The vibrational frequency of the C-H bonds in methane CH4 is approximately 3000 cm wavenumbers . This value can vary slightly depending on the specific sample and measurement conditions. Infrared spectroscopy is used to study the vibrational frequencies of molecules, as these frequencies correspond to the energy levels that can be absorbed by the molecule when it interacts with infrared radiation.To relate the vibrational frequency to the wavelength of the radiation absorbed, we can use the following equation:v = c / where v is the vibrational frequency, c is the speed of light 2.998 x 10^10 cm/s in vacuum , and is the wavelength of the radiation absorbed.Rearranging the equation to solve for , we get: = c / vPlugging in the values for the vibrational frequency of the C-H bond in methane 3000 cm and the speed of light, we get: = 2.998 x 10^10 cm/s / 3000 cm = 9.993 x 10^6 cmConverting this value to micrometers m , we get: = 9.993 x 10^6 cm * 1 m / 10^4 cm = 999.3 mSo, the wavelength of the radiation absorbed by the C-H bonds in methane during infrared spectroscopy is approximately 999.3 m.