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Oxides: Naming and Use Oxides: naming and use Oxides: naming and use Lesson plan (Polish) Lesson plan (English) Oxides: naming and use Link to the lesson Before you start you should know the properties of oxygen; the use of oxygen; how to define combustion; how to write the synthesis reaction of metal and non‐metal oxides; what oxides are and how they are produced; examples of oxides. You will learn to name oxides; to correctly write molecular and structural formulas of selected metal and non‐metal oxides basing on their names; to name the oxide basing on its molecular formula; to indicate those oxides that can be found in nature; what the uses of oxides are; to describe the physical properties of selected oxides (e.g. calcium oxide, aluminum oxide, iron oxides, carbon oxides, silicon dioxide, sulfur oxides). Nagranie dostępne na portalu epodreczniki.pl Nagranie dźwiękowe abstraktu Naming of oxides Oxides are binary compounds with oxygen where the oxidation state of oxygen is O-II. Oxygen in chemical compounds is always divalent. Other elements may have different valency number and form one or more oxides (alkali metals, alkaline earth metals, fluoride have only valence of 1). In the names of oxides, the word “oxide” must be preceded by the name of the element that binds to oxygen. The name is composed of the cation name and the word oxide. Examples: Na2O sodium oxide CaO calcium oxide SnO tin(II) oxide or stannous oxide SnO2 tin(IV) oxid Oxides of non‐metals are named by stating the name of the element first, followed by the word oxide. Numeral prefixes are used where necessary: Examples: NO nitrogen oxide or nitrogen monoxide N2O5 dinitrogen pentoxide Cl2O dichlorine oxide Cl2O5 dichlorine pentoxide Some elements form only one type of oxide. In these cases, the use of numerical prefixes is not necessary: Examples: Al2O3 aluminum oxide SiO2 silicon oxide To derive a formula for an oxide, write the symbols of the elements together with indices according to the numerical prefix that indicates the number of specified atoms in the molecule. If a given element forms more than one oxide, then its valency number should also be specified by Roman numeral in brackets. Example: dinitrogen oxide N2O In the case of metal oxides, where the numerical prefixes are not usually used, we have to obey the rule of electroneutrality. Examples: III II boron oxide B2 O3 → B2O3 V II diarsenic pentaoxide As2 O5 → As2O5 Naming of oxides Source: GroMar Sp. z o.o., licencja: CC BY 3.0. Task 1 Watch the presentaon. Note how the names of oxides are created. Source: GroMar Sp. z o.o., licencja: CC BY-SA 3.0. Examples of oxides Valence Elemental number Molecular formula Oxide name symbol in of oxide compounds Mg II MgO magnesium oxide monosulfur dioxide or sulfur S IV SO2 dioxide monosulfur trioxide or sulfur S VI SO3 trioxide C II CO carbon monoxide monocarbon dioxide or C IV CO2 carbon dioxide N IV NO2 nitrogen dioxide N III N2O3 dinitrogen trioxide N V N2O5 dinitrogen pentoxide Cu I Cu2O copper(I) oxide Cu II CuO copper(II) oxide Fe III Fe2O3 iron(III) oxide Uses of oxides Metal and non‐metal oxides are widely used. Some oxides are found in nature. They include: metal oxides: iron, aluminum; non‐metal oxides: hydrogen (water), silicon (main component of sand), carbon, nitric. Aplet Iron(III) oxide occurs in the form of a mineral - hematite. Due to its red color, it can be used as a pigment in the production of paints and varnishes. Aluminum oxide occurs in the form of a mineral - corundum. Gemstones are used in jewelery, while aluminum oxide, due to its high hardness, is used for polishing and as an abrasive. Calcium oxide is used for the production of cement and masonry mortars (quicklime) and in laboratories for the drying of liquids and gases. It is also used in the production of artificial fertilizers. Task 2 Look at the interacve illustraon and remember uses of several oxides. 1 6 7 5 2 4 3 1. arsenic(III) oxide (arsenic), very strong poison, the ingredient of a rat trunk, enamel and paints, used also for the preservaon of hides and skins and wood 2. sulfur dioxide a bleaching and disinfecon agent used in the producon of paper and wine 3. magnesium oxide for use in the manufacture of casngs, cement and refractories 4. silicon dioxide for use in the manufacture of glass, mortar, cement and ceramics, and to obtain silicon 5. nitrous oxide laughing gas used for local anesthezaon and as a chemical food addive 6. carbon dioxide for use in the manufacture of carbonated beverages and as a fire exnguishing agent 7. use of oxides Exercise 1 Exercise 2 Pair the molecular formula with the oxide name. nitric oxide, calcium oxide, iron(III) oxide, manganese(IV) oxide, silicon monoxide, sulfur dioxide SO2 CaO SiO Fe2O3 NO MnO2 Exercise 3 Write the name of the oxide based on formula. P4O10 .................................................. Li2O2 ................................ SO3 .............................. CO2 ............................ N2O ...................................... Fe2O3 .............................. Ag2O .............................. Al2O3 ........................................ CuO ................................ Naming of peroxides Metal peroxides Source: GroMar Sp. z o.o., licencja: CC BY 3.0. Conclusion Oxides are compounds of oxygen with other elements. Oxides are formed as a result of synthesis reactions, oxidation reactions of decomposition reactions and reduction reactions. Names of all oxides in English are formed and read from left to right. First you mention the name of the element that reacts with oxygen, and then you use the term “oxide”. If a given element forms more than one oxide, then its valency number should also be specified by Roman numeral in brackets. Metal and non‐metal oxides are widely used. Some oxides are found in nature. Source: GroMar Sp. z o.o., licencja: CC BY-SA 3.0. Keywords oxygen, oxides, use of oxides, synthesis reaction, combustion, naming of oxygens, metal oxide, non‐metal oxide Glossary oxide Nagranie dostępne na portalu epodreczniki.pl Nagranie dźwiękowe słówka tlenek – związek, w którym tlen jest związany z innym pierwiastkiem chemicznym, np.: K2O, MgO, SiO2, SO3, Cl2O7 hydrogen peroxide Nagranie dostępne na portalu epodreczniki.pl Nagranie dźwiękowe słówka nadtlenek wodoru (H2O2, woda utleniona) – najprostszy nadtlenek (związek z pojedynczym wiązaniem tlen‐tlen); jest stosowany jako utleniacz, środek wybielający i antyseptyczny Lesson plan (Polish) Temat: Tlenki: tworzenie nazw i zastosowanie Adresat Uczeń szkoły podstawowej (klasy 7. i 8.) Podstawa programowa: Szkoła podstawowa. Chemia. IV. Tlen, wodór i ich związki chemiczne. Powietrze. Uczeń: 1) projektuje i przeprowadza doświadczenie polegające na otrzymaniu tlenu oraz bada wybrane właściwości fizyczne i chemiczne tlenu; odczytuje z różnych źródeł (np. układu okresowego pierwiastków, wykresu rozpuszczalności) informacje dotyczące tego pierwiastka; wymienia jego zastosowania; pisze równania reakcji otrzymywania tlenu oraz równania reakcji tlenu z metalami i niemetalami; 2) opisuje właściwości fizyczne oraz zastosowania wybranych tlenków (np. tlenku wapnia, tlenku glinu, tlenków żelaza, tlenków węgla, tlenku krzemu(IV), tlenków siarki). Ogólny cel kształcenia Uczeń wyjaśnia, na czym polega reakcja spalania pierwiastków w tlenie. Wskazuje zastosowanie tlenków Kompetencje kluczowe porozumiewanie się w językach obcych; kompetencje informatyczne; umiejętność uczenia się. Kryteria sukcesu Uczeń nauczy się: tworzyć nazwy tlenków; zapisywać poprawnie wzory sumaryczne i strukturalne przykładowych tlenków metali i niemetali na podstawie nazwy; podawać nazwę tlenku na podstawie wzoru sumarycznego; wskazywać, które tlenki występują w przyrodzie; jakie jest zastosowanie tlenków; opisywać właściwości fizyczne wybranych tlenków (np. tlenku wapnia, tlenku glinu, tlenków żelaza, tlenków węgla, tlenku krzemu(IV), tlenków siarki). Metody/techniki kształcenia aktywizujące dyskusja. podające pogadanka. eksponujące film. programowane z użyciem komputera; z użyciem e‐podręcznika. praktyczne ćwiczeń przedmiotowych. Formy pracy praca indywidualna; praca w parach; praca w grupach; 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. 3. BHP – przed przystąpieniem do eksperymentów uczniowie zapoznają się z kartami charakterystyk substancji, które będą używane na lekcji. Nauczyciel wskazuje na konieczność zachowania ostrożności w pracy z nimi. Faza realizacyjna 1. Prowadzący zajęcia wyświetla na tablicy multimedialnej tabelę „Tworzenie nazw tlenków” i omawia ją, tłumacząc zasady konstruowania nazw tlenków. Zadaje uczniom pytanie: „Co to są tlenki?”. Podczas rozmowy podaje przykładowe nazwy tlenków naprzemiennie z wzorami sumarycznymi – chętni zapisują nazwy tlenków oraz wzory sumaryczne i strukturalne na tablicy. 2. Nauczyciel w oparciu o tabelę „Przykłady
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