I- is converted into I2 by the addition of an aqueous solution of KMnO4 to an aqueous solution of KI. What is the oxidation number assigned to I2??
wallah ani ma3rf. Bas ga3d en6adther ila an akhlas hal khara
To determine the oxidation number assigned to I2 in the given reaction, we can follow these steps:
Step 1: Determine the oxidation number of K (potassium).
The oxidation number of an alkali metal, such as potassium (K), is +1.
Step 2: Determine the oxidation number of O (oxygen).
The oxidation number of oxygen is typically -2, except in peroxides where it is -1 (which isn't the case here).
Step 3: Assign the oxidation number of Mn (manganese) in KMnO4.
Since there are four oxygen atoms in KMnO4, and the total charge of oxygen is -8 (4 × -2), the oxidation number of Mn can be determined by the equation:
Oxidation number of Mn + 4(-2) = -1 (the charge of KMnO4)
Oxidation number of Mn - 8 = -1
Oxidation number of Mn = -1 + 8
Oxidation number of Mn = +7
Step 4: Determine the oxidation number of I (iodine) in I2.
Let the oxidation number of I in I2 be x.
Since there is no charge specified, we assume the total charge to be zero since I2 is a neutral molecule.
According to the equation, the sum of the oxidation numbers of all atoms in a neutral molecule is zero.
So, 2x = 0
x = 0/2
x = 0
Therefore, the oxidation number assigned to I2 in the reaction is 0.
To determine the oxidation number assigned to I2, we need to understand the concept of oxidation numbers and the rules for assigning oxidation numbers in a compound.
Oxidation number is a concept used to keep track of electron transfers during chemical reactions. It is a positive or negative number that represents the hypothetical charge an atom would have if all its bonds were 100% ionic.
In this case, we are considering the reaction where I- is converted into I2 by the addition of KMnO4 to KI. The reaction can be represented as follows:
2 I- + 2 KMnO4 + H2O → I2 + 2 MnO2 + 2 KOH
Here are the steps to determine the oxidation number assigned to I2:
1. Identify the oxidation numbers of other elements in the reaction. In this case, manganese (Mn) has an oxidation number of +7 in KMnO4, and potassium (K) has an oxidation number of +1 in KI.
2. Determine the total charge of I2 in the reaction. Since we know that the overall charge of the compound should be zero, we can use the oxidation numbers of the other elements to calculate the oxidation number of I2.
In KMnO4, the total oxidation number of MnO4 is -1 (since it is a polyatomic ion with an overall charge of -1) and the total oxidation number of potassium (K) is still +1. Therefore, for the compound to have a total charge of zero, the oxidation number of I2 must be +2.
So, the oxidation number assigned to I2 in this reaction is +2.