Organic Chemistry Semester 1 LABORATORY MANUAL - Moravian ...

Part V. Experiments 38 Fall 2010
• The presence of chlorine in a compound leads to two molecular ions (with 17 Cl 35
or with 17 Cl 37 ) differing by 2 mass units. For a molecule with one chlorine atom,
what should be the relative intensities of these two molecular ions
b. Additional Molecular Ion Considerations.
As we learned in developing our methods for calculating double bond equivalents:
• The general formula for a hydrocarbon is C n H 2n+2 . Considering the mass of
carbon and hydrogen, predict if the molecular ion of a hydrocarbon should be an
even or odd number. (choose one)
• A molecule with one oxygen atom adds a total mass of 16 to the mass of a
corresponding the hydrocarbon. That makes the molecular ion of a compound
containing an O an (even or odd) number (choose one).
• A molecule with one nitrogen atom also has an additional hydrogen atom
compared to a corresponding the hydrocarbon, a total mass of 15 (14 + 1). That
makes the molecular ion of a compound containing an N an (even or odd)
number (choose one).
• A bromine atom replaces a hydrogen atom in a hydrocarbon. That makes the two
molecular ions of a compound containing one Br:
(1) Both even numbers.
(2) Both odd numbers.
(3) One odd number and one even number
• A chlorine atom replaces a hydrogen atom in a hydrocarbon. That makes the two
molecular ions of a compound containing one Cl:
(1) Both even numbers.
(2) Both odd numbers.
(3) One odd number and one even number