Oxidation Numbers

Oxidation number of Nb is +4. Oxidation number of O is -2.

-1 for Carbon (in carbide) and +2 for Ca

Whatever the charge on that ion is.

In the anions of oxyacids, oxygen is always assigned an oxidation number of -2. Therefore, in an MnO4-1 anion, manganese must have an oxidation number of +7 to achieve electrical balance for the anion. (There is no neutral compound with the formula MnO4.)

-2 for each O, +7 for Mn

The oxidation number for the element in group 15 (nitrogen group) is usually -3, as these elements tend to gain 3 electrons to achieve a stable electron configuration.

Transition metals have variable oxidation numbers because they have incompletely filled d orbitals in their outermost electronic shell. These d orbitals can participate in bonding and easily change their oxidation states by gaining or losing electrons. This flexibility allows transition metals to exhibit a wide range of oxidation states in different compounds.

The oxidation number of nitrogen in nitrogen dioxide (NO2) is +4. Each oxygen atom in NO2 has an oxidation number of -2, and since the molecule is neutral, the sum of the oxidation numbers must equal zero. Therefore, the oxidation number of nitrogen is calculated as follows: 2(-2) + x = 0, where x represents the oxidation number of nitrogen. Solving for x gives x = +4.

The oxidation number of atom B will depend on the compound or molecule it is a part of and its surrounding atoms. It is determined based on the number of valence electrons B has contributed to the compound or molecule.

0 in the elemental form, +1 in its compounds

The oxidation number of sulfur in sodium bisulfate is +5. In bisulfate ion (HSO4-), the overall charge is -1, so the oxidation number of sulfur can be calculated as -1, taking into account the oxidation number of sodium as +1.

The oxidation number for NO3 is -1. Since oxygen is usually assigned an oxidation number of -2 in compounds, the total oxidation number for the nitrate ion (NO3) must be -1 to account for the three oxygens.

The oxidation number of sulfur in sulfuric acid (H2SO4) is +6. This is because oxygen typically has an oxidation number of -2, and there are four oxygen atoms in sulfuric acid. Each hydrogen atom has an oxidation number of +1. Using this information, we can calculate that the oxidation number of sulfur must be +6 in order for the overall charge of the molecule to be neutral.

The oxidation number of oxygen in Cr2O7 is -2. Since there are seven oxygen atoms in the dichromate ion (Cr2O7), and the overall charge of the ion is -2, each oxygen atom is assigned an oxidation number of -2.

Argon is generally considered to be unreactive element, i.e. it cannot form compounds. But new researchs have found that argon can form a compound called Argon fluorohydride(HArF) which is very unstable. Here Argon's charge may be neutral, i.e. 0

The question should be either 'alkali metals' or 'alkaline earth metals'.

For alkali metals or group 1 elements, the oxidation number is +1 (note. hyddrogen can have +1 and -1).

For alkaline earth metals, the oxidation number is +2

In addition all these elements will have an oxidation number of 0 in their elemental form

The oxidation number of sulfur in aluminum sulfate is +6. This is because each oxygen atom has an oxidation number of -2, and there are four oxygen atoms in the sulfate ion (SO4). The overall charge of the sulfate ion is -2, so the oxidation number of sulfur must be +6 to balance the charge.

The oxidation number of H in H3PO4 is +1. In a compound, the oxidation numbers of all the elements add up to the overall charge of the compound, which is 0 in this case. Since the oxidation number of oxygen is typically -2 and there are four oxygen atoms in H3PO4, the oxidation number of hydrogen must be +1 to balance the charge.

The oxidation number of Br- is -1. Bromine typically has an oxidation state of -1 when it forms an ion by gaining one electron.

The oxidation number of an element in an ionic bond indicates its charge when it gains or loses electrons to achieve a stable octet. By comparing the oxidation numbers of the elements involved, you can determine how many electrons each element has gained or lost in the formation of the bond.

The oxidation number of hydrogen in iodic acid (HIO3) is +1.

Usually the oxidation no of oxygen is -2 and the oxidation no of hydrogen is +1 in a compound.

Oxidation number is the charge per atom in a compound.

Cl2= 2- (Cl= 1-)

Cu would have to be 2+ to balance the compound, because there is only one copper atom.

+2 for iron, +1 for hydrogen and -2 for oxygen in Fe(OH)2

The oxidation number of Fe in Fe2O3 (iron (III) oxide) is +3. This is because oxygen usually has an oxidation number of -2, and since there are three oxygen atoms in Fe2O3, the total oxidation number contributed by oxygen is -6. This means the Fe atoms must have a combined oxidation number of +6 to balance the charge, leading to an oxidation number of +3 for each Fe atom.