Let’s take a closer look at Oxidation States (Module 3 Preliminary Chemistry)
Hosted by our Talent 100 Academic Director Dr Nikhil Vasan, we’re going to break down a few of the most important topics for each section of Module 3: Metal Activity Series and Displacement Reactions for Preliminary Chemistry (Year 11).
In this episode of Preliminary Chemistry Talent Teaching Series, we’re going to explore the difficult topic of Oxidation State, and show you a really easy rule to remember the rules of Redox.
Now that we’ve gone through Redox Reactions, we’re going to take a bit of time and go through Oxidation States. This might give us a little more clarity as to why we use the terms oxidation and reduction in that we looked at in our previous blog on Year 11 Preliminary Chemistry: Redox Reactions.
What are Oxidation States?
An oxidation state of a particular element or substance refers to essentially how much above or below neutral its charge or electron content is. Using the same example we did earlier in Redox Reactions, let’s pick Magnesium and we’ll show it getting oxidised. Remember, that oxidation is the loss of electrons!
We’ll also use Fluorine gas which will gain a couple of electrons (probably donated from the Magnesium).
To find out how oxidation states work, catch the rest of Nikhil’s revision lesson by watching the video below:
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