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Carbon monoxide and hydrochloric acid absorb infrared light at 4.66 μm and 3.46 μm, respectively. Use the quantum mechanical harmonic oscillator to treat these as absorption transitions from the v=0 to v=1states.
(a) Determine the force constants for the 12C - 16O Bond, and for the 1H - 35Cl bond. Which molecule has the stronger bond?
(b) Analyze the Lewis (electron dot) structures of each molecule. Are the lewis structures consistent with the results from infrared spectroscopy? Expain.
What functional group gave rise to the peak that appears at1700cm-1 on the IR?
sp2 Carbon-hydrogen stretch.
Carbon-oxygen double bond stretch of the carbonyl group of thediacid.
Carbon-oxygen single bond stretch.
Oxygen-hydrogen stretch of the hydroxyl group of the diacid.
The lowest-frequency pure rotational line for 12C16O occurs at 115,271 MHz. Assume that the bond distance the force constants are the same for isotopes of the same molecule.
a. What is the C-O bond distance in this molecule?
b. What is the lowest-frequency rotational line for 13C16O? For 12C18O?
c. If the fundamental vibration of 12C16O occurs at 2143 cm-1, at what wavenumber should the fundamental vibration of 12C18O appear?
d. Which techinique is more sensitive to isotopic shifts: infrared or microwave spectroscopy? Explain your answer.