Oxidation Numbers

For PtCl6^2-, let x be the oxidation number of Pt, and -1 be the oxidation number of Cl. Since there are 6 Cl atoms each with an oxidation number of -1, the sum of the oxidation numbers must equal the charge of the ion, which is -2. Therefore, x + 6(-1) = -2. Solving for x, we get x = +4. So, the oxidation number of Pt in PtCl6^2- is +4.

The group number of an element often corresponds to the typical oxidation state it will exhibit. For main group elements (groups 1, 2, 13-18), the oxidation state is typically equal to the group number. However, transition metals (groups 3-12) can exhibit multiple oxidation states due to their partially filled d orbitals.

The oxidation number of Al in Al2(SO4)3 is +3 because each sulfate ion (SO4) has a charge of -2 and there are 3 sulfate ions, leading to a total charge of -6. In order for the compound to be neutral, the aluminum ions must have a total charge of +6, leading to an oxidation number of +3 for each aluminum ion.

The sum of the oxidation numbers for P2O5 is zero. In P2O5, the oxidation number for phosphorus is +5, and each oxygen atom has an oxidation number of -2. Since there are five oxygen atoms, the total sum of the oxidation numbers is 2(+5) + 5(-2) = 0.

The oxidation number of cobalt in Co2O3 is +3, and the oxidation number of oxygen is -2. This is based on the rules for assigning oxidation numbers, where the overall charge of the compound must equal zero.

Halogens typically have an oxidation number of -1 in compounds because they have seven valence electrons and need to gain only one electron to achieve a full octet. Exception: in compounds with oxygen or other halogens, halogens may have positive oxidation numbers.

The oxidation number of C in CO3^2- is +4. Each oxygen atom has an oxidation number of -2, and since the overall charge of the carbonate ion is 2-, the carbon atom must have an oxidation number of +4 to balance the charge.

The oxidation state of Na in Na2O2 is +1, as each Na atom carries a +1 charge while the O atoms carry a -1 charge. In KO2, the oxidation state of K is +1, similar to Na2O2, as each K atom carries a +1 charge while the O atoms carry a -1/2 charge.

The sum of the oxidation numbers in a neutral compound is always zero. This is because the total charge of the compound is zero, so the sum of the oxidation numbers of the individual elements must also add up to zero.

The sum of the oxidation numbers of all carbons in C6H5CHO is equal to 0. This is because the oxidation number of carbon is -2 in CH3CHO, and there are six carbons in C6H5CHO. So, 6 * (-2) = -12. However, since the overall charge of the molecule is 0, the sum of the oxidation numbers of all carbons must be 0 to balance the charge.

The oxidation number for Ni in NiS (nickel sulfide) is +2, while the oxidation number for S (sulfur) is -2. This is because in a compound, the overall charge must be neutral.

The oxidation number of B in H3BO3 is +3. Each hydrogen atom has an oxidation number of +1, and the overall molecule has a neutral charge. Since oxygen has an oxidation number of -2, the oxidation number of B must be +3 in order to balance the charges.

The oxidation state of Li in its elemental form (Li) is 0 because it is in its pure state and not involved in a chemical reaction where it would gain or lose electrons.

NaClO4 is sodium perchlorate, which is a chemical compound commonly used as an oxidizing agent in chemistry and industry. It is a white crystalline solid that is soluble in water and stable under normal conditions.

Negative (such as -2 in compounds like O2 or Cl-) or positive (such as +3 in compounds like NCl3), depending on the element and the compounds involved.

The oxidation number of chlorine in AlCl4 is -1. Since aluminum has an oxidation number of +3, the overall charge of the AlCl4 ion is -1, meaning each chlorine atom has an oxidation number of -1 to balance the charge.

In CH2Br2, carbon has an oxidation number of -2 because hydrogen has an oxidation number of +1 and bromine has an oxidation number of -1. The sum of the oxidation numbers in a neutral compound is zero.

The oxidation number of Br in BrO2- is +3. Oxygen is typically assigned an oxidation number of -2, so in this case the total charge on the ion is -1, meaning bromine must have an oxidation number of +3.

The oxidation number of iodine in IF is +1 because fluorine is more electronegative than iodine and will take on a charge of -1. Since the compound is neutral, the oxidation number of iodine must be +1 to balance the -1 charge of fluorine.

Elements with positive oxidation numbers have excess electrons that they can share or transfer with elements having negative oxidation numbers that have electron deficiencies. This transfer or sharing of electrons allows the elements to achieve a more stable electron configuration, forming compounds through the formation of ionic or covalent bonds.

Technetium (Tc) typically has oxidation states ranging from -1 to +7, with the most common oxidation states being +4 and +7. The specific oxidation number of technetium in a compound depends on the overall charge and bonding characteristics of the compound.

No, not all metals have two oxidation numbers. Some metals may have multiple oxidation numbers depending on the bonding situation and the compounds they form.

In K₂CrO₄, the oxidation number of potassium (K) is +1, and the oxidation number of oxygen (O) is -2. Since the compound is neutral, the oxidation number of chromium (Cr) can be calculated as follows: 2(+1) + Cr + 4(-2) = 0. Solving for chromium, the oxidation number of chromium in K₂CrO₄ is +6.

The oxidation number of tungsten (W) in WO4^2- is +6. Since the overall charge of the ion is 2-, each oxygen atom has an oxidation number of -2.

H is +1, O is -2 overall carbon will have an oxidation # of -3