I'm reading NMR & IR via book,wiki, etc...However, I can't seem to understand the theory behind why things work. I want to really understand why things shift up/down field and why corresponding peaks form.
Frustrated atm, so I definitely appreciate any help!
For IR, it basically measures the vibration pattern of the bonds in a molecule.
You probably still remember in physics they talked about the vibration of a spring. The vibration of a bond is somewhat like that. And if you remember that the vibration frequency is proportional to (k/m)^(1/2), where k represents the strength of the spring and m is the mass, you can understand IR in a similar way. In fact, if the numbers are given, you can calculate the IR spectrum from them, and that is exactly what those softwares do.
Let's come back to MCAT. For example, let's pretend someone asks in which order is the frequency of the stretch vibration mode of C#C, C=C, and C-C? So, obviously m is the same, triple bond (#) is the strongest in terms of bond energy, followed by double bound, therefore, the frequency (or equivalently wavenumber) is C#C > C=C > C-C, which is exactly the case in IR. Another example, C=O, C=N, C=C, well they are quite similar in the strength of the double bond, but in terms of mass, O>N>C. So in IR, C=O has higher wavenumbers, and C=C has lower ones, just as you may have seen on wiki. You may ask why there are overlaps on the wiki figure? Very good question, because the bond strength will be affected by the substituents on the atoms. if you have, for example, a conjugated double bond, attached to the C=O, that will cause the C=O double bond less strong as in isolated ones, because of delocalization of the pi electrons, and therefore, leading to a shift of the C=O stretch toward the lower wavelength side. Such effect can also be seen with an electronegative atom attached to the carbonyl, that is why the C=O stretch in ketone is higher than in ester, amide, etc. Similarly you can expect the C=O stretch can be affected by hydrogen bond formation of the carbonyl oxygen. So if you have a benzaldehyde, and a o-hydroxyl benzaldehyde, which one would you expect having a higher C=O stretch wavenumber in IR? I guess you already know by now. Same reason, hydrogen bonding with solvent, or coordination with metal, or anything that may affect the bond strength, may have impact on the IR, causing the peak shift, larger or smaller.
Regarding NMR, tttgo gave a fair explanation, especially the link within that post is worth reading. The key word would be the shielding, which causes the different chemical environment of each and every proton. Let me know if you need further help.
Good luck and have fun!