Name: periodic table patterns and element groups
Uploaded: 2020-09-03T13:38:25.000Z
Duration: 3 min 25 s
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North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.2.1

The Periodic Table

La tavola periodica degli elementi &#xE8; un riferimento importante in chimica per l&#x27;organizzazione degli elementi. La tavola ha sette righe, o linee, numerate dall&#x27;alto verso il basso e diciotto colonne, chiamate gruppi o famiglie. Questi gruppi possono essere numerati in due modi diversi.Mentre il moderno sistema di numerazione, raccomandato dall&#x27;Unione Internazionale di Chimica Pura e Applicata, o IUPAC, numera i gruppi da 1 a 18, i Servizi Chimici Astratti utilizzano numeri romani e lettere per designare i gruppi. Gli elementi del gruppo principale sono designati con la lettera A e gli elementi di transizione sono designati con la lettera B.Gli elementi in una tavola periodica sono ordinati da sinistra a destra e dall&#x27;alto verso il basso, aumentando il numero atomico. Quelli con propriet&#xE0; simili rientrano nello stesso gruppo.Alcuni gruppi hanno nomi comuni. Gli elementi del gruppo 1, ad eccezione dell&#x27;idrogeno, sono noti come metalli alcalini e gli elementi del gruppo 2 come metalli alcalino terrosi. Tutti questi metalli sono molto reattivi e si trovano in natura combinati con altri elementi.Gli elementi non metallici altamente reattivi nel gruppo 17 sono noti come alogeni. Gli elementi non reattivi e non metallici del gruppo 18 sono indicati come gas nobili o inerti. Gli elementi possono essere suddivisi in tre grandi classi:metalli, non metalli e metalloidi.I metalli sono raggruppati a sinistra e al centro della tavola periodica e rapresentano la stragrande maggioranza degli elementi. Sono buoni conduttori di elettricit&#xE0; e calore. Tutti sono solidi a temperatura ambiente, eccezion fatta per il mercurio, che &#xE8; liquido.I metalli sono lucidi e possono essere lavorati in fogli e ridotti a fili. I metalli, come il potassio, tendono a perdere elettroni per formare cationi, ioni carichi positivamente, quando reagiscono con altri elementi. I non metalli sono raggruppati sul lato destro della tavola periodica e solitamente sono pessimi conduttori di calore ed elettricit&#xE0;.A temperatura ambiente, alcuni sono solidi, mentre altri sono liquidi o gas. I non metalli tendono ad acquisire elettroni e formare anioni, ioni carichi negativamente, quando reagiscono con altri elementi. I metalloidi sono elementi che si trovano lungo la divisione fra metalli e non metalli.Sono la classe di elementi pi&#xF9; piccola e presentano propriet&#xE0; miste. Tutti i metalloidi esistono come solidi a temperatura ambiente. Alcuni di essi, per esempio il silicio e il germanio, agiscono come semiconduttori, il che significa che a differenza dei metalli, migliorano la conduzione dell&#x27;elettricit&#xE0; con l&#x27;aumentare della temperatura.A temperatura ambiente, tutti i metalloidi esistono come solidi. Gli elementi nella tavola periodica sono spesso divisi anche in tre categorie in base alla loro posizione:gli elementi del gruppo principale, i metalli di transizione e i metalli di transizione interni, conosciuti anche come lantanidi e attinidi per il primo elemento della serie in ogni riga.

la tavola periodica

Quando i primi chimici scoprirono pi&#xF9; elementi, si resero conto che vari elementi potevano essere raggruppati per i loro simili comportamenti chimici. Uno di questi raggruppamento include litio (Li), sodio (Na) e potassio (K). Tutti questi elementi sono lucenti, conducono bene calore ed elettricit&#xE0; e hanno propriet&#xE0; chimiche simili. Un secondo raggruppamento comprende calcio (Ca), stronzio (Sr) e bario (Ba), che sono anche lucidi, buoni conduttori di calore ed elettricit&#xE0;, e hanno propriet&#xE0; chimiche in comune. Tuttavia, le propriet&#xE0; specifiche di questi due raggruppamenti sono notevolmente diverse l&#x27;una dall&#x27;altra. Ad esempio, Li, Na e K sono molto pi&#xF9; reattivi di Ca, Sr e Ba. Inoltre, Li, Na e K formano composti con ossigeno in un rapporto tra due dei loro atomi e un atomo di ossigeno, mentre Ca, Sr e Ba formano composti con uno dei loro atomi in un atomo di ossigeno. Anche il fluoro (F), il cloro (Cl), il bromo (Br) e lo iodio (I) presentano propriet&#xE0; simili tra loro, ma queste propriet&#xE0; sono drasticamente diverse da quelle di uno qualsiasi degli elementi sopra.

