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Izvedbeni Planovi SVEU ČILIŠTE U SPLITU SVEU ČILIŠNI ODJEL ZA STUDIJE MORA DETALJNI IZVEDBENI NASTAVNI PLANOVI PREDDIPLOMSKI STUDIJ BIOLOGIJA I EKOLOGIJA MORA Naziv predmeta OP ĆA KEMIJA Kod predmeta SMB101 Satnica predmeta 45/30/30 (P/S/V) ECTS 8 (5 - predavanja, seminari, konzultacije, samostalno u čenje i 3- laboratorijske vježbe, (uz obrazloženje) kolokviji) Status predmeta obavezan X izborni (ozna čiti X) temeljni X napredni specijalisti čki Studijski program i Biologija i ekologija mora / Preddiplomski studij razina studija Godina/semestar I. godina / I. semestar Preduvjeti za upis - Jezik poduke i mogu ćnost pra ćenja na Hrvatski drugim jezicima Nositelj predmeta Prof. dr. sc. Slobodan Brini ć, izvanredni profesor Voditelj - voditelj seminara: doc. dr. sc. Marijo Buzuk vježbi/seminara - voditelj vježbi: Nives Vladislavi ć, dipl. ing., asistent O predmetu (kratak opis, osnovna zada ća i cilj predmeta, u kojem se obliku organizira nastava, op će upute te upute o poha đaju nastave, obveze studenata...) Poha đanjem predmeta Op ća kemija studenti će se upoznati sa temeljnim kemijskim zakonitostima i principima. Savladat će kemijsku nomenklaturu i upoznati se sa osnovama laboratorijskog rada. Razviti će sposobnost kriti čkog razmišljanja o eksperimentima provedenim u laboratoriju i uklju čenosti kemije u svakodnevni život. Nastava iz kolegija Op ća kemija odvija se kroz predavanja, seminare i vježbe. Svi oblici nastave su obavezni. Da bi student dobio potpis iz kolegija, a koji mu je nužan za polaganje ispita treba zadovoljiti slijede će uvjete: • prisutnost predavanjima (minimalno 10 predavanja), • prisutnost seminarima (minimalno 10 seminara), • odra đene vježbe (100% iznos). Da bi student mogao pristupiti izvo đenju pojedine vježbe prethodno mora položiti kolokvij iz gradiva vježbe. Kolokvij može biti pismeni ili usmeni. Bez položenog kolokvija nije mogu će pristupiti izvo đenju vježbe. Vježbe koje nisu odra đene u dogovorenim terminima nadokna đuju se na kraju semestra. Mogu će je nadoknaditi dvije vježbe. Tijekom semestra student zbog opravdanog razloga (bolest – opravdava se lije čni čkom potvrdom) može izostati maksimalno sa dvije vježbe. Vježbe koje je student izostao nadokna đuju se na kraju semestra. Popis obavezne literature 1. Filipovi ć, S. Lipanovi ć, 1995. Op ća i anorganska kemija 1. i 2. dio, Školska knjiga, Zagreb. 2. B. Peri ć, Kemijsko ra čunanje, HDKI/Kemija u industriji, Zagreb, 2006. 3. M. Sikirica, 2001. Stehiometrija, Školska knjiga, Zagreb. 4. Vježbe iz op će i anorganske kemije I. Interna skripta, 2004. Kemijsko - tehnološki fakultet u Splitu, Split. Popis izborne literature 1. R. Chang, Chemistry, McGraw-Hill, Inc., New York, 1991. 2. J. W. Hill, R. H. Petrucci, General Chemistry, Prentice-Hall, New Jersey, 2002. 