Name: periodic table patterns and element groups
Uploaded: 2020-09-03T13:38:25.000Z
Duration: 3 min 25 s
Channel: JoVE

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North Carolina K-12 Science Standard Course of Study

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Chemistry

Matter and its Interactions

PS.Chm.2.1

The Periodic Table

Het periodiek systeem der elementen is een belangrijke referentie in de chemie voor het organiseren van de elementen. De tabel heeft zeven rijen of periodes, van boven naar beneden genummerd, en achttien kolommen die groepen of families worden genoemd. Deze groepen kunnen op twee verschillende manieren worden genummerd.Terwijl het moderne nummeringssysteem wordt aanbevolen door de International Union of Pure and Applied Chemistry of IUPAC, die de groepen nummert van 1 tot 18, gebruikt de Chemical Abstracts Services Romeinse cijfers en letters om de groepen aan te duiden. Hier worden de belangrijkste groepselementen aangeduid met letter A en de overgangselementen worden aangeduid met letter B.De elementen in een periodiek systeem zijn gerangschikt van links naar rechts en van boven naar beneden door oplopend atoomnummer. Degenen met vergelijkbare eigenschappen vallen in dezelfde groep.Sommige groepen hebben algemene namen. De elementen in groep 1, behalve waterstof, staan bekend als alkalimetalen en de elementen in groep 2 als aardalkalimetalen. Al deze metalen zijn zeer reactief en worden in de natuur aangetroffen in combinatie met andere elementen.Zeer reactieve, niet-metalen elementen in groepen 17 staan bekend als halogenen. De niet-reactieve, niet-metalen elementen van groep 18 worden edelgassen of inerte gassen genoemd. De elementen kunnen worden onderverdeeld in drie brede klassen:metalen, niet-metalen en metalloïden.Metalen zijn gegroepeerd aan de linkerkant en in het midden van het periodiek systeem en vormen de overgrote meerderheid van de elementen. Ze zijn goede geleiders van elektriciteit en warmte. Alle zijn vast bij kamertemperatuur, behalve kwik, dat vloeibaar is.Metalen zijn glanzend en kunnen in platen worden gehamerd en tot draden worden getrokken. Metalen, zoals kalium, hebben de neiging elektronen te verliezen om kationen, positief geladen ionen, te vormen wanneer ze reageren met andere elementen. Niet-metalen zijn gegroepeerd aan de rechterkant van het periodiek systeem en zijn meestal slechte geleiders van warmte en elektriciteit.Sommige zijn bij kamertemperatuur vast, terwijl andere vloeistoffen of gassen zijn. Niet-metalen hebben de neiging elektronen te winnen en anionen, negatief geladen ionen, te vormen wanneer ze reageren met andere elementen. Metalloïden zijn elementen die worden gevonden langs de scheiding tussen het metaal en niet-metalen.Ze zijn de kleinste klasse elementen en vertonen gemengde eigenschappen. Alle metalloïden bestaan als vaste stof bij kamertemperatuur. Sommigen van hen, bijvoorbeeld silicium en germanium, werken als halfgeleiders, wat betekent dat ze, in tegenstelling tot metalen, beter worden in het geleiden van elektriciteit naarmate de temperatuur stijgt.Bij kamertemperatuur bestaan alle metalloïden als vaste stoffen. Elementen in het periodiek systeem worden vaak ook onderverdeeld in drie categorieën op basis van hun locatie:de hoofdgroepelementen, de overgangsmetalen en de binnenste overgangsmetalen ook wel bekend als de lanthaniden en de actiniden voor het eerste element in de reeks in elke rij.

