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

K12 Standards

north-carolina-k-12-science-standard-course-of-study

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

لنتذكر أن،المدارات الذرية لها طاقات مختلفة ويمكن أن تستوعب إلكترونين لكل منهما. يفرض مبدأ أوفباو توزيع الإلكترونات بين الأغلفة الفرعية للذرة،وقاعدة هوند للتعددية القصوى تشرح ملء المدارات في الأغلفة الفرعية. ينص مبدأ أوفباو على أنه في الحالة الأساسية،تملأ الإلكترونات المدارات الذرية من الأدنى إلى الأعلى طاقة لتحقيق التكوين الأقل طاقة.على الرغم من زيادة الطاقة بشكل عام مع زيادة رقم الغلاف،فإنّالاختراق الأكبر للمدارات s غالبًا ما يؤدي إلى أن تكون مدارات 4s و 5s ذات طاقات أقل من المدارات 4d و 5d،على التوالي. يمكن تذكر الترتيب باستخدام الرسوم البيانية مثل هذا،حيث مسار السهم يكشف عن تسلسل تعيين الإلكترونات للمدارات. لنضع في اعتبارنا كتابة تكوين الإلكترون للكربون و هو عنصر برقم ذري ستة.بالتأكيد،مدار 1s،الذي لديه أقل طاقة،يجب أن يمتلئ قبل المدار 2s. يمكن لكل مدار أن يحتوي على إلكترونين كحد أقصى. يدخل الإلكترون الخامس الي الغلاف الجزئي 2p.ولكن أي من المدارات الثلاثة التي تتكون من 2p يسكنها؟حسنا! المدارات،في أي غلاف فرعي،مفترض أن يكون متحلل،مما يعني أن لديهم نفس الطاقة. وهكذا،يمكن للإلكترون الخامس أن يدخل أيًا من الثلاث مدارات 2p المتحللة.ماذا عن الإلكترون السادس؟هل يدخل مدار 2p ذو الإلكترون أم واحد من مدارات 2p الشاغرة؟وفقًا لقاعدة Hund الخاصة بالتعددية القصوى،تحتل الإلكترونات المنفردة جميع مدارات طاقة معينة المستوى قبل بدء التزاوج،والإلكترونات غير المتزاوجة لا يمكن أن يكون لها دوران معاكس:يجب أن تكون دورانها متوازي. ومن ثم،بالنسبة للكربون،فإن الإلكترونين في 2p يجب أن تشغل مدارين مختلفين ويكون لها دوران متوازي. بهذه الطريقة،يمكن للإلكترونات أن تنتشر على مساحة أكبر.هذا يقلل من حماية بعضهم البعض،وبالتالي تقليل طاقة الذرة. بالنسبة للنيتروجين،كل من المدارات الثلاثة 2p مشغولة بالكترون مفرد. اما الأكسجين،عندما تكون المدارات 2p ممتلئة بالكترون مفرد،فإنّآخر إلكترون يجب أن يقترن مع إلكترون آخر في 2p.تحتوي الذرة على إلكترونين غير متزاوجين. التكوين الإلكتروني للنيون يكشف أن الغلاف الخارجي هو مملوء بسعته القصوى البالغة ثمانية إلكترونات. يحتوي النيون على إلكترونين،يُطلق عليهما الإلكترونان الأساسيان في الغلاف الداخلي،وثمانية إلكترونات،تسمى إلكترونات التكافؤ،في الغلاف الخارجي.

