Skip main navigation

£199.99 £139.99 for one year of Unlimited learning. Offer ends on 28 February 2023 at 23:59 (UTC). T&Cs apply

Find out more

Natural antioxidants: Vitamin C

Vitamin C is an anti-oxidant. It participates in processes where it is repeatedly reduced (gains an electron) and oxidised (loses the electron).
Broccoli in a wooden crate
© UEA and Biochemical Society, 2018. This work is licensed under a Creative Commons Attribution-NonCommercial 4.0 International License.

Many natural products found in foods directly influence reactions that are involved in cellular metabolism. This is the case for some of the vitamins that are found widely in foods, including vitamin C, which acts as an “antioxidant”.

Oxidation was originally the term used for combining a substance with oxygen. This is what happens when we burn a fuel, such as a candle, which releases energy as heat and light. In this case the fuel has been oxidised – combined with oxygen.

In biochemistry, the term oxidation has a broader meaning: it means the loss of electrons. When there is something in a reaction that can be identified as being oxidised, and thus losing electrons, there must also be something that can gain them. A substance which accepts electrons in this way is said to be reduced. Many chemical reactions rely on the transfer of electrons in this way. As there is both a REDuction and an OXidation these are referred to as redox reactions.

It can be tricky to remember the distinctions between oxidation and reduction. A number mnemonics have been developed to help remember the distinction and you may have heard of some of these. One that is well known is “OIL RIG”, where each letter describes what is happening to the electrons, like so:
Oxidation Is Losing (Electrons), Reduction Is Gaining (Electrons)

Redox reactions drive many processes around us. Batteries rely on redox reactions, but instead of the electrons being transferred directly to another atom or molecule they are forced to flow around a circuit. Many biological processes, such as photosynthesis that we heard about in week 2 of this course, rely on such electron transfer reactions where molecules repeatedly become reduced (gain an electron) and oxidised (lose the electron again) to store and release energy.

These types of redox properties can be used to measure the amount of vitamin C in a sample. Not only is vitamin C a vitamin but it is an anti-oxidant, which means that it can act to reduce other substances. If combined with molecules that change colour when they are reduced (or oxidised), this allows an indicator system to be set up that measures the amount of vitamin C. An example of such a system involves starch and iodine and we will see an experiment that exploits such a system in the next steps in the course.

© UEA and Biochemical Society, 2018. This work is licensed under a Creative Commons Attribution-NonCommercial 4.0 International License.
This article is from the free online

Biochemistry: the Molecules of Life

Created by
FutureLearn - Learning For Life

Our purpose is to transform access to education.

We offer a diverse selection of courses from leading universities and cultural institutions from around the world. These are delivered one step at a time, and are accessible on mobile, tablet and desktop, so you can fit learning around your life.

We believe learning should be an enjoyable, social experience, so our courses offer the opportunity to discuss what you’re learning with others as you go, helping you make fresh discoveries and form new ideas.
You can unlock new opportunities with unlimited access to hundreds of online short courses for a year by subscribing to our Unlimited package. Build your knowledge with top universities and organisations.

Learn more about how FutureLearn is transforming access to education