Oxidation Numbers

The element which has the same oxidation number in all of its known compounds is fluorine. Fluorine always has an oxidation number of -1 in its compounds because it is the most electronegative element.

The oxidation number of bromine in aqueous HBrO (hypobromous acid) is +1. This is because in HBrO, oxygen is more electronegative than bromine and will have an oxidation number of -2, leaving bromine with a +1 oxidation state to balance the overall charge of the molecule.

The oxidation number of Cu in Cu2S (copper sulfide) is +1. This is because the overall charge of the compound is 0 and there are two Cu atoms each with an oxidation state of +1.

0 in the elemental form. +1 or +3 in its compounds

The oxidation number of barium is +2.

The oxidation number of nitrogen in the nitrate ion (NO3-) is +5. This is because oxygen generally has an oxidation number of -2, and the overall charge of the nitrate ion is -1. Thus, nitrogen must have an oxidation number of +5 to balance the charge.

The oxidation number of oxygen in hydroxide (OH-) is -2 since oxygen typically has an oxidation number of -2 in compounds. The oxidation number of hydrogen in hydroxide is +1 since hydrogen usually has an oxidation number of +1 when bonded to nonmetals like oxygen.

there are two for silicone.those are 0 and 4.

Atomic silicon has oxidation number 0. It forms a wide variety of compounds, specially with oxygen. In these compounds, the oxidation number of silicon can vary from 0 to +4.

The oxidation number of each carbon atom in C6H8O6 is +4. Each hydrogen atom has an oxidation number of +1, and each oxygen atom has an oxidation number of -2.

In S2O82-, each S atom has an oxidation number of +5. In SO42-, the oxidation number of S is also +5. There is no change in oxidation number for sulfur when transitioning from S2O82- to SO42-.

Barium nitride is Ba3N2

And the oxidation numbers are +2 for Ba and -3 for N

The oxidation number of copper (Cu) in CuF2 is +2. The oxidation number of fluorine (F) in compounds is almost always -1, and since there are two fluorine atoms in CuF2, the total negative charge is -2, which balances with the +2 oxidation state of copper.

The oxidation number of an elementary substance is zero because there is no transfer of electrons between atoms of the same element in a compound. Each atom in an elementary substance is considered to have an oxidation number of zero.

To find the oxidation number in a reaction, you can assign oxidation numbers to individual atoms in the compounds involved based on known rules and then adjust them based on the charges of the ions or molecules they are a part of. Keep in mind that oxidation numbers are not actual charges, but rather a conceptual tool to help track electron transfer in chemical reactions.

Elements with oxidation numbers of +1 include elements in Group 1 of the periodic table, like hydrogen and sodium. Elements with oxidation numbers of -1 include elements in Group 17, like fluorine and chlorine.

The oxidation number of sodium (Na) in sodium carbonate (Na2CO3) is +1. The oxidation number of oxygen (O) is -2, and the oxidation number of carbon (C) is +4. Therefore, the overall compound has a charge of 0.

The oxidation number of nitrogen in NO is +2. This is because oxygen has an oxidation number of -2, and since the overall charge of NO (nitrogen monoxide) is 0, the nitrogen atom must have an oxidation number of +2 to balance the equation.

Potassium typically has an oxidation number of +1. This is because it readily gives away its one valence electron to form a stable ion.

The oxidation number for oxygen in KMnO4 is -2. The total oxidation number for the compound must equal zero (since it is neutral), and since the oxidation number for potassium (K) is +1 and for manganese (Mn) is +7, the oxidation number for oxygen must be -2 to balance the charges.

The oxidation number of carbon in carbonate (CO3^2-) is +4. In the carbonate ion, each oxygen atom has an oxidation number of -2, so the overall charge of the ion is -2. This means the oxidation number of carbon must be +4 to balance the charges in the compound.

The oxidation number of nitrogen in hydrazine (N2H4) is -2. This is because hydrogen usually has an oxidation number of +1, and in this case, since there are two hydrogens bonded to each nitrogen, the total oxidation number for nitrogen must be -2 to balance it out.

hydrogen

+1 in most of the compounds

-1 in metal hydrides

For most elements, their highest attainable oxidation number is equal to the number of valence electrons. Examples are the maximum oxidation numbers for: sulfur is +6, phosphorus is +5 and chlorine is +7. Fluorine is an exception which bears oxidation numbers 0, -1/2 and -1.

The oxidation number of phosphorus is typically -3 in ionic compounds, such as phosphides (e.g., Na3P), and can vary in covalent compounds depending on the electronegativity of other elements involved.