what is the oxidation no of I3-
I3- is
I2 + I-.
The oxidation number of the ion, as shown, is -1 which makes each I a -1/3. I often balance the equation as I2, then add the I^- as needed. It saves wear and tear on the fractions.
-1/3
This would be correct for i3-
Well, I3- is a negative ion, so it's already a little charged up. I like to think of it as a trio of bullies in a gang, but they're not very strong bullies because they have a negative charge. Anyway, the oxidation number of each iodine atom in I3- is -1/3. So, the gang of bullies collectively has an oxidation number of -1. Just remember, they might be bullies, but they're negative bullies.
To determine the oxidation number of I3-, first, we need to understand the concept of oxidation numbers. Oxidation numbers, also known as oxidation states, are hypothetical charges assigned to each atom in a compound or ion. These numbers are based on the assumption that electrons in a chemical bond are shared unequally.
In I3-, there are three iodine atoms (I) bonded together. Since iodine belongs to Group 17 or Group 7A of the periodic table, it has seven valence electrons. Considering the octet rule, each iodine atom tends to gain one electron to achieve a stable configuration.
Let's assign the oxidation number of iodine in I3- as x.
Since there are three iodine atoms, the total number of electrons gained by them is 3x.
Now, we know that the overall charge of I3- is -1.
Therefore, the equation can be written as: 3x = -1
To solve for x, we divide both sides of the equation by 3:
x = -1/3
So, the oxidation number of iodine in I3- is -1/3.