Oxidation Numbers

The oxidation number of hydrogen in ethane (C2H6) is +1. Hydrogen tends to have a +1 oxidation state when bonded to nonmetals like carbon.

Flourine has an oxidation number of -1 one because it only needs one electron to become stable ( to have neon's stractures), Hydrogen is the same thing. one electron away from being stable. oxidation numbers of elements are their electric charges on the periodic table. O2(g) has an oxidation number of 0, along with all the diatomics, Oxyden in a compound has ON of of -2, H has +1, the rest you calculate using algebra.

In all sulphate compounds 'S' is in 6+ oxidation state.

In HgCl2, mercury's oxidation number is 2+ and chlorine's is 1-.

For any element before reaction, its oxidation number is 0. Molecules made from the atoms of the same element have 0 oxidation state in each atom. Examples are gaseous hydrogen and liquid bromine.

The oxidation number of potassium (K) is +1, hydrogen (H) is +1, phosphorus (P) can vary but in K2HPO4, it is +5, and oxygen (O) is -2. Therefore, the oxidation number of K2HPO4 is +1 for K, + 1 for H, +5 for P, and -2 for O.

it would be +3 then you have to -3 so yyeah. finish your science homework kids! i know i need to.. /:

The cobalt in the formula given has an oxidation number of +3, so that the total charge of the two cobalt ions will balance the total charge of the 3 oxide ions, which have an oxidation number of -2 each.

The oxidation number of Cr in acidified potassium dichromate (K2Cr2O7) is +6. This is because each oxygen atom has an oxidation number of -2, and the overall charge of the dichromate ion is -2.

6.

To determine this the CrO4 ion must be 2- as it is balanced by 2 potassium ions which can only have a +1 charge.

The oxygen atoms are considered to be present as O2- so all four contribute 8-. As the net charge is only 2- then chromium must have charge (oxidation number or state) of 6+.

The oxidation number of oxygen in carbon suboxide is -1. In carbon suboxide, C3O2, the carbon atom has an oxidation number of +4, while the two oxygen atoms each have an oxidation number of -1 to give a total charge of zero for the molecule.

To predict an element's oxidation number, you can use the rules based on the periodic table and chemical bonding principles. For example, in many cases, elements prefer to have a full valence shell, so they will gain or lose electrons to achieve that stable electron configuration. Additionally, the group number of an element can provide a general idea of its typical oxidation number.

The correct oxidation number for HCl is -1 for Cl and +1 for H.

There is at least one oxidation number shared by all the elements in a periodic table column, but some of the elements may have more than one oxidation number and some of these additional oxidation numbers may not be possible for all the elements in a column.

The oxidation number of Cl in PtCl4^2- is -1. This can be determined by considering that the overall charge of the complex ion is 2-, and each Cl atom has an oxidation number of -1.

In S2Cl2, each sulfur atom has an oxidation number of 0, and each chlorine atom has an oxidation number of -1.

In Sb₂O₄, oxygen is almost always assigned an oxidation number of -2. To find the oxidation number of Sb, you can set up the equation: 2x + 4(-2) = 0, where x is the oxidation number of Sb. By solving this equation, you'll find that the oxidation number of Sb in Sb₂O₄ is +5.

The sum of the oxidation numbers in a neutral compound is equal to zero. This is because in a neutral compound, the total positive oxidation numbers are balanced by the total negative oxidation numbers to give a net charge of zero.

S2O3: +2 for S KCl: +1 for K, -1 for Cl He: 0 Cl2: 0 CO3^2-: -2 for O, +2 for C NO3-: -2 for O, +5 for N NO2-: -2 for O, +4 for N H3N: -3 for H, +1 for N

The oxidation number of N in NO2 is +4. Each oxygen atom has an oxidation number of -2, so the sum of the oxidation numbers in NO2 must equal the overall charge of the molecule, which is 0. This means that the oxidation number of N must be +4 to balance the -4 oxidation contributed by the two oxygen atoms.

This may best be demonstrated by example:

Here are two forms (read: oxidation numbers) of iron, as FeO and Fe2O3. Because we know oxygen has a -2 charge per atom, the oxidation number of Fe in FeO is II. As for Fe2O3, we know that the oxidation number of Fe is III; there is no charge on the compound, so the two iron molecules must equally offset the -6 charge from the three oxygen atoms.

Oxidation numbers are written as roman numerals. You would write these two forms of iron oxide as iron(II) oxide and iron(III) oxide, respectively. Oxidation states are the (+) or (-) charges written as a superscript.

It is zero since it is a free element and it does not react with anything

The oxidation number of Pt in K2PtCl6 is +4. In this compound, the total charge of potassium (K) is +2 (from 2*K+1), and the total charge of chloride (Cl) is -1 (from Cl-1), so the oxidation number of Pt must be +4 to balance the overall charge of the compound.

The oxidation number of manganese changes from +4 in MnO2 to +3 in Mn2O3. This indicates a reduction of the manganese atom.

The oxidation number of a carbon atom in diamond is 0, because carbon atoms in diamond have a formal charge of 0. Each carbon atom in diamond is bonded to four other carbon atoms, forming a tetrahedral structure, and there are no net charges on the molecule.