Name: electron filling order in atomic orbitals
Uploaded: 2020-09-03T13:38:28.000Z
Duration: 3 min 2 s
Channel: JoVE

K12 Standards

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NC K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.1.3

The Aufbau Principle and Hund's Rule

Atomik orbitallerin farklı enerjilere sahip olduğunu ve her birinin iki elektron barındırabileceğini hatırlayalım. Aufbau ilkesi, elektronların atomun alt kabukları arasındaki dağılımını belirler ve Hund'un maksimum çokluk kuralı alt kabuklardaki orbitallerin doldurulmasını açıklar. Aufbau ilkesi, temel durumda elektronların en düşük enerjili konfigürasyonu elde etmek için atomik orbitalleri en düşükten en yükseğe kadar doldurduğunu belirtir.Enerjinin genel olarak kabuk sayısı ile artmasına rağmen, s orbitallerinin yüksek penetrasyonu dört-s ve beş-s orbitallerinin sırasıyla üç-d ve dört-d orbitallerinden daha düşük enerjilere sahip olmalarına yol açar. Sıra, bunun gibi diyagramlar kullanılarak hatırlanabilir;burada okun yolu, elektronların orbitallere atandığı sekansları gösterir. Atom numarası altı olan karbon elementi için elektron konfigürasyonunu yazmayı düşünelim.Elbette, en düşük enerjiye sahip olan bir s orbitali, iki s orbitalinden önce doldurulmalıdır Her orbital en fazla iki elektron tutabilir. Beşinci elektron iki p'lik bir alt kabuğa girer. Ama üç adet iki-p orbitalinden hangisini dolduruyor?Peki! Herhangi bir alt kabuktaki orbitallerin dejenere olduğu varsayılır, bu da aynı enerjiye sahip oldukları anlamına gelir. Böylece, beşinci elektron, üç dejenere iki-p orbitalinden herhangi birine girebilir.Peki altıncı elektron? İki-p orbitaline bir elektronla mı yoksa boş iki-p orbitalinden biriyle mi giriyor? Hund'un maksimum çokluk kuralına göre, elektronlar eşleşmeye başlamadan önce belirli bir enerji seviyesinin tüm orbitallerini tek başlarına işgal ederler ve eşleşmemiş elektronların ters dönüşleri olamaz:dönüşleri paralel olmalıdır.Dolayısıyla, karbon için, 2 adet iki p elektronu iki farklı orbitali işgal etmeli ve paralel dönüşlere sahip olmalıdır. Bu şekilde elektronlar daha geniş bir alana yayılabilir. Bu, birbirlerini perdelemelerini azaltır ve böylece atomun enerjisini en aza indirir.Azot için, üç adet iki-p orbitalinin her biri tek başına işgal edilmiştir. Oksijen için, dejenere iki-p orbitalleri tek tek doldurulduktan sonra, son elektron başka bir iki-p elektronu ile eşleşmelidir. Atomun iki eşleşmemiş elektronu vardır.Neonun elektron konfigürasyonu, en dıştaki kabuğun maksimum sekiz elektron kapasitesine kadar doldurulduğunu gösterir. Neon, iç kabukta çekirdek elektron olarak adlandırılan iki elektrona ve en dıştaki kabukta değerlik elektronları olarak adlandırılan 8 elektrona sahiptir.

aufbau İlkesi ve hund kuralı

Herhangi bir atomun elektron konfigürasyonunu belirlemek için, yapıları atom numarası sırasına göre inşa edebiliriz. Hidrojen ile başlayıp periyodik tablonun periyotları boyunca devam ederek, tüm elementlerin elektron konfigürasyonlarını tanımlayana kadar çekirdeğe her seferinde bir proton ve uygun alt kabuğa bir elektron ekliyoruz. Bu prosedür, Almanca aufbau (“inşa etmek”) kelimesinden gelen aufbau ilkesi olarak adlandırılır. Eklenen her elektron, Pauli dışarlama ilkesine göre izin verilen kuantum sayılarının getirdiği sınırlamalara tabi olarak, mevcut en düşük enerjinin alt kabuğunu kaplar. Elektronlar daha yüksek enerjili alt kabuklara ancak daha düşük enerjili alt kabukların kapasiteleri doldurulduktan sonra girer. Şekil 1, atomik orbitaller için doldurma sırasını hatırlamanın geleneksel yolunu göstermektedir. 
 
 <img alt="Figure1" src="https://www.jovecore.com/CDNSource/lessons/986/986Image_1.png" style="width: 700px;" />
 
 Şekil 1 Bu diyagram, atomik orbitaller için enerji sırasını tasvir etmektedir ve temel-durum elektron konfigürasyonlarının türetilmesi için kullanışlıdır.
 
