Oxidation Numbers

The oxidation number for hydrogen in the compound HCl is +1. Hydrogen typically has an oxidation number of +1 when bonded to nonmetals like chlorine in covalent compounds.

The most common oxidation states for tungsten are +2, +4, and +6.

The oxidation number of hydrogen (H) in H2SO4 is +1.

The oxidation number for Sn (tin) can vary depending on the compound it is in. In the most common compounds, like SnCl2, Sn is typically in the +2 oxidation state. In other compounds, such as SnCl4, Sn can have an oxidation state of +4.

For an uncombined atom, the oxidation number is 0. It does not give away any electrons. It does not accept electrons from anywhere either.

The oxidation number of silver in Ag2O is +1. In Ag2O, there are two silver atoms each having an oxidation state of +1. Oxygen has an oxidation state of -2.

Transition metals are the most likely elements to have various oxidation numbers due to their unstable electron configuration and ability to gain or lose electrons easily. Examples include iron, copper, and chromium.

The oxidation numbers in a neutral compound must equal zero. This is because the overall charge of a neutral compound is zero, so the sum of the oxidation numbers must balance out to zero.

The sum of oxidation numbers in a compound is zero for a neutral compound and equal to the charge of the ion for an ionic compound. This rule stems from the fact that the total charge of a compound must be zero for a neutral compound and must balance out for an ionic compound.

The oxidation number of an atom in its elemental form is 0. This is because there is no transfer of electrons between atoms of the same element, resulting in a neutral charge.

The oxidation number for K in KCl is +1, as alkali metals (Group 1 elements) typically have a +1 oxidation state. For Cl in KCl, the oxidation number is -1, as halogens (Group 17 elements) typically have a -1 oxidation state when they form ionic compounds.

In a combustion reaction, the oxidation number of hydrogen in water is +1 and the oxidation number of oxygen is -2. The oxidation number of an element in a compound represents the charge it would have if all shared electrons were assigned to the more electronegative element.

The oxidation number for iodine in iodine pentoxide (I2O5) is +5. This is determined by taking into account the overall charge of the compound and the known oxidation number of oxygen atoms in a molecule.

+3 in its compounds

0 in elemental form

Its no one cares makw it up because Ms. D gives s to much homework likwe it up

Arsenic is in group 15, it can lose 5 valence electrons or gain 3 valence electrons to achieve the octet. Its minimum oxidation state we can predict as being -3, and its maximum as +5

Ah, the oxidation number of Cl in ClO is -1. You see, in compounds, oxygen usually has an oxidation number of -2, so in this case, chlorine takes on a +1 oxidation number to balance it out. It's all about finding that perfect harmony in chemistry, just like adding the right colors to a painting.

To find the oxidation number or charge of a polyatomic ion, consider the known charges of the individual atoms within the ion. For example, in the sulfate ion (SO4)2-, oxygen typically has an oxidation number of -2, and sulfur would then have an oxidation number to balance the charge of the ion. The sum of the oxidation numbers of all the atoms in the ion should equal the overall charge of the ion.

In NH4₂SO3, the oxidation number of N is -3 (since H is +1), the oxidation number of S is +3, and the oxidation number of O is -2. The sum of the oxidation numbers in a neutral compound is always zero, so the oxidation number of H is +1.

0 in the elemental form, +3 in its compounds.

+1 only for all elements (except for hydrogen)

hydrogen can have +1 and -1 as their oxidation numbers.

The oxidation number of sulfur in Li2SO4 is +6. This is because the oxidation numbers of Li and O are +1 and -2 respectively, and in a neutral compound the sum of all oxidation numbers must equal zero.

+1 for Na

-1 for Cl

0 in elemental form, +3 in its compounds

Elemntal argon has an oxidation number of zero. The only compound known (aunstable and only very small amounts made at low temperature) HArF has an oxidation number of zero also!