Redox Reactions

Flashcards covering the key concepts of redox reactions, including definitions, processes, and methods for balancing equations.

What is oxidation in a redox reaction?

Oxidation is the process where a species loses one or more electrons.

What is reduction in a redox reaction?

Reduction is the process where a species gains one or more electrons.

What always occurs together in redox reactions?

Oxidation and reduction always occur together; if one species is oxidized, another must be reduced.

What does an increase in oxidation number indicate?

An increase in oxidation number indicates that an atom has lost electrons and therefore has been oxidized.

What does a decrease in oxidation number indicate?

A decrease in oxidation number indicates that an atom has gained electrons and therefore has been reduced.

How is the oxidation state of an uncombined element defined?

The oxidation state of an atom in an uncombined element is 0.

What are the oxidation states of group 1 and group 2 elements?

Group 1 elements have an oxidation state of +1 and group 2 elements have an oxidation state of +2.

What is the oxidation state of fluorine in compounds?

Fluorine always has an oxidation state of -1 in compounds.

What method can be used to balance redox reactions?

The half equation method and the oxidation number method can both be used to balance redox reactions.

In the oxidation of Fe2+ to Fe3+, what is the element that is oxidized?

The Fe2+ ion is oxidized to Fe3+.

What is a reducing agent?

A reducing agent is a species that donates electrons during a redox reaction and gets oxidized.

What is an oxidizing agent?

An oxidizing agent is a species that accepts electrons during a redox reaction and gets reduced.

How do you calculate n in the context of ammonium iron(II) sulfate crystals?

By using the mass dissolved, concentration of KMnO4, and the volume titrated to find the number of moles of Fe, then solving for n.