Redox Reactions Flashcards
Category: Definitions of Redox
What is the definition of redox reactions in terms of oxygen gain or loss?
Oxidation refers to the gain in oxygen while reduction is the loss of oxygen.
Category: Definitions of Redox
What is the definition of redox reactions in terms of hydrogen gain or loss?
Oxidation refers to the loss of hydrogen while reduction is the gain in hydrogen.
Category: Definitions of Redox
What is the definition of redox reactions in terms of electron gain or loss?
Oxidation is the loss of electrons while reduction is the gain in electrons.
Category: Definitions of Redox
What is the definition of redox reactions in terms of increase or decrease in oxidation state?
Oxidation refers to the increase in oxidation state while reduction is the decrease in oxidation state.
Oxidation state is the hypothetical charge that an atom of an element would have if all bonds to atoms of different elements are fully ionic.
E.g oxidation state of Na in NaNO3 would be +1. even though the ionic compound is electrically neutral.
Category: Definitions of Redox
What is the oxidation state of a free element?
It is 0.
Category: Definitions of Redox
What is the O.S of a simple ion? (e.g F-)
The O.S of a simple ion is equal to the charge on the ion. For example, the oxidation state of F- would be -1.
Category: Definitions of Redox
What is the O.S of oxygen when combined with F, or it is in a peroxide?
The oxidation state of O when combined with F is (+2), not (-2).
The oxidation state of O when it is in a peroxide is -1.
Category: Definitions of Redox
What is the O.S of hydrogen when combined with a metal?
The oxidation state of hydrogen when combined with a metal is -1.
E.g NaH
Category: Definitions of Redox
What is the sum of the oxidation state of all atoms in a neutral compound?
The sum of all O.S is zero.
Category: Definitions of Redox
What is the sum of the oxidation state of all atoms in a polyatomic ion equal to?
The sum of O.S of a polyatomic ion is equal to the charge of the ion.
Category: Oxidising and Reducing agents
What is an oxidising agent?
An oxidising agent oxidises another substance and is itself reduced.
Category: Oxidising and Reducing agents
What are some common examples of an oxidising agent?
Common examples include oxygen, concentrated sulphuric acid, acidified potassium manganate, acidified potassium dichromate.
Category: Oxidising and Reducing agents
What is a reducing agent?
A reducing agent reduces another substance and is itself oxidised.
Category: Oxidising and Reducing agents
What are some common examples of a reducing agent?
Some common examples of reducing agents include hydrogen, carbon, carbon monoxide, sulphur dioxide, aqueous potassium iodide.
Category: Test for Oxidising and Reducing Agents
Describe the test for oxidising agent, making use of the appropriate reducing agent.
test for oxidising agent using a reducing agent. The reducing agent added should be aqueous potassium iodide. The observation observed would be the colourless solution turning brown.
This is because the iodide ion (I-) is colourless. However, during the reaction it is oxidised to form I2, which is brown in solution.
Category: Test for Oxidising and Reducing Agents
How does one test for a reducing agent?
Name the appropriate oxidising agent used.
By making use of acidified potassium manganate(VII), KMnO4.
The observation made would be the purple solution turns colourless. This is due to the MnO4- ion being purple in colour, but after the reaction, it is reduced to Mn2+ which is colourless.
The same observation would be made if a reducing agent (H2O2) were to be used, as the reaction would yield the same ion, Mn2+.
