Oxidation Numbers

The oxidation state of N in NH4Cl is -3. In this compound, nitrogen is in the ammonium ion (NH4+) which has an overall charge of +1, so each hydrogen atom has an oxidation state of +1. Given that the overall charge of the ion is +1, nitrogen must have an oxidation state of -3 to balance the charges.

The valence electrons of an atom determine its ability to form bonds and participate in chemical reactions. The oxidation number of an atom indicates the number of electrons it has gained, lost, or shared in a chemical compound. The valence electrons of an atom can help determine its oxidation number by considering how many electrons the atom needs to reach a stable configuration.

Yes, iron is a transition metal that can have multiple oxidation states, including +2 and +3. These different oxidation states enable iron to participate in a wide range of chemical reactions and form various compounds.

Na2Cr2O7

Sodium always has ox. number = 1,

and oxygen = -2.

Therefore you got 2x1 = 2 for sodium,

and 7*(-2) = -14 for oxygen.

2 + 2*x = 14

x = 6

The oxidation number of H in H2SO4 is +1, the oxidation number of S is +6, and the oxidation number of O is -2. This is because the sum of the oxidation numbers in a neutral compound like H2SO4 must equal zero.

The oxidation number of sulfur in hydrogen sulfide (H2S) is -2. Each hydrogen atom has an oxidation number of +1, so in order to balance the overall charge of the compound (which is neutral), sulfur must have an oxidation number of -2.

The sum of oxidation numbers in a neutral compound is always zero, as the charges balance out. In polyatomic ions, the sum of oxidation numbers equals the charge of the ion. When determining oxidation numbers, rules such as assigning elements in their elemental state an oxidation number of zero and hydrogen an oxidation number of +1 are typically followed.

The oxidation number of lead (Pb) in the compound PbCl2 has to be what?

The oxidation number (formal charge) on oxygen can be 0, -1/2, -1 or -2. The formal charge on oxygen in a peroxide is -1. Elemental oxygen exists as O2 or O3. The formal charge on all elements is 0. The formal charges on oxygen in an oxide and superoxide, respectively, are -2 and -1/2.

The oxidation number of iron in ferrocyanide is +2, as each cyanide ligand has a -1 charge. Therefore, since there are four cyanide ligands, they contribute a total charge of -4, balancing the +2 charge of the iron atom.

The oxidation number of sodium (Na) in NaIO4 is +1. The sum of the oxidation numbers of all atoms in a neutral compound like NaIO4 must equal zero. Since oxygen typically has an oxidation number of -2, the oxidation number of iodine (I) in NaIO4 is +7 to balance the charges.

1. In a neutral compound, the sum of oxidation numbers of all atoms will be zero.
2. In a polyatomic ion, the sum of oxidation numbers of all atoms will be equal to the charge of the ion.
3. The oxidation number of an element in its elemental form is zero.
4. Fluorine always has an oxidation number of -1 in compounds.
5. Oxygen usually has an oxidation number of -2 in compounds.

The oxidation number for Mn in MnO4^- is +7. This is found by balancing the charges on the formula MnO4^- where O has an oxidation number of -2.

In molybdenum disulfide (MoS2), molybdenum typically has an oxidation state of +4, and sulfur has an oxidation state of -2. Each Mo atom contributes a +4 oxidation state, while each S atom contributes a -2 oxidation state, which balances the overall charge of the compound.

The oxidation number of sulfur in sulfide is -2. This is because in most compounds, such as sulfide (S2-), sulfur tends to gain two electrons to achieve a stable octet configuration.

-1 only for F

Other elements could have -1 to +7 depending on the compound

In compounds such as H2Se yes it is, and the oxidation number ofd -2 is well known. However there are many compounds where Se has other oxidation numbers (Se is very similar to Sulfur another group 16 elemnt) for example compounds where Se has an ox number of +4, SeF4, +6, SeF6, -1 in the polyselenide compound Na2Se2

Oxygen almost always keeps an oxidation number of -2.

Since the overall ion has a charge of -1 you just have to balance the ion.

2*-2 for the oxygen = - 4

In order for the overall charge to be -1, the chlorine must have a +3 oxidation numbers.

0 in the elemental form. +2 and +4 in its compounds

When naming ionic compounds with variable oxidation numbers, the cation's charge is specified using Roman numerals in parentheses after the metal's name. For example, iron(II) chloride and iron(III) chloride for FeCl2 and FeCl3, respectively.

Using the periodic table of elements you can find the oxidation number of NaHCO3.

Na has a charge of +1 so it's oxidation number is +1.

H has a charge of +1 so again, the oxidation number is +1.

CO3(carbonate) has an oxidation number of -2.

As far as I know, you can find the oxidation number for CO3 because all charges together come out to be zero. With Na and H adding up to 2, CO3 can be seen to be -2.

Also, CO3 is -2 because it's Lewis structure is two electrons short from being complete.

the oxidation number of nitrogen is 5

The formula for iron using the highest oxidation number is Fe2O3, which is iron(III) oxide. In this compound, iron is in the +3 oxidation state.

Nonmetals typically have negative oxidation numbers when they form compounds. For example, oxygen usually has an oxidation number of -2, while hydrogen typically has an oxidation number of +1. The oxidation number of a nonmetal can vary depending on the compound it is part of.