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Isotopes of Elements Part 1

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Isotopes of Elements Part 1 Isotopes of elements part 1 Isotopes of elements part 1 Lesson plan (Polish) Lesson plan (English) Isotopes of elements part 1 Link to the lesson Before you start you should know that atoms are built from the atomic nucleus and electrons moving around it; that the atomic nucleus consists of protons and neutrons; that the sum of proton and neutron numbers is called a mass number; that the number of protons in the nucleus is an atomic number; that the elements in the periodic table are ordered according to the increase of the atomic number. You will learn explain what are isotopes; describe isotopes with symbols; discuss differences in the structure of hydrogen isotope atoms; calculate the mass of the isotope. Nagranie dostępne na portalu epodreczniki.pl nagranie dźwiękowe abstraktu Differences in the atoms of the same element Atoms belonging to the same element have the same nucleus charge (identical number of protons) and the same number of electrons moving around the nucleus. However, as it turns out, these atoms can differ in mass. The reason for this phenomenon is the possibility that different numbers of neutrons occurs in the nucleus of atoms of the same element. Those atoms that have more neutral particles have a larger mass. The atoms of the element with the same number of protons, and different number of neutrons in the nucleus are called isotopes. Task 1 Consider whether the isotopes of the same element have the same atomic and mass numbers. If not, which of these numbers may be different and why? The different number of isotopes of the same element is... Why it can differ? The element with several isotopes is nitrogen. There are seven neutrons in the nucleus of one of them, and in the nucleus of the other – eight neutrons. Each of these isotopes has the same number of protons that can be found in the periodic table. The atomic number of nitrogen is 7, and this is also amount of protons found in the nuclei of all atoms of this element. In the case of the isotopes described above, the sum of protons and neutrons will be different. Mass number Number Number of Atomic Number of Description (sum of protons of atom protons number neutrons of atom and neutrons) 14 1 7 7 7 7 + 7 = 14 7N 15 2 7 7 8 7 + 8 = 15 7N The information on the number of neutrons isotopes contain is important in their description. Therefore, mainly mass number providing information on the number of these particles is used in its description. The atomic number is usually omitted due to the fact that it can be found in the periodic table. Isotopes are presented in two ways: the mass number is placed in the upper index on the left side of the symbol of the element or after the dash after the name of the element, e.g. 14 N or nitrogen‐14. Task 2 Using periodic table that shows the percentage of stable isotopes of parcular elements, determine how many elements have only one natural type of isotope and which elements have the most of them. How many elements has only one natural isotope? Which elements have the most isotopes? Isotopes of hydrogen in nature Isotopes with the same atomic number belong to the same element. In principle, these show identical properties, with the only exception being hydrogen isotopes. The hydrogen in 1 2 nature is a mixture of mainly two isotopes in stable‐state: H (99.985%) and H (0.015%). It 1 2 means that of 100,000 atoms of hydrogen, 99,985 are isotopes H, and 15 atoms – isotopes H 3 . There is also the third, unstable isotope H. It occurs in trace amounts. The isotopes of hydrogen were the only ones in the world of elements to have their names: protium, deuterium and tritium. Symbol of hydrogen isotope 1 H or hydrogen‐1 Name of hydrogen isotope – protium Symbol of hydrogen isotope 2 H or hydrogen‐2 Name of hydrogen isotope – deuterium Symbol of hydrogen isotope 3 H or hydrogen‐3 Name of hydrogen isotope – tritium It is easy to see that hydrogen isotopes differ in the number of nucleons. For this reason, there is a large mass difference between them, for example the deuterium atom has a mass twice as large as the weight of the protium and the tritium mass is three times larger than protium. This phenomenon affects the properties of these isotopes: protium, deuterium and tritium have different properties. Symbol of Density Melting point Boiling point Isotope isotope [g/dm3] [K] [K] protium H 0.08233 13.83 20.27 deuterium D 0.1645 18.73 23.67 tritium T 0.2464 20.62 25.04 Task 3 Watch the presentaon „Potassium isotopes”. Which of the types of the element are stable? What is the applicaon of its isotopes? Source: GroMar Sp. z o.o., licencja: CC BY-SA 3.0. Nagranie dostępne na portalu epodreczniki.pl Nagranie audio prezentujące właściwości izotopów. Which types of potassium are stable? What are applicaons of potassium isotopes? Exercise 1 Assign atoms to the appropriate sets of