AP Chemistry
1.2 Mass Spectra of Elements
A student uses mass spectrometry to analyze a metal sample known to consist primarily of zirconium (\(\text{Zr}\), atomic number \(40\)) that is suspected to be contaminated with molybdenum (\(\text{Mo}\), atomic number \(42\)). Naturally occurring zirconium has isotopes with mass numbers \(90\), \(91\), \(92\), \(94\), and \(96\). Naturally occurring molybdenum has isotopes with mass numbers \(92\), \(94\), \(95\), \(96\), \(97\), \(98\), and \(100\). The mass spectrum data for the singly charged (\(+1\)) ions generated from the sample are shown in the table below.
Which of the following conclusions is best supported by the data in the table?
| Mass-to-charge ratio (\(m/z\)) | Relative intensity |
|---|---|
| \(90\) | \(51.5\) |
| \(91\) | \(11.2\) |
| \(92\) | \(18.5\) |
| \(94\) | \(18.1\) |
| \(95\) | \(2.4\) |
| \(96\) | \(4.8\) |
| \(98\) | \(3.6\) |
Which of the following conclusions is best supported by the data in the table?
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