You're probably nearly there. You must learn all the possible organic reactions (including reagents and reaction conditions). Have a really good look through the spec because they are difficult to find sometimes. Then you can make a large A3 poster and write down all the different functional groups and use arrows to show how to turn one into another. Haloalkanes can be placed in the centre because they are involved in loads of routes. You can also stick on the characteristic IR absorptions too so you can quickly recongise a functional group by shape and wavenumber. This will help you see the bigger picture.
Redox can be difficult. A lot of organic involves reduction so make sure you know that reduction is the gain of hydrogen as well as OILRIG (electrons). Be absolutely certain that you know what a reducing agent is. It does reducing. It donates hydrogen (often as hydride ions) or it donates electrons.
Electrons are always written on the left hand side of standard electrode potentials. Why?
The more negative the E° value, the more the equilibrium lies to the left.
The species on the right is being oxidised it is losing electrons and it is therefore trying to act as a reducing agent. The more negative the E° value, the more the equilibrium lies to the left and the species on the right is therefore a good reducing agent – it is good at giving electrons away.
The species on the left is being reduced – it is trying to act as an oxidising agent. The more positive the E° value, the more the equilibrium lies to the right and the better the species on the left is at receiving electrons – it is a better oxidising agent.
Because these questions are all about redox, a given chemical equation can be split into two half equations. Copper Oxide and Zinc makes Zinc Oxide and Copper. This overall reaction can be expressed as two half-equations; you should be able to do that. You can then calculate whether a reaction is feasible using the two relevant standard electrode potentials.
1) Select the half equation that you want to move to the right (in this case copper ions gain electrons and make copper)
2) Make this the right hand electrode (in your mind)
3) Select the half equation that you want to move to the left (in this case, zinc atoms lose electrons to make zinc ions.
4) Make this the left hand electrode (in your mind)
Then:
3) Perform the calculation e.m.f. = Right hand electrode - left hand electrode (in this case: +0.34- (-0.76)
4) If the answer is POSITIVE then reaction is feasible.
In this case, the answer is +1.1 V. So the reaction can occur.