- 1 - Core Chemistry Topic 2 Atomic Structure
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1 - 1 - Core Chemistry
2 REVIEW a model for matter (10 mins) 1. On your own take 5 minutes to construct a concept map organizing what you know about the structure of matter. 2. Take 5 more minutes and share what you have with a partner. 3. Make a list of the big ideas you share about the structure of matter. 4. Think of 2 or 3 questions you might have about the structure of matter. MATTER - 2 -
3 2.1 Basic and Notation Core Chemistry Proton Neutron Electron Location Relative Mass Relative Charge A-Z notation For example carbon C PRACTICE list all the information provided by the notation below Ions DEFINE ion. Distinguish between cations and anions
4 PRACTICE list all the information provided by the notation below 37 Cl Ca +2 Core Chemistry Isotopes DEFINE isotope and provide examples. How are the isotopes of an element similar and how are they different? an example three isotopes of hydrogen List some specific uses of radioisotopes - 4 -
5 Review Questions for this topic are from Chemistry 3 rd Edition, Green and Damji. Exercise Which of the following are usually found in the nucleus of an atom? A. Electrons and neutrons only. B. Neutrons only. C. Protons neutrons and electrons. D. Protons and neutrons only. 2. The number of neutrons in an atom of Ba is A. 56 B. 82 C. 138 D How many electrons would have about the same mass as a proton or a neutron? A. 200 B. 500 C D Which one of the following is not a common use of radioactive isotopes? A. As a fuel in fuel cells B. Irradiating tumors in patients with cancer. C. Measuring the rate of uptake of a drug that has been swallowed. D. Finding the age of rocks. 5. Radioisotopes of normally stable elements are A. chemically extracted from the natural element B. mined from scarce underground deposits. C. formed from the stable element in nuclear reactors. D. produced through chemical reactions of the stable element 6. Identify the following subatomic particles: a) The particle that has a much lower mass than the others. b) The particle that has no electrical charge. c) The particle that is not found in the nucleus. d) The number of these in the nucleus is equal to the atomic number. e) The particle that is gained or lost when ions are formed - 5 -
6 7. Calculate the number of protons, neutrons and electrons for the following: 8. Boron has atomic number 5. It comprises two isotopes, one with five neutrons, the other with six. a) Define the term isotope. b) Calculate the mass numbers of the two isotopes and represent them in the form x y B. 9. Omit c) In naturally occurring boron, 20% of the atoms contain five neutrons and 80% six neutrons. Calculate the relative atomic mass of boron. 10. Naturally occurring copper is a mixture of two isotopes. One of these has 29 protons and 34 neutrons, the other one two more neutrons. Complete the following table for both isotopes: Challenge: If the relative atomic mass of copper is 63.55, calculate the natural abundances of the two isotopes
7 11. Complete the following table: - 7 -
8 Outline the purpose of each step in the function of a mass spectrometer. Vaporization Ionization Acceleration Deflection Detection - 8 -
9 A sample mass spectrometer output.. Note the labeling of the x-axis. Explain the meaning of m/z. Define average atomic mass and explain why this is a relative measurement. EXAMPLE 1: Calculate the average atomic mass of chlorine if its abundance in nature is 75.77% 35 Cl, and 24.23% 37 Cl. EXAMPLE 2: Gallium has two naturally occurring isotopes, Ga-69 and Ga-71, with masses of amu and amu, respectively. Calculate the percent abundances of these isotopes - 9 -
10 Exercise Describe briefly how in the mass spectrometer a) the atoms are converted into ions. b) the ions of different mass are separated. c) the ions are detected. 2. Germanium (atomic number 32) contains 20% germanium-70, 8% germanium-72, 37% germanium-73 and the remainder is germanium-74. Draw a graph of the mass spectrum that you would expect germanium to produce. If an atom of germanium-70 lost two electrons during the ionization process to become a +2 ion, at what m/z would it appear in the spectrum?
11 3. The graph shows the mass spectrum of the element which contains 76 protons in its nucleus. a) Write down, in the form A Z X, the isotopes that it is composed of with their natural abundances (as a %). b) Calculate the relative atomic mass of the element
12 Core Chemistry
13 Core Chemistry Electromagnetic Spectrum ACTIVITY Atomic Emission Spectra you should have notes about the electromagnetic spectrum completed as part of this assignment. EXPLAIN:: ensure you are aware how an emission spectrum occurs and can distinguish between a continuous spectrum and a line spec spectrum. ACTIVITY Electron Transitions in Hydrogen (evidence for the Bohr model)
14 Electron Arrangement A simple understanding of how electrons are arranged around the nucleus of atoms follows these basic rules i. electrons occupy regions of space called orbitals which have fixed energy levels ii. electrons will occupy the lowest energy level orbitals first iii. each energy level has a set number of orbitals and therefore a maximum number of electrons Core syllabus requires application of the 2,8,8,2 rule for electron configuration of atoms up to calcium (atomic number 20). For example carbon: Periodic Table Connections
15 Exercise An atom has an atomic number of 13 and a mass number of 27. How many electrons will it have in its valence level? A. 1 B. 2 C. 3 D Which of the following would produce a line spectrum rather than a continuous spectrum? A. A yellow (sodium) street light. B. A normal filament light bulb. C. Sunlight. D. A white hot piece of steel. 3. Which of the following colors corresponds to light of the highest energy A. Yellow B. Red C. Green D. Blue
16 4. Which one of the following is not a valid electronic structure? A. 2,8,4 B. 2,6 C. 2,9,1 D. 2,8,8,2 Core Chemistry 5. Which one of the following electron transitions in a hydrogen atom would produce light in the visible region of the spectrum? A. n=2 to n=1 B. n=5 to n=4 C. n=6 to n=2 D. n=4 to n=1 6. Which one of the following is not true for both absorption and an emission spectra? A. They are the result of the movement of electrons between energy levels. B. The electrons can move between any two energy levels. C. The frequency of the light is related to the difference in the energy levels. D. There is a convergence towards the high frequency end. 7. Which of the following transitions in the hydrogen atom would produce light of the shortest wavelength? A. n=2 to n=1 B. n=5 to n=4 C. n=6 to n=2 D. n=4 to n=1 8. Given the atomic numbers of the following elements, write their simple electronic structures: a) Beryllium (At. No. = 4) b) Aluminium (At. No. = 13) c) Fluorine (At. No. = 9) d) Argon (At. No. = 18) e) Sulfur (At. No. = 16) 9. Two particles have the following composition: A: 37 protons; 38 neutrons, 37 electrons B: 37 protons; 40 neutrons, 37 electrons a) What is the relationship between these particles? b) These two particles have very similar chemical properties. Explain why
17 10. Explain why, in the hydrogen atom spectrum: a) only light of certain frequencies is observed. b) different series are observed in different spectral regions. c) these series all converge at the high frequency end. Core Chemistry
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