Oxidation Numbers:

-oxidation numbers are the hypothetical charge an atom in a compound would have if the bonds were fully ionic

-NOT the same as formal charge

-more electronegative atoms will take electrons from less electronegative atoms

-elements and diatomic gases have an oxidation number of 0 because there are no more electronegative atoms to give up the electrons to

-transition metals have variable oxidation numbers depending on the compound they are in (bc/ of their d suborbitals)

-using the rules above, you can find the oxidation numbers of every atom except the transition metal, then subtract those oxidation numbers from the overall charge of the compound to find the transition metal’s oxidation number

-sometimes oxidation numbers of transition metals are indicated in the name (e.g. Copper(II) oxide (CuO), copper has an oxidation number of 2; Chromium(VI) hydrogen phosphate (Cr(HPO4)3), chromium has an oxidation number of 6)

Coordination Compounds:

How to Calculate the Oxidation State of Transition Metals in Coordination Compounds

Oxidation Numbers of Carbon in organic molecules:

-each bond to a less electronegative atom (i.e. H) gives an electron to carbon confers a -1 oxidation number

-each bond to a more electronegative atom (e.g. O, N, F) takes away an electron from carbon confers a +1 oxidation number

-remember: double bonds count as two bonds, triple bonds count as three

-each bond to another carbon is a zero change in oxidation number (bc/ no electronegativity difference)

-takeaway: electronegativity directly affects the oxidation number of carbon

CO2: oxidation state of C = +4

Balancing Redox Reactions in Acidic Solutions:

1. Split up whole reactions into half reactions; then for each half reaction:
   
   1. Balance all atoms except O and H
   2. Add H2O to balance O
   3. Add H+ to balance H
   4. Finally, Add e– to balance charges
2. Bring together half reactions back together, making sure the number of elections balance out
3. Cancel stuff on both sides of the arrow

How to Balance Redox Equations in Acidic Solution

Balancing Redox Reactions in Basic Solutions:

Same as above, but AT THE END:

1. Add OH– to each side for each H+
2. Combine each OH– and H+ to make H2O
3. Cancel H2O’s

How to Balance Redox Equations in Basic Solution

Redox Titrations:

Redox titrations | Chemical reactions | AP Chemistry | Khan Academy

Coordination Complexes:

Transition Metal Complexes

Coordination Complex Nomenclature