ࡱ> 7 x4bjbjUU P7|7|u0lpppp$ y y y $ Dy W "y y y M M M M y 8M y M FM  p~Rlp= 0 M TABELUL PERIODIC AL ELEMENTELOR Au existat in decursul timpului mai multe tentative ale chimistilor de clasificare a elementelor chimice: in metale si nemetale, acizi si baze, in functie de valenta sau de alte proprietati. Aplicarea acestor metode facea insa ca o serie de elemente sa se regaseasca in mai multe grupe concomitent. O clasificare mai detaliata si mai utila s-a bazat la inceput pe greutatea atomica si apoi pe numarul atomic. Aceasta clasificare a condus la ceea ce cunoastem astazi sub denumirea de sistemul periodic, inclus in tabelul periodic care ilustreaza grafic legaturile dintre diferite elemente. Notatia atomica Notatia atomica este o modalitate de de a descrie doua proprietati principale ale unui element numarul atomic si numarul de masa. Elementele se scriu de obicei sub forma baX, unde X este simbolul chimic al elementului, a este numarul sau atomic iar b este numarul de masa. 1. Scurt istoric Clasificarea initiala a elementelor cunoscute in metale si nemetale a condus mai departe la diferentieri in functie de reactivitate. S-a observat ca unele elemente au proprietati intermediare intre metale si nemetale, acestea primind denumirea de metaloizi. In 1828, J.W. Dbereiner a remarcat ca la unele elemente exista aceeasi diferenta intre greutatea lor atomica (termenul actual utilizat este masa atomica relativa) atunci cind sunt aranjate in grupe de cite trei. De exemplu, a observat aceeasi diferenta intre greutatea atomica a elementelor clor brom si brom iod. Pe aceeasi baza a gasit si alte grupari asemanatoare care au devenit cunoscute sub denumirea de triadele lui Dbereiner. John Newlands a aratat in 1864 ca aceste clasificari sunt parte integranta dintr-o schema mai generala. Newlands a grupat elementele pe linie in ordinea masei lor atomice si atunci cind a observat aparitia unor elemente cu proprietati similare la intervale regulate, a regrupat elementele si in in coloane:  Newlands a observat ca proprietatile primelor sapte elemente reapar si la urmatoarele sapte, astfel incit primul si al optulea, al doilea si al noulea si asa mai departe, apartin aceluiasi grup sau familii. El a numit acest fenomen legea octavelor. Gazele nobile care nu fusesera descoperite pina in anul 1890, si-au gasit locul in aceasta schema la sfirsitul fiecarei linii. Aceasta teorie nu a fost luata in serios la acea vreme mai mult datorita alegerii termenului muzical de octava de catre Newlands. Ideile lui Newlands au fost dezvoltate si reformulate mai clar de catre chimistul rus Dmitry Mendeleyev. Mendeleyev a formulat legea periodicitatii care se bazeaza pe ipoteza ca proprietatile elementelor sunt intr-o dependenta periodica in functie de masele lor atomice. El a aranjat elementele intr-un tabel, lasind spatii libere acolo unde nu existau elemente cunoscute cu masa atomica sau proprietati fizice si chimice corespunzatoare pozitiei respective. Primele opt elemente dupa hidrogen si heliu sunt litiu, beriliu, bor, carbon, nitrogen, oxigen, fluor si neon (neonul inca nu fusese descoperit la vremea aceea). Aceste elemente au fost grupate de catre Mendeleyev pentru a forma prima linie sau perioada din tabelul periodic. Celelalte elemente cunoscute au fost aranjate sub aceasta prima linie in ordinea masei lor atomice astfel incit sa rezulte un tabel in care elementele de pe coloane prezinta proprietati similare. Mendeleyev a aranjat de asemenea si elementele pe care le cunoastem astazi sub denumirea de metale tranzitorii in perioade mai lungi astfel incit sa nu se regaseasca in tabel in regiunea ocupata de nemetale. Decizia lui Mendeleyev de a lasa anumite locuri libere in tabel a fost confirmata ulterior prin descoperirea de elemente ale caror proprietati fusesera astfel anticipate. De exemplu, el a prognozat descoperirea unui element pe care l-a numit eka-aluminiu si ale carui proprietati le-a intuit printr-un studiu al tendintelor si similitudinilor dintre elementele din tabelul sau. Patru ani mai tirziu a fost descoperit galiu ale