I am not sure but I think it means that the compound Cupper Sulphate can have different oxidation states depending on the valency of copper.Cheman said:
Cheman said:I have read that the "idea of oxidation states is contrived." Why then do we use the idea and why does it work if it is not really the case? Why should we suppose everything acts like its ionic, etc?
Thanks.
Oxidation states, also known as oxidation numbers, are a measure of the electron distribution in a compound or molecule. They indicate the charge that an atom would have if all of its bonds were 100% ionic.
Oxidation states work because they help us understand the distribution of electrons in a molecule or compound. They allow us to determine how many electrons have been lost or gained by an atom, which can help us predict its reactivity and chemical behavior.
The oxidation state of an element can be determined by looking at its position on the periodic table, as well as the number of valence electrons it has. In general, elements in the same group or column will have the same oxidation state.
Oxidation states and formal charges are both ways to represent the distribution of electrons in a molecule or compound. However, formal charges take into account all of the valence electrons in an atom, while oxidation states only consider the bonding electrons. Additionally, formal charges can be fractional, while oxidation states are always whole numbers.
Oxidation states are important in chemistry because they help us understand the reactivity and behavior of elements and compounds. They also play a crucial role in balancing redox reactions and predicting the products of chemical reactions. Additionally, they are used in naming and classifying compounds.