Dimitri Mendeleev in Russia (1869) e Lothar Meyer in Germania (1870) riconobbero indipendentemente una relazione periodica tra le propriet&#xE0; degli elementi conosciuti a quel tempo. Entrambe le tabelle pubblicate con gli elementi disposti in base all&#x27;aumento della massa atomica. Tuttavia, Mendeleev and&#xF2; un passo oltre Meyer; us&#xF2; il suo tavolo per prevedere l&#x27;esistenza di elementi che avrebbero avuto propriet&#xE0; simili all&#x27;alluminio e al silicio ma non erano ancora noti. Le scoperte del gallio (1875) e del germanio (1886) fornivano un supporto significativo al lavoro di Mendeleev. Sebbene Mendeleev e Meyer avessero una lunga disputa sulla priorit&#xE0;, i contributi di Mendeleev allo sviluppo della tavola periodica sono ora pi&#xF9; ampiamente riconosciuti.

Nel XX secolo, divenne evidente che la relazione periodica riguardava i numeri atomici piuttosto che le masse atomiche. L&#x27;affermazione moderna di questa relazione, la legge periodica, afferma quanto segue: le propriet&#xE0; deglielementi sono funzioni periodiche dei loro numeri atomici. Una tavola periodica moderna dispone gli elementi in ordine crescente dei loro numeri atomici, e raggruppa atomi con propriet&#xE0; simili nella stessa colonna verticale. Ogni casella rappresenta un elemento e contiene il suo numero atomico, simbolo, massa atomica media e (a volte) nome.

Gli elementi sono disposti in sette righe orizzontali, chiamate periodi o serie, e 18 colonne verticali, chiamate gruppi. I gruppi sono etichettati nella parte superiore di ogni colonna. Affinch&#xE9; la tabella si adatti a una singola pagina, parti di due righe, per un totale di 14 colonne, vengono solitamente scritte sotto il corpo principale della tabella.

Molti elementi differiscono significativamente nelle loro propriet&#xE0; chimiche e fisiche, ma alcuni elementi sono simili nei loro comportamenti. Ad esempio, molti elementi appaiono lucidi, sono malleabili e duttili e conducono bene calore ed elettricit&#xE0;. Altri elementi non sono lucidi, malleabili o duttili e sono poveri conduttori di calore ed elettricit&#xE0;. Gli elementi possono essere ordinati in grandi classi con propriet&#xE0; comuni: metalli (elementi lucidi, malleabili, buoni conduttori di calore ed elettricit&#xE0; - giallo ombreggiato); non metalli (elementi che appaiono opachi, poveri conduttori di calore ed elettricit&#xE0; - rosso ombreggiato); e metalloidi (elementi che conducono moderatamente bene il calore e l&#x27;elettricit&#xE0;, e possiedono alcune propriet&#xE0; dei metalli e alcune propriet&#xE0; dei non metalli - viola ombreggiato).

<img alt="Figure1" src="https://www.jove.com/files/core/CDNSource/lessons/806/806_Image_1_white.png" style="width: 700px;" />

Gli elementi possono anche essere classificati negli elementi del gruppo principale (o elementi rappresentativi) nelle colonne etichettate 1, 2 e 13-18; i metalli di transizione nelle colonne etichettati 3&#x2013;12; e metalli di transizione interni nelle due file nella parte inferiore del tavolo. Gli elementi della riga superiore nella parte inferiore della tabella sono lantanidi e gli elementi della riga inferiore sono attinidi. Gli elementi possono essere ulteriormente suddivisi per propriet&#xE0; pi&#xF9; specifiche, come la composizione dei composti che formano. Ad esempio, gli elementi del gruppo 1 (la prima colonna) formano composti che consistono in un atomo dell&#x27;elemento e un atomo di idrogeno. Questi elementi (eccetto l&#x27;idrogeno) sono noti come metalli alcalini, e tutti hanno propriet&#xE0; chimiche simili. Gli elementi del gruppo 2 (la seconda colonna) formano composti costituiti da un atomo dell&#x27;elemento e due atomi di idrogeno: questi sono chiamati metalli alcalini della terra, con propriet&#xE0; simili tra i membri di quel gruppo.

Altri gruppi con nomi specifici sono i pnictogeni (gruppo 15), i calcogeni (gruppo 16), gli alogeni (gruppo 17) e i gas nobili (gruppo 18, noto anche come gas inerti). I gruppi possono anche essere indicati dal primo elemento del gruppo: Ad esempio, i calcogeni possono essere chiamati gruppo ossigeno o famiglia di ossigeno. L&#x27;idrogeno &#xE8; un elemento unico e non metallico con propriet&#xE0; simili agli elementi del gruppo 1 e del gruppo 17. Per questo motivo, l&#x27;idrogeno pu&#xF2; essere mostrato nella parte superiore di entrambi i gruppi, o da solo.