carui proprietati corespundeau pe deplin cu cele prognozate de catre Mendeleyev. Tabelul periodic al elementelor este instrumentul cel mai valoros in studiul chimiei anorganice. A ajutat la estimarea masei atomice relative reale a elementelor si la descoperirea de noi elemente. Un studiu mai riguros al sistemului periodic bazat pe masa atomica scoate insa in evidenta si o serie de anomalii; de exemplu, argonul si potasiul, iodul si telluriumul, cobaltul si nichelul, judecind dupa proprietatile lor, ar trebui sa fie plasate incorect in functie de masele lor atomice. Aceasta anomalie a ramas o lunga perioada de timp neexplicata, dar acum se cunoaste ca masa atomica a unui element are o importanta mai mare decit masa atomica relativa. Aceste anomalii dispar atunci cind elementele sunt aranjate in functie de numarul atomic. 2. Gruparea elementelor in tabelul periodic Tabelul periodic al elementelor este aranjat astfel incit sa scoata in evidenta similitudinea dintre anumite elemente. Elementele dintr-o anumita zona a tabelului au proprietati asemanatoare in timp ce elementele situate la o distanta semnificativa au un comportament diferit. Intre aceste extreme exista o variatie gradata a proprietatilor fizice si chimice ca rezultat al masei atomice relative si configuratiei electronice a elementelor care intervin in aceasta zona intermediara. 2.1 Perioade Elementele dintr-o perioada au acelasi numar de straturi electronice in atom, numar care coincide si cu numarul stratului exterior. In cadrul aceleasi perioade elementele sunt aranjate in ordinea crescatoare a numerelor atomice. In aceeasi perioada fiecare element contine un electron in plus pe ultimul strat comparativ cu elementul anterior. Aceasta conduce la o crestere a masei nucleului si sarcinii elementelor de la stinga spre dreapta in cadrul fiecarei perioade, fara a avea insa si o crestere a numarului de straturi de electroni. Rezulta in acest fel o crestere a fortei de atractie exercitata de catre nucleu asupra electronilor din ultimul strat numit si strat de valenta. O alta consecinta este si contractarea stratului de valenta de la stinga spre dreapta, cu electronii din acest strat orbitind mai aproape de nucleu (scade raza atomica). Acest fenomen reflecta o tendinta de crestere a atractiei atomului pentru electroni pe masura ce ne deplasam de la stinga spre dreapta in cadrul aceleasi perioade. Metalele alcaline si alcalino-pamintoase care sunt situate la capatul din stinga al perioadelor prezinta o slaba atractie pentru electronii din stratul exterior de valenta, electroni pe care ii cedeaza usor formind astfel ioni pozitivi. Spunem ca aceste elemente sunt electropozitive, spre deosebire de elementele situate la dreapta perioadelor care sunt electronegative. Halogenii, situati la extremitatea din dreapta a perioadelor, sunt elemente puternic electronegative si, posedind o afinitate mare pentru electroni, formeaza usor ioni negativi cu metalele sau cu hidrogenul prin atragerea unui electron in stratul de valenta. 2.2 Grupe Deplasindu-ne de sus in jos in coloanele (grupele) tabelului periodic, fiecare element va avea un strat de electroni in plus fata de cel de deasupra lui. Chiar daca sarcina nucleului creste pe aceasta directie, straturile suplimentare si distanta din ce in ce mai mare a nucleului fata de electronii de pe ultimul strat face ca acesti electroni sa fie mai putin legati. Una dintre cauze o constituie influenta straturilor interioare de electroni care au un efect de ecranare, reducind astfel forta de atractie exercitata asupra electronilor de valenta, ceea ce conduce la formarea de cationi. Influenta combinata a acestor factori conduce la o tendinta puternica a elementelor metalice din coltul din stinga jos al tabelului periodic (metalele alcaline grele) de a forma cationi, in timp ce elementele nemetalice din coltul din dreapta sus (halogenii usori) formeaza anioni. 