Dear friend
A few words about the different chemistry fields.
Inorganic Chemistry deals with all elements and simple(generally)compounds of one element with one or a few others. The formation and transformation of inorganic compounds is generally accompanied by color changes or other visible characteristics.
Therefore I believe that experiments in inorganic chemistry are the best suited for you.
Organic Chemistry deals mainly with compounds of carbon and a few other elements (Hydrogen,Oxygen,Nitrogen,Sulphur,Phosphor) combined to form simple to very complex molecules.
Since many reactions take place with limited visible changes, the follow up of the reaction is more difficult, needs special lab apparatus, is generally more dangerous, and the reaction products must often be characterized with special instruments, like a refractometer.
In both fields the most evident reactions are used for identifying a compound (analytical methods, both qualitative, to see what, and quantitative, to determine how much) and the most efficient ones are recommended to prepare a certain compound (inorganic preparations and organic syntheses).
The effect of electric current through a solution is related to the field of electrochemistry, and can be applied both to inorganic and organic compounds.
In the academic course I followed, the entry point was with simple inorganic qualitative analysis.
I think you should start in the same way.
To start doing something, I suggest you a simple experiment, just to synthonize each other.
Remember always that any experiment must be conducted paying great attention to what happens, never be in a hurry, always wear some hand and face protection.
But since you work already in a lab, you should know.
A simple electrochemical experiment
Materials needed: a clear plastic cup, a 3 or 4.5 volts battery, some electrical wire, some table salt, some vinegar and some ammonia solution.
Have also a notebook to annotate all made and observed. Learn the difficult art of documenting the experiments!
Fill the cup with tap water for at least two inches, add a teaspoon of table salt, cut two 20 inches pieces of wire, remove the insulation for about two inches at one extremity of each wire, and about one inch at the other, connect these last to each battery pole, and immerge the free 2 inches extremities in the cup water.
Put the whole above a white paper in a well lit place and observe, from sides and from above, what happens.
You should see near the wire connected to the negative pole, the cathode, a shower of small bubbles, and apparently nothing at the other wire(the anode).
After about half an hour you will observe in the solution some insoluble material (a precipitate), partly light blue, partly yellowish: here are some copper hydrate and maybe oxychloride.
Let things go on for a day then withdraw the wires: the cathode will appear blackish, the anode whitish and when cleaned, will show a sensible reduction in diameter as if it were corroded. And it was.
The solution will probably show the same colors, yellowish and light blue, and maybe greenish and also reddish particles.
Leave overnight after some stirring. The precipitate will probably appear all pale yellow.
In the morning, without agitating the liquid, tilt the cup and dispose of most of the liquid(decant), then add again tap water until 2 inches, and leave for 2 hours. Decant again, and pour half of the remaining suspension into another cup.Mark each cup for later identification.
To this cup add two tea spoons of vinegar. Observe and stir every half an hour. Observe the gradual dissolution of the insoluble copper compounds to yield a greenish-bluish liquid.
Put in a quiet place and let it dry. It will be used for next experiments.
In the original cup, pour some drops of ammonia and stir. Observe the dissolution and the onset of intense blue color. Add ammonia until all is dissolved. Place the cup near the other and leave it as well.
End of the first experiment.
Tell me if you succeeded and I will explain, to the extent I can, the theory behind the practice.
Attention!!! The copper compounds you prepared are toxic.Put the cups in a safe place!!!