مبدأ أوفباو وقاعدة هوند

لتحديد التوزيع الإلكتروني لأي ذرة معينة، يمكننا بناء البنى بترتيب الأعداد الذرية. نبدأ بالهيدروجين، ونواصل العمل عبر فترات الجدول الدوري، ونضيف بروتون واحد في كل مرة إلى النواة وإلكترون واحد إلى القشرة الفرعية المناسبة إلى أن نصفنا التوزيع الإلكتروني لجميع العناصر. ويطلق على هذا الإجراء مبدأ أوفباو، من الكلمة الألمانيةأوفباو (“لبناء up”). يشغل كل إلكترون مضاف أسفل أدنى طاقة متوفرة، مع مراعاة القيود المفروضة بواسطة الأرقام الكمية المسموح بها وفقًا لمبدأ استبعاد باولي. لا تدخل الإلكترونات في حاويات فرعية ذات طاقة أعلى إلا بعد ملء الحاويات الفرعية ذات الطاقة المنخفضة بالسعة. يوضح الشكل 1 الطريقة التقليدية لتذكر ترتيب ملء المدارات الذرية.  <img alt="Figure1" src="https://www.jovecore.com/CDNSource/lessons/986/986Image_1.png" style="width: 700px;" />الصورة 1 يوضح هذا المخطط ترتيب الطاقة للمدارات الذرية ويكون مفيداً في تكوين التوزيع الإلكتروني لحالة الأرض. فكر في كتابة التوزيع الإلكتروني للكربون— عنصر يحتوي على العدد الذري السادس. تملأ أربعة إلكترونات المدارات 1s و2s. يشغل الإلكترونات الباقيان الهيكل السفلي 2p. ولدينا الآن خيار ملء أحد المدارات ذات المستوى 2p وإقران الإلكترونات أو ترك الإلكترونات غير مقترنة في مدارين مختلفين، ولكن دون توليد مدارات p. يتم ملء المدارات كما هو موضح في قاعدة هوند’: إن أقل تكوين للطاقة بالنسبة لذرة تحتوي على إلكترونات ضمن مجموعة من المدارات التي تتسبب في انخفاض عدد الإلكترونات غير المقترنة. وبالتالي، فإن الإلكترونات الموجودة في المدارات p الكربونية لها n, l, و ms أعداد كمّية متطابقة وتختلف في ml أعدادها الكمّية (بما يتوافق مع مبدأ استبعاد باولي). المخطط المداري للكربون، مع التوزيع الإلكتروني 1s22s21p2 هو: <img alt="Figure2" src="https://www.jovecore.com/CDNSource/lessons/986/986Image_2.png" style="width: 300px;" />يملأ النيتروجين (العدد الذري 7) الهياكل الفرعية 1s و2s ويحتوي على إلكترون واحد في كل من المدارات 2p الثلاثة، وفقاً لقاعدة هوند’. تحتوي هذه الإلكترونات الثلاثة على مغازل غير مقترنة. يحتوي الأكسجين (العدد الذري 8) على زوج من الإلكترونات في أي من المدارات 2p (تحتوي الإلكترونات على مغازل متعاكسة) وإلكترون واحد في كل من المدارين الآخرين. يحتوي الفلورين (العدد الذري 9) على مدار 2p واحد فقط يحتوي على إلكترون غير مقترن. جميع الإلكترونات في الغاز النبيل نيون (العدد الذري 10) هي مقترنة، ويتم ملء جميع المدارات في الهياكل n = 1 و n = 2. تم اقتباس هذا النص من <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>

لتحديد تكوين الإلكترون لأي ذرة معينة، يمكننا بناء الهياكل حسب ترتيب الأعداد الذرية. بدءا من الهيدروجين ، و ...

Education

JoVE Core

الكيمياء

واحد

Electronic Structure of Atoms

البنية الإلكترونية للذرات

KEY TERMS AND CONCEPTS

المصطلحات والمفاهيم الأساسية

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

the wave nature of light

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the bohr model

Bohr’s Quantized Atomic Orbits

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Electron waves and standing orbits explain how tiny particles can behave like waves. Large objects in the macroscopic world, like a billiard ball on a table, follow classical physics. A ball keeps moving in a straight line unless it hits another ball or a force such as friction acts on it. It also has a well-defined position, velocity, and momentum, where momentum is mass times velocity. Waves behave differently from macroscopic particles. When waves interact, they can form interference...

the uncertainty principle

Electron Position and Momentum Limits

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the quantum-mechanical model of an atom

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Quantum mechanics explains how electrons behave in atoms using waves and probability. Erwin Schrödinger built on de Broglie’s idea that an electron in hydrogen could act like a circular standing wave instead of moving in fixed circular paths. He then derived the Schrödinger equation, which became a major step in modern atomic theory. When Schrödinger applied his equation to hydrogen-like atoms, it matched Bohr’s energy expression and the Rydberg formula for hydrogen spectra. He described...

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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 =...

the pauli exclusion principle

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...

the energies of atomic orbitals

Shielding and Orbital Penetration

Shielding and orbital penetration help explain why electrons in an atom have different energies. Electrons are attracted to the positive nucleus, but they also repel one another in atoms with more than one electron. The strength of these forces depends on the charge and the distance between the particles. Opposite charges attract, like charges repel, and the force gets weaker as the particles move farther apart. An electron that stays closer to the nucleus is held more tightly. That means...

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...

electron configuration of multielectron atoms

electron-configuration-of-multielectron-atoms

Valence Electrons and Noble Gas Shorthand

Valence electrons and noble gas shorthand help show how electrons are arranged in multielectron atoms. Sodium, the alkali metal with atomic number 11, has one more electron than neon. That extra electron goes into the lowest-energy subshell available, the 3s orbital, so sodium has the configuration 1s2 2s2 2p6 3s1. Electrons in the outermost shell, where n is highest, are called valence electrons. Electrons in the inner shells are called core electrons. Because core electrons often match a...

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

chemistry

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Louisiana Student Standards for Science

High School

Matter And Its Interactions

HS-PS1-1

HS-PS1-2

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Ohio’s Learning Standards and Model Curriculum

Structure And Properties Of Matter

Atomic structure

Tennessee Academic Standards

Matter and Its Interactions

CHEM1.PS1.12

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CH.2

CH.2.e

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PS.2

PS.2.a

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HS.P1U1.1

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CHEM.6

CHEM.6.B

Alabama Course of Study Science

9-12.C.1.1.c

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Florida Department of Education

SC.912.P.8

SC.912.P.8.5

SC.912.P.10

SC.912.P.10.9

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New York State Science Learning Standards

HS. Structure and Properties of Matter

HS-PS1-1.

HS. Chemical Reactions

HS-PS1-7.

Georgia Standards of Excellence

SC1.

electron-configuration-and-chemical-properties

Electron Configuration and Chemical Properties

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PS.Chm.1.2

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Electron Filling Order in Atomic Orbitals

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