Oxidation Numbers

The oxidation number of lead (Pb) in PbF4 is +4. Fluorine (F) always has an oxidation number of -1, so for PbF4, the four fluorine atoms contribute a total oxidation number of -4. This means the lead atom must have an oxidation number of +4 to balance the charge.

Potassium is the metal here and it has an Oxidation number of +1 in every compound because all Alkali Earth metals have an Oxidation Number of +1.

(The other elements: Oxygen -2 and Chromium (Cr) +6)

The oxidation number for Ga (gallium) is typically +3. This is because gallium, as a metal, tends to lose three electrons in chemical reactions to achieve a stable electron configuration.

-1 is most common, but Cl can exhibit oxidation numbers from -1 to +7 in its compounds.

The oxidation number of americium is typically +3. However, americium can exhibit other oxidation states, such as +2 and +4, in some chemical compounds.

The oxidation number of P2O5 is Phisphorus +5, Oxygen -2.

In anions that contain oxygen along with a less electronegative element, each oxygen atoms is assigned an oxidation number of -2. Therefore, a WO4-2 anion requires the tungsten atoms to have an oxidation number of +6, to result in the specified charge of the anion.

The oxidation number of Mn in MnCO3 is +2. MnCO3 is a neutral compound, so the overall sum of the oxidation numbers of all elements in the compound should equal zero. Since the oxidation number of oxygen is typically -2 and there are three oxygen atoms, the oxidation number of Mn must be +2 to balance out the charges.

The oxidation number for Br2 is 0. This is because each bromine atom in Br2 has a zero oxidation number, as they both have a balanced number of electrons.

The oxidation number of carbon (C) in CH2O is +2. This is because hydrogen (H) has an oxidation number of +1 and oxygen (O) has an oxidation number of -2, so the sum of the oxidation numbers in CH2O must be zero to balance the charge.

In MgO (magnesium oxide), the oxidation number of magnesium (Mg) is +2, and the oxidation number of oxygen (O) is -2. Magnesium typically has a +2 oxidation state because it loses two electrons to form a stable ionic bond with oxygen, which gains two electrons to achieve a full outer shell.

The oxidation number for O in K2O is -2. Oxygen typically has an oxidation number of -2 in most compounds. Since there are two oxygen atoms in K2O, the total oxidation number contributed by the oxygen atoms is -4.

The atomic number of an element is based on the number of protons in its nucleus, which is unique for each element. The oxidation number, on the other hand, is related to the charge that an atom carries in a compound or ion. The oxidation number does not directly determine the atomic number, as they are two distinct properties of an element.

The oxidation number for Cr in CrO3 is +6. Each oxygen atom has an oxidation number of -2, and since there are three oxygen atoms in CrO3, the total oxidation number contributed by oxygen is -6. This means that the oxidation number of chromium must be +6 to balance the overall charge of the compound, which is neutral.

The oxidation number of phosphorus in PL3 is -3. Each hydrogen has an oxidation number of +1, so in order for the overall charge of the compound to be neutral, phosphorus must have an oxidation number of -3.

The oxidation number of carbon in Na2C2O4 is +3. Sodium has an oxidation state of +1, and oxygen typically has a -2 oxidation state, so by setting up an equation, we can determine that carbon must have an oxidation state of +3 in this compound.

The sulfur in potash alum occurs in sulfate ions, which have the formula SO4-2. Since sulfur is less electronegative than oxygen, the oxygen has an oxidation number of -2; 4 atoms of oxygen give a total negative charge of -8, and the sulfur atom must have an oxidation number of +6 to match the -2 charge of the sulfate ion as a whole.

In H3PO3, also known as phosphorous acid, the oxidation number of hydrogen is +1 and the oxidation number of phosphorous is +3. This is because hydrogen typically has an oxidation number of +1 in compounds, and the sum of oxidation numbers in a neutral compound must be zero.

The oxidation number for sulfur (S) in tin(IV) sulfate (Sn(SO4)2) is +6. This is because the overall charge of the sulfate ion (SO4) is -2, and there are two sulfate ions present in the compound, leading to a total charge of -4. The oxidation number of tin (Sn) in this compound is +4.

K has an oxidation number of +1

O has an oxidation number of (-2) x 4

So... the oxidation number for Mn is whatever is needed to make 1-8 equal to zero.

Therefore, the oxidation number for Mn is +7

The oxidation number for Co in CoS is +2, a divalent cobalt cation, since the only anion formed from a single sulfur atom has a charge of -2.

The oxidation number of Au (gold) in AuPO4 is +3. This is because in most compounds, the oxidation number of oxygen is -2, and the overall charge of PO4 3- ion is -3. So, the oxidation number of Au must be +3 to balance the charges.

The oxidation number of Li in Li3N is +1, as it is a Group 1 element. The nitrogen (N) in Li3N has an oxidation number of -3.

In MnCl2, the oxidation number of Mn is +2, as it is in the +2 oxidation state. The oxidation number of Cl is -1 each, as it is typically in the -1 oxidation state when bonded to metals such as manganese.