Oxidation Numbers

0 in elemental form

+1 in its compounds

+1 for H

-2 for each O

+5 for Sn

The charge. Cations and anions have an oxidation number equal to their charge, for example in Fe2+, Fe hasan oxidation number of +2 and in S2- S has an oxidation number of -2. Uncharged atoms have zero oxidation number.

Noble gases, such as helium, neon, argon, krypton, xenon, and radon, will never have a positive oxidation number. This is because they have a full outer electron shell, making them stable and unreactive.

The oxidation number of hydrogen is +1 when combined with nonmetals, and -1 when combined with metals.

Fe3O4 is a complex oxide (a crystaline solid containing more than one cation).

In this case Fe exists as both the 2+ and 3+ cation. There are two 3+ ions and one 2+ ion for every four O2- ions.

The charge balance is: 2x3+ + 2+ + 4x2- = 0

The oxidation number of Sodium in the Na + ion = 1

For the hydrogen atoms the oxidation state is 1+, for the oxygen it is 2-

In PbI2, lead (Pb) would have an oxidation number of +2, and iodine (I) would have an oxidation number of -1. This is because iodine typically has an oxidation number of -1 in ionic compounds, while lead usually has an oxidation number of +2.

Roman numeral following the name shows the ions charge. For example Fe(II) in a compound name means that the iron is present as Fe2+ and Fe(III) in a name means that it is present as Fe3+

The same convention is used for all metals that can have more than one charge, not just transition metals for example thallium (I) and thallium (III) (thallium is in group 13)

The oxidation number of NCS is -1. N has an oxidation number of -3, while S has an oxidation number of +6 in the NCS molecule.

The oxidation number of manganese in KMnO₄ is +7. Manganese has an oxidation number of +7 in this compound because oxygen has an oxidation number of -2, and the overall charge of the permanganate ion is -1, so the sum of the oxidation numbers must equal -1.

No: An oxidation number, if shown at all in a chemical formula, is shown with a superscript. The oxidation number is usually shown only for monatomic ions.

A positive oxidation number represents the charge an atom would have if electrons were transferred to the more electronegative atom in a compound. It signifies that the atom is losing electrons and becoming oxidized in a chemical reaction.

The sum of the oxidation numbers in a neutral compound is always zero. This is because the total positive charges from the oxidation numbers of the elements must balance out the total negative charges for a compound to be neutral.

Silver metal, Ag has an oxidation number of 0.

The most common oxidation state in compounds is +1 (as in AgCl)

There are compounds such as AgO where the oxidation number is not +1 which actually contains Ag with +1 and +3

The oxidation number of lithium is +1.

The oxidation number of chlorine can vary depending on the compound it is in. It can have an oxidation number of -1 in most compounds, but it can also have positive oxidation numbers in compounds like ClO4- where it has an oxidation number of +7.

The oxidation number of ammonium is 1+. The oxidation number of ammonium is 1+.

In general, oxidation is the loss of electrons and reduction is the gain of electons. When something is oxydized, the oxidation number will increase and when something is reduced the oxidation number will decrease. Oxidizing agent (oxidant) is a species which causes another to be oxidized. Reducing agent (reductant) is any species that causes another species to be reduced.

A common example of oxidation is when oxygen in water combines with an element in an object. When metal rusts it is usually caused by the oxygen in water combining with the metal (usually the iron in steel) to form iron oxide or some other "oxide".

When burning organic material such as wood the technical term for fire is "rapid oxidation", because what is happening is the oxygen atoms are breaking apart carbon atoms from their molecules and bonding with them (because oxygen and carbon bond more easily) and the chemical breaking and bonding is releasing enough heat energy to break more carbon loose, then it keeps bonding with the oxygen in the air to form carbon dioxide, carbon monoxide etc, "fueling the fire" until there is not enough heat to break up more carbon molecules, or there is no more oxygen for it to bind with, which is why putting a glass over a candle will put it out.

The oxidation in rust is the same thing, just with different elements and much too slow to give off noticable heat or sustain a chemical reaction.

Zn is a d block element. Oxidation number of it is +2.

H is +1, O3 is -6, that is -5

-5 and the total charge is -1 so a -4 has to be contributed by S

Bromine has an oxidation number of negative one, except when with oxygen or flourine.

Here are a few from a list I am compiling, some elements can have multiple charge types, which are notated with the Roman numerals, such as Cu (I) or Au (III):

+1 Charge [Lithium, Sodium, Potassium, Rubidium, Cesium, Copper (I), Silver, Francium, Gold (I), Gallium (I), Indium (I), Thallium (I), Hydrogen, Titanium (I), and Mercury (I)]

+2 Charge [Magnesium, Calcium, Strontium, Barium, Cadmium, Chromium (II), Cobalt (II), Copper (II), Iron (II), Lead (II), Manganese (II), Mercury (II), Nickel (II), Tin (II), Vanadium (II), and Zinc]

+3 Charge [Aluminum, Chromium (III), Iron (III), Vanadium (III), Yttrium, Scandium, Gallium (III), Indium (III), Thallium (III), Bismuth, Arsenic (III), Cerium (III), Cobalt (III), Gold (III), Titanium (III), Manganese (III)]

+4 Charge [Lead (IV), Vanadium (IV), Tin (IV), Cerium (IV), Titanium (IV), Germanium (IV)]

-1 Charge [Fluoride, Chloride, Bromide, Iodide]

-2 Charge [Oxide, Sulfide, Selenide, Telluride]

-3 Charge [Nitride, Phosphide]

-4 Charge [Carbide, Silicide]

Note, this is not a complete list, nor is it 100% assured that it is right. If you find anymore or have problems, leave a note at kyto_beta@yahoo.com