het periodiek systeem

Toen vroege scheikundigen meer elementen ontdekten, realiseerden ze zich dat verschillende elementen gegroepeerd konden worden op basis van hun vergelijkbare chemische gedrag. Eén zo'n groep omvat lithium (Li), natrium (Na) en kalium (K). Al deze elementen zijn glanzend, geleiden warmte en elektriciteit goed en hebben vergelijkbare chemische eigenschappen. Een tweede groep omvat calcium (Ca), strontium (Sr) en barium (Ba), die ook glanzend zijn, goede warmte- en elektriciteitsgeleiders zijn en chemische eigenschappen gemeen hebben. De specifieke eigenschappen van deze twee groepen verschillen echter opmerkelijk van elkaar. Li, Na en K zijn bijvoorbeeld veel reactiever dan Ca, Sr en Ba. Bovendien vormen Li, Na en K verbindingen met zuurstof in een verhouding van twee van hun atomen tot één zuurstofatoom, terwijl Ca, Sr en Ba verbindingen vormen met een van hun atomen tot één zuurstofatoom. Fluor (F), chloor (Cl), broom (Br) en jodium (I) vertonen ook vergelijkbare eigenschappen, maar deze eigenschappen verschillen drastisch van die van elk van de bovenstaande elementen. 
 Dimitri Mendelejev in Rusland (1869) en Lothar Meyer in Duitsland (1870) erkenden onafhankelijk van elkaar een periodieke relatie tussen de eigenschappen van de toen bekende elementen. Beide publiceerden tabellen met de elementen gerangschikt volgens toenemende atoommassa. Mendelejev ging echter nog een stap verder dan Meyer; hij gebruikte zijn tabel om het bestaan te voorspellen van elementen die eigenschappen zouden hebben die vergelijkbaar zijn met die van aluminium en silicium, maar die nog niet bekend waren. De ontdekkingen van gallium (1875) en germanium (1886) vormden een belangrijke steun voor het werk van Mendelejev. Hoewel Mendelejev en Meyer lange tijd onenigheid hadden over de prioriteit, worden Mendelejevs bijdragen aan de ontwikkeling van het periodiek systeem nu breder erkend. 
 Tegen de twintigste eeuw werd het duidelijk dat de periodieke relatie betrekking had op atoomnummers in plaats van op atoommassa's. De moderne verklaring van deze relatie, de periodieke wet, stelt het volgende: de eigenschappen van de elementen zijn periodieke functies van hun atoomnummers. Een modern periodiek systeem rangschikt de elementen in oplopende volgorde van hun atoomnummers, en groepeert atomen met vergelijkbare eigenschappen in dezelfde verticale kolom. Elk vakje vertegenwoordigt een element en bevat het atoomnummer, het symbool, de gemiddelde atoommassa en (soms) de naam.  
 De elementen zijn gerangschikt in zeven horizontale rijen, perioden of reeksen genoemd, en 18 verticale kolommen, groepen genoemd. Groepen worden bovenaan elke kolom gelabeld. Om ervoor te zorgen dat de tabel op één pagina past, worden delen van twee van de rijen, in totaal veertien kolommen, gewoonlijk onder het hoofdgedeelte van de tabel geschreven. 
 Veel elementen verschillen aanzienlijk in hun chemische en fysische eigenschappen, maar sommige elementen zijn vergelijkbaar in hun gedrag. Veel elementen zien er bijvoorbeeld glanzend uit, zijn kneedbaar en taai, en geleiden warmte en elektriciteit goed. Andere elementen zijn niet glanzend, kneedbaar of ductiel, en zijn slechte geleiders van warmte en elektriciteit. De elementen kunnen worden onderverdeeld in grote klassen met gemeenschappelijke eigenschappen: metalen (elementen die glanzend en kneedbaar zijn, goede geleiders van warmte en elektriciteit — geel gearceerd); niet-metalen (elementen die dof lijken, slechte geleiders van warmte en elektriciteit — rood gearceerd); en metalloïden (elementen die warmte en elektriciteit redelijk goed geleiden, en enkele eigenschappen van metalen en enkele eigenschappen van niet-metalen bezitten — paars gearceerd). 
 <img alt="Figure1" src="https://www.jove.com/files/core/CDNSource/lessons/806/806_Image_1_white.png" style="width: 700px;"> 

 De elementen kunnen ook worden ingedeeld in de hoofdgroepelementen (of representatieve elementen) in de kolommen met de namen 1, 2 en 13–18; de overgangsmetalen in de kolommen met het label 3–12; en binnenste overgangsmetalen in de twee rijen onderaan de tafel. De elementen op de bovenste rij onder aan de tabel zijn lanthaniden, en de elementen op de onderste rij zijn actiniden. De elementen kunnen verder worden onderverdeeld op basis van meer specifieke eigenschappen, zoals de samenstelling van de verbindingen die ze vormen. De elementen in groep 1 (de eerste kolom) vormen bijvoorbeeld verbindingen die bestaan uit één atoom van het element en één waterstofatoom. Deze elementen (behalve waterstof) staan bekend als alkalimetalen en ze hebben allemaal vergelijkbare chemische eigenschappen. De elementen in groep 2 (de tweede kolom) vormen verbindingen die bestaan uit één atoom van het element en twee waterstofatomen: deze worden aardalkalimetalen genoemd, met vergelijkbare eigenschappen onder de leden van die groep. 

 Andere groepen met specifieke namen zijn de pnictogenen (groep 15), chalcogenen (groep 16), halogenen (groep 17) en de edelgassen (groep 18, ook bekend als inerte gassen). De groepen kunnen ook worden aangeduid met het eerste element van de groep: de chalcogenen kunnen bijvoorbeeld de zuurstofgroep of zuurstoffamilie worden genoemd. Waterstof is een uniek, niet-metaalachtig element met eigenschappen die vergelijkbaar zijn met de elementen uit groep 1 en groep 17. Om die reden kan waterstof bovenaan beide groepen worden weergegeven, of op zichzelf. 

 Van element 43 (technetium), element 61 (promethium) en van de meeste elementen met atoomnummer 84 (polonium) en hoger wordt de atoommassa tussen vierkante haken weergegeven. Dit gebeurt voor elementen die volledig uit onstabiele, radioactieve isotopen bestaan (radioactiviteit wordt uitgebreider behandeld in het hoofdstuk kernchemie). Voor deze elementen kan geen gemiddeld atoomgewicht worden bepaald, omdat hun radio-isotopen aanzienlijk kunnen variëren in relatieve aantallen, afhankelijk van de bron, of misschien zelfs niet eens in de natuur voorkomen. Het getal tussen vierkante haken is het atomaire massagetal, dat bij benadering de atomaire massa is van de meest stabiele isotoop van dat element.

Het periodiek systeem

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 atomic theory of matter

Dalton’s Laws and Early Atomic Ideas

Dalton’s atomic theory explains matter with atoms, elements, and compounds. It also shows how chemical changes follow simple laws. This idea gave chemistry a microscopic model for what can be seen in the lab. The earliest recorded ideas about matter came from ancient Greek philosophers. Leucippus and Democritus said all matter was made of tiny, finite particles called atomos, meaning “indivisible.” Aristotle and others later argued that matter was made from four elements: fire, earth, air, and...

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elements: chemical symbols and isotopes

Reading Element Symbols and Isotope Notation

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the periodic table

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...

atomic mass

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Learn how the periodic table groups elements by repeating patterns, atomic number, and chemical behavior, including metals, nonmetals, groups, and special names.

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PS.Chm.1.3

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PS.Chm.3.1

Analyze the structure of atoms and isotopes.

Periodic Table Patterns and Element Groups

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