2.3 Legaturi pe diagonala Ca urmare a celor doua tendinte importante din tabelul periodic contractia straturilor de electroni de la stinga la dreapta perioadelor (cresterea electronegativitatii) si cresterea numarului de straturi de electroni in grupe de sus in jos (descresterea electronegativitatii) se intimpla deseori ca un element sa aiba o raza atomica si raza ionica apropiate de ale elementului pozitionat mai jos pe diagonala decit elementele din propria grupa. Deoarece exista o serie de proprietati care sunt dependente de aceste raze si de valorile electronegativitatii, comportarea elementelor situate pe diagonala poate fi uneori asemanatoare. De exemplu, litiu se aseamana ca proprietati chimice cu magneziu mai mult decit ne-am astepta. Astfel de asemanari pot fi observate si in cazul altor perechi de elemente pozitionate similar. Exemple de legaturi pe diagonala in tabelul periodic 3. Blocurile de elemente de tip s, p, d si f Este cunoscut ca substraturile de electroni sunt formate din orbitali de acelasi tip si care au aceeasi energie; acestia sunt notati cu simbolurile s, p, d, f. Tipuri de orbitali Elementele chimice se pot clasifica in grupuri sau blocuri, dupa tipul de orbital in care intra electronul distinctiv. 3.1 Elemente de tip bloc s Toate elementele din blocul s sunt metale si se regasesc in grupele 1 si 2 ale tabelului periodic. Blocul s contine metalele alcaline si metalele alcalino-pamintoase. Aceste metale sunt puternic reactive, pierzind cu usurinta electronii lor de valenta pentru a forma compusi ionici cu numere de oxidare +1 sau +2 (Numarul de oxidare este un numar care indica citi electroni trebuie sa primeasca sau sa cedeze atomul dintr-un compus pentru a forma un atom neutru. Avind numai unul sau doi electroni de valenta, legatura metalica din structura metalelor din blocul s este relativ slaba, astfel incit acestea sunt metale cu temperaturi de topire scazute. 3.2 Elementele de tip bloc p Elementele de tip bloc p sunt cele din grupele 13-18 din tabelul periodic. Blocul include un amestec de metale de tip bloc p si nemetale. Metaloizii (sau semi-metalele germaniu, arsenic, antimoniu) se gasesc si ei in acest bloc. Toate aceste elemente au orbitalii de tip p partial ocupati. Aceste elemente prezinta o variatie mai mare a proprietatilor fizice si chimice comparativ cu cele din blocul de tip s. Blocul p include si halogenii puternic reactivi si un numar de nemetale extrem de importante cum ar fi carbonul, nitrogenul si oxigenul. Aceste elemente tind sa formeze intre ele compusi covalenti. Tot in blocul p se regasesc si gazele nobile. 3.3 Elemente de tip bloc d Blocul d contine metalele tranzitionale care au partial ocupat orbitalii d. Energetic, acesti orbitali sunt asemanatori cu cei situati imediat deasupra lor. Ca urmare a energiei tranzitionale scazute, electronii din orbitalul d pot trece usor pe un nivel energetic mai inalt prin absorbtia de radiatii electromagnetice din domeniul vizibil. Unele dintre elementele cele mai grele din blocul d prezinta o puternica instabilitate nucleara, motiv pentru care nu se gasesc in forma naturala ci trebuie produse numai pe cale sintetica. 3.4 Elemente de tip bloc f Elementele din blocul f sunt lantanidele si actinidele. Acestea au orbitalii 4f sau 5f ocupati partial sau total si uneori au orbitalul 5d sau 6d ocupat pe jumatate. Ca urmare a diferentelor mici intre nivelele energetice din aceasta regiune a tabelului periodic, lantanidele au proprietati asemanatoare. O contractie pronuntata apare in seria lantanidelor din blocul f. Ca rezultat al acestei contractii, elementele care urmeaza in tabel imediat dupa lantanide au raze atomice si ionice similare cu elementele din grupa situata imediat la stinga lantanidelor. Tendinta generala pentru elementele cu electronegativitate puternic diferita intre ele este de a forma legaturi ionice. Atomii metalelor tind sa formeze cationi (ioni pozitivi) avind o raza ionica mare. Nemetalele tind sa formeze legaturi covalente intre ele. Oricare dintre elementele din grupa metalelor tranzitionale, inclusiv lantanidele si actinidele prezinta o mai mare asemanare intre ele decit exista in alte zone ale tabelului periodic. 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