I'm trying to apply conjugate theory, which I can apply very well to acids/bases, to redox. Can you verify my logic, which I have broken down below?
1) I know that solid sodium is a strong reducer.
2) I know this because solid sodium when placed in water reacts violently, forming, among other products, sodium ion.
3) Reducers are oxidized. Reducers lose electrons. Correct; $\ce{Na^{+}}$ is the product of placing solid sodium in water.
4) So in this half-reaction: $\ce{Na<=>Na^{+} +e^-}$, sodium is the reducer. $\ce{Na^{+}}$ is the conjugate oxidizer.
5) Oxidizers are reduced. Oxidizers gain electrons.
6) Because sodium is a strong reducer, which means it has a strong tendency to be oxidized, or a strong tendency to lose electrons, its conjugate oxidizer must be weak. Oxidizers are reduced; oxidizers gain electrons. The potential for $\ce{Na^{+}}$ to gain the electron that $\ce{Na}$ just lost must be small, or $\ce{Na}$ would not be a good reducer.
7) Therefore, a strong reducer's conjugate oxidizer must be weak.
8) Likewise, a strong oxidizer's conjugate reducer must be weak.
9) Likewise, a weak reducer's conjugate oxidizer must be strong.
10) Likewise, a weak oxidizer's conjugate reducer must be strong.
Also, if anyone could point me to a good reference on gaining insight into redox, tha would be great!
And while we're on the topic of redox, what's the mechanism for this reaction? Are both bonds cleaved homolytically? I see how the nucleophilic chlorines attack the electrophilic hydrogens but how's the bond broken?
$\ce{H_2 + Cl_2 ->2HCl}$