Redox

Question 1

Oxidation

Answer 1

Loss of electrons

Question 2

reduction

Answer 2

gain of electrons

Question 3

Oxidising agent

Answer 3

A reagent that oxidises another species

Electron acceptor

Question 4

Reducing agent

Answer 4

A reagent that reduces another species

electron donor

Question 5

Redox reactions

Answer 5

Reduction-oxidation reactions, describes reactions where electrons are transferred from one species to another

Question 6

Half equation

Answer 6

Equations for redox reactions that only considers one species involved and explicitly shows the electrons transferred

Question 7

What is the procedure for writing half equations?

Answer 7

1. Balance the main element atoms
2. Balance the oxygens with water
3. Balance the hydrogens with H+ions
4. Balance the charges with electrons

Question 8

Oxidation states

Answer 8

Used to see what has been oxidised and what has been reduces in a redox reaction

Question 9

What should the oxidation states add up to in a compound?

Answer 9

Oxidation states in a compound should equal zero.

Question 10

Which metal elements have fixed oxidation states in compounds?

Answer 10

Group 1 (+1), Group 2 (+2) and Group 3 (+3)

Question 11

When does oxygen not have an oxidation state of -2?

Answer 11

When in peroxides eg. H2O2 where it is -1

Question 12

When is hydrogen not +1?

Answer 12

When in metal hydrides eg NaH where it is -1

Question 13

What is the oxidation state of Hydrogen usually?

Answer 13

Hydrogen: +1

Question 14

What is the oxidation state of Oxygen usually?

Answer 14

Oxygen: -2

Question 15

What is the oxidation of Fluorine in it’s compounds?

Answer 15

flourine: -1

Question 16

What is the oxidation state of a monatomic ion?

Answer 16

monatomic ion: charge of ion
eg NH4+ will be +4

Question 17

What is the oxidation state of an atom in an element?

Answer 17

element= 0