Why are electrons not removed?
I am currently going over the topic of redox reactions and oxidation states. I was watching this video on half equations and how to write them. But mostly all of the videos said that electrons need to be added always and not removed. So you put the electrons on the side of the equation where they will be added and not removed.
For example:
Fe (+2). + 2e- ------->. Fe.
But it cannot be
Fe (+2) --------> Fe - 2e-
But why?
For example:
Fe (+2). + 2e- ------->. Fe.
But it cannot be
Fe (+2) --------> Fe - 2e-
But why?
Reply 1
Is is because the oxidation states need to add up to zero?
Reply 2
12
Original post
by HelloeveryoneeI am currently going over the topic of redox reactions and oxidation states. I was watching this video on half equations and how to write them. But mostly all of the videos said that electrons need to be added always and not removed. So you put the electrons on the side of the equation where they will be added and not removed.
For example:
Fe (+2). + 2e- ------->. Fe.
But it cannot be
Fe (+2) --------> Fe - 2e-
But why?
For example:
Fe (+2). + 2e- ------->. Fe.
But it cannot be
Fe (+2) --------> Fe - 2e-
But why?
For the example you gave, it's because the oxidation number wants to be at 0. The first one is right because +2 + 2e- = 0. The second one is basically saying +2 - -2, so you would end up with Fe (+4)
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