 Atom numarası altı olan bir element olan karbon için elektron konfigürasyonunu yazmayı düşünün. Dört elektron 1s ve 2s orbitallerini doldurur. Kalan iki elektron, 2p alt kabuğunu işgal eder. Şimdi 2p orbitallerinden birini doldurma ve elektronları eşleştirme veya elektronları iki farklı, ancak dejenere p orbitalinde eşleşmemiş halde bırakma seçeneğimiz var. Orbitaller, Hund kuralına göre doldurulur: bir dejenere orbital kümesi içinde elektronlara sahip bir atom için en düşük enerjili konfigürasyon, maksimum sayıda eşleşmemiş elektrona sahip olandır. Bu nedenle, karbon 2p orbitallerindeki iki elektron aynı n, l ve ms kuantum numaralarına sahiptir ve ml kuantum sayılarında farklılık gösterir (Pauli dışarlama ilkesine göre). 1s22s21p2 elektron konfigürasyonuna sahip karbon orbital diyagramı şöyledir: 
 
 <img alt="Figure2" src="https://www.jovecore.com/CDNSource/lessons/986/986Image_2.png" style="width: 300px;" />
 
 Nitrojen (atom numarası 7) 1s ve 2s alt kabuklarını doldurur ve Hund kuralına göre üç 2p orbitalinin her birinde bir elektrona sahiptir. Bu üç elektronun eşleşmemiş spinleri var. Oksijen (atom numarası 8), 2p orbitallerinin herhangi birinde bir çift elektrona (elektronlar zıt spinlere sahiptir) ve diğer ikisinin her birinde tek bir elektrona sahiptir. Flor (atom numarası 9), eşleşmemiş bir elektron içeren yalnızca bir 2p orbitaline sahiptir. Soy gaz neondaki (atom numarası 10) tüm elektronlar eşleşmiştir ve n = 1 ve n = 2 kabuklarındaki tüm orbitaller doludur. 
 
 Bu metin bu kaynaktan uyarlanmıştır: <a href="https://openstax.org/books/chemistry-2e/pages/6-4-electronic-structure-of-atoms-electron-configurations">Openstax, Chemistry 2e, Section 6.4: Electronic Structure of Atoms.</a>

Aufbau İlkesi ve Hund Kuralı

Herhangi bir atomun elektron konfigürasyonunu belirlemek için, yapıları atom numaraları sırasına göre oluşturabiliriz. Hidrojenden başlayarak ve ...

Education

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Electronic Structure of Atoms

Atomların Elektronik Yapısı

KEY TERMS AND CONCEPTS

TEMEL TERİMLER VE KAVRAMLAR

electron filling order in atomic orbitals

Electron filling order in atomic orbitals follows the aufbau principle and Hund's rule. To write an electron configuration, we build atoms in order of atomic number. Starting with hydrogen and moving across the periods of the periodic table, one proton is added to the nucleus and one electron is placed into the correct subshell. This process describes the ground-state electron configurations of the elements.

The aufbau principle comes from the German word aufbau, which means &quot;to build up.&quot; It says that each added electron enters the lowest-energy subshell available. The Pauli exclusion principle still applies, so electrons must follow the allowed quantum numbers. Higher-energy subshells do not fill until lower-energy subshells reach capacity.

A common filling-order diagram helps show the energy sequence of the atomic orbitals. Carbon is a useful example because it has atomic number 6. Four electrons fill the 1s and 2s orbitals, and the remaining two electrons go into the 2p subshell. At that point, the electrons can either pair in one 2p orbital or stay unpaired in two different p orbitals.

Hund's rule gives the lower-energy choice for degenerate orbitals, which are orbitals with the same energy. The rule states that electrons in a set of degenerate orbitals occupy the arrangement with the maximum number of unpaired electrons. In carbon, the two 2p electrons have the same n, l, and m_s quantum numbers, and they differ in m_l, which matches the Pauli exclusion principle.

Nitrogen, with atomic number 7, fills the 1s and 2s subshells and places one electron in each of the three 2p orbitals. These three electrons are unpaired. Oxygen, atomic number 8, has one pair of electrons in one 2p orbital and one single electron in each of the other two. Fluorine, atomic number 9, has only one 2p orbital with an unpaired electron.

Neon, atomic number 10, has all paired electrons. Its n = 1 and n = 2 shells are completely filled. This pattern shows how electron configurations build step by step across the first ten elements.

Electron Filling Order in Atomic Orbitals

electron-filling-order-in-atomic-orbitals

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the aufbau principle and hund's rule

Electron filling order in atomic orbitals follows the aufbau principle and Hund's rule. To write an electron configuration, we build atoms in order of atomic number. Starting with hydrogen and moving across the periods of the periodic table, one proton is added to the nucleus and one electron is placed into the correct subshell. This process describes the ground-state electron configurations of the elements. The aufbau principle comes from the German word aufbau, which means "to build up." It...

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key terms and concepts

Learn how electron configurations build by atomic number, why lower-energy orbitals fill first, and how Hund's rule shapes carbon, nitrogen, oxygen, fluorine, and neon.

Electron Filling Order in Atomic Orbitals | JoVE K12

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Electron Filling Order in Atomic Orbitals

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