3.1.7 -oxidation, Reduction And Redox Equations Flashcards
What are the oxidation states of atoms and simple ions ?
The number of electrons which must be added or removed to become neutral
What should the oxidation states do in molecules
Sum of the oxidation states should add up to 0
What is the oxidation states of c and o in co2
C is +4
O is -2
What should the oxidation states be in a complex ion
The sum of the oxidation states should add up to the charge on the ion
What are the bench marks
Hydrogen (+1)
Oxygen (-2)
Fluorine (-1)
What is the exception of hydrogen to the bench mark
It’s 0 in H and H2
-1 in hydride ion eg NaH
What’s the exception of oxygen in the bench marks
It’s 0 in O and O2
-1 in hydrogen peroxide
+2 in F2O
What is the exception in fluorine to the bench mark
0 in F and F2
What are the usual oxidation values of metals
- usually postive values
- can go up to the group number
What are the normal oxidation states of non- metals
Mostly negative
Values up to group number
Define redox
When reduction and oxidation takes place
Define oxidation
Removal of electrons
Na—> Na+
Define reduction
Gain of electrons
Cl—> Cl-
Define oxidising agent
Accepts electrons
Define reducing agent
Donates electrons
