Match the four processes (on the right) to the following descriptions. (Click and Drag the descriptions to the correct processes)
| Draggable item | arrow_right_alt | Corresponding Item |
|---|---|---|
Electrons are knocked off sample particles to form (mostly) +1 ions. | arrow_right_alt | Detector |
Ions collide with a metal plate. Electrons are transferred from the metal to the ion, producing a current and thus a signal to a computer. | arrow_right_alt | Deflection |
Ions move through a series of charged plates to form a narrow bean of high speed particles with equal kinetic energy. | arrow_right_alt | Ionizer |
Ions are attracted to the negative side of an electromagnetic field causing separation of the mixture based on mass and charge. | arrow_right_alt | Accelerator |
When a sample is injected into the mass spectrometer, do the atoms or molecules turn into positive or negative ions? Justify your answer with at least two pieces of evidence from Model 1.
Based on your new learning of Mass Spectroscopy, what causes a sample to become separated?
Consider the following ions formed in a mass spectrometer. Rank the ions in terms of their degree of deflection by the electromagnet from least to greatest. (Click and Drag each ion to its correct ranking where 1 is the least deflected and 3 is the most deflected)
19F1+ 16O1+ 17O1+
19F1+
17O1+
16O1+
In Mass Spectrometry, a computer creates a graph of isotope mass and relative abundance. See Figure 2.
Since the tallest (most abundant) line is for mass number 20, it can be deduced that neon’s average atomic mass is closer to 20.
These graphs can also be used to calculate the average atomic mass using this equation:
For example: To calculate the average atomic mass of Neon from the Mass Spec data:
Consider this mass spectrum for the element boron below.
How many naturally occurring isotopes does boron have?
Calculate the atomic mass of boron-‐ check your answer with the atomic mass on the periodic table. Show your work!
How does boron’s atomic mass compare with the mass numbers of its isotopes?
Consider the mass spectrum for zirconium.
Which isotope is most abundant?
Which isotope is least abundant?
Predict, what will the atomic mass of zirconium be: (multiple choice)
a. 93.5 u
b. 92 u
c. 90.5 u
Lead has four naturally occurring, stable isotopes. The table shows their masses and relative abundances.
Draw a mass spectrum for lead, based on the data in the table:
Calculate the atomic mass of Lead. Show your work!
Challenge Question:
Carbon has two naturally occurring isotopes, carbon-12 and carbon-13. Its atomic mass is
12.011 u. Based on this data, calculate the relative abundances of each of carbons isotopes. Show your work and give your answer with 3 sig figs.
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