3.1.7 Oxidation, Redox, Reduction Reactions Flashcards
Reducing agent
Lose electrons so they oxidise themselves
Oxidising agent
Gain electrons so they reduce themselves
Oxidation number of elements E.g. Cl2
0
Oxidation number of ions
Same as charge
Group 1 oxidation number
+1
Group 2 oxidation number
+2
Aluminium oxidation number
+3
Hydrogen oxidation number
+1
Except in hydrides it’s -1 E.g. NaH
What is a hydride
When hydrogen is bonded to a metal
Chlorine oxidation number
-1
Except in compounds with F and O E.g. ClF3 it’s Cl+3
Fluorine oxidation number
-1
Oxygen oxidation number
-2
Except in peroxides it’s -1
Except in OF2 it’s +2
When giving oxidation numbers what would H2O2 the oxidation state of oxygen be
-1
1) because peroxide
2) only given oxidation state of 1 oxygen not 2
How do you find oxidation state if molecule has a charge
The charges don’t add to 0 they add up to the charge on the molecule
Reduction is an increase/decrease in oxidation number
Decrease