Redox

Question 1

For oxidation and reduction which does oxidation state increase and decrease for

Answer 1

Oxidation : oxidation state increases
Reduction : Oxidation state decreases

Question 2

What is a disproportionation reaction

Answer 2

When the same element gets oxidised and reduced

Question 3

Define
a) oxidising agent
b) reducing agent

Answer 3

a) electron acceptor
b) electron donor

Question 4

Which of these species is the best reducing agent?
A Cl2
B Cl−
C I2
D I−

Answer 4

Cl2 and I2 are both oxidising agents
Reducing agents lose electrons
In the halide ions (Cl⁻ and I⁻), the outermost electron is the one that would be lost in oxidation.
Iodine is a larger atom than chlorine — it has more electron shells.
That means the outermost electron in I⁻ is farther from the nucleus and less tightly held.
As a result, it’s easier to remove that electron from I⁻ than from Cl⁻.
So, I⁻ gives up electrons more easily, making it a stronger reducing agent.
Answer : D

Question 5

Order of oxidation states

Answer 5

• Uncombined elements (0)
• Metals
• Fluorine (−1)
• Hydrogen (+1)
• Oxygen (−2)
• Chlorine (−1)
  Under My Face Here’s Our Chin

Question 6

Answer 6

A) copper gets reduced as it gains an electron
B) Oxidation of Fe decreases from 3+ to 2+, hence it is reduced
C) Another ligand substitution like Fe, however unlike Fe, Co stays at 2+ throughout, no redux just coordination change
D) Mg becomes Mg^2+ hence it is oxidised
Correct answer : D

Question 7

A solution of sodium chlorate(I) was added to a colourless solution of potassium iodide. Suggest what is observed. Explain the reaction that leads to this observation.

Answer 7

Mark scheme answer :
Goes brown
Due to iodine
Because I^- is oxidised

Question 8

Answer 8

Question 9

Use answer to Q16 to help with Q17

Answer 9

Question 10

Answer 10

A