L&#x27;elemento 43 (tecnezio), l&#x27;elemento 61 (promezio), e la maggior parte degli elementi con numero atomico 84 (polonio) e superiore hanno la loro massa atomica data tra parentesi quadre. Questo viene fatto per elementi che consistono interamente in isotopi radioattivi instabili (la radioattivit&#xE0; &#xE8; coperta in modo pi&#xF9; dettagliato nel capitolo sulla chimica nucleare). Un peso atomico medio non pu&#xF2; essere determinato per questi elementi perch&#xE9; i loro radioisotopi possono variare significativamente in abbondanza relativa, a seconda della fonte, o potrebbero anche non esistere in natura. Il numero tra parentesi quadre &#xE8; il numero di massa atomica, che &#xE8; una massa atomica approssimativa dell&#x27;isotopo pi&#xF9; stabile di quell&#x27;elemento.

Testo adattato da <a href="https://openstax.org/books/chemistry-2e/pages/2-5-the-periodic-table"> Openstax, Chimica 2e, Sezione 2.5: La Tavola Periodica.</a>

La tavola periodica

As early chemists discovered more elements, they realized that various elements could be grouped by their similar chemical behaviors. One such grouping ...

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periodic table patterns and element groups

The periodic table organizes elements by repeating patterns in their properties. Chemists first noticed that some elements behaved alike, so they grouped them by chemical behavior. Lithium, sodium, and potassium are one example. They are shiny and conduct heat and electricity well. Calcium, strontium, and barium form another group with similar physical and chemical properties. Yet these two groups are not the same. The lithium group is much more reactive, and its elements form oxygen compounds in a 2-to-1 atom ratio. The calcium group is less reactive, and its elements form oxygen compounds in a 1-to-1 atom ratio. Fluorine, chlorine, bromine, and iodine also share similar properties, but those properties are very different from the metal groups above.

Dimitri Mendeleev in Russia and Lothar Meyer in Germany both recognized this repeating pattern in the elements in the 1860s and 1870s. They arranged the known elements by increasing atomic mass. Mendeleev went further by predicting elements that had not yet been discovered. He expected elements with properties similar to aluminum and silicon. Later, gallium and germanium were discovered, and they supported his work. Mendeleev and Meyer later disputed who deserved priority, but Mendeleev is now more widely recognized for helping develop the periodic table.

By the twentieth century, scientists saw that the pattern depends on atomic number, not atomic mass. The periodic law says that the properties of the elements change in a repeating way as atomic number increases. A modern periodic table follows this rule. It places elements in order of increasing atomic number and groups elements with similar properties in the same vertical column.

Each box on the periodic table shows one element. It usually includes the atomic number, symbol, average atomic mass, and sometimes the name. The table has seven horizontal rows, called periods, and 18 vertical columns, called groups. The group labels appear at the top. To fit the table on one page, parts of two rows are often shown below the main table. These 14 columns belong to the lanthanides and actinides.

Elements can also be sorted by their physical properties. Metals are shiny, malleable, and ductile, and they conduct heat and electricity well. Nonmetals are usually dull and are poor conductors. Metalloids fall between these two groups. They conduct heat and electricity moderately well and have some properties of metals and some of nonmetals. The table also separates main-group elements in columns 1, 2, and 13 through 18, transition metals in columns 3 through 12, and inner transition metals in the two rows at the bottom.

Some groups have special names based on their chemistry. Group 1 elements, except hydrogen, are alkali metals. They form compounds with one atom of the element and one atom of hydrogen. Group 2 elements are alkaline earth metals, and they form compounds with one atom of the element and two atoms of hydrogen. Other named groups include the pnictogens, chalcogens, halogens, and noble gases. The chalcogens are also called the oxygen family. Hydrogen is unusual because it is a nonmetal with properties similar to both group 1 and group 17. It may appear at the top of either group or by itself.

Some elements have atomic masses shown in square brackets. This includes element 43, technetium, element 61, promethium, and most elements with atomic number 84 and higher, such as polonium. These elements are made entirely of unstable, radioactive isotopes. Because their isotopes can vary in abundance or may not occur naturally, an average atomic weight cannot be given. The bracketed value is the mass number of the most stable isotope, which is an approximate atomic mass.

Periodic Table Patterns and Element Groups

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The periodic table organizes elements by repeating patterns in their properties. Chemists first noticed that some elements behaved alike, so they grouped them by chemical behavior. Lithium, sodium, and potassium are one example. They are shiny and conduct heat and electricity well. Calcium, strontium, and barium form another group with similar physical and chemical properties. Yet these two groups are not the same. The lithium group is much more reactive, and its elements form oxygen compounds...

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Analyze the structure of atoms and isotopes.

Periodic Table Patterns and Element Groups

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