1. Separate into ox and red half-reactions
2. Mass balance
3. Add oxygen by adding H₂O
4. Balance oxygen with H⁺
5. Add electrons to balance charges on both sides
6. Multiply both sides by opposite number of electrons
7. Add half-reactions together
8. IF IN BASIC SOLUTION- add OH^- to neutralize H⁺ on both sides (so H₂O will be on one side, OH^- on the other)

# electrons in bonding orb's - # electrons in antibonding

2

Cations: Group I and IIA

Anions: Bases of strong acids

In H-X bonds, the more polar the bond is (more electronegative X is) then the stronger the acid

(F>O>N)

Weaker bond --> better acid

as size increases, bond strength decreases, acid strength increases

Smaller the metal with the same charge, stronger acid

Co⁺³ is smaller than Fe⁺³, so stronger acid

If there are too many big ligands on a base, then it will become less basic

This can compensate for base strengthening effects, such as addition of methyl groups (which donate electrons)

Small with large positive charge ( mostly +3 or larger)

H⁺, Li⁺, Na⁺, K⁺, Be⁺², Mg⁺², Ba⁺², Al⁺³, Me₃Al, AlCl₃, Cr⁺³, Mn⁺², Fe⁺³, Co⁺³

More electrons and larger size

I^-, H₂S, HS^-, S^-2, SCN^-, CN^-, CO, PR₃, R₃As

Bigger oxidation state:

Bigger size:

Bigger oxidation state: hard

Bigger size: soft