Oxidation Numbers

Possible valences of plutonium are: +2,3,4,5,6.

In any neutral compound, this number must be zero.

To calculate the oxidation number of Co(NH3)6, first identify the oxidation number of ammonia (NH3), which is -3. Since there are six ammonia molecules surrounding the cobalt (Co) atom, the total charge contributed by the ammonia ligands is -3 x 6 = -18. Since the overall charge of the complex is usually 0, the oxidation state of cobalt (Co) in this complex is +3 to balance the charge.

Oxidation number can be best described as a hypothetical charge assigned to each atom in a molecule or ion based on the assumption that the shared electrons are divided equally between atoms in a chemical bond.

Most nonmetals typically have negative oxidation numbers when in compounds, such as -1 for halogens (F, Cl, Br, I) and -2 for oxygen (O). However, some nonmetals like nitrogen (N) can have positive oxidation numbers depending on the compound.

The oxidation state of Mn in Mn(ClO4)3 is +7. This is because the overall charge of the perchlorate ion (ClO4)- is -1, and there are 3 perchlorate ions in Mn(ClO4)3, resulting in a total charge of -3. To balance this, the Mn ion must have an oxidation state of +7.

O.S of Mn = 3+

O.S. of Cl = 7+

O.S. of O = 2-

In MgBr2, the magnesium ion (Mg) has an oxidation number of +2, while the bromide ion (Br) has an oxidation number of -1.

In chemistry, "Sn" stands for the element tin. Tin is a metallic element with the atomic number 50.

Reverse oxidation, also known as reduction, is a chemical reaction where a molecule or atom gains electrons. This process leads to a decrease in the oxidation state of the species involved. Reverse oxidation typically involves the removal of oxygen atoms or the addition of hydrogen atoms.

Transition elements in zero or lower oxidation states have vacant d orbitals, making them more prone to form complexes with ligands like CO and NO through dative bonding. These ligands are able to donate electron density to the empty d orbitals of the metal ion, stabilizing the complex. Additionally, the small size and ability to form multiple bonds of ligands like CO and NO make them effective at forming stable complexes with transition metals.

In the compound NaF2, sodium typically has an oxidation state of +1, and fluorine has an oxidation state of -1. When combined in a compound, the total oxidation numbers must add up to zero, but in NaF2 they add up to +2 (-1 for each fluorine and +1 for sodium), which is incorrect. The correct formula should be NaF.

The oxidation number of Al in Al2Br6 is +3. Each bromine atom has an oxidation number of -1, and since the compound is neutral, the sum of the oxidation numbers must equal zero. Hence, each Al atom must have an oxidation number of +3 to balance the -6 from the bromine atoms.

Well, without being given an equation, we presume you mean the o.n. of chromium.

H in this is +1, so H+H=+2

4 x O= -2 x 4 = -8,

therefore Cr = +6 as the whole element has to equal zero.

and i do believe in this form it normally goes to Cr +3

The oxidation number of group 17 elements, also known as the halogens, is typically -1. This is because they have seven valence electrons and tend to gain one electron to achieve a full outer shell configuration.

The oxidation number of Iodine (I) in HI (hydroiodic acid) is -1. In binary compounds with hydrogen, hydrogen is assigned an oxidation number of +1. Therefore, the oxidation number of Iodine must be -1 in order for the overall compound to be neutral.

The oxidation number of C in C2O4^2- is +3. This is because each O atom is assigned an oxidation number of -2, and the overall charge of the ion is -2, so the two C atoms must have a total oxidation number of +6 in order to balance the charge.

The oxidation number of Mg is +2. The oxidation number of O is -2, and since there are 6 oxygen atoms in Mg2Si2O6, the total oxidation number contributed by O is -12. The oxidation number of Si is +4. Therefore, to find the oxidation number of Mg in Mg2Si2O6, you can set up an equation as follows: 2x + 2(+4) + 6(-2) = 0, where x is the oxidation number of Mg. By solving this equation, you find that the oxidation number of Mg is +2 in Mg2Si2O6.

"Ne3s23p3" is the electron configuration notation for sodium (Na). It represents the distribution of electrons in the various energy levels and orbitals within the atom.

The oxidation number of phosphorus (P) in H3PO5 is +5. Each hydrogen atom has an oxidation number of +1, and the oxygen atoms have oxidation numbers of -2. The sum of the oxidation numbers in a neutral compound must equal zero.

The oxidation state of Mn in the compound Mn2 is +2. Each Mn atom has an oxidation state of +2, as indicated by the subscript 2 in the formula Mn2.

The oxidation state of carbon in formaldehyde (CH2O) is +2. This is because oxygen typically has an oxidation state of -2, and there are only two atoms of oxygen present in formaldehyde. The overall charge of formaldehyde is zero, so the sum of the oxidation states must equal zero, leading to carbon having an oxidation state of +2.

The oxidation number of Ca in CaC2O4 is +2 because Ca, a group 2 element, typically has a +2 oxidation state in compounds. The oxidation number of C in C2O4 is +3 because the overall charge of the oxalate ion is -2, and there are two C atoms, each with an oxidation state of +3 to balance the charge.

The oxidation number of calcium (Ca) in CaF2 is +2. This is because fluorine (F) typically has an oxidation number of -1, and the overall charge of CaF2 is neutral. Since there are two fluorine atoms each with a -1 charge, the calcium atom must have a +2 oxidation number to balance the charges.

The oxidation number of Zn in the complex ion Zn(OH)4 2- is +2. This is because the overall charge of the complex ion is -2, and each hydroxide ion (OH-) has a -1 charge. Hence, the zinc (Zn) ion must have a +2 charge to balance the overall charge of the complex ion.