How to find the Oxidation Number for I in the ICl4 ion

>> YOUR LINK HERE: ___ http://youtube.com/watch?v=ypC3uaCaOy4

To find the correct oxidation state of I in ICl4 - (the Tetrachloroiodide ion), and each element in the ion, we use a few rules and some simple math. • First, since the Tetrachloroiodide Ion has an overall charge of 1- we could say that the oxidation numbers in ICl4 - need to add up to charge on the ion. • We write the oxidation number (O.N.) for elements that we know and use these to figure out oxidation number for I. • • --------- • RESOURCES • How to Find Oxidation Numbers (rules and examples): • How to Find Oxidation Numbers (Rules... • Oxidation Numbers Practice: • Finding Oxidation Numbers Practice Pr... • ---------- • GENERAL RULES • Free elements have an oxidation state of zero (e.g. Na, Fe, H2, O2, S8). • In an ion the all Oxidation numbers must add up to the charge on the ion. • In a neutral compound all Oxidation Numbers must add up to zero. • Group 1 = +1 • Group 2 = +2 • Hydrogen with Non-Metals = +1 • Hydrogen with Metals (or Boron) = -1 • Fluorine = -1 • Oxygen = -2 (except in H2O2 or with Fluorine) • Group 17(7A) = -1 except with Oxygen and other halogens lower in the group • ---------- • We know that Oxygen usually is -2 with a few exceptions. When Oxygen is in a peroxide, like H2O2 (Hydrogen peroxide), it has a charge of -1. When it is bonded to Fluorine (F) it has an oxidation number of +1. • Here it is bonded to I so the oxidation number on Oxygen is -2. Using this information we can figure out the oxidation number for the element I in ICl4 -.

#############################

New on site