Halogenated compounds are particularly easy to identify by their mass spectra because chlorine and bromine occur naturally as mixtures of two abundant isotopes. Chlorine occurs as 35Cl (75.8%) and 37Cl (24.2%); Bromine occurs as 79Br (50.7%) and 81Br (49.3%); Boron compounds also stand out owing to the two isotopes 10B (19.9%) and 11B (80.1%).

Required:
a. At what masses do the molecular ions occur for the following formulas?
b. What are the relative percentages of each molecular ion?

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ajeigbeibraheem ajeigbeibraheem · Answer 1 · 2021-02-01T21:04:08+01:00

Answer:

Explanation:

From the given information:

The compound in question here is [tex]\mathbf{C_2H_5Br}[/tex]

The molar mass of [tex]\mathbf{C_2H_5Br}[/tex] with 79 Br is;

= (2 × 12) + (1 × 5) + 79

= 108 g/mol

The molar mass of [tex]\mathbf{C_2H_5Br}[/tex] with 81 Br is:

= (2 × 12) + (1 × 5) + 81

= 110 g/mol

Thus, the mass at which the molecular ions occurs are:

108 and 110.

The relative percentage of mass 108 occurred at 50.7%

The relative percentage of mass 110 occurred at 49.3%