Draw the molecular ion (M+) for this molecule formed in the mass spectrometer. Br: - e- 6

Match the molecular ion (from electron impact mass spectrometry) with the correct compound. (Make sure to consider the isotope pattern) 100 120 Br A 121 x B NH ន 122 Mass M/e 123 123 Me 124 124 OH но ма 125 D 126

Use the isotope method to determine the molecular formula

In the mass spectrum of an unknown organic compound, the molecular ion had a relative abundance of 19.0 while the M+1 had a relative abundance of 1.5. Estimate the number of carbons in the molecule. 1 4 7 2 LO 5 8 carbons 3 6 9 X C

In a mass spectrum, what m/z value would correspond to the fragment shown below?

Using the rule of 13, what is a possible formula for M=113 (100%) on a mass spectrum? all of the above are possible molecular formulas CH130 CH15N

please help identify the mass spectrometry

Halogenated compounds are particularly easy to identify by their mass spectra because both chlorine and bromine occur naturally as mixtures of two abundant isotopes. Recall that chlorine occurs as 35Cl (75.8%) and 37Cl (24.2%); and bromine occurs as 79Br (50.7%) and 81Br (49.3%). At what masses do the molecular ions occur for the following formulas? What are the relative percentages of each molecular ion? (a) Bromomethane, CH3Br (b) 1-Chlorohexane, C6H13Cl

Draw the molecular ion (M*) for this molecule formed in the mass spectrometer. H. H -e-

Determine if the compounds contain a Chlorine, Bromine or Fluorine atom.