Redox Flashcards
What is a redox reaction?
A reaction involving a transfer of electrons from the reducing agent to the oxidising agent.
What is oxidation?
The process of electron loss.
What are oxidising agents?
Electron acceptors.
What is reduction?
The process of electron gain.
What are reducing agents?
Electron donors.
How is the change in oxidation state used in redox reactions?
To identify the element that has been oxidised or reduced.
What is written to represent the oxidation and reduction processes in redox reactions?
Separate half-equations.
What can be combined to give an overall equation for any redox reaction?
Half-equations.
What should students be able to work out from a compound or ion’s formula?
The oxidation state of an element.
Fill in the blank: Oxidation is the process of electron loss, and _______ are electron acceptors.
oxidising agents
Fill in the blank: Reduction is the process of electron gain, and _______ are electron donors.
reducing agents
True or False: In redox reactions, the oxidation state of an element can change.
True
What is the primary skill students should develop regarding half-equations in redox reactions?
Writing half-equations identifying the oxidation and reduction processes.
What are the two main processes involved in a redox reaction?
- Oxidation
- Reduction
What is a reducing agent?
An electron donor that gets oxidised as it donates electrons
A reducing agent facilitates the reduction of another substance while being oxidised itself.
What is an oxidising agent?
An electron acceptor that gets reduced as it gains electrons
An oxidising agent facilitates the oxidation of another substance while being reduced itself.
What is the half-equation for the oxidation of sodium?
Na → Na⁺ + e⁻
This reaction indicates that sodium loses an electron, which is characteristic of oxidation.
What type of reaction does the half-equation Fe³⁺ → Fe²⁺ + e⁻ represent?
Oxidation
In this half-equation, iron is losing an electron, which categorizes it as oxidation.
Complete the fill-in-the-blank: In the half-equation O₂ + 2 e⁻ → 2 O²⁻, oxygen is undergoing _______.
reduction
Oxygen is gaining electrons, indicating that it is being reduced.
What is the half-equation for the reduction of nitrogen
2N₂ + 3 e⁻ → 2 N³⁻
This half-equation shows nitrogen gaining electrons, which is a reduction process.
What is the half-equation for the reaction involving manganese in acidic conditions?
8H⁺ + MnO₄⁻ → Mn²⁺ + 4H₂O
This reaction shows the reduction of permanganate ion to manganese ion in an acidic medium.
What is the half-equation for the reduction involving dichromate?
14H⁺ + Cr₂O₇²⁻ → 2Cr³⁺ + 7H₂O
This half-equation illustrates the reduction of dichromate ion to chromium ion in acidic conditions.
What is the oxidation state of uncombined elements?
0
Uncombined elements like Mg, Na, O2, H2, and C2 have an oxidation state of zero.
What is the sum of all oxidation states in a neutral compound?
0
The oxidation states in a compound such as NaCl sum up to zero.
