Name: electron regions in atomic orbitals
Uploaded: 2020-09-03T13:38:27.000Z
Duration: 2 min 44 s
Channel: JoVE

K12 Standards

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IPC.7

IPC.7.E

Atomic Orbitals

Het dichtste gebied van de elektronenwolk waar het meest waarschijnlijk een elektron wordt gevonden wordt beschreven in termen van atomaire orbitalen. De vorm van een atomaire orbitaal wordt bepaald door het impulsmomentkwantumgetal, l. Bedenk dat de waarden van l zijn gebaseerd op het hoofdkwantumgetal, n mogelijke waarden van l variëren van nul tot n min één.Als n groter is dan één, bestaan er meerdere subniveaus. Elke waarde van l komt overeen met een s, p, d of f orbitaal. De orbitaal met de laagste energie is de 1-s-orbitaal.Dit is een sferisch symmetrische orbitaal. De waarschijnlijkheidsdichtheid van een 1-s-orbitaal laat zien dat het elektron waarschijnlijk in de kern wordt gevonden. Gezien de elektrostatische krachten tussen protonen en elektronen is dit echter niet waarschijnlijk.Het vermenigvuldigen van de waarschijnlijkheidsdichtheid met het volume van dunne bolvormige schillen met straal r is representatiever. De totale kans om een elektron te vinden in de dunne schil op een afstand r van de kern is de radiale verdelingsfunctie. Voor waterstof is de grootste kans om een elektron te vinden op 52, 9 picometer van de kern.De vorm van de 1-s atomaire orbitaal voor waterstof is dus bolvormig met een straal van 52, 9 picometer. De 2s en 3s orbitalen zijn ook bolvormig. Ze zijn groter en hebben knoopvlakken.Bij een knoopvlak is de kans om een elektron te vinden nul. Hoofdniveaus met n gelijk aan twee of meer bevatten ook 3p-orbitalen. Deze zijn haltervormig met een knoopvlak in de kern.Hun oriëntatie wordt beschreven door de waarde van m-l. De 3p-orbitalen staan orthogonaal op elkaar. Hoofdniveaus van n gelijk aan drie of meer hebben ook 5d-orbitalen.De d-orbitalen met de klaverbladvorm hebben vier elektronendichte halters en twee loodrechte knoopvlakken. Een van de d-orbitalen is iets anders. De f-orbitalen hebben meer halters en knoopvlakken.Deze orbitalen bestaan voor hoofdniveaus van n gelijk aan vier of meer. Wanneer de orbitalen op elkaar worden gelegd, ontstaat er ongeveer een bolvorm. Dit is de reden waarom atomen over het algemeen worden weergegeven als bollen.

atomaire orbitalen

Een atomaire orbitaal vertegenwoordigt de driedimensionale gebieden in een atoom waar een elektron de grootste kans heeft om te verblijven. De radiale verdelingsfunctie geeft de totale waarschijnlijkheid aan van het vinden van een elektron binnen de dunne schil op een afstand r van de atoomkern. De atomaire orbitalen hebben verschillende vormen die worden bepaald door l, het kwantumgetal van het impulsmoment. De orbitalen zijn vaak getekend met een grensvlak, dat de dichtste delen van de wolk omsluit.  Het kwantumgetal van het impulsmoment is een geheel getal dat de waarden kan aannemen: l = 0, 1, 2, …, n – 1. Een orbitaal met een hoofdkwantumgetal van 1 (n = 1) kan slechts één waarde van l hebben ( l = 0), terwijl een hoofdkwantumgetal van 2 (n = 2) l = 0 en l = 1 toestaat. Orbitalen met dezelfde waarde van l definiëren een subshell. Orbitalen met l = 0 worden s-orbitalen genoemd en vormen de s-subshells. De waarde l = 1 komt overeen met de p-orbitalen. Voor een gegeven n vormen p-orbitalen een p-subshell (dwz 3p als n = 3). De orbitalen met l = 2 worden de d-orbitalen genoemd. De orbitalen met l = 3, 4 en 5 zijn de f, g en h orbitalen.  De orbitaal met de laagste energie is de 1s-orbitaal. Dit is een bolsymmetrische orbitaal. De waarschijnlijkheidsdichtheid (ψ2) van een 1s-orbitaal impliceert dat het elektron hoogstwaarschijnlijk in de atoomkern wordt aangetroffen. Gezien de elektrostatische krachten tussen protonen en elektronen geeft dit echter niet nauwkeurig weer waar het elektron zich zal bevinden. In plaats daarvan wordt de Radiale Distributiefunctie gebruikt,  wat een grafiek is van de totale waarschijnlijkheid dat een elektron in een orbitaal wordt gevonden met een bepaalde straal r. De radiale verdelingsfunctie wordt gevonden door de waarschijnlijkheidsdichtheid te vermenigvuldigen met het volume van dunne bolvormige schillen met stralen r. Voor de 1s-orbitaal van waterstof heeft de radiale verdelingsfunctie een waarde nul bij de atoomkern, die toeneemt tot een maximum bij 52,9 picometer voordat deze afneemt met toenemende r. Er zijn bepaalde afstanden tot de atoomkern waarop de waarschijnlijkheidsdichtheid van het vinden van een elektron in een bepaalde orbitaal nul is. Met andere woorden: de waarde van de golffunctie ψ is nul op deze afstand voor deze orbitaal. Een dergelijke waarde van r wordt een radiaal knooppunt genoemd. Het aantal radiale knooppunten in een orbitaal is n – l – 1. Voor 2s-orbitalen, waarbij n = 1, is er één radiaal knooppunt, terwijl 3s-orbitalen twee radiale knooppunten hebben.  Elk hoofdniveau met n = 2 of meer bevat drie p-orbitalen. De drie p-orbitalen hebben twee lobben met een knooppunt in de atoomkern. De oriëntatie van p-orbitalen in de ruimte wordt beschreven door de waarde van ml. De drie p-orbitalen staan onderling loodrecht (orthogonaal) op elkaar. De hogere p-orbitalen (3p, 4p, 5p en hoger) hebben vergelijkbare vormen, maar zijn groter van formaat met extra radiale knooppunten. Hoofdniveaus met n = 3 of meer bevatten vijf d-orbitalen. Vier van deze orbitalen bestaan uit een klaverbladvorm, met vier elektronendichte lobben. Er zijn twee loodrechte knoopvlakken die elkaar snijden in de atoomkern. Op deze knoopvlakken is de elektronendichtheid nul. Eén van de d-orbitalen heeft een iets andere vorm en heeft twee lobben die in de z-as zijn georiënteerd met een donutvormige ring in het xy-vlak. Hoofdniveaus met n = 4 en groter bevatten zeven f-orbitalen, die complexe vormen hebben. Deze orbitalen hebben meer knooppunten en lobben dan d-orbitalen. <img alt="Figure1" src="https://www.jove.com/files/core/CDNSource/lessons/983/983Image 1.png" style="width: 700px;"> Figuur 1: Representatieve s, p, d, en f orbitalen. Deze verschillende vormen van de atomaire orbitalen vertegenwoordigen de driedimensionale gebieden waarbinnen het elektron waarschijnlijk wordt aangetroffen. Alle orbitalen samen vormen een ruwweg bolachtige vorm, en daarom worden atomen over het algemeen weergegeven als bollen. Deze tekst is aangepast van <a href="https://openstax.org/books/chemistry-2e/pages/6-3-development-of-quantum-theory">Openstax, Chemistry 2e, Sectie 6.3: Ontwikkeling van de kwantumtheorie.</a>

Atomaire orbitalen

An atomic orbital represents the three-dimensional regions in an atom where an electron has the highest probability to reside. The radial distribution ...

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electron regions in atomic orbitals

Electron regions in atomic orbitals show where an electron is most likely to be found in an atom. These three-dimensional regions are often drawn as boundary surfaces around the densest part of the cloud.

The shape of an orbital depends on the angular momentum quantum number, l. This value can range from 0 to n - 1, where n is the principal quantum number. For n = 1, only l = 0 is allowed. For n = 2, both l = 0 and l = 1 are allowed.

Orbitals with the same value of l form a subshell. The l = 0 orbitals are s orbitals, and they make up s subshells. The l = 1 orbitals are p orbitals, which form a p subshell such as 3p when n = 3. The l = 2 orbitals are d orbitals. The l = 3, 4, and 5 orbitals are called f, g, and h orbitals.

The lowest-energy orbital is the 1s orbital. It is spherically symmetric. The probability density, ψ², suggests that an electron is most likely found at the nucleus. But this does not fully match electron behavior. The radial distribution function gives the total probability of finding an electron at a distance r from the nucleus. It is found by multiplying the probability density by the volume of thin spherical shells.

For the 1s orbital of hydrogen, the radial distribution function is zero at the nucleus. It rises to a maximum at 52.9 picometers and then decreases as r increases. Some distances from the nucleus have zero probability density for a given orbital. These points are called radial nodes. The number of radial nodes is n - l - 1. A 2s orbital has one radial node, and a 3s orbital has two.

Each principal level with n = 2 or more contains three p orbitals. Each p orbital has two lobes and a node at the nucleus. Their orientation in space is described by m_l. The three p orbitals are mutually perpendicular. Higher p orbitals, such as 3p, 4p, and 5p, have the same general shape but are larger and contain additional radial nodes.

Principal levels with n = 3 or more contain five d orbitals. Four of them have a cloverleaf shape with four electron-dense lobes. They also have two perpendicular nodal planes that meet at the nucleus. The fifth d orbital has two lobes along the z-axis and a donut-shaped ring in the xy plane.

Principal levels with n = 4 and greater contain seven f orbitals. These orbitals have complex shapes with more nodes and lobes than d orbitals. Together, s, p, d, and f orbitals help explain why atoms are often drawn as spheres, even though the electron regions inside them have distinct shapes.

Electron Regions in Atomic Orbitals

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Electron regions in atomic orbitals show where an electron is most likely to be found in an atom. These three-dimensional regions are often drawn as boundary surfaces around the densest part of the cloud. The shape of an orbital depends on the angular momentum quantum number, l. This value can range from 0 to n - 1, where n is the principal quantum number. For n = 1, only l = 0 is allowed. For n = 2, both l = 0 and l = 1 are allowed. Orbitals with the same value of l form a subshell. The l =...

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Explore electron regions in atomic orbitals, including s, p, d, and f shapes, radial nodes, and the radial distribution function for high school chemistry.

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Electron Regions in Atomic Orbitals

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