Olovo

Olovo
Opšta svojstva
Ime, simbol	olovo, Pb
Izgled	metalično siv
U periodnome sistemu
talijum ← olovo → bizmut	‍
Atomski broj (Z)	82
Grupa, perioda	grupa 14 (ugljenikova grupa), perioda 6
Blok	p-blok
Kategorija	postprelazni metal
Rel. at. masa (Ar)	207,2(1)
El. konfiguracija
po ljuskama	2, 8, 18, 32, 18, 4
Fizička svojstva
Tačka topljenja	600,61 K (327,46 °‍C, 621,43 °F)
Tačka ključanja	2022 K (1749 °‍C, 3180 °F)
Gustina pri s.t.	11,34 g/cm3
tečno st., na t.t.	10,66 g/cm3
Toplota fuzije	4,77 kJ/mol
Toplota isparavanja	179,5 kJ/mol
Mol. topl. kapacitet	26,650 J/(mol·K)
Atomska svojstva
Elektronegativnost	1,87 (+2)
Energije jonizacije	1: 715,6 kJ/mol ; 2: 1450,5 kJ/mol ; 3: 3081,5 kJ/mol
Atomski radijus	175 pm
Kovalentni radijus	146±5 pm
Valsov radijus	202 pm
	Spektralne linije
Ostalo
Kristalna struktura	postraničnocentr. kubična (FCC)
Brzina zvuka tanak štap	1190 m/s (na s.t.)
Topl. širenje	28,9 µm/(m·K) (na 25 °‍C)
Topl. vodljivost	35.3 W/(m·K)
Elektrootpornost	208 nΩ·m (na 20 °‍C)
Magnetni raspored	dijamagnetik
Magnetna susceptibilnost (χmol)	−23,0×10−6 cm3/mol (na 298 K)
Jangov modul	16 GPa
Modul smicanja	5,6 GPa
Modul stišljivosti	46 GPa
Poasonov koeficijent	0,44
Mosova tvrdoća	1,5
Brinelova tvrdoća	38–50 MPa
CAS broj	7439-92-1
Istorija
Otkriće	na Bliskom istoku (7000. p. n. e.)
Glavni izotopi
	Izotopska zastupljenost uveliko se razlikuje zavisno o uzorku
	reference • Vikipodaci

U prirodi, olovo se najčešće javlja u vidu sulfida, PbS, kao ruda galenit.

Prženjem se ruda prevodi u oksid čijom redukcijom nastaje sirovo olovo.^[3] Sirovo olovo sadrži: bakar, antimon, arsen, bizmut, cink, sumpor, kalaj, srebro i zlato. Prečišćavanjem sirovog olova (najčešće elektrolitičkim putem) dobija se čisto olovo plavičastobele boje, samo na svežem preseku je metalnog sjaja, no brzo potamni od stvorenog sloja oksida i baznog olovo(II) karbonata Pb(OH)₂*2PbCO₃, koji ga štite od dalje oksidacije. To je mek metal, velike gustine i niske temperature topljenja.^[4]

Olovo se u destilovanoj vodi ne rastvara, dok se rastvara u kiselinama sa oksidacionim dejstvom (npr. azotna kiselina). Pri dejstvu razblažene sumporne kiseline stvara se zaštitni sloj olovo- sulfata PbSO₄ te rastvaranje prestaje. Alkalije ne deluju na olovo. Na vazduhu se fino sprašeno olovo tzv. piroforno olovo pali samo od sebe.

Olovo (II) oksid se koristi za glaziranje keramičkih proizvoda, za izradu minijuma, kao žuta boja u slikarstvu. Olovo se koristi za izradu limova, kanalizacionih i vodovodnih cevi ukoliko vode nisu kisele; njime se oblažu električni kablovi i prevlači posuđe. Olovo se koristi i u vojnoj industriji, industriji boja, za izradu olovnih akumulatora, za zaštitu od rendgenskog i radioaktivnog zračenja.

Prve mine za olovke pravile su se od olovnih ruda, ali ih je u savremenom dobu zamenio neotrovni grafit, koji se kombinuje sa drugim primesama.

Vidi još

Reference

^ Meija et al. 2016.
^ Weast, Astle & Beyer 1983, str. E110.
^ Parkes, G.D. & Phil, D. (1973). Melorova moderna neorganska hemija. Beograd: Naučna knjiga.
^ Housecroft, C. E.; Sharpe, A. G. (2008). Inorganic Chemistry (3. izd.). Prentice Hall. ISBN 978-0-13-175553-6.

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Spoljašnje veze

[FOOTNOTEMeijaCoplenBerglundBrand2016-1] Meija et al. 2016.

[FOOTNOTEWeastAstleBeyer1983E110-2] Weast, Astle & Beyer 1983, str. E110.

[ParkesNeorganskaHemija-3] Parkes, G.D. & Phil, D. (1973). Melorova moderna neorganska hemija. Beograd: Naučna knjiga.

[Housecroft3rd-4] Housecroft, C. E.; Sharpe, A. G. (2008). Inorganic Chemistry (3. izd.). Prentice Hall. ISBN 978-0-13-175553-6.

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