The oxidation number of an element essentially tells you the charge that an element would like to achieve by bonding in order to either fill an octet of electrons or lose an outer layer of electrons exposing an octet. For example, a neutral oxygen atom will have 6 valence electrons so in order to have a full set of 8, it wants to gain 2 electrons, and since an electron has a negative charge, it has an oxidation number of -2. Sodium on the other hand has 1 valence electron, and its easier to lose this one then gain 7 more, so when it losses this electron, it will have more positive charges in the nucleus than negative charges, giving it an oxidation number of +1.
Oxidation numbers are important in bonding because it determines the ratio of elements needed. In general, compounds need to be neutral, meaning the sum of the oxidation numbers of its elements must be 0. For example, Magnesium has an oxidation number of +2 and Chlorine of -1. To cancel out, you need to have 2 Chlorine per Magnesium, meaning the result will be MgCl2.
Zero The oxidation number of an element in any of its elemental forms (allotropes) is always zero
The halogens (group 17) have an oxidation number of -1, though the halogens below fluorine can have other oxidation numbers as well. Hydrogen can also have an oxidation number of -1 when it forms hydrides.
Phosphorous, or P, has a zero oxidation number in the element. Common oxidation numbers are:- It has a -3 in phosphides, where it forms the P3- ion It has a +3 in oxidation number in for example P4O6, and PCl3 It has a +5 oxidation number in for example P4O10 and PCl5
The oxidation state (or number) is zero. This is true for any element in any of its allotropic elemental forms.
The oxidation state (or number) is zero. This is true for any element in any of its allotropic elemental forms.
Zero The oxidation number of an element in any of its elemental forms (allotropes) is always zero
The halogens (group 17) have an oxidation number of -1, though the halogens below fluorine can have other oxidation numbers as well. Hydrogen can also have an oxidation number of -1 when it forms hydrides.
Phosphorous, or P, has a zero oxidation number in the element. Common oxidation numbers are:- It has a -3 in phosphides, where it forms the P3- ion It has a +3 in oxidation number in for example P4O6, and PCl3 It has a +5 oxidation number in for example P4O10 and PCl5
Selenium forms selnides which contain the ion Se2-.
The oxidation state (or number) is zero. This is true for any element in any of its allotropic elemental forms.
The oxidation state (or number) is zero. This is true for any element in any of its allotropic elemental forms.
Oxidation number is a concept that refers to atoms not molecules. The oxidation number of S in S8 is zero. The oxidation number of an atom in the pure element is always 0. S8 is a form of sulfur, the most commonly encountered , there are many other forms (allotropes). The oxidation number of S in any of its allotrpes is zero.
As it forms the I- ion froming an octet its most likely oxidation number is -1
there are two for silicone.those are 0 and 4.Atomic silicon has oxidation number 0. It forms a wide variety of compounds, specially with oxygen. In these compounds, the oxidation number of silicon can vary from 0 to +4.
Carbon is the element that forms maximum number of compounds
Ammonium, NH4, forms a +1 ion.
If the question is Cu2, then it is equivalent to Cu and the oxidation number for any element is zero. If the question is Cu2+, then the oxidation number is +2.