Name: electron spin and orbital pairing
Uploaded: 2020-09-03T13:38:27.000Z
Duration: 3 min 6 s
Channel: JoVE

K12 Standards

Texas Essential Knowledge and Skills

High School

Chemistry and Physics

IPC.7

IPC.7.E

The Pauli Exclusion Principle

Atomik orbitaller, bir atomun elektronlarının bulunma olasılığının en yüksek olduğu bölgelerdir. Ama her bir yörünge kaç elektron içerebilir? Pauli dışlama ilkesi bu soruyu yanıtlar çünkü bir atomdaki iki elektronun aynı dört kuantum sayı kümesine sahip olamayacağını söyler.Her yörünge, sabit ilkeye karşılık gelir;açısal momentum veya azimut;ve manyetik kuantum sayı değerleri. Örneğin, 1s yörüngesindeki bir elektron her zaman bir ana kuantum sayısına ve sıfır azimut ve manyetik kuantum sayılarına sahiptir. Buna göre, elektronların aynı atomik yörüngede kalması için farklı spin kuantum sayısı değerlerine veya dönüşlerine sahip olması gerekir.Spin kuantum sayısının yalnızca iki olası değeri olduğunu hatırlayın:1/2 ve 1/2. Bu nedenle, yalnızca iki elektron aynı yörüngeyi işgal edebilir. Bu nedenle, bir yörüngeye sahip her bir alt kabuğu, yalnızca iki elektron barındırabilir ve üç yörüngeye sahip her bir p alt kabuğu, altı elektron tutabilir.d ve f alt kabuklarının her biri, sırasıyla on ve on dört elektronluk maksimum kapasiteye sahiptir. Elektronların bir atomun atomik orbitalleri arasındaki dağılımı, metin veya diyagram biçiminde elektron konfigürasyonu ile temsil edilir. Bir elektronun en düşük enerjili yörüngeyi işgal ettiği temel haldeki bir hidrojen atomunu düşünelim:1s.Yazılı elektron konfigürasyonu, işgal edilen her alt kabuğu karşılık gelen kabuğun numarası, alt kabuğun harfi ve alt kabuktaki elektron sayısını belirten bir üst simge numarasıyla belirtir. Elektron konfigürasyonunun yörünge diyagram stili, işgal edilmiş bir alt kabuk içindeki her bir yörüngeyi bir kutu veya çizgi olarak ve her elektronu bir ok olarak gösterir. Yukarı doğru bir ok 1/2 dönüş veya yukarı dönüşü, aşağı doğru ise 1/2 dönüş veya aşağı dönüş anlamına gelir.Hidrojenin yörünge diyagramında bu nedenle bir yukarı doğru ok vardır. Helyumun elektron dizilimi 1s^2'dir. İki elektronun aynı kabuğa ve alt kabuğa ait oldukları için üç özdeş kuantum numarası vardır.Pauli dışlama ilkesine göre spin kuantum sayıları farklıdır. Ters dönüşlere sahip elektronlar, aynı yörüngeyi işgal ederlerse çift"olarak adlandırılır. Atom numarası üç olan lityum için, 1s yörüngesindeki iki elektron eşlenir ve 2s yörüngesindeki elektron eşlenmez.Geleneksel olarak, eşleşmemiş elektronlar spin-up olarak temsil edilir.

pauli dışarlama İlkesi

Bir atomun yörüngesindeki elektronların dizilişine elektron konfigürasyonu denir. Üç parça bilgi içeren bir sembolle bir elektron konfigürasyonunu açıklıyoruz:
 
 <ol>
 <li>Baş kuantum sayısı, n,</li>
 <li>Yörünge tipini (alt kabuk, l) belirten harf ve</li>
 <li>Söz konusu alt kabuktaki elektronların sayısını belirten üst simge numarası.</li>
 </ol>
 
 Örneğin, 2p4 notasyonu p alt kabuğundaki (l = 1) 2 baş kuantum sayısı (n) ile dört elektronu gösterir. 3d 8 gösterimi baş kuantum sayısının n = 3 olduğunu ve d alt kabuğundaki ( l = 2) sekiz elektronu gösterir.
 
