Summary
Summary Unit 13 Assignment B
- Module
- Unit 13
- Institution
- PEARSON (PEARSON)
Qualification Distinction Pearson BTEC Level 3 National Diploma in Applied Science Pearson BTEC Level 3 National Extended Diploma in Applied Science
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Being oxidised is the process of oxidation. The removal of oxygen is the process of reduction.When an atom, molecule, or ion loses one or more electrons during a chemical reaction,
oxidation takes place. In a type of chemical reaction known as a reduction-oxidation or redox
reaction, reduction and oxidation take place at the same time.
A chemical that oxidises is referred to as an "oxidising agent." An oxidising agent constantly
reduces because it receives electrons from the species it oxidises. Tracking the transport of
electrons is done using a number called the oxidation number. Ionic and molecular
substances are both assigned oxidation numbers. The half-reaction that causes the loss of
electrons is the oxidation reaction. Redox reactions are oxidation-reduction processes that
also involve electron transport. As electrons are transferred, the oxidation number of various
substances changes. When a molecule undergoes reduction, it appears as though it is
gaining electrons. It's connected to a drop in oxidation number. A reduction reaction is a
half-reaction in which electrons are gained. A reducing agent is a species that lessens the
amount of something. Because a reducing agent constantly donates electrons to the species
it reduces, it is always oxidised.
Redox (oxidation-reduction) reactions are common in our surroundings. The burning of fossil
fuels and the oxidising properties of sodium hypochlorite, the main component in home
bleach, are just a few of these processes or reactions. We have all probably come across at
least one redox reaction or characteristic at some point in our lives. Rust on iron, tarnish on
cutlery and greening on copper or brass surfaces or materials are all signs of corrosion that
we can see all around us. These constant changes that we witness without even recognising
it You can observe redox reactions at work by looking at their chemical makeup or origin. By
oxidation or reduction reactions, many of the metallic and non-metallic elements used in
modern life are extracted from their ores. These are only a few examples of the effects of
oxidation-reduction reactions. These are electron-transfer processes in their purest form.
Over the years, oxidation-reduction analysis has been employed as an alternative technique
for assessing materials with a variety of oxidation states.
The elements with a higher oxidation number for example, such as hydrogen and sulphur,
are oxidised. Because the amount of chlorine and oxygen has been decreased, their
oxidation values are lower than before. In HCl, the sum of the H and Cl oxidation values (+1
and -1) is zero, which is important to know. Combining the changes on S (+4) and the two
atoms of O [2x (-2) yields zero. Because the HCl and SO2 molecules are both neutral, the
charges must balance out.
Titration is a typical analytical method used in the food industry. It enables food producers
to calculate the amount of reactant in a sample. It can be used to identify a product's salt or
sugar content as well as how much vitamin C or E is present, all of which have an impact on
the product's colour.
Kits for oxygen demand.
A wastewater metric called chemical oxygen demand counts how much of a particular
oxidant is present after it reacts under controlled circumstances with organic material. A
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