3. J. C. Kotz, P. Treichel Jr., Chemistry & Chemistry reactivity, Sounders College Publishing, New York, 1999. Nastavni plan (popis svih predavanja/seminara/vježbi s naslovima, pojašnjenjima i ishodima u čenja) Predavanje 1. Uvod - Prirodne znanosti i kemija. Mjerne jedinice i mjerenje. Klasifikacija materije. Čiste tvari. Rastavljanje tvari na čiste tvari. Svojstva čistih tvari. Vrste čistih tvari, atom i kemijski element. Ishod u čenja: Ponoviti definicije mjernih jedinica, decimalne jedinice. Upoznati podjelu tvari i na čine njihovog rastavljanja. Usvojiti razlike izme đu pojmova mase i težine. Predavanje 2. Svojstva čistih tvari, fizi čka i kemijska svojstva. Atom i kemijski element. Kemijski simboli elemenata. Zakoni kemijskog spajanja po masi i volumenu. Atomska teorija - od ranih ideja do Johna Daltona. Avogadrova hipoteza. Ishod u čenja: Znati razlikovati fizi čka i kemijska svojstva tvari, intenzivna i ekstenzivna svojstva. Znati definirati zakone kemijskog spajanja po masi. Upoznavanje s razlozima uvo đenja i povijesne definicije atoma i relativne atomske mase. Objasniti Gay-Lussacov zakon spojnih volumena pomo ću kojeg je Avogadro uveo pojam molekula. Predavanje 3. Otkri će strukture atoma. Otkri će rendgenskih zraka i radioaktivnosti. Rutherfordov model atoma. Rendgenske zrake i struktura kristala. Braggova jednadžba. Izotopi i struktura atomske jezgre. Ishod u čenja: Ponašanje nabijene čestice u elektri čnom i magnetnom polju. Elektron i na čin otkri ća njegovog naboja i mase. Objašnjenje radioaktivnosti. Otkri će atomske jezgre i protona. Objašnjnje strukture atomske jezgre i izotopa. Predavanje 4. Struktura čistih tvari. Atomska struktura čistih tvari. Tipovi kristalnih sustava i karakteristike kristala. Kubi čni kristalni sustav. Molekulska struktura čistih tvari. Priroda plina. Priroda teku ćine. Pojam temperature. Kineti čka teorija plinova. Ishod u čenja: Poznavanje kristalnih sustava. Teseralni kristalni sustav. Agregatna stanja tvari i temperatura. Predavanje 5. Plinski zakoni i jednadžba stanja idealnog plina. Realni plinovi. Relativna atomske i molekulske mase. Metode odre đivanja relativnih atomskih (Dulong-Petitova metoda, difrakcija rendgenskih zraka, spektrograf masa) i molekulskih masa (iz gusto će plina, metodom Victora Mayera, Hoffmanova metoda). Periodni sustav elemenata i periodni zakon. Ishod u čenja: Definirati varijable koje opisuju stanje plina. Objasniti Boyle Mariottov zakon i Charles Guy lissacov zakon te jednadžbu stanja idealnog plina. razlika izme đu realnih i idealnih plinova. Predavanje 6. Elektronska struktura atoma - Bohrov model atoma, kvantni brojevi. Kvantna teorija i elektronska struktura atoma. Atomske orbitale. Ishod u čenja: Objasniti spektar elektromagnetskog zra čenja. Uzroci apsorpcije i emisije zra čenja. Objasniti Planckovu jednadžbu energije i zra čenja. Objasniti fotoelektri čni efekt i Einsteinovu fotoelektri čnu jednadžbu. Objasniti Bohrov model atoma vodika i rješenje modela. Predavanje 7. Periodi čna klasifikacija elemenata i periodni sustav. Periodi čne promjene fizikalnih osobina. Atomski radijus. Energija ionizacije. Elektronski afinitet. Elektronegativnost. Ishod u čenja: Objasniti današnji periodni sustav elemenata i njihovu elektronsku strukturu. Predavanje 8. Kemijska veza i struktura molekula - Elektronska teorija valencije, ionski i kovalentni spojevi. Elektronegativnost i stupanj oksidacije. Pisanje Lewisovih struktura i pravilo okteta. Formalni naboji. Izuzeci od pravila okteta. VSEPR model i geometrija molekule. Ishod u čenja: Objasniti pojam valencije atoma elemenata. Objasniti uzroke ispajanja