number of 0 in elemental form (Xe), but it can also have oxidation numbers of +2, +4, +6, or +8 in different compounds.

The oxidation number of mercury (Hg) can vary depending on the compound it is in. For example, in elemental form or in compounds where it is not bound to other elements, the oxidation number of Hg is 0. In compounds like HgCl2, where it is bonded to other atoms, its oxidation number is usually +2.

+1 for H

-1 for I

The oxidation number of arsenic (As) in As₂O₅ is +5. Oxygen typically has an oxidation number of -2, so by using the overall charge of the compound being 0, the oxidation number of arsenic in this case can be determined as +5.

The oxidation number for H is +1, and the oxidation number for O is -1.

The correct chemical formula should be P2O5 or P4O10 (its dimer) and not P3O10 (as originally asked in the question).

The oxidation numbers are

-2 for each O

+5 for each P

Oxygen forms a -2 ion.

x0 - x= +2.

The compound overall needs to be neutral, so you add up all the charges from the oxygen and add whatever you need to make it neutral.

eg:

FeO - oxidation state of iron = +2, since oxygen forms -2 and compound is overall neutral.

Fe2O3 - -6 from the oxygen. So you need to add +3, and there are two Fe's so you divide it by two - therefore iron is +3.

Hope that helps.

In N2O3, the oxidation state of nitrogen is +3 because oxygen is usually assigned an oxidation state of -2, and there are three oxygen atoms in N2O3. The sum of the oxidation states in a neutral compound should be zero, so the oxidation state of nitrogen must be +3 in order to balance the -6 from the three oxygen atoms.

The oxidation number of Cr in Cr2O7^2- ion is +6. Each oxygen atom has a -2 charge, and the overall charge of the ion is 2-, so combining the charges gives -2*(-7) = -14. Since the overall charge is 2-, the oxidation number of Cr must be +6 to balance the charges.

In Rb₂SO₃, rubidium (Rb) has an oxidation number of +1 and oxygen (O) has an oxidation number of -2. Since it is a neutral compound, the sum of the oxidation numbers must equal zero. Therefore, sulfur (S) in this case has an oxidation number of +4.

The oxidation number of Br in ZnBr2 is -1. In ZnBr2, zinc (Zn) has an oxidation number of +2, so the two bromine (Br) atoms each have an oxidation number of -1 to balance the charge of the compound.

In Li2Co3, lithium has an oxidation number of +1, oxygen has an oxidation number of -2, and cobalt's oxidation number can be calculated as +3 to balance the overall charge of the compound, which is zero.

The oxidation number of chromium in CrBr2 is +2. This is because bromine typically has an oxidation number of -1 and there are two bromine atoms in CrBr2, leading to a total oxidation number of -2. The oxidation number of chromium must therefore be +2 to balance the charges.

The oxidation number of carbon is +4 in CCl4. Each chlorine atom has an oxidation number of -1, and since there are 4 chlorine atoms bonded to carbon, the total oxidation number must equal 0 for a neutral molecule.

The oxidation number of nitrogen in N2H5Cl is -2. This is because hydrogen is usually assigned an oxidation number of +1 and chlorine is usually assigned an oxidation number of -1. Therefore, the total oxidation numbers must add up to 0 since the compound is neutral.