isotopes. <sup>40</sup><sub>20</sub>E, <sup>50</sup><sub>24</sub>E, <sup>54</sup> <sub>24</sub>E, <sup>52</sup><sub>24</sub>E, <sup>42</sup><sub>20</sub>E, <sup>54</sup><sub>26</sub>E, <sup>60</sup><sub>28</sub>E, <sup>58</sup> <sub>26</sub>E, <sup>56</sup><sub>26</sub>E, <sup>39</sup><sub>19</sub>E, <sup>38</sup><sub>18</sub>E, <sup>40</sup><sub>19</sub>E, <sup>44</sup> <sub>20</sub>E, <sup>40</sup><sub>18</sub>E, <sup>58</sup><sub>28</sub>E isotopes of chromium isotopes of iron isotopes of potassium isotopes of nicle isotopes of argon isotopes of calcium Exercise 2 What are the differences between atoms of the elements? Complete the gaps in the table. informaon about elements35Cl 37Cl number of protons number of electrons number of netrons electron configuraon a, b, c Exercise 3 What are the differences between atoms of the elements? Complete the gaps in the table. informaon about elements64Zn 70Zn number of protons number of electrons number of netrons electron configuraon a, b, c Exercise 4 What are the differences between atoms of the elements? Complete the gaps in the table. informaon about elements16O 17O 18O number of protons number of electrons number of netrons electron configuraon a, b, c Summary Isotopes are atoms of the same chemical element that have the same number of protons and different number of neutrons. Most of the chemical elements found in nature are a mixture of isotopes with a stable composition. 1 2 3 Isotopes of hydrogen are: protium ( H), deuterium ( H) and tritium ( H). Their properties are different. Source: GroMar Sp. z o.o., licencja: CC BY-SA 3.0. Keywords isotope, atom, proton, neutron, protium, deuterium, tritium Glossary isotopes Nagranie dostępne na portalu epodreczniki.pl Nagranie dźwiękowe słówka izotopy – odmiany tego samego pierwiastka, które mają jednakową liczbę atomową (liczbę protonów w jądrze) i różną liczbę masową (liczbę neutronów w jądrze) Lesson plan (Polish) Temat: Izotopy pierwiastków cz. 1 Adresat Uczeń szkoły podstawowej (klasy 7. i 8.) Podstawa programowa: Szkoła podstawowa. Chemia. I. Wewnętrzna budowa materii. Uczeń: 4) definiuje pojęcie izotopu; opisuje różnice w budowie atomów izotopów, np. wodoru; wyszukuje informacje na temat zastosowań różnych izotopów. Ogólny cel kształcenia Uczeń definiuje pojęcie izotopu pierwiastka. Kompetencje kluczowe porozumiewanie się w języku ojczystym; porozumiewanie się w językach obcych; kompetencje matematyczne i podstawowe kompetencje naukowo‐techniczne; kompetencje informatyczne; umiejętność uczenia się. Kryteria sukcesu Uczeń nauczy się: wyjaśniać, co to są izotopy; opisywać izotopy za pomocą symboli; omawiać różnice w budowie atomów izotopów wodoru; obliczać masę izotopu. Metody/techniki kształcenia podające pogadanka. aktywizujące dyskusja. eksponujące film. programowane z użyciem komputera; z użyciem e‐podręcznika. praktyczne ćwiczeń przedmiotowych. Formy pracy praca indywidualna; praca w parach; praca całego zespołu klasowego. Środki dydaktyczne e‐podręcznik; zeszyt i kredki lub pisaki; tablica interaktywna, tablety/komputery. Przebieg lekcji Faza wstępna 1. Nauczyciel rozdaje uczniom metodniki lub kartki w trzech kolorach: zielonym, żółtym i czerwonym do zastosowania w pracy techniką świateł drogowych. Przedstawia cele lekcji sformułowane w języku ucznia na prezentacji multimedialnej oraz omawia kryteria sukcesu (może przesłać uczniom cele lekcji i kryteria sukcesu pocztą elektroniczną lub zamieścić je np. na Facebooku, dzięki czemu uczniowie będą mogli prowadzić ich portfolio). 2. Prowadzący wspólnie z uczniami ustala – na podstawie wcześniej zaprezentowanych celów lekcji – co będzie jej tematem, po czym zapisuje go na tablicy interaktywnej/tablicy kredowej. Uczniowie przepisują temat do zeszytu. Faza realizacyjna 1. Nauczyciel – w celu przypomnienia uczniom wiadomości na temat budowy atomu – zadaje pytania, np.: „Czym jest atom?”, „Jakie rodzaje cząstek elementarnych wchodzą w skład atomu?”, „Jakie cząstki elementarne znajdują się w jądrze, a jakie na zewnątrz jądra?”. Następnie prosi o przypomnienie pojęć: liczba atomowa, masa atomowa, jednostka masy atomowej. 2. Uczniowie czytają fragment pt. „Różnice w atomach tego samego pierwiastka” i własnymi słowami wyjaśniają pojęcie izotopu. Następnie prowadzący zajęcia prosi podopiecznych, żeby zastanowili się, czy izotopy tego samego pierwiastka mają jednakowe liczby: atomową i masową, a jeśli nie, która z tych liczb może być różna. Zaakceptowane przez nauczyciela odpowiedzi, uczniowie zapisują w formularzu zamieszczonym w abstrakcie. 3. Nauczyciel prezentuje tabelę przedstawiającą izotopy azotu. Prosi uczniów o jej wspólną analizę: zwraca uwagę na opis izotopów pierwiastka za pomocą symbolu. 4. Uczniowie wykonują polecenie nr 2: na podstawie układu okresowego przedstawiającego procentową zawartość trwałych izotopów poszczególnych pierwiastków ustalają, ile pierwiastków ma tylko jedną naturalną odmianę izotopową i które pierwiastki mają ich najwięcej. 5. Uczniowie czytają fragment pt.
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