atoma elemenata. Objasniti uzroke nastajanja ionske veze i svojstava ionskih spojeva. Predavanje 9. Karakteristike veze. Teorija valentne veze i teorija molekulskih orbitala.. Ishod u čenja: Objasniti kako nastaje kovalentna veza. Razlika izme đu teorije valentne veze i teorije molekulskih orbitala. Predavanje 10. Me đumolekularne sile. Dipolni moment, Van der Waalsove i Londonove sile, vodikova veza. Struktura i osobine teku ćina i krutina. Fizikalne osobine otopina. Vrste otopina. Izražavanje koncentracije. Ishod u čenja: Objasniti vrste me đumolekulskih sila i zbog čega one nastaju. Objasniti što su to otopine. Navesti vrste otopina. Navesti na čine izražavanja koncentracija. Predavanje 11. Otopine teku ćina u teku ćinama. Otopine krutina u teku ćinama. Otopine plinova u teku ćinama. Utjecaj temperature na topljivost. Utjecaj tlaka na topljivost plinova. Koligativne osobine otopina neelektrolita i koligativne osobine otopina elektrolita. Ishod u čenja: Objasniti razloge otapanja ionskih spojeva. Objasniti ovisnost otapanja o toplini i Le Chatellierov princip. Predavanje 12. Kemijske reakcije - vrste kemijskih reakcija, redoks reakcije, reakcije kompleksa (protoliti čke reakcije i reakcije taloženja i otapanja), složene reakcije. Ishod u čenja: Objasniti redoks reakcije. Razumijeti što su oksidacijska, a što redukcijska sredstva. Objasnit kako nastaju reakcije otapanja i taloženja. Predavanje 13. Kemijska kinetika, brzina reakcije, mehanizam reakcije, energija aktivacije. Kemijska ravnoteža - Pojam ravnoteže, kemijska ravnoteža i konstanta kemijske ravnoteže. Faktori koji utje ču na kemijsku ravnotežu. Ishod u čenja: Objasniti endotermne i egzotermne reakcije. Objasniti što je energija aktivacije i kako na nju djeluju katalizatori. Navesti o čemu ovisi brzina kemijske rekcije. Predavanje 14. Ravnoteže u homogenim i heterogenim sustavima. Ishod u čenja: Objasniti kada u reakcijama nastaje stanje ravnoteže. Navesti i objasniti zakon kemijske ravnoteže. Objasniti utjecaj temperature na kemijsku ravnotežu. Predavanje 15. Ravnoteže u otopinama elektrolita - ravnoteže u otopinama kiselina i baza, ravnoteže u otopinama kompleksa, ravnoteže izme đu otopine i neotopljenog kristala, redoks ravnoteže Ishod u čenja: Objasniti ravnotežu u otopinama elektrolita. Ionski produkt vode, pH. Seminar 1. Stupanj oksidacije: Definicija, pravila za odre đivanje stupnja oksidacije atoma, iona, molekula. Primjeri i uvježbavanje. Ishod u čenja: Odrediti stupanj oksidacije atoma, iona i molekule. Seminar 2. Nomenklatura anorganske kemije. Nazivi monoatomnih kationa. Nazivi monoatomnih aniona. Nazivi poliatomnih kationa. Nazivi poliatomnih aniona. Nazivi liganada. Nazivi kompleksniih iona. Nazivi oksokiselina i njihovih soli. Ishod u čenja: Pravila za imenovanje anorganskih iona i spojeva Seminar 3. Uvježbavanje naziva anorganskih spojeva. Ishod u čenja: Ispravno imenovati ion i spoj. Na osnovu imena napisati formulu. Seminar 4. Uravnotežavanje kemijskih jednadžbi. Redoks jednadžbe Ishod u čenja: Uz pomo ć parcijalnih redoks jednadžbi uravnotežiti redoks jednadžbu. Seminar 5. Uvježbavanje pisanja redoks jednadžbi. Ishod u čenja: Uz pomo ć parcijalnih redoks
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