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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High School

Chemistry and Physics

IPC.7

IPC.7.E

Atomic Orbitals

Elektron bulutunun en yoğun bölgesi bir elektronun bulunma olasılığının en yüksek olduğu yer atomik orbitaller cinsinden tanımlanır. Bir atom yörüngesinin şekli, açısal momentum kuantum sayısı, l ile belirlenir. l'nin değerlerinin temel kuantum sayısına dayandığını hatırlayalım, n l'nin olası değerleri sıfırdan n eksi bire kadar değişmektedir.n birden büyük olduğunda, birden çok alt düzey vardır. Her bir l değeri bir s, p, d veya f orbitaline karşılık gelir. En düşük enerjili yörünge 1'in yörüngesidir.Bu küresel simetrik bir yörüngedir. 1 s'lik bir yörüngenin olasılık yoğunluğu, elektronun büyük olasılıkla çekirdekte bulunduğunu ortaya çıkarır. Bununla birlikte, protonlar ve elektronlar arasındaki elektrostatik kuvvetler göz önüne alındığında bu durum pek olası değil.Olasılık yoğunluğunu r yarıçaplı ince küresel kabukların hacmi ile çarpmak daha tutarlı bir yaklaşımdır. Çekirdekten r uzaklıkta ince kabuk içinde bir elektron bulunmasının toplam olasılığı, radyal dağılım fonksiyonudur. Hidrojen için, en yüksek elektron bulma olasılığı, çekirdekten 52, 9 pikometre uzaklıktadır.Bu nedenle, hidrojenin 1'in atomik yörüngesinin şekli, 52, 9 pikometre yarıçapı ile küreseldir. İki ve üç s orbitalleri de küreseldir. Daha büyükler ve düğümler de mevcuttur.Bir düğümde elektron bulma olasılığı sıfırdır. n'nin iki veya daha fazlasına eşit olduğu temel seviyeler ayrıca üç p-orbital içerir. Bunlar, çekirdekte bir düğüm bulunan lob şeklindedir.Yönleri m-l değeri ile tanımlanır. Üç p-orbitali birbirine ortogonaldir. n'nin üç veya daha fazlasına eşit ana seviyeleri ayrıca beş d orbitaline sahiptir.Yonca yaprağı şeklindeki d orbitallerinin dört elektron yoğun lob ve iki dikey düğüm düzlemi vardır. d-orbitallerinden bir tanesi biraz farklıdır. f orbitallerinin daha fazla lobu ve düğümü vardır.Bu orbitaller, dörde veya daha fazlasına eşit n ana seviyeleri için mevcuttur. Orbitalleri üst üste bindirdiğinizde, kabaca küresel bir şekil ortaya çıkar. Atomların genellikle küreler olarak temsil edilmesinin nedeni budur.

atomik orbitaller

Bir atomik yörünge, bir elektronun bulunma olasılığının en yüksek olduğu atomdaki üç boyutlu bölgeleri temsil eder. Radyal dağılım fonksiyonu, ince kabuk içinde çekirdekten r uzaklıkta bir elektron bulunma olasılığını gösterir. Atomik orbitaller, açısal momentum kuantum sayısı olan l ile belirlenen farklı şekillere sahiptir. Orbitaller genellikle bulutun en yoğun bölgelerini çevreleyen bir sınır yüzeyi ile çizilir. 
 
 Açısal momentum kuantum sayısı, l = 0, 1, 2, …, n – 1 değerlerini alabilen bir tamsayıdır. Baş kuantum sayısı 1 olan (n = 1) bir yörünge yalnızca bir l (l = 0) değerine sahip olabilir, oysa 2 (n = 2) baş kuantum sayısı l = 0 ve l = 1'e izin verir. Aynı l değerine sahip orbitaller bir alt kabuğu tanımlar.
 
 l = 0 olan orbitallere s orbitalleri denir ve s alt kabuklarını oluştururlar. l = 1 değeri p orbitallerine karşılık gelir. Belirli bir n için, p orbitalleri bir p alt kabuğu oluşturur (yani, n = 3 ise 3p). l = 2 olan orbitallere d orbitalleri denir. l = 3, 4 ve 5 olan orbitaller f, g ve h orbitalleridir. 
 
 En düşük enerjili orbital, 1s orbitalidir. Bu küresel olarak simetrik bir orbitaldir. 1s orbitalin olasılık yoğunluğu (ψ2), elektronun büyük olasılıkla çekirdekte bulunduğunu gösterir. Bununla birlikte, protonlar ve elektronlar arasındaki elektrostatik kuvvetler göz önüne alındığında, bu, elektronun nerede bulunacağını tam olarak temsil etmemektedir. Bunun yerine, belirli bir r yarıçapında bir orbitalde bir elektron olmasının toplam olasılığının bir grafiği olan Radyal Dağılım Fonksiyonu kullanılır. Radyal dağılım fonksiyonu, olasılık yoğunluğunun ince küresel kabukların hacmiyle yarıçapların, r çarpılmasıyla bulunur. Hidrojenin 1s orbitali için, Radyal Dağılım Fonksiyonu çekirdekte sıfır değerine sahiptir ve bu değer 52,9 pikometrede maksimuma değeri alır. Daha sonra bu değer, artan r ile azalmaya başlar.
 
 Belirli bir yörüngede bulunan bir elektronu bulma olasılığının sıfır olduğu çekirdekten belirli mesafeler vardır. Başka bir deyişle, bu yörünge için bu mesafede dalga fonksiyonunun değeri ψ sıfırdır. Böyle bir r değerine radyal düğüm denir. Bir yörüngedeki radyal düğüm sayısı n – l – 1'dir. n = 1 olan 2s orbitalleri için, bir radyal düğüm varken 3s orbitallerinin iki radyal düğümü vardır. 
 
 n = 2 veya daha fazla olan her baş seviye üç p orbitali içerir. Üç p orbitalinin, çekirdekte bulunan bir düğüme sahip iki lobu vardır. Uzayda p orbitallerinin yönü ml değeri ile tanımlanır. Üç p orbitali birbirine diktir (ortogonal). Daha yüksek p orbitalleri (3p, 4p, 5p ve daha yüksek) benzer şekillere sahiptir ancak ek radyal düğümlerle boyut olarak daha büyüktür.
 
 n = 3 veya daha fazla baş seviyeler beş d orbitali içerir. Bu yörüngelerden dördü, elektrondan yoğun dört loblu bir yonca yaprağı şeklinden oluşur. Çekirdekte kesişen iki dikey düğüm düzlemi vardır. Bu düğüm düzlemlerinde elektron yoğunluğu sıfırdır. d orbitallerinden birinin şekli biraz farklıdır ve xy düzleminde halka şeklinde bir halka ile z ekseninde yönlendirilmiş iki lobu vardır. n = 4 ve daha büyük baş seviyeler, karmaşık şekillere sahip yedi f orbitali içerir. Bu orbitallerin d orbitallerden daha fazla düğümü ve lobu vardır.
 
 <img alt="Figure1" src="https://www.jovecore.com/CDNSource/lessons/983/983Image 1.png" style="width: 700px;" />
 
 Şekil 1: s, p, d ve f orbitallerinin temsili görünümü.
 
 Atomik yörüngelerin bu farklı şekilleri, içinde elektronun bulunma olasılığı bulunan üç boyutlu bölgeleri temsil eder. Tüm orbitaller birlikte kabaca küresel bir şekil oluşturur, bu nedenle atomlar genellikle küreler olarak temsil edilir.
 
 Bu metin bu kaynaktan uyarlanmıştır: <a href="https://openstax.org/books/chemistry-2e/pages/6-3-development-of-quantum-theory">Openstax, Chemistry 2e, Section 6.3: Development of Quantum Theory.</a>

Atomik Orbitaller

Bir atomik orbital, bir elektronun bulunma olasılığının en yüksek olduğu bir atomdaki üç boyutlu bölgeleri temsil eder. Radyal dağılım ...

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Electronic Structure of Atoms

Atomların Elektronik Yapısı

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

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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