what is the oxidation state of chlorine in Cl2O7
The oxidation number of oxygen is always -2.
Therefore (2×Cl) + (-2×7) = 0, and so Cl = 7, i.e. the oxidation number of chlorine = 7
+7 for each Cl.
Hydrogen carries +1 charge, so for two Hydrogen +2, so for one oxygen atom -1 charge, because it is peroxide
To determine the oxidation state of chlorine in Cl2O7, we need to assign oxidation states to each element in the compound.
Let's first understand the concept of oxidation state:
The oxidation state of an atom in a compound refers to the hypothetical charge that atom would have if all bonds in the compound were purely ionic. It is a way to keep track of the distribution of electrons in a molecule.
Here, Cl2O7 is a binary compound consisting of chlorine (Cl) and oxygen (O). Oxygen is known to have an oxidation state of -2 in most compounds unless it is bonded to fluorine (F) or in a peroxide (O22-) where it has an oxidation state of -1.
To find the oxidation state of chlorine (Cl), we can set up an equation:
2x + 7(-2) = 0
In this equation, 2x represents the total oxidation state of the two chlorine atoms, and 7(-2) represents the total oxidation state of the seven oxygen atoms.
By solving the equation, we can find the value of x, which represents the oxidation state of chlorine.
2x - 14 = 0
2x = 14
x = 7
Therefore, the oxidation state of chlorine in Cl2O7 is +7.