Question

average atomic mass
from the textbook, read section 3.2 and, on pages 115 and 115a, do #39, 40, 41
mass spectroscopy

1. the mass spectrum below represents a mixture of elements. what elements are present? justify your answer. (check your answer using the websites listed at bottom of document.)

Explanation:

Step1: Identify characteristic masses

In mass - spectrometry, elements have characteristic mass - to - charge ($m/z$) ratios for their isotopes. The $m/z$ values of 107 and 109 are characteristic of the isotopes of silver (Ag). Silver has two stable isotopes, $^{107}$Ag and $^{109}$Ag. The $m/z$ value of approximately 74.92 is characteristic of germanium (Ge) as one of its isotopes has a mass close to this value.

Step2: Justify elements

By comparing the $m/z$ values in the mass spectrum to the known isotopic masses of elements in the periodic table, we can conclude that the elements present are silver (Ag) due to the 107 and 109 $m/z$ peaks and germanium (Ge) due to the 74.92 $m/z$ peak.

Answer:

The elements present are germanium (Ge) and silver (Ag).