Oxidation Numbers

The oxidation number of the CN^- ion is -1. Carbon typically has an oxidation number of +4 and nitrogen of -3, so in the CN^- ion, carbon has a -3 oxidation number to balance the -1 overall charge.

The oxidation number of Zr in ZrI4 is +4. Each iodine atom has an oxidation number of -1, and since there are four iodine atoms in ZrI4, the overall charge must be balanced by the Zr atom having an oxidation number of +4.

In KCrO2, potassium (K) has an oxidation number of +1, oxygen (O) has an oxidation number of -2, and the overall compound has a neutral charge. The sum of the oxidation numbers must equal zero, so the oxidation number of chromium (Cr) is +4.

The oxidation number for Ba in BaO2 is +2, as the oxidation number for oxygen is typically -2. Since there are two oxygen atoms in BaO2, the overall charge must be balanced out by Ba having a +2 oxidation number.

The oxidation number of aluminum in aluminum chloride (AlCl3) is +3. This is because each chlorine atom has an oxidation number of -1, and there are three chlorine atoms bonded to the aluminum atom, resulting in a total charge of -3 for the chlorine atoms. For the compound to be neutral, the aluminum atom must have an oxidation number of +3.

LiBrO3 this decomposes to Li^(+) & BrO3^(-)

The bromate anion has a charge of '-1'

Use the standard for oxygen at '-2'

Since there are 3 oxygens then the oxygen moiety is 3 X -2 = -6

Creating a little sum

Br + -6( oxygen moiety) = -1( anion charge)

Br - 6 = -1

Add '6 'to both sides

Br = (+)5 The oxidation state of bromine.

The oxidation number of oxygen is typically -2. Since there are four oxygen atoms in MoO4-2 and the overall charge is -2, the oxidation number of molybdenum (Mo) is calculated to be +6 to balance the negative charge.

The oxidation number of N in (N2H5)2SO4 is -1. This is because the overall charge of the compound is neutral, and the oxidation number of S is +6. By using the oxidation numbers of S and O, we can determine that the oxidation number of N must be -1 to balance the charges in the compound.

0 in N2

The oxidation number for Sn in SnO4^2- is +4. Oxygen is typically assigned an oxidation number of -2, so the sum of the oxidation numbers in the compound equals the overall charge of -2 for the ion.

For CaSO4 (calcium sulfate), the oxidation number of sulfur is +6. For SO4 (sulfate ion), the oxidation number of sulfur is +6. For SO2 (sulfur dioxide), the oxidation number of sulfur is +4. For SO3 (sulfur trioxide), the oxidation number of sulfur is +6.

In AgNO3, since Ag is in Group 1A, it always has a +1 oxidation state. Oxygen is typically -2, so the sum of the oxidation states must equal the overall charge of the compound, which is 0 for AgNO3. Therefore, N must have an oxidation state of +5 to balance out the charges.

The oxidation number of Ni in Ni(OH)2- is +2. This is because each hydroxide ion has a charge of -1, and the overall charge of the compound is -1. Therefore, the nickel ion must have a charge of +2 to balance the charge of the two hydroxide ions.

The oxidation state of sodium is +1, as it typically loses one electron to achieve a stable electron configuration. Chlorine's oxidation state is -1, as it usually gains one electron to satisfy its octet rule.

The charge an element would have if it lost or gained electrons

The oxidation number of phosphorus (P) in PH3 is -3. This is because hydrogen (H) has an oxidation number of +1, and there are three hydrogen atoms bonded to phosphorus, resulting in a total charge of +3 that is balanced by phosphorus having an oxidation number of -3.

The oxidation number of nitrogen in nitrosyl fluoride (NOF) is +3, while the oxidation number of fluorine is -1. This is calculated by recognizing that the overall charge of the molecule is zero, and the sum of the oxidation numbers of each atom must equal this charge.

The oxidation number of a compound is zero (nitrogen -3, hydrogen +1, chromium +3, oxygen -2).

The oxidation number of Li in Li2 is +1. The oxidation number of O in Li2O is -2.

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.

The oxidation number of PF5 is +5 for phosphorus and -1 for each of the four fluorine atoms, resulting in a total charge of 0 for the compound.

The oxidation number of Ca is 0 in its elemental form and is +2 in its compounds.

The oxidation number of manganese (Mn) can vary depending on the compound it is in. In MnO2, the oxidation number of Mn is +4, while in KMnO4, the oxidation number of Mn is +7.

The overall charge is -1. Oxidation number of oxygen in -2. By balancing the charges, chlorine is in +7 state.

The oxidation number of Na in NaH is +1. In general, group 1 elements like sodium (Na) have an oxidation number of +1 in most compounds.