Redox

Question 1

Define oxidation in terms of oxygen

Answer 1

An element gains oxygen to form an oxide

Question 2

Define oxidation in terms of electrons

Answer 2

Loss of electrons

Question 3

Define oxidation in terms of oxidation numbers

Answer 3

An element is oxidised if it’s oxidation number increases

Question 4

What is the oxidising agent

Answer 4

The reactant which gains electrons

Question 5

1 What is the oxidation state of uncombined elements

Answer 5

0

Question 6

2 What is the oxidation state of monatomic ions

Answer 6

Charge

Question 7

3 What is the sum of oxidations states in a compound

Answer 7

Overall charge

Question 8

4 What is the oxidation state of Group 1 atoms (in a compound)

Answer 8

+1

Question 9

5 What is the oxidation state of Group 2 atoms (in a compound)

Answer 9

+2

Question 10

6 What is the oxidation state of Flourine (in a compound)

Answer 10

-1

Question 11

7 What is the oxidation state of Hydrogen (in a compound)

Answer 11

+1

Question 12

8 What is the oxidation state of Oxygen (in a compound)

Answer 12

-2

Question 13

9 What is the oxidation state of Chlorine (in a compound)

Answer 13

-1

Question 14

Describe what is meant by a redox reaction

Answer 14

Any reaction in which oxidation states change

Question 15

Describe what is meant by Disproportionation reactions

Answer 15

Reactions in which an element is both oxidised and reduced at the same time.

Question 16

Do all disproportionation reactions count as redox reactions? Explain why

Answer 16

All disproportionation reactions involve changes in oxidation state, so they all count as redox reactions.

Question 17

What is the reducing agent

Answer 17

The reactant that gains an electron

Question 18

Describe what is meant by a double displacement reaction

Answer 18

Not a redox reaction because the oxidation state remains the same