halkogeni elementi
DESCRIPTION
HALKOGENI ELEMENTI. ELEMENTI 16. SKUPINE (ns 2 np 4 ). O, S – nemetali Se, Te – polumetali Po – radioaktivni metal. Tvore VIŠEATOMNE MOLEKULE Broj atoma u molekuli ovisi o veličini atoma pr. O 2 , O 3 – plinovi S 8 - krutina. Spajaju se s VODIKOM → hidridi. - PowerPoint PPT PresentationTRANSCRIPT
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HALKOGENI ELEMENTI
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ELEMENTI 16. SKUPINE
(ns2 np4)
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• O, S – nemetali• Se, Te – polumetali• Po – radioaktivni metal
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• Tvore VIŠEATOMNE MOLEKULE
• Broj atoma u molekuli ovisi o veličini atoma
• pr. O2, O3 – plinovi
S8 - krutina
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• Spajaju se s VODIKOM → hidridi
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• Spajaju se s KISIKOM → oksidi
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KISIK
• Rasprostranjenost...
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KISIK
• Paramagnetična molekula
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ALOTROPSKE MODIFIKACIJE
• Molekula kisika: O2
• Molekula ozona: O3
• ALOTROPI – različiti oblici istovrsnih elemenata u kojima su kemijske veze različite
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SVOJSTVA
• Plin bez boje, okusa, mirisa• Ne gori, ali podržava gorenje
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DOBIVANJE KISIKA
• Iz spojeva bogatih kisikom• npr. elektrolizom vode• npr. frakcijskom destilacijom tekućeg zraka• npr. žarenjem KMnO4 ili KClO3
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ŽARENJE KMnO4
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ŽARENJE KClO3
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OZON
• Alotropska modifikacija kisika• Plavkasti plin karakterističnog mirisa• Nastajanje ozona...• Freoni, haloni• Upotreba ozona
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FREONI
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H2O2
• Jako oksidacijsko sredstvo• Nestabilna bezbojna tekućina• Može biti oksidans i reducens• Raspad H2O2: 2 H2O2 → 2 H2O + O2
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RASPAD VODIKOVOG PEROKSIDA
2 H2O2 → 2 H2O + O2
SKICIRAJ POKUS!
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H2O
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TVRDOĆA VODE
• U prirodnim se vodama nalaze Ca2+, Mg2+, HCO3
-, Na+, SO42-, Cl- ...
→ to je TVRDA VODA
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KARBONATNA TVRDOĆA
Ca(HCO3)2
Mg(HCO3)2
→ zagrijavanjem se talože u obliku KAMENCA
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STALNA (NEKARBONATNA) TVRDOĆA
• Čine je OSTALE SOLI• Može se ukloniti samo kemijskim postupcima
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UKUPNA TVRDOĆA
KARBONATNA TVRDOĆA + STALNA TVRDOĆA
- Jedinica za iskazivanje tvrdoće vode: oNj
1 oNj = 10 mg CaO na L vode
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MEKŠANJE VODE1. KATIONSKI IZMJENJIVAČI - zamjenjuju se kationi (Ca2+, Mg2+) s H+
2. ANIONSKI IZMJENJIVAČI - izmjenjuju se anioni (SO42-) s OH-
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SUMPOR
• Rasprostranjenost...• Minerali sumpora
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SVOJSTVA
• Čvrsta tvar, svijetložute boje• Molekulski kristal prstenaste strukture (S8)
• Netopljiv u vodi• Topljiv u nepolarnim otapalima
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POLIMORFI SUMPORA
• ROMPSKI (S8) MONOKLINSKI (S8)
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DOBIVANJE SUMPORA
• Iskapanjem iz Zemljine kore
ili
• FRASCHOVIM POSTUPKOM
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SPOJEVI SUMPORA
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H2S
• Po obliku sličan H2O
• Ali nema H-veza jer je S manje elektronegativan od O
• Zato je H2S PLINOVIT pri sobnoj temperaturi
• Vrlo OTROVAN• Topljiv u H2O: H2S(g) → H2S(aq)
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DOBIVANJE H2S(g)
FeS(s) + 2 HCl(aq) → H2S(g) + FeCl2(aq)
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SO2
• Bezbojan plin, oštrog mirisa, izaziva kašalj• Dobivanje: S + O2 → SO2
• Topljiv u H2O: SO2 + H2O → H2SO3
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SO3
• Hlapljiva tekućina• Kristalizira pri temp. nižoj od 16,8oC• Dobivanje: SO2 + O2 → SO3
• Topljiv u vodi: SO3 + H2O → H2SO4
• Topljiv u konc. H2SO4: SO3 + H2SO4 → H2S2O7
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H2SO4
• Spada među najjače kiseline• Čista H2SO4 je BEZBOJNA ULJASTA TEKUĆINA
• Zagrijavanjem otpušta SO3, dok ne dostigne konstantno vrelište (338oC)
• Tada ima konstantan sastav s masenim udjelom od 98% → obična KONC. H2SO4
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DOBIVANJE H2SO4
• KONTAKTNI POSTUPAK:
S + O2 → SO2
2 SO2 + O2 → 2 SO3
SO3 + H2SO4(conc) → H2S2O7
OLEUM (“dimeća”)
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POKUSI...
Dolazi dječak iz škole.-Što ste danas radili u školi, sine - upita ga otac.-Pokuse iz kemije.-A što ćete raditi sutra u školi?-U kojoj školi?
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SVOJSTVA H2SO4
1. TKANINA (PAPIR) + H2SO4(conc)
2. CuSO4 5H∙ 2O + H2SO4(conc)
3. RAZRJEĐIVANJE H2SO4(conc)
4. ŠEĆER + H2SO4(conc)
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DOBIVANJE PLASTIČNOG SUMPORA