 Üç kuantum sayısı elektron orbitallerini tanımlamak için iyi çalışsa da, bazı deneyler bunların tüm gözlemlenen sonuçları açıklamak için yeterli olmadığını gösterdi. 1920'lerde, hidrojen çizgisi spektrumları aşırı yüksek çözünürlükte incelendiğinde, bazı çizgilerin aslında tek bir tepe noktasının olmadığını, yakın aralıklı çizgi çiftlerinin olduğu kanıtlandı. Bu, spektrumun sözde ince yapısıdır ve aynı yörüngede konumlandıklarında bile elektronların enerjilerinde ek küçük farklılıklar olduğunu ima eder. Bu gözlemler, Samuel Goudsmit ve George Uhlenbeck'in elektronların dördüncü bir kuantum sayısına sahip olduğunu önermesine yol açtı. Buna spin kuantum numarası veya ms adını verdiler.
 
 Uygulanan bir manyetik alanda, bir elektronun farklı enerjilere sahip iki olası yönü vardır; biri yukarı dönmeli, manyetik alanla hizalı ve diğeri aşağı doğru, buna karşı hizalı.
 
 Dördüncü kuantum sayısı, spin kuantum sayısı (ms) bir elektronun bu iki farklı spin durumunu tanımlar. Bir spin kuantum sayısının iki olası değeri vardır, −1/2 (spin yukarı) ve +1/2 (spin aşağı).
 
 Elektron spini, içsel bir elektron "rotasyonu" veya "dönüşü."'nü tanımlar. Her elektron, açısal momentuma sahip küçük bir mıknatıs veya küçük dönen bir nesne veya elektrik akımına sahip bir döngü gibi davranır, ancak bu dönüş veya akım mekansal koordinatlar açısından gözlenemez.
 
 Genel elektron spininin büyüklüğü yalnızca bir değere sahip olabilir ve bir elektron yalnızca nicelenmiş iki durumdan birinde “dönebilir”. Biri, spinin z bileşeninin z-axis pozitif yönünde olduğu α durumu olarak adlandırılır. Bu, spin kuantum sayısı ms = +1/2'ye karşılık gelir. Diğeri, spinin z bileşeni negatif ve ms = −1/2 olan β durumu olarak adlandırılır.
 
 İçinde bulunduğu atomik yörünge ne olursa olsun herhangi bir elektron, spin kuantum sayısının bu iki değerinden yalnızca birine sahip olabilir. Harici bir manyetik alan uygulanırsa, farklı dönüşlere sahip elektronların enerjileri farklıdır.
 
 Bir atomdaki bir elektron tamamen dört kuantum sayısıyla tanımlanır: n, l, ml ve ms. İlk üç kuantum sayısı yörüngeyi tanımlar ve birbirine bağımlıdır, dördüncü kuantum sayısı ise spin adı verilen içsel elektron özelliğini tanımladığı için diğer kuantum sayılarından bağımsızdır. Avusturyalı bir fizikçi Wolfgang Pauli (Nobel Fizik Ödülü: 1945), elektronların atomlardaki genel davranışını anlamamız için ihtiyaç duyduğumuz son bilgiyi veren genel bir ilkeyi formüle etti. Pauli dışarlama ilkesi şu şekilde formüle edilebilir: Aynı atomdaki iki elektron, dört kuantum sayısının tümünün tam olarak aynı setine sahip olamaz. Bunun anlamı, iki elektronun aynı yörüngeyi (aynı n, l ve ml kuantum sayıları seti) ancak spin kuantum sayılarının farklı değerlere sahip olması durumunda paylaşabileceğidir. Spin kuantum sayısı (ms) yalnızca +1/2 ve -1/2 iki değere sahip olabileceğinden, ikiden fazla elektron aynı yörüngeyi işgal edemez (ve aynı yörüngede iki elektron bulunuyorsa, ters dönüşlere sahip olmaları gerekir. Bu nedenle, herhangi bir atomik yörünge yalnızca sıfır, bir veya iki elektronla doldurulabilir.
 
