Consider the following unbalanced equation between copper(I) ions and iron to produce copper metal and iron(II) ions: Cu+ + Fe → Cu + Fe2+ What is oxidized in this reaction?
A) copper(I) ion
B) iron
C) copper
D) iron(II) ion
Remember the definitions.
Oxidation is the loss of electrons.
So Cu goes from +1 to zero and iron goes from zero to +2. Which loses electrons?
Hi, I'm a 10th grade student and this is how I would look at it...
So what is being oxidized is what is losing electrons.
So take Copper for example.
Copper is going from a 1+ charge to no charge as a solid...so is it gaining an electron or losing.
Now think of Iron.
Iron is going from no charge to a charge of 2+. So would that be losing electrons or gaining?
Whichever element loses the electrons would be oxidized in this reaction.
Hope this helps!
To determine what is being oxidized in the given reaction, we need to look at the changes in oxidation states of different elements.
In the reaction, the copper(I) ion (Cu+) is being converted into neutral copper (Cu), while the iron is being converted from neutral to an iron(II) ion (Fe2+).
The oxidation state of copper is increasing from +1 to 0, indicating that copper(I) ion is being oxidized.
On the other hand, the oxidation state of iron is decreasing from 0 to +2, indicating that iron is being reduced.
Based on this information, we can conclude that the element being oxidized in this reaction is the copper(I) ion.
Therefore, the correct answer is:
A) Copper(I) ion
To determine what is oxidized in the reaction, we need to identify the elements that undergo a change in oxidation state.
In this reaction: Cu+ + Fe → Cu + Fe2+
The oxidation state of copper(I) ions changes from +1 to 0. This means that copper(I) ions are reduced, as their oxidation state decreases.
On the other hand, the oxidation state of iron changes from 0 to +2. This means that iron is oxidized, as its oxidation state increases.
Therefore, the element that is oxidized in this reaction is iron.
The answer is B) iron.