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Chapter 2: Q150CP (page 87)

Boron trifluoride is used as a catalyst in the synthesis of organic compounds. When this compound is analyzed by mass spectrometry (see Tools of the Laboratory, p. 55), several different 1+ ions form, including ions representing the whole molecule as well as molecular fragments formed by the loss of one, two, and three F atoms. Given that boron has two naturally occurring isotopes, 10B and 11B, and fluorine has one, 19F, calculate the masses of all possible 1+ ions.

Short Answer

Expert verified

The masses of all possible 1+ ions are 48 and 49 am respectively

Step by step solution

01

Calculating the mass of BF3

It can be denoted as,

MolecularmassofBF3=1脳Atomicmassof10B+3脳Atomicmassof19F=1脳10+3脳19=67

On losing one of the F- ion the mass will be 48 amu.

02

Calculating another mass of BF3

Then,

MolecularmassofBF3=1脳Atomicmassof11B+3脳Atomicmassof19F

On losing one of the F- ion the mass will be 49amu.

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