Page 14 Questions

1. Page 14 Questions

2. Mass Spectra Objectives: • Interpret mass spectra of elements • Calculate Relative Atomic Mass from isotopic abundance of mononuclear ions • Know a significant use of mass spectometry

3. Mass Spectra

4. Mass Spectra

5. What does the mass spectrum tell us? Relative abundance Mass/charge ratio (m/z) -You can assume the charge is 1+, so m/z is just mass (relative isotopic mass)

6. What does the mass spectrum tell us? Questions to try… How many isotopes are present In this spectra? Which element are these isotopes of? What is the relative isotopic mass of each isotope? What is the relative isotopic abundance of each isotope?

7. Calculating Relative Atomic mass from spectra Step 1: For each peak, multiply the relative atomic abundance by the relative atomic mass. This gives you the mass of each isotope Step 2: Add up the total mass of each isotope Step 3: (if % abundance) divide by 100 [NB: if not % abundance, then divide by the total relative abundance instead] Step 1: 1st isotope: 51.5 x 90 = 4635 2nd isotope: 11.2 x 91 = 1019.2 3rd isotope: 17.1 x 92 = 1573.2 4th isotope: 17.4 x 94 = 1635.6 5th isotope: 2.8 x 96 = 268.8 Step 2: 4635 + 1019.2 + 1573.2 + 1635.6 + 268.8 = 9131.8 Step 3: 9131.8 / 100 = 91.318 51.5 17.1 17.4 11.2 2.8

8. Calculating Relative Atomic mass from spectra Step 1: For each peak, multiply the relative atomic abundance by the relative atomic mass. This gives you the mass of each isotope Step 2: Add up the total mass of each isotope Step 3: (if % abundance) divide by 100 [NB: if not % abundance, then divide by the total relative abundance instead] Step 1: 1st isotope: 51.5 x 90 = 4635 2nd isotope: 11.2 x 91 = 1019.2 3rd isotope: 17.1 x 92 = 1573.2 4th isotope: 17.4 x 94 = 1635.6 5th isotope: 2.8 x 96 = 268.8 Step 2: 4635 + 1019.2 + 1573.2 + 1635.6 + 268.8 = 9131.8 Step 3: 9131.8 / 100 = 91.318 51.5 17.1 17.4 11.2 2.8

9. Calculating Relative Atomic mass from spectraNow try these… Boron 100 Krypton 23

10. What do you think has happened in the graph on the right hand side?

11. Using mass spectra to determine molecular mass As well as elemental isotopes, a mass spectrometer can detect molecules too! When a vapourised sample is bombarded with high energy electrons, a single electron can be removed from a molecule This creates a molecular ion, M+ (g), but also the molecule can break up and create a Fragmentation pattern, which then shows up on the spectrum as the lines to the LEFT of the Mr of the molecule…

12. Using mass spectra to determine molecular mass As well as elemental isotopes, a mass spectrometer can detect molecules too! When a vapourised sample is bombarded with high energy electrons, a single electron can be removed from a molecule This creates a molecular ion, M+ (g), but also the molecule can break up and create a Fragmentation pattern, which then shows up on the spectrum as the lines to the LEFT of the Mr of the molecule…

13. Using mass spectra to determine molecular mass Now try the examples on page 17

14. PRACTICE!!! Now try the Lesson 5-6 past paper questions and finish for homework

15. Long form practice exam question Q1. (a) State the relative charge and relative mass of a proton, of a neutron and of an electron. In terms of particles, explain the relationship between two isotopes of the same element. Explain why these isotopes have identical chemical properties. (7 marks) (b) Define the term relative atomic mass. An element exists as a mixture of three isotopes. Explain, in detail, how the relative atomic mass of this element can be calculated from data obtained from the mass spectrum of the element. (7 marks) (Total 14 marks)

16. Long form practice exam question M1. (a) Proton: mass 1, charge + 1 (1) Neutron: mass 1, charge 0 (1) Electron mass 1/1840, charge -1 (1) Allow mass = 0, or negligible, or 1/1800 to 1/2000 Isotopes have the same number of protons (1) OR atomic number different number of neutrons (1) Isotopes have the same electronic configuration (1) OR same number of electrons Chemical properties depend on electrons (1) 7 Marks

17. Long form practice exam question (b) ×12 (1) OR × 12 or in words Spectrum gives (relative) abundance (1) OR % or amount And m/z (1) Multiply m/z by relative abundance for each isotope (1) Allow instead of m/z mass no, Ar or actual value from example Sum these values (1) Divide by the sum of the relative abundances (1) only award this mark if previous 2 given Max 2 if e.g. has only 2 isotopes 7 Marks [14]

18. OTHER USES OF MASS SPECTROMETRY - SPACE EXPLORATION - Mass spectrometry is used on space probes to identify elements and compounds on the surface of planets. In August and September 1975 the USA launched Viking 1 and 2. Both probes entered Mars orbit to map the planet, dropping landers that transmitted pictures, acted as weather and scientific stations and analysed the Martian soil. VIKING LANDER THE MARTIAN SURFACE

19. REVISION CHECK What should you be able to do? Recall the four basic stages in obtaining a mass spectrum Understand what happens during each of the above four stages Understand why particles need to be in the form of ions Recall the the meaning of mass to charge ratio (m/z) Explain how the mass/charge value affects the path of a deflected ion Interpret a simple mass spectrum and calculate the average atomic mass Understand how mass spectrometry can be used to calculate molecular mass Recall that mass spectrometry can be used to in space exploration Recall other uses of mass spectrometry