Bell-Ringer. Define the term isotope. [2 marks]
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2 Bell-Ringer Define the term isotope. [2 marks]
3 Bell-Ringer Define the term isotope. [2 marks] Answer per IB Mark scheme: atoms of the same element/same number of protons/same atomic number that have different numbers of neutrons/different mass numbers Award only [1] max if reference made to elements but not atoms.
4 QUIZ NEXT CLASS MONDAY November 19 -Atomic Models -Atomic Structure -Isotopes -Mass number -RAM -Percent abundances -Atomic Emission Spectra of hydrogen -Electromagnetic Radiation
5 Relative Atomic Mass (RAM) How do you calculate the RAM of an element? To calculate the RAM of an element, multiply the mass of each isotope by its natural abundance (in decimal form), and then add the products. (Mass # of isotope 1 x Abundance of isotope 1) + (Mass # of isotope 2 x Abundance) + (etc ) This is done for ALL isotopes that exist for that particular element.
6 Test Yourself Consider an element Z that has two naturally occurring isotopes with the following percent abundances: the isotope with a mass number of 19.0 is 55.0% abundant; the isotope with a mass number of 21.0 is 45.0% abundant. What is the relative atomic mass for element Z? You should always calculate RAM values to two places after the decimal.
7 Test Yourself Consider an element Z that has two naturally occurring isotopes with the following percent abundances: the isotope with a mass number of 19.0 is 55.0% abundant; the isotope with a mass number of 21.0 is 45.0% abundant. What is the relative atomic mass for element Z? You should always calculate RAM values to two places after the decimal
8 Test Yourself The element vanadium has two isotopes,, and a relative atomic mass of State and explain which isotope is more abundant.
9 Test Yourself The element vanadium has two isotopes,, and a relative atomic mass of State and explain which isotope is more abundant. V-51 is more abundant because the RAM is closer to 51 than to 50.
10 Mass Spectrometer The proportion of each isotope present in a sample of an element can be measured using an instrument called a mass spectrometer. The readout from a mass spectrometer is called a mass spectrum. In a mass spectrum of an element, we get one peak for each individual isotope. The height of each peak is proportional to the number of atoms of this isotope in the sample tested. Mass spectrum for Rubidium (Rb)
11 Test Yourself Deduce the relative atomic mass of the element rubidium from the data given in the figure. Mass spectrum for Rubidium (Rb)
12 Test Yourself Deduce the relative atomic mass of the element rubidium from the data given in the figure. Answer: Pretend there is a sample of 100 atoms, meaning that 77 out of the 100 are Rb-85 atoms and the remaining 23 are Rb-87 atoms. (85 x 77) + (87 x 23) Mass spectrum for Rubidium (Rb)
13 Practice A certain sample of element Z contains 82% of ⁴⁹Z and 18% of ⁵¹Z. What is the relative atomic mass of element Z in this sample?
14 A certain sample of element Z contains 82% of ⁴⁹Z and 18% of ⁵¹Z. What is the relative atomic mass of element Z in this sample? Answer: 49.36
15 Tricky IB Question for RAM #1 Iridium (Ir) has a relative atomic mass of and consists of Ir-191 and Ir-193 isotopes. Calculate the percentage composition of a naturally occurring sample of iridium.
16 Answer: We can deduce the percent abundance of the one of the isotopes, and then subtract that value from 100 to get the percent abundance of the other isotope = (191 x) + [193 (100 )] , 222 = 191x + 19, x -78 = 191x - 193x -78 = 2x x = 39 39% abundance of Ir-191 and 61% abundance of Ir-193
17 Tricky IB Question for RAM #2 Naturally occurring nitrogen (N) is composed of two stable isotopes, N-14 and N-16. Using the RAM of nitrogen found on the periodic table, calculate the percent abundances of each isotope.
18 Answer: = [14(x) + 16(100 - x)] x = 99.5% abundance for N % abundance for N-16 1,401 = 14x + 1,600-16x -199 = 14x - 16x -199 = -2x x = 99.5
19 Tricky IB Question for RAM #3 Naturally occurring silver (Ag) is composed of two stable isotopes, Ag-107 and Ag-110. The Ar of silver is Calculate the percent abundances of each isotope.
20 Answer: = [107(x) + 110(100 - x)] x = 71% abundance for Ag % abundance for Ag-110
21 Tricky IB Question for RAM #4 Magnesium has three stable isotopes, ²⁴Mg, ²⁵Mg, and ²⁶Mg. The lightest isotope has an abundance of 78.90%. Calculate the percentage abundance of the other two isotopes.
22 Answer Magnesium has three stable isotopes, ²⁴Mg, ²⁵Mg, and ²⁶Mg. The lightest isotope has an abundance of 78.90%. Calculate the percentage abundance of the other two isotopes. Answer: In this kind of question you MUST refer to magnesium s RAM! Magnesium s RAM according to the periodic table is = (24 x 78.90) + (25 x) + [26 ( x)] 100 2,431 = x x 2,431 = x x = 11.2% abundance for Mg-25, therefore 9.90% abundance for Mg-26
23 Practice Which is correct for the chromium isotope? A. 24 neutrons and 53 nucleons B. 24 protons and 29 nucleons C. 24 protons and 29 neutrons D. 24 electrons and 53 neutrons
24 Answer Which is correct for the chromium isotope? A. 24 neutrons and 53 nucleons B. 24 protons and 29 nucleons C. 24 protons and 29 neutrons D. 24 electrons and 53 neutrons
25 Schrödinger and the Electron Cloud -Based on Heisenberg s uncertainty principle, Erwin Schrödinger in 1926 developed a mathematical equation to figure out where an electron might be located within the electron cloud based on its level of energy. -He knew that an electron s location within the electron cloud could not be known for certain- but a probability of where an electron might be could be calculated! -We call areas of high probability of where an electron might be an atomic orbital.
26 Atomic orbitals describe the three-dimensional areas where there is a high probability that the electron will be located. They are regions around an atom s nucleus in which there is a 90% probability of finding the electron. Shapes of orbitals will depend on the energy of the electron and its motion in that area. When an electron is in an orbital of higher energy, it means it is most likely far from the nucleus. s orbitals are spherical p orbitals are dumbbell-shaped. There are three of them, located on an x, y, and z axis.
27 Current Atomic Model: Quantum Mechanical Model Incorrect: Bohr thought the energy levels around a nucleus were predictable orbits that electrons traveled on; he figured that electrons had fixed positions in an atom. He believed these orbits were equidistant from each other. Correct: Electrons occupy areas of space called atomic orbitals within the area we call the electron cloud. These orbitals have different levels of energy depending, in part, on their proximity to the nucleus. These orbitals are not equidistant from each other.
28 The energy levels in an atom and all the orbitals that pertain to those energy levels are not equidistant from each other. Energy levels closer to the nucleus are further away from each other. Energy levels further away from the nucleus are closer to each other. WRONG!
29 Energy levels increase in energy the farther away they are from the nucleus. Each energy level is sometimes referred to as a principal quantum number, and is given the variable, n. For instance, the first energy level (the level nearest to the nucleus) would be referred to as n=1, or principal quantum number 1.
30 Due to the unequal distances between energy levels in an atom, different frequencies of light can be emitted from an atom. This figure illustrates a hydrogen atom.
31 Hydrogen produces visible light when its excited electron falls to the second energy level (n = 2). It doesn t matter where it jumped to when excited; if it falls and takes a pit stop at energy level 2, then it will release visible light. It releases Infrared light if it lands on n=3. If its ground state is n=1 then it will release UV radiation once it returns there. Notice that the electron travels a longer distance to get back to n=1 versus n=2. This explains why it releases UV radiation, which is much stronger than visible light.
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34 Test Yourself a) A b) B c) C d) D
35 Test Yourself Answer: b) B
36 Practice
37 Answer
38 Practice Question
39 Practice Question Answer: D
40 QUIZ! After Quiz Exercises from Topic 2 Separate sheet of paper. Write the questions. Start in class, finish for homework. Will be picked up after Thanksgiving break
Bell-Ringer. Define the term isotope. [2 marks] Answer per IB Mark scheme:
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