Redox

Question 1

What is an oxidation number?

Answer 1

A measure of the number of electrons that an atom uses to bond with an atom of another element

Question 2

How many rules is there?

Answer 2

10

Question 3

What is rule 1?

Answer 3

Elements oxidation number = zero

Question 4

What is rule 2?

Answer 4

Monoatomic ion oxidation number = charge of ion

Na+ = +1

Question 5

What is rule 3?

Answer 5

Sum of oxidation numbers in neutral compound = zero

Question 6

What is rule 4?

Answer 6

Sum of oxidation number in polyatomic ion = charge on ion

CO2 3- = -3

Question 7

What is rule 5?

Answer 7

Oxidation numbers of compounds in:
Group 1 = +1
Group 2= +2
Group 3 = +3

Question 8

What is rule 6?

Answer 8

Oxidation number of H normally is +1 but with a metal it is -1

Question 9

What is rule 7?

Answer 9

F’s oxidation number = -1 in compounds

Question 10

What is rule 8?

Answer 10

O’s oxidation number is normally -2 but in a peroxide it is
-1
And bonded with F it is +1

Question 11

What is rule 9?

Answer 11

Transition metals’ oxidation number can vary

Question 12

What is rule 10?

Answer 12

Cl, Br + I usually -1 except when in a compound with oxygen

Question 13

What is the Roman numerals of SnO2?

Answer 13

Tin (IV) oxide

Question 14

What is the Roman numerals of Mn(OH)2?

Answer 14

Manganese (II) hydroxide

Question 15

What is oxidation?

Answer 15

Loss of electrons

Question 16

What is reduction?

Answer 16

Gain of electrons

Question 17

What is a disproportionation reaction?

Answer 17

The same element is oxidised and reduced at the same time

Question 18

How can you tell if an element has been oxidised or reduced using oxidation states?

Answer 18

Oxidation number increases = oxidised

Oxidation number decreases = reduced

Question 19

Which element is the reducing agent?

Answer 19

The one that has been oxidised

Question 20

Which element is the oxidising agent?

Answer 20

The one that has been reduced