Getting Around an IR Spectra
Because the wavelength range of IR radiation useful in vibraional spectroscopy has wavelengths which are rather small numbers (i.e about 2.5x10-6 to 25x10-6 meters) chemists have devised an alternative units of reciprocal centimeters (cm-1). This is sometimes referred to as wave-number and is the x-axis on an IR spectra. The useful range for molecules is between 4000 cm-1 and about 400 cm-1. Wave-number is really a measure of energy and higher energy is to the left and lower energy is to the right on a spectra. Vibrational modes with high energy will show up on the left and those with lower energy will be on the right.
The y-axis is either the intensity of light absorbed or transmitted. In an absorbance spectra the signal intensity indicates the amount of light absorbed. The signals or features you are looking for are peaks in an absorbance spectra. In a transmittance spectra the signal intensity shows the amount of light that passed through (transmitted) the sample. In a transmittance spectra you/re looking for valleys (or upside down peaks). They can be inter-converted by using A=-log(T/100). Most FTIR will do the conversion for you. Below are the transmittance and absorbance spectra for 1-propanol.
Absorbance Spectra (1-propanol)
Transmittance Spectra (1-propanol)
General Procedure for Interpreting IR Spectra (Beginner)
There are three regions of an IR spectra from which most of the info you will use in organic chemistry will come from.
Why are C-H and N-H signals in the high energy end of the spectrum?
When a heavy atom (C, O, N) is bound to a light atom such as H the vibration is at a higher frequency (energy). See Hooke's law for a harmonic oscillator. Assume one of the m1 is infinite then examine the dependence of frequency on mass m2.
Why are sp C-H stretches at a higher energy than sp3 C-H stretches?
Again see Hookes law. In this case an sp C-H bond has a greater spring constant (stronger bond) than an sp3 C-H bond and therefore a higher frequency of vibration.