 Elektron konfigürasyonunun yörünge diyagram stili, işgal edilmiş bir alt kabuk içindeki her bir yörüngeyi bir kutu veya çizgi olarak ve her elektronu bir ok olarak temsil eder. 1s1'in elektron konfigürasyonu olan hidrojenin yörünge diyagramı şöyledir:
 
 <img alt="Figure1" src="https://www.jovecore.com/CDNSource/lessons/984/984Image_1.png" style="height: 40px;" />
 
 Yukarı doğru bir ok, artı yarım spini veya spin yukarıyı belirtir ve aşağı doğru ok, eksi yarım spin veya spin aşağı anlamına gelir. Hidrojenin yörünge diyagramı bu nedenle bir yukarı doğru oka sahiptir.
 
 Helyumun elektron konfigürasyonu 1s2'dir. Aynı kabuk ve alt kabuğa ait oldukları için iki elektronun üç özdeş kuantum numarası vardır. Pauli dışarlama ilkesine göre spin kuantum sayıları farklıdır. Ters spinlere sahip elektronlar, aynı yörüngeyi işgal ederse çift olarak adlandırılır.
 
 <img alt="Figure2" src="https://www.jovecore.com/CDNSource/lessons/984/984Image_2.png" style="height: 40px;" />
 
 Bu metin bu kaynaktan uyarlanmıştır: <a 6-3-development-of-quantum-theory="" books="" chemistry-2e="" href="" https:="" openstax.org="" pages="">Openstax, Chemistry 2e, Section 6.3: Development of Quantum Theory. </a>

Pauli Dışarlama İlkesi

Bir atomun orbitallerindeki elektronların düzenlenmesine elektron konfigürasyonu denir. Bir elektron konfigürasyonunu şu sembolle tanımlıyoruz ...

Education

JoVE Core

Chemistry

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Electronic Structure of Atoms

Atomların Elektronik Yapısı

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

electron spin and orbital pairing

Electron spin and orbital pairing explain why only two electrons can fit in one atomic orbital. Electron configuration describes how electrons are arranged in an atom’s orbitals. It is written with three parts: the principal quantum number, n, the orbital type, or subshell, and a superscript that shows how many electrons are in that subshell. For example, 2p4 means four electrons in a p subshell with n = 2, and 3d8 means eight electrons in a d subshell with n = 3.

The three quantum numbers describe orbitals well, but they do not explain every experimental result. In the 1920s, very high-resolution hydrogen spectra showed fine structure, where some lines split into two close peaks instead of one. This suggested that electrons in the same orbital can still have small energy differences. Samuel Goudsmit and George Uhlenbeck proposed a fourth quantum number to explain this behavior. They called it the spin quantum number, ms.

An electron can have two spin states in an external magnetic field. One state is spin up, which aligns with the magnetic field, and the other is spin down, which points against it. The spin quantum number has only two values, +1/2 and -1/2. These are also called the alpha and beta states. Electron spin is an intrinsic property, so each electron behaves like a tiny magnet, even though this motion cannot be observed in normal space.

A complete electron description uses four quantum numbers: n, l, ml, and ms. The first three quantum numbers define the orbital and depend on one another. The spin quantum number is independent because it describes the electron’s spin. Austrian physicist Wolfgang Pauli used this idea to state the Pauli exclusion principle. It says that no two electrons in the same atom can have the same set of all four quantum numbers.

This principle means that two electrons may share the same orbital only if their spin quantum numbers are different. Because ms has only two possible values, no more than two electrons can occupy one orbital. An atomic orbital can therefore hold zero, one, or two electrons. In orbital diagrams, each orbital is shown as a box or line and each electron as an arrow. A hydrogen atom with configuration 1s1 has one upward arrow, which means one spin-up electron.

Helium has the configuration 1s2. Its two electrons share the same shell and subshell, so they have three identical quantum numbers. They differ in spin, which follows the Pauli exclusion principle. Electrons with opposite spins in the same orbital are called paired.

Electron Spin and Orbital Pairing

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Learn how electron spin, quantum numbers, and orbital pairing explain why each atomic orbital holds at most two electrons in high school chemistry.

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Electron Spin